[go: up one dir, main page]

US20130195738A1 - Process for the recovery of titanium dioxide and value metals and system for same - Google Patents

Process for the recovery of titanium dioxide and value metals and system for same Download PDF

Info

Publication number
US20130195738A1
US20130195738A1 US13/567,013 US201213567013A US2013195738A1 US 20130195738 A1 US20130195738 A1 US 20130195738A1 US 201213567013 A US201213567013 A US 201213567013A US 2013195738 A1 US2013195738 A1 US 2013195738A1
Authority
US
United States
Prior art keywords
titanium dioxide
solution
hydrochloric acid
leach solution
hcl
Prior art date
Legal status (The legal status 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 status listed.)
Abandoned
Application number
US13/567,013
Other languages
English (en)
Inventor
Bryn Harris
Carl White
Current Assignee (The listed assignees may be inaccurate. Google has not performed a legal analysis and makes no representation or warranty as to the accuracy of the list.)
Neomet Technologies Inc
Original Assignee
Neomet Technologies Inc
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 Neomet Technologies Inc filed Critical Neomet Technologies Inc
Priority to US13/567,013 priority Critical patent/US20130195738A1/en
Assigned to NEOMET TECHNOLOGIES INC. reassignment NEOMET TECHNOLOGIES INC. ASSIGNMENT OF ASSIGNORS INTEREST (SEE DOCUMENT FOR DETAILS). Assignors: HARRIS, BRYN, WHITE, CARL
Publication of US20130195738A1 publication Critical patent/US20130195738A1/en
Abandoned legal-status Critical Current

Links

Images

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
    • 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
    • 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
    • C22B3/22—Treatment or purification of solutions, e.g. obtained by leaching by physical processes, e.g. by filtration, by magnetic means, or by thermal decomposition
    • 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
    • C22B34/1259—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
    • C22B34/00—Obtaining refractory metals
    • C22B34/20—Obtaining niobium, tantalum or vanadium
    • C22B34/22—Obtaining vanadium
    • 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 invention relates to a process and system for recovery of titanium dioxide and value metals from ores, intermediates or concentrates.
  • a process for the extraction of iron from iron-containing titaniferous ores is described in U.S. Pat. No. 2,167,628 and U.S. Pat. No. 2,406,577 of Alessandroni et al., who disclose the leaching of titaniferous ore with a solution of hydrochloric acid of a specific gravity of approximately 1.10 and at least 0.5 mole of a soluble chloride e.g. alkali metal chlorides, alkaline earth metal chlorides and aluminum chloride, at a temperature between 70° C. and the boiling point of the solution.
  • the specific gravity of 1.10 is stated to correspond to a concentration of hydrochloric acid of about 230 g/L i.e. about 21% hydrochloric acid.
  • the selective extraction of iron is illustrated. In the former U.S. Pat. No. 2,167,628, it is described as being necessary to reduce any iron present to the ferrous state in order to recover substantially pure titanium dioxide by hydrolysis.
  • McLaughlin describes a method of dissolving titanium minerals wherein it is necessary to add a fluoride to the mixture.
  • the purpose of the fluoride is to break down the silicate matrix of the titanium mineral, thereby allowing the titanium to be dissolved. Subsequent hydrolysis of the solution, however, yields a mixed titanium dioxide-fluoride compound. As with the above processes, it is necessary to reduce ferric iron to ferrous to prevent iron contamination of the subsequent titanium precipitate.
  • a process for leaching ilmenite is described in U.S. Pat. No. 3,903,239 of S. A. Berkovich.
  • the process comprising contacting ilmenite, or a concentrate thereof, with concentrated hydrochloric acid lixiviant solution at a temperature of about 15-30° C. to solubilize and leach from the ore at least 80% and preferably at least 95% of the iron and titanium values.
  • the leaching time is typically 3-25 days, using counter-current flow or the use of closed cycle loops in which hydrochloric acid is continuously passed through a bed of the ore.
  • the reaction is exothermic, and cooling of the reactants may be required.
  • ferric ion in the lixiviant solution is converted to ferrous ion e.g. using a gaseous reductant such as sulphur dioxide, after which the solution is subjected to hydrolysis.
  • the ore may be pre-treated prior to contact with the concentrated hydrochloric acid to increase the rate of dissolution of titanium and iron values during leaching.
  • the pre-treatment is a smelting step that may include oxidation at elevated temperature e.g. 600-1000° C. in the presence of air or oxygen, followed by a reduction of at least part of the iron oxide in the ore with carbon or carbon monoxide.
  • Ti-rich solution from SX1 will undergo a second solvent extraction step, where residual iron is recovered, leaving a concentrated solution of titanium chloride, which is then spray hydrolyzed under controlled conditions to make TiO2 hydrate.
  • This material is said to be a pigment grade product.
  • the lixiviant used has a high chloride content, especially >400 g/L, and the vapour pressure of the solution is greater than atmospheric.
  • the leachate is separated from solids and the ferric ions in the leachate are reduced to ferrous ions.
  • the solution is then cooled to crystallize ferrous chloride.
  • the resultant solution containing titanium ions, ferric ions and ferrous ions is contacted with a water-immiscible organophosphorus extractant.
  • the pregnant strip solution containing titanium and ferric ions, and a minor amount of ferrous ions, is contacted with an amine extractant.
  • the raffinate obtained, which contains titanium ions, is hydrolyzed to produce titanium dioxide.
  • HCl solutions from pyrohydrolysis and from TiO2 hydrolysis are combined and converted into HCl gas and water by pressure-swing distillation, which is a very expensive process and energy-consuming process.
  • U.S. Pat. No. 6,500,396 of V. I. Lakshmanan et al. describes a method for the production of titanium metal from titanium-bearing ore.
  • ore or concentrate is leached with an aqueous solution of a hydrogen halide, especially hydrochloric acid, at a temperature of at least 90° C., followed by a solids/liquids separation and extraction with an immiscible organic phase.
  • the ore is leached with the hydrogen halide in the presence of an oxidizing agent.
  • oxidizing agents include air, hydrogen or other peroxides, or sodium or other perchlorates.
  • iron is solubilized and titanium is converted into titanium dioxide.
  • U.S. Pat. No. 7,803,336 by V. I. Lakshmanan et al. describes a method for the production of titanium metal from titanium-bearing ore.
  • the method provides a process for leaching a value metal from a titanium-bearing ore material containing said value metal, said titanium-bearing ore material being selected from the group consisting of a titanium-bearing ore, concentrate thereof, intermediates and tailings thereof, and mixtures thereof, comprising the step of leaching the titanium-bearing ore material at atmospheric pressure with a lixiviant comprising hydrochloric acid at a concentration of less than 20% (mass ratio), and a chloride selected from the group consisting of alkali metal chlorides, magnesium chloride and calcium chloride, and mixtures thereof.
  • hydrometallurgical processes involve digestion of the ore in a mineral acid, such as hydrochloric acid or sulphuric acid, to extract at least the titanium values from the ore, but generally the iron and vanadium values are also extracted.
  • a mineral acid such as hydrochloric acid or sulphuric acid
  • Each process requires a purification process step of the leach solution before TiO2 recovery is achieved, either the reduction of any ferric iron to its ferrous state, or a separate solvent extraction step to recover the titanium in a pure form.
  • pigment grade being defined as titanium dioxide of purity ⁇ 98.5% TiO 2
  • value metals from titanium bearing materials from a non-purified leach solution containing TiO 2 , as well as, other metals dissolved by hydrochloric acid.
  • a process for recovery of pigment grade titanium dioxide and value metals from a titanium bearing solid comprising the steps of: (a) leaching the solid in hydrochloric acid to produce a leachate comprising undissolved solids and a leach solution comprising the titanium dioxide and the value metals, wherein the hydrochloric acid concentration is maintained above a value required to maintain the titanium dioxide and the value metals dissolved in the leach solution at atmospheric pressure; (b) separating the leachate into the leach solution and the undissolved solids; and (c) reducing the concentration of hydrochloric acid concentration in the leach solution to recover titanium dioxide by hydrolysis and precipitation to produce a titanium dioxide rich slurry.
  • reducing the hydrochloric acid concentration is by heating the leach solution and removing free HCl by HCl distillation of the leach solution.
  • a system for recovering titanium dioxide comprising: a) a leaching section comprising a vessel comprising an ore inlet for a titanium dioxide bearing solid, an acid inlet for hydrochloric acid, an agitator mixing the titanium dioxide bearing solid and the acid to produce a leachate comprising a leach solution and undissolved solids; and a leachate outlet for discharging the leachate; b) a solid liquid separator comprising a leachate inlet hydraulically connected to the leachate outlet, a separation device hydraulically connected to the leachate inlet, for separating the leach solution from the undissolved solids, the device comprising an undissolved solids discharge and a leach solution outlet; and c) a titanium dioxide precipitator for reducing the concentration of the acid in the leach solution and recovering titanium dioxide by precipitation from the leach solution, the precipitator comprising a leach solution inlet hydraulically connected to the leach solution outlet, an HCl acid outlet, and titanium dioxide s
  • the titanium dioxide precipitator comprises a heater for boiling the leach solution to liberate free HCl via the HCl acid outlet and a means of collecting and discharging the precipitated a titanium dioxide slurry.
  • the system described herein further comprising a solvent extraction system hydraulically linked to the leach solution outlet, the solvent extraction system for extractant LIX63 comprising a raffinate outlet.
  • a HCl recovery system comprising a circulating matrix solution and an injection inlet for an oxygen containing gas.
  • the HCl recovery system comprising a reactor for recovering hydrochloric acid and for oxidation/hydrolysis of metal from metal chloride solution, the reactor comprising: a tank compatible with a mixture comprising the metal chloride solution, a matrix solution, an oxygen containing gas and a solid comprising a metal oxide, the tank comprising a base, the base defining a first diameter and a first cross sectional area, the base comprising a metal oxide slurry outlet, a matrix solution outlet and a gas inlet; a top opposite the base, the top comprising a solution inlet, a hydrochloric acid outlet, a matrix solution inlet, the top defining gas an expansion zone having a second cross sectional area and, a wall attached to the top and the base defining a volume and a height of the tank; wherein a ratio of the second cross sectional area to the first cross sectional area is greater than 1 and whereby the hydrochlor
  • the reactor comprises an aspect ratio of the height to the first diameter from 5 to 1-20 to 1.
  • the circulating matrix solution comprises ZnCl 2 .
  • FIG. 1 is a block diagram of a process for the recovery of titanium dioxide and value metals from titanium-bearing ore or concentrate according to one embodiment of the present invention.
  • the present invention relates to a process for leaching of a value metal from a titanium-bearing material.
  • the present invention is directed to the recovery of titanium in the form of pigment-grade quality titanium dioxide from titanium-bearing ores, especially ilmenite or titaniferous magnetite.
  • the present invention relates to processes operated at atmospheric pressure for leaching titanium-bearing ores containing value metals, especially at least one of titanium, vanadium or iron. Titanium is the preferred value metal but where present in sufficient quantities, vanadium is also recovered.
  • the value metal content of the ore may vary widely in type and amount, depending on the source of the ore.
  • the process 1 is operated at atmospheric pressure, using recycled hydrochloric acid 13 that is about 10% to 35% (mass %).
  • Such a concentration of acid may be obtained by hydrolytic distillation of chloride solutions.
  • the titanium-bearing feed material 5 is preferably an ore, but may be a concentrate or intermediate.
  • FIG. 1 uses the abbreviation RoM (run of mill) ore.
  • ore 5 in a form as discussed above is fed to a chloride leach step 10 in which the ore 5 is contacted and leached with a lixiviant comprising a chloride and hydrochloric acid 13 , optionally also containing an oxidant 12 .
  • concentration of hydrochloric acid is 10% (mass ratio) to 35%. Sufficient excess acid is added to ensure that premature precipitation of titanium dioxide does not occur. It is also important to keep the temperature below 70° C., and preferably in the range 50-60° C.
  • the chloride leach step 10 may be conducted continuously as a co-current step, a countercurrent step or in another manner, or the leaching step may be conducted as a batch step.
  • the leaching step 10 is carried out at atmospheric (ambient) pressure i.e. it is not necessary to conduct the leaching step under pressure.
  • the leaching step 10 is carried out with hydrochloric acid having a maximum concentration of 30-35% (mass %).
  • the leaching section of the present system that encompasses block 1 of FIG. 1 includes a vessel that is adapted for HCl acid and suspended solids.
  • the vessel has at least: a solids inlet for a titanium dioxide bearing solid; an acid inlet for hydrochloric acid; an agitator mixing the titanium dioxide bearing solid and the acid and a leachate outlet for discharging the value-metal rich leachate 19 .
  • the agitation of the raw material entering the vessel produces the leachate that is a suspension of the leach solution and undissolved solids.
  • the value metal-rich slurry (leachate) 19 is produced in the leach step is typically in the form of a suspension.
  • the leachate 19 is fed to a solid/liquid separation step 20 to effect separation of leachate 19 into a leach solution 29 and a solids fraction 25 e.g. leach residue and other gangue.
  • solid/liquid separators such as a pressure or vacuum filter, counter-current decanter or centrifuge.
  • the solid/liquid separator is a vacuum belt filter.
  • the leachate 29 obtained from the above solids/liquid separation step is subjected to one or more steps to separate value metals.
  • Techniques for the separation and recovery of value metals from the leachate will be apparent to persons skilled in the art.
  • value metals especially titanium in the form of the metal per se or as titanium dioxide may be recovered from the leach solution by standard or other known methods.
  • separation methods e.g. ion exchange, solvent extraction or precipitation may be used to remove impurities e.g. iron, chromium and vanadium, followed by recovery of titanium as, in particular titanium metal or especially titanium dioxide, using e.g. precipitation.
  • an important advantage of the present process is that the production of pigment-quality TiO 2 can be undertaken directly from the leach solution 29 , after solids removal without any further recovery process steps.
  • the titanium values in the leach solution 29 will be in the form of a titanium chloride compound.
  • the leach solution 29 is heated to its boiling point in a TiO 2 recovery step 30 to distill off any free hydrochloric acid 33 , as a gas which is condensed and collected for recycle for to chloride leach 10 .
  • the action of eliminating the acid causes titanium dioxide to be formed by hydrolysis and precipitates. Therefore, the titanium dioxide is recovered in a TiO 2 precipitator that is understood to be included within the block 30 of FIG. 1 .
  • the precipitator is adapted to allow a reduction of the concentration of the HCl in the leach solution 29 and the precipitation of the TiO 2 solid and removal thereof in a TiO 2 slurry 39 .
  • the precipitator has at least: a leach solution inlet, an HCl acid outlet and a titanium dioxide slurry outlet.
  • ferric iron in the leach solution 29 is first reduced to ferrous iron by the addition of metallic iron powder, prior to heating and titanium dioxide hydrolysis; represented by the following reactions:
  • the TiO 2 slurry 39 is fed to a solid liquid separation step where the TiO 2 45 is removed for example by vacuum filtration, and a TiO 2 free filtrate 49 is produced.
  • the titanium dioxide-free filtrate 49 may be treated to recover vanadium 50 .
  • vanadium when the solution is predominantly ferrous iron chloride, vanadium may be recovered by ion exchange or by solvent extraction with the extractant D2EHPA (di-2-ethyl hexyl phosphoric acid).
  • D2EHPA di-2-ethyl hexyl phosphoric acid
  • the solvent extractant LIX 63 is preferred, thereby removing vanadium 55 .
  • the vanadium 55 may be recovered in any one of several forms including vanadium pentoxide, VOCl 3 , VCl 3 and combinations thereof, where vanadium pentoxide is preferred
  • the loaded resin and D2EHPA solvent extractant is stripped with hydrochloric acid or the solvent extractant
  • the LIX63 is scrubbed with water and stripped with caustic soda and ammonia is added to produce in situ ammonium chloride which precipitates ammonium metavanadate which may then be calcined to produce vanadium pentoxide or vanadium trioxide depending on the temperature of the furnace, the furnace atmosphere and appropriate residence time.
  • the resultant ferrous or ferric or mixtures thereof chloride solution 59 is heated to approximately 180° C. in a Fe 2 O 3 recovery step 60 , where oxidation and hydrolysis takes place, recovering iron as a solid iron oxide 75 , that is substantially hematite in a solid/liquid separation step 70 . Simultaneously, high strength HCl 63 is recovered for recycle.
  • Substantially hematite is defined, as mainly hematite with less that 7% by weight of other materials.
  • the method of the present invention combines the iron precipitation/hydrochloric acid recovery process with titanium dioxide precipitation.
  • this iron recovery 70 and precipitation can occur after TiO 2 recovery.
  • the iron recovery 70 is by Fe 2 O 3 precipitation and Fe 2 O 3 recovery 75 .
  • a barren Fe free MgCl 2 containing solution 79 which is left over can be treated in a MgO recovery step 80 by the reactions including:
  • the leaching process 10 may be conducted continuously in at least one stirred tank reactor. Preferably, at least two reactors are used.
  • a matrix solution may be used in the present process, and may be any compound which is capable of being oxygenated to form, even transiently, a hypochlorite compound, and which remains liquid at temperatures up to at least 190° C., and preferably up to 250° C. It is also preferable that said matrix solution will act as a solvent for any base and light metals which might be present in the feed ferrous iron solution. In practice, there are very few such materials.
  • Zinc chloride is a preferred matrix. Other such compounds are calcium chloride and magnesium chloride, and it is understood that there may be other such matrices alone or in combination. In this application, particularly where the feed is ferrous chloride solution 59 , zinc chloride is preferred since it is both a chloride salt and remains liquid to a temperature >250° C.
  • the matrix solution remains fluid at such temperatures, and the hematite solids are removed by any suitable separation device, for example hot vacuum or pressure filtration.
  • the matrix solution is substantially inert, but acts as a catalyst for oxygen transfer to accelerate the oxidation and hydrolysis reactions.
  • the matrix solution is generally a molten salt hydrate, e.g. ZnCl 2 .2H 2 O in a liquid state and in various states of hydration ZnCl 2 .2H 2 O to ZnCl 2 .5H 2 O depending on the temperature.
  • a base metal is understood as a non-ferrous metal but excluding the precious metals (Au, Ag, Pt, Pd, etc.).
  • the HCl recovery/Fe 2 O 3 precipitation method is conducted in an inert matrix solution according to one embodiment of the present invention, the method steps comprising: an iron oxidation from the solution 59 including light metals (in this case Mg), iron recovery hydrolysis 70 with HCl removal and recycle 63 and hematite production, solid/liquid separation 70 of the hematite 75 , a hydrolysis of the light metals 80 with a further HCl recovery and recycle 83 and MgO separation 26 , and recycle of the inert matrix solution 74 .
  • light metals in this case Mg
  • iron recovery hydrolysis 70 with HCl removal and recycle 63 and hematite production solid/liquid separation 70 of the hematite 75
  • a hydrolysis of the light metals 80 with a further HCl recovery and recycle 83 and MgO separation 26 and recycle of the inert matrix solution 74 .
  • the ferrous chloride solution 59 is added and mixed into the matrix solution together with air or oxygen 61 at 130-160° C. to produce a reaction mixture.
  • Any ferrous iron may be oxidized and subsequently hydrolysed by water at 170-180° C. to form hematite according to the following chemical reactions with HCl 63 produced:
  • the reaction mixture 69 includes: the liquor solution, the matrix solution, the precipitating metal solids, any dissolved solids, unreacted oxygen and HCl. While air can be used to effect the oxidation, its use is not recommended, unless sub-azeotropic ( ⁇ 20% HCl) hydrochloric acid is acceptable to the overall process. This is because the large quantity of nitrogen present in air requires the addition of water to scrub the hydrochloric acid liberated into the off-gas system.
  • the remaining solution 69 /reaction mixture (now an iron-depleted matrix chloride liquor) including the hematite product 75 are then subjected to a solid/liquid separation step 70 .
  • the hematite product thus recovered may be dried and sold, or simply disposed of.
  • magnesium-rich matrix solution 74 is simply recycled in order to build up the concentration of Mg.
  • the remaining matrix solution 79 will contain magnesium chloride.
  • Heating the solution 79 to 220-225° C. will effect the precipitation 50 of magnesium, according to the following reaction using water and/or steam and with HCl 83 produced:
  • the magnesium compounds 89 may be separated from solution leaving hydrolysis by any appropriate separation device, washed and dried.
  • the matrix reactor in a preferred embodiment is a column reactor, defined as tank with a height that is greater than its diameter by at least 5 times.
  • a column reactor is distinguished from a stirred tank reactor, in that it does not have mechanical agitation.
  • the column reactor the liquid flow through the column reactor is downward and countercurrent to the oxygen containing gas flow upward through the column reactor.
  • Advantages of such a column reactor include a preliminary separation of hematite solid in the direction liquid flow downward towards a solids separation apparatus. In a stirred tank reactor the solids would remain equally suspended. However, the process could be performed at lower efficiency in a stirred tank reactor as will be seen in the Examples.
  • the process involves the oxidation and hydrolysis of ferrous iron of the ferrous chloride solution with recovery of associated hydrochloric acid and an iron material (hematite).
  • the reactor comprises electrical heating coils, which are used to heat the reactor to maintain the desired temperature of operation.
  • the heating coils can alternatively be replaced with a jacketed reactor with a thermal fluid such a steam as the heating medium.
  • ferrous iron is oxidized to ferric, hydrolysing the ferric iron and recovering hydrochloric acid and useful metal oxidic materials from any chloride-based feed solution.
  • a method of recovering hydrochloric acid and metal from a ferrous chloride liquor wherein the improvement comprises injecting the liquor into an oxygenated matrix solution in a reaction column countercurrent to the gas flow, wherein the solution assists hydrolysis of the metal and HCl production.
  • the matrix column reactor has an oxygen containing gas injected at the bottom and the ferrous iron chloride, removed from the base.
  • the weight of the liquid in the column of height 1-2 meters, and preferably 1.4-1.8 meters, holds up the oxygen gas in the column, thereby providing sufficient time for the reactions to take place.
  • the first reactor is preferably at 130-170° C., and more preferably at 140-160° C.
  • the temperature of additional reactors in series may be raised to 170-250° C., and more preferably to 180-200° C., in order for the hematite particles to grow. It has been discovered that by maintaining temperature gradients, different particle sizes of hematite in the range 1-100 microns may be formed, thus generating hematite particles with differing color and size. Finer particles will be red in colour, whereas larger, more dense particles vary in color from purple to black.
  • the reactor in a preferred embodiment, has an aspect ratio of reactor height to diameter (in the base portion) of from 5 to 1 to 20 to 1.
  • the top portion of the reactor may comprise a further sampling or injection, as well as a gas expansion zone.
  • the top portion further includes a ferrous chloride solution feed inlet, a hydrochloric acid collection outlet and an optional gas outlet, if a second reactor is connected in series.
  • the uppermost sampling and injection port typically includes an inlet for the circulation of the matrix solution.
  • the matrix solution is usually withdrawn from the bottom-most sampling and injection unit via outlet. From outlet the matrix solution including a slurry of produced hematite is pumped to a solid removal step, such as filtration.
  • the present reactor is meant to oxygenate the matrix solution that generates a concentration, however transient, of hypochlorite, according to the following reaction (using zinc as an example):
  • the ferrous chloride solution may be added from the top of the reactor, such that it meets the oxygenated matrix solution countercurrently.
  • the hypochlorite solution is a very powerful oxidant and thus highly reactive, and instantaneously reacts with the ferrous iron according to the following reaction:
  • Additional water for the reaction is provided by that associated with the incoming feed solution.
  • concentration of the incoming feed solution may be adjusted to give the desired strength showing ports for the addition of fresh ferrous iron feed, a port for the collection of hydrochloric acid vapour, and a third port for unused oxygen gas to proceed to the next reactor.
  • the process of recovery of TiO 2 of the present invention does not require pre-treatment of the titanium-bearing ore prior to the leaching step.
  • a particular advantage of the process 1 of the present invention is that high rates of extraction of value metals are obtained in a leaching step that operates at atmospheric pressure with hydrochloric acid. It is not necessary to operate the leaching step under pressure. The use of atmospheric pressure results in substantial economic advantages, especially in capital costs. Value metals may be recovered. The use of chloride chemistry offers advantages in operating and capital costs of the process. Leaching agent may be regenerated and recycled, especially using hydrolysis step. The use of hydrochloric acid permits recovery and recycle of hydrochloric acid ( 33 , 63 , 83 ) to the leaching step 10 , especially with relatively small amounts of make-up hydrochloric acid.
  • the method of the present invention is conducted in a system having at least three principal components.
  • the first component is a leaching section where the hydrochloric acid leach 10 is performed.
  • the leaching section comprises a vessel having a solids inlet for the titanium dioxide bearing solid, an acid inlet for hydrochloric acid required to leach the titanium dioxide bearing solid, an agitator that is used to mix the solid and acid.
  • a leachate is produced and comprises a leach solution containing dissolved titanium and value metals as well as undissolved solids in suspension.
  • the leaching section vessel also comprises an outlet for discharging the leachate.
  • the second component of the system is a solid/liquid separator connected hydraulically to the leaching section.
  • the separator includes a leachate inlet connected to the leachate outlet of the leaching section.
  • the separator further has a separation device hydraulically connected to the leachate inlet that separates the leach solution from the undissolved solids.
  • the device comprises an undissolved solids discharge and a leach solution outlet.
  • the solid/liquid separator is a vacuum belt filter.
  • the third component of the system is a titanium dioxide precipitator where the concentration of the hydrochloric acid in the leach solution is reduced. With the reduction of concentration of hydrochloric acid the titanium dissolved in solution is hydrolyzed and precipitates from the leach solution.
  • the precipitator includes a leach solution inlet hydraulically linked to the leach solution outlet of the solid liquid separator, an HCl acid inlet and a titanium dioxide slurry outlet.
  • the titanium dioxide precipitator comprises a heater either within the precipitator or in an external circulating loop that heats the leach solution to boiling, thus liberating free HCl as gas via the acid outlet.
  • This free HCl gas can then be condensed via a condenser and preferably recycled back to the leaching section.
  • Table 1 show the chloride leach essentially complete in 1 hour.
  • the Ti dissolves and then hydrolyses (re-precipitates) as TiO 2 as the free HCl is depleted. Therefore, during leaching, it is important to maintain enough free acid to keep the Ti in solution, so that the unleached solids can be filtered off.
  • a continuous miniplant was operated for 10 days leaching a titaniferous magnetite ore containing 20% TiO 2 , 0.38% V 2 O 5 and 67% Fe 3 O 4 . Residence time was 20 minutes and temperature was maintained at 50° C. Ti and V extractions averaged close to 95% at steady state, and iron extraction was 80%.
  • the resulting leach solution on average analyzing 18.5 g/L Ti, 700 mg/L V and 100 g/L Fe, of which 70% was in the ferric form, was subjected to Ti hydrolysis by raising the temperature to 95° C. Ti recovery was 99.9%, with an average analysis of 99% TiO 2 , which is the equivalent of pigment grade titanium dioxide.

Landscapes

  • Chemical & Material Sciences (AREA)
  • Engineering & Computer Science (AREA)
  • Environmental & Geological Engineering (AREA)
  • General Life Sciences & Earth Sciences (AREA)
  • Geology (AREA)
  • Life Sciences & Earth Sciences (AREA)
  • Mechanical Engineering (AREA)
  • Materials Engineering (AREA)
  • Manufacturing & Machinery (AREA)
  • Metallurgy (AREA)
  • Organic Chemistry (AREA)
  • Geochemistry & Mineralogy (AREA)
  • Chemical Kinetics & Catalysis (AREA)
  • General Chemical & Material Sciences (AREA)
  • Manufacture And Refinement Of Metals (AREA)
  • Inorganic Compounds Of Heavy Metals (AREA)
US13/567,013 2010-02-04 2012-08-04 Process for the recovery of titanium dioxide and value metals and system for same Abandoned US20130195738A1 (en)

Priority Applications (1)

Application Number Priority Date Filing Date Title
US13/567,013 US20130195738A1 (en) 2010-02-04 2012-08-04 Process for the recovery of titanium dioxide and value metals and system for same

Applications Claiming Priority (5)

Application Number Priority Date Filing Date Title
US30145810P 2010-02-04 2010-02-04
US30571810P 2010-02-18 2010-02-18
US42050010P 2010-12-07 2010-12-07
PCT/CA2011/000142 WO2011094858A1 (fr) 2010-02-04 2011-02-04 Procédé et système de récupération de dioxyde de titane et de métaux de valeur par réduction de la concentration d'acide chlorhydrique dans une solution de lixiviation
US13/567,013 US20130195738A1 (en) 2010-02-04 2012-08-04 Process for the recovery of titanium dioxide and value metals and system for same

Related Parent Applications (1)

Application Number Title Priority Date Filing Date
PCT/CA2011/000142 Continuation-In-Part WO2011094858A1 (fr) 2010-02-04 2011-02-04 Procédé et système de récupération de dioxyde de titane et de métaux de valeur par réduction de la concentration d'acide chlorhydrique dans une solution de lixiviation

Publications (1)

Publication Number Publication Date
US20130195738A1 true US20130195738A1 (en) 2013-08-01

Family

ID=44354839

Family Applications (1)

Application Number Title Priority Date Filing Date
US13/567,013 Abandoned US20130195738A1 (en) 2010-02-04 2012-08-04 Process for the recovery of titanium dioxide and value metals and system for same

Country Status (6)

Country Link
US (1) US20130195738A1 (fr)
EP (1) EP2531628A1 (fr)
AU (2) AU2011213512A1 (fr)
CA (1) CA2788384C (fr)
WO (1) WO2011094858A1 (fr)
ZA (1) ZA201206582B (fr)

Cited By (8)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US20150252448A1 (en) * 2014-03-05 2015-09-10 Fouad F. KAMALEDDINE Production of high-grade synthetic rutile from low-grade titanium-bearing ores
EP3214190A1 (fr) * 2016-03-01 2017-09-06 SMS Siemag Process Technologies GmbH Procédé de séparation de vanadium
WO2020237312A1 (fr) * 2019-05-28 2020-12-03 Avanti Materials Ltd Récupération de produits à base de titane à partir de minerais de titanomagnétite
WO2021056110A1 (fr) * 2019-09-25 2021-04-01 9203-5468 Quebec Inc. Dba Nmr360 Procédé de récupération d'oxydes de vanadium à partir de divers matériaux
CN112759164A (zh) * 2020-12-31 2021-05-07 北京永新环保有限公司 一种氯化法制钛白粉收尘废渣水资源化处理方法
EP4051818A4 (fr) * 2019-10-31 2023-11-01 Tivan Limited Procédé de récupération de vanadium
WO2024057024A1 (fr) * 2022-09-15 2024-03-21 Fodere Titanium Limited Procédé de production de dioxyde de titane et/ou d'oxyde de vanadium
US12331380B2 (en) * 2020-05-26 2025-06-17 Commonwealth Scientific And Industrial Research Organisation Process for recovering titanium dioxide

Families Citing this family (17)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US7837961B2 (en) 2007-05-21 2010-11-23 Exploration Orbite Vspa Inc. Processes for extracting aluminum and iron from aluminous ores
US9260767B2 (en) 2011-03-18 2016-02-16 Orbite Technologies Inc. Processes for recovering rare earth elements from aluminum-bearing materials
WO2012149642A1 (fr) 2011-05-04 2012-11-08 Orbite Aluminae Inc. Procédés d'extraction d'éléments de terres rares dans divers minerais
IN2014DN03007A (fr) 2011-09-16 2015-05-08 Orbite Aluminae Inc
BR112014016732A8 (pt) 2012-01-10 2017-07-04 Orbite Aluminae Inc processos para tratar lama vermelha
AU2013203808B2 (en) 2012-03-29 2016-07-28 Aem Technologies Inc. Processes for treating fly ashes
MY175471A (en) 2012-07-12 2020-06-29 Orbite Tech Inc Processes for preparing titanium oxide and various other products
JP2015535886A (ja) 2012-09-26 2015-12-17 オーバイト アルミナ インコーポレイテッドＯｒｂｉｔｅ Ａｌｕｍｉｎａｅ Ｉｎｃ． 種々の材料のＨＣｌ浸出によるアルミナおよび塩化マグネシウムを調製するためのプロセス
BR112015011049A2 (pt) 2012-11-14 2017-07-11 Orbite Aluminae Inc métodos para purificação de íons de alumínio
CN103276207B (zh) * 2013-05-17 2015-02-18 中国科学院过程工程研究所 一种湿法处理钒钛磁铁精矿制备钛液的方法
CN103276211B (zh) * 2013-05-17 2015-02-18 中国科学院过程工程研究所 一种从钒钛磁铁精矿中提取铁和钒的方法
CN110678564A (zh) * 2017-04-05 2020-01-10 Tng有限公司 制备浸出给料的方法
CN107475540B (zh) * 2017-08-30 2019-03-29 河南理工大学 一种钛白废液回收钒和钛的工艺
CA3097188A1 (fr) 2018-05-18 2019-11-21 California Institute Of Technology Procede de conversion d'especes de soufre reduit et d'eau en hydrogene et en acide sulfurique
CA3147352A1 (fr) 2019-08-13 2021-02-18 California Institute Of Technology Procede de fabrication d'oxyde de calcium ou de ciment portland ordinaire a partir de roches et de mineraux contenant du calcium
WO2021072534A1 (fr) * 2019-10-15 2021-04-22 9203-5468 Quebec Inc. Dba Nmr360 Procédé de récupération de composés de dioxyde de titane, de vanadium et de fer à partir de divers matériaux
CN112126794A (zh) * 2020-09-02 2020-12-25 衡阳百赛化工实业有限公司 一种次氧化锌除杂富集有价金属锌的烟尘净化处理设备

Citations (1)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
EP0186370A2 (fr) * 1984-12-10 1986-07-02 Grampian Mining Company Limited Préparation du dioxyde de titane pigmentaire à partir d'ilménite

Family Cites Families (11)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US2167628A (en) 1937-10-06 1939-08-01 Nat Lead Co Preparation of titanium dioxide pigments
US2406577A (en) 1942-08-08 1946-08-27 Nat Lead Co Extraction of iron from titaniferous ores
GB1008676A (en) 1960-11-17 1965-11-03 Laporte Titanium Ltd Improvements in and relating to the manufacture of titanium dioxide
BE620418A (fr) 1961-08-05 1900-01-01
US3682592A (en) 1970-07-20 1972-08-08 Pori Inc Treatment of waste hci pickle liquor
US3903239A (en) 1973-02-07 1975-09-02 Ontario Research Foundation Recovery of titanium dioxide from ores
AU8223375A (en) 1974-06-21 1976-12-23 Univ Melbourne Benefication of titaniferous ores
US6500396B1 (en) * 1998-11-17 2002-12-31 Vaikuntam Iyer Lakshmanan Separation of titanium halides from aqueous solutions
US6375923B1 (en) 1999-06-24 2002-04-23 Altair Nanomaterials Inc. Processing titaniferous ore to titanium dioxide pigment
CA2513309C (fr) 2003-11-19 2010-06-15 Process Research Ortech Inc. Procede de recuperation de titane dans des milieux de chlorures melanges
US8628740B2 (en) 2008-06-19 2014-01-14 Sms Siemag Aktiengesellschaft Processing method for recovering iron oxide and hydrochloric acid

Patent Citations (1)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
EP0186370A2 (fr) * 1984-12-10 1986-07-02 Grampian Mining Company Limited Préparation du dioxyde de titane pigmentaire à partir d'ilménite

Cited By (13)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
EP3114244A4 (fr) * 2014-03-05 2017-11-08 Kamaleddine, Fouad F. Production de rutile synthétique de haute qualité à partir de minerais contenant du titane de qualité
CN106232840A (zh) * 2014-03-05 2016-12-14 福阿德·F·卡迈勒丁 从低级含钛矿石生产高级合成金红石
US20150252448A1 (en) * 2014-03-05 2015-09-10 Fouad F. KAMALEDDINE Production of high-grade synthetic rutile from low-grade titanium-bearing ores
US10724119B2 (en) 2016-03-01 2020-07-28 Sms Group Process Technologies Gmbh Process for the separation of vanadium
WO2017148922A1 (fr) * 2016-03-01 2017-09-08 Sms Group Process Technologies Gmbh Procédé de séparation du vanadium
CN108699625A (zh) * 2016-03-01 2018-10-23 Sms集团工艺技术有限公司 用于分离钒的方法
EP3214190A1 (fr) * 2016-03-01 2017-09-06 SMS Siemag Process Technologies GmbH Procédé de séparation de vanadium
WO2020237312A1 (fr) * 2019-05-28 2020-12-03 Avanti Materials Ltd Récupération de produits à base de titane à partir de minerais de titanomagnétite
WO2021056110A1 (fr) * 2019-09-25 2021-04-01 9203-5468 Quebec Inc. Dba Nmr360 Procédé de récupération d'oxydes de vanadium à partir de divers matériaux
EP4051818A4 (fr) * 2019-10-31 2023-11-01 Tivan Limited Procédé de récupération de vanadium
US12331380B2 (en) * 2020-05-26 2025-06-17 Commonwealth Scientific And Industrial Research Organisation Process for recovering titanium dioxide
CN112759164A (zh) * 2020-12-31 2021-05-07 北京永新环保有限公司 一种氯化法制钛白粉收尘废渣水资源化处理方法
WO2024057024A1 (fr) * 2022-09-15 2024-03-21 Fodere Titanium Limited Procédé de production de dioxyde de titane et/ou d'oxyde de vanadium

Also Published As

Publication number Publication date
AU2016204038B2 (en) 2018-05-24
CA2788384C (fr) 2019-02-19
AU2011213512A1 (en) 2012-08-16
WO2011094858A1 (fr) 2011-08-11
ZA201206582B (en) 2014-03-26
CA2788384A1 (fr) 2011-08-11
AU2016204038A1 (en) 2016-07-14
EP2531628A1 (fr) 2012-12-12

Similar Documents

Publication Publication Date Title
AU2016204038B2 (en) Process for the recovery of titanium dioxide and value metals by reducing the concentration of hydrochloric acid in leach solution and system for same
Zhang et al. A literature review of titanium metallurgical processes
EP2784166B1 (fr) Procédé de fabrication de sulfate de nickel de haute pureté
AU2011217756B2 (en) Process for the recovery of metals and hydrochloric acid
JP6025868B2 (ja) 赤泥を処理するプロセス
US6500396B1 (en) Separation of titanium halides from aqueous solutions
US7803336B2 (en) Process for the recovery of titanium in mixed chloride media
US9970078B2 (en) Method for producing a solid scandium-containing material of enhanced scandium content
US20150176103A1 (en) Production of titanium dioxide pigments
CN116209779A (zh) 回收二氧化钛的方法
CN115427592A (zh) 从炉渣材料中回收钒
WO2020237312A1 (fr) Récupération de produits à base de titane à partir de minerais de titanomagnétite
US4119696A (en) Production of titanium metal values
CN1800422A (zh) 一种处理钴铜合金的方法
CA2891360C (fr) Procede pour la separation de fer pendant l'extraction de titane dans des milieux contenant des chlorures melanges
RU2398030C1 (ru) Способ переработки остатков синтеза карбонильного никеля
CN119144852A (zh) 一种氯碱耦合铌钽氯化精馏分离提纯方法
HK1191065A (en) Process for the recovery of titanium in mixed chloride media

Legal Events

Date Code Title Description
AS Assignment

Owner name: NEOMET TECHNOLOGIES INC., CANADA

Free format text: ASSIGNMENT OF ASSIGNORS INTEREST;ASSIGNORS:HARRIS, BRYN;WHITE, CARL;REEL/FRAME:029133/0423

Effective date: 20121015

STCB Information on status: application discontinuation

Free format text: ABANDONED -- FAILURE TO RESPOND TO AN OFFICE ACTION