WO2008139412A1 - Procédé d'obtention d'un métal du type zinc à partir de minerais de type sulfures par lixiviation aux chlorures et extraction électrolytique - Google Patents

Procédé d'obtention d'un métal du type zinc à partir de minerais de type sulfures par lixiviation aux chlorures et extraction électrolytique Download PDF

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Publication number
WO2008139412A1
WO2008139412A1 PCT/IB2008/051873 IB2008051873W WO2008139412A1 WO 2008139412 A1 WO2008139412 A1 WO 2008139412A1 IB 2008051873 W IB2008051873 W IB 2008051873W WO 2008139412 A1 WO2008139412 A1 WO 2008139412A1
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WO
WIPO (PCT)
Prior art keywords
metal
cell
zinc
chlorine gas
electrolytic
Prior art date
Application number
PCT/IB2008/051873
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English (en)
Inventor
Johann Du Toit Steyl
Jan Tjeerd Smit
Original Assignee
Anglo Operations Limited
Priority date (The priority date is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the date listed.)
Filing date
Publication date
Application filed by Anglo Operations Limited filed Critical Anglo Operations Limited
Publication of WO2008139412A1 publication Critical patent/WO2008139412A1/fr

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Classifications

    • 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
    • C22B19/00—Obtaining zinc or zinc oxide
    • C22B19/20—Obtaining zinc otherwise than by distilling
    • C22B19/22—Obtaining zinc otherwise than by distilling with leaching with acids
    • 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
    • C22B15/00—Obtaining copper
    • C22B15/0063—Hydrometallurgy
    • C22B15/0065—Leaching or slurrying
    • C22B15/0067—Leaching or slurrying with acids or salts thereof
    • C22B15/0069—Leaching or slurrying with acids or salts thereof containing halogen
    • 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
    • C22B23/00—Obtaining nickel or cobalt
    • C22B23/04—Obtaining nickel or cobalt by wet processes
    • C22B23/0407—Leaching processes
    • C22B23/0415—Leaching processes with acids or salt solutions except ammonium salts solutions
    • C22B23/0423—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
    • C22B3/04—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
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
    • C25B1/00—Electrolytic production of inorganic compounds or non-metals
    • C25B1/01—Products
    • C25B1/24—Halogens or compounds thereof
    • C25B1/26—Chlorine; Compounds thereof
    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25C—PROCESSES FOR THE ELECTROLYTIC PRODUCTION, RECOVERY OR REFINING OF METALS; APPARATUS THEREFOR
    • C25C1/00—Electrolytic production, recovery or refining of metals by electrolysis of solutions
    • C25C1/16—Electrolytic production, recovery or refining of metals by electrolysis of solutions of zinc, cadmium or mercury
    • 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 invention provides a process for producing a metal from sulphide ores.
  • roast Leach Electrowinning RLE
  • This process produces zinc metal and excess acid (SO 2 - equivalent to the sulphur entering with the ore), which cannot be directly discharged into the environment.
  • Zinc ferrite (formed during the roasting step) processing is expensive and technically challenging (especially when the feed ore contains high iron), since a high acid leach (HAL) is associated with more iron leaching (which has to be neutralised in situ during hydrolysation).
  • HAL high acid leach
  • ferri- hydrite formation is effective in controlling various heavy metal impurities, this residue material is not environmentally inert, thus it has to be contained and cannot be simply used as landfill.
  • jarosite precipitation has been proposed as an alternative (the zinc ferrite would have to be leached under conditions where jarosite is stable). Long residence times would, however, be required to achieve this, as well as a suitable cation, such as sodium. Some sulphur is lost from the circuit as part of the jarosite phase. Similarly to ferri-hydrite, jarosite disposal is a problem (it is bulky and further treatment is required in order for it to be used as landfill).
  • goethite is not considered a good alternative because the feed solution requires pre-reduction (prior to slow oxidation) or dilution ⁇ in large tanks) in order to kinetically favour goethite formation during hydrolysis and goethite would not stand up to the harsh HAL conditions.
  • hematite despite containing the highest weight percentage iron, as compared to the other hydrolysis products precipitation would not integrate well with a ferrite leaching step (high lime cost), not to mention the fact that pre-reduction (reductant), followed by slow oxidation (oxidant) and seeding would be required in order for it to form under atmospheric conditions.
  • the Pressure Oxidation (POX) Process resolves the iron issue because hydrolysis is temperature driven, and thus there is no need for in-situ neutralisation ( Figure 2).
  • the process takes place in an autoclave at 15O 0 C and hematite is the preferred hydrolysis product. Sulphur, entering with the sulphide ore, is almost stoichiometricaily converted into elemental sulphur, exiting with the final hematite residue, i.e. it does not add to process revenue (from producing elemental sulphur).
  • the POX Process is simple and acid is utilised optimally due to the rejection of iron in the main process step (the autoclave) itself, thus releasing the sulphate that was initially consumed by the iron impurity.
  • a counter-current integration of two autoclaves is utilised to achieve both high zinc extraction and near complete iron removal.
  • the inefficiency of the process is exclusively contained in approximately 10 g/l residual acid and 2 g/l iron in the final PLS, and less than 1% zinc in the final residue. This is exactly the aspect that would be difficult to compete with in an atmospheric process, where acid cannot be regenerated in situ.
  • chloride medium may be adopted in the leaching step in order to achieve a more efficient integration with the rest of the circuit.
  • the HydroCopper Process (Hyvarinen and Hamalainen, 1999) integrates the chloride leach with the chlor-alkali cell (standard technology), to produce internally all the reagents required for regenerating the primary leaching agent (cupric ion) and to recover value metal.
  • the lntec process (www.intec.com.au).
  • a method for producing a metal from a metal sulphide ore or mineral including the steps of:
  • the hydrogen sulphide, or a portion thereof, may be used to convert the chlorine gas into hydrochloric acid, thereby also producing elemental sulphur.
  • an additional hydrogen source whether produced in the process or not, may be used to convert the chlorine gas into hydrochloric acid.
  • the hydrochloric acid may be returned to the chloride solution.
  • the chlorine may be produced in an electrolytic cell, such as a zinc metal electrowinning cell, a chlor-alkali cell, an iron metal electrowinning cell, a manganese metal electrowinning cell, an iron-manganese alloy electrowinning cell or any combination of these electrolytic cells or any other electrolytic cell that can be used to selectively remove a metal from solution while producing chlorine gas at the anode.
  • an electrolytic cell such as a zinc metal electrowinning cell, a chlor-alkali cell, an iron metal electrowinning cell, a manganese metal electrowinning cell, an iron-manganese alloy electrowinning cell or any combination of these electrolytic cells or any other electrolytic cell that can be used to selectively remove a metal from solution while producing chlorine gas at the anode.
  • the metal may be a valuable (value) metal, such as zinc.
  • the method may be conducted at atmospheric pressure and without the formation of elemental sulphur.
  • the bulk of the sulphide sulphur may be recovered as an elemental sulphur byproduct, while harvesting the energy of the sulphide sulphur oxidation to elemental sulphur and reducing the need for fresh reagent make-up.
  • Impurities may be removed from soiution to levels required by electrolytic processes.
  • chemicals produced in the process such as chlorine gas, caustic soda, hydrogen sulphide, hydrogen gas, metal (for example zinc), sulphur dioxide, and/or sulphur dioxide/oxygen mixture, will be used to remove the impurities.
  • Cooling, salting out or evaporative crystallisation may also be used to remove impurities.
  • solvent extraction may be used to produce a solution, pure enough to be subjected to the electrolytic process.
  • electrolytic processes may be included in the integrated flowsheet to directly remove iron as a metal and/or manganese as a metal or alternatively in one single cell as an iron- manganese alloy.
  • the method may be used without first pre-concentrating the minerals in a cleaner concentrate.
  • direct treatment of the minerals in the form of a bulk concentrate may be possible, or even direct treatment of the raw ore.
  • the overall metal recovery may thereby be increased.
  • the method may therefore be performed without the need for a fine grinding step of the ore.
  • a portion or all of the hydrogen sulphide may be converted to elemental sulphur using Claus or other technology.
  • a portion of the hydrogen sulphide may be burned in air or oxygen to produce sulphur dioxide, which may be converted to sulphuric acid.
  • the sulphuric acid may then be used to replace an equivalent amount of hydrochloric acid in a mixed chloride/sulphate brine leach.
  • Sulphate salts of metals may be produced and removed from the leach process, thermally decomposed to oxides and sulphur dioxide and subsequently converted to sulphuric acid.
  • FIG 1 shows the commercial Roast-Leach-Electrowinning (RLE) process
  • FIG. 1 shows the commercial Pressure Oxidation (POX) process
  • Figure 3 shows the generic oxidative atmospheric leach (AL) concept (near commercialisation ref. Albion Process);
  • Figure 4 shows a first embodiment of the present invention, integrating a non- oxidative sulphide leach step with a Chlor-alkali electrolytic cell, and regenerating hydrochloric acid via reaction of chlorine gas with hydrogen sulphide gas;
  • Figure 5 shows a second embodiment of the present invention, integrating the non-oxidative sulphide leach step with the Zn electrowinning cell, and regenerating hydrochloric acid via reaction of chlorine gas with hydrogen sulphide gas;
  • Figure 6 shows a third embodiment of the present invention, integrating the non- oxidative sulphide leach step with both the chlor-alkali electrolytic cell and the zinc electrowinning cell, and regenerating hydrochloric acid via reaction of chlorine gas with hydrogen sulphide gas, hydrogen gas from the chlor-alkali electrolytic cell and/or an alternative source of hydrogen;
  • Figure 7 shows a fourth embodiment of the present invention, integrating the non-oxidative sulphide leach / purification / zinc electrowinning / hydrochloric acid regeneration circuit with the chlor-alkali electrolytic cell and/or the iron-manganese electrowinning cell/s.
  • the new process will be described and exemplified below with reference to zinc as the metaf to be obtained from the sulphide ore, but it is intended that the invention could apply to any metal, and in particular any value metal, i.e. any metal from which revenue can be generated.
  • the metal may be a light metal, base metal or precious metal, such as Zn, Cu, Mo, Ti, Al, Cr, Ni, Co, Mn, Fe 1 Pb, Na, K, Ca, Ag, Au and platinum group metals.
  • the ore may be any metal bearing ore containing sulphide (e.g. sphalerite), which may be in a disseminated form.
  • sulphide e.g. sphalerite
  • the major drawback of operating under atmospheric pressure is the absence of a thermal driving force for the in-situ regeneration of the acid (equivalent to the amount of Fe entering the leach).
  • a major advantage of opting for a heap leaching operation would be the direct utilisation of the ore, thus eliminating the need for upgrading (and hence the associated metal losses).
  • Process selection may be a playoff between POX (low risk but high capex) or, for example, heap leaching (lower capex and probably a higher overall Zn recovery, but also higher neutralisation costs and a high risk associated with controlling the heap).
  • Local environmental factors fluorhydrite vs. hematite formation
  • the Zn grade of the feed ore would also be important. If the primary leach is to be conducted in a tank, using ferric ion ⁇ Albion approach), ultra-fine grinding (80% passing 3 ⁇ m) would be required. It would also be necessary to remove the elemental sulphur (via flotation, for example), prior to disposal, to ensure that the tailings (containing the jarosite precipitate) are environmentally acceptable.
  • All of these process flowsheets require an effluent stream and, at least, a bleed stream to be neutralised (the residual acid, present as free acid and Fe) in order to control the impurity levels and to recover the Zn. If a major portion of the sulphide sulphur is converted to elemental sulphur (stoichiometricaily more than what is recovered during the electrowinning of Zn), a deficiency of sulphate would exist, which would have to be added externally, resulting in higher operating costs. This is not desirable, especially since the feed ore introduces a potential source of sulphur that is best utilised in order to compete with POX. Heap leaching, on the other hand, produces excess amounts of acid during the oxidation of sulphide sulphur and would require a neutralising reagent to be added.
  • This process introduces an atmospheric leaching process, which utilises chloride brine (the term 'brine' as used herein is intended to possibly include sulphate as well as NaCI) solution as the lixiviant, ensuring comparative (cf. other atmospheric leaching processes) leaching kinetics, but without the need for fine-grinding.
  • chloride brine the term 'brine' as used herein is intended to possibly include sulphate as well as NaCI
  • the applicant has shown that the presence of ZnCI 2 negatively effects zinc extraction, but this can be overcome by the addition of NaCI, which increases zinc extraction. It is therefore beneficial to conduct the leaching step in a high sodium chloride environment.
  • the leaching process operates non-oxidatively, which eliminates the presence of elemental sulphur product layers that may adversely affect leaching kinetics under otherwise oxidative conditions:
  • the vapour stream of the non-oxidative leaching step can be integrated with an electrochemica ⁇ y generated chlorine gas stream in order to control the extent of elemental sulphur production.
  • Hydrogen sulphide gas a product of the non-oxidative Jeaching step, reacts with chlorine gas to produce elemental sulphur and hydrochloric acid (Sims and Sheinbaum): H 2 S + Cl 2 ⁇ S° + 2HCI (2)
  • Chlorine gas production using electrical energy, may be incorporated into the flowsheet via the conventional chlor-alkali technology, as commercially applied throughout the world, using, for example, cheap and readily available sodium chloride sa!t as make-up reagent
  • the chloride processes are characterised by improved current efficiency, besides the fact that chlorine gas may be used to regenerate the primary leaching agent, i.e. hydrochioric acid.
  • the two schemes described above are independently illustrated in Figures 4 and 5, respectively.
  • These electrolytic processes may also be combined in a novel way into one flowsheet, as depicted in Figure 6.
  • the function of the chlor-alkali cell would be primarily to regenerate the equivalent amount of chlorine (hydrochloric acid) that was originally consumed by the impurities in the primary leach, and at the same time produce the required amount of caustic to remove these impurities from the circuit.
  • the water balance in the circuit would probably be maintained by a multiple-effect evaporation step. This is the point in the circuit where sodium chloride is likely to precipitate (due to super-saturation).
  • This salt may then be recycled back to the chlor- alkali cell, which would substantially reduce or eliminate the sodium chloride make-up requirement.
  • impurities such as iron and manganese may also be electrowon, thereby reducing the relative size of the chlor-alkali plant.
  • impurities such as iron and manganese may also be electrowon, thereby reducing the relative size of the chlor-alkali plant.
  • the major advantage of such a scheme wouid be associated with the potential by-product value from producing iron and/or manganese metal.
  • This unit is expected to be a minor electrowin ⁇ ing operation since the iron content in a zinc concentrate is typically a 1/5 th or less compared to the zinc content.
  • Another advantage of producing iron metal would be its low volume compared to an iron hydrolysis residue. Very little wash-water would also be added to the circuit, making the water balance (and hence, the energy requirement) more favourable:
  • Figure 7 represents a schematic illustration of how this electrowinning of iron and/or manganese impurity may be integrated into the circuit. However, this step may potentially be introduced in any part of the circuit, provided the operating conditions at that specific point in the circuit are conducive to the technical and economical viability of flowsheet.
  • these purification steps may include any commercial or non-commercial method without detracting from the main process concept, as described above.
  • these purification steps would utilise the chemicals produced in the process itself, for example: chlorine gas, caustic soda, hydrogen sulphide, zinc metal, hydrogen gas, sulphur dioxide, and/or sulphur dioxide/oxygen mixture, and the like, although external reagents could also be added.
  • cooling, evaporative or salting-out crystallisation may be utilised to remove impurities, such as Fe(II).
  • Solvent extraction may also be utilised to produce a pure enough solution for the electrolytic processes. Solvent extraction may be integrated into the basic concept of this invention to the best benefit of the workings of the basic flowsheet.
  • a portion of the hydrogen sulphide gas may be converted to elemental sulphur using the well-known Claus technology, or other similar technology, as, for example, frequently applied in the petrochemical industry.
  • any source of hydrogen may be used to covert chlorine gas into hydrochloric acid.
  • a portion of the hydrogen sulphide gas may be burned in air or oxygen to produce sulphur dioxide, which may be converted to sulphuric acid in an acid plant.
  • This sulphuric acid may then replace the equivalent amount of hydrochloric acid in a mixed chloride/sulphate brine leach.
  • sulphate salts of any of the metals may be produced and removed from the process stream, thermally decomposed to the oxide and sulphur dioxide gas and similarly converted to sulphuric acid. Any one or combination of the above schemes may be utilised to control the reagent regeneration cycles and the management of the hydronium ion, total chloride and total sulphur balance around the circuit. This would automatically reduce the requirement of fresh reagent make-up in the control of the circuit and management of the major impurities.
  • the process of this invention has the potential for: a) reducing capital and operating expenditure - the reagent consumption is essentially nil (excluding reagent top-up as required).
  • the primary leaching agent is regenerated, there is no neutralisation of the main process stream amd the neutralisation agents are regenerated internally; b) catering for ores which cannot be treated or are difficult to treat by conventional means (e.g.
  • extractants e.g. Alamine 336TM, Aliquat 336TM, Cyanex 921 TM, Cyanex 923TM, isodecanol, t ⁇ -/7-butylphosphate and dJbutylbutylphosphonate.
  • Alamine 336TM Aliquat 336TM
  • Cyanex 921 TM Cyanex 923TM
  • isodecanol t ⁇ -/7-butylphosphate
  • dJbutylbutylphosphonate dJbutylbutylphosphonate
  • the plating of relatively smooth, adherent deposits of zinc and iron has been achieved by electrowinning.
  • the energy consumption for the plating from the chloride medium is lower than that for the sulphate medium (energy consumption of 2.7 kWh/kg Zn for the deposition of zinc from the chloride system as compared to 3.2-3.3 kWh/kg Zn for the typical sulphate systems).
  • Tests have also been conducted to codeposit iron and manganese.

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  • Engineering & Computer Science (AREA)
  • Organic Chemistry (AREA)
  • Metallurgy (AREA)
  • Materials Engineering (AREA)
  • Manufacturing & Machinery (AREA)
  • Mechanical Engineering (AREA)
  • Inorganic Chemistry (AREA)
  • Chemical Kinetics & Catalysis (AREA)
  • Electrochemistry (AREA)
  • Geology (AREA)
  • Geochemistry & Mineralogy (AREA)
  • General Life Sciences & Earth Sciences (AREA)
  • Environmental & Geological Engineering (AREA)
  • Life Sciences & Earth Sciences (AREA)
  • Manufacture And Refinement Of Metals (AREA)
  • Electrolytic Production Of Metals (AREA)

Abstract

L'invention porte sur un procédé de fabrication d'un métal à partir d'un minerai ou minéral de type sulfure métallique. Le minerai de type sulfure métallique est lixivié par dissolution non oxydante dans un solution de chlorure pour donner une solution de chlorure métallique et du sulfure d'hydrogène; la solution de chlorure métallique est soumise à un ou plusieurs procédés électrolytiques pour produire du chlore gazeux; et le chlore gazeux est ensuite converti en acide chlorhydrique. Le chlore peut être produit dans une cellule électrolytique, telle qu'une cellule d'extraction électrolytique de zinc métallique, une cellule chlore-alcali, une cellule d'extraction électrolytique de fer métallique, une cellule d'extraction électrolytique de manganèse métallique, une cellule d'extraction électrolytique d'alliage fer-manganèse ou toute combinaison de ces cellules ou toute autre cellule électrolytique qui peut éliminer sélectivement un métal à partir d'une solution tout en produisant du chlore à l'anode. Le métal peut être Zn, Cu, Mo, Ti, Al, Cr, Ni, Co, Mn, Fe, Pb, Na, K, Ca, Ag, Au ou tout métal du groupe platine.
PCT/IB2008/051873 2007-05-10 2008-05-12 Procédé d'obtention d'un métal du type zinc à partir de minerais de type sulfures par lixiviation aux chlorures et extraction électrolytique WO2008139412A1 (fr)

Applications Claiming Priority (4)

Application Number Priority Date Filing Date Title
ZA2007/03789 2007-05-10
ZA200703789 2007-05-10
ZA200709205 2007-10-25
ZA2007/09205 2007-10-25

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WO2008139412A1 true WO2008139412A1 (fr) 2008-11-20

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Cited By (5)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
WO2011140593A1 (fr) * 2010-05-10 2011-11-17 Wintermute Metals Pty Ltd Récupération de métaux du groupe platine à partir de matériaux contenant des métaux du groupe platine
CN102534215A (zh) * 2010-12-08 2012-07-04 中国环境科学研究院 一种电解锰浸出液净化除铁的方法
JP2013528696A (ja) * 2010-01-22 2013-07-11 モリーコープ ミネラルズ エルエルシー 水精錬加工プロセスおよび金属の回収方法
US10400306B2 (en) 2014-05-12 2019-09-03 Summit Mining International Inc. Brine leaching process for recovering valuable metals from oxide materials
US11408053B2 (en) 2015-04-21 2022-08-09 Excir Works Corp. Methods for selective leaching and extraction of precious metals in organic solvents

Citations (4)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US4097271A (en) * 1975-12-11 1978-06-27 Cominco Ltd. Hydrometallurgical process for recovering copper and other metal values from metal sulphides
US4272341A (en) * 1980-01-09 1981-06-09 Duval Corporation Process for recovery of metal values from lead-zinc ores, even those having a high carbonate content
US4536214A (en) * 1983-07-07 1985-08-20 Duval Corporation Metal sulphide extraction
US6007600A (en) * 1997-08-29 1999-12-28 Outokumpu Oyj Method for producing copper in hydrometallurgical process

Patent Citations (4)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US4097271A (en) * 1975-12-11 1978-06-27 Cominco Ltd. Hydrometallurgical process for recovering copper and other metal values from metal sulphides
US4272341A (en) * 1980-01-09 1981-06-09 Duval Corporation Process for recovery of metal values from lead-zinc ores, even those having a high carbonate content
US4536214A (en) * 1983-07-07 1985-08-20 Duval Corporation Metal sulphide extraction
US6007600A (en) * 1997-08-29 1999-12-28 Outokumpu Oyj Method for producing copper in hydrometallurgical process

Cited By (10)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
JP2013528696A (ja) * 2010-01-22 2013-07-11 モリーコープ ミネラルズ エルエルシー 水精錬加工プロセスおよび金属の回収方法
US8936770B2 (en) 2010-01-22 2015-01-20 Molycorp Minerals, Llc Hydrometallurgical process and method for recovering metals
US10179942B2 (en) 2010-01-22 2019-01-15 Secure Natural Resources Llc Hydrometallurgical process and method for recovering metals
WO2011140593A1 (fr) * 2010-05-10 2011-11-17 Wintermute Metals Pty Ltd Récupération de métaux du groupe platine à partir de matériaux contenant des métaux du groupe platine
CN102534215A (zh) * 2010-12-08 2012-07-04 中国环境科学研究院 一种电解锰浸出液净化除铁的方法
CN102534215B (zh) * 2010-12-08 2013-10-23 中国环境科学研究院 一种电解锰浸出液净化除铁的方法
US10400306B2 (en) 2014-05-12 2019-09-03 Summit Mining International Inc. Brine leaching process for recovering valuable metals from oxide materials
US11408053B2 (en) 2015-04-21 2022-08-09 Excir Works Corp. Methods for selective leaching and extraction of precious metals in organic solvents
US11427886B2 (en) 2015-04-21 2022-08-30 Excir Works Corp. Methods for simultaneous leaching and extraction of precious metals
US11814698B2 (en) 2015-04-21 2023-11-14 Excir Works Corp. Methods for simultaneous leaching and extraction of precious metals

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