US20160153067A1 - Processes for preparing titanium oxide and various other products - Google Patents

Processes for preparing titanium oxide and various other products Download PDF

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US20160153067A1
US20160153067A1 US15/014,227 US201615014227A US2016153067A1 US 20160153067 A1 US20160153067 A1 US 20160153067A1 US 201615014227 A US201615014227 A US 201615014227A US 2016153067 A1 US2016153067 A1 US 2016153067A1
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hcl
metal
solid
chloride
leachate
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US15/014,227
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Richard Boudreault
Joël Fournier
Denis Primeau
Marie-Maxime Labrecque-Gilbert
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Orbite Technologies Inc
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Orbite Technologies Inc
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Priority claimed from PCT/CA2012/000871 external-priority patent/WO2013037054A1/en
Priority claimed from PCT/CA2013/000021 external-priority patent/WO2013104059A1/en
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Priority to US15/014,227 priority Critical patent/US20160153067A1/en
Assigned to ORBITE ALUMINAE INC. reassignment ORBITE ALUMINAE INC. ASSIGNMENT OF ASSIGNORS INTEREST (SEE DOCUMENT FOR DETAILS). Assignors: PRIMEAU, Denis, FOURNIER, JOEL, LABRECQUE-GILBERT, Marie-Maxime, BOUDREAULT, RICHARD
Assigned to ORBITE TECHNOLOGIES INC. reassignment ORBITE TECHNOLOGIES INC. CHANGE OF NAME (SEE DOCUMENT FOR DETAILS). Assignors: ORBITE ALUMINAE INC.
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    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
    • C01B7/00—Halogens; Halogen acids
    • C01B7/01—Chlorine; Hydrogen chloride
    • C01B7/03—Preparation from chlorides
    • C01B7/035—Preparation of hydrogen chloride from chlorides
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
    • C01B33/00—Silicon; Compounds thereof
    • C01B33/113—Silicon oxides; Hydrates thereof
    • C01B33/12—Silica; Hydrates thereof, e.g. lepidoic silicic acid
    • C01B33/18—Preparation of finely divided silica neither in sol nor in gel form; After-treatment thereof
    • C01B33/187—Preparation of finely divided silica neither in sol nor in gel form; After-treatment thereof by acidic treatment of silicates
    • C01B33/193—Preparation of finely divided silica neither in sol nor in gel form; After-treatment thereof by acidic treatment of silicates of aqueous solutions of silicates
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01F—COMPOUNDS OF THE METALS BERYLLIUM, MAGNESIUM, ALUMINIUM, CALCIUM, STRONTIUM, BARIUM, RADIUM, THORIUM, OR OF THE RARE-EARTH METALS
    • C01F7/00—Compounds of aluminium
    • C01F7/02—Aluminium oxide; Aluminium hydroxide; Aluminates
    • C01F7/20—Preparation of aluminium oxide or hydroxide from aluminous ores using acids or salts
    • C01F7/22—Preparation of aluminium oxide or hydroxide from aluminous ores using acids or salts with halides or halogen acids
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01F—COMPOUNDS OF THE METALS BERYLLIUM, MAGNESIUM, ALUMINIUM, CALCIUM, STRONTIUM, BARIUM, RADIUM, THORIUM, OR OF THE RARE-EARTH METALS
    • C01F7/00—Compounds of aluminium
    • C01F7/02—Aluminium oxide; Aluminium hydroxide; Aluminates
    • C01F7/30—Preparation of aluminium oxide or hydroxide by thermal decomposition or by hydrolysis or oxidation of aluminium compounds
    • C01F7/306—Thermal decomposition of hydrated chlorides, e.g. of aluminium trichloride hexahydrate
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01F—COMPOUNDS OF THE METALS BERYLLIUM, MAGNESIUM, ALUMINIUM, CALCIUM, STRONTIUM, BARIUM, RADIUM, THORIUM, OR OF THE RARE-EARTH METALS
    • C01F7/00—Compounds of aluminium
    • C01F7/48—Halides, with or without other cations besides aluminium
    • C01F7/56—Chlorides
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01G—COMPOUNDS CONTAINING METALS NOT COVERED BY SUBCLASSES C01D OR C01F
    • C01G23/00—Compounds of titanium
    • C01G23/02—Halides of titanium
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01G—COMPOUNDS CONTAINING METALS NOT COVERED BY SUBCLASSES C01D OR C01F
    • C01G23/00—Compounds of titanium
    • C01G23/04—Oxides; Hydroxides
    • C01G23/047—Titanium dioxide
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01G—COMPOUNDS CONTAINING METALS NOT COVERED BY SUBCLASSES C01D OR C01F
    • C01G49/00—Compounds of iron
    • C01G49/02—Oxides; Hydroxides
    • C01G49/06—Ferric oxide (Fe2O3)
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01G—COMPOUNDS CONTAINING METALS NOT COVERED BY SUBCLASSES C01D OR C01F
    • C01G53/00—Compounds of nickel
    • C01G53/04—Oxides; Hydroxides
    • C—CHEMISTRY; METALLURGY
    • C22—METALLURGY; FERROUS OR NON-FERROUS ALLOYS; TREATMENT OF ALLOYS OR NON-FERROUS METALS
    • C22B—PRODUCTION AND REFINING OF METALS; PRETREATMENT OF RAW MATERIALS
    • C22B21/00—Obtaining aluminium
    • C22B21/0015—Obtaining aluminium by wet processes
    • C—CHEMISTRY; METALLURGY
    • C22—METALLURGY; FERROUS OR NON-FERROUS ALLOYS; TREATMENT OF ALLOYS OR NON-FERROUS METALS
    • C22B—PRODUCTION AND REFINING OF METALS; PRETREATMENT OF RAW MATERIALS
    • C22B26/00—Obtaining alkali, alkaline earth metals or magnesium
    • C22B26/20—Obtaining alkaline earth metals or magnesium
    • C22B26/22—Obtaining magnesium
    • C—CHEMISTRY; METALLURGY
    • C22—METALLURGY; FERROUS OR NON-FERROUS ALLOYS; TREATMENT OF ALLOYS OR NON-FERROUS METALS
    • C22B—PRODUCTION AND REFINING OF METALS; PRETREATMENT OF RAW MATERIALS
    • C22B3/00—Extraction of metal compounds from ores or concentrates by wet processes
    • C22B3/04—Extraction of metal compounds from ores or concentrates by wet processes by leaching
    • C22B3/06—Extraction of metal compounds from ores or concentrates by wet processes by leaching in inorganic acid solutions, e.g. with acids generated in situ; in inorganic salt solutions other than ammonium salt solutions
    • C22B3/10—Hydrochloric acid, other halogenated acids or salts thereof
    • C—CHEMISTRY; METALLURGY
    • C22—METALLURGY; FERROUS OR NON-FERROUS ALLOYS; TREATMENT OF ALLOYS OR NON-FERROUS METALS
    • C22B—PRODUCTION AND REFINING OF METALS; PRETREATMENT OF RAW MATERIALS
    • C22B3/00—Extraction of metal compounds from ores or concentrates by wet processes
    • C22B3/20—Treatment or purification of solutions, e.g. obtained by leaching
    • C22B3/44—Treatment or purification of solutions, e.g. obtained by leaching by chemical processes
    • C—CHEMISTRY; METALLURGY
    • C22—METALLURGY; FERROUS OR NON-FERROUS ALLOYS; TREATMENT OF ALLOYS OR NON-FERROUS METALS
    • C22B—PRODUCTION AND REFINING OF METALS; PRETREATMENT OF RAW MATERIALS
    • C22B34/00—Obtaining refractory metals
    • C22B34/10—Obtaining titanium, zirconium or hafnium
    • C22B34/12—Obtaining titanium or titanium compounds from ores or scrap by metallurgical processing; preparation of titanium compounds from other titanium compounds see C01G23/00 - C01G23/08
    • C22B34/1236—Obtaining titanium or titanium compounds from ores or scrap by metallurgical processing; preparation of titanium compounds from other titanium compounds see C01G23/00 - C01G23/08 obtaining titanium or titanium compounds from ores or scrap by wet processes, e.g. by leaching
    • C22B34/124—Obtaining titanium or titanium compounds from ores or scrap by metallurgical processing; preparation of titanium compounds from other titanium compounds see C01G23/00 - C01G23/08 obtaining titanium or titanium compounds from ores or scrap by wet processes, e.g. by leaching using acidic solutions or liquors
    • C22B34/1245—Obtaining titanium or titanium compounds from ores or scrap by metallurgical processing; preparation of titanium compounds from other titanium compounds see C01G23/00 - C01G23/08 obtaining titanium or titanium compounds from ores or scrap by wet processes, e.g. by leaching using acidic solutions or liquors containing a halogen ion as active agent
    • C—CHEMISTRY; METALLURGY
    • C22—METALLURGY; FERROUS OR NON-FERROUS ALLOYS; TREATMENT OF ALLOYS OR NON-FERROUS METALS
    • C22B—PRODUCTION AND REFINING OF METALS; PRETREATMENT OF RAW MATERIALS
    • C22B34/00—Obtaining refractory metals
    • C22B34/10—Obtaining titanium, zirconium or hafnium
    • C22B34/12—Obtaining titanium or titanium compounds from ores or scrap by metallurgical processing; preparation of titanium compounds from other titanium compounds see C01G23/00 - C01G23/08
    • C22B34/1236—Obtaining titanium or titanium compounds from ores or scrap by metallurgical processing; preparation of titanium compounds from other titanium compounds see C01G23/00 - C01G23/08 obtaining titanium or titanium compounds from ores or scrap by wet processes, e.g. by leaching
    • C22B34/1259—Obtaining titanium or titanium compounds from ores or scrap by metallurgical processing; preparation of titanium compounds from other titanium compounds see C01G23/00 - C01G23/08 obtaining titanium or titanium compounds from ores or scrap by wet processes, e.g. by leaching treatment or purification of titanium containing solutions or liquors or slurries
    • C—CHEMISTRY; METALLURGY
    • C22—METALLURGY; FERROUS OR NON-FERROUS ALLOYS; TREATMENT OF ALLOYS OR NON-FERROUS METALS
    • C22B—PRODUCTION AND REFINING OF METALS; PRETREATMENT OF RAW MATERIALS
    • C22B59/00—Obtaining rare earth metals
    • Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
    • Y02—TECHNOLOGIES OR APPLICATIONS FOR MITIGATION OR ADAPTATION AGAINST CLIMATE CHANGE
    • Y02P—CLIMATE CHANGE MITIGATION TECHNOLOGIES IN THE PRODUCTION OR PROCESSING OF GOODS
    • Y02P10/00—Technologies related to metal processing
    • Y02P10/20—Recycling

Definitions

  • the present disclosure relates to improvements in the field of chemistry applied to the production of alumina and/or titanium oxide. For example, it relates to processes for the production of alumina via the extraction of aluminum from aluminum-containing materials and production of titanium oxide via the extraction of titanium from titanium-containing materials. These processes can also be efficient for preparing other products such as hematite, MgO, silica and oxides of various metals, titanium chloride as well as rare earths and aluminum.
  • a process for preparing various products comprising:
  • a process for preparing alumina comprising:
  • a process for preparing aluminum comprising:
  • a process for preparing alumina and optionally other products comprising:
  • a process for preparing alumina and optionally other products comprising:
  • a process for preparing titanium oxide comprising:
  • a process for preparing titanium oxide comprising:
  • a process for preparing titanium oxide comprising:
  • a process for preparing titanium oxide comprising:
  • a process for preparing titanium oxide comprising:
  • a process for preparing titanium oxide comprising:
  • a process for preparing titanium oxide comprising:
  • a process for preparing titanium oxide comprising:
  • a process for preparing titanium oxide comprising:
  • a process for preparing alumina and optionally other products comprising:
  • a process for preparing alumina and optionally other products comprising:
  • a process for preparing alumina and optionally other products comprising:
  • a process for preparing alumina and optionally other products comprising:
  • a process for preparing alumina and optionally other products comprising:
  • a process for preparing alumina and optionally other products comprising:
  • a process for preparing aluminum and optionally other products comprising:
  • FIG. 1 shows a bloc diagram of an example of process for preparing alumina and various other products according to the present disclosure
  • FIG. 2 is an extraction curve for Al and Fe in which the extraction percentage is expressed as a function of a leaching time in a process according to an example of the present application;
  • FIG. 3 shows a bloc diagram of another example of process for preparing alumina and various other products according to the present disclosure
  • FIG. 4 is a schematic representation of an example of a process for purifying/concentrating HCl according to the present disclosure
  • FIG. 5 is a schematic representation of an example of a process for purifying/concentrating HCl according to the present disclosure
  • FIG. 6 shows another bloc diagram of an example of process for preparing alumina and various other products according to the present disclosure
  • FIG. 7 shows another bloc diagram of an example of process for preparing alumina and various other products according to the present disclosure
  • FIG. 8 shows another bloc diagram of an example of process for preparing various products.
  • FIGS. 9A and 9B show further bloc diagrams of examples of processes according to the present disclosure.
  • the material can be, for example, a titanium-containing material.
  • the material can be, for example, an aluminum-containing material.
  • the material can be, for example, an iron-containing material.
  • the aluminum-containing material can be for example chosen from aluminum-bearing ores (such as clays, argillite, mudstone, beryl, cryolite, garnet, spinel, bauxite, or mixtures thereof can be used).
  • the aluminum-containing material can also be a recycled industrial aluminum-containing material such as slag, red mud or fly ashes.
  • the titanium-containing material can be for example chosen from a titanium-bearing ores (such as ilmenite, rutile, anatase, brookite, perovskite, sphene, ecandrewsite, geikielite, pyrophanite or titanomagnetite or mixtures thereof can be used).
  • the titanium-containing material can also be a recycled industrial titanium-containing material such as slag red mud or fly ashes.
  • the material can be chosen from industrial refractory materials.
  • the material chosen from aluminosilicate minerals chosen from aluminosilicate minerals.
  • red mud refers to an industrial waste product generated during the production of alumina.
  • a waste product can contain silica, aluminum, iron, calcium, titanium. It can also contains an array of minor constituents such as Na, K, Cr, V, Ni, Ba, Cu, Mn, Pb, Zn etc.
  • red mud can comprises about 15 to about 80% by weight of Fe 2 O 3 , about 1 to about 35% by weight Al 2 O 3 , about 1 to about 65% by weight of SiO 2 , about 1 to about 20% by weight of Na 2 O, about 1 to about 20% by weight of CaO, and up to about 35% by weight of TiO 2 .
  • red mud can comprise about 30 to about 65% by weight of Fe 2 O 3 , about 10 to about 20% by weight Al 2 O 3 , about 3 to about 50% by weight of SiO 2 , about 2 to about 10% by weight of Na 2 O, about 2 to about 8% by weight of CaO, and from 0 to about 25% by weight of TiO 2 .
  • fly ashes refers to an industrial waste product generated in combustion.
  • a waste product can contain various elements such as silica, oxygen, aluminum, iron, calcium.
  • fly ashes can comprise silicon dioxide (SiO 2 ) and aluminium oxide (Al 2 O 3 ).
  • fly ashes can further comprises calcium oxide (CaO) and/or iron oxide (Fe 2 O 3 ).
  • fly ashes can comprise fine particles that rise with flue gases.
  • fly ashes can be produced during combustion of coal.
  • fly ashes can also comprise at least one element chosen from arsenic, beryllium, boron, cadmium, chromium, chromium VI, cobalt, lead, manganese, mercury, molybdenum, selenium, strontium, titanium, thallium, and/or vanadium.
  • fly ashes can also comprise rare earth elements.
  • fly ashes can be considered as an aluminum-bearing material.
  • slag refers to an industrial waste product comprising oxides such as oxides of aluminum, calcium, titanium, magnesium, iron, and/or silicon.
  • titanium chloride refers, for example, to a compound chosen from TiCl 2 , TiCl 3 and TiCl 4 and mixtures thereof. For example, it refers to TiCl 4 .
  • hematite refers, for example, to a compound comprising ⁇ -Fe 2 O 3 , ⁇ -Fe 2 O 3 , ⁇ -FeO.OH or mixtures thereof.
  • iron ions refers, for example to ions comprising to at least one type of iron ion chosen from all possible forms of Fe ions.
  • the at least one type of iron ion can be Fe 2+ , Fe 3+ , or a mixture thereof.
  • aluminum ions refers, for example to ions comprising to at least one type of aluminum ion chosen from all possible forms of Al ions.
  • the at least one type of aluminum ion can be Al 3+ .
  • At least one aluminum ion refers, for example, to at least one type of aluminum ion chosen from all possible forms of Al ions.
  • the at least one aluminum ion can be Al 3+ .
  • At least one iron ion refers, for example, to at least one type of iron ion chosen from all possible forms of Fe ions.
  • the at least one iron ion can be Fe 2+ , Fe 3+ , or a mixture thereof.
  • At least one precipitated iron ion refers, for example, to at least one type of iron ion chosen from all possible forms of Fe ions that was precipitated in a solid form.
  • the at least one iron ion present in such a precipitate can be Fe 2+ , Fe 3+ , or a mixture thereof.
  • substantially selectively recovering refers, for example, to recovering or isolating such a compound together with less than 30, 25, 20, 15, 10, 5, 3, 2 or 1% of impurities.
  • impurities can be other compounds such as other metals.
  • substantially selectively precipitating refers, for example, to precipitating such a compound together with less than 30, 25, 20, 15, 10, 5, 3, 2 or 1% of impurities.
  • impurities can be other compounds such as other metals.
  • the at least one metal can comprise a first metal that is chosen from aluminum, iron, zinc, copper, gold, silver, molybdenum, cobalt, magnesium, lithium, manganese, nickel, palladium, platinum, thorium, phosphorus, uranium and titanium, and/or at least one rare earth element and/or at least one rare metal.
  • the first metal can be aluminum, iron, or magnesium.
  • the liquid can comprise a second metal.
  • the liquid can comprise a third metal.
  • the second metal can be chosen from aluminum, iron, zinc, copper, gold, silver, molybdenum, cobalt, magnesium, lithium, manganese, nickel, palladium, platinum, thorium, phosphorus, uranium and titanium, and/or at least one rare earth element and/or at least one rare metal.
  • the process can comprise separating Si from Ti that are contained in the solid comprises leaching the solid with an acid so as to obtain a liquid portion comprising Ti and a solid portion containing Si and wherein the liquid portion is separated from the solid portion.
  • the material can be leached with HCl having a concentration of about 15 to about 45 weight %, of about 20 to about 45 weight %, of about 25 to about 45 weight %, of about 26 to about 42 weight %, of about 28 to about 40 weight %, of about 30 to about 38 weight %, or between 25 and 36 weight %.
  • HCl at about 18 wt % or about 32 wt % can be used.
  • the material can be leached with HCl having a concentration of about 1 M to about 12 M, about 2 M to about 10 M, about 3 M to about 9 M, about 4 M to about 8 M, about 5 M to about 7 M or about 6 M.
  • Leaching can also be carried out by adding dry highly concentrated acid (for example, 85%, 90% or 95%) in gas phase into the aqueous solution.
  • leaching can also be carried out by using a weak acid solution (for example ⁇ 3 wt %).
  • leaching can be carried out by using HCl having a concentration of about 18 to about 32 wt % in a first reactor and then, by using HCl having concentration of about 90 to about 95% (gaseous) in a second reactor.
  • leaching can be carried out by using HCl having a concentration of about 18 to about 32 wt % in a first reactor then, by using HCl having concentration of about 90 to about 95% (gaseous) in a second reactor; and by using HCl having concentration of about 90 to about 95% (gaseous) in a third reactor.
  • leaching can be carried out under an inert gas atmosphere (for example argon or nitrogen).
  • inert gas atmosphere for example argon or nitrogen.
  • leaching can be carried out under an atmosphere of NH 3 .
  • the material can be leached at a temperature of about 125 to about 225° C., about 140 to about 165° C., about 145 to about 160° C., about 150 to about 200° C., about 150 to about 190° C., about 160 to about 190° C., about 185 to about 190° C., about 160 to about 180° C., about 160 to about 175° C., or about 165 to about 170° C.
  • the material can be leached at a pressure of about 4 to about 10 barg, about 4 to about 8 barg, or about 5 to about 6 barg.
  • the material can be leached at a pressure of about 50 to about 150 psig, about 60 to about 100 psig, or about 70 to about 80 psig.
  • the material can be leached with HCl having a concentration of about 10 to about 50 weight %, about 15 to about 45 weight %, of about 18 to about 45 weight % of about 18 to about 32 weight %, of about 20 to about 45 weight %, of about 25 to about 45 weight %, of about 26 to about 42 weight %, of about 28 to about 40 weight %, of about 30 to about 38 weight %, or between 25 and 36 weight %.
  • HCl at about 18 wt % or about 32 wt % can be used.
  • Leaching can also be carried out by adding dry highly concentrated acid (for example, 85%, 90% or 95%) in gas phase into the aqueous solution.
  • leaching can also be carried out by using a weak acid solution (for example ⁇ 3 wt %).
  • leaching can be carried out by using HCl having a concentration of about 18 to about 32 wt % in a first reactor and then, by using HCl having concentration of about 90 to about 95%, or about 95 to about 100% (gaseous) in a second reactor.
  • leaching can be carried out by using HCl having a concentration of about 18 to about 32 wt % in a first reactor then, by using HCl having concentration of about 90 to about 95% (gaseous) in a second reactor; and by using HCl having concentration of about 90 to about 95% (gaseous) in a third reactor.
  • leaching can be carried out under an inert gas atmosphere (for example argon or nitrogen).
  • inert gas atmosphere for example argon or nitrogen.
  • leaching can be carried out under an atmosphere of NH 3 .
  • a first leaching can be carried out at atmospheric pressure and then, at least one further leaching (for example 1, 2 or 3 subsequent leaching steps) can be carried out under pressure.
  • at least one further leaching for example 1, 2 or 3 subsequent leaching steps
  • the material can be leached at a temperature of about 125 to about 225° C., about 150 to about 200° C., about 160 to about 180° C., or about 165 to about 170° C.
  • the material can be leached at a temperature of about 125 to about 225° C., about 140 to about 165° C., about 145 to about 160° C., about 150 to about 200° C., about 150 to about 190° C., about 160 to about 190° C., about 185 to about 190° C., about 160 to about 180° C., about 160 to about 175° C., or about 165 to about 170° C.
  • leaching can be a continuous leaching or semi-continous.
  • the processes can further comprise recycling the gaseous HCl so-produced by contacting it with water so as to obtain a composition having a concentration of about 18 to about 45 weight %, about 26 to about 42 weight %, about 25 to about 45 weight %, about 28 to about 40 weight %, about 30 to about 38 weight %, about 18 to about 36%, or about 25 to about 36%.
  • the processes can further comprise recycling the gaseous HCl so-produced by contacting it with water so as to obtain a composition having a concentration of about 18 to about 45 weight % or about 25 to about 45 weight % and using the composition for leaching the material.
  • the liquid can comprise iron chloride.
  • Iron chloride can comprise at least one of FeCl 2 , FeCl 3 , and a mixture thereof.
  • the iron chloride can be hydrolyzed into iron oxide.
  • iron chloride can be hydrolyzed into hematite.
  • the liquid can have an iron chloride concentration of at least 30% by weight; and can then be hydrolyzed at a temperature of about 155 to about 350° C.
  • the liquid can be concentrated to a concentrated liquid having an iron chloride concentration of at least 30% by weight; and then the iron chloride can be hydrolyzed at a temperature of about 155 to about 350° C. while maintaining a ferric chloride concentration at a level of at least 65% by weight, to generate a composition comprising a liquid and precipitated hematite, and recovering the hematite.
  • non-hydrolysable elements with hematite can be concentrated back to a concentration of about 0.125 to about 52% wt. in circulation loop in view of selective extraction.
  • the liquid can be concentrated to a concentrated liquid having a concentration of the at least one iron chloride of at least 30% by weight; and then hydrolyzed at a temperature of about 155 to about 350° C.
  • the at least one iron chloride can be hydrolyzed at a temperature of about, 150 to about 175, 160 to about 175, 155 to about 170, 160 to about 170 or 165 to about 170° C.
  • the liquid can be concentrated to a concentrated liquid having a concentration of the at least one iron chloride of at least 30% by weight; and then the at least one iron chloride is hydrolyzed at a temperature of about 155 to about 350° C. while maintaining a ferric chloride concentration at a level of at least 65% by weight, to generate a composition comprising a liquid and precipitated hematite, and recovering the hematite.
  • the liquid can be concentrated to a concentrated liquid having an iron chloride concentration of at least 30% by weight; and then the iron chloride can be hydrolyzed at a temperature of about 155 to about 350° C. while maintaining a ferric chloride concentration at a level of at least 65% by weight, to generate a composition comprising a liquid and precipitated hematite; recovering the hematite; and recovering rare earths from the liquid.
  • iron chloride can be treated by pyrohydrolysis so as to generate Cl 2 .
  • a pyrohydrolysis can be carried out under oxidizing conditions (for example O 2 can be present at a concentration of at least 4, 5, 6, 7, 8, 9, or 10% by weight).
  • O 2 can be present at a concentration of at least 4, 5, 6, 7, 8, 9, or 10% by weight.
  • such a pyrohydrolysis can be carried out in a fluid bed reactor.
  • the Cl 2 so produced can eventually used for treating the solid comprising Ti.
  • iron chloride can be pyrohydrolzed so as to generate Cl 2 .
  • the Cl 2 so generated can be used for treating said solid and to react with said Ti contained therein.
  • Cl 2 so generated can be used for treating said solid and to react with TiO 2 contained in said solid, thereby producing TiCl 4 .
  • said Fe ions can be substantially selectively extracted by converting them into Fe 2 O 3 via an hydrolysis.
  • said Fe ions can be substantially selectively extracted by converting them into Fe 2 O 3 via a pyrohydrolysis that allows for generating Cl 2 .
  • said Fe ions can be substantially selectively isolated by converting them into Fe 2 O 3 via a pyrohydrolysis that allows for generating Cl 2 .
  • said Cl 2 so produced can be effective for treating said solid so as to obtain said liquid portion comprising the titanium chloride.
  • the process can further comprise, after recovery of the rare earths, reacting the liquid with HCl so as to cause precipitation of MgCl 2 , and recovering same.
  • the processes can further comprise calcining MgCl 2 into MgO.
  • the processes can further comprise calcining MgCl 2 into MgO and recycling the gaseous HCl so-produced by contacting it with water so as to obtain a composition having a concentration of about 25 to about 45 weight % or about 18 to about 45 weight % and using the composition for leaching the red mud.
  • the processes can further comprises, after recovery of the rare earths, reacting the liquid with HCl, and substantially selectively precipitating Na 2 SO 4 .
  • Na 2 SO 4 can be precipitated by reacting the liquid with H 2 SO 4 .
  • the processes can further comprises, after recovery of the rare earths, reacting the liquid with HCl, and substantially selectively precipitating K 2 SO 4 .
  • K 2 SO 4 can be precipitated by adding H 2 SO 4 .
  • the liquid can be concentrated to a concentrated liquid having an iron chloride concentration of at least 30% by weight; and then the iron chloride can be hydrolyzed at a temperature of about 155 to about 350° C. while maintaining a ferric chloride concentration at a level of at least 65% by weight, to generate a composition comprising a liquid and precipitated hematite; recovering the hematite; and reacting the liquid with HCl.
  • a process can further comprises reacting the liquid with H 2 SO 4 so as to substantially selectively precipitate K 2 SO 4 .
  • the processes can also comprise further reacting the liquid with H 2 SO 4 so as to substantially selectively precipitating K 2 SO 4 .
  • the processes can comprise reacting dry individual salts (for example Na or K salts) obtained during the processes with H 2 SO 4 and recovering HCl while producing marketable K 2 SO 4 and Na 2 SO 4 and recovering hydrochloric acid of about 15 to about 90% wt.
  • dry individual salts for example Na or K salts
  • sodium chloride produced in the processes can undergo a chemical reaction with sulfuric acid so as to obtain sodium sulfate and regenerate hydrochloric acid.
  • Potassium chloride can undergo a chemical reaction with sulfuric acid so as to obtain potassium sulfate and regenerate hydrochloric acid.
  • Sodium and potassium chloride brine solution can alternatively be the feed material to adapted small chlor-alkali electrolysis cells. In this latter case, common bases (NaOH and KOH) and bleach (NaOCl and KOCl) are produced.
  • the processes can further comprise, after recovery of the rare earth elements and/or rare metals, recovering NaCl from the liquid, reacting the NaCl with H 2 SO 4 , and substantially selectively precipitating Na 2 SO 4 .
  • the processes can further comprise, downstream of recovery of the rare earth elements and/or rare metals, recovering KCl from the liquid, reacting the KCl with H 2 SO 4 , and substantially selectively precipitating K 2 SO 4 .
  • the processes can further comprise, downstream of recovery of the rare earth elements and/or rare metals, recovering NaCl from the liquid, carrying out an electrolysis to generate NaOH and NaOCl.
  • the processes can further comprise, downstream of recovery of the rare earth elements and/or rare metals, recovering KCl from the liquid, reacting the KCl, carrying out an electrolysis to generate KOH and KOCl.
  • the liquid can be concentrated to a concentrated liquid having a concentration of the at least one iron chloride of at least 30% by weight; and then the at least one iron chloride is hydrolyzed at a temperature of about 155 to about 350° C. while maintaining a ferric chloride concentration at a level of at least 65% by weight, to generate a composition comprising a liquid and precipitated hematite; recovering the hematite; and extracting NaCl and/or KCl from the liquid.
  • the processes can further comprise reacting the NaCl with H 2 SO 4 so as to substantially selectively precipitate Na 2 SO 4 .
  • the processes can further comprise reacting the KCl with H 2 SO 4 so as to substantially selectively precipitate K 2 SO 4 .
  • the processes can further comprise carrying out an electrolysis of the NaCl to generate NaOH and NaOCl.
  • the processes can further comprise carrying out an electrolysis of the KCl to generate KOH and KOCl.
  • the processes can comprise separating the solid from the leachate and washing the solid so as to obtain silica having a purity of at least 95%, at least 96%, at least 97%, at least 98%, at least 99%, at least 99.5% or at least 99.9%.
  • the process can comprise separating the solid from the leachate and washing the solid so as to obtain silica having a purity of at least 95%.
  • the processes can comprise reacting the leachate with gaseous HCl so as to obtain the liquid and the precipitate comprising the first metal under the form of a chloride.
  • the processes can comprise reacting the leachate with dry gaseous HCl so as to obtain the liquid and the precipitate comprising the first metal under the form of a chloride.
  • precipitating AlCl 3 can comprise crystallizing AlCl 3 .6H 2 O.
  • the process can comprise reacting the leachate with HCl recovered during the process and a having a concentration of at least 30% as to obtain the liquid and the precipitate comprising the aluminum ions, the precipitate being formed by crystallization of AlCl 3 .6H 2 O.
  • the first metal can be chosen from aluminum, iron, zinc, copper, gold, silver, molybdenum, cobalt, magnesium, lithium, manganese, nickel, palladium, platinum, thorium, phosphorus and uranium, and/or at least one rare earth element and/or at least one rare metal.
  • the second metal can be iron or aluminum.
  • the liquid can comprise a second metal.
  • the second metal can be chosen from aluminum, iron, zinc, copper, gold, silver, molybdenum, cobalt, magnesium, lithium, manganese, nickel, palladium, platinum, thorium, phosphorus and uranium and titanium, and/or at least one rare earth element and/or at least one rare metal
  • the second metal can be iron or aluminum.
  • the process can comprise separating the precipitate from the liquid and heating the second metal in order to convert a chloride of the second metal into an oxide of the second metal.
  • the processes can comprise:
  • the third metal can be chosen from aluminum, iron, zinc, copper, gold, silver, molybdenum, cobalt, magnesium, lithium, manganese, nickel, palladium, platinum, thorium, phosphorus, uranium and titanium, and/or at least one rare earth element and/or at least one rare metal.
  • the third metal can be titanium.
  • the acid used for leaching can be chosen from HCl, HNO 3 , H 2 SO 4 and mixtures thereof.
  • the acid can be HCl.
  • the acid can be gaseous HCl.
  • the process can comprise recovering the third metal from the another leachate by precipitating the third metal.
  • the third metal can be precipitated by reacting it with HCl.
  • the process can further comprise heating the third metal in order to convert a chloride of the third metal into an oxide of the third metal.
  • the first metal can be aluminum.
  • the first metal can be magnesium.
  • the first metal can be nickel.
  • the second metal can be magnesium.
  • the second metal can be nickel.
  • the second metal can be iron.
  • the processes can comprise controlling the temperature of the leachate so as to substantially selectively precipitate the first metal ions in the form of a chloride, and removing the precipitate from the leachate.
  • the process can comprise reacting the leachate with HCl so as to obtain a liquid and a precipitate comprising a chloride of the first metal, and separating the precipitate from the liquid.
  • controlling the temperature of the leachate so as to precipitate the first metal in the form of a chloride, and removing the precipitate from the leachate can be carried out before reacting the leachate with HCl so as to obtain a liquid and a precipitate comprising a chloride of the second metal, and separating the precipitate from the liquid.
  • controlling the temperature of the leachate so as to precipitate the first metal in the form of a chloride, and removing the precipitate from the leachate can be carried out after reacting the leachate with HCl so as to obtain a liquid and a precipitate comprising a chloride of the second metal, and separating the precipitate from the liquid.
  • reacting the leachate with HCl so as to obtain a precipitate comprising the first metal in the form of a chloride can be carried out by substantially selectively precipitating the first metal chloride.
  • reacting the leachate with HCl so as to obtain a precipitate comprising the second metal in the form of a chloride can be carried out by substantially selectively precipitating the second metal chloride.
  • controlling the temperature of the leachate so as to precipitate the first metal in the form of a chloride can be carried out substantially selectively.
  • controlling the temperature of the leachate so as to precipitate the second metal in the form of a chloride can be carried out substantially selectively.
  • controlling the concentration of HCl in the leachate and/or the temperature of the leachate so as to precipitate the first metal in the form of a chloride can be carried out substantially selectively.
  • controlling the concentration of HCl in the leachate and/or the temperature of the leachate so as to precipitate the second metal in the form of a chloride can be carried out substantially selectively.
  • the processes can comprise reacting the leachate with gaseous HCl so as to obtain the liquid and the precipitate comprising the aluminum ions in the form of AlCl 3 .6H 2 O.
  • the processes can comprise reacting the leachate with dry gaseous HCl so as to obtain the liquid and the precipitate comprising the aluminum ions in the form of AlCl 3 .6H 2 O.
  • the processes can comprise reacting the leachate with acid of at least 30% wt. that was recovered, regenerated and/or purified as indicated in the present disclosure so as to obtain the liquid and the precipitate comprising the aluminum ions in the form of AlCl 3 .6H 2 O.
  • the processes can comprise reacting the leachate with gaseous HCl so as to obtain the liquid and the precipitate comprising the aluminum ions, the precipitate being formed by crystallization of AlCl 3 .6H 2 O.
  • the processes can comprise reacting the leachate with dry gaseous HCl so as to obtain the liquid and the precipitate comprising the aluminum ions, the precipitate being formed by crystallization of AlCl 3 .6H 2 O.
  • aluminum ions can be precipitated under the form of AlCl 3 (for example AlCl 3 .6H 2 O) in a crystallizer, for example, by adding HCl having a concentration of about 26 to about 32 wt %.
  • AlCl 3 for example AlCl 3 .6H 2 O
  • a crystallizer for example, by adding HCl having a concentration of about 26 to about 32 wt %.
  • the solid can be treated so as to separate Ti from Si contained therein.
  • the gaseous HCl can have a HCl concentration of at least 85% wt. or at least 90% wt.
  • the gaseous HCl can have a HCl concentration of about 90% wt., about 90% to about 95% wt. or about 90% to about 99% wt.
  • the liquid can be maintained at a concentration of HCl of about 25 to about 35% by weight or about 30 to about 32% by weight.
  • the crystallization can be carried out at a temperature of about 45 to about 65° C. or about 50 to about 60° C.
  • crystallization of AlCl 3 .6H 2 O can be carried out by adding concentrated gaseous HCl to reach a proprietary concentration established of free HCl in the crystalliser.
  • the average results obtained from the crystals For example, the hexahydrate crystals can be fed to the calcination unit. AlCl 3 hydrolysis and conversion can occur at very low temperature ( ⁇ 200° C.).
  • the crystals can pass through a first step where decomposition occurs followed by the calcination itself.
  • the circulating fluid bed can be operated such that energy consumption is less than 30% of the energy normally required for hexahydrate crystal calcination.
  • the alumina produced can be washed to remove unconverted salt if required.
  • the HCl can be obtained from the gaseous HCl so-produced.
  • a given batch or quantity of the aluminum-containing material will be leached, will then be converted into AlCl 3 and when the HCl generated during calcination of AlCl 3 into Al 2 O 3 will be used for example to leach another given batch or quantity of the aluminum-containing material.
  • the processes can comprise heating the precipitate at a temperature of at least 180, 230, 250, 300, 350, 400, 450, 500, 550, 600, 650, 700, 750, 800, 850, 900, 925, 930, 1000, 1100, 1200 or 1250° C. for converting AlCl 3 into Al 2 O 3 .
  • converting AlCl 3 into Al 2 O 3 can comprise calcination of AlCl 3 .
  • calcination is effective for converting AlCl 3 into beta-Al 2 O 3 .
  • calcination is effective for converting AlCl 3 into alpha-Al 2 O 3 .
  • converting AlCl 3 into Al 2 O 3 can comprise carrying out a calcination via a two-stage circulating fluid bed reactor.
  • converting AlCl 3 into Al 2 O 3 can comprise carrying out a calcination via a two-stage circulating fluid bed reactor that comprises a preheating system.
  • converting AlCl 3 into Al 2 O 3 can comprise carrying out a calcination at low temperature, for example, about 300 to about 600° C., about 325 to about 550° C., about 350 to about 500° C., about 375 to about 450° C., about 375 to about 425° C., or about 385 to about 400° C. and/or injecting steam.
  • converting AlCl 3 into Al 2 O 3 can comprise carrying out a calcination at low temperature, for example, at least 180° C., at least 250° C., at least 300° C., at least 350° C. and/or injecting steam.
  • converting AlCl 3 into Al 2 O 3 can comprise carrying out a calcination at low temperature, for example, less than 600° C. and/or injecting steam.
  • converting AlCl 3 into Al 2 O 3 can comprise carrying out a calcination by using coal as combustion source and by using a degasification unit.
  • the process can comprise converting AlCl 3 .6H 2 O into Al 2 O 3 by carrying out a calcination of AlCl 3 .6H 2 O, the calcination comprising steam injection.
  • steam (or water vapor) can be injected at a pressure of about 200 to about 700 psig, about 300 to about 700 psig, about 400 to about 700 psig, about 550 to about 650 psig, about 575 to about 625 psig, or about 590 to about 610 psig.
  • steam or water vapor
  • a plasma torch can be used for carrying fluidization.
  • the steam (or water vapor) can be overheated.
  • the steam (or water vapor) can be at a temperature of about 300 to about 400° C.
  • acid from the offgases generated during calcination can be then treated via a gas phase purification process.
  • converting AlCl 3 into Al 2 O 3 can comprise carrying out a calcination by means of carbon monoxide (CO).
  • CO carbon monoxide
  • converting AlCl 3 into Al 2 O 3 can comprise carrying out a calcination by means of a Refinery Fuel Gas (RFG).
  • RFG Refinery Fuel Gas
  • calcination can be carried out by injecting water vapor or steam and/or by using a combustion source chosen from fossil fuels, carbon monoxide, a Refinery Fuel Gas, coal, or chlorinated gases and/or solvants.
  • a combustion source chosen from fossil fuels, carbon monoxide, a Refinery Fuel Gas, coal, or chlorinated gases and/or solvants.
  • calcination can be carried out by injecting water vapor or steam and/or by using a combustion source chosen from natural gas or propane.
  • calcination can be carried out by providing heat by means of electric heating, gas heating, microwave heating.
  • the processes can comprise precipitating the Al 3+ ions under the form of Al(OH) 3 .
  • precipitating the Al 3+ under the form of Al(OH) 3 is carried out at a pH of about 7 to about 10; about 9 to about 10; about 9.2 to about 9.8; about 9.3 to about 9.7; about 9.5; 7.5 to about 8.5; about 7.8 to about 8.2; or about 8.
  • the iron ions can be precipitated at a pH greater than 11, a pH greater than 12, a pH comprised between 10 and 11, a pH about 11.5 to about 12.5, or a pH about 11.8 to about 12.0.
  • the Al 3+ ions can be purified.
  • the process can comprise precipitating Al 3+ ions under the form of AlCl 3 so as to purify the Al 3+ ions.
  • precipitating AlCl 3 can be carried out by crystallizing the AlCl 3 under the form of AlCl 3 .6H 2 O.
  • the process can comprise converting AlCl 3 into Al 2 O 3 , for example, by converting AlCl 3 into Al 2 O 3 under an inert gas atmosphere or by converting AlCl 3 into Al 2 O 3 under a nitrogen atmosphere.
  • the obtained alumina can be washed by demineralized water so as to at least partially remove NaCl and/or KCl.
  • the fluid bed reactor can comprise a metal catalyst chosen from metal chlorides.
  • thee fluid bed reactor can comprise a metal catalyst that is FeCl 3 , FeCl 2 or a mixture thereof.
  • the fluid bed reactor can comprise a metal catalyst that is FeCl 3 .
  • the preheating system can comprise a plasma torch.
  • steam can be used as the fluidization medium heating.
  • Heating can also be electrical.
  • a plasma torch can be used for preheating the calcination reactor.
  • a plasma torch can be used for preheating air entering in the calcination reactor.
  • the plasma torch can be used for generating steam that is injected into a calcination reactor.
  • the plasma torch can be effective for generating steam that is as fluidization medium in a fluid bed reactor.
  • a plasma torch can be used for preheating a fluid bed.
  • the calcination medium can be substantially neutral in terms of O 2 (or oxidation).
  • the calcination medium can favorize reduction (for example a concentration of CO of about 100 ppm).
  • the calcination medium is effective for preventing formation of Cl 2 .
  • the processes can comprise converting AlCl 3 .6H 2 O into Al 2 O 3 by carrying out a calcination of AlCl 3 .6H 2 O, for example, that is provided by the combustion of gas mixture that comprises:
  • the air to natural gas ratio of (Nm 3 /h over Nm 3 /h) in the fluid bed can be about 9.5 to about 10
  • the air to CO gas ratio of (Nm 3 /h over Nm 3 /h) in the fluid bed can be about 2 to about 3.
  • O 2 can be substantially absent from the gas mixture.
  • the processes can comprise, before leaching the material, a pre-leaching removal of fluorine optionally contained in the material.
  • the HCl can obtained from the gaseous HCl so-produced.
  • the processes can comprise heating the precipitate at a temperature of at least 1000, 1100, 1200 or 1250° C. for converting AlCl 3 into Al 2 O 3 .
  • a given batch or quantity of the material can be leached, will then be converted into AlCl 3 and when the HCl generated during calcination of AlCl 3 into Al 2 O 3 will be used for example to leach another given batch or quantity of the aluminum-containing material.
  • the processes can be effective for providing an Al 2 O 3 recovery yield of at least 93%, at least 94%, at least 95%, about 90 to about 95%, about 92 to about 95%, or about 93 to about 95%.
  • the processes can be effective for providing a Fe 2 O 3 recovery yield of at least 98%, at least 99%, about 98 to about 99.5%, or about 98.5 to about 99.5%.
  • the processes can be effective for providing a MgO recovery yield of at least 96%, at least 97%, at least 98%, or about 96 to about 98%.
  • the processes can be effective for providing a HCl recovery yield of at least 98%, at least 99%, or about 98 to about 99.9%.
  • the aluminum-containing material can be argillite.
  • the aluminum-containing material can be bauxite.
  • the aluminum-containing material can be red mud.
  • the processes can be effective for avoiding producing red mud.
  • the alumina and the other products are substantially free of red mud.
  • HCl can be recycled.
  • such a recycled HCl can be concentrated and/or purified.
  • gaseous HCl can be concentrated and/or purified by means of H 2 SO 4 .
  • gaseous HCl can be passed through a packed column where it is contacted with a H 2 SO 4 countercurrent flow.
  • concentration of HCl can be increased by at least 50 wt %, at least 60 wt %, at least 70 wt %, at least 75 wt %, at least 80 wt %, about 50 wt % to about 80 wt %, about 55 wt % to about 75 wt %, or about 60 wt %.
  • the column can be packed with a polymer such as polypropylene or polytrimethylene terephthalate (PTT).
  • PTT polytrimethylene terephthalate
  • gaseous HCl can be concentrated and/or purified by means of CaCl 2 .
  • gaseous HCl can be passed through a column packed with CaCl 2 .
  • the processes can further comprise converting alumina (Al 2 O 3 ) into aluminum.
  • Conversion of alumina into aluminum can be carried out, for example, by using the Hall-Héroult process. References is made to such a well known process in various patents and patent applications such as US 20100065435; US 20020056650; U.S. Pat. No. 5,876,584; U.S. Pat. No. 6,565,733. Conversion can also be carried out by means of other methods such as those described in U.S. Pat. No. 7,867,373; U.S. Pat. No. 4,265,716; U.S. Pat. No. 6,565,733 (converting alumina into aluminum sulfide followed by the conversion of aluminum sulfide into aluminum.)
  • the various products obtained by the processes of the present disclosure such as alumina, hematite, titanium oxides, magnesium oxides, rare earth elements and rare metals, etc can be further purified by means of a plasma torch.
  • a plasma torch For example, they can be individually injected into a plasma torch so as to further purify them.
  • converting AlCl 3 into Al 2 O 3 can comprise carrying out a one-step calcination.
  • calcination can be carried out at different temperatures with steam.
  • Temperature applied of superheated steam can be of about 350° C. to about 550° C. or about 350° C. to about 940° C. or about 350° C. to about 1200° C.
  • multi stage evaporation step of the hydrolyser can be carried out to reduce drastically energy consumption.
  • calcination can be carried out at very low temperature with steam.
  • multi stage evaporation step of the hydrolyser can be carried out to reduce drastically energy consumption.
  • leaching of the solid with HCl can be done so as to obtain a leachate comprising titanium ions (for example TiCl 4 ).
  • leaching of the solid with HCl can be done in the presence of a chloride so as to obtain a leachate comprising titanium ions (for example TiCl 4 ).
  • a leachate comprising titanium ions (for example TiCl 4 ).
  • Such a leaching can be carried out as described in U.S. Pat. No. 7,803,336 and WO 2005049872. These documents are hereby integrated by reference in their entirety.
  • the chloride can be magnesium chloride, calcium chloride or sodium chloride.
  • the processes when applicable, can further comprise converting titanium chloride into titanium oxide.
  • Such a conversion can be carried out as described in U.S. Pat. No. 7,803,336 and WO 2005049872. These documents are hereby integrated by reference in their entirety.
  • the processes can comprise leaching of the material with HCl so as to obtain the leachate comprising aluminum ions and the solid, separating the solid from the leachate; and further treating the solid so as to separate SiO 2 from TiO 2 that are contained therein.
  • the processes can comprise leaching the material with HCl so as to obtain the leachate comprising aluminum ions and the solid, separating the solid from the leachate; and further treating the solid so as to separate Si from Ti that are contained therein.
  • the processes can comprise leaching the material with HCl so as to obtain the leachate comprising aluminum ions and the solid, separating the solid from the leachate; and further treating the solid with HCl so as to separate Si from Ti that are contained therein.
  • the process can comprise leaching the material with HCl so as to obtain the leachate comprising aluminum ions and the solid, separating the solid from the leachate; and further treating the solid with HCl, in the presence of a chloride (for example chosen from akali chlorides and alkaline earth chlorides), so as to separate Si from Ti that are contained therein.
  • a chloride for example chosen from akali chlorides and alkaline earth chlorides
  • leaching of the solid with HCl in the presence of a chloride allows for obtaining a leachate comprising titanium chloride.
  • the solid can be treated with HCl and the chloride so as to obtain a liquid portion comprising Ti and a solid portion containing Si and wherein the liquid portion is separated from the solid portion.
  • the solid can be treated with HCl and the chloride so as to obtain a liquid portion comprising TiCl 4 .
  • the process can further comprise converting TiCl 4 into TiO 2 .
  • TiCl 4 can be converted into TiO 2 by solvent extraction of the third liquid fraction and subsequent formation of titanium dioxide from the solvent extraction.
  • TiCl 4 can be reacted with water and/or a base to cause precipitation of TiO 2 .
  • TiCl 4 can be converted into TiO 2 by means of a pyrohydrolysis, thereby generating HCl.
  • TiCl 4 can be converted into TiO 2 by means of a pyrohydrolysis, thereby generating HCl that is recycled.
  • TiCl 4 can be converted into TiO 2 by reacting TiCl 4 with O 2 .
  • TiCl 4 can be converted into TiO 2 by reacting TiCl 4 with O 2 under heating.
  • HCl generated in the conversion of TiCl 4 into TiO 2 can be recovered.
  • HCl generated in the conversion of TiCl 4 into TiO 2 can be recovered and reused for leaching the titanium-containing material or the solid
  • the metal chloride can be MgCl 2 or ZnCl 2 .
  • the solid can comprise TiO 2 and SiO 2 and the solid can be treated with Cl 2 and carbon in order to obtain a liquid portion and a solid portion, and wherein the solid portion and the liquid portion are separated from one another.
  • the solid can comprise Ti and Si and the solid can be treated with Cl 2 and carbon in order to obtain a liquid portion and a solid portion, and wherein the solid portion and the liquid portion are separated from one another.
  • the solid can comprise TiO 2 and SiO 2 and the solid can be treated with Cl 2 and carbon in order to obtain a liquid portion and a solid portion, and wherein the solid portion and the liquid portion are separated from one another.
  • the solid can comprise Ti and Si and the solid can be treated with Cl 2 in order to obtain a liquid portion and a solid portion, and wherein the solid portion and the liquid portion are separated from one another.
  • the solid can comprise TiO 2 and SiO 2 and the solid can be treated with Cl 2 in order to obtain a liquid portion and a solid portion, and wherein the solid portion and the liquid portion are separated from one another.
  • the processes can comprise heating titanium chloride so as to convert it into TiO 2 .
  • the liquid portion can comprise TiCl 2 and/or TiCl 4 .
  • the liquid portion can comprise TiCl 4 .
  • the process can further comprise heating TiCl 4 so as to convert it into TiO 2 .
  • obtained TiO 2 can be purified by means of a plasma torch.
  • the solid can be treated as described in U.S. Pat. No. 7,182,931 (hereby incorporated by reference in its entirety) in order to obtain TiCl 4 and then converting TiCl 4 into TiO 2 .
  • examples of processes are also provided in U.S. Pat. No. 6,207,131, which is hereby incorporated in its entirety.
  • the processes can comprise leaching the material with HCl so as to obtain the leachate comprising aluminum ions and the solid, separating the solid from the leachate; and further treating the solid with HCl at a concentration of less than 20% wt., at a temperature of less than 85° C., in the presence of a chloride, so as to separate Si from Ti that are contained therein.
  • the chloride can be chosen from akali chlorides and alkaline earth chlorides.
  • the chloride can be MgCl 2 or CaCl 2 .
  • titanium ions under the form of titanium chloride can be in a liquid phase and the Si remains solid. Therefore, Si can thus be simply separated from Ti by a solid/liquid separation. Then, titanium chloride can be converted into TiO 2 . It has to be noted that titanium oxychloride can also be present in the leachate.
  • separation methods such as solvent extraction, precipitation or ion exchange can be used to remove impurities various impurities e. g. iron, chromium and vanadium, followed by recovery of titanium.
  • the leachate in order to purify titanium ions, can be treated with an organic phase.
  • the organic phase can be selected so that ions of a given can be selectively extracted into the organic phase, with titanium ions remaining in the aqueous solution.
  • oxides of this given metal can also be obtained in high purity.
  • Examples of the organic phase are quaternary ammonium chlorides, amines (primary, secondary or tertiary), phosphoric and phosphinic acids, and esters and oxides thereof, e. g. tri-n-butyl phosphate, di-2-ethylhexyl phosphoric acid and phosphine oxide.
  • the organic phase may be stripped from the iron values and recycled.
  • Such an organic phase can be selected so that the titanium chloride can be soluble in the organic phase.
  • the organic phase can be selected such that the organic phase and titanium chloride may be separated by fractional distillation (for example with a separation in boiling points between the organic phase and titanium chloride.)
  • the titanium chloride can be treated with water or a base, (for example magnesium oxide), or by raising the temperature of the solution to 85-110 C, to effect precipitation of titanium dioxide.
  • a base for example magnesium oxide
  • the titanium chloride product obtained can also be subjected to calcination in a pyrohydrolysis reactor or be treated in a plasma torch so as to convert it into TiO 2 .
  • NaCl recovered from the processes of the present disclosure can be reacted with SO 2 , so as to produce HCl and Na 2 SO 4 .
  • Such a reaction that is an exothermic reaction can generate steam that can be used to activate a turbine and eventually produce electricity.
  • U and/or Th can be tretaed with the processes of the present disclosure.
  • these two elements can be in such processes in admixtures with iron ions and they can be separated therefrom by means of at least one ion exchange resin.
  • the processes can involve the following steps (the reference numbers in FIG. 1 correspond to the following steps):
  • the processes can involve the following steps (the reference numbers in FIG. 1 correspond to the following steps):
  • the aluminum-containing material is reduced to an average particle size of about 50 to about 80 ⁇ m.
  • the reduced and classified material is treated with hydrochloric acid which allows for dissolving, under a predetermined temperature and pressure, the aluminum with other elements like iron, magnesium and other metals including rare earth elements and/or rare metals.
  • the silica and titanium (if present in raw material) remain totally undissolved.
  • step 4 The spent acid (leachate) obtained from step 3 is then brought up in concentration with dry and highly concentrated gaseous hydrogen chloride by sparging this one into a crystallizer. This results into the crystallization of aluminum chloride hexahydrate (precipitate) with a minimum of other impurities. Depending on the concentration of iron chloride at this stage, further crystallization step(s) can be required. The precipitate is then separated from the liquid.
  • particle size of crystals can be about 100 to about 500 microns, about 200 to about 400 microns, or about 200 to about 300 microns.
  • particle size of crystals can be about 100 to about 200 microns, about 300 to about 400 microns or about 400 to 500 microns.
  • the aluminum chloride hexahydrate is then calcined (for example by means of a rotary kiln, fluid bed, etc) at high temperature in order to obtain the alumina form.
  • Highly concentrated gaseous hydrogen chloride is then recovered and excess is brought in aqueous form to the highest concentration possible so as to be used (recycled) in the acid leaching step.
  • Acid can also be directly sent in gas phase to the acid purification stage to increase HCl concentration from about 30 wt % to about 95 wt %. This can be done, for example, during drying stage.
  • Iron chloride (the liquid obtained from step 4 ) is then pre-concentrated and hydrolyzed at low temperature in view of the Fe 2 O 3 (hematite form) extraction and acid recovery from its hydrolysis. All heat recovery from the calcination step (step 5 ), the leaching part exothermic reaction (step 1 ) and other section of the processes is being recovered into the pre-concentrator.
  • the iron chloride can be treated by means of a pyrohydrolysis in order to generate Cl 2 (instead of mianly NCl).
  • the Cl 2 so produced can be used in step 13 of FIG. 1 for treating the solid that comprises Ti.
  • Such a reaction can be carried under oxidizing conditions (for example more than 4% of O 2 ).
  • the pyrohydrolysis can be carried out in in a fluid bed reactor under such oxidizing conditions.
  • a solution rich in rare earth elements and/or rare metals can be processed.
  • an internal recirculation can be done (after the removal of hematite) and the solution rich in rare earth elements and/or rare metals can be used for crystallization stage 4 .
  • Extraction of the rare earth elements and/or rare metals can be done as described in WO/2012/126092 and/or WO/2012/149642. These two documents are hereby integrated by reference in their entirety.
  • MgCl 2 Other non-hydrolysable metal chlorides (Me-Cl) such as MgCl 2 and others then undergo the following steps:
  • Magnetic chloride hexahydrate is then calcined (either through a rotary kiln, fluid bed, etc.) and hydrochloric acid at very high concentration is thus regenerated and brought back to the leaching step.
  • Me-Cl undergo a standard pyrohydrolysis step where mixed oxides (Me-O) can be produced and hydrochloric acid at the azeotropic point (20.2% wt.) is regenerated.
  • Ti contained in the solid obtained from step 3 can be treated so as to separate Si from Ti and thus obtain SiO 2 and TiO 2 .
  • NaCl produced in this process can undergo chemical reaction with H 2 SO 4 to produce Na 2 SO 4 and HCl at a concentration at or above azeotropic concentration.
  • KCl can undergo chemical reaction with H 2 SO 4 to produce K 2 SO 4 and HCl having a concentration that is above the azeotropic concentration.
  • Sodium and potassium chloride brine solution can be the feed material to adapted small chlor-alkali electrolysis cells. In this latter case, common bases (NaOH and KOH) and bleach (NaOCl and KOCl) are produced as well as HCl.
  • the liquid can be concentrated to a concentrated liquid having an iron chloride concentration of at least 30% by weight; and then the iron chloride can be hydrolyzed at a temperature of about 155 to about 350° C. while maintaining a ferric chloride concentration at a level of at least 65% by weight, to generate a composition comprising a liquid and precipitated hematite, and recovering the hematite.
  • the liquid can be concentrated to a concentrated liquid having an iron chloride concentration of at least 30% by weight; and then the iron chloride can be hydrolyzed at a temperature of about 155 to about 350° C. while maintaining a ferric chloride concentration at a level of at least 65% by weight, to generate a composition comprising a liquid and precipitated hematite; recovering the hematite; and recovering rare earth elements and/or rare metals from the liquid.
  • the process can further comprise, after recovery of the rare earth elements and/or rare metals, reacting the liquid with HCl so as to cause precipitation of MgCl 2 , and recovering same.
  • various aluminum-containing materials can be used as starting material of the processes disclosed in the present disclosure. Examples with clays and bauxite have been carried out.
  • the continuous processes can handle high percentages of silica (>55%) and impurities as well as relatively low percentages of aluminum (for example as low as about 15%) and still being economically and technically viable. Satisfactory yields can be obtained (>93-95%) on Al 2 O 3 and greater than 75%, 85 or 90% on rare earth elements and/or rare metals. No pre-thermal treatment in most cases are required.
  • the processes disclosed in the present disclosure involve special techniques on leaching and acid recovery at very high strength, thereby offering several advantages over alkaline processes.
  • step 1 the mineral, whether or not thermally treated is crushed, milled, dried and classified to have an average particle size of about 50 to about 80 ⁇ m.
  • step 2 the milled raw material is introduced into the reactor and will undergo the leaching phase.
  • the leaching hydrochloric acid used in step 2 can be a recycled or regenerated acid from steps 5 , 6 , 8 , 9 , 10 and 11 (see FIG. 3 ) its concentration can vary from 15% to 45% weight. percent. Higher concentration can be obtained using membrane separation, cryogenic and/or high pressure approach.
  • the acid leaching can be carried out under pressure and at temperature close to its boiling point thus, allowing a minimal digestion time and extended reaction extent (90%-100%).
  • Leaching (step 2 ) can be accomplished in a semi-continuous mode where spent acid with residual free hydrochloric acid is replaced by highly concentrated acid at a certain stage of the reaction or allowing a reduced acid/mineral ratio, thereby reducing reaction time and improving reaction kinetics.
  • kinetic constant k can be: 0.5-0.75 g/mole ⁇ L.
  • leaching can be continuous leaching.
  • alkali metals, iron, magnesium, sodium, calcium, potassium, rare earth elements and other elements will also be in a chloride form at different stages.
  • Silica and optionally titanium can remain undissolved and will undergo (step 3 ) a liquid/solid separation and cleaning stage.
  • the processes of the present disclosure tend to recover maximum amount of free hydrochloric acid left and chlorides in solution in order to maximize hydrochloric acid recovery yield, using techniques such as rake classifying, filtration with band filters, centrifugation, high pressure, rotofilters and others. Thanks to step 13 , Ti contained in the solid obtained from step 3 can be treated so as to separate Si from Ti and thus obtain SiO 2 and TiO 2 .
  • Various possible strategies can be used to separated Si from Ti as previously indicated.
  • the solid can be further leached (for example with HCl in the presence of a metal chloride (for example MgCl 2 or ZnCl 2 ) so as to solubilize Ti (for example in the form of TiCl 4 ) while the Si remains solid.
  • a metal chloride for example MgCl 2 or ZnCl 2
  • the solid can be reacted with Cl 2 (see FIGS. 9A and 9B ).
  • he purified silica can then optionally undergo one or two additional leaching stages (for example at a temperature of about 150 to about 160° C.) so as to increase the purity of silica above 99.9%.
  • iron chloride generated in certain processes of the disclosure is to be treated by means of a pyrohydrolysis in order to generate Cl 2 , the latter can eventually be used in the processes of FIGS. 9A and 9B as a source of Cl 2 .
  • step 4 the spent acid (or leachate) with a substantial amount of aluminum chloride is then saturated with dry and highly concentrated gaseous hydrogen chloride obtained or recycled from step 5 or with aqueous HCl>30% wt., which results in the precipitate of aluminum chloride hexahydrate (AlCl 3 .6H 2 O).
  • the precipitate retained is then washed and filtered or centrifuged before being fed to the calcination stage (step 5 ).
  • the remaining of the spent acid from step 4 is then processed to acid recovery system (steps 6 to 8 ) where pure secondary products will be obtained.
  • step 5 aluminum oxide (alumina) is directly obtained from high temperature conditions.
  • the highly concentrated hydrogen chloride in gaseous form obtained can be fed to steps 4 and 7 for crystallization where it can be treated through hydrophobic membranes.
  • the excess hydrogen chloride is absorbed and used as regenerated acid to the leaching step 2 as highly concentrated acid, higher than the concentration at the azeotropic point (>20.2%).
  • concentration at the azeotropic point >20.2%
  • concentration at the azeotropic point >20.2%
  • concentration at the azeotropic point can be about 18 to about 45 weight %, about 25 to about 45 weight % or between 25 and 36 weight %.
  • Acid can also be redirected in gas phase directly (>30 wt %) to acid purification.
  • step 4 various chlorides derivatives (mainly iron with magnesium and rare earth elements and rare metals) are next subjected to an iron extraction step.
  • a step can be carried out for example by using the technology disclosed in WO 2009/153321, which is hereby incorporated by reference in its entirety.
  • hematite can be seeded for crystal growth.
  • hematite seeding can comprise recirculating the seeding.
  • step 6 a hydrolysis at low temperature (155-350° C.) is carried out and pure Fe 2 O 3 (hematite) is being produced and hydrochloric acid of at least 15% concentration is being regenerated.
  • the method as described in WO 2009/153321 is processing the solution of ferrous chloride and ferric chloride, possible mixtures thereof, and free hydrochloric acid through a series of steps pre-concentration step, oxidation step where ferrous chloride is oxidized into ferric form, and finally through an hydrolysis step into an operational unit called hydrolyser where the ferric chloride concentration is maintained at 65 weight % to generate a rich gas stream where concentration ensures a hydrogen chloride concentration of 15-20.2% and a pure hematite that will undergo a physical separation step. Latent heat of condensation is recovered to the pre-concentration and used as the heating input with excess heat from the calcination stage (step 5 ).
  • the mother liquor from the hydrolyser (step 6 ) can be recirculated partially to first step crystallization process where an increase in concentration of non-hydrolysable elements is observed.
  • the liquor is rich in other non-hydrolysable elements and mainly comprises magnesium chloride or possible mixture of other elements (various chlorides) and rare earth elements and rare metals that are, for example, still in the form of chlorides.
  • Rare earth elements and rare metals in form of chlorides are highly concentrated, in percentage, into the hydrolyser operational unit (step 6 ) and are extracted from the mother liquor (step 10 ) where various known techniques can be employed to extract a series of individual RE-O (rare earth oxides).
  • the processes of the present disclosure allows to concentrate to high concentration the following elements, within the hydrolyser: scandium (Sc), galium (Ga), yttrium (Y), dysperosium (Dy), cerium (Ce), praseodynium (Pr), neodynium (Nd), europium (Eu), lanthanum (La), samarium (Sm), gadolinium, (Gd), erbium (Er), zirconium (Zr) and mixtures of thereof.
  • technologies that can be used for extracting rare earth elements and/or rare metals can be found, for example, in Zhou et al. in RARE METALS, Vol. 27, No.
  • step 7 The spent acid liquor from steps 6 and 10 rich in value added metals, mainly magnesium, is processed to step 7 .
  • the solution is saturated with dry and highly concentrated gaseous hydrogen chloride from step 5 , which results in the precipitation of magnesium chloride hexahydrate. For example, same can be accomplished with HCl in aqueous form over 30% wt.
  • the precipitate retained, is fed to a calcination stage step 8 where pure MgO (>98% wt.) is obtained and highly concentrated hydrochloric acid (for example of at least 38%) is regenerated and diverted to the leaching step (step 2 ).
  • An alternative route for step 7 is using dry gaseous hydrochloric acid from step 8 .
  • step 9 metal chlorides unconverted are processed to a pyrohydrolysis step (700-900° C.) to generate mixed oxides and where hydrochloric acid from 15-20.2% wt. concentration can be recovered.
  • the processes can be similar to the example shown in FIG. 1 but can comprise some variants as below discussed.
  • the processes can comprise (after step 6 or just before step 10 ) an internal recirculation back to the crystallization step 4 .
  • the mother liquor from the hydrolyser (step 6 ) can be recirculated fully or partially to the crystallization of step 4 where a concentration increase will occur with respect to the non-hydrolysable elements including rare earth elements and/or rare metals.
  • Such a step can be useful for significantly increasing the concentration of rare earth elements and/or rare metals, thereby facilitating their extraction in step 10 .
  • the solution rich in magnesium chloride and other non-hydrolysable products at low temperature is, as previously discussed, then brought up in concentration with dry and highly concentrated gaseous hydrogen chloride by sparging it into a crystallizer. This can result into the precipitation of magnesium chloride as an hexahydrate (for example after sodium and potassium chloride removal). This can also be accomplished with HCl in aqueous form.
  • an extra step 11 can be added.
  • Sodium chloride can undergo a chemical reaction with sulfuric acid so as to obtain sodium sulfate and regenerate hydrochloric acid at a concentration at or above the azeotropic point.
  • Potassium chloride can undergo a chemical reaction with sulfuric acid so as to obtain potassium sulfate and regenerate hydrochloric acid at a concentration above the azeotropic concentration.
  • Sodium and potassium chloride brine solution can be the feed material to adapted small chlor-alkali electrolysis cells. In this latter case, common bases (NaOH and KOH) and bleach (NaOCl and KOCl) are produced and can be reused to some extent in other areas of the processes of the present disclosure (scrubber, etc.).
  • Rare earth elements and/or rare metals 0.04%-0.07%;
  • This material is thereafter leached in a two-stage procedure at 140-170° C. with 18-32 weight % HCl.
  • the HCl solution was used in a stoichiometric excess of 10-20% based on the stoichiometric quantity required for the removal of the acid leachable constituents of the clay.
  • the clay was contacted for 2.5 hours with required amount or certain proportion of the total amount of hydrochloric acid. After removal of the spent acid, the clay was contacted again with a minimum 18 weight % hydrochloric acid solution for about 1.5 hour at same temperature and pressure.
  • FIG. 2 A typical extraction curve obtained for both iron and aluminum for a single stage leaching is shown in FIG. 2 .
  • the leachate was filtered and the solid was washed with water and analyzed using conventional analysis techniques (see step 3 of FIG. 1 ). Purity of obtained silica was of 95.4% and it was free of any chlorides and of HCl.
  • the purity of the silica was 99.67% through an extra leaching step.
  • Spent acid was then crystallized using about 90 to about 98% pure dry hydrochloric acid in gas phase in two stages with less than 25 ppm iron in the aluminum chloride hexahydrate formed.
  • concentration of HCl in solution (aqueous phase) was about 22 to about 32% or 25 to about 32%, allowing 95.3% of Al 2 O 3 recovery.
  • the recovered crystallized material (hydrate form of AlCl 3 having a minimum purity of 99.8%) was then calcined at 930° C. or 1250° C., thus obtaining the a form of the alumina. Heating at 930° C. allows for obtaining the beta-form of alumina while heating at 1250° C. allows for obtaining the alpha-form.
  • Iron chloride (about 90-95% in ferric form) is then sent to a hydrothermal process in view of its extraction as pure hematite (Fe 2 O 3 ). This can be done by using the technology described in WO 2009/153321 of low temperature hydrolysis with full heat recovery from calcining, pyrohydrolysis and leaching stage.
  • Rare earth elements and rare metals are extracted from the mother liquor of the hydrolyzer where silica, aluminum, iron and a great portion of water have been removed and following preconcentration from hydrolyser to crystallization. It was observed that rare earth elements can be concentrated by a factor of about 4.0 to 10.0 on average within the hydrolyzer itself on a single pass through it i.e. without concentration loop. The following concentration factors have been noted within the hydrolyzer (single pass):
  • Remaining magnesium chloride is sparged with dry and highly concentrated hydrochloric acid and then calcinated to MgO while recovering high concentration acid (for example up to 38.4%).
  • a similar feed material (bauxite instead of clay) was processed as per in example 1 up to the leaching stage and revealed to be easily leachable under the conditions established in example 1. It provided an extraction percentage of 100% for the iron and over 90-95% for aluminum. The technology was found to be economically viable and no harmful by-products (red mud) were generated. Samples tested had various concentrations of Al 2 O 3 (up to 51%), Fe 2 O 3 (up to 27%) and MgO (up to 1.5%). Gallium extraction of 97.0% was observed. Scandium extraction was 95%.
  • H 2 SO 4 can be used for carrying out purification of HCl. It can be carried out by using a packing column with H 2 SO 4 flowing counter currently (see FIG. 4 ). This allows for converting the recovered HCl into HCl having a concentration above the azeotropic point (20.1% wt) and increase its concentration by about 60 to about 70% at minimum.
  • H 2 SO 4 Water is absorbed by H 2 SO 4 and then H 2 SO 4 regeneration is applied where H 2 SO 4 is brought back to a concentration of about 95 to about 98% wt. Water release at this stage free of sulphur is recycled back and used for crystallization dissolution, etc.
  • Packing of the column can comprise polypropylene or polytrimethylene terephthalate (PTT).
  • Combustion energy can be performed with off gas preheating air and oxygen enrichment.
  • Oxygen enrichment: +2% represents flame temperature increase by: 400° C. maximum.
  • CaCl 2 can be used for drying HCl.
  • CaCl 2 can be used for absorbing water contained into HCl.
  • CaCl 2 is converted into its hexachloride form (CaCl 2 .6H 2 O) and one saturated system is eventually switched into regeneration mode where hot air recovered from calcination off gas of alumina and magnesium oxide spray roasting is introduced to regenerate the fixed bed.
  • other absorbing agent such as LiCl can be used instead of CaCl 2 .
  • Such an ion/exchange type process can be seen in FIG. 4 and the cycle can be inversed to switch from one column to another one.
  • FIGS. 6 and 7 This example was carried out by using a process as represented in FIGS. 6 and 7 . It should be noted that the processes represented in FIGS. 6 and 7 differ mainly by the fact that FIG. 7 shows an extra stage i.e. stage 112 .
  • Raw material clay for example, was processed in a secondary crusher in the clay preparation plant 101 . Dry milling and classifying occurs on a dry basis in vertical roller mills (for example Fuller-Loesche LM 30.41).
  • the clay preparation 101 included three roller mills; two running at a capacity of approximately 160-180 tph and one on standby.
  • Raw material if required, can be reduced to 85% less than 63 microns.
  • Processed material was then stored in homogenization silos before being fed to the acid leaching plant 102 . Below in Table 1 are shown results obtained during stage 101 . If the ore contains the fluorine element, a special treatment can be applied before carrying out the 102 stage. In presence of hydrochloric acid, fluorine can produce hydrofluoric acid.
  • Stage 112 can comprise treating the processed material coming from stage 101 with an acid in a pre-leaching treatment so as to remove hydrofluoric acid. Therefore, depending on the composition of the raw material, a fluorine separation stage 112 (or pre-leaching stage 112 ) can be carried out.
  • acid leaching 102 was performed semi-continuously in an 80 m 3 glass-lined reactor.
  • Semi-continuous mode comprises replacing reacted acid 1 ⁇ 3 in the reaction period with higher concentration regenerated acid, which greatly improves reaction kinetics.
  • the reactor arrangement comprises for example, a series of three reactors. Other examples have been carried out with a first leaching at 1 atm was carried out and then, a second and third semi-continous or continuous leaching was carried out with aqueous or gaseous HCl.
  • Leaching was performed at high temperature and pressure (about 160 to about 195° C. and pressures of about 5 to about 8 barg) for a fixed period of time. Reaction time was a function of the reaction extent targeted (98% for Al 2 O 3 ), leaching mode, acid strength, and temperature/pressure applied.
  • Step 113 can then be carried out in various manners as indicated previously for step 13 . This allows, for example, a maximum quantity of about 30 ppm SiO 2 going into spent liquor. Cleaned silica at a concentration of ⁇ 96%+SiO 2 is then produced. Various options are possible at that point. For example, the 96% silica can undergo final neutralization through caustic bath, cleaning, and then bricketing before storage.
  • the silica purified by adding another leaching step followed by a solid separation step that ensures TiO 2 removal see stage 113 in FIGS. 6 and 7 ).
  • stage 113 titanium and silicium can be separated from one another in various manners.
  • the solid obtained from stage 103 can be leached in the presence of MgCl 2 at a temperature below 90 or 80° C. and at low acid concentration.
  • acid concentration can be below 25 or 20%.
  • the acid can be HCl or H 2 SO 4 .
  • titanium remains soluble after such a leaching while titanium is still in a solid form. The same also applies when the solid is treated with Cl 2 .
  • Spent acid with an aluminum chloride content of about 20 to about 30%, was then processed in the crystallization stage 104 .
  • Dry and highly concentrated HCl (>90% wt.) in gas phase was sparged in a two-stage crystallization reactor, which allows the crystallization of aluminum chloride hexahydrate.
  • the flow rate of acid through these reactors is about 600 to about 675 m 3 /h and the reactor was maintained at about 50 to about 60° C. during this highly exothermic reaction. Heat was recovered and exchanged to the acid purification 107 part of the plant thus ensuring proper heat transfer and minimizing heat consumption of the plant.
  • Aluminum chloride solubility decreases rapidly, compared to other elements, with the increase in concentration of free HCl in the crystallization reactor. The concentration of AlCl 3 for precipitation/crystallization was about 30%
  • the HCl concentration during crystallization was thus about 30 to about 32% wt.
  • the aqueous solution from the crystallization stage 104 was then submitted to the hydrothermal acid recovery plant 105 , while the crystals are processed through the decomposition/calcination stage in the calcination plant 106 .
  • a one-step crystallization stage or a multi-step crystallization stage can be done.
  • a two-steps crystallization stage can be carried out.
  • the calcination 106 comprises the use of a two-stage circulating fluid bed (CFB) with preheating systems.
  • the preheating system can comprise a plasma torch to heat up steam to process. It processes crystals in the decomposition/calcination stage. The majority of the hydrochloric acid was released in the first stage which was operated at a temperature of about 350° C., while the second stage performs the calcination itself. Acid from both stages (about 66 to about 68% of the recovered acid from the processes) was then recovered and sent to either to the acid leaching 102 or to the acid purification 107 .
  • CFB circulating fluid bed
  • iron oxides productions and acid recovery 105 system which comprises, aqueous solution from the crystallization 104 first undergoes a pre-concentration stage followed by processing in the hydrolyzer reactor.
  • hematite was produced during low temperature processing (about 165° C.).
  • a recirculation loop was then taken from the hydrolyzer and is recirculated to the pre-concentrator, allowing the concentration of REE, Mg, K, and other elements.
  • This recirculation loop allows rare earth element chlorides and/or rare metal chlorides and various metal chlorides concentration to increase without having these products precipitating with hematite up to a certain extent.
  • Table 5 shows results obtained in stage 106 .
  • the reactants were oxalic acid, NaOH, DEHPA (Di-(2-ethylhexyl)phosphoric acid) and TBP (tri-n-butyl phosphate) organic solution, kerosene, and HCl were used to convert rare earth element chlorides and rare metals chlorides to hydroxides.
  • a ion exchange technique is also capable of achieving same results as polytrimethylene terephtalate (PET) membrane.
  • Iron powder from 105, or scrap metal as FeO can be used at a rate dependent on Fe 3+ concentration in the mother liquor.
  • HCl (100% wt) at the rate of 1 tph can be required as the stripped solution in REE Solvent Extraction (SX) separation and re-leaching of rare earth elements and/or rare metals oxalates.
  • Oxalic acid as di-hydrate at a rate of 0.2 tph was added and contributes to the rare earth elements and rare metals oxalates precipitation.
  • NaOH or MgOH at a rate of 0.5 tph can be used as a neutralization agent.
  • DEHPA SX organic solution at the rate of 500 g/h was used as active reagent in rare earth elements separation while TBP SX organic solution at the rate of 5 kg/h is used as the active reagent for gallium recovery and yttrium separation. Finally, a kerosene diluent was used at the rate of approximately 2 kg/h in all SX section. Calcination occurs in an electric rotary furnace via indirect heating to convert contents to REE 2 O 3 (oxides form) and maintain product purity.
  • stage 108 can be carried out as described in WO/2012/126092 and/or WO/2012/149642, that are hereby incorporated by reference in their entirety.
  • the solution after stages 108 and 109 contained mainly MgCl 2 , NaCl, KCl, CaCl 2 , FeCl 2 /FeCl 3 , and AlCl 3 (traces), and then undergoes the 111 stage.
  • Na, K, Ca that follows the MgO can be extracted in stage 110 by crystallization in a specific order; Na first, followed by K, and then Ca.
  • This technique can be employed for example in the Israeli Dead Sea salt processing plant to produce MgO and remove alkali from the raw material.
  • the process chosen for the conversion can generate value-added products
  • NaCl and KCl with intent of recovering HCl.
  • One example can be to contact them with highly concentrated sulfuric acid (H 2 SO 4 ), which generates sodium sulphate (Na 2 SO 4 ) and potassium sulfate (K 2 SO 4 ), respectively, and regenerates HCl at a concentration above 90% wt.
  • H 2 SO 4 highly concentrated sulfuric acid
  • K 2 SO 4 potassium sulfate
  • Another example is the use of a sodium and potassium chloride brine solution as the feed material to adapted small chlor-alkali electrolysis cells. In this latter case, common bases (NaOH and KOH) and bleach (NaOCl and KOCl) are produced.
  • the electrolysis of both NaCl and KCl brine is done in different cells where the current is adjusted to meet the required chemical reaction.
  • the reduced flow which was substantially free of most elements (for example AlCl 3 , FeCl 3 , REE-CI, NaCl, KCl) and rich in MgCl 2 , was then submitted to the magnesium oxides plant 111 .
  • MgO pyrohydrolysis of MgCl 2 and any other leftover impurities were converted into oxide while regenerating acid.
  • the first step was a pre-evaporator/crystallizer stage in which calcium is removed and converted into gypsum (CaSO 4 .2H 2 O) by a simple chemical reaction with sulfuric acid, for which separation of MgO is required. This increases the capacity of MgO roasting and also energy consumption slightly, while substantially recovering HCl.
  • the next step was the specific pyrohydrolysis of MgO concentrated solution by spray roasting.
  • Two (2) main products were generated; MgO that was further treated and HCl (about 18% wt.), which was either recycled back to the upstream leaching stage 102 or to the hydrochloric acid purification plant ( 107 )
  • the MgO-product derived from the spray roaster can require further washing, purification, and finally calcining depending on the quality targeted.
  • the purification and calcining can comprise a washing-hydration step and standard calcining step.
  • the MgO from the spray roaster is highly chemically active and was directly charged into a water tank where it reacts with water to form magnesium hydroxide, which has poor solubility in water.
  • the Mg(OH) 2 suspension after settling in a thickener, was forwarded to vacuum drum filters, which remove the remaining water.
  • the cleaned Mg(OH) 2 is then forwarded into a calcination reactor where it is exposed to high temperatures in a vertical multi-stage furnace. Water from hydration is released and allows the transformation of the Mg(OH) 2 to MgO and water. At this point, the magnesium oxide was of high purity (>99%).
  • the hydrochloric acid purification stage 107 is effective for purifying HCl regenerated from different sectors (for example 105, 106, 111) and to increase its purity for crystallization, whereas dry highly concentrated acid (>90% wt.) can be used as the sparging agent. Stage 107 also allowed for controlling the concentration of the acid going back to stage 102 (about 22 to about 32% wt.) and allows total acid and water balance. Total plant water balance is performed mainly by reusing wash water as absorption medium, as quench agent or as dissolution medium at the crystallization stages.
  • HCl purification can be carried out as shown in FIGS. 4 and 5 .
  • purification can be carried out by means of a membrane distillation process.
  • the membrane distillation process applied here occurs when two aqueous liquids with different temperatures are separated through a hydrophobic membrane.
  • the driving force of the process was supplied by the partial pressure vapour difference caused by the temperature gradient between these solutions. Vapour travels from the warm to the cold side.
  • the separation mechanism was based on the vapour/liquid equilibrium of the HCl/water liquid mixture. Practical application of such a technology has been applied to HCl/water, H 2 SO 4 /water systems and also on large commercial scales on aqueous solution of sodium chloride with the purpose of obtaining potable water from seawater and nano water production.
  • membrane distillation was a separation process based on evaporation through a porous hydrophobic membrane. The process was performed at about 60° C. and was effective to recover heat from the 104 and 102 stage with an internal water circulation loop, in order to maintain a constant incoming temperature to the membranes. For example, eight membranes of 300,000 m 2 equivalent surface area can be used per membrane to obtain a concentration of HCl well above the azeotropic point (i.e. >36%) of the ⁇ 750 m 3 /h and final 90% concentration is then obtained through pressure distillation (rectification column).
  • stage 107 was operated at about 60° C. and heat input provided by heat recovery from stages 102 to 110 .
  • Rectification column was operated at about 140° C. in the reboiler part. Net energy requirement was neutral (negative in fact at ⁇ 3.5 Gj/t Al 2 O 3 ) since both systems were in equilibrium and in balance.
  • the acid purification can be carried out by using adsorption technology over an activated alumina bed.
  • adsorption technology In continuous mode, at least two adsorption columns are required to achieve either adsorption in one of them and regeneration in the other one.
  • Regeneration can be performed by feeding in counter-current a hot or depressurized gas. This technology will result in a purified gas at 100% wt.
  • the acid purification can be made by using calcium chloride as entrainer of water.
  • a lean hydrochloric acid solution is contacted with a strong calcium chloride solution through a column.
  • the water is then removed from the hydrochloric acid solution and 99.9% gaseous HCl comes out of the process.
  • Cooling water and cryogenic coolant is used to condense water traces in the HCl.
  • the weak CaCl 2 solution is concentrated by an evaporator that ensures the recuperation of calcium chloride.
  • some metals can contaminate the calcium chloride concentrated solution.
  • a precipitation with Ca(OH) 2 and a filtration allows the removal of those impurities.
  • the column can operate for example at 0.5 barg. This technology can allow for the recuperation of 98% of the HCl.
  • Table 7 shows the results obtained concerning the process shown in FIG. 6 .
  • Tables 8 to 26 show results obtained concerning the products made in accordance with the process shown in FIG. 6 in comparison with standard of the industry.
  • P 2 O 5 removal technique can include, for example, after leaching, phosphorous precipitation using zirconium sulphate. It can be provided, for example, in a solution heated at 80 to about 90° C. or about 85 to about 95° C., under vacuum.
  • REE-O/RM-O PSD mean 2-30 ⁇ m Density 5500-13000 kg/m 3 LOI ⁇ 1%
  • Another starting material has been used for preparing acidic compositions comprising various components.
  • a material that is a concentrate of rare earth elements and rare metals (particularly rich in zirconium) has been tested.
  • Table 27 shows the results carried out on such a starting material using a similar process as shown in FIGS. 1, 3, 6 and 7 and as detailed in Examples 1, 2 and 5. It can thus be inferred from the results shown in Table 27 that the various components present in the leaching (various metals such as aluminum, iron, magnesium as well as rare earth elements and rare metals) can be extracted from the obtained leaching composition and that they can eventually be isolated by the processes of the present disclosure such as, for example, those presented in Examples 1, 2 and 5.
  • the process shown in FIG. 8 is similar to the process of FIG. 1 , with the exception that in FIG. 8 , the term “aluminum” is replaced by a “first metal”.
  • the first metal can be chosen from Al, Fe, Ti, Zn, Ni, Co, Mg, Li, Mn, Cu, Au, Ag, Pd, Pt. and mixtures thereof etc. Such a process can thus be used for recovering various other metals than aluminum.
  • the first metal will be precipitated as a chloride in stage 5 and eventually converted into an oxide.
  • the person skilled in the art would understand that by replacing in FIGS. 1, 3, 6 and 7 the term “aluminum” with the expression “first metal” the processes shown in these figures can be used to obtain various other products than alumina and also used for treating various different starting material.
  • the first metal can be recovered as a chloride (as it is the case for aluminum chlorides in the processes of FIGS. 1, 3, 6 and 7 ) and all the other stages of these processes can thus be carried out (when applicable) depending on the nature of the starting material used.
  • the first metal chloride can be precipitated or crystallized.
  • the first metal can be removed from the leachate in various manner.
  • a precipitating agent can be added or HCl (for example gaseous) can be reacted with the liquid obtained from step 3 so as to cause precipitation and/or crystallization of the first metal chloride.
  • the temperature of the leachate can be controlled so as to substantially selectively cause precipitation of the first metal chloride. This can also be done, for example, by using an ion exchange resin, by adding a precipitating agent, etc. Combinations of various possibilities mentioned in this paragraph can also be envisaged. All these methods of at least substantially selectively recovering the first metal chloride can also be applied on the first metal oxide.
  • the liquid obtained after stage 4 can be treated so as to convert the second metal chloride into the corresponding oxide and then, the second metal oxide can be substantially selectively recovered by selectively precipitating and/or crystalizing such a second metal oxide, for example by controlling the temperature, by using an ion exchange resin, by adding a precipitating agent, by adding HCl, or mixtures thereof.
  • the processes of the present disclosure can be efficient for treating material comprising Al, Fe, Ti, Zn, Ni, Co, Mg, Li, Mn, Cu, Au, Ag, Pd, Pt.
  • the material when treating a material that comprises, for example, Mg and Fe, the material can be leached for example by using HCl. Then, while the mixture (comprising a solid and a liquid) so obtained is still hot, it can be treated so as to separate the solid from the solid (for example by means of a solid/liquid separation). That will be effective for removing solids such as Si and optionally others such as Ti.
  • the liquid can be cooled down to a temperature of about 5 to about 70° C., about 10 to about 60° C., about 10 to about 50° C., about 10 to about 40° C., or about 15 to about 30° C.
  • the expression “iron oxides” in step 6 can be replaced in FIG. 8 by “second metal oxide”.
  • second metal oxide another metal than iron could be recovered as an oxide pursuant, for example, to a treatment of the liquid obtained from step 4 .
  • the chloride of the second metal obtained from step 4 can be treated so as to substantially selectively recover the chloride of the second metal. This can be done, for example, by selectively precipitating and/or crystallizing such a second metal chloride by controlling the temperature, by substantially selectively hydrolyzing such a second metal chloride, by using an ion exchange resin, by adding a precipitating agent, by adding HCl, or mixtures thereof.
  • All these methods of at least substantially selectively recovering the second metal chloride can also be applied on the second metal oxide.
  • The can be applied to only the second metal chloride, only to the second metal oxide or to both of them.
  • the liquid obtained after stage 4 can be treated so as to convert the second metal chloride into the corresponding oxide and then, the second metal oxide can be substantially selectively recovered by selectively precipitating and/or crystalizing such a second metal oxide, for example by controlling the temperature, by using an ion exchange resin, by adding a precipitating agent, by adding HCl, or mixtures thereof.
  • the iron chloride can be treated by means of a pyrohydrolysis in order to generate Cl 2 .
  • the Cl 2 so produced can be used in step 13 of FIG. 8 for treating the solid that comprises Ti.
  • it can be used to convert TiO 2 into TiCl 4 .
  • Such a reaction can be carried under oxidizing conditions (for example more than 4% of O 2 ).
  • the pyrohydrolysis can be carried out in in a fluid bed reactor under such oxidizing conditions.
  • platinum and palladium can also be treated similarly.
  • their separation can also be accomplished with ion exchange: selective crystallization in HCl is possible and can be temperature sensitive.
  • FIGS. 9A and 9B show methods for separating Si from Ti.
  • leaching can be carried out in the presence of Cl 2 (optionally in the presence of carbon) so as to maintain Ti under the form of TiCl 4 since in remains in solution (fluid) while Si remains solid (SiO 2 ).
  • Ti such as TiCl 4
  • it can be injected into a plasma torch for being purified.
  • Such a method for purifying Si and Ti can be used in all the processes of the present disclosure when there is a need for separating these two entities. See stage 13 in FIGS. 1, 3 and 8 and stage 113 in FIGS. 6 and 7 .
  • the processes of the present disclosure can provide economical solutions that can successfully extract various products from various type of materials while providing ultra pure secondary products of high added value including highly concentrated rare earth elements and rare metals.
  • the technology described in the present disclosure can allow for an innovative amount of total acid recovery and also for a ultra high concentration of recovered acid. When combing it to the fact that combined with a semi-continuous leaching approach that favors very high extraction yields and allows a specific method of crystallization of some products, and concentration of other value added elements.
  • the crystallization of AlCl 3 into AlCl 3 .6H 2 O using dried, cleaned and highly concentrated gaseous HCl as the sparging agent allows for a pure aluminum chloride hexahydrate with only few parts per million of iron and other impurities. A minimal number of stages are required to allow proper crystal growth.
  • the processes allow for the production of substantially pure alumina and other value added products purified such as purified silica, pure hematite, titanium oxide, pure other minerals (ex: magnesium oxide) and rare earth elements products.
  • the processes do not necessary require thermal pre-treatment before the acid leach operation. Acid leach can be carried out using semi-continuous techniques with high pressure and temperature conditions and very high regenerated hydrochloric acid concentration.
  • the processes do not generate any residues not sellable, thus eliminating harmful residues to environment like in the case of alkaline processes.
  • the advantage of the high temperature calcination stage in addition for allowing to control the ⁇ -form of alumina required, can be effective for providing a concentration of hydrochloric acid in the aqueous form (>38%) that is higher than the concentration of HCl at the azeotropic point and thus providing a higher incoming HCl concentration to the leaching stage.
  • the calcination stage hydrochloric acid network can be interconnected to two (2) crystallization systems and by pressure regulation excess HCl can be being absorbed at the highest possible aqueous concentration.
  • the advantage of having a hexahydrate chloride with low moisture content ( ⁇ 2%) incoming feed can allow for a continuous basis to recover acid at a concentration that is higher than the azeotropic concentration. This HCl balance and double usage into three (3) common parts of the processes and above azeotropic point is a substantial advance in the art.
  • Another advantage can be the use of the incoming chemistry (ferric chloride) to the iron oxide and hydrochloric acid recovery unit where all excess heat load from any calcination part, pyrohydrolysis and leaching part is being recovered to preconcentrate the mother liquor in metal chloride, thus allowing, at very low temperature, the hydrolysis of the ferric chloride in the form of very pure hematite and the acid regeneration at the same concentration than at its azeotropic point.
  • ferric chloride iron oxide and hydrochloric acid recovery unit
  • the processes of the present disclosure can be effective for providing, at the ferric chloride hydrolysis step, the possibility to concentrate rare earth elements in form of chlorides at very high concentration within the hydrolyser reactor through an internal loop between hydrolyzer and crystallization.
  • the advantage in that the processes of the present disclosure benefit from the various steps where gradual concentration ratios are applied.
  • Another advantage of the processes can be a selective crystallization of MgCl 2 through the sparging of HCl. Highly concentrated acid both in gaseous phase or in aqueous form can thus be be generated. As previously indicated, Mg(OH) 2 can also be obtained.
  • the HCl gas very high concentration about 85 to about 95%, about 90 to 95% or about 90% by weight
  • the HCl gas very high concentration can allow for exact adjustment in continuous of the crystallizer based on quality of magnesium oxide targeted.
  • the pyrohydrolysis can allow for conversion of any remaining chloride and the production of refined oxides that can be used (in case of clay as starting material) as a fertilizer and allowing the processing of large amount of wash water from the processes with the recovery hydrochloric acid in close loop at the azeotropic point for the leaching step. This is related to the fact that it does totally close the process loop in terms of acid recovery and the insurance that no residues harmful to the environment are being generated while processing any type of raw material, as previously described.
  • the present disclosure provides fully integrated processes for the extraction and/or recovery of titanium and/or for the preparation of titanium chloride or titanium oxide using a hydrochloric acid treatment while producing high purity and high quality products (minerals) and optionally extracting rare earth elements and rare metals.

Abstract

There are provided processes for preparing various products from various materials. For example, such processes are effective for extracting various metals from various materials, thereby allowing for preparing products such as aluminum chloride, alumina, titanium chloride and titanium oxide. These processes can comprise leaching the starting material with HCl so as to obtain a leachate and a solid. The solid can be treated so as to substantially selectively extract titanium therefrom while the leachate can be treated so as to substantially selectively recover a first metal chloride therefrom.

Description

    CROSS-REFERENCE TO RELATED APPLICATIONS
  • The present application is a continuation of U.S. Ser. No. 14/413,940, filed on Jan. 9, 2015, that is a 35 USC 371 national stage entry of PCT/CA2013/000638 filed on Jul. 12, 2013, that claims priority on U.S. 61/670,645 filed on Jul. 12, 2012; on PCT/CA2012/000871 filed on Sep. 17, 2012; on U.S. 61/726,971 filed on Nov. 15, 2012; and on PCT/CA2013/000021 filed on Jan. 10, 2013. These documents are hereby incorporated by reference in their entirety.
    • TECHNICAL FIELD
  • The present disclosure relates to improvements in the field of chemistry applied to the production of alumina and/or titanium oxide. For example, it relates to processes for the production of alumina via the extraction of aluminum from aluminum-containing materials and production of titanium oxide via the extraction of titanium from titanium-containing materials. These processes can also be efficient for preparing other products such as hematite, MgO, silica and oxides of various metals, titanium chloride as well as rare earths and aluminum.
    • BACKGROUND OF THE DISCLOSURE
  • There have been several known processes for the production of alumina. Many of them were using bauxite as starting material. These processes, that were mainly alkaline processes, have been employed throughout the years. Several of such alkaline processes have the disadvantage of being inefficient to segregate and extract value added secondary products, thus leaving an important environmental impact. There have also been development work employing hydrochloric acid for the leaching step but, it has been found that such processes were not efficient for removing most part of the impurities and especially iron. Removal of iron was also difficult to be carried out via adequate and economical techniques especially when using continuous processes.
  • There have also been several processes proposed for preparing titanium oxide but there is still room for improvement.
    • SUMMARY OF THE DISCLOSURE
  • According to one aspect, there is provided a process for preparing various products, the process comprising:
      • leaching a titanium-containing material comprising Ti, Si and a first metal with HCl so as to obtain a leachate comprising ions of the first metal and a solid comprising titanium, and separating the solid from the leachate;
      • reacting the leachate with HCl so as to obtain a liquid and a precipitate comprising a chloride of the first metal, and separating the precipitate from the liquid;
      • heating the precipitate under conditions effective for converting the chloride of the first metal into an oxide of the first metal; and
      • treating the solid so as to substantially separate Si from Ti that are contained therein.
  • According to another aspect, there is provided a process for preparing alumina, the process comprising:
      • leaching an aluminum-containing material with HCl so as to obtain a leachate comprising aluminum ions and a solid, and separating the solid from the leachate;
      • reacting the leachate with HCl so as to obtain a liquid and a precipitate comprising the aluminum ions in the form of AlCl3, and separating the precipitate from the liquid;
      • heating the precipitate under conditions effective for converting AlCl3 into Al2O3 and optionally recovering gaseous HCl so-produced; and
      • leaching the solid with HCl optionally in the presence of a chloride so as to obtain a leachate comprising titanium ions.
  • According to another aspect, there is provided a process for preparing aluminum, the process comprising:
      • leaching an aluminum-containing material with HCl so as to obtain a leachate comprising aluminum ions and a solid, and separating the solid from the leachate;
      • reacting the leachate with HCl so as to obtain a liquid and a precipitate comprising the aluminum ions in the form of AlCl3, and separating the precipitate from the liquid;
      • heating the precipitate under conditions effective for converting AlCl3 into Al2O3 and optionally recovering gaseous HCl so-produced;
      • converting the Al2O3 into alumina; and
      • leaching the solid with HCl optionally in the presence of a chloride so as to obtain a leachate comprising titanium ions.
  • According to another aspect, there is provided a process for preparing alumina and optionally other products, the process comprising:
      • leaching an aluminum-containing material with HCl so as to obtain a leachate comprising aluminum ions and a solid, and separating the solid from the leachate;
      • reacting the leachate with HCl so as to obtain a liquid and a precipitate comprising the aluminum ions in the form of AlCl3, and separating the precipitate from the liquid;
      • heating the precipitate under conditions effective for converting AlCl3 into Al2O3 and recovering gaseous HCl so-produced;
      • recycling the gaseous HCl so-produced by contacting it with water so as to obtain a composition having a concentration higher that HCl azeotrope concentration (20.2 weight %) and reacting the composition with a further quantity of aluminum-containing material so as to leaching it; and
      • leaching the solid with HCl optionally in the presence of a chloride so as to obtain a leachate comprising titanium ions.
  • According to another aspect, there is provided a process for preparing alumina and optionally other products, the process comprising:
      • leaching an aluminum-containing material with HCl so as to obtain a leachate comprising aluminum ions and a solid, and separating the solid from the leachate;
      • reacting the leachate with HCl so as to obtain a liquid and a precipitate comprising the aluminum ions in the form of AlCl3, and separating the precipitate from the liquid;
      • heating the precipitate under conditions effective for converting AlCl3 into Al2O3 and recovering gaseous HCl so-produced;
      • recycling the gaseous HCl so-produced by contacting it with water so as to obtain a composition having a concentration of about 25 to about 45 weight % and reacting the composition with a further quantity of aluminum-containing material so as to leaching it; and
      • leaching the solid with HCl optionally in the presence of a chloride so as to obtain a leachate comprising titanium ions.
  • According to another aspect, there is provided a process for preparing titanium chloride, the process comprising:
      • leaching a titanium-containing material with HCl so as to obtain a leachate comprising ions from at least one metal and a solid, and separating the solid from the leachate;
      • at least substantially isolating the ions of the at least one metal from the leachate; and
      • leaching the solid with HCl optionally in the presence of a chloride so as to obtain a leachate comprising titanium chloride.
  • According to another aspect, there is provided a process for preparing titanium oxide, the process comprising:
      • leaching a titanium-containing material with HCl so as to obtain a leachate comprising ions from at least one metal and a solid, and separating the solid from the leachate;
      • at least substantially isolating the ions of the at least one metal from the leachate;
      • leaching the solid with HCl optionally in the presence of a chloride so as to obtain a leachate comprising titanium chloride; and
      • converting the titanium chloride into titanium oxide.
  • According to another example, there is provided a process for preparing titanium oxide, the process comprising:
      • leaching a titanium-containing material with HCl so as to obtain a first leachate comprising ions from at least one metal and a solid, and separating the solid from the first leachate;
      • at least substantially isolating the ions of the at least one metal from the first leachate;
      • leaching the solid with HCl optionally in the presence of a chloride so as to obtain a second leachate comprising titanium chloride; or reacting the solid with Cl2 and a carbon source so as to obtain a liquid portion comprising the titanium chloride and a solid portion, and separating the liquid portion form the solid portion; and
      • converting the titanium chloride into titanium oxide.
  • According to another example, there is provided a process for preparing titanium oxide, the process comprising:
      • leaching a titanium-containing material with HCl so as to obtain a first leachate comprising ions from at least one metal and a solid, and separating the solid from the first leachate;
      • at least substantially isolating the ions of the at least one metal from the first leachate;
      • leaching the solid with HCl optionally in the presence of a chloride so as to obtain a second leachate comprising titanium chloride; and
      • converting the titanium chloride into titanium oxide.
  • According to another example, there is provided a process for preparing titanium oxide, the process comprising:
      • leaching a titanium-containing material with HCl so as to obtain a first leachate comprising ions from at least one metal and a solid, and separating the solid from the first leachate;
      • at least substantially isolating the ions of the at least one metal from the first leachate;
      • reacting the solid with Cl2 so as to obtain a liquid portion comprising the titanium chloride and a solid portion, and separating the liquid portion form the solid portion; and
      • converting the titanium chloride into titanium oxide.
  • According to another example, there is provided a process for preparing titanium chloride, the process comprising:
      • leaching a titanium-containing material with HCl so as to obtain a first leachate comprising ions from at least one metal and a solid, and separating the solid from the first leachate;
      • at least substantially isolating the ions of the at least one metal from the leachate; and
      • leaching the solid with HCl optionally in the presence of a chloride so as to obtain a second leachate comprising titanium chloride.
  • According to another example, there is provided a process for preparing titanium chloride, the process comprising:
      • leaching a titanium-containing material with HCl so as to obtain a first leachate comprising ions from at least one metal and a solid, and separating the solid from the leachate;
      • at least substantially isolating the ions of the at least one metal from the first leachate; and
      • reacting the solid with Cl2 so as to obtain a liquid portion comprising the titanium chloride and a solid portion, and separating the liquid portion form the solid portion.
  • According to another example, there is provided a process for preparing various products, the process comprising:
      • leaching a titanium-containing material comprising Ti and a first metal with HCl so as to obtain a leachate comprising ions of the first metal and a solid comprising titanium, and separating the solid from the leachate;
      • substantially selectively recovering the first metal from the leachate; and
      • treating the solid so as at least partially recover Ti.
  • According to another example, there is provided a process for preparing various products, the process comprising:
      • leaching a titanium-containing material comprising Ti and Al with HCl so as to obtain a leachate comprising ions of Al and a solid comprising titanium, and separating the solid from the leachate;
      • substantially selectively recovering the Al from the leachate; and
      • treating the solid so as at least partially recover Ti.
  • According to another example, there is provided a process for preparing various products, the process comprising:
      • leaching a titanium-containing material comprising Ti and Fe with HCl so as to obtain a leachate comprising ions of Fe and a solid comprising titanium, and separating the solid from the leachate;
      • substantially selectively recovering the Fe from the leachate; and
      • treating the solid so as at least partially recover Ti.
  • According to another example, there is provided a process for preparing titanium oxide, the process comprising:
      • leaching a titanium-containing material with HCl so as to obtain a first leachate comprising Al ions and a solid, and separating the solid from the first leachate;
      • at least substantially isolating the Al ions from the first leachate;
      • leaching the solid with HCl optionally in the presence of a chloride so as to obtain a second leachate comprising titanium chloride; or reacting the solid with Cl2 so as to obtain a liquid portion comprising the titanium chloride and a solid portion, and separating the liquid portion form the solid portion; and
      • converting the titanium chloride into titanium oxide.
  • According to another example, there is provided a process for preparing titanium oxide, the process comprising:
      • leaching a titanium-containing material with HCl so as to obtain a first leachate comprising Al ions and a solid, and separating the solid from the first leachate;
      • at least substantially isolating the Al ions from the first leachate;
      • leaching the solid with HCl optionally in the presence of a chloride so as to obtain a second leachate comprising titanium chloride; and
      • converting the titanium chloride into titanium oxide.
  • According to another example, there is provided a process for preparing titanium oxide, the process comprising:
      • leaching a titanium-containing material with HCl so as to obtain a first leachate comprising Fe ions and a solid, and separating the solid from the first leachate;
      • at least substantially isolating the Fe ions from the first leachate;
      • leaching the solid with HCl optionally in the presence of a chloride so as to obtain a second leachate comprising titanium chloride; or reacting the solid with Cl2 so as to obtain a liquid portion comprising the titanium chloride and a solid portion, and separating the liquid portion form the solid portion; and
      • converting the titanium chloride into titanium oxide.
  • According to another example, there is provided a process for preparing titanium oxide, the process comprising:
      • leaching a titanium-containing material with HCl so as to obtain a first leachate comprising Al ions and a solid, and separating the solid from the first leachate;
      • at least substantially isolating the Al ions from the first leachate;
      • leaching the solid with HCl optionally in the presence of a chloride so as to obtain a second leachate comprising titanium chloride; and
      • converting the titanium chloride into titanium oxide.
  • According to another example, there is provided a process for preparing titanium oxide, the process comprising:
      • leaching a titanium-containing material with HCl so as to obtain a first leachate comprising Fe ions and a solid, and separating the solid from the first leachate;
      • at least substantially isolating the Fe ions from the first leachate;
      • leaching the solid with HCl optionally in the presence of a chloride so as to obtain a second leachate comprising titanium chloride; and
      • converting the titanium chloride into titanium oxide.
  • According to another example, there is provided a process for preparing titanium chloride, the process comprising:
      • leaching a titanium-containing material with HCl so as to obtain a first leachate comprising ions from at least one metal and a solid, and separating the solid from the first leachate;
      • at least substantially isolating the ions of the at least one metal from the leachate; and
      • leaching the solid with HCl optionally in the presence of a chloride so as to obtain a second leachate comprising titanium chloride.
  • According to another example, there is provided a process for preparing titanium chloride, the process comprising:
      • leaching a titanium-containing material with HCl so as to obtain a first leachate comprising ions from at least one metal and a solid, and separating the solid from the leachate;
      • at least substantially isolating the ions of the at least one metal from the first leachate; and
      • reacting the solid with Cl2 so as to obtain a liquid portion comprising the titanium chloride and a solid portion, and separating the liquid portion form the solid portion.
  • According to another aspect, there is provided a process for preparing alumina and optionally other products, the process comprising:
      • leaching an aluminum-containing material with HCl so as to obtain a leachate comprising aluminum ions and a solid, and separating the solid from the leachate;
      • reacting the leachate with HCl so as to obtain a liquid and a precipitate comprising the aluminum ions in the form of AlCl3, and separating the precipitate from the liquid;
      • heating the precipitate under conditions effective for converting AlCl3 into Al2O3 and recovering gaseous HCl so-produced; and
      • recycling the gaseous HCl so-produced by contacting it with water so as to obtain a composition having a concentration higher that HCl azeotrope concentration (20.2 weight %) and reacting the composition with a further quantity of aluminum-containing material so as to leaching it.
  • According to another aspect, there is provided a process for preparing alumina and optionally other products, the process comprising:
      • leaching an aluminum-containing material with HCl so as to obtain a leachate comprising aluminum ions and a solid, and separating the solid from the leachate;
      • reacting the leachate with HCl so as to obtain a liquid and a precipitate comprising the aluminum ions in the form of AlCl3, and separating the precipitate from the liquid;
      • heating the precipitate under conditions effective for converting AlCl3 into Al2O3 and recovering gaseous HCl so-produced; and
      • recycling the gaseous HCl so-produced by contacting it with water so as to obtain a composition having a concentration of about 25 to about 45 weight % and reacting the composition with a further quantity of aluminum-containing material so as to leaching it.
  • According to another aspect, there is provided a process for preparing alumina and optionally other products, the process comprising:
      • leaching an aluminum-containing material with HCl so as to obtain a leachate comprising aluminum ions and a solid, and separating the solid from the leachate;
      • reacting the leachate with HCl so as to obtain a liquid and a precipitate comprising the aluminum ions in the form of AlCl3, and separating the precipitate from the liquid;
      • heating the precipitate under conditions effective for converting AlCl3 into Al2O3 and recovering gaseous HCl so-produced; and
      • recycling the gaseous HCl so-produced by contacting it with water so as to obtain a composition having a concentration of about 25 to about 45 weight % and using the composition for leaching the aluminum-containing material.
  • According to another aspect, there is provided a process for preparing alumina and optionally other products, the process comprising:
      • leaching an aluminum-containing material with HCl so as to obtain a leachate comprising aluminum ions and a solid, and separating the solid from the leachate;
      • reacting the leachate with HCl so as to obtain a liquid and a precipitate comprising the aluminum ions in the form of AlCl3, and separating the precipitate from the liquid;
      • heating the precipitate under conditions effective for converting AlCl3 into Al2O3 and recovering gaseous HCl so-produced; and
      • recycling the gaseous HCl so-produced by contacting it with the leachate so as to precipitate the aluminum ions in the form of AlCl3.6H2O.
  • According to another aspect, there is provided a process for preparing alumina and optionally other products, the process comprising:
      • leaching an aluminum-containing material with HCl so as to obtain a leachate comprising aluminum ions and a solid, and separating the solid from the leachate;
      • reacting the leachate with HCl so as to obtain a liquid and a precipitate comprising the aluminum ions in the form of AlCl3, and separating the precipitate from the liquid; and
      • heating the precipitate under conditions effective for converting AlCl3 into Al2O3.
  • According to another aspect, there is provided a process for preparing alumina and optionally other products, the process comprising:
      • leaching an aluminum-containing material with HCl so as to obtain a leachate comprising aluminum ions and a solid, and separating the solid from the leachate;
      • reacting the leachate with HCl so as to obtain a liquid and a precipitate comprising the aluminum ions in the form of AlCl3, and separating the precipitate from the liquid; and
      • heating the precipitate under conditions effective for converting AlCl3 into Al2O3 and optionally recovering gaseous HCl so-produced.
  • According to one aspect, there is provided a process for preparing aluminum and optionally other products, the process comprising:
      • leaching an aluminum-containing material with HCl so as to obtain a leachate comprising aluminum ions and a solid, and separating the solid from the leachate;
      • reacting the leachate with HCl so as to obtain a liquid and a precipitate comprising the aluminum ions in the form of AlCl3, and separating the precipitate from the liquid;
      • heating the precipitate under conditions effective for converting AlCl3 into Al2O3; and
      • converting Al2O3 into aluminum.
  • According to another aspect, there is provided a process for preparing aluminum and optionally other products, the process comprising:
      • leaching an aluminum-containing material with HCl so as to obtain a leachate comprising aluminum ions and a solid, and separating the solid from the leachate;
      • reacting the leachate with HCl so as to obtain a liquid and a precipitate comprising the aluminum ions in the form of AlCl3, and separating the precipitate from the liquid;
      • heating the precipitate under conditions effective for converting AlCl3 into Al2O3 and optionally recovering gaseous HCl so-produced; and
      • converting Al2O3 into aluminum.
    BRIEF DESCRIPTION OF DRAWINGS
  • In the following drawings, which represent by way of example only, various embodiments of the disclosure:
  • FIG. 1 shows a bloc diagram of an example of process for preparing alumina and various other products according to the present disclosure;
  • FIG. 2 is an extraction curve for Al and Fe in which the extraction percentage is expressed as a function of a leaching time in a process according to an example of the present application;
  • FIG. 3 shows a bloc diagram of another example of process for preparing alumina and various other products according to the present disclosure;
  • FIG. 4 is a schematic representation of an example of a process for purifying/concentrating HCl according to the present disclosure;
  • FIG. 5 is a schematic representation of an example of a process for purifying/concentrating HCl according to the present disclosure;
  • FIG. 6 shows another bloc diagram of an example of process for preparing alumina and various other products according to the present disclosure;
  • FIG. 7 shows another bloc diagram of an example of process for preparing alumina and various other products according to the present disclosure;
  • FIG. 8 shows another bloc diagram of an example of process for preparing various products; and
  • FIGS. 9A and 9B show further bloc diagrams of examples of processes according to the present disclosure.
    •  DETAILED DESCRIPTION OF VARIOUS EMBODIMENTS
  • The following non-limiting examples further illustrate the technology described in the present disclosure.
  • In the processes of the present disclosure, the material can be, for example, a titanium-containing material.
  • In the processes of the present disclosure, the material can be, for example, an aluminum-containing material.
  • In the processes of the present disclosure, the material can be, for example, an iron-containing material.
  • The aluminum-containing material can be for example chosen from aluminum-bearing ores (such as clays, argillite, mudstone, beryl, cryolite, garnet, spinel, bauxite, or mixtures thereof can be used). The aluminum-containing material can also be a recycled industrial aluminum-containing material such as slag, red mud or fly ashes.
  • The titanium-containing material can be for example chosen from a titanium-bearing ores (such as ilmenite, rutile, anatase, brookite, perovskite, sphene, ecandrewsite, geikielite, pyrophanite or titanomagnetite or mixtures thereof can be used). The titanium-containing material can also be a recycled industrial titanium-containing material such as slag red mud or fly ashes.
  • For example, the material can be chosen from industrial refractory materials.
  • For example, the material chosen from aluminosilicate minerals.
  • The expression “red mud” as used herein refers to an industrial waste product generated during the production of alumina. For example, such a waste product can contain silica, aluminum, iron, calcium, titanium. It can also contains an array of minor constituents such as Na, K, Cr, V, Ni, Ba, Cu, Mn, Pb, Zn etc. For example, red mud can comprises about 15 to about 80% by weight of Fe2O3, about 1 to about 35% by weight Al2O3, about 1 to about 65% by weight of SiO2, about 1 to about 20% by weight of Na2O, about 1 to about 20% by weight of CaO, and up to about 35% by weight of TiO2. According to another example, red mud can comprise about 30 to about 65% by weight of Fe2O3, about 10 to about 20% by weight Al2O3, about 3 to about 50% by weight of SiO2, about 2 to about 10% by weight of Na2O, about 2 to about 8% by weight of CaO, and from 0 to about 25% by weight of TiO2.
  • The expression “fly ashes” as used herein refers to an industrial waste product generated in combustion. For example, such a waste product can contain various elements such as silica, oxygen, aluminum, iron, calcium. For example, fly ashes can comprise silicon dioxide (SiO2) and aluminium oxide (Al2O3). For example, fly ashes can further comprises calcium oxide (CaO) and/or iron oxide (Fe2O3). For example fly ashes can comprise fine particles that rise with flue gases. For example, fly ashes can be produced during combustion of coal. For example, fly ashes can also comprise at least one element chosen from arsenic, beryllium, boron, cadmium, chromium, chromium VI, cobalt, lead, manganese, mercury, molybdenum, selenium, strontium, titanium, thallium, and/or vanadium. For example, fly ashes can also comprise rare earth elements. For example, fly ashes can be considered as an aluminum-bearing material.
  • The expression “slag” as used herein refers to an industrial waste product comprising oxides such as oxides of aluminum, calcium, titanium, magnesium, iron, and/or silicon.
  • Terms of degree such as “about” and “approximately” as used herein mean a reasonable amount of deviation of the modified term such that the end result is not significantly changed. These terms of degree should be construed as including a deviation of at least ±5% or at least ±10% of the modified term if this deviation would not negate the meaning of the word it modifies.
  • The expression “titanium chloride” as used herein refers, for example, to a compound chosen from TiCl2, TiCl3 and TiCl4 and mixtures thereof. For example, it refers to TiCl4.
  • The term “hematite” as used herein refers, for example, to a compound comprising α-Fe2O3, γ-Fe2O3, β-FeO.OH or mixtures thereof.
  • The expression “iron ions” as used herein refers, for example to ions comprising to at least one type of iron ion chosen from all possible forms of Fe ions. For example, the at least one type of iron ion can be Fe2+, Fe3+, or a mixture thereof.
  • The expression “aluminum ions” as used herein refers, for example to ions comprising to at least one type of aluminum ion chosen from all possible forms of Al ions. For example, the at least one type of aluminum ion can be Al3+.
  • The expression “at least one aluminum ion”, as used herein refers, for example, to at least one type of aluminum ion chosen from all possible forms of Al ions. For example, the at least one aluminum ion can be Al3+.
  • The expression “at least one iron ion”, as used herein refers, for example, to at least one type of iron ion chosen from all possible forms of Fe ions. For example, the at least one iron ion can be Fe2+, Fe3+, or a mixture thereof.
  • The expression “at least one precipitated iron ion”, as used herein refers, for example, to at least one type of iron ion chosen from all possible forms of Fe ions that was precipitated in a solid form. For example, the at least one iron ion present in such a precipitate can be Fe2+, Fe3+, or a mixture thereof.
  • The expressions “substantially selectively recovering”, “substantially selectively recovered” and their equivalents as used herein when referring to recovering a compound refers, for example, to recovering or isolating such a compound together with less than 30, 25, 20, 15, 10, 5, 3, 2 or 1% of impurities. Such impurities can be other compounds such as other metals.
  • The expressions “substantially selectively precipitating”, “substantially selectively precipitate” and their equivalents as used herein when referring to precipitating a compound refers, for example, to precipitating such a compound together with less than 30, 25, 20, 15, 10, 5, 3, 2 or 1% of impurities. Such impurities can be other compounds such as other metals.
  • For example, the at least one metal can comprise a first metal that is chosen from aluminum, iron, zinc, copper, gold, silver, molybdenum, cobalt, magnesium, lithium, manganese, nickel, palladium, platinum, thorium, phosphorus, uranium and titanium, and/or at least one rare earth element and/or at least one rare metal.
  • For example, the first metal can be aluminum, iron, or magnesium.
  • For example, the liquid can comprise a second metal. For example, the liquid can comprise a third metal.
  • For example, the second metal can be chosen from aluminum, iron, zinc, copper, gold, silver, molybdenum, cobalt, magnesium, lithium, manganese, nickel, palladium, platinum, thorium, phosphorus, uranium and titanium, and/or at least one rare earth element and/or at least one rare metal.
  • For example, the process can comprise separating Si from Ti that are contained in the solid comprises leaching the solid with an acid so as to obtain a liquid portion comprising Ti and a solid portion containing Si and wherein the liquid portion is separated from the solid portion.
  • For example, the material can be leached with HCl having a concentration of about 15 to about 45 weight %, of about 20 to about 45 weight %, of about 25 to about 45 weight %, of about 26 to about 42 weight %, of about 28 to about 40 weight %, of about 30 to about 38 weight %, or between 25 and 36 weight %. For example, HCl at about 18 wt % or about 32 wt % can be used.
  • For example, the material can be leached with HCl having a concentration of about 1 M to about 12 M, about 2 M to about 10 M, about 3 M to about 9 M, about 4 M to about 8 M, about 5 M to about 7 M or about 6 M.
  • Leaching can also be carried out by adding dry highly concentrated acid (for example, 85%, 90% or 95%) in gas phase into the aqueous solution. Alternatively, leaching can also be carried out by using a weak acid solution (for example <3 wt %).
  • For example, leaching can be carried out by using HCl having a concentration of about 18 to about 32 wt % in a first reactor and then, by using HCl having concentration of about 90 to about 95% (gaseous) in a second reactor.
  • For example, leaching can be carried out by using HCl having a concentration of about 18 to about 32 wt % in a first reactor then, by using HCl having concentration of about 90 to about 95% (gaseous) in a second reactor; and by using HCl having concentration of about 90 to about 95% (gaseous) in a third reactor.
  • For example, leaching can be carried out under an inert gas atmosphere (for example argon or nitrogen).
  • For example, leaching can be carried out under an atmosphere of NH3.
  • For example, the material can be leached at a temperature of about 125 to about 225° C., about 140 to about 165° C., about 145 to about 160° C., about 150 to about 200° C., about 150 to about 190° C., about 160 to about 190° C., about 185 to about 190° C., about 160 to about 180° C., about 160 to about 175° C., or about 165 to about 170° C.
  • For example, the material can be leached at a pressure of about 4 to about 10 barg, about 4 to about 8 barg, or about 5 to about 6 barg.
  • For example, the material can be leached at a pressure of about 50 to about 150 psig, about 60 to about 100 psig, or about 70 to about 80 psig.
  • For example, the material can be leached with HCl having a concentration of about 10 to about 50 weight %, about 15 to about 45 weight %, of about 18 to about 45 weight % of about 18 to about 32 weight %, of about 20 to about 45 weight %, of about 25 to about 45 weight %, of about 26 to about 42 weight %, of about 28 to about 40 weight %, of about 30 to about 38 weight %, or between 25 and 36 weight %. For example, HCl at about 18 wt % or about 32 wt % can be used.
  • Leaching can also be carried out by adding dry highly concentrated acid (for example, 85%, 90% or 95%) in gas phase into the aqueous solution. Alternatively, leaching can also be carried out by using a weak acid solution (for example <3 wt %).
  • For example, leaching can be carried out by using HCl having a concentration of about 18 to about 32 wt % in a first reactor and then, by using HCl having concentration of about 90 to about 95%, or about 95 to about 100% (gaseous) in a second reactor.
  • For example, leaching can be carried out by using HCl having a concentration of about 18 to about 32 wt % in a first reactor then, by using HCl having concentration of about 90 to about 95% (gaseous) in a second reactor; and by using HCl having concentration of about 90 to about 95% (gaseous) in a third reactor.
  • For example, leaching can be carried out under an inert gas atmosphere (for example argon or nitrogen).
  • For example, leaching can be carried out under an atmosphere of NH3.
  • For example a first leaching can be carried out at atmospheric pressure and then, at least one further leaching (for example 1, 2 or 3 subsequent leaching steps) can be carried out under pressure.
  • For example, the material can be leached at a temperature of about 125 to about 225° C., about 150 to about 200° C., about 160 to about 180° C., or about 165 to about 170° C.
  • For example, the material can be leached at a temperature of about 125 to about 225° C., about 140 to about 165° C., about 145 to about 160° C., about 150 to about 200° C., about 150 to about 190° C., about 160 to about 190° C., about 185 to about 190° C., about 160 to about 180° C., about 160 to about 175° C., or about 165 to about 170° C.
  • For example, leaching can be a continuous leaching or semi-continous.
  • For example, the processes can further comprise recycling the gaseous HCl so-produced by contacting it with water so as to obtain a composition having a concentration of about 18 to about 45 weight %, about 26 to about 42 weight %, about 25 to about 45 weight %, about 28 to about 40 weight %, about 30 to about 38 weight %, about 18 to about 36%, or about 25 to about 36%.
  • For example, the processes can further comprise recycling the gaseous HCl so-produced by contacting it with water so as to obtain a composition having a concentration of about 18 to about 45 weight % or about 25 to about 45 weight % and using the composition for leaching the material.
  • For example, the liquid can comprise iron chloride. Iron chloride can comprise at least one of FeCl2, FeCl3, and a mixture thereof.
  • For example, the iron chloride can be hydrolyzed into iron oxide.
  • For example, iron chloride can be hydrolyzed into hematite.
  • For example, the liquid can have an iron chloride concentration of at least 30% by weight; and can then be hydrolyzed at a temperature of about 155 to about 350° C.
  • For example, the liquid can be concentrated to a concentrated liquid having an iron chloride concentration of at least 30% by weight; and then the iron chloride can be hydrolyzed at a temperature of about 155 to about 350° C. while maintaining a ferric chloride concentration at a level of at least 65% by weight, to generate a composition comprising a liquid and precipitated hematite, and recovering the hematite.
  • For example, non-hydrolysable elements with hematite can be concentrated back to a concentration of about 0.125 to about 52% wt. in circulation loop in view of selective extraction.
  • For example, the liquid can be concentrated to a concentrated liquid having a concentration of the at least one iron chloride of at least 30% by weight; and then hydrolyzed at a temperature of about 155 to about 350° C.
  • For example, the at least one iron chloride can be hydrolyzed at a temperature of about, 150 to about 175, 160 to about 175, 155 to about 170, 160 to about 170 or 165 to about 170° C.
  • For example, the liquid can be concentrated to a concentrated liquid having a concentration of the at least one iron chloride of at least 30% by weight; and then the at least one iron chloride is hydrolyzed at a temperature of about 155 to about 350° C. while maintaining a ferric chloride concentration at a level of at least 65% by weight, to generate a composition comprising a liquid and precipitated hematite, and recovering the hematite.
  • For example, the liquid can be concentrated to a concentrated liquid having an iron chloride concentration of at least 30% by weight; and then the iron chloride can be hydrolyzed at a temperature of about 155 to about 350° C. while maintaining a ferric chloride concentration at a level of at least 65% by weight, to generate a composition comprising a liquid and precipitated hematite; recovering the hematite; and recovering rare earths from the liquid.
  • Alternatively, iron chloride can be treated by pyrohydrolysis so as to generate Cl2. For example, such a pyrohydrolysis can be carried out under oxidizing conditions (for example O2 can be present at a concentration of at least 4, 5, 6, 7, 8, 9, or 10% by weight). Such a reaction can be described as follows:
  • Figure US20160153067A1-20160602-C00001
  • For example, such a pyrohydrolysis can be carried out in a fluid bed reactor. For example, the Cl2 so produced can eventually used for treating the solid comprising Ti.
  • For example, iron chloride can be pyrohydrolzed so as to generate Cl2.
  • For example, the Cl2 so generated can be used for treating said solid and to react with said Ti contained therein.
  • For example, Cl2 so generated can be used for treating said solid and to react with TiO2 contained in said solid, thereby producing TiCl4.
  • For example, said Fe ions can be substantially selectively extracted by converting them into Fe2O3 via an hydrolysis.
  • For example, said Fe ions can be substantially selectively extracted by converting them into Fe2O3 via a pyrohydrolysis that allows for generating Cl2.
  • For example, said Fe ions can be substantially selectively isolated by converting them into Fe2O3 via a pyrohydrolysis that allows for generating Cl2.
  • For example, said Cl2 so produced can be effective for treating said solid so as to obtain said liquid portion comprising the titanium chloride.
  • For example, the process can further comprise, after recovery of the rare earths, reacting the liquid with HCl so as to cause precipitation of MgCl2, and recovering same.
  • For example, the processes can further comprise calcining MgCl2 into MgO.
  • For example, the processes can further comprise calcining MgCl2 into MgO and recycling the gaseous HCl so-produced by contacting it with water so as to obtain a composition having a concentration of about 25 to about 45 weight % or about 18 to about 45 weight % and using the composition for leaching the red mud.
  • For example, the processes can further comprises, after recovery of the rare earths, reacting the liquid with HCl, and substantially selectively precipitating Na2SO4. For example, Na2SO4 can be precipitated by reacting the liquid with H2SO4.
  • For example, the processes can further comprises, after recovery of the rare earths, reacting the liquid with HCl, and substantially selectively precipitating K2SO4. For example, K2SO4 can be precipitated by adding H2SO4.
  • For example, the liquid can be concentrated to a concentrated liquid having an iron chloride concentration of at least 30% by weight; and then the iron chloride can be hydrolyzed at a temperature of about 155 to about 350° C. while maintaining a ferric chloride concentration at a level of at least 65% by weight, to generate a composition comprising a liquid and precipitated hematite; recovering the hematite; and reacting the liquid with HCl. For example, such a process can further comprises reacting the liquid with H2SO4 so as to substantially selectively precipitate K2SO4. The processes can also comprise further reacting the liquid with H2SO4 so as to substantially selectively precipitating K2SO4.
  • For example, the processes can comprise reacting dry individual salts (for example Na or K salts) obtained during the processes with H2SO4 and recovering HCl while producing marketable K2SO4 and Na2SO4 and recovering hydrochloric acid of about 15 to about 90% wt.
  • For example, sodium chloride produced in the processes can undergo a chemical reaction with sulfuric acid so as to obtain sodium sulfate and regenerate hydrochloric acid. Potassium chloride can undergo a chemical reaction with sulfuric acid so as to obtain potassium sulfate and regenerate hydrochloric acid. Sodium and potassium chloride brine solution can alternatively be the feed material to adapted small chlor-alkali electrolysis cells. In this latter case, common bases (NaOH and KOH) and bleach (NaOCl and KOCl) are produced.
  • For example, the processes can further comprise, after recovery of the rare earth elements and/or rare metals, recovering NaCl from the liquid, reacting the NaCl with H2SO4, and substantially selectively precipitating Na2SO4.
  • For example, the processes can further comprise, downstream of recovery of the rare earth elements and/or rare metals, recovering KCl from the liquid, reacting the KCl with H2SO4, and substantially selectively precipitating K2SO4.
  • For example, the processes can further comprise, downstream of recovery of the rare earth elements and/or rare metals, recovering NaCl from the liquid, carrying out an electrolysis to generate NaOH and NaOCl.
  • For example, the processes can further comprise, downstream of recovery of the rare earth elements and/or rare metals, recovering KCl from the liquid, reacting the KCl, carrying out an electrolysis to generate KOH and KOCl.
  • For example, the liquid can be concentrated to a concentrated liquid having a concentration of the at least one iron chloride of at least 30% by weight; and then the at least one iron chloride is hydrolyzed at a temperature of about 155 to about 350° C. while maintaining a ferric chloride concentration at a level of at least 65% by weight, to generate a composition comprising a liquid and precipitated hematite; recovering the hematite; and extracting NaCl and/or KCl from the liquid.
  • For example, the processes can further comprise reacting the NaCl with H2SO4 so as to substantially selectively precipitate Na2SO4.
  • For example, the processes can further comprise reacting the KCl with H2SO4 so as to substantially selectively precipitate K2SO4.
  • For example, the processes can further comprise carrying out an electrolysis of the NaCl to generate NaOH and NaOCl.
  • For example, the processes can further comprise carrying out an electrolysis of the KCl to generate KOH and KOCl.
  • For example, the processes can comprise separating the solid from the leachate and washing the solid so as to obtain silica having a purity of at least 95%, at least 96%, at least 97%, at least 98%, at least 99%, at least 99.5% or at least 99.9%.
  • For example, the process can comprise separating the solid from the leachate and washing the solid so as to obtain silica having a purity of at least 95%.
  • For example, the processes can comprise reacting the leachate with gaseous HCl so as to obtain the liquid and the precipitate comprising the first metal under the form of a chloride.
  • For example, the processes can comprise reacting the leachate with dry gaseous HCl so as to obtain the liquid and the precipitate comprising the first metal under the form of a chloride.
  • For example, precipitating AlCl3 can comprise crystallizing AlCl3.6H2O.
  • For example, the process can comprise reacting the leachate with HCl recovered during the process and a having a concentration of at least 30% as to obtain the liquid and the precipitate comprising the aluminum ions, the precipitate being formed by crystallization of AlCl3.6H2O.
  • For example, the first metal can be chosen from aluminum, iron, zinc, copper, gold, silver, molybdenum, cobalt, magnesium, lithium, manganese, nickel, palladium, platinum, thorium, phosphorus and uranium, and/or at least one rare earth element and/or at least one rare metal.
  • For example, the second metal can be iron or aluminum.
  • For example, the liquid can comprise a second metal.
  • For example, the second metal can be chosen from aluminum, iron, zinc, copper, gold, silver, molybdenum, cobalt, magnesium, lithium, manganese, nickel, palladium, platinum, thorium, phosphorus and uranium and titanium, and/or at least one rare earth element and/or at least one rare metal
  • For example, the second metal can be iron or aluminum.
  • For example, the process can comprise separating the precipitate from the liquid and heating the second metal in order to convert a chloride of the second metal into an oxide of the second metal.
  • For example, the processes can comprise:
  • separating the solid from the leachate;
  • leaching the solid with an acid so as to obtain another leachate; and
  • recovering a third metal from the another leachate.
  • For example, the third metal can be chosen from aluminum, iron, zinc, copper, gold, silver, molybdenum, cobalt, magnesium, lithium, manganese, nickel, palladium, platinum, thorium, phosphorus, uranium and titanium, and/or at least one rare earth element and/or at least one rare metal.
  • For example, the third metal can be titanium.
  • For example, the acid used for leaching can be chosen from HCl, HNO3, H2SO4 and mixtures thereof.
  • For example, the acid can be HCl.
  • For example, the acid can be gaseous HCl.
  • For example, the process can comprise recovering the third metal from the another leachate by precipitating the third metal.
  • For example, the third metal can be precipitated by reacting it with HCl.
  • For example, the process can further comprise heating the third metal in order to convert a chloride of the third metal into an oxide of the third metal.
  • For example, the first metal can be aluminum.
  • For example, the first metal can be magnesium.
  • For example, the first metal can be nickel.
  • For example, the second metal can be magnesium.
  • For example, the second metal can be nickel.
  • For example, the second metal can be iron.
  • For example, the processes can comprise controlling the temperature of the leachate so as to substantially selectively precipitate the first metal ions in the form of a chloride, and removing the precipitate from the leachate.
  • For example, the process can comprise reacting the leachate with HCl so as to obtain a liquid and a precipitate comprising a chloride of the first metal, and separating the precipitate from the liquid.
  • For example, controlling the temperature of the leachate so as to precipitate the first metal in the form of a chloride, and removing the precipitate from the leachate, can be carried out before reacting the leachate with HCl so as to obtain a liquid and a precipitate comprising a chloride of the second metal, and separating the precipitate from the liquid.
  • For example, controlling the temperature of the leachate so as to precipitate the first metal in the form of a chloride, and removing the precipitate from the leachate, can be carried out after reacting the leachate with HCl so as to obtain a liquid and a precipitate comprising a chloride of the second metal, and separating the precipitate from the liquid.
  • For example, reacting the leachate with HCl so as to obtain a precipitate comprising the first metal in the form of a chloride, can be carried out by substantially selectively precipitating the first metal chloride.
  • For example, reacting the leachate with HCl so as to obtain a precipitate comprising the second metal in the form of a chloride, can be carried out by substantially selectively precipitating the second metal chloride.
  • For example, controlling the temperature of the leachate so as to precipitate the first metal in the form of a chloride can be carried out substantially selectively.
  • For example, controlling the temperature of the leachate so as to precipitate the second metal in the form of a chloride can be carried out substantially selectively.
  • For example, controlling the concentration of HCl in the leachate and/or the temperature of the leachate so as to precipitate the first metal in the form of a chloride, can be carried out substantially selectively.
  • For example, controlling the concentration of HCl in the leachate and/or the temperature of the leachate so as to precipitate the second metal in the form of a chloride, can be carried out substantially selectively.
  • For example, the processes can comprise reacting the leachate with gaseous HCl so as to obtain the liquid and the precipitate comprising the aluminum ions in the form of AlCl3.6H2O.
  • For example, the processes can comprise reacting the leachate with dry gaseous HCl so as to obtain the liquid and the precipitate comprising the aluminum ions in the form of AlCl3.6H2O.
  • For example, the processes can comprise reacting the leachate with acid of at least 30% wt. that was recovered, regenerated and/or purified as indicated in the present disclosure so as to obtain the liquid and the precipitate comprising the aluminum ions in the form of AlCl3.6H2O.
  • For example, the processes can comprise reacting the leachate with gaseous HCl so as to obtain the liquid and the precipitate comprising the aluminum ions, the precipitate being formed by crystallization of AlCl3.6H2O.
  • For example, the processes can comprise reacting the leachate with dry gaseous HCl so as to obtain the liquid and the precipitate comprising the aluminum ions, the precipitate being formed by crystallization of AlCl3.6H2O.
  • For example, aluminum ions can be precipitated under the form of AlCl3 (for example AlCl3.6H2O) in a crystallizer, for example, by adding HCl having a concentration of about 26 to about 32 wt %.
  • For example, the solid can be treated so as to separate Ti from Si contained therein.
  • For example, the gaseous HCl can have a HCl concentration of at least 85% wt. or at least 90% wt.
  • For example, the gaseous HCl can have a HCl concentration of about 90% wt., about 90% to about 95% wt. or about 90% to about 99% wt.
  • For example, during the crystallization of AlCl3.6H2O, the liquid can be maintained at a concentration of HCl of about 25 to about 35% by weight or about 30 to about 32% by weight.
  • For example, the crystallization can be carried out at a temperature of about 45 to about 65° C. or about 50 to about 60° C.
  • For example, crystallization of AlCl3.6H2O can be carried out by adding concentrated gaseous HCl to reach a proprietary concentration established of free HCl in the crystalliser. The average results obtained from the crystals For example, the hexahydrate crystals can be fed to the calcination unit. AlCl3 hydrolysis and conversion can occur at very low temperature (<200° C.). The crystals can pass through a first step where decomposition occurs followed by the calcination itself. The circulating fluid bed can be operated such that energy consumption is less than 30% of the energy normally required for hexahydrate crystal calcination. The alumina produced can be washed to remove unconverted salt if required.
  • For example, the HCl can be obtained from the gaseous HCl so-produced.
  • For example, in the processes of the present disclosure, a given batch or quantity of the aluminum-containing material will be leached, will then be converted into AlCl3 and when the HCl generated during calcination of AlCl3 into Al2O3 will be used for example to leach another given batch or quantity of the aluminum-containing material.
  • For example, the processes can comprise heating the precipitate at a temperature of at least 180, 230, 250, 300, 350, 400, 450, 500, 550, 600, 650, 700, 750, 800, 850, 900, 925, 930, 1000, 1100, 1200 or 1250° C. for converting AlCl3 into Al2O3.
  • For example, converting AlCl3 into Al2O3 can comprise calcination of AlCl3.
  • For example, calcination is effective for converting AlCl3 into beta-Al2O3.
  • For example, calcination is effective for converting AlCl3 into alpha-Al2O3.
  • For example, converting AlCl3 into Al2O3 can comprise carrying out a calcination via a two-stage circulating fluid bed reactor.
  • For example, converting AlCl3 into Al2O3 can comprise carrying out a calcination via a two-stage circulating fluid bed reactor that comprises a preheating system.
  • For example, converting AlCl3 into Al2O3 can comprise carrying out a calcination at low temperature, for example, about 300 to about 600° C., about 325 to about 550° C., about 350 to about 500° C., about 375 to about 450° C., about 375 to about 425° C., or about 385 to about 400° C. and/or injecting steam.
  • For example, converting AlCl3 into Al2O3 can comprise carrying out a calcination at low temperature, for example, at least 180° C., at least 250° C., at least 300° C., at least 350° C. and/or injecting steam.
  • For example, converting AlCl3 into Al2O3 can comprise carrying out a calcination at low temperature, for example, less than 600° C. and/or injecting steam.
  • For example, converting AlCl3 into Al2O3 can comprise carrying out a calcination by using coal as combustion source and by using a degasification unit.
  • For example, the process can comprise converting AlCl3.6H2O into Al2O3 by carrying out a calcination of AlCl3.6H2O, the calcination comprising steam injection.
  • For example, steam (or water vapor) can be injected at a pressure of about 200 to about 700 psig, about 300 to about 700 psig, about 400 to about 700 psig, about 550 to about 650 psig, about 575 to about 625 psig, or about 590 to about 610 psig.
  • For example, steam (or water vapor) can be injected and a plasma torch can be used for carrying fluidization.
  • For example, the steam (or water vapor) can be overheated.
  • For example, the steam (or water vapor) can be at a temperature of about 300 to about 400° C.
  • For example, acid from the offgases generated during calcination can be then treated via a gas phase purification process.
  • For example, converting AlCl3 into Al2O3 can comprise carrying out a calcination by means of carbon monoxide (CO).
  • For example, converting AlCl3 into Al2O3 can comprise carrying out a calcination by means of a Refinery Fuel Gas (RFG).
  • For example, calcination can be carried out by injecting water vapor or steam and/or by using a combustion source chosen from fossil fuels, carbon monoxide, a Refinery Fuel Gas, coal, or chlorinated gases and/or solvants.
  • For example, calcination can be carried out by injecting water vapor or steam and/or by using a combustion source chosen from natural gas or propane.
  • For example, calcination can be carried out by providing heat by means of electric heating, gas heating, microwave heating.
  • For example, the processes can comprise precipitating the Al3+ ions under the form of Al(OH)3. For example, precipitating the Al3+ under the form of Al(OH)3 is carried out at a pH of about 7 to about 10; about 9 to about 10; about 9.2 to about 9.8; about 9.3 to about 9.7; about 9.5; 7.5 to about 8.5; about 7.8 to about 8.2; or about 8.
  • For example, the iron ions can be precipitated at a pH greater than 11, a pH greater than 12, a pH comprised between 10 and 11, a pH about 11.5 to about 12.5, or a pH about 11.8 to about 12.0.
  • For example, the Al3+ ions can be purified.
  • For example, the process can comprise precipitating Al3+ ions under the form of AlCl3 so as to purify the Al3+ ions. For example, precipitating AlCl3 can be carried out by crystallizing the AlCl3 under the form of AlCl3.6H2O.
  • For example, the process can comprise converting AlCl3 into Al2O3, for example, by converting AlCl3 into Al2O3 under an inert gas atmosphere or by converting AlCl3 into Al2O3 under a nitrogen atmosphere.
  • The obtained alumina can be washed by demineralized water so as to at least partially remove NaCl and/or KCl.
  • For example, the fluid bed reactor can comprise a metal catalyst chosen from metal chlorides.
  • For example, thee fluid bed reactor can comprise a metal catalyst that is FeCl3, FeCl2 or a mixture thereof.
  • For example, the fluid bed reactor can comprise a metal catalyst that is FeCl3.
  • For example, the preheating system can comprise a plasma torch.
  • For example, steam can be used as the fluidization medium heating. Heating can also be electrical.
  • For example, a plasma torch can be used for preheating the calcination reactor.
  • For example, a plasma torch can be used for preheating air entering in the calcination reactor.
  • For example, the plasma torch can be used for generating steam that is injected into a calcination reactor.
  • For example, the plasma torch can be effective for generating steam that is as fluidization medium in a fluid bed reactor.
  • For example, a plasma torch can be used for preheating a fluid bed.
  • For example, the calcination medium can be substantially neutral in terms of O2 (or oxidation). For example, the calcination medium can favorize reduction (for example a concentration of CO of about 100 ppm).
  • For example, the calcination medium is effective for preventing formation of Cl2.
  • For example, the processes can comprise converting AlCl3.6H2O into Al2O3 by carrying out a calcination of AlCl3.6H2O, for example, that is provided by the combustion of gas mixture that comprises:
  • CH4: 0 to about 1% vol;
  • C2H6: 0 to about 2% vol;
  • C3H8: 0 to about 2% vol,
  • C4H10: 0 to about 1% vol;
  • N2: 0 to about 0.5% vol;
  • H2: about 0.25 to about 15.1% vol;
  • CO: about 70 to about 82.5% vol; and
  • CO2: about 1.0 to about 3.5% vol.
  • Such a mixture can be efficient for reduction in off gas volume of 15.3 to 16.3%; therefore the capacity increases of 15.3 to 16.3% proven on practical operation of the circulating fluid bed. Thus for a same flow it represents an Opex of 0.65*16.3%=10.6%.
  • For example, the air to natural gas ratio of (Nm3/h over Nm3/h) in the fluid bed can be about 9.5 to about 10
  • For example, the air to CO gas ratio of (Nm3/h over Nm3/h) in the fluid bed can be about 2 to about 3.
  • For example, O2 can be substantially absent from the gas mixture.
  • For example, the processes can comprise, before leaching the material, a pre-leaching removal of fluorine optionally contained in the material.
  • For example, the HCl can obtained from the gaseous HCl so-produced.
  • For example, the processes can comprise heating the precipitate at a temperature of at least 1000, 1100, 1200 or 1250° C. for converting AlCl3 into Al2O3.
  • For example, in the processes of the present disclosure, a given batch or quantity of the material can be be leached, will then be converted into AlCl3 and when the HCl generated during calcination of AlCl3 into Al2O3 will be used for example to leach another given batch or quantity of the aluminum-containing material.
  • For example, the processes can be effective for providing an Al2O3 recovery yield of at least 93%, at least 94%, at least 95%, about 90 to about 95%, about 92 to about 95%, or about 93 to about 95%.
  • For example, the processes can be effective for providing a Fe2O3 recovery yield of at least 98%, at least 99%, about 98 to about 99.5%, or about 98.5 to about 99.5%.
  • For example, the processes can be effective for providing a MgO recovery yield of at least 96%, at least 97%, at least 98%, or about 96 to about 98%.
  • For example, the processes can be effective for providing a HCl recovery yield of at least 98%, at least 99%, or about 98 to about 99.9%.
  • For example, the aluminum-containing material can be argillite.
  • For example, the aluminum-containing material can be bauxite.
  • For example, the aluminum-containing material can be red mud.
  • For example, the processes can be effective for avoiding producing red mud.
  • For example, the alumina and the other products are substantially free of red mud.
  • For example, HCl can be recycled. For example, such a recycled HCl can be concentrated and/or purified.
  • For example, gaseous HCl can be concentrated and/or purified by means of H2SO4. For example, gaseous HCl can be passed through a packed column where it is contacted with a H2SO4 countercurrent flow. For example, by doing so, concentration of HCl can be increased by at least 50 wt %, at least 60 wt %, at least 70 wt %, at least 75 wt %, at least 80 wt %, about 50 wt % to about 80 wt %, about 55 wt % to about 75 wt %, or about 60 wt %. For example, the column can be packed with a polymer such as polypropylene or polytrimethylene terephthalate (PTT).
  • For example, gaseous HCl can be concentrated and/or purified by means of CaCl2. For example, gaseous HCl can be passed through a column packed with CaCl2.
  • For example, the processes can further comprise converting alumina (Al2O3) into aluminum. Conversion of alumina into aluminum can be carried out, for example, by using the Hall-Héroult process. References is made to such a well known process in various patents and patent applications such as US 20100065435; US 20020056650; U.S. Pat. No. 5,876,584; U.S. Pat. No. 6,565,733. Conversion can also be carried out by means of other methods such as those described in U.S. Pat. No. 7,867,373; U.S. Pat. No. 4,265,716; U.S. Pat. No. 6,565,733 (converting alumina into aluminum sulfide followed by the conversion of aluminum sulfide into aluminum.)
  • For example, the various products obtained by the processes of the present disclosure such as alumina, hematite, titanium oxides, magnesium oxides, rare earth elements and rare metals, etc can be further purified by means of a plasma torch. For example, they can be individually injected into a plasma torch so as to further purify them.
  • For example, converting AlCl3 into Al2O3 can comprise carrying out a one-step calcination.
  • For example, calcination can be carried out at different temperatures with steam. Temperature applied of superheated steam can be of about 350° C. to about 550° C. or about 350° C. to about 940° C. or about 350° C. to about 1200° C.
  • For example, multi stage evaporation step of the hydrolyser can be carried out to reduce drastically energy consumption.
  • For example, calcination can be carried out at very low temperature with steam.
  • For example, multi stage evaporation step of the hydrolyser can be carried out to reduce drastically energy consumption.
  • For example, leaching of the solid with HCl can be done so as to obtain a leachate comprising titanium ions (for example TiCl4).
  • For example, leaching of the solid with HCl can be done in the presence of a chloride so as to obtain a leachate comprising titanium ions (for example TiCl4). Such a leaching can be carried out as described in U.S. Pat. No. 7,803,336 and WO 2005049872. These documents are hereby integrated by reference in their entirety.
  • For example, the chloride can be magnesium chloride, calcium chloride or sodium chloride.
  • For example, the processes, when applicable, can further comprise converting titanium chloride into titanium oxide. Such a conversion can be carried out as described in U.S. Pat. No. 7,803,336 and WO 2005049872. These documents are hereby integrated by reference in their entirety.
  • For example, the processes can comprise leaching of the material with HCl so as to obtain the leachate comprising aluminum ions and the solid, separating the solid from the leachate; and further treating the solid so as to separate SiO2 from TiO2 that are contained therein.
  • For example, the processes can comprise leaching the material with HCl so as to obtain the leachate comprising aluminum ions and the solid, separating the solid from the leachate; and further treating the solid so as to separate Si from Ti that are contained therein.
  • For example, the processes can comprise leaching the material with HCl so as to obtain the leachate comprising aluminum ions and the solid, separating the solid from the leachate; and further treating the solid with HCl so as to separate Si from Ti that are contained therein.
  • For example, the process can comprise leaching the material with HCl so as to obtain the leachate comprising aluminum ions and the solid, separating the solid from the leachate; and further treating the solid with HCl, in the presence of a chloride (for example chosen from akali chlorides and alkaline earth chlorides), so as to separate Si from Ti that are contained therein.
  • For example, leaching of the solid with HCl in the presence of a chloride allows for obtaining a leachate comprising titanium chloride.
  • For example, the solid can be treated with HCl and the chloride so as to obtain a liquid portion comprising Ti and a solid portion containing Si and wherein the liquid portion is separated from the solid portion.
  • For example, the solid can be treated with HCl and the chloride so as to obtain a liquid portion comprising TiCl4.
  • For example, the process can further comprise converting TiCl4 into TiO2.
  • For example, TiCl4 can be converted into TiO2 by solvent extraction of the third liquid fraction and subsequent formation of titanium dioxide from the solvent extraction.
  • For example, TiCl4 can be reacted with water and/or a base to cause precipitation of TiO2.
  • For example, TiCl4 can be converted into TiO2 by means of a pyrohydrolysis, thereby generating HCl.
  • For example, TiCl4 can be converted into TiO2 by means of a pyrohydrolysis, thereby generating HCl that is recycled.
  • For example, TiCl4 can be converted into TiO2 by reacting TiCl4 with O2.
  • For example, TiCl4 can be converted into TiO2 by reacting TiCl4 with O2 under heating.
  • For example, HCl generated in the conversion of TiCl4 into TiO2 can be recovered.
  • For example, HCl generated in the conversion of TiCl4 into TiO2 can be recovered and reused for leaching the titanium-containing material or the solid
  • For example, the metal chloride can be MgCl2 or ZnCl2.
  • For example, the solid can comprise TiO2 and SiO2 and the solid can be treated with Cl2 and carbon in order to obtain a liquid portion and a solid portion, and wherein the solid portion and the liquid portion are separated from one another.
  • For example, the solid can comprise Ti and Si and the solid can be treated with Cl2 and carbon in order to obtain a liquid portion and a solid portion, and wherein the solid portion and the liquid portion are separated from one another.
  • For example, the solid can comprise TiO2 and SiO2 and the solid can be treated with Cl2 and carbon in order to obtain a liquid portion and a solid portion, and wherein the solid portion and the liquid portion are separated from one another.
  • For example, the solid can comprise Ti and Si and the solid can be treated with Cl2 in order to obtain a liquid portion and a solid portion, and wherein the solid portion and the liquid portion are separated from one another.
  • For example, the solid can comprise TiO2 and SiO2 and the solid can be treated with Cl2 in order to obtain a liquid portion and a solid portion, and wherein the solid portion and the liquid portion are separated from one another.
  • For example, the processes can comprise heating titanium chloride so as to convert it into TiO2.
  • For example, the liquid portion can comprise TiCl2 and/or TiCl4.
  • For example, the liquid portion can comprise TiCl4.
  • For example, the process can further comprise heating TiCl4 so as to convert it into TiO2.
  • For example, obtained TiO2 can be purified by means of a plasma torch.
  • For example, the solid can be treated as described in U.S. Pat. No. 7,182,931 (hereby incorporated by reference in its entirety) in order to obtain TiCl4 and then converting TiCl4 into TiO2. Regarding the conversion of TiCl4 into TiO2, examples of processes are also provided in U.S. Pat. No. 6,207,131, which is hereby incorporated in its entirety.
  • For example, the processes can comprise leaching the material with HCl so as to obtain the leachate comprising aluminum ions and the solid, separating the solid from the leachate; and further treating the solid with HCl at a concentration of less than 20% wt., at a temperature of less than 85° C., in the presence of a chloride, so as to separate Si from Ti that are contained therein.
  • For example, the chloride can be chosen from akali chlorides and alkaline earth chlorides.
  • For example, the chloride can be MgCl2 or CaCl2.
  • After the leaching, the titanium ions under the form of titanium chloride can be in a liquid phase and the Si remains solid. Therefore, Si can thus be simply separated from Ti by a solid/liquid separation. Then, titanium chloride can be converted into TiO2. It has to be noted that titanium oxychloride can also be present in the leachate.
  • Various methods of recovering titanium from a leachate are discussed in CA 2,513,309, which is hereby integrated by reference in its entirety.
  • For example, separation methods such as solvent extraction, precipitation or ion exchange can be used to remove impurities various impurities e. g. iron, chromium and vanadium, followed by recovery of titanium. Some of these techniques are discussed in the U.S. Pat. No. 6,500,396 (also integrated by reference in its entirety).
  • For example, in order to purify titanium ions, the leachate can be treated with an organic phase. The organic phase can be selected so that ions of a given can be selectively extracted into the organic phase, with titanium ions remaining in the aqueous solution. Thus, oxides of this given metal can also be obtained in high purity.
  • Examples of the organic phase are quaternary ammonium chlorides, amines (primary, secondary or tertiary), phosphoric and phosphinic acids, and esters and oxides thereof, e. g. tri-n-butyl phosphate, di-2-ethylhexyl phosphoric acid and phosphine oxide. The organic phase may be stripped from the iron values and recycled. Such an organic phase can be selected so that the titanium chloride can be soluble in the organic phase. For example, the organic phase can be selected such that the organic phase and titanium chloride may be separated by fractional distillation (for example with a separation in boiling points between the organic phase and titanium chloride.)
  • For example, the titanium chloride can be treated with water or a base, (for example magnesium oxide), or by raising the temperature of the solution to 85-110 C, to effect precipitation of titanium dioxide.
  • The titanium chloride product obtained can also be subjected to calcination in a pyrohydrolysis reactor or be treated in a plasma torch so as to convert it into TiO2.
  • For example, NaCl recovered from the processes of the present disclosure can be reacted with SO2, so as to produce HCl and Na2SO4. Such a reaction that is an exothermic reaction can generate steam that can be used to activate a turbine and eventually produce electricity.
  • For example, U and/or Th can be tretaed with the processes of the present disclosure. For example, these two elements can be in such processes in admixtures with iron ions and they can be separated therefrom by means of at least one ion exchange resin.
  • According to one example as shown in FIG. 1, the processes can involve the following steps (the reference numbers in FIG. 1 correspond to the following steps):
  • According to one example as shown in FIG. 1, the processes can involve the following steps (the reference numbers in FIG. 1 correspond to the following steps):
  • 1—The aluminum-containing material is reduced to an average particle size of about 50 to about 80 μm.
  • 2—The reduced and classified material is treated with hydrochloric acid which allows for dissolving, under a predetermined temperature and pressure, the aluminum with other elements like iron, magnesium and other metals including rare earth elements and/or rare metals. The silica and titanium (if present in raw material) remain totally undissolved.
  • 3—The mother liquor from the leaching step then undergoes a separation, a cleaning stage in order to separate the solid from the metal chloride in solution.
  • 4—The spent acid (leachate) obtained from step 3 is then brought up in concentration with dry and highly concentrated gaseous hydrogen chloride by sparging this one into a crystallizer. This results into the crystallization of aluminum chloride hexahydrate (precipitate) with a minimum of other impurities. Depending on the concentration of iron chloride at this stage, further crystallization step(s) can be required. The precipitate is then separated from the liquid. For example, particle size of crystals can be about 100 to about 500 microns, about 200 to about 400 microns, or about 200 to about 300 microns. Alternatively, particle size of crystals can be about 100 to about 200 microns, about 300 to about 400 microns or about 400 to 500 microns.
  • 5—The aluminum chloride hexahydrate is then calcined (for example by means of a rotary kiln, fluid bed, etc) at high temperature in order to obtain the alumina form. Highly concentrated gaseous hydrogen chloride is then recovered and excess is brought in aqueous form to the highest concentration possible so as to be used (recycled) in the acid leaching step. Acid can also be directly sent in gas phase to the acid purification stage to increase HCl concentration from about 30 wt % to about 95 wt %. This can be done, for example, during drying stage.
  • 6—Iron chloride (the liquid obtained from step 4) is then pre-concentrated and hydrolyzed at low temperature in view of the Fe2O3 (hematite form) extraction and acid recovery from its hydrolysis. All heat recovery from the calcination step (step 5), the leaching part exothermic reaction (step 1) and other section of the processes is being recovered into the pre-concentrator. Alternatively, the iron chloride can be treated by means of a pyrohydrolysis in order to generate Cl2 (instead of mianly NCl). In such a case, the Cl2 so produced can be used in step 13 of FIG. 1 for treating the solid that comprises Ti. For example, it can be used to convert TiO2 into TiCl4. Such a reaction can be carried under oxidizing conditions (for example more than 4% of O2). The pyrohydrolysis can be carried out in in a fluid bed reactor under such oxidizing conditions.
  • 10—After the removal of hematite, a solution rich in rare earth elements and/or rare metals can be processed. As it can be seen in FIG. 3, an internal recirculation can be done (after the removal of hematite) and the solution rich in rare earth elements and/or rare metals can be used for crystallization stage 4. Extraction of the rare earth elements and/or rare metals can be done as described in WO/2012/126092 and/or WO/2012/149642. These two documents are hereby integrated by reference in their entirety.
  • Other non-hydrolysable metal chlorides (Me-Cl) such as MgCl2 and others then undergo the following steps:
  • 7—The solution rich in magnesium chloride and other non-hydrolysable products at low temperature is then brought up in concentration with dry and highly concentrated gaseous hydrogen chloride by sparging it into a crystallizer. This results into the precipitation of magnesium chloride as an hexahydrate, for example after sodium and potassium chloride removal.
  • 8—Magnesium chloride hexahydrate is then calcined (either through a rotary kiln, fluid bed, etc.) and hydrochloric acid at very high concentration is thus regenerated and brought back to the leaching step.
  • 9—Other Me-Cl undergo a standard pyrohydrolysis step where mixed oxides (Me-O) can be produced and hydrochloric acid at the azeotropic point (20.2% wt.) is regenerated.
  • 11—Ti contained in the solid obtained from step 3 can be treated so as to separate Si from Ti and thus obtain SiO2 and TiO2.
  • NaCl produced in this process can undergo chemical reaction with H2SO4 to produce Na2SO4 and HCl at a concentration at or above azeotropic concentration. Moreover, KCl can undergo chemical reaction with H2SO4 to produce K2SO4 and HCl having a concentration that is above the azeotropic concentration. Sodium and potassium chloride brine solution can be the feed material to adapted small chlor-alkali electrolysis cells. In this latter case, common bases (NaOH and KOH) and bleach (NaOCl and KOCl) are produced as well as HCl.
  • For example, the liquid can be concentrated to a concentrated liquid having an iron chloride concentration of at least 30% by weight; and then the iron chloride can be hydrolyzed at a temperature of about 155 to about 350° C. while maintaining a ferric chloride concentration at a level of at least 65% by weight, to generate a composition comprising a liquid and precipitated hematite, and recovering the hematite.
  • For example, the liquid can be concentrated to a concentrated liquid having an iron chloride concentration of at least 30% by weight; and then the iron chloride can be hydrolyzed at a temperature of about 155 to about 350° C. while maintaining a ferric chloride concentration at a level of at least 65% by weight, to generate a composition comprising a liquid and precipitated hematite; recovering the hematite; and recovering rare earth elements and/or rare metals from the liquid. For example, the process can further comprise, after recovery of the rare earth elements and/or rare metals, reacting the liquid with HCl so as to cause precipitation of MgCl2, and recovering same.
  • As previously indicated, various aluminum-containing materials can be used as starting material of the processes disclosed in the present disclosure. Examples with clays and bauxite have been carried out. However, the person skilled in the art will understand that the continuous processes can handle high percentages of silica (>55%) and impurities as well as relatively low percentages of aluminum (for example as low as about 15%) and still being economically and technically viable. Satisfactory yields can be obtained (>93-95%) on Al2O3 and greater than 75%, 85 or 90% on rare earth elements and/or rare metals. No pre-thermal treatment in most cases are required. The processes disclosed in the present disclosure involve special techniques on leaching and acid recovery at very high strength, thereby offering several advantages over alkaline processes.
  • In step 1 the mineral, whether or not thermally treated is crushed, milled, dried and classified to have an average particle size of about 50 to about 80 μm.
  • In step 2, the milled raw material is introduced into the reactor and will undergo the leaching phase.
  • The leaching hydrochloric acid used in step 2 can be a recycled or regenerated acid from steps 5, 6, 8, 9, 10 and 11 (see FIG. 3) its concentration can vary from 15% to 45% weight. percent. Higher concentration can be obtained using membrane separation, cryogenic and/or high pressure approach. The acid leaching can be carried out under pressure and at temperature close to its boiling point thus, allowing a minimal digestion time and extended reaction extent (90%-100%). Leaching (step 2) can be accomplished in a semi-continuous mode where spent acid with residual free hydrochloric acid is replaced by highly concentrated acid at a certain stage of the reaction or allowing a reduced acid/mineral ratio, thereby reducing reaction time and improving reaction kinetics. For example, kinetic constant k can be: 0.5-0.75 g/mole·L. For example, leaching can be continuous leaching.
  • As previously indicated, alkali metals, iron, magnesium, sodium, calcium, potassium, rare earth elements and other elements will also be in a chloride form at different stages. Silica and optionally titanium can remain undissolved and will undergo (step 3) a liquid/solid separation and cleaning stage. The processes of the present disclosure tend to recover maximum amount of free hydrochloric acid left and chlorides in solution in order to maximize hydrochloric acid recovery yield, using techniques such as rake classifying, filtration with band filters, centrifugation, high pressure, rotofilters and others. Thanks to step 13, Ti contained in the solid obtained from step 3 can be treated so as to separate Si from Ti and thus obtain SiO2 and TiO2. Various possible strategies can be used to separated Si from Ti as previously indicated. For example, the solid can be further leached (for example with HCl in the presence of a metal chloride (for example MgCl2 or ZnCl2) so as to solubilize Ti (for example in the form of TiCl4) while the Si remains solid. Alternatively, the solid can be reacted with Cl2 (see FIGS. 9A and 9B). he purified silica can then optionally undergo one or two additional leaching stages (for example at a temperature of about 150 to about 160° C.) so as to increase the purity of silica above 99.9%.
  • As previously indicated, if iron chloride generated in certain processes of the disclosure is to be treated by means of a pyrohydrolysis in order to generate Cl2, the latter can eventually be used in the processes of FIGS. 9A and 9B as a source of Cl2.
  • Pure SiO2 (one additional leaching stage) cleaning with nano water purity 99% min. Mother liquor free of silica is then named as spent acid (various metal chlorides and water) and goes to the crystallization step (step 4). Free HCl and chlorides recovery can be at least 99, 99.5 or 99.9%
  • In step 4, the spent acid (or leachate) with a substantial amount of aluminum chloride is then saturated with dry and highly concentrated gaseous hydrogen chloride obtained or recycled from step 5 or with aqueous HCl>30% wt., which results in the precipitate of aluminum chloride hexahydrate (AlCl3.6H2O). The precipitate retained is then washed and filtered or centrifuged before being fed to the calcination stage (step 5). The remaining of the spent acid from step 4 is then processed to acid recovery system (steps 6 to 8) where pure secondary products will be obtained.
  • In step 5, aluminum oxide (alumina) is directly obtained from high temperature conditions. The highly concentrated hydrogen chloride in gaseous form obtained can be fed to steps 4 and 7 for crystallization where it can be treated through hydrophobic membranes. The excess hydrogen chloride is absorbed and used as regenerated acid to the leaching step 2 as highly concentrated acid, higher than the concentration at the azeotropic point (>20.2%). For example, such a concentration can be about 18 to about 45 weight %, about 25 to about 45 weight % or between 25 and 36 weight %. Acid can also be redirected in gas phase directly (>30 wt %) to acid purification.
  • After step 4, various chlorides derivatives (mainly iron with magnesium and rare earth elements and rare metals) are next subjected to an iron extraction step. Such a step can be carried out for example by using the technology disclosed in WO 2009/153321, which is hereby incorporated by reference in its entirety. Moreover, hematite can be seeded for crystal growth. For example, hematite seeding can comprise recirculating the seeding.
  • In step 6, a hydrolysis at low temperature (155-350° C.) is carried out and pure Fe2O3 (hematite) is being produced and hydrochloric acid of at least 15% concentration is being regenerated. The method as described in WO 2009/153321 is processing the solution of ferrous chloride and ferric chloride, possible mixtures thereof, and free hydrochloric acid through a series of steps pre-concentration step, oxidation step where ferrous chloride is oxidized into ferric form, and finally through an hydrolysis step into an operational unit called hydrolyser where the ferric chloride concentration is maintained at 65 weight % to generate a rich gas stream where concentration ensures a hydrogen chloride concentration of 15-20.2% and a pure hematite that will undergo a physical separation step. Latent heat of condensation is recovered to the pre-concentration and used as the heating input with excess heat from the calcination stage (step 5).
  • The mother liquor from the hydrolyser (step 6) can be recirculated partially to first step crystallization process where an increase in concentration of non-hydrolysable elements is observed. After iron removal, the liquor is rich in other non-hydrolysable elements and mainly comprises magnesium chloride or possible mixture of other elements (various chlorides) and rare earth elements and rare metals that are, for example, still in the form of chlorides.
  • Rare earth elements and rare metals in form of chlorides are highly concentrated, in percentage, into the hydrolyser operational unit (step 6) and are extracted from the mother liquor (step 10) where various known techniques can be employed to extract a series of individual RE-O (rare earth oxides). Among others, the processes of the present disclosure allows to concentrate to high concentration the following elements, within the hydrolyser: scandium (Sc), galium (Ga), yttrium (Y), dysperosium (Dy), cerium (Ce), praseodynium (Pr), neodynium (Nd), europium (Eu), lanthanum (La), samarium (Sm), gadolinium, (Gd), erbium (Er), zirconium (Zr) and mixtures of thereof. Technologies that can be used for extracting rare earth elements and/or rare metals can be found, for example, in Zhou et al. in RARE METALS, Vol. 27, No. 3, 2008, p223-227, and in US 2004/0042945, hereby incorporated by reference in their entirety. The person skilled in the art will also understand that various other processes normally used for extracting rare earth elements and/or rare metals from the Bayer process can also be used. For example, various solvent extraction techniques can be used. For certain elements, a technique involving octylphenyl acid phosphate (OPAP) and toluene can be used. HCl can be used as a stripping agent. This can be effective for recovering Ce2O3, Sc2O3, Er2O3 etc. For example, different sequence using oxalic acid and metallic iron for ferric chloride separation can be used.
  • The spent acid liquor from steps 6 and 10 rich in value added metals, mainly magnesium, is processed to step 7. The solution is saturated with dry and highly concentrated gaseous hydrogen chloride from step 5, which results in the precipitation of magnesium chloride hexahydrate. For example, same can be accomplished with HCl in aqueous form over 30% wt. The precipitate retained, is fed to a calcination stage step 8 where pure MgO (>98% wt.) is obtained and highly concentrated hydrochloric acid (for example of at least 38%) is regenerated and diverted to the leaching step (step 2). An alternative route for step 7 is using dry gaseous hydrochloric acid from step 8.
  • In step 9, metal chlorides unconverted are processed to a pyrohydrolysis step (700-900° C.) to generate mixed oxides and where hydrochloric acid from 15-20.2% wt. concentration can be recovered.
  • According to another example as shown in FIG. 3, the processes can be similar to the example shown in FIG. 1 but can comprise some variants as below discussed.
  • In fact, as shown in FIG. 3, the processes can comprise (after step 6 or just before step 10) an internal recirculation back to the crystallization step 4. In such a case, The mother liquor from the hydrolyser (step 6) can be recirculated fully or partially to the crystallization of step 4 where a concentration increase will occur with respect to the non-hydrolysable elements including rare earth elements and/or rare metals.
  • Such a step can be useful for significantly increasing the concentration of rare earth elements and/or rare metals, thereby facilitating their extraction in step 10.
  • With respect to step 7, the solution rich in magnesium chloride and other non-hydrolysable products at low temperature is, as previously discussed, then brought up in concentration with dry and highly concentrated gaseous hydrogen chloride by sparging it into a crystallizer. This can result into the precipitation of magnesium chloride as an hexahydrate (for example after sodium and potassium chloride removal). This can also be accomplished with HCl in aqueous form.
  • As shown in FIG. 3, an extra step 11 can be added. Sodium chloride can undergo a chemical reaction with sulfuric acid so as to obtain sodium sulfate and regenerate hydrochloric acid at a concentration at or above the azeotropic point. Potassium chloride can undergo a chemical reaction with sulfuric acid so as to obtain potassium sulfate and regenerate hydrochloric acid at a concentration above the azeotropic concentration. Sodium and potassium chloride brine solution can be the feed material to adapted small chlor-alkali electrolysis cells. In this latter case, common bases (NaOH and KOH) and bleach (NaOCl and KOCl) are produced and can be reused to some extent in other areas of the processes of the present disclosure (scrubber, etc.).
  • As previously indicated, if iron chloride is treated in stage 6 of FIG. 3 by means of a pyrohydrolysis under oxidizing conditions, Cl2 will thus be produced and it can be used for treating the solid of stage 13. In such a case an arrow from box 6 towards box 13 can be inserted in FIG. 3 and the arrow from after box 6 to box 4 can be optionally removed.
  • Similarly, for the processes of FIGS. 6 and 7, if iron chloride is treated in stage 105 by means of a pyrohydrolysis under oxidizing conditions, Cl2 will thus be produced and it can be used for treating the solid of stage 113. In such a case an arrow from box 105 towards box 113 can be inserted in FIG. 3 and the arrow from after box 105 to box 104 can be optionally removed.
  • The following are non-limitative examples.
    • Example 1 Preparation of Alumina and Various Other Products
  • As a starting material a sample of clay was obtained from the Grande Vallee area in Québec, Canada.
  • These results represent an average of 80 tests carried out from samples of about 900 kg each.
  • Crude clay in the freshly mined state after grinding and classification had the following composition:
  • Al2O3: 15%-26%;
    • SiO2: 45%-50%;
  • Fe2O3: 8%-9%;
    • MgO: 1%-2%;
  • Rare earth elements and/or rare metals: 0.04%-0.07%;
    • LOI: 5%-10%.
  • This material is thereafter leached in a two-stage procedure at 140-170° C. with 18-32 weight % HCl. The HCl solution was used in a stoichiometric excess of 10-20% based on the stoichiometric quantity required for the removal of the acid leachable constituents of the clay. In the first leaching stage of the semi-continuous operation (step 2), the clay was contacted for 2.5 hours with required amount or certain proportion of the total amount of hydrochloric acid. After removal of the spent acid, the clay was contacted again with a minimum 18 weight % hydrochloric acid solution for about 1.5 hour at same temperature and pressure.
  • A typical extraction curve obtained for both iron and aluminum for a single stage leaching is shown in FIG. 2.
  • The leachate was filtered and the solid was washed with water and analyzed using conventional analysis techniques (see step 3 of FIG. 1). Purity of obtained silica was of 95.4% and it was free of any chlorides and of HCl.
  • In another example, the purity of the silica was 99.67% through an extra leaching step.
  • After the leaching and silica removal, the concentration of the various metal chlorides was:
    • AlCl3: 15-20%; FeCl2: 4-6%; FeCl3: 0.5-2.0%; MgCl2: 0.5-2.0%; REE-CI: 0.1-2% Free HCl: 5-50 g/l
  • Spent acid was then crystallized using about 90 to about 98% pure dry hydrochloric acid in gas phase in two stages with less than 25 ppm iron in the aluminum chloride hexahydrate formed. The concentration of HCl in solution (aqueous phase) was about 22 to about 32% or 25 to about 32%, allowing 95.3% of Al2O3 recovery. The recovered crystallized material (hydrate form of AlCl3 having a minimum purity of 99.8%) was then calcined at 930° C. or 1250° C., thus obtaining the a form of the alumina. Heating at 930° C. allows for obtaining the beta-form of alumina while heating at 1250° C. allows for obtaining the alpha-form.
  • Another example was carried out at low temperature (decomposition and calcination at about 350° C.) and the a form of the alumina was less than 2%. HCl concentration in gas phase exiting the calcination stage was having a concentration greater than 30% and was used (recycled) for crystallization of the AlCl3 and MgCl2. Excess of hydrochloric acid is absorbed at the required and targeted concentration for the leaching steps.
  • Iron chloride (about 90-95% in ferric form) is then sent to a hydrothermal process in view of its extraction as pure hematite (Fe2O3). This can be done by using the technology described in WO 2009/153321 of low temperature hydrolysis with full heat recovery from calcining, pyrohydrolysis and leaching stage.
  • Rare earth elements and rare metals are extracted from the mother liquor of the hydrolyzer where silica, aluminum, iron and a great portion of water have been removed and following preconcentration from hydrolyser to crystallization. It was observed that rare earth elements can be concentrated by a factor of about 4.0 to 10.0 on average within the hydrolyzer itself on a single pass through it i.e. without concentration loop. The following concentration factors have been noted within the hydrolyzer (single pass):
  • Ce>6
  • La>9
  • Nd>7
  • Y>9
  • Remaining magnesium chloride is sparged with dry and highly concentrated hydrochloric acid and then calcinated to MgO while recovering high concentration acid (for example up to 38.4%).
  • Mixed oxides (Me-O) containing other non-hydrolysable components were then undergoing a pyrohydrolysis reaction at 700-800° C. and recovered acid (15-20.2% wt.) was rerouted for example to the leaching system.
    • Overall Yields Obtained:
  • Al2O3: 93.0-95.03% recovery;
    Fe2O3: 92.65-99.5% recovery;
    Rare earth elements: 95% minimum recovery (mixture);
    MgO: 92.64-98.00% recovery;
    Material discarded: 0-5% maximum;
    HCl global recovery: 99.75% minimum;
    HCl strength as feed to leaching 15-32% (aqueous); 95% (gas)
    Red mud production: none.
    • Example 2 Preparation of Alumina and Various Other Products
  • A similar feed material (bauxite instead of clay) was processed as per in example 1 up to the leaching stage and revealed to be easily leachable under the conditions established in example 1. It provided an extraction percentage of 100% for the iron and over 90-95% for aluminum. The technology was found to be economically viable and no harmful by-products (red mud) were generated. Samples tested had various concentrations of Al2O3 (up to 51%), Fe2O3 (up to 27%) and MgO (up to 1.5%). Gallium extraction of 97.0% was observed. Scandium extraction was 95%.
    • Example 3 HCl Gas Enrichment and Purification: H2SO4 Route
  • H2SO4 can be used for carrying out purification of HCl. It can be carried out by using a packing column with H2SO4 flowing counter currently (see FIG. 4). This allows for converting the recovered HCl into HCl having a concentration above the azeotropic point (20.1% wt) and increase its concentration by about 60 to about 70% at minimum.
  • Water is absorbed by H2SO4 and then H2SO4 regeneration is applied where H2SO4 is brought back to a concentration of about 95 to about 98% wt. Water release at this stage free of sulphur is recycled back and used for crystallization dissolution, etc. Packing of the column can comprise polypropylene or polytrimethylene terephthalate (PTT).
  • Combustion energy can be performed with off gas preheating air and oxygen enrichment. Oxygen enrichment: +2% represents flame temperature increase by: 400° C. maximum.
  • Thus, HCl of the processes of the present disclosure can thus be treated accordingly.
    • Example 4 HCl Gas Enrichment and Purification: Calcium Chloride to Calcium Chloride Hexahydrate (Absorption/Desorption Process)
  • As shown in FIG. 5, CaCl2 can be used for drying HCl. In fact, CaCl2 can be used for absorbing water contained into HCl. In such a case, CaCl2 is converted into its hexachloride form (CaCl2.6H2O) and one saturated system is eventually switched into regeneration mode where hot air recovered from calcination off gas of alumina and magnesium oxide spray roasting is introduced to regenerate the fixed bed. Alternatively, other absorbing agent such as LiCl can be used instead of CaCl2. Such an ion/exchange type process can be seen in FIG. 4 and the cycle can be inversed to switch from one column to another one.
  • The person skilled in the art would understand that the processes described in examples 3 and 4 (see FIGS. 4 and 5) can be used in various different manners. For example, these processes can be combined with the various processes presented in the present disclosure. For example, such purifications techniques can be integrated to the processes shown in FIGS. 1, 3 and 6 to 8. For example, these techniques can be used downstream of at least one of step chosen from steps 5, 6, 8, 9, 10, 11, 13 and 20 (see FIGS. 1, 3 and 8). They can also be used downstream of step 4 and/or step 7. They can also be used downstream of at least one of step chosen from steps 104 to 111 (see FIGS. 6 and 7).
    • Example 5 Preparation of Alumina and Various Other Products
  • This example was carried out by using a process as represented in FIGS. 6 and 7. It should be noted that the processes represented in FIGS. 6 and 7 differ mainly by the fact that FIG. 7 shows an extra stage i.e. stage 112.
    • Raw Material Preparation
  • Raw material, clay for example, was processed in a secondary crusher in the clay preparation plant 101. Dry milling and classifying occurs on a dry basis in vertical roller mills (for example Fuller-Loesche LM 30.41). The clay preparation 101 included three roller mills; two running at a capacity of approximately 160-180 tph and one on standby. Raw material, if required, can be reduced to 85% less than 63 microns. Processed material was then stored in homogenization silos before being fed to the acid leaching plant 102. Below in Table 1 are shown results obtained during stage 101. If the ore contains the fluorine element, a special treatment can be applied before carrying out the 102 stage. In presence of hydrochloric acid, fluorine can produce hydrofluoric acid. This acid is extremely corrosive and damaging for human health. Thus, before leaching 102, an optional treatment fluorine separation 112 can be done. Stage 112 can comprise treating the processed material coming from stage 101 with an acid in a pre-leaching treatment so as to remove hydrofluoric acid. Therefore, depending on the composition of the raw material, a fluorine separation stage 112 (or pre-leaching stage 112) can be carried out.
  • TABLE 1
    Clay preparation
    Rate 290 tph
    Composition feed SiO2:  50.9%
    (main constituents) Al2O3:  24.0%
    Fe2O3:  8.51%
    CaO:  0.48%
    MgO:  1.33%
    Na2O:  1.06%
    K2O:  2.86%
    MnO:  0.16%
    Cr2O3:  0.01%
    TiO2:  0.85%
    P2O5:  0.145%
    SrO:  0.015%
    BaO:  0.05%
    V2O5 0.0321%
    Other (including H2O and 9.63%
    REE):
    Obtained particle size 85% < 63 μm
    Residual moisture 0.5-0.7%
    Yield 99.5% min
    • Acid Leaching
  • Next, acid leaching 102 was performed semi-continuously in an 80 m3 glass-lined reactor. Semi-continuous mode comprises replacing reacted acid ⅓ in the reaction period with higher concentration regenerated acid, which greatly improves reaction kinetics. The reactor arrangement comprises for example, a series of three reactors. Other examples have been carried out with a first leaching at 1 atm was carried out and then, a second and third semi-continous or continuous leaching was carried out with aqueous or gaseous HCl.
  • Leaching was performed at high temperature and pressure (about 160 to about 195° C. and pressures of about 5 to about 8 barg) for a fixed period of time. Reaction time was a function of the reaction extent targeted (98% for Al2O3), leaching mode, acid strength, and temperature/pressure applied.
  • Spent acid recovered out of the acid leaching 102 was then filtered 103 from unreacted silica and titanium dioxide and washed through an automated filter press where all free HCl and chloride are recovered. Step 113 can then be carried out in various manners as indicated previously for step 13. This allows, for example, a maximum quantity of about 30 ppm SiO2 going into spent liquor. Cleaned silica at a concentration of ≈96%+SiO2 is then produced. Various options are possible at that point. For example, the 96% silica can undergo final neutralization through caustic bath, cleaning, and then bricketing before storage. According to another example, the silica purified by adding another leaching step followed by a solid separation step that ensures TiO2 removal (see stage 113 in FIGS. 6 and 7). In that specific case, high purity silica 99.5%+ is produced. In stage 113, titanium and silicium can be separated from one another in various manners. For example, the solid obtained from stage 103 can be leached in the presence of MgCl2 at a temperature below 90 or 80° C. and at low acid concentration. For example, acid concentration can be below 25 or 20%. The acid can be HCl or H2SO4. In such a case, titanium remains soluble after such a leaching while titanium is still in a solid form. The same also applies when the solid is treated with Cl2. These solid and liquid obtained after stage 113 are thus separated to provide eventually TiO2 and SiO2. Water input and flow for silica cleaning is in a ratio of 1:1 (silica/water) (150 t/h SiO2/150 t/h H2O), but comprises of wash water circulation in closed loop in the process and limited amount of process water for final cleaning of the silica and recovery of all chlorides and free HCl generated at the leaching stage. Below in Table 2 are shown results obtained during stage 102.
  • TABLE 2
    Acid Leaching
    Equivalent solid feed rate 259.6 tph
    Operation mode Semi-continuous
    Acid to clay ratio 3.10 @ 23% wt
    (Equivalent to 3.35 with semi-continuous at
    18.0% wt)
    Regenerated acid 18.0-32.0%
    concentration
    Operating temperature 150-155° C. (Pilot)
    165-200° C. (Plant)
    MAWP 120 psig
    Typical chemical Fe2O3 + 6 HCl → 2 FeCl3 + 3H2O
    reactions Al2O3 + 6 HCl → 2 AlCl3 + 3 H2O
    MgO + 2 HCl → MgCl2 + H2O
    K2O + 2 HCl→ 2 KCl + H2O
    Re2O3 + 6 HCl → 2 ReCl3 + 3H2O
    Spent acid flow to 600-1100 m3/h
    crystallization
    Practical chemical FeCl3 4.33%
    composition after step FeCl2 0.19%
    102 without solid (SiO2) AlC13 16.6%
    MgCl2 0.82%
    NaCl  1.1%
    KCl  1.2%
    CaCl2 0.26%
    Extraction yields Iron  100%
    Al2O3   98%
    SiO2 Recovery 99.997%
    Energy consumption Activation energy only and self-sustained
    exothermic reaction from 130° C.
    • AlCl3 Crystallization
  • Spent acid, with an aluminum chloride content of about 20 to about 30%, was then processed in the crystallization stage 104. Dry and highly concentrated HCl (>90% wt.) in gas phase was sparged in a two-stage crystallization reactor, which allows the crystallization of aluminum chloride hexahydrate.
  • The flow rate of acid through these reactors is about 600 to about 675 m3/h and the reactor was maintained at about 50 to about 60° C. during this highly exothermic reaction. Heat was recovered and exchanged to the acid purification 107 part of the plant thus ensuring proper heat transfer and minimizing heat consumption of the plant. Aluminum chloride solubility decreases rapidly, compared to other elements, with the increase in concentration of free HCl in the crystallization reactor. The concentration of AlCl3 for precipitation/crystallization was about 30%
  • The HCl concentration during crystallization was thus about 30 to about 32% wt.
  • The aqueous solution from the crystallization stage 104 was then submitted to the hydrothermal acid recovery plant 105, while the crystals are processed through the decomposition/calcination stage in the calcination plant 106.
  • A one-step crystallization stage or a multi-step crystallization stage can be done. For example, a two-steps crystallization stage can be carried out.
  • Below in Tables 3A and 3B are shown results obtained during stage 104.
  • TABLE 3A
    Aluminum chloride crystallization
    Number of crystallization 2
    steps
    Operating temperature 50-60° C.
    Sparging HCl concentration 90% (gaseous)
    Typical chemicals formed AlCl3•6H2O (s)
    Metal chlorides (aq)
    AlCl3•6H2O residual <5% (practical); 8%
  • TABLE 3B
    Typical crystals composition main constituents
    obtained at pilot scale and feeding calcination
    Component Weight distribution (%)
    AlCl3•6H2O 99.978
    BaCl2•2H2O 0.0000
    CaCl2•6H2O 0.0009
    CrCl4 0.0022
    CuCl2•2H2O 0.0000
    FeCl3•6H2O 0.0019
    KCl 0.0063
    MgCl2•6H2O 0.0093
    MnCl2•4H2O 0.0011
    NaCl 0.0021
    SiCl4 0.0004
    SrCl2•6H2O 0.0000
    TiCl4 0.0001
    VCl4 0.0000
    Free Cl− 0.0000
    • Calcination and Hydrothermal Acid Recovery
  • The calcination 106 comprises the use of a two-stage circulating fluid bed (CFB) with preheating systems. The preheating system can comprise a plasma torch to heat up steam to process. It processes crystals in the decomposition/calcination stage. The majority of the hydrochloric acid was released in the first stage which was operated at a temperature of about 350° C., while the second stage performs the calcination itself. Acid from both stages (about 66 to about 68% of the recovered acid from the processes) was then recovered and sent to either to the acid leaching 102 or to the acid purification 107. In the second reactor, which was operated at a temperature of about 930° C., acid was recovered through the condensation and absorption into two columns using mainly wash water from the acid leaching sector 102. Latent heat from this sector was recovered at the same time as large amounts of water, which limits net water input.
  • In the iron oxides productions and acid recovery 105 system, which comprises, aqueous solution from the crystallization 104 first undergoes a pre-concentration stage followed by processing in the hydrolyzer reactor. Here, hematite was produced during low temperature processing (about 165° C.). A recirculation loop was then taken from the hydrolyzer and is recirculated to the pre-concentrator, allowing the concentration of REE, Mg, K, and other elements. This recirculation loop, allows rare earth element chlorides and/or rare metal chlorides and various metal chlorides concentration to increase without having these products precipitating with hematite up to a certain extent.
  • Depending on acid balance in the plant, recovered acid is sent either directly to the 102 or 107 stage. Table 4 shows results obtained in stage 105.
  • TABLE 4
    Hydrothermal acid recovery
    Flowrate from crystallization to 592 m3/h (design)
    HARP 600 m3/h (design)
    Operating hydrolyser 155-170° C.
    temperature
    Regenerated acid concentration   27.4%
    Regenerated acid flowrate 205.2 tph HCl
    Hematite total production rate 24 TPH (design)
    HCl recovery >99.8%
    Reflux (recirculation loop) rate in 56 tph
    between hydrolyzer and pre-
    concentrator
    Rare earth element chlorides ≈12.8 t/h
    and/or rare metal chlorides rate
    in recirculation loop
    Hematite quality obtained and/or projected
    Fe2O3 purity >99.5%
    Hydrolysable chlorides  <0.2%
    Moisture Max 20% after filtration
    PSD 25-35 microns
    Density (bulk) 2-3 kg/l
    Typical chemical reaction in stage 105
    2FeCl3 + 3H2O → Fe2O3 + 6 HCl
    155-170° C.
  • Table 5 shows results obtained in stage 106.
  • TABLE 5
    Calcination Plant 106
    Process characteristics: Two-stage circulating fluid bed
    (CFB) with pre-heating system
    Two-stage hydrochloric acid
    regeneration
    Production rate (practical) About 66 tph
    CFB feed rate 371 tph @ 2-3% humidity*
    Typical chemical reaction occurring
    2(AlCl3•6 H2O) + Energy → Al2O3 + 6 HCl + 9H2O
    Typical alumina chemical composition obtained from
    aluminum chloride hexahydrate crystals being fed to
    calcination
    Component Weight distribution (%)
    Al2O3 99.938
    Fe2O3 0.0033
    SiO2 0.0032
    Cr2O3 0.0063
    V2O5 0.0077
    Na 0.0190
    MgO 0.0090
    P2O5 0.0039
    K 0.0053
    Ca 0.0020
    MnO 0.0002
    Free Cl− Undetectable
    • Rare Earth Elements and Rare Metals Extractions
  • The stream that was taken out of 105 recirculation then was treated for rare earth elements and are metals extraction 108, in which the reduction of the remaining iron back to iron 2 (Fe2+), followed by a series of solvent extraction stages, was performed. The reactants were oxalic acid, NaOH, DEHPA (Di-(2-ethylhexyl)phosphoric acid) and TBP (tri-n-butyl phosphate) organic solution, kerosene, and HCl were used to convert rare earth element chlorides and rare metals chlorides to hydroxides. Countercurrent organic solvent with stripping of solution using HCl before proceeding to specific calcination from the rare earth elements and rare metals in form of hydroxide and conversion to high purity individual oxides. A ion exchange technique is also capable of achieving same results as polytrimethylene terephtalate (PET) membrane.
  • Iron powder from 105, or scrap metal as FeO, can be used at a rate dependent on Fe3+ concentration in the mother liquor. HCl (100% wt) at the rate of 1 tph can be required as the stripped solution in REE Solvent Extraction (SX) separation and re-leaching of rare earth elements and/or rare metals oxalates.
  • Water of very high quality, demineralized or nano, at the rate of 100 tph was added to the strip solution and washing of precipitates.
  • Oxalic acid as di-hydrate at a rate of 0.2 tph was added and contributes to the rare earth elements and rare metals oxalates precipitation. NaOH or MgOH at a rate of 0.5 tph can be used as a neutralization agent.
  • DEHPA SX organic solution at the rate of 500 g/h was used as active reagent in rare earth elements separation while TBP SX organic solution at the rate of 5 kg/h is used as the active reagent for gallium recovery and yttrium separation. Finally, a kerosene diluent was used at the rate of approximately 2 kg/h in all SX section. Calcination occurs in an electric rotary furnace via indirect heating to convert contents to REE2O3 (oxides form) and maintain product purity.
  • Results of various tests made regarding stage 108 are shown in Table 6. One line divided in subsections (5) to isolate the following elements using solvent extraction:
      • Ga2O3
      • Y2O3
      • Sc2O3
      • Eu2O3+Er2O3+Dy2O3
      • Ce2O3+Nd2O3+Pr2O3
  • Equivalent output 166.14 kg/h
    earths oxides
    Projected production as per pilot testing results
    Incoming Final extraction individual
    Feed (kg/h) (kg/h)
    Ga2O3 15.66 11.98
    Sc2O3 9.06 8.11
    Y2O3 22.56 20.22
    La2O3 32.24 25.67
    Ce2O3 61.37 51.82
    Pr2O3 8.08 6.18
    Nd2O3 30.3 27.24
    Sm2O3 5.7 4.51
    Eu2O3 1.06 0.95
    Gd2O3 4.5 4.06
    Dy2O3 3.9 3.55
    Er2O3 2.1 1.86
    Total 196.55 166.14
    Global yield: 84.53%
  • Alternatively, stage 108 can be carried out as described in WO/2012/126092 and/or WO/2012/149642, that are hereby incorporated by reference in their entirety.
  • The solution after stages 108 and 109 contained mainly MgCl2, NaCl, KCl, CaCl2, FeCl2/FeCl3, and AlCl3 (traces), and then undergoes the 111 stage. Na, K, Ca that follows the MgO can be extracted in stage 110 by crystallization in a specific order; Na first, followed by K, and then Ca. This technique can be employed for example in the Israeli Dead Sea salt processing plant to produce MgO and remove alkali from the raw material.
  • HCl regeneration
  • Alkali (Na, K), once crystallized, was sent and processed in the alkali hydrochloric acid regeneration plant 110 for recovering highly concentrated hydrochloric acid (NCl). The process chosen for the conversion can generate value-added products
  • Various options are available to convert NaCl and KCl with intent of recovering HCl. One example can be to contact them with highly concentrated sulfuric acid (H2SO4), which generates sodium sulphate (Na2SO4) and potassium sulfate (K2SO4), respectively, and regenerates HCl at a concentration above 90% wt. Another example, is the use of a sodium and potassium chloride brine solution as the feed material to adapted small chlor-alkali electrolysis cells. In this latter case, common bases (NaOH and KOH) and bleach (NaOCl and KOCl) are produced. The electrolysis of both NaCl and KCl brine is done in different cells where the current is adjusted to meet the required chemical reaction. In both cases, it is a two-step process in which the brine is submitted to high current and base (NaOH or KOH) is produced with chlorine (Cl2) and hydrogen (H2). H2 and Cl2 are then submitted to a common flame where highly concentrated acid in gas (100% wt.) phase is produced and can be used directly in the crystallization stage 104, or to crystallization stages requiring dry highly concentrated acid.
    • Magnesium Oxide
  • The reduced flow, which was substantially free of most elements (for example AlCl3, FeCl3, REE-CI, NaCl, KCl) and rich in MgCl2, was then submitted to the magnesium oxides plant 111. In the MgO, pyrohydrolysis of MgCl2 and any other leftover impurities were converted into oxide while regenerating acid. The first step was a pre-evaporator/crystallizer stage in which calcium is removed and converted into gypsum (CaSO4.2H2O) by a simple chemical reaction with sulfuric acid, for which separation of MgO is required. This increases the capacity of MgO roasting and also energy consumption slightly, while substantially recovering HCl. The next step was the specific pyrohydrolysis of MgO concentrated solution by spray roasting. Two (2) main products were generated; MgO that was further treated and HCl (about 18% wt.), which was either recycled back to the upstream leaching stage 102 or to the hydrochloric acid purification plant (107) The MgO-product derived from the spray roaster can require further washing, purification, and finally calcining depending on the quality targeted. The purification and calcining can comprise a washing-hydration step and standard calcining step.
  • The MgO from the spray roaster is highly chemically active and was directly charged into a water tank where it reacts with water to form magnesium hydroxide, which has poor solubility in water. The remaining traces of chlorides, like MgCl2, NaCl, dissolved in water. The Mg(OH)2 suspension, after settling in a thickener, was forwarded to vacuum drum filters, which remove the remaining water. The cleaned Mg(OH)2 is then forwarded into a calcination reactor where it is exposed to high temperatures in a vertical multi-stage furnace. Water from hydration is released and allows the transformation of the Mg(OH)2 to MgO and water. At this point, the magnesium oxide was of high purity (>99%).
    • HCl Purification
  • The hydrochloric acid purification stage 107 is effective for purifying HCl regenerated from different sectors (for example 105, 106, 111) and to increase its purity for crystallization, whereas dry highly concentrated acid (>90% wt.) can be used as the sparging agent. Stage 107 also allowed for controlling the concentration of the acid going back to stage 102 (about 22 to about 32% wt.) and allows total acid and water balance. Total plant water balance is performed mainly by reusing wash water as absorption medium, as quench agent or as dissolution medium at the crystallization stages.
  • For example, HCl purification can be carried out as shown in FIGS. 4 and 5.
  • For example, purification can be carried out by means of a membrane distillation process. The membrane distillation process applied here occurs when two aqueous liquids with different temperatures are separated through a hydrophobic membrane. The driving force of the process was supplied by the partial pressure vapour difference caused by the temperature gradient between these solutions. Vapour travels from the warm to the cold side. Without wishing to be bound to such a theory, the separation mechanism was based on the vapour/liquid equilibrium of the HCl/water liquid mixture. Practical application of such a technology has been applied to HCl/water, H2SO4/water systems and also on large commercial scales on aqueous solution of sodium chloride with the purpose of obtaining potable water from seawater and nano water production. Therefore membrane distillation was a separation process based on evaporation through a porous hydrophobic membrane. The process was performed at about 60° C. and was effective to recover heat from the 104 and 102 stage with an internal water circulation loop, in order to maintain a constant incoming temperature to the membranes. For example, eight membranes of 300,000 m2 equivalent surface area can be used per membrane to obtain a concentration of HCl well above the azeotropic point (i.e. >36%) of the ≈750 m3/h and final 90% concentration is then obtained through pressure distillation (rectification column).
  • Purification of HCl by processing thus regenerated acid through hydrophobic membrane and separating water from HCl; therefore increasing HCl concentration up to about 36% (above azeotropic point) and therefore allowing with a single stage of rectification through a pressure stripping column to obtain >90% in gaseous phase, for crystallization stage (sparging); and therefore controlling acid concentration into crystallization stages up to 30-35%(aq).
  • As indicated stage 107 was operated at about 60° C. and heat input provided by heat recovery from stages 102 to 110. Rectification column was operated at about 140° C. in the reboiler part. Net energy requirement was neutral (negative in fact at −3.5 Gj/t Al2O3) since both systems were in equilibrium and in balance.
  • For example, the acid purification can be carried out by using adsorption technology over an activated alumina bed. In continuous mode, at least two adsorption columns are required to achieve either adsorption in one of them and regeneration in the other one. Regeneration can be performed by feeding in counter-current a hot or depressurized gas. This technology will result in a purified gas at 100% wt.
  • For example, the acid purification can be made by using calcium chloride as entrainer of water. A lean hydrochloric acid solution is contacted with a strong calcium chloride solution through a column. The water is then removed from the hydrochloric acid solution and 99.9% gaseous HCl comes out of the process. Cooling water and cryogenic coolant is used to condense water traces in the HCl. The weak CaCl2 solution is concentrated by an evaporator that ensures the recuperation of calcium chloride. Depending on the impurities in the incoming HCl solution feed to the column, some metals can contaminate the calcium chloride concentrated solution. A precipitation with Ca(OH)2 and a filtration allows the removal of those impurities. The column can operate for example at 0.5 barg. This technology can allow for the recuperation of 98% of the HCl.
  • Table 7 shows the results obtained concerning the process shown in FIG. 6.
  • Composition Stage 101 Stage 102 Stage 106 Stage 105 MgO Stage 107 Stage 108 TOTAL PRODUCED
    (% wt) Yield (%) Yield (%) Yield (%) Yield (%) try Yield (%) Yield (%) Yield (%) Yield (%)
    Main constituents
    SiO2 — 99.997% — — — — — — 99.997% 
    Al —  93.02% 96.03% — — — — — 95.08%
    Fe — 100.00% — 92.65% — — — — 92.69%
    Mg — 98.998% — — 29,756 92.64% — — 92.64%
    Ca — 99.998% — — — — — — 98.28%
    Na — 99.988% — — — — — — 92.76%
    K — 100.00% — — — — — — 93.97%
    Others incl. H2O — — — — — — — —
    RE/RM —  99.80% — 92.32% — — — 84.67% 84.67%
    By Products
    NaOH — — — — 68,556 — — — —
    NaOCl — — — —  9,269 — — — —
    KOH — — — — 73,211 — — — —
    KOCl — — — —  9,538 — — — —
    CaSO4 — — — — 46,837 — — — —
    Reactants
    H2SO4(*) — — — — 19,204 — — — —
    Fresh HCl M-UP — — — — — — 99.75% — 99.78%
    Total —  93.55% 95.03% 256,416  92.64% 99.75% 84.67%
  • Tables 8 to 26 show results obtained concerning the products made in accordance with the process shown in FIG. 6 in comparison with standard of the industry.
  • TABLE 8
    Chemical composition of obtained alumina
    Standard used in
    Element % Weight* industry
    Al2O3 99.938 98.35 min
    Fe2O3 0.0033 0.0100
    SiO2 0.0032 0.0150
    TiO2 0.0003 0.0030
    V2O5 0.0008 0.0020
    ZnO 0.0005 0.0030
    Cr2O3 0.0003 N/A
    MgO 0.0090 N/A
    MnO 0.0002 N/A
    P2O5 0.0039 0.0010
    Cu 0.0030 N/A
    Ca 0.0020 0.0030
    Na 0.0190 0.4000
    K 0.0053 0.0150
    Li 0.0009 N/A
    Ba <0.00001 0.0000
    Th <0.000001 0.0000
    U <0.000001 0.0000
    Free Cl− Not detectable 0.0000
    LOI <1.0000 <1.0000
  • P2O5 removal technique can include, for example, after leaching, phosphorous precipitation using zirconium sulphate. It can be provided, for example, in a solution heated at 80 to about 90° C. or about 85 to about 95° C., under vacuum.
  • TABLE 9
    Physical properties of obtained alumina
    Standard used in
    Property Orbite Alumina industry
    PSD < 20 μm  5-10% N/A
    PSD < 45 μm 10-12%   <10%
    PSD > 75 μm 50-60% N/A
    SSA (m2/g) 60-85   60-80
    Att. Index 10-12%   <10%
    α Al2O3  2-5% <7-9%
  • TABLE 10
    Chemical composition of obtained hematite
    Element % Weight
    Fe2O3 >99.5%
    Hydrolysable elements  <0.2%
  • TABLE 11
    Physical properties of obtained hematite*
    Property Orbite hematite
    PSDmean 25-35 μm
    Density (bulk) 2000-3000 kg/m3
    Humidity after filtration <10%
    *Material can be produced as brickets
  • TABLE 12
    Chemical composition of obtained silica
    Element % Weight
    SiO2 >99.7
    Al2O3 <0.25%
    MgO  ≈0.1%
    Fe2O3  ≈0.1%
    CaO ≈0.01%
    Na2O  <0.1%
    K2O  <0.1%
    Note:
    Product may have unbleached cellulose fiber filteraid. Cellulose wood flour.
  • TABLE 13
    Physical properties of obtained silica
    Property Orbite silica
    PSDmean 10-20 μm
    Specific surface area 34 m2/g
    Density (bulk) 2000-2500 kg/m3
    Humidity after filtration <30%
  • TABLE 14
    Purity of obtained rare earth element oxides
    Element Purity (%)
    Ga2O3 >99%
    Sc2O3
    Y2O3
    La2O3
    Ce2O3
    Pr2O3
    Nd2O3
    Sm2O3
    Eu2O3
    Gd2O3
    Dy2O3
    Er2O3
    Physical properties of obtained REE-O/RM-O
    Property Orbite REE-O/RM-O
    PSDmean 2-30 μm
    Density 5500-13000 kg/m3
    LOI <1%
  • TABLE 15
    Chemical composition of obtained MgO
    Element Typical Specification
    MgO 99.0+ 98.35 min 
    CaO 0.0020 0.83
    SiO2 0.0000 0.20 max
    B2O3 0.0000 0.02 max
    Al2O3 0.0300 0.12 max
    Fe2O3 0.0160 0.57 max
    MnO2 <0.14 0.14 max
    LOI 0.7% <1%
  • TABLE 16
    Physical properties of obtained MgO
    Property Orbite MgO
    PSD
    mean 10 μm
    Density N/A
    LOI 650 kg/m3
  • TABLE 17
    Chemical composition of obtained NaOH
    Element % Weight
    Sodium hydroxide
    32%
    Water 68%
  • Table 18
    Physical properties of obtained NaOH
    Sodium hydroxide
    Property (NaOH)
    Physical state Liquid
    Vapour pressure 14 mmHg
    Viscosity >1
    Boiling point 100° C.
    Melting point
     0° C.
    Specific gravity 1.0
  • TABLE 19
    Chemical composition of obtained sodium
    hypochlorite (bleach)
    Element % Weight
    Sodium hypochlorite 12%
    Sodium hydroxide <1%
    Water >80% 
  • TABLE 20
    Physical properties of obtained NaOCl
    Sodium hypochlorite
    Property (NaOCl)
    Physical state Liquid
    Vapour pressure 1.6 kPa
    Viscosity N/A
    Boiling point 100° C.
    Melting point  −3° C.
    Specific gravity 1.2
  • TABLE 21
    Chemical composition of obtained
    potassium hydroxide
    Element % Weight
    Potassium hydroxide
    32%
    Water 68%
  • TABLE 22
    Physical properties of obtained potassium hydroxide
    Property KOH
    Physical state Liquid
    Vapour pressure 17.5 mmHg
    Viscosity N/A
    Boiling point 100° C.
    Melting point N/A
    Specific gravity 1.18
  • TABLE 23
    Chemical composition of obtained potassium
    hypochlorite (KOCl)
    Element % Weight
    Potassium hypochlorite 12%
    Potassium hydroxide <1%
    Water >80% 
  • TABLE 24
    Physical properties of obtained potassium
    hypochlorite
    Property KOCl
    Physical state Liquid
    Vapour pressure N/A
    Viscosity N/A
    Boiling point
    103° C.
    Melting point N/A
    Specific gravity >1.0
  • TABLE 25
    Chemical composition of obtained calcium
    sulphate dihydrate
    Element % Weight
    Calcium sulphate 100%
    dehydrate
  • TABLE 26
    Physical properties of obtained calcium sulphate
    dehydrate
    Property Orbite CaSO4•2H2O
    Physical state Solid
    Specific gravity 2.32
  • In order to demonstrate the versatility of the processes of the present disclosure, several other tests have been made so as to shown that these processes can be applied to various sources of starting material.
    • Example 6
  • Another starting material has been used for preparing acidic compositions comprising various components. In fact, a material that is a concentrate of rare earth elements and rare metals (particularly rich in zirconium) has been tested. Table 27 shows the results carried out on such a starting material using a similar process as shown in FIGS. 1, 3, 6 and 7 and as detailed in Examples 1, 2 and 5. It can thus be inferred from the results shown in Table 27 that the various components present in the leaching (various metals such as aluminum, iron, magnesium as well as rare earth elements and rare metals) can be extracted from the obtained leaching composition and that they can eventually be isolated by the processes of the present disclosure such as, for example, those presented in Examples 1, 2 and 5.
    • Example 7
  • Other tests have been made in a similar manner as described in Example 6. In the present example, carbonatite has been used as a starting material. (see Table 28 below).
  • TABLE 27
    Tests made on a zirconium rich material.
    Composition Average Extraction O All
    measure rate Orbite
    and/or measured measured process
    Raw evaluated for testing (ALP) recovery
    material (% wt.) (% wt.) (%) (%)
    Al2O3 6.12 6.12 89.65 86.97
    Fe2O3 15.80 15.80 99.50 97.51
    SiO2 36.00 36.00 0.000 99.997
    MgO 3.08 3.08 99.75 92.66
    Na2O 1.13 1.13 99.50 99.50
    K2O 2.12 2.12 99.50 99.50
    CaO 6.10 6.10 99.50 99.00
    S total 0.22 0.22 100.00
    F 1.98 1.98 99.50 99.00
    TiO2 0.13 0.13 0.000 99.03
    V2O5 0.00 0.00 98.00 96.04
    P2O5 1.10 1.10 98.00 96.04
    MnO 0.43 0.43 98.00 96.04
    ZrO2 12.43 12.43 22.70 20.43
    Cr2O3 0.00 0.00 0.00 0.00
    Ce2O3 3.05 3.045 97.31 92.98
    La2O3 1.34 1.337 99.55 92.68
    Nd2O3 1.55 1.551 98.40 94.79
    Pr2O3 0.37 0.375 99.75 97.52
    Sm2O3 0.15 0.151 88.75 84.80
    Dy2O3 0.09 0.089 80.35 76.77
    Er2O3 0.03 0.030 72.60 69.37
    Eu2O3 0.03 0.027 85.57 81.76
    Gd2O3 0.21 0.205 82.85 79.16
    Ho2O3 0.01 0.013 77.10 73.67
    Lu2O3 0.00 0.003 60.15 57.47
    Tb2O3 0.02 0.022 78.05 74.58
    Th 0.02 0.022 88.10 84.18
    Tm2O3 0.00 0.004 66.85 63.88
    U 0.01 0.014 81.90 78.26
    Y2O3 0.30 0.300 72.70 69.46
    Yb2O3 0.02 0.023 62.80 60.01
    Ga2O3 0.02 0.016 96.90 92.59
    Sc2O3 0.00 0.003 95.00 90.77
    LOI 6.122023973 6.12
    (inc. water)
  • TABLE 28
    Tests made on carbonatite
    Composition Average Extraction O All
    measure measured rate Orbite
    and/or for measured process
    Raw evaluated testing (ALP) recovery
    material (% wt.) (% wt.) (%) (%)
    Al2O3 0.70 0.70 84.31 81.61
    Fe2O3 11.22 11.22 94.14 92.15
    SiO2 2.11 2.11 0.00003 99.997
    MgO 6.50 6.500 100 96.25
    Na2O 0.07 0.07 92.54 90.55
    K2O 0.18 0.181 37.33 37.33
    CaO 16.51 16.51 100 98.00
    TiO2 0.00 0.000 0.00000 100.000
    V2O5 0.00 0.000 0 100.000
    P2O5 0.00 0.000 0 100.000
    MnO 0.00 0.000 0 100.000
    ZrO2 0.00 0.000 0 100.000
    Cr2O3 0.00 0.000 0 100.000
    Ce2O3 1.19 1.195 64.04 61.190
    La2O3 0.46 0.463 63.86 61.018
    Nd2O3 0.45 0.448 81.46 77.835
    Pr2O3 0.14 0.142 67.59 64.582
    Sm2O3 0.03 0.033 65.32 62.413
    Dy2O3 0.00 0.000 78.12 74.644
    Er2O3 0.00 0.000 86.15 82.316
    Eu2O3 0.01 0.007 66.45 63.493
    Gd2O3 0.01 0.013 54.46 52.037
    Ho2O3 0.00 0.000 83.12 79.421
    Lu2O3 0.00 0.000 88.86 84.906
    Tb2O3 0.00 0.001 41.42 39.577
    Th 0.06 0.065
    Tm2O3 0.00 0.000 90.70 86.664
    U 0.01 0.007
    Y2O3 0.00 0.000 84.68 80.912
    Yb2O3 0.00 0.000 85.11 81.323
    Ga2O3 0.00 0.000 0 0.000
    Sc2O3 0.00 0.000 0 0.000
    LOI 60.33
    (Inc. water)
  • It can thus be inferred from the results shown in Table 28 that the various metals, rare earth elements and rare metals extracted present in the obtained leaching composition can eventually be isolated by the processes of the present disclosure such as, for example, those presented in Examples 1, 2 and 5.
  • The process shown in FIG. 8 is similar to the process of FIG. 1, with the exception that in FIG. 8, the term “aluminum” is replaced by a “first metal”. The person skilled in the art would thus understand that in accordance with the present disclosure, the processes can also encompass recovering various other products and using various types of material as starting material. The first metal can be chosen from Al, Fe, Ti, Zn, Ni, Co, Mg, Li, Mn, Cu, Au, Ag, Pd, Pt. and mixtures thereof etc. Such a process can thus be used for recovering various other metals than aluminum. Thus, the first metal will be precipitated as a chloride in stage 5 and eventually converted into an oxide.
  • In fact, the person skilled in the art would understand that by replacing in FIGS. 1, 3, 6 and 7 the term “aluminum” with the expression “first metal” the processes shown in these figures can be used to obtain various other products than alumina and also used for treating various different starting material. Thus, the first metal can be recovered as a chloride (as it is the case for aluminum chlorides in the processes of FIGS. 1, 3, 6 and 7) and all the other stages of these processes can thus be carried out (when applicable) depending on the nature of the starting material used.
  • In step 4, the first metal chloride can be precipitated or crystallized. In fact, the first metal can be removed from the leachate in various manner. For example, a precipitating agent can be added or HCl (for example gaseous) can be reacted with the liquid obtained from step 3 so as to cause precipitation and/or crystallization of the first metal chloride. Alternatively, the temperature of the leachate can be controlled so as to substantially selectively cause precipitation of the first metal chloride. This can also be done, for example, by using an ion exchange resin, by adding a precipitating agent, etc. Combinations of various possibilities mentioned in this paragraph can also be envisaged. All these methods of at least substantially selectively recovering the first metal chloride can also be applied on the first metal oxide. They can be applied to only the first metal chloride, only to the second metal oxide or to both of them. In fact, the liquid obtained after stage 4 can be treated so as to convert the second metal chloride into the corresponding oxide and then, the second metal oxide can be substantially selectively recovered by selectively precipitating and/or crystalizing such a second metal oxide, for example by controlling the temperature, by using an ion exchange resin, by adding a precipitating agent, by adding HCl, or mixtures thereof.
  • As previously indicated, the processes of the present disclosure can be efficient for treating material comprising Al, Fe, Ti, Zn, Ni, Co, Mg, Li, Mn, Cu, Au, Ag, Pd, Pt.
  • For example, when treating a material that comprises, for example, Mg and Fe, the material can be leached for example by using HCl. Then, while the mixture (comprising a solid and a liquid) so obtained is still hot, it can be treated so as to separate the solid from the solid (for example by means of a solid/liquid separation). That will be effective for removing solids such as Si and optionally others such as Ti. Thus, the liquid can be cooled down to a temperature of about 5 to about 70° C., about 10 to about 60° C., about 10 to about 50° C., about 10 to about 40° C., or about 15 to about 30° C. so as to substantially selectively precipitate or crystalize magnesium (for example as MgCl2 (first metal chloride in FIG. 8)), as shown in 4 of such a figure. Then, the first metal chloride can be converted as shown in 5 so as to obtain the first metal oxide. The iron can then be treated as in 6 of FIG. 8. The remainder of the process shown in FIG. 8 (stages 6 to 10) being as described previously for FIG. 1.
  • In a similar manner, the expression “iron oxides” in step 6 can be replaced in FIG. 8 by “second metal oxide”. The person skilled in the art would thus understand that another metal than iron could be recovered as an oxide pursuant, for example, to a treatment of the liquid obtained from step 4. As previously discussed, the chloride of the second metal obtained from step 4 can be treated so as to substantially selectively recover the chloride of the second metal. This can be done, for example, by selectively precipitating and/or crystallizing such a second metal chloride by controlling the temperature, by substantially selectively hydrolyzing such a second metal chloride, by using an ion exchange resin, by adding a precipitating agent, by adding HCl, or mixtures thereof. All these methods of at least substantially selectively recovering the second metal chloride can also be applied on the second metal oxide. The can be applied to only the second metal chloride, only to the second metal oxide or to both of them. In fact, the liquid obtained after stage 4 can be treated so as to convert the second metal chloride into the corresponding oxide and then, the second metal oxide can be substantially selectively recovered by selectively precipitating and/or crystalizing such a second metal oxide, for example by controlling the temperature, by using an ion exchange resin, by adding a precipitating agent, by adding HCl, or mixtures thereof.
  • Alternatively, the iron chloride can be treated by means of a pyrohydrolysis in order to generate Cl2. In such a case, the Cl2 so produced can be used in step 13 of FIG. 8 for treating the solid that comprises Ti. For example, it can be used to convert TiO2 into TiCl4. Such a reaction can be carried under oxidizing conditions (for example more than 4% of O2). The pyrohydrolysis can be carried out in in a fluid bed reactor under such oxidizing conditions.
  • For example, platinum and palladium can also be treated similarly. Moreover, their separation can also be accomplished with ion exchange: selective crystallization in HCl is possible and can be temperature sensitive.
  • FIGS. 9A and 9B show methods for separating Si from Ti. For example, when using an ore as starting material, leaching can be carried out in the presence of Cl2 (optionally in the presence of carbon) so as to maintain Ti under the form of TiCl4 since in remains in solution (fluid) while Si remains solid (SiO2). Then, Ti (such as TiCl4) can be heated so as to be converted into TiO2. For example, it can be injected into a plasma torch for being purified.
  • Such a method for purifying Si and Ti can be used in all the processes of the present disclosure when there is a need for separating these two entities. See stage 13 in FIGS. 1, 3 and 8 and stage 113 in FIGS. 6 and 7.
  • The processes of the present disclosure provide a plurality of important advantages and distinction over the known processes. This is true for the production of various products has previously indicated.
  • The processes of the present disclosure can provide economical solutions that can successfully extract various products from various type of materials while providing ultra pure secondary products of high added value including highly concentrated rare earth elements and rare metals. The technology described in the present disclosure can allow for an innovative amount of total acid recovery and also for a ultra high concentration of recovered acid. When combing it to the fact that combined with a semi-continuous leaching approach that favors very high extraction yields and allows a specific method of crystallization of some products, and concentration of other value added elements.
  • For example, the crystallization of AlCl3 into AlCl3.6H2O using dried, cleaned and highly concentrated gaseous HCl as the sparging agent allows for a pure aluminum chloride hexahydrate with only few parts per million of iron and other impurities. A minimal number of stages are required to allow proper crystal growth.
  • The direct interconnection with the calcination of AlCl3.6H2O into Al2O3 which does produce very high concentration of gas allows the exact adjustment in continuous of the HCl concentration within the crystallizer and thus proper control of the crystal growth and crystallization process.
  • The applicants have now discovered fully integrated and continuous processes with substantially total hydrochloric acid recovery for the extraction of alumina and other value added products from various materials that contain aluminum (clay, bauxite, aluminosilicate materials, slag, red mud, fly ashes etc.) containing aluminum. In fact, the processes allows for the production of substantially pure alumina and other value added products purified such as purified silica, pure hematite, titanium oxide, pure other minerals (ex: magnesium oxide) and rare earth elements products. In addition, the processes do not necessary require thermal pre-treatment before the acid leach operation. Acid leach can be carried out using semi-continuous techniques with high pressure and temperature conditions and very high regenerated hydrochloric acid concentration. In addition, the processes do not generate any residues not sellable, thus eliminating harmful residues to environment like in the case of alkaline processes.
  • The advantage of the high temperature calcination stage, in addition for allowing to control the α-form of alumina required, can be effective for providing a concentration of hydrochloric acid in the aqueous form (>38%) that is higher than the concentration of HCl at the azeotropic point and thus providing a higher incoming HCl concentration to the leaching stage. The calcination stage hydrochloric acid network can be interconnected to two (2) crystallization systems and by pressure regulation excess HCl can be being absorbed at the highest possible aqueous concentration. The advantage of having a hexahydrate chloride with low moisture content (<2%) incoming feed can allow for a continuous basis to recover acid at a concentration that is higher than the azeotropic concentration. This HCl balance and double usage into three (3) common parts of the processes and above azeotropic point is a substantial advance in the art.
  • Another advantage can be the use of the incoming chemistry (ferric chloride) to the iron oxide and hydrochloric acid recovery unit where all excess heat load from any calcination part, pyrohydrolysis and leaching part is being recovered to preconcentrate the mother liquor in metal chloride, thus allowing, at very low temperature, the hydrolysis of the ferric chloride in the form of very pure hematite and the acid regeneration at the same concentration than at its azeotropic point.
  • For example, the processes of the present disclosure can be effective for providing, at the ferric chloride hydrolysis step, the possibility to concentrate rare earth elements in form of chlorides at very high concentration within the hydrolyser reactor through an internal loop between hydrolyzer and crystallization. The advantage in that the processes of the present disclosure benefit from the various steps where gradual concentration ratios are applied. Thus, at this stage, in addition to an internal concentration loop, having the silica, the aluminum, the iron and having in equilibrium a solution close to saturation (large amount of water evaporated, no presence of free hydrochloric acid) allows for taking rare earth elements and non-hydrolysable elements in parts per million into the incoming feed and to concentrate them in high percentage directly at the hydrolyser after ferric chloride removal Purification of the specific oxides (RE-O) can then be performed using various techniques when in percentage levels. The advantage is doubled here: concentration at very high level of rare earth elements using integrated process stages and most importantly the approach prevents from having the main stream (very diluted) of spent acid after the leaching step with the risk of contaminating the main aluminum chloride stream and thus affecting yields in Al2O3. Another important improvement of the art is that on top of being fully integrated, selective removal of components allows for the concentration of rare earth elements to relatively high concentration (percentages).
  • Another advantage of the processes can be a selective crystallization of MgCl2 through the sparging of HCl. Highly concentrated acid both in gaseous phase or in aqueous form can thus be be generated. As previously indicated, Mg(OH)2 can also be obtained. As per aluminum chloride specific crystallization, the direct interconnection with the calcination reactor, the HCl gas very high concentration (about 85 to about 95%, about 90 to 95% or about 90% by weight) can allow for exact adjustment in continuous of the crystallizer based on quality of magnesium oxide targeted.
  • The pyrohydrolysis can allow for conversion of any remaining chloride and the production of refined oxides that can be used (in case of clay as starting material) as a fertilizer and allowing the processing of large amount of wash water from the processes with the recovery hydrochloric acid in close loop at the azeotropic point for the leaching step. This is related to the fact that it does totally close the process loop in terms of acid recovery and the insurance that no residues harmful to the environment are being generated while processing any type of raw material, as previously described.
  • It was demonstrated that the processes of the present disclosure offer effective solutions for extracting various metals from various materials. For example, it was demonstrated that materials that contain titanium can be efficiently treated so as to recover titanium therefrom while also recovering other metals as those described in the present disclosure.
  • It was thus demonstrated that the present disclosure provides fully integrated processes for the extraction and/or recovery of titanium and/or for the preparation of titanium chloride or titanium oxide using a hydrochloric acid treatment while producing high purity and high quality products (minerals) and optionally extracting rare earth elements and rare metals.
  • With respect to the above-mentioned examples 1 to 5, the person skilled in the art will also understand that depending on the starting material used some parameters might need to be adjusted consequently. In fact, for example, certain parameters such as reaction time, concentration, temperature may vary in accordance with the reactivity of the selected starting material.
  • While a description was made with particular reference to the specific embodiments, it will be understood that numerous modifications thereto will appear to those skilled in the art. Accordingly, the above description and accompanying drawings should be taken as specific examples and not in a limiting sense.

Claims (22)

What is claimed is:
1. A process for preparing various products, the process comprising:
leaching a titanium-containing material comprising Ti, Si and a first metal with HCl so as to obtain a leachate comprising ions of said first metal and a solid comprising titanium, and separating the solid from the leachate;
reacting the leachate with HCl so as to obtain a liquid and a precipitate comprising a chloride of the first metal, and separating the precipitate from the liquid;
optionally heating the precipitate under conditions effective for converting the chloride of the first metal into an oxide of the first metal and optionally recovering HCl so-produced; and
treating said solid so as to substantially separate Si from Ti that are contained therein.
2. The process of claim 1, wherein said first metal is chosen from aluminum, iron, zinc, copper, gold, silver, molybdenum, cobalt, magnesium, lithium, manganese, nickel, palladium, platinum, thorium, phosphorus, uranium and titanium, and/or at least one rare earth element and/or at least one rare metal
3. The process of claim 1, wherein said first metal is chosen from aluminum, iron, zinc, copper, gold, silver, magnesium, nickel, palladium, platinum, and/or at least one rare earth element and/or at least one rare metal
4. The process of claim 2, wherein the liquid comprises a second metal.
5. The process of claim 3, wherein said second metal is chosen from aluminum, iron, zinc, copper, gold, silver, molybdenum, cobalt, magnesium, lithium, manganese, nickel, palladium, platinum, thorium, phosphorus, uranium and titanium, and/or at least one rare earth element and/or at least one rare metal.
6. The process of claim 4, wherein said process comprises separating the precipitate from the liquid and heating the second metal in order to convert a chloride of the second metal into an oxide of the second metal.
7. The process of claim 5, wherein separating Si from Ti that are contained in said solid comprises leaching said solid with an acid so as to obtain a liquid portion comprising Ti and a solid portion containing Si and wherein the liquid portion is separated from the solid portion.
8. The process of claim 6, wherein said acid is chosen from HCl, HNO3, H2SO4 and mixtures thereof.
9. The process of claim 6, wherein said solid is leached with HCl in the presence of a chloride.
10. The process of claim 8, comprising treating said solid with HCl at a concentration of less than 20% by weight, at a temperature of less than 85° C., in the presence of a chloride, so as to separate Si from Ti that are contained therein.
11. The process of claim 8, wherein said chloride is MgCl2 or ZnCl2.
12. The process of claim 1, wherein said solid comprises TiO2 and SiO2 and said solid is treated with Cl2 and carbon in order to obtain a liquid portion and a solid portion, and wherein said solid portion and said liquid portion are separated from one another.
13. The process of claim 1, wherein said process comprises
separating the solid from the leachate;
leaching said solid with an acid so as to obtain another leachate and another solid comprising Si and Ti, and
recovering a third metal from said another leachate.
14. The process of claim 13, wherein said third metal is chosen from aluminum, iron, zinc, copper, gold, silver, molybdenum, cobalt, magnesium, lithium, manganese, nickel, palladium, platinum, thorium, phosphorus, uranium and titanium, and/or at least one rare earth element and/or at least one rare metal.
15. The process of claim 1, wherein said titanium-containing material is leached with HCl having a concentration of about 25 to about 45 weight %.
16. The process of claim 1, wherein said process further comprises recycling said gaseous HCl so-produced by contacting it with water so as to obtain a composition having a concentration of about 25 to about 45 weight % and using said composition for leaching said titanium-containing material.
17. The process of claim 16, wherein said recycled gaseous HCl so-produced is contacted with water so as to obtain said composition having a concentration of about 26 to about 42 weight.
18. The process of claim 1, wherein said titanium-containing material is red mud or fly ash.
19. The process of claim 18, wherein converting the chloride of the first metal into an oxide of the first metal is carried out by a calcination, the calcination comprising steam injection.
20. A process for preparing various products, the process comprising:
leaching an aluminum-containing material HCl so as to obtain a leachate comprising ions of said first metal and a solid, and separating the solid from the leachate;
reacting the leachate with HCl so as to obtain a liquid and a precipitate comprising a chloride of the first metal, and separating the precipitate from the liquid;
optionally heating the precipitate under conditions effective for converting the chloride of the first metal into an oxide of the first metal and optionally recovering HCl so-produced;
carrying out an hydrolysis on said liquid in order to recover a second metal in the form of an oxide; and
optionally treating said solid so as to recover a third metal.
21. The process of claim 20, wherein said second metal is chosen from zinc, copper, and nickel.
22. The process of claim 21, wherein said first metal is chosen from aluminum, manganese and magnesium.
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