WO2010079369A1 - Produits de valeur obtenus à partir de boue rouge - Google Patents

Produits de valeur obtenus à partir de boue rouge Download PDF

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WO2010079369A1
WO2010079369A1 PCT/GR2010/000003 GR2010000003W WO2010079369A1 WO 2010079369 A1 WO2010079369 A1 WO 2010079369A1 GR 2010000003 W GR2010000003 W GR 2010000003W WO 2010079369 A1 WO2010079369 A1 WO 2010079369A1
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solution
hydrochloric acid
sulfate
solid
red mud
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PCT/GR2010/000003
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Nikolaos Papadopoulos
Haido-Stefania Karayianni
Evangelos Hristoforou
Eleni Metaxa
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Nikolaos Papadopoulos
Haido-Stefania Karayianni
Evangelos Hristoforou
Eleni Metaxa
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Publication of WO2010079369A1 publication Critical patent/WO2010079369A1/fr

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    • 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
    • C01F7/04—Preparation of alkali metal aluminates; Aluminium oxide or hydroxide therefrom
    • C01F7/06—Preparation of alkali metal aluminates; Aluminium oxide or hydroxide therefrom by treating aluminous minerals or waste-like raw materials with alkali hydroxide, e.g. leaching of bauxite according to the Bayer process
    • C01F7/066—Treatment of the separated residue
    • 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
    • C01F7/04—Preparation of alkali metal aluminates; Aluminium oxide or hydroxide therefrom
    • C01F7/06—Preparation of alkali metal aluminates; Aluminium oxide or hydroxide therefrom by treating aluminous minerals or waste-like raw materials with alkali hydroxide, e.g. leaching of bauxite according to the Bayer process
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
    • C01B17/00—Sulfur; Compounds thereof
    • C01B17/69—Sulfur trioxide; Sulfuric acid
    • C01B17/74—Preparation
    • 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
    • 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
    • C01F11/00—Compounds of calcium, strontium, or barium
    • C01F11/46—Sulfates
    • 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
    • C01F7/68—Aluminium compounds containing sulfur
    • C01F7/74—Sulfates
    • C01F7/76—Double salts, i.e. compounds containing, besides aluminium and sulfate ions, only other cations, e.g. alums
    • 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
    • C01F7/68—Aluminium compounds containing sulfur
    • C01F7/74—Sulfates
    • C01F7/76—Double salts, i.e. compounds containing, besides aluminium and sulfate ions, only other cations, e.g. alums
    • C01F7/762—Ammonium or alkali metal aluminium sulfates
    • C01F7/765—Ammonium aluminium sulfates
    • 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
    • C01G23/053—Producing by wet processes, e.g. hydrolysing titanium salts
    • 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
    • C01G23/053—Producing by wet processes, e.g. hydrolysing titanium salts
    • C01G23/0532—Producing by wet processes, e.g. hydrolysing titanium salts by hydrolysing sulfate-containing salts
    • 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
    • C01G49/08—Ferroso-ferric oxide [Fe3O4]

Definitions

  • red mud is the solid by-product of the Bayer method employed in aluminum industries when bauxite is treated with sodium hydroxide, usually at moderate temperatures and under pressure in order to produce soluble sodium aluminate.
  • the insoluble material is then called “red mud", with “red” implying the solid's color caused by its high content in iron. Since about half of the initial bauxite is used to produce aluminum metal at the next electrolytic step, it is obvious that a large amount of alkaline material has to be properly treated. Environmental issues are of great importance, too. Even at traces, toxic metals are also present in red mud sludge and because of the fine material's dispersion these often travel over long distances contaminating soil and groundwater.
  • red mud comprised mainly by the oxides of iron, aluminum, titanium, calcium, sodium and silicon varies from place to place. As far as the mineralogical phases are concerned the main differences are those of the corresponding oxides of titanium (anatase or rutile structure) and aluminum. The latter, in temperate countries (such as Mediterranean Europe) occur mainly as the monohydrate AlOOH (boehmite and diaspore), whereas in the tropics they are generally closer to the trihydrate (gibbsite and hydrargillite).
  • AlOOH is less soluble in aqueous NaOH than is Al(OH) 3 , this has a major bearing on the extraction process for Al manufacture, requiring higher concentrations of NaOH and higher temperatures and pressures than do bauxites approximating to Al(OH) 3 .
  • Red mud from the company "Aluminum of Greece” was used in the form it was received as the raw material for our experiments.
  • the composition of this material was determined by means of the ICP and XRF techniques.
  • a typical composition of red mud's components is presented in Table 1, demonstrating, in each case, the mean value of both technique's measurements.
  • red mud varies from place to place, at a ratio of +/- 10%.
  • other metals also exist in traces, the sum of which usually does not exceed 0.5 %.
  • both these aspects have been neglected for reasons of simplicity, since their adopting does not change the whole concept.
  • Red mud is digested with diluted hydrochloric acid.
  • the vessel used for the digestion should be preferably made of teflon, but pyrex or teflon-lined steel can also be used. It is equipped with a valve at its bottom, which opens at certain intervals to allow removal of the soluble chlorides and consequently to accelerate the rate of reaction. It was found that the material to be digested required no prior drying, since it proved beneficiary to first add the required amount of water with a temperature range of 50 to 90 0 C, for at least 15 minutes and under vigorous stirring in order to evoke an initial hydrolysis, of the species involved and then, at room temperature, to add the required amount of the acid. Drinking water could also be used instead of distilled.
  • the combination of concentrated hydrochloric acid, water and red mud solid residue provides a resultant solid to liquid ratio lying within a range of 1:5 - 1.25 and a water to concentrated hydrochloric acid ratio lying within a range of 1:0.5 - 1:5.
  • the reaction vessel consisting mainly of CO 2
  • a concentrated Ca(OH) 2 solution in order insoluble CaCO 3 to be precipitated.
  • concentrated hydrochloric acid is added and the vessel is closed from its top.
  • the formed solution is slowly heated and after a reasonable time it reaches its azeotropic temperature (around 110 0 C).
  • the vessel is opened from its top and the solution is left to evaporate under constant composition for at least half an hour by continuous and vigorous stirring, until a slurry of the corresponding chloride salts is produced. About 15 minutes prior to this point heating ceases and the solution is left to cool down slowly to room temperature.
  • open digestion the vapors are left to escape from the mixture, are liquefied by a simple side condenser and finally are trapped into a suitable annex.
  • half of the collected vapors are added again to the slurry in order to form a new solution.
  • the combination of concentrated hydrochloric acid, water and red mud's digestion solid residue provides a resultant solid to liquid ratio lying within a range of 1 : 1 - 1 :25 and a water to concentrated hydrochloric acid ratio lying within a range of 1:0.5 - 1:5.
  • the solution is filtrated by gravity filtration, vacuum filtration or decantation.
  • the solid residue is washed with the remaining condensed vapors, then sequentially with warm (40 - 70 0 C) diluted (concentrated between 1 and 6M) hydrochloric acid, and cold (3 - 8 0 C) water.
  • the combination of concentrated hydrochloric acid, water and the enriched solid residue yields a resultant solid to liquid ratio lying within a range of 1:5 - 1:250 and a water to concentrated hydrochloric acid ratio lying within a range of 1 :0.01 - 1:5.
  • the remaining solid consists mainly of insoluble TiO 2 and SiO 2 and the washings are mixed with the above filtrate.
  • the analysis of the filtrate and the solution based on the initial red mud composition showed the following extraction yields:
  • variable red mud's composition as well as the relative inconvenience in maintaining the exact experimental conditions, mainly temperature, during the process, but this is of minor importance as will be explained hereafter.
  • the washings are separately kept for re-use, in which the required amount of NaOH is added to again prepare a solution of the corresponding concentration.
  • the latter will probably contain a small amount of Al +3 and Ca +2 ions.
  • the resultant solid is placed inside a desiscator, with calcium chloride, barium oxide or phosphorus pentoxide being the desiscants.
  • the filtrate is a solution containing the soluble chlorides of aluminum, calcium and sodium, as well as traces of iron. This is preferably evaporated to about 1/4 of its initial volume and then a saturated solution of NaOH is added at room temperature. Calcium hydroxide is precipitated, with the precipitation starting at a pH value of around 11 and completing at a pH value of almost 14. The precipitant is left in the mother liquor for at least 15 minutes and is separated by gravity filtration or another suitable technique.
  • the volume of the latter solution used is calculated based on the stoichiometric amount of sulfuric acid needed to simple replace sodium chloride and convert it to acidic sodium sulfate.
  • the solid mass is considered to be a unit consisting only of aluminum chloride. Since however the amount of sodium chloride is by no means negligible, an excess of a sulfuric acid solution is, in fact, used. During this process the liberated fuming hydrochloric acid is regained according to previously mentioned methods.
  • the resulting solution consists of Al +3 , Na + , SO 4 "2 along with traces of Cl " ions.
  • Ca(OH) 2 which was separated in the previous step is dissolved in a sufficient amount of water and then the resultant solution is slowly added to the above solution to precipitate sulfuric ligands in the form OfCaSO 4 . At this point a reasonable time of at least 30 minutes is needed for the supertarnant to be clarified completely. An additional amount of Ca(OH) 2 may be needed to completely entrap these ligands, which may be considered as an extra cost of the process proposed. But this can be minimized to a significant extent by optimizing the anion-replacement conditions, e.g. by slightly raising the temperature and, as much as possible, lowering the volume of concentrated sulfuric acid solution.
  • a small quantity (e.g. a few ml) of diluted Ba(NOs) 2 solution can also be used to result in insoluble BaSO 4 .
  • the supertarnant is a liquid consisting of Al +3 , Na + and OH " ions and therefore can be fed back to the Bayer method to increase the amount of soluble sodium aluminate and eventually the amount of pure aluminum metal.
  • the purity of calcium hydroxide precipitant is not of major industrial importance, since soluble chlorides are transformed into soluble sulfates.
  • the impurities (mainly iron) existing in the final solution will be removed again at the step of sodium hydroxide digestion of the new bauxite feed in the Bayer method as red mud enriched in iron content.
  • the solid residue (CaSO 4 ) together with the other insoluble compounds, such as SiO 2 can be a useful starting material for the cement industry, but this will be explained more thoroughly below.
  • the solid residue produced by red mud's digestion with hydrochloric acid is comprised mainly by SiO 2 and TiO 2 .
  • the major part of silicon dioxide can be removed from titanium dioxide by the addition of diluted hydrochloric acid (1-6 M) to the solids' mixture and centrifugation at low to moderate speeds.
  • diluted hydrochloric acid 1-6 M
  • the best way, however, is to stir the suspension by introducing compressed air into a vessel, which has an outlet at its side for the exit of the colloidal suspended matters and reflux the liquid from an outlet at the top via a mechanical pump. Free silicon dioxide lies at the bottom.
  • Silicon dioxide if combined with the previously precipitated calcium sulfate can yield a useful raw material for the cement industry.
  • the necessary composition i.e. CaO ⁇ 70%, SiO 2 ⁇ 20%, Al 2 O 3 ⁇ 5%, Fe 2 O 3 ⁇ 3%, can be achieved by existing red mud's components.
  • the remaining solid consists primarily of titanium dioxide with the main impurities being insoluble diasporic forms of aluminum. Traces of physisorpted iron and calcium compounds are also present, which can be removed by complexing compounds or chelating agents, which, in this case, must be regarded as an increase in the total process's cost. Taking into account the relative proportion of each oxide in the initial red mud's composition, it is obvious that the purity of titanium dioxide lies in the region of 70-80%, which makes it improper for pigment usage. In this form however, it could be a very useful starting material for the ilmenite industry.
  • the purity of titanium dioxide can be further improved in the following way: A solution of concentrated sulfuric acid is heated in a temperature range between 150 0 C and 250 0 C, into which the remaining solid is added. Grinding may be useful at this point. An excess of sulfuric acid is used, i.e. a solid to liquid ratio of at least 1:2. The solution is evaporated until a slurry of soluble sulfates is formed and the SO 3 vapors are recycled inside a vessel containing concentrated sulfuric acid, in such a way that the "oleum" acid produced at this point is accompanied by the generation of large amounts of heat. This fact can be exploited in certain stages of the entire procedure via heat exchangers.
  • Oleum acid can as well be used to achieve a faster and complete replacement of chloride by sulfuric anions.
  • the slurry is introduced hot enough (i.e. at a temperature of at least 95 0 C) into enough amount of water in order soluble TiOSO 4 to be hydrolysed.
  • the volume of water used must be such that in the final solution sulfuric acid in free form does not exceed 50% w/w.
  • a white precipitant of hydrated titanium dioxide is formed. Seeding may also be needed to produce anatase or rutile as desired.
  • the solid is separated by the mother liquor by filtration.
  • the evaporation step can be accelerated by placing a funnel of submicron porosity with an aqueous solution of Ca(OH) 2 , CaCl 2 , or Ba(NO 3 ) 2 at the top of the vessel. Furthermore, a small quantity of saturated CaCl 2 solution is added slowly to the solution to dissolve precipitated alkaline iron salts and trap sulfuric ligands from still soluble TiOSO 4 . Instead of CaCl 2 , one may use the corresponding quantities of aqueous Ca(OH) 2 and HCl.
  • ferrous iron salts are less susceptible to hydrolysis than ferric ones. Iron traces should then be removed out of the solution as coarse ferrous sulfate. If remaining traces of insoluble iron salts are still caged inside the crystal structure of titanium dioxide, a small quantity of diluted sodium or ammonium thiocyanate solution (of about 0.1 M concentration) can be used to remove them in the form of [Fe(SCN) n ] 3" ".
  • the solid residue consists of TiO 2 .xH 2 O and probably a small amount of CaSO 4 . If sodium or ammonium thiocyanate salts have been physisorpted to the filtrate, they must be removed with the aid of a small amount of amylic alcohol.
  • the spent reagent sodium or ammonium thiocynate solution
  • the spent reagent can be recovered through the addition of sodium hydroxide or ammonia solution, respectively, and the removal of the precipitated hydroxy iron (III) sulphate by filtration.
  • Titanium dioxide can be further purified by washing the solid residue with a hot (i.e. having a temperature of at least 45 0 C) solution of concentrated ammonium sulfate and again filtration or decantation.
  • Ammonium sulfate and calcium sulfate can be also recovered by acidifying the solution with sulfuric acid.
  • Anhydrous titanium dioxide is produced by calcination at high temperatures (800-900 0 C). It should be noted that the afore-mentioned separation of silicon dioxide can well be employed at this stage as well, if it has not already been separated.
  • the resulting filtrate consists mainly of Al +3 and SO 4 - 2 ions. Final traces of iron, if any, must be eliminated before continuing. For this purpose, a few drops of hydrogen peroxide and then an ammonia solution 25 % v/v are subsequently added to precipitate hydroxy iron (III) sulfate, which is removed by filtration. Similarly to the above, seeding may be needed, if iron ions' concentration is of the order of a few ppm. To the filtrate an excess of the same ammonia solution is added. After cooling down to room temperature, it is again heated for at least 30 min at 60-120 0 C.
  • crystals of hydrated ammonium aluminum sulfate are formed. This process is accelerated by providing seeding crystals and cooling at room temperature or below it, preferably between 3 and 8 0 C. The crystals are removed from the solution by filtration and are washed with a water/alcohol solution.
  • Hydroxy iron (III) chloride is the starting material for ferrite production. Prior to use this is dried inside a desiscator with barium oxide, calcium chloride or phosphorus pentoxide being the desiscants. It must be noted that the drying step can be passed over in industrial scale if the solid's humidity proportion is precisely calculated, since this is to be again diluted at the steps that follow.
  • the same NaOH solution after the addition of a small amount of NaOH pellets, can be used for new mixture feeds.
  • the formed salts (mainly NaHSO 4 and NaCl) eventually will reach their solubility limit into the alkaline solution and must be removed by filtration.
  • magnétique fluids or ferrofluids
  • a liquid medium such as oleum acid
  • gaseous SO 2 can be bubbled through the alkaline solution at room temperature.
  • Sulfur dioxide is very soluble into aqueous solutions and by its reaction with diluted oxygen sulfar trioxide can be formed accompanied with liberation of heat.
  • This indirect heating prevents atmospheric oxygen to be again diluted into the alkaline solution.
  • sulfur trioxide formation a small quantity of soluble NaHSO 4 may be formed, which renders no inconvenience to ferrite precipitation.
  • Another approach of producing ferrites by coprecipitation is crystallizing hydrated ferrous sulfate, known as "copperas" out of the sulfates' solution, but this process is slow under normal experimental conditions.
  • ferrous sulfate solutions resist strongly to oxidation, which is not the case if ferrous sulfate is in solid form. This is why it is best for ferrite production the ferrous sulfate solution to be recently prepared.
  • double salts such as the "Mohr salt” can be used.
  • Mohr's salt can be prepared by mixing equimolar quantities of ferrous sulfate and ammonium sulfate by applying moderate heating. Upon cooling to room temperature crystallization of FeSO 4 ' (NHt) 2 SO 4 occurs.
  • the purity of the solid samples produced (silicon dioxide, titanium dioxide, calcium sulfate and magnetic ferrite) was determined by melting point analysis. In all cases a high degree of purity was confirmed. Especially in the case of ferrites, it was found that the sum of the amounts of calcium oxide, sodium oxide, potassium oxide and silicon dioxide present was less than 1%, denoting that red mud's hematite can well be used as a potential ferrites' precursor material.
  • the radioactivity of ten samples, corresponding to certain stages of the procedure, was also measured by a Certified Third Body. The results were obtained by ⁇ -spectroscopy. An ultra- pure germanium detector was utilized and the duration of each sample's measurement was more than 8 hours. No artificial radioactive nuclides were detected.
  • the following figure 2 presents the maximum levels of Ra, U, Th and K, calculated by the Curie method. The low radioactivity levels in every case indicate the proposed method's industrial feasibility.
  • Solid material of red mud was received by the company "Aluminum of Greece". This was ground under the size of 100 ⁇ m into a suitable mill to increase surface reaction area.
  • An initial quantity of 100 g of red mud was at first heated at 75 0 C with 540 ml of distilled water for 30 min in an open pyrex vessel. Then it was allowed to cool down slowly to room temperature. Then 860 ml of 37% fuming hydrochloric acid were added and the vessel was closed from its top. From the above values one can estimate the solid to liquid ratio (1:14). Other ratios also gave satisfactory results, but the one proposed is, in fact, a compromise between significant yields and economic procedure. The solution was slowly heated and within about 30 min had reached its azeotropic temperature.
  • the vessel was opened from its top and the solution was left to evaporate under constant composition for about 3 hours by supplying a moderate heating power and with continuous and vigorous stirring, until a slurry of the corresponding chloride salts was produced. About 15 minutes prior to this point heating ceased and the solution was left to cool down slowly to room temperature. During open digestion the vapors were left to escape from the mixture, were liquefied by a simple side condenser and finally were trapped into a suitable annex. When the digestion had ended, half of the collected vapors were added again to the slurry in order to form a new solution. After about 30 minutes the solution was filtrated by gravity filtration.
  • EXAMPLE 2 Dried hydroxy iron (III) chloride was used as the starting material for magnetite production. Drying was complete after about 12 hours, but this time was considerably shortened, i.e. to about 2 hours, by applying a low vacuum (30 mm Hg was adequate) via a water pump and at a temperature of about 90 0 C inside a properly modified Abderhalden-like drying apparatus. Then 70 g of solid Fe(OH)Cl 2 was weighted and split into three equiponderant parts. The
  • the undissolved portion of metallic iron was separated in the presence of a magnet and the supertarnant was added to the former chlorides' solution.
  • the mixture was then added dropwise at 90 0 C to 2.5 L of a NaOH solution concentrated between 1.6 and 2.2 M, preferably around 2.0 M to precipitate magnetite particles.
  • the pH value at this point should lie between 11 and 12, preferably around 11.85.
  • These particles were removed by the mother liquor in the presence of a magnet and subsequent decantation and were washed with 250 ml of diluted hydrochloric acid concentrated around 0.01 M.
  • the mother liquor after the addition of a small amount of NaOH pellets, could be re-used in new feeds of mixtures comprised by soluble chlorides and soluble sulfates.

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  • Chemical & Material Sciences (AREA)
  • Organic Chemistry (AREA)
  • Inorganic Chemistry (AREA)
  • Life Sciences & Earth Sciences (AREA)
  • Geology (AREA)
  • General Life Sciences & Earth Sciences (AREA)
  • Geochemistry & Mineralogy (AREA)
  • Environmental & Geological Engineering (AREA)
  • Analytical Chemistry (AREA)
  • Compounds Of Iron (AREA)
  • Compounds Of Alkaline-Earth Elements, Aluminum Or Rare-Earth Metals (AREA)
  • Inorganic Compounds Of Heavy Metals (AREA)

Abstract

La présente invention porte sur la récupération totale d'oxydes purs des éléments présents dans de la boue rouge, ainsi que sur leur transformation partielle en produits de haute valeur ajoutée. La boue rouge contient des oxydes de valeur, tels que des oxydes de titane ou d'aluminium, en proportions élevées, ainsi que de l'oxyde de fer, qui peut être utilisé efficacement comme matière de départ pour la production de ferrites. La méthodologie et les voies chimiques sont présentées ici en ce qui concerne leur faisabilité industrielle. Plus précisément, le procédé proposé produit des produits ultra-purs de dioxyde de silicium, de sulfate de calcium (tous deux appropriés pour l'industrie du ciment), de dioxyde de titane (destiné à être utilisé comme pigment), d'aluns (destinés à être utilisés dans des produits pharmaceutiques) et enfin de ferrites, c'est-à-dire de magnétite (pour des applications électriques et électroniques). De plus, le produit final du procédé est une solution ne contenant que des cations du sodium et de l'aluminium, appropriée pour être recyclée dans le procédé Bayer. Les principaux réactifs utilisés, à savoir l'acide chlorhydrique, l'acide sulfurique, l'hydroxyde de sodium ou l'ammoniac, peuvent être presque totalement recyclés. À cette fin, des installations simples de distillation sont nécessaires. Le recyclage est également possible pour des réactifs plus compliqués ou des agents chélatants, alors que des produits intermédiaires pendant le procédé sont utilisés comme précurseurs pour les étapes qui suivent. De l'énergie est produite à certaines étapes, ce qui élimine ainsi la consommation d'énergie d'une installation industrielle. Enfin, à l'achèvement de ce procédé, il n'existera pas de restes de boue rouge.
PCT/GR2010/000003 2009-01-12 2010-01-12 Produits de valeur obtenus à partir de boue rouge WO2010079369A1 (fr)

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Cited By (32)

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WO2012001700A1 (fr) * 2010-06-30 2012-01-05 Keki Hormusji Gharda Procédé d'extraction de métaux contenus dans des résidus et des minerais alumino-ferreux et titano-ferreux
CN102432074A (zh) * 2011-08-30 2012-05-02 刘明诗 一种拜耳法、拜耳烧结法氧化铝赤泥零污染、零残留处理方法
CN102491346A (zh) * 2011-12-02 2012-06-13 太原理工大学 一种用氧化铝赤泥制备白炭黑的方法
WO2012100004A1 (fr) * 2011-01-18 2012-07-26 Mohsen Amiran Procédés de récupération d'un résidu de magnétite et de bauxite
CN102745733A (zh) * 2012-07-18 2012-10-24 潘爱芳 一种从烧结法赤泥中分离有用组分的方法
CN102757078A (zh) * 2012-07-18 2012-10-31 潘爱芳 一种从拜耳法赤泥中分离有用组分的方法
WO2013104059A1 (fr) * 2012-01-10 2013-07-18 Orbite Aluminae Inc. Procédés de traitement de boue rouge
WO2013125828A1 (fr) * 2012-02-24 2013-08-29 에스케이이노베이션 주식회사 Procédé de préparation de boue rouge modifiée, à l'aide de chlorure et d'acide phosphorique
US8597600B2 (en) 2007-05-21 2013-12-03 Orbite Aluminae Inc. Processes for extracting aluminum from aluminous ores
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CN114655972A (zh) * 2022-04-27 2022-06-24 云南省生态环境科学研究院 拜耳法氧化铝溶液有机物高效脱除的方法
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