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WO2002010068A1 - Production d'oxydes metalliques - Google Patents

Production d'oxydes metalliques Download PDF

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Publication number
WO2002010068A1
WO2002010068A1 PCT/GB2001/003370 GB0103370W WO0210068A1 WO 2002010068 A1 WO2002010068 A1 WO 2002010068A1 GB 0103370 W GB0103370 W GB 0103370W WO 0210068 A1 WO0210068 A1 WO 0210068A1
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WO
WIPO (PCT)
Prior art keywords
process according
oxide
carbonate
metal oxide
red mud
Prior art date
Application number
PCT/GB2001/003370
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English (en)
Inventor
Animesh Jha
Malpan Pailo Antony
Vilas D. Thathavadkar
Original Assignee
University Of Leeds
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Publication date
Application filed by University Of Leeds filed Critical University Of Leeds
Priority to AU2001276466A priority Critical patent/AU2001276466A1/en
Publication of WO2002010068A1 publication Critical patent/WO2002010068A1/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
    • C22B1/00—Preliminary treatment of ores or scrap
    • C22B1/02—Roasting processes
    • 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
    • C01F7/08—Preparation of alkali metal aluminates; Aluminium oxide or hydroxide therefrom by treating aluminous minerals with sodium carbonate, e.g. sinter processes
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01G—COMPOUNDS CONTAINING METALS NOT COVERED BY SUBCLASSES C01D OR C01F
    • C01G1/00—Methods of preparing compounds of metals not covered by subclasses C01B, C01C, C01D, or C01F, in general
    • C01G1/02—Oxides
    • 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
    • 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
    • C22B34/1204—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 preliminary treatment of ores or scrap to eliminate non- titanium constituents, e.g. iron, without attacking the titanium constituent
    • C22B34/1209—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 preliminary treatment of ores or scrap to eliminate non- titanium constituents, e.g. iron, without attacking the titanium constituent by dry processes, e.g. with selective chlorination of iron or with formation of a titanium bearing slag
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
    • C01P2002/00—Crystal-structural characteristics
    • C01P2002/70—Crystal-structural characteristics defined by measured X-ray, neutron or electron diffraction data
    • C01P2002/72—Crystal-structural characteristics defined by measured X-ray, neutron or electron diffraction data by d-values or two theta-values, e.g. as X-ray diagram
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
    • C01P2002/00—Crystal-structural characteristics
    • C01P2002/80—Crystal-structural characteristics defined by measured data other than those specified in group C01P2002/70
    • C01P2002/85—Crystal-structural characteristics defined by measured data other than those specified in group C01P2002/70 by XPS, EDX or EDAX data
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
    • C01P2004/00—Particle morphology
    • C01P2004/01—Particle morphology depicted by an image
    • C01P2004/03—Particle morphology depicted by an image obtained by SEM
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
    • C01P2004/00—Particle morphology
    • C01P2004/51—Particles with a specific particle size distribution

Definitions

  • the present invention relates to a process for the production of metal oxides.
  • the process relates to the production of iron, aluminium and titanium from aluminous minerals such as bauxite, alumina-rich clays and the solid waste generated from the Bayer's process called, the red mud.
  • the process further involves roasting of the above mentioned materials with alkali, eg sodium or potassium carbonate or sodium or potassium hydroxide, mixed with the carbonates, in air and subsequent leaching by water and sulphuric acid.
  • alkali eg sodium or potassium carbonate or sodium or potassium hydroxide
  • Aluminium is the most abundant metallic element in the earth's crust. It is normally found combined with other elements, and does not occur in the pure state. It appears in a wide variety of minerals combined with oxygen, silicon, the alkali and alkaline- earth metals and as hydroxides, sulphates and phosphates.
  • the bauxite is a sedimentary rock that contains economically recoverable quantities of the aluminium oxide minerals Gibbsite, Bohmite, and Diaspore.
  • iron is present as Goethite, ⁇ -FeO(OH) and hematite, ⁇ -Fe 2 O 3 ; titanium is present in bauxite as Anatase TiO 2 ; and Silicon dioxide may occur either as quartz, or as complex silicates.
  • Bayer's process is widely used for the production of pure Al 2 O 3 from bauxite.
  • bauxite is dissolved in an NaOH solution at 400 - 500K to produce Sodium aluminate which is (NaAlO 2 ).
  • the (NaAlO 2 ) formed is soluble in water and filtered out.
  • Aluminium hydroxide (Al(OH) 3 ) is then precipitated from the solution and the.
  • Al(OH) 3 is calcined at 1350 to 1400K to produce pure alumina (Al 2 O 3 ) [1] .
  • the unreacted constituents of bauxite are the oxides of iron, titanium and a fraction of unreacted alumina. These oxides form the residue from the process and it is called the red mud. A complete recovery of alumina is economically not possible via the Bayer process.
  • the Bayer process begins with the preparations of bauxite by grinding to produce a uniform composition.
  • the bauxite is ground while suspended in a portion of the Bayer process alkali solution. This slurry is then mixed with the remaining NaOH solution at 400K. The mixture, with hot NaOH solution is then treated in a digester vessel at well above atmospheric pressure.
  • the main reaction in the digester is given by equation 2:
  • the filtered solution containing sodium aluminate is cooled from 400 K down to 335 - 345K temperature range.
  • the concentration at this temperature is such that the solution is saturated with Al(OH) 3 , but is not supersaturated to cause spontaneous crystallisation.
  • a seed of aluminium hydroxide is added at this point to precipitate Al(OH) 3 from the sodium aluminate mother liquor.
  • the aluminium hydroxide precipitate is calcined in the temperature range of 1350 to 1400K for the production of pure Al 2 O 3 via the decomposition of aluminium hydroxide, shown in reaction 1.
  • one disadvantage of the Bayer process is that Al 2 O 3 is not completely removed from the bauxite ore. A fraction of alumina always remains in the solid filter residue, this is known as "the red mud".
  • the other major constituents of bauxite e.g. iron and titanium, remain as complex oxides in the red mud.
  • the red mud also has a high Al 2 O 3 content.
  • the average chemical composition of the constituents of red mud is:-
  • Al 2 O 3 (23 -30 wt%), SiO 2 (8 t%), Fe 2 O 3 (35-50 wt%), and TiO 2 (15-18 wt%).
  • a micrograph of red mud sample is shown in figure 1. It mainly consists of three phases as marked A, B, and C in the micrograph. Phase A is rich in aluminium, whereas phrase B and phase C are rich in iron and titanium respectively. Electron Diffraction X-Ray (EDX) analysis of the three phases can be seen in figures 2 to 4. An X-ray diffraction pattern of dry red mud is shown in figure 5. Therefore, from the X-ray diffraction and EDX analysis, it is apparent that alumina, silica, iron oxide, and titanium dioxide are present in complex mineralogical forms in red mud.
  • EDX Electron Diffraction X-Ray
  • the object of the present invention is to provide a process, which enables the recovery of, particularly, unreacted Al 2 O 3 , and TiO from bauxite and/or from the process residue, red mud.
  • the process offered by the present invention advantageous because, tnter alia, it provides an opportunity for the recovery of minerals from red mud, but also it has been found that the above oxides and hydroxides could be extracted more efficiently, not only from bauxite, but also from alumina-rich clays and/or red mud via the process of the invention.
  • the present invention provides an alternative and more environmentally acceptable process for the extraction of aluminium oxide and oxides of iron and titanium from, red mud, bauxite and/or alumina-rich clays.
  • step (ii) extracting the desired metal salt produced in step (i); (iii) precipitation of a hydroxide salt;
  • the process comprises the steps of;
  • step (i) roasting a mineral ore (bauxite/clay) and alumina-containing residues in the presence of an alkali and/or alkali mixture; (ii) extracting the desired metal salt produced in step (i) using an aqueous and/or a dilute ammoniacal solution in aqueous media to separate water-soluble alkali aluminate from undigested metal oxide filter residue;
  • step (iv) calcining aluminium hydroxide formed in step (iii).
  • the actual temperature used in step (i) of the process of the invention may vary, depending, r ⁇ ter alia, upon the nature of the mineral ore, the nature of the metal oxide to be isolated, etc.
  • the temperature used in step (i) of the process of the invention is greater than 400K, preferably greater than 500K, more preferably between 600 and 1300K, especially between 700 to 1200K, e.g. at 1150K.
  • 1150K is the optimum temperature for the isolation of aluminium, although variations on this temperature, within the ranges identified herein, will also produce satisfactory results.
  • the process of the invention is suitable for use in purification of mineral ores, e.g. bauxite.
  • the process is also suitable for the purification of waste materials, such as red mud.
  • waste materials such as red mud.
  • the phrase "mineral ore" when used in the definition of the invention herein should be construed as including alumina-rich clays, waste materials from other processes and in particular red mud produced from the Bayer process.
  • the alkali used in step(i) of the process of the invention is preferentially a carbonate which may comprise any conventionally known carbonate or a mixture of carbonates.
  • Especially preferred carbonates are the carbonates of the Group la and Group Ila metals, i.e. the alkali or alkaline earth metals.
  • Such metal salts therefore include, for example, lithium, sodium, potassium, magnesium and/or calcium carbonates.
  • Carbonates of the alkali metals are most preferred, for example sodium or potassium carbonate. Most preferentially sodium carbonate is used.
  • a mixture of a hydroxide, eg sodium or potassium hydroxide, and a carbonate may be used.
  • the extraction process of step (ii) may use a variety of solvents or mixtures of solvents.
  • the solvent may be varied depending upon the nature of metal salt being isolated. However, preferentially, the solvent will be one which can readily be disposed of with minimal damage to the environment. Thus, the most preferred solvent is water, usually hot water above 25°C.
  • a dilute solution of ammonium salts in water is recommended for enhancing the extraction of alkali aluminate.
  • the treatment of calcined minerals with water or with dilute ammonical solution enhances the efficiency of alkali aluminate extraction from the roasted minerals.
  • the precipitation of aluminium hydroxide, Al(OH) 3 from alkali aluminate solution is initiated by passing CO 2 or oxalic acid solution.
  • the precipitated aluminium hydroxide is dried and calcined at 1400K for producing alumina powder as it is done in the Bayer process.
  • any conventionally known acids may be used, including organic and inorganic acids. Alternatively mixtures of acids may be used. Inorganic acids are preferred and such acids may be selected from, but are not limited to, hydrofluoric acid, hydrochloric acid, nitric acid, sulphuric acid and an acidic oxide or mixtures thereof. When the metal ore being isolated is aluminium, then an acidic oxide is preferred. The most preferred acidic oxide is carbon dioxide.
  • the conversion of the hydroxide salt to the oxide end product may comprise any conventionally known oxidation step, such steps may include thermal decomposition, calcining, etc.
  • the metal oxide is alumina, then the oxidation step preferentially comprises calcining.
  • the material flow sheet is similar to the Bayer process, except the NaAlO 2 formation is carried out at an elevated temperature above 1050 K in the absence of water and in the presence of sodium carbonate.
  • bauxite ore or red mud is homogeneously mixed with the stoichiometric amount of sodium carbonate required to convert alumina to sodium aluminate.
  • the mixture is roasted above 105 OK in air.
  • the reactions which take place above 1050K are:
  • the roasted mass contains water soluble sodium aluminate and other insoluble components of ore.
  • the roast product is extracted with hot water so that all of the sodium aluminate phase dissolves in water.
  • the filtrate consists of the water-soluble sodium aluminate, whereas the hydroxides of iron, titanium oxide and other impurities remain present in the solid residue, which is part of the unreacted bauxite.
  • a micrograph of the solid residue calcined at 1400K is shown in figure 6.
  • EDX analysis of the two phases as marked B and C is given in figures 7 and 8.
  • the phase B is rich in iron
  • the phase C is comparatively richer in titanium.
  • aluminium oxide is not detected in the EDX analysis, as its concentration appears to be well below 5 wt%.
  • Alumina is completely extracted from the red mud as sodium aluminate, which is converted to Al(OH) 3 via the acidification with carbon dioxide gas.
  • Al(OH) 3 precipitate is then filtered and calcined at 1350-1400K to produce pure Al O 3 .
  • the micrographs and X-ray powder diffraction of the alumina extracted from the red mud and bauxite are shown in figures 9a and 9b respectively.
  • the phases identified in the powder diffraction pattern show the evidence for the dominant ⁇ and ⁇ types of alumina.
  • the grains are well defined and clean.
  • Figures 10a and 10b the particle size distribution of dried and calcined aluminium hydroxide and alumina are shown respectively.
  • the alumina particle size distribution shown in Figure 10b is bimodal, which can be altered by varying the time and temperature of calcination.
  • the filtrate containing Na 2 CO 3 is evaporated to regenerate sodium carbonate.
  • Production of soda is one of the main advantages of this new process.
  • the residue containing iron and titanium is mixed with 98% H 2 SO 4 so as to make a slurry.
  • the ratio of H 2 SO 4 to residue is chosen such that the weight ratio of H 2 SO 4 to TiO 2 in the suspension produced by the hydrolysis is between 2-2.5.
  • the slurry obtained by digestion is dissolved in cold water or in dilute aqueous sulphuric acid (H 2 SO 4 ). Undissolved solid material containing silicates is removed completely by filtration. Titanium oxide hydrate is precipitated from the filtered solution by hydrolysis at 375 -390K.
  • the hydrate is filtered off from the solution and washed with water or dilute acids to remove dissolved sulphates of other metallic impurities adhered on to the precipitate surface. Finally the hydrate is calcined in the temperature range of 1050 to 1300K to produce pure titanium oxide, which can be used for manufacturing pigments.
  • the solution containing iron salts are concentrated and then thermally decomposed to form iron oxide and sulphur dioxide.
  • the filtrate can also be evaporated to obtain FeSO 4 , which can be used for water purification.
  • the metal oxide produced may be selected from an aluminium oxide, an iron oxide and a titanium oxide.
  • the metal oxide produced is selected from Al 2 O 3 , Fe 2 O 3 and TiO 2 ; most preferably the metal oxide produced is Al 2 O 3 .
  • the process of the present invention is advantageous, inter alia, because alumina present in bauxite and red mud was extracted with 98 % efficiency via the alkali- roasting process by forming sodium or potassium aluminate above 400K. Furthermore, TiO 2 was recovered from the residue obtained after extracting aluminium by dissolving the residue in concentrated sulphuric acid and by subsequent hydrolysis and calcination. In addition, Fe 2 O 3 was recovered by precipitating Fe(OH) 3 from the filtrate by the addition of an alkali or thermal decomposition of the filtrate. The filtrate residue derived from potassium carbonate/potash roasting of alumina containing minerals yield residues rich in K ions. Potassium ion containing residue can advantageously be used as a soil conditioner and for making fertiliser by mixing with phosphate residue, phospho-gypsum, and/or Basic Oxygen Furnace slag from steel making plant.
  • the new process of the invention has been developed for extracting alumina, iron oxide (Fe 2 O 3 ) and/or titanium oxide (TiO 2 ) from bauxite and red mud.
  • the process involves roasting of bauxite and/ or red mud with sodium carbonate (Na 2 CO 3 ) in air. The roasted mass is digested in water and filtered. The filtrate contains sodium aluminate. Al(OH) is precipitated by passing carbon dioxide (CO ) through the filtrate. Pure alumina is produced by calcining the Al(OH) 3 precipitate. Residue is digested in concentrated sulphuric acid (H 2 SO ) and diluted with water.
  • H 2 SO concentrated sulphuric acid
  • Titanium oxide hydrate is precipitated via the hydrolysis of the acid solution at 375-390K. Iron oxide is recovered from the filtrate by evaporation and thermal decomposition. The CO 2 generated from the decomposition of sodium carbonate can be recycled during the precipitation of Al(OH) 3 from the NaAlO 2 solution to reform Na 2 CO . The recovery of other oxides, TiO 2 and Fe 2 O will yield a zero waste process for the manufacture of alumina.
  • Figure 2 is an EDX analysis of an alumina-rich phase
  • Figure 3 is an EDX analysis of an iron rich phase
  • Figure 4 is an EDX analysis of a titanium rich phase
  • Figure 5 is an X-ray diffraction pattern of dry red mud
  • Figure 6 is a micrograph of red mud after alumina extraction
  • Figure 7 is an EDX analysis of the iron rich phase after extracting aluminia from red mud
  • Figure 8 is an EDX analysis of the titanium rich phase after extracting alumina
  • Figure 9a is a micrograph of alumina extracted from red mud
  • Figure 9b is an X-ray diffraction pattern of alumina extracted from red mud
  • Figure 10a is a particle size distribution of Al(OH) 3 after drying
  • Figure 10b is a particle size distribution of alumina after calcining at 1400K
  • Figure 11 is a schematic representation of a process of the invention.
  • the extraction efficiency is defined by ⁇ in percentage, which is dependent on the concentration of aluminium in the ore and in the residue.
  • Bauxite ore from Ghana (approximate composition: 55% of Al 2 O 3 , 12 % of Fe 2 O , 2% of TiO 2 , 2 % of SiO 2 , and moisture) was homogeneously mixed with sodium carbonate in the ratio 1 : 0.60 .
  • the mixture was heated at 1150°C for 2 hours in an electrically heated furnace in air.
  • reaction product was digested in hot water and filtered.
  • the filtrate was acidified with carbon dioxide to convert water-soluble sodium aluminate to Al(OH) 3 precipitate.
  • the residue containing iron oxide (Fe O 3 ) and titanium dioxide (TiO 2 ) was mixed with 98% H 2 SO 4 for making a slurry.
  • the ratio of H 2 SO 4 to residue was chosen in such a way that the weight ratio of H 2 SO 4 to TiO 2 in the suspension produced by the hydrolysis was maintained between 2 to 2.5.
  • Titanium oxide hydrate was precipitated from the filtered solution by hydrolysis in the temperature range 375 to 390K.
  • the titanium oxide hydrate was filtered off from the solution and calcined in the temperature range of 1050 to 1300K to produce pure titanium oxide.
  • the filtrate was treated with NaOH to precipitate Fe as Fe(OH) .
  • the precipitate was filtered out and calcined to produce Fe 2 O .
  • Red mud from ALCAN (approximate composition: 46 % Fe 2 O 3 , 22 % of Al 2 O 3 , 8% of TiO2, 8 % of SiO 2 , 3-4 MgO and CaO and loss on ignition was 10-12 wt%) was homogeneously mixed with sodium carbonate in the ratio 1: 0.25.
  • the experiments were carried out as described in the above examples by steps 2 to 12.
  • the extraction efficiency for alumina was over 98 %.
  • the extraction efficiency of alumina from bauxite and red mud does not change when soda is replaced by potassium carbonate or potash.
  • the red mud obtained in this case contains alkali in the form of potassium ions and does not have harmful effect of soda in red mud, which cannot be used as a fertiliser or soil conditioner.
  • alkali roasting of red mud and bauxite for the extraction of alumina, titania, and iron oxides as by-product.

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

Abstract

L'invention concerne un procédé de purification d'oxydes métalliques consistant à (i) griller un minerai en présence d'un alcali, (ii) extraire le sel métallique désiré produit au cours de l'étape (i), (iii) précipiter un sel hydroxyde et (iv) convertir ce sel hydroxyde en un oxyde approprié. Ledit procédé convient à la récupération d'alumine, de titane et d'oxyde ferrique à partir de bauxite et/ou de boues rouges.
PCT/GB2001/003370 2000-07-29 2001-07-30 Production d'oxydes metalliques WO2002010068A1 (fr)

Priority Applications (1)

Application Number Priority Date Filing Date Title
AU2001276466A AU2001276466A1 (en) 2000-07-29 2001-07-30 Production of metal oxides

Applications Claiming Priority (2)

Application Number Priority Date Filing Date Title
GBGB0018592.6A GB0018592D0 (en) 2000-07-29 2000-07-29 Production of oxides of iron aluminium and titanium from bauxite and red mud
GB0018592.6 2000-07-29

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WO2002010068A1 true WO2002010068A1 (fr) 2002-02-07

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Cited By (9)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
WO2004113230A1 (fr) * 2003-06-16 2004-12-29 The University Of Leeds Procede d'extraction d'oxydes metalliques reactifs
WO2005028369A1 (fr) * 2003-09-18 2005-03-31 The University Of Leeds Procede pour recuperer du dioxyde de titane a partir de compositions contenant de l'oxyde de titane
US7494631B2 (en) * 2007-03-26 2009-02-24 Millennium Inorganic Chemicals Titaniferous ore beneficiation
US7771679B2 (en) 2003-09-18 2010-08-10 The University Of Leeds Process for the recovery of titanium dioxide from titanium-containing compositions
WO2011137481A1 (fr) * 2010-05-03 2011-11-10 Bhp Billiton Worsley Alumina Pty Ltd Procédé pour la récupération d'alumine à l'aide d'aluminate tricalcique
CN103614547A (zh) * 2013-11-28 2014-03-05 中南大学 一种从一水硬铝石型铝土矿中分离铁铝硅的方法
WO2015058239A1 (fr) * 2013-10-21 2015-04-30 Peloton Resources Pty Ltd Obtention de produits de grande valeur à partir d'une boue rouge résiduaire
CN105776265A (zh) * 2016-02-06 2016-07-20 杭州锦江集团有限公司 一种基于球团法利用低品位铝土矿生产氧化铝的方法
CN110408773A (zh) * 2019-08-13 2019-11-05 昆明理工大学 一种利用钠盐强化高铝褐铁矿铝铁分离效果的方法

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Publication number Priority date Publication date Assignee Title
GB601968A (en) * 1944-12-08 1948-05-18 Monolith Portland Midwest Comp Improvements in the extraction of alumina from its ores
GB848230A (en) * 1956-08-27 1960-09-14 Blancs De Zinc De La Mediterra A process of separately recovering aluminium, iron and titanium values from material such as "red mud" containing said values
US4119698A (en) * 1976-11-26 1978-10-10 Kernforschungsanlage Julich, Gesellschaft Mit Beschrankter Haftung Reclamation treatment of red mud
US4254088A (en) * 1979-03-27 1981-03-03 The United States Of America As Represented By The United States Department Of Energy Salt-soda sinter process for recovering aluminum from fly ash
US4265864A (en) * 1978-02-13 1981-05-05 Mizusawa Kagaku Kogyo Kabushiki Kaisha Process for treating bauxite or similar raw material

Patent Citations (5)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
GB601968A (en) * 1944-12-08 1948-05-18 Monolith Portland Midwest Comp Improvements in the extraction of alumina from its ores
GB848230A (en) * 1956-08-27 1960-09-14 Blancs De Zinc De La Mediterra A process of separately recovering aluminium, iron and titanium values from material such as "red mud" containing said values
US4119698A (en) * 1976-11-26 1978-10-10 Kernforschungsanlage Julich, Gesellschaft Mit Beschrankter Haftung Reclamation treatment of red mud
US4265864A (en) * 1978-02-13 1981-05-05 Mizusawa Kagaku Kogyo Kabushiki Kaisha Process for treating bauxite or similar raw material
US4254088A (en) * 1979-03-27 1981-03-03 The United States Of America As Represented By The United States Department Of Energy Salt-soda sinter process for recovering aluminum from fly ash

Cited By (16)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
JP2012121798A (ja) * 2003-06-16 2012-06-28 Univ Of Leeds 反応性金属酸化物の抽出方法
JP2006527698A (ja) * 2003-06-16 2006-12-07 ザ ユニヴァーシティ オヴ リーズ 反応性金属酸化物の抽出方法
WO2004113230A1 (fr) * 2003-06-16 2004-12-29 The University Of Leeds Procede d'extraction d'oxydes metalliques reactifs
AU2004249473B2 (en) * 2003-06-16 2010-08-19 The University Of Leeds Extraction process for reactive metal oxides
US8834600B2 (en) 2003-06-16 2014-09-16 The University Of Leeds Extraction process for reactive metal oxides
WO2005028369A1 (fr) * 2003-09-18 2005-03-31 The University Of Leeds Procede pour recuperer du dioxyde de titane a partir de compositions contenant de l'oxyde de titane
JP2007505812A (ja) * 2003-09-18 2007-03-15 ザ・ユニバーシテイ・オブ・リーズ チタン含有組成物から二酸化チタンを回収するための方法
US7771679B2 (en) 2003-09-18 2010-08-10 The University Of Leeds Process for the recovery of titanium dioxide from titanium-containing compositions
US7494631B2 (en) * 2007-03-26 2009-02-24 Millennium Inorganic Chemicals Titaniferous ore beneficiation
AU2011250647B2 (en) * 2010-05-03 2013-11-07 South32 Worsley Alumina Pty Ltd Process for recovery of alumina using tricalcium aluminate
WO2011137481A1 (fr) * 2010-05-03 2011-11-10 Bhp Billiton Worsley Alumina Pty Ltd Procédé pour la récupération d'alumine à l'aide d'aluminate tricalcique
WO2015058239A1 (fr) * 2013-10-21 2015-04-30 Peloton Resources Pty Ltd Obtention de produits de grande valeur à partir d'une boue rouge résiduaire
US10273561B2 (en) 2013-10-21 2019-04-30 Peloton Resources Pty Ltd Deriving high value products from waste red mud
CN103614547A (zh) * 2013-11-28 2014-03-05 中南大学 一种从一水硬铝石型铝土矿中分离铁铝硅的方法
CN105776265A (zh) * 2016-02-06 2016-07-20 杭州锦江集团有限公司 一种基于球团法利用低品位铝土矿生产氧化铝的方法
CN110408773A (zh) * 2019-08-13 2019-11-05 昆明理工大学 一种利用钠盐强化高铝褐铁矿铝铁分离效果的方法

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