WO2001012555A2 - Processing aqueous titanium chloride solutions to ultrafine titanium dioxide - Google Patents

Processing aqueous titanium chloride solutions to ultrafine titanium dioxide Download PDF

Info

Publication number
WO2001012555A2
WO2001012555A2 PCT/US2000/016355 US0016355W WO0112555A2 WO 2001012555 A2 WO2001012555 A2 WO 2001012555A2 US 0016355 W US0016355 W US 0016355W WO 0112555 A2 WO0112555 A2 WO 0112555A2
Authority
WO
WIPO (PCT)
Prior art keywords
solution
salts
titanium
temperature
group
Prior art date
Application number
PCT/US2000/016355
Other languages
French (fr)
Other versions
WO2001012555A3 (en
Inventor
Willem P. C. Duyvesteyn
Timothy Malcome Spitler
Bruce James Sabacky
Jan Prochazka
Original Assignee
Altair 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
Priority claimed from US09/500,207 external-priority patent/US6375923B1/en
Application filed by Altair Technologies Inc. filed Critical Altair Technologies Inc.
Priority to CA002375623A priority Critical patent/CA2375623C/en
Priority to DE60015763T priority patent/DE60015763T2/en
Priority to AU19128/01A priority patent/AU769225B2/en
Priority to JP2001516860A priority patent/JP4653916B2/en
Priority to EP00982051A priority patent/EP1194380B9/en
Publication of WO2001012555A2 publication Critical patent/WO2001012555A2/en
Publication of WO2001012555A3 publication Critical patent/WO2001012555A3/en

Links

Classifications

    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B82—NANOTECHNOLOGY
    • B82Y—SPECIFIC USES OR APPLICATIONS OF NANOSTRUCTURES; MEASUREMENT OR ANALYSIS OF NANOSTRUCTURES; MANUFACTURE OR TREATMENT OF NANOSTRUCTURES
    • B82Y30/00—Nanotechnology for materials or surface science, e.g. nanocomposites
    • 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
    • C01G23/0536—Producing by wet processes, e.g. hydrolysing titanium salts by hydrolysing chloride-containing salts
    • C—CHEMISTRY; METALLURGY
    • C09—DYES; PAINTS; POLISHES; NATURAL RESINS; ADHESIVES; COMPOSITIONS NOT OTHERWISE PROVIDED FOR; APPLICATIONS OF MATERIALS NOT OTHERWISE PROVIDED FOR
    • C09C—TREATMENT OF INORGANIC MATERIALS, OTHER THAN FIBROUS FILLERS, TO ENHANCE THEIR PIGMENTING OR FILLING PROPERTIES ; PREPARATION OF CARBON BLACK  ; PREPARATION OF INORGANIC MATERIALS WHICH ARE NO SINGLE CHEMICAL COMPOUNDS AND WHICH ARE MAINLY USED AS PIGMENTS OR FILLERS
    • C09C1/00—Treatment of specific inorganic materials other than fibrous fillers; Preparation of carbon black
    • C09C1/36—Compounds of titanium
    • C09C1/3607—Titanium dioxide
    • C09C1/3615—Physical treatment, e.g. grinding, treatment with ultrasonic vibrations
    • C09C1/363—Drying, calcination
    • 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
    • C01P2004/30—Particle morphology extending in three dimensions
    • C01P2004/32—Spheres
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
    • C01P2004/00—Particle morphology
    • C01P2004/30—Particle morphology extending in three dimensions
    • C01P2004/32—Spheres
    • C01P2004/34—Spheres hollow
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
    • C01P2004/00—Particle morphology
    • C01P2004/60—Particles characterised by their size
    • C01P2004/62—Submicrometer sized, i.e. from 0.1-1 micrometer
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
    • C01P2004/00—Particle morphology
    • C01P2004/60—Particles characterised by their size
    • C01P2004/64—Nanometer sized, i.e. from 1-100 nanometer
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
    • C01P2004/00—Particle morphology
    • C01P2004/80—Particles consisting of a mixture of two or more inorganic phases
    • C01P2004/82—Particles consisting of a mixture of two or more inorganic phases two phases having the same anion, e.g. both oxidic phases
    • C01P2004/84—Particles consisting of a mixture of two or more inorganic phases two phases having the same anion, e.g. both oxidic phases one phase coated with the other
    • C01P2004/86—Thin layer coatings, i.e. the coating thickness being less than 0.1 time the particle radius
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
    • C01P2006/00—Physical properties of inorganic compounds
    • C01P2006/12—Surface area

Definitions

  • the present invention relates to a process for producing ultrafine or "nano- sized" titanium dioxide, parts of the process, and the product of the process.
  • the present invention relates to the processing of aqueous titanium solutions to ultrafine titanium dioxide.
  • the process includes a novel combination of operational steps to economically produce a high quality ultrafine titanium dioxide.
  • Titanium dioxide (TiO 2 ) for pigment use may be present in either of two predominant forms, anatase or rutile, and is used in paints, paper, plastics, ceramics, inks, etc.
  • the titanium dioxide for pigment use generally has an average particle size of 150 to 250 nanometer and is considered the principal white pigment of commerce. It has an exceptionally high refractive index, negligible color, and is quite inert. Titanium dioxide having a smaller average particle size, for instance in the 10 to 100 nanometer median particle size range, is used commercially in cosmetics and personal care products, plastics, surface coatings, self-cleaning surfaces, and photovoltaic applications. This titanium dioxide is referred to as ultrafine or nano-sized titanium dioxide.
  • the present invention provides an economical hydrometallurgical process for producing ultrafine TiO 2 from aqueous titanium chloride solutions.
  • the solutions may be derived from any of several sources, but are practically derived from processing mineral ores and, in particular, ilmenite ore or an ilmenite mineral concentrate.
  • the processing to produce the solutions can be, for instance, a leaching or dissolution process, followed by any of several means for solution purification.
  • the solution could also be produced by hydration of anhydrous titanium tetrachloride.
  • the solution may also be derived from the process described in application no. 60/141 ,114 and U.S. application no. (attorney docket no.
  • the aqueous titanium chloride solution is generally comprised of water, hydrochloric acid, titanium oxychlorides and titanium chlorides.
  • the solutions may vary widely in composition with respect to the hydrochloric acid content and the titanium content.
  • Minor quantities of any of several chemical control agents may be introduced into the solution.
  • the solution is further converted to a titanium oxide solid in a process involving total, controlled evaporation of the solution and the formation of a thin film of titanium dioxide. This process is conducted above the boiling point of the solution and below the temperature where there is significant crystal growth.
  • the water and hydrochloric acid are vaporized and the hydrochloric acid may be recovered.
  • the titanium oxide is next calcined at an elevated temperature to induce and control crystallization.
  • the concentration and type of chemical control agent as well as the calcination conditions determine the desired crystalline form and crystal size of the ultrafine titanium dioxide.
  • the titanium dioxide is milled or dispersed to yield a final nano-sized or ultrafine titanium dioxide having a narrow particle size distribution.
  • the advantages of the process according to the present invention include a superior high quality ultrafine titanium dioxide due to the narrow particle size distribution and readily controlled physical and chemical characteristics, and low cost processing.
  • FIG. 1 is a flow sheet of the general aspect of the process according to the present invention.
  • FIG. 2 is a flow sheet of one embodiment of the process according to the present invention, including vacuum evaporation and recycling of gases.
  • FIG. 3 is a scanning electron micrograph of a spherical particle of unmilled nano-sized titanium dioxide produced according to the method of the present invention and which is magnified 70,000 fold. An amount of 0.16% phosphoric acid was added to the solution as a chemical control.
  • FIG. 4 is a scanning electron micrograph showing the cross-section of a shell of the material depicted in FIG. 3. It is magnified 140,000 fold.
  • FIG. 5 is a scanning electron micrograph of unmilled nano-sized titanium dioxide produced according to the method of the present invention and which is magnified 100,000 fold. An amount of 0.32 % phosphoric acid was added as a chemical control.
  • the present invention is a hydrometallurgical process for producing ultra-fine or "nano-sized" grade TiO 2 from an aqueous titanium chloride solution.
  • Such solutions may be derived from any of several sources including anhydrous titanium chloride, but are preferably derived from the processing of titaniferous ores using hydrochloric acid.
  • FIG. 1 the general process according to the present invention is shown.
  • the aqueous titanium chloride solution is comprised of water, hydrochloric acid, titanium oxychlorides and titanium chlorides.
  • the solution may vary widely in composition with the respect to the hydrochloric acid content and the titanium content.
  • the content of the feed solution may vary from about 3 wt. percent hydrochloric acid to as high as 40 wt. percent HCI and the titanium content may vary from as low as 30 grams of titanium per liter to as high as 200 grams titanium per liter.
  • the source of the titanium chloride solution may be from any known process in which chloride is used during the processing of titanium containing material.
  • the titanium chloride solution may be derived from the processing of titaniferous ores using hydrochloric acid.
  • the solution may also be produced by hydration of anhydrous TiCI 4 .
  • the source of the titanium chloride may be from those described in U.S. application serial no. 60/141 ,057 and 60/141 ,114, and U.S. patent application serial no. (attorney docket no. 9378/4, filed Feb.
  • Minor quantities of chemical control agents may be introduced into the titanium chloride solution to control the physical and mineralogical characteristics of the solid titanium dioxide product resulting from the conversion of the solutions.
  • These chemical control and seeding agents can be, but are not limited to, the chloride salts of sodium, potassium, aluminum, tin, and zinc. Carbonate, fluoride, sulfate and other suitable salts of the same aforementioned elements may be used. Additionally, phosphoric acid and phosphate salts of the aforementioned elements may be used. Furthermore, a number of organic additives may also be used.
  • organic acids such as oxalic, citric, stearic, etc.
  • salts from these organic acids and inorganic compounds include, but are not limited to: organic acids such oxalic, citric, stearic, etc.; salts from these organic acids and inorganic compounds; other organic additives, such as polyacrylates, glycols, siloxane and their compounds.
  • the titanium chloride feed solutions to the process, before or after the chemical control and seeding agents are added may be concentrated with respect to titanium content by any of several methods.
  • a preferred method is by vacuum evaporation, as is shown in FIG. 2.
  • the solutions can be vacuum evaporated under conditions to inhibit formation of titanium dioxide while removing excess water and HCI as vapors. Hydrolysis
  • the titanium chloride solutions containing the chemical control agents are converted to a titanium oxide solid in a process involving total evaporation of the solution and the formation of a thin film of titanium dioxide. This process is conducted above the boiling point of the solution and below the temperature where there is significant crystallization. Water and hydrochloric acid gas are vaporized and the hydrochloric acid may be recovered by any known process.
  • the evaporation, hydrolysis and drying are performed in a manner to control the physical form of the product oxide.
  • hydrolysis is accomplished by spraying the solution while it is heated at a temperature in the range form about 120°C. to about 350°C, and most preferably in the range from about 200°C. to about 250°C. This process is called spray hydrolysis.
  • Spray hydrolysis may be effected in a spray dryer.
  • the resulting physical and chemical characteristics of the solid titanium product can be reliably controlled within a fairly narrow range.
  • the titanium oxide resulting from spray hydrolysis in a spray dryer will be composed of hollow, thin- filmed spheres or parts of spheres.
  • the dimensions of the spheres may vary over a wide range, from less than 1 ⁇ m to 100 ⁇ m or more in diameter, and a shell thickness in the range from about 30 nanometer to about 1000 nanometer or more.
  • the structure of the shell consists of an amorphous, hydrated, polymeric titanium oxide containing some residual chloride.
  • Spray hydrolysis in the given conditions yields spheres composed of a thin film of an amorphous solid that can readily be converted to nano-sized rutile, nano-sized anatase titanium dioxide, or mixtures thereof, depending on the types of chemical controls introduced in the titanium chloride feed solutions and on the physical parameters used in the spray hydrolysis operation.
  • Spray hydrolysis also has the advantage of direct processing of the solution so that the formation of titanium dioxide and evaporation of water and HCI are simultaneously accomplished.
  • the titanium oxide product resulting from the spray hydrolysis operation is calcined at a temperature and for a length of time sufficient to convert the amorphous oxide to titanium dioxide of the desired crystal structure, namely ultrafine titanium dioxide.
  • the temperature is low enough and the time is sufficiently short to limit excessive crystal growth.
  • Calcination temperatures can range between about 450°C to over 1100°C.
  • the calcination is conducted at temperatures ranging from about 600° C to about 900° C.
  • the calcination time also varies over a wide range, from about 20 minutes to as long as 80 hours.
  • the calcination time is in the range from about 30 minutes to about 8 hours. Lower temperatures will require longer calcination times.
  • the product of calcination is a thin film showing a structure of individual units that can be broken up by milling into particles of the desired median size and size distribution.
  • any residual chloride in the amorphous oxide feed is expelled as HCI gas, which can be recovered.
  • chemical control agents may be added to the amorphous oxide just prior to calcination to promote and control conversion of the oxide to the desired crystal structure and other physical characteristics such as crystal size and millability.
  • These chemical control agents can be but are not limited to the chloride salts of sodium, potassium, aluminum, tin, and zinc. Carbonate, fluoride, sulfate and other suitable salts of the same aforementioned elements may be used. Additionally, phosphoric acid and phosphate salts of the aforementioned elements may be used. Milling and Finishing
  • the titanium dioxide After calcination, the titanium dioxide consists of more than 99.5% of either ultrafine (“nano-sized”) anatase or ultrafine (“nano-sized”) rutile, depending on the conditions and chemical control agents used in spray hydrolysis and calcination. After calcination, the titanium dioxide is milled and dispersed to break up the thin film into individual particles. Finishing steps may be added as required.
  • a solution containing 30 g/l Ti and 210 g/l Cl was made according to the process described in U.S. Patent Application Serial No. 60/141 ,114.
  • Phosphoric acid was added in an amount equal to 0.08 wt-% of the amount of solution.
  • the solution was fed to a spray dryer, consisting of a reaction chamber followed by bag filters and an HCI absorption system.
  • the solution was injected at a rate of 2.25 liters/min through an atomizing disk. Gases from the combustion of natural gas, diluted with air to 550°C were also injected around the disk.
  • the outlet temperature was 250°C, and the total gas flow rate was about 800 scfm.
  • Reactor off gasses were sent to a bag filter to collect the TiO 2 product.
  • the recovered product was further calcined at 920°C for 1 hour.
  • Scanning electron micrographs of the product after calcination show spheres with an elemental particle size of the order of 50 nanometer and a film thickness of the order of 1000 nanometer.
  • EXAMPLE 2 A solution containing 30 g/l Ti and 136 g/l Cl was made by dissolving anhydrous liquid TiCI 4 in 3 M HCI and further diluting with water to reach to required titanium concentration. Phosphoric acid was added in an amount equal to 0.16% of the weight of solution. The solution was fed to a spray dryer under the same conditions as those mentioned in Example 1. The product recovered on the bag filter was calcined at 800°C for 6 hours.
  • FIG. 3 is a scanning electron micrograph of the calcined product magnified 70,000 fold.
  • the diameter of the particle shown is about 1.2 ⁇ m.
  • Fig. 4 is a scanning electron micrograph of the same product, showing the edge of a shell.
  • the shell thickness is about 350 nm and elemental particles have a size of about 40 nm.
  • the product is subsequently milled to liberate the individual particles.
  • the milled product has a specific surface area measured by the BET method of 33 m 2 /gram.
  • Example 2 In the same solution used in Example 2, phosphoric acid was added in an amount equal to 0.32% of the weight of solution. The solution was fed to a spray dryer and the product was calcined under the same conditions as those mentioned in Example 1.
  • FIG. 5 is a scanning electron micrograph, magnified 100,000 fold, of the section of a shell after calcination. Individual particles are about 30 nanometer in diameter. The shell thickness is about 400 nm. The product is subsequently milled to liberate the individual particles. The specific surface area of the milled product as measured by the BET method is 43 m 2 /gram.
  • a weight of oxalic acid equal to 1 % of the amount of solution was added to a solution of Ti chloride in hydrochloric acid containing 50 g/l Ti and 230 g/l total chloride.
  • the solution was fed to a spray hydrolyzer under the same conditions as those given in Example 3. While the product after spray hydrolysis had a brown- gray-buff color, due to the presence of some organic residue, the subsequent calcination step reduced the residual carbon content to very low levels as the calcined product had a pure white appearance.
  • the conditions of calcination were the same as those mentioned in Example 3.
  • the calcined product showed a structure of relatively large rutile crystals that were more easily millable than those of the previous example. After milling in a media mill, a product with a median particle size of 50 nm was obtained.

Abstract

A hydrometallurgical process is provided for producing ultrafine or nano-sized titanium dioxide containing solutions, particularly titanium chloride solutions. The process is conducted by total evaporation of the solution, above the boiling point of the solution and below the temperature where there is significant crystal growth. Chemical control additives may be added to control particle size. Nano-sized elemental particles are formed after calcination. The titanium dioxide can be either anatase or rutile. Following calcination, the titanium dioxide is milled to liberate the elemental particles and provide a high quality nano-sized TiO2 with a narrow particle size distribution.

Description

PROCESSING AQUEOUS TITANIUM CHLORIDE SOLUTIONS TO ULTRAFINE TITANIUM DIOXIDE
This application claims priority to U.S. application serial no. 60/141 ,057 and 60/141 ,114 both filed on June 24, 1999, and to U.S. application serial no. 09/500,207, the entire contents of each are incorporated herein by reference.
The present invention relates to a process for producing ultrafine or "nano- sized" titanium dioxide, parts of the process, and the product of the process. In particular, the present invention relates to the processing of aqueous titanium solutions to ultrafine titanium dioxide. The process includes a novel combination of operational steps to economically produce a high quality ultrafine titanium dioxide. BACKGROUND OF THE INVENTION
Titanium dioxide (TiO2) for pigment use may be present in either of two predominant forms, anatase or rutile, and is used in paints, paper, plastics, ceramics, inks, etc. The titanium dioxide for pigment use generally has an average particle size of 150 to 250 nanometer and is considered the principal white pigment of commerce. It has an exceptionally high refractive index, negligible color, and is quite inert. Titanium dioxide having a smaller average particle size, for instance in the 10 to 100 nanometer median particle size range, is used commercially in cosmetics and personal care products, plastics, surface coatings, self-cleaning surfaces, and photovoltaic applications. This titanium dioxide is referred to as ultrafine or nano-sized titanium dioxide.
There are several processes for making ultrafine titanium dioxide, some in commercial use and some in development. Some use anhydrous titanium tetrachloride as a feedstock and burn it in an oxygen-hydrogen flame or in a plasma arc. Another process uses a titanyl sulfate solution as the feedstock. In this process, titanium dioxide is precipitated from the feedstock in a controlled manner, followed sequentially by calcination and intense steam micronization to break up agglomerates formed during the calcination step.
Both types of processes, however, suffer from a lack of control over the product particle size distribution, as well as the product mineralogy. In other words, although the average particle size of the titanium dioxide may be from 10 to 100 nanometer, the particle size distribution may vary greatly. Furthermore, the titanyl sulfate process produces an anatase form whereas the anhydrous chloride oxidation produces a rutile crystallographic modification. Therefore, there is a need for a process to economically make ultrafine titanium dioxide having a narrow particle size distribution and having a specific crystallographic modification made by an easily controlled, lower cost, environmentally sound route.
SUMMARY OF THE INVENTION
The present invention provides an economical hydrometallurgical process for producing ultrafine TiO2 from aqueous titanium chloride solutions. The solutions may be derived from any of several sources, but are practically derived from processing mineral ores and, in particular, ilmenite ore or an ilmenite mineral concentrate. The processing to produce the solutions can be, for instance, a leaching or dissolution process, followed by any of several means for solution purification. The solution could also be produced by hydration of anhydrous titanium tetrachloride. The solution may also be derived from the process described in application no. 60/141 ,114 and U.S. application no. (attorney docket no.
9378/4 filed Feb. 7, 2000), the entire contents of which are incorporated herein by reference.
The aqueous titanium chloride solution is generally comprised of water, hydrochloric acid, titanium oxychlorides and titanium chlorides. The solutions may vary widely in composition with respect to the hydrochloric acid content and the titanium content.
Minor quantities of any of several chemical control agents may be introduced into the solution. The solution is further converted to a titanium oxide solid in a process involving total, controlled evaporation of the solution and the formation of a thin film of titanium dioxide. This process is conducted above the boiling point of the solution and below the temperature where there is significant crystal growth. The water and hydrochloric acid are vaporized and the hydrochloric acid may be recovered. The titanium oxide is next calcined at an elevated temperature to induce and control crystallization. The concentration and type of chemical control agent as well as the calcination conditions determine the desired crystalline form and crystal size of the ultrafine titanium dioxide.
Following calcination, the titanium dioxide is milled or dispersed to yield a final nano-sized or ultrafine titanium dioxide having a narrow particle size distribution.
The advantages of the process according to the present invention include a superior high quality ultrafine titanium dioxide due to the narrow particle size distribution and readily controlled physical and chemical characteristics, and low cost processing. BRIEF DESCRIPTION OF THE DRAWINGS
FIG. 1 is a flow sheet of the general aspect of the process according to the present invention.
FIG. 2 is a flow sheet of one embodiment of the process according to the present invention, including vacuum evaporation and recycling of gases.
FIG. 3 is a scanning electron micrograph of a spherical particle of unmilled nano-sized titanium dioxide produced according to the method of the present invention and which is magnified 70,000 fold. An amount of 0.16% phosphoric acid was added to the solution as a chemical control.
FIG. 4 is a scanning electron micrograph showing the cross-section of a shell of the material depicted in FIG. 3. It is magnified 140,000 fold.
FIG. 5 is a scanning electron micrograph of unmilled nano-sized titanium dioxide produced according to the method of the present invention and which is magnified 100,000 fold. An amount of 0.32 % phosphoric acid was added as a chemical control.
DETAILED DESCRIPTION OF THE INVENTION
The present invention is a hydrometallurgical process for producing ultra-fine or "nano-sized" grade TiO2 from an aqueous titanium chloride solution. Such solutions may be derived from any of several sources including anhydrous titanium chloride, but are preferably derived from the processing of titaniferous ores using hydrochloric acid. Referring now to FIG. 1 , the general process according to the present invention is shown.
Titanium Chloride Solutions
The aqueous titanium chloride solution is comprised of water, hydrochloric acid, titanium oxychlorides and titanium chlorides. The solution may vary widely in composition with the respect to the hydrochloric acid content and the titanium content. For example, the content of the feed solution may vary from about 3 wt. percent hydrochloric acid to as high as 40 wt. percent HCI and the titanium content may vary from as low as 30 grams of titanium per liter to as high as 200 grams titanium per liter.
The source of the titanium chloride solution may be from any known process in which chloride is used during the processing of titanium containing material. For example, the titanium chloride solution may be derived from the processing of titaniferous ores using hydrochloric acid. The solution may also be produced by hydration of anhydrous TiCI4. Additionally, the source of the titanium chloride may be from those described in U.S. application serial no. 60/141 ,057 and 60/141 ,114, and U.S. patent application serial no. (attorney docket no. 9378/4, filed Feb.
7, 2000), the entire contents of which are incorporated herein by reference.
Minor quantities of chemical control agents may be introduced into the titanium chloride solution to control the physical and mineralogical characteristics of the solid titanium dioxide product resulting from the conversion of the solutions. These chemical control and seeding agents can be, but are not limited to, the chloride salts of sodium, potassium, aluminum, tin, and zinc. Carbonate, fluoride, sulfate and other suitable salts of the same aforementioned elements may be used. Additionally, phosphoric acid and phosphate salts of the aforementioned elements may be used. Furthermore, a number of organic additives may also be used. They include, but are not limited to: organic acids such oxalic, citric, stearic, etc.; salts from these organic acids and inorganic compounds; other organic additives, such as polyacrylates, glycols, siloxane and their compounds. Vacuum Evaporation
Optionally, the titanium chloride feed solutions to the process, before or after the chemical control and seeding agents are added, may be concentrated with respect to titanium content by any of several methods. A preferred method is by vacuum evaporation, as is shown in FIG. 2. The solutions can be vacuum evaporated under conditions to inhibit formation of titanium dioxide while removing excess water and HCI as vapors. Hydrolysis
The titanium chloride solutions containing the chemical control agents are converted to a titanium oxide solid in a process involving total evaporation of the solution and the formation of a thin film of titanium dioxide. This process is conducted above the boiling point of the solution and below the temperature where there is significant crystallization. Water and hydrochloric acid gas are vaporized and the hydrochloric acid may be recovered by any known process.
The evaporation, hydrolysis and drying are performed in a manner to control the physical form of the product oxide. Preferably, hydrolysis is accomplished by spraying the solution while it is heated at a temperature in the range form about 120°C. to about 350°C, and most preferably in the range from about 200°C. to about 250°C. This process is called spray hydrolysis. Spray hydrolysis may be effected in a spray dryer.
Through control of the operating parameters, including temperature and chemical composition of the feed solutions to the spray hydrolysis operation, the resulting physical and chemical characteristics of the solid titanium product can be reliably controlled within a fairly narrow range. For example, the titanium oxide resulting from spray hydrolysis in a spray dryer will be composed of hollow, thin- filmed spheres or parts of spheres. The dimensions of the spheres may vary over a wide range, from less than 1 μm to 100 μm or more in diameter, and a shell thickness in the range from about 30 nanometer to about 1000 nanometer or more. The structure of the shell consists of an amorphous, hydrated, polymeric titanium oxide containing some residual chloride.
Without being bound by any theory, it is believed that spray hydrolysis in the given conditions yields spheres composed of a thin film of an amorphous solid that can readily be converted to nano-sized rutile, nano-sized anatase titanium dioxide, or mixtures thereof, depending on the types of chemical controls introduced in the titanium chloride feed solutions and on the physical parameters used in the spray hydrolysis operation. Spray hydrolysis also has the advantage of direct processing of the solution so that the formation of titanium dioxide and evaporation of water and HCI are simultaneously accomplished.
Calcination
The titanium oxide product resulting from the spray hydrolysis operation is calcined at a temperature and for a length of time sufficient to convert the amorphous oxide to titanium dioxide of the desired crystal structure, namely ultrafine titanium dioxide. The temperature is low enough and the time is sufficiently short to limit excessive crystal growth. Calcination temperatures can range between about 450°C to over 1100°C. Preferably, the calcination is conducted at temperatures ranging from about 600° C to about 900° C. The calcination time also varies over a wide range, from about 20 minutes to as long as 80 hours. Preferably, the calcination time is in the range from about 30 minutes to about 8 hours. Lower temperatures will require longer calcination times. The product of calcination is a thin film showing a structure of individual units that can be broken up by milling into particles of the desired median size and size distribution.
During calcination, any residual chloride in the amorphous oxide feed is expelled as HCI gas, which can be recovered.
Additionally and optionally, chemical control agents may be added to the amorphous oxide just prior to calcination to promote and control conversion of the oxide to the desired crystal structure and other physical characteristics such as crystal size and millability. These chemical control agents can be but are not limited to the chloride salts of sodium, potassium, aluminum, tin, and zinc. Carbonate, fluoride, sulfate and other suitable salts of the same aforementioned elements may be used. Additionally, phosphoric acid and phosphate salts of the aforementioned elements may be used. Milling and Finishing
After calcination, the titanium dioxide consists of more than 99.5% of either ultrafine ("nano-sized") anatase or ultrafine ("nano-sized") rutile, depending on the conditions and chemical control agents used in spray hydrolysis and calcination. After calcination, the titanium dioxide is milled and dispersed to break up the thin film into individual particles. Finishing steps may be added as required.
The following examples illustrate, but do not limit, the present invention. Unless otherwise indicated, all parts and percentages are by weight.
EXAMPLE 1
A solution containing 30 g/l Ti and 210 g/l Cl was made according to the process described in U.S. Patent Application Serial No. 60/141 ,114. Phosphoric acid was added in an amount equal to 0.08 wt-% of the amount of solution. The solution was fed to a spray dryer, consisting of a reaction chamber followed by bag filters and an HCI absorption system. The solution was injected at a rate of 2.25 liters/min through an atomizing disk. Gases from the combustion of natural gas, diluted with air to 550°C were also injected around the disk. The outlet temperature was 250°C, and the total gas flow rate was about 800 scfm. Reactor off gasses were sent to a bag filter to collect the TiO2 product. The recovered product was further calcined at 920°C for 1 hour.
Scanning electron micrographs of the product after calcination show spheres with an elemental particle size of the order of 50 nanometer and a film thickness of the order of 1000 nanometer.
EXAMPLE 2 A solution containing 30 g/l Ti and 136 g/l Cl was made by dissolving anhydrous liquid TiCI4 in 3 M HCI and further diluting with water to reach to required titanium concentration. Phosphoric acid was added in an amount equal to 0.16% of the weight of solution. The solution was fed to a spray dryer under the same conditions as those mentioned in Example 1. The product recovered on the bag filter was calcined at 800°C for 6 hours.
FIG. 3 is a scanning electron micrograph of the calcined product magnified 70,000 fold. The diameter of the particle shown is about 1.2 μm. Fig. 4 is a scanning electron micrograph of the same product, showing the edge of a shell. The shell thickness is about 350 nm and elemental particles have a size of about 40 nm. The product is subsequently milled to liberate the individual particles. The milled product has a specific surface area measured by the BET method of 33 m2/gram.
EXAMPLE 3
In the same solution used in Example 2, phosphoric acid was added in an amount equal to 0.32% of the weight of solution. The solution was fed to a spray dryer and the product was calcined under the same conditions as those mentioned in Example 1.
FIG. 5 is a scanning electron micrograph, magnified 100,000 fold, of the section of a shell after calcination. Individual particles are about 30 nanometer in diameter. The shell thickness is about 400 nm. The product is subsequently milled to liberate the individual particles. The specific surface area of the milled product as measured by the BET method is 43 m2/gram.
EXAMPLE 4
A weight of oxalic acid equal to 1 % of the amount of solution was added to a solution of Ti chloride in hydrochloric acid containing 50 g/l Ti and 230 g/l total chloride. The solution was fed to a spray hydrolyzer under the same conditions as those given in Example 3. While the product after spray hydrolysis had a brown- gray-buff color, due to the presence of some organic residue, the subsequent calcination step reduced the residual carbon content to very low levels as the calcined product had a pure white appearance. The conditions of calcination were the same as those mentioned in Example 3. The calcined product showed a structure of relatively large rutile crystals that were more easily millable than those of the previous example. After milling in a media mill, a product with a median particle size of 50 nm was obtained.
While there have been described what are presently believed to be the preferred embodiments of the invention, those skilled in the art will realize that changes and modifications may be made thereto without departing from the spirit of the invention. It is intended to claim all such changes and modifications that fall within the true scope of the invention.

Claims

What is claimed is:
1. A process for producing ultrafine titanium dioxide from a titanium chloride solution comprising: a. adding a chemical control agent to the titanium chloride solution to form a feed solution; b. hydrolyzing the solution in a controlled temperature, total evaporation process at a temperature higher than the boiling point of the solution but lower than the temperature where crystallization becomes significant; c. calcining the hydrolyzed product; and, d. milling the calcined product to liberate the elemental nano-sized particles
2. The process of claim 1 wherein the hydrolyzing step successively evaporates part of the solution, hydrolyzes the titanium in solution to form TiO2, and evaporates the remainder of the solution.
3. The process of claim 1 wherein during the hydrolyzing step, hydrochloric acid is formed and water is removed.
4. The process of claim 3 wherein the hydrochloric acid and water are recovered.
5. The process of claim 1 wherein the hydrolyzing is effected by a spray dryer.
6. The process of claim 5 wherein the spray dryer temperature is between about 120°C and about 350°C.
7. The process of claim 4 wherein the spray dryer temperature is between about 200°C and about 250°C.
8. The process of claim 1 wherein the chemical control agent is selected from the group consisting of chloride salts, fluoride salts, sulfate salts, carbonate salts, phosphate salts of a metal, phosphoric acid, and mixtures thereof.
9. The process of claim 1 wherein the chemical control agent is selected from the group consisting of organic acids selected from the group consisting of oxalic, citric, stearic, a lithium, sodium, potassium, or ammonium salt of these organic acids, polyacrylates, glycols, siloxanes, and mixtures thereof.
10. The process of claim 8 further including a chemical control agent selected from the group consisting of organic acids selected from the group consisting of oxalic, citric, stearic, a lithium, sodium, potassium, and ammonium salt of these organic acids, polyacrylates, glycols, siloxanes, and mixtures thereof.
11. The process of claim 1 wherein the chemical control agent is selected from the group consisting of chloride salts, carbonate salts, fluoride salts, sulfate salts, phosphate salts of sodium, potassium, aluminum, tin, zinc, and mixtures thereof.
12. The process of claim 1 where a thin film of amorphous titanium oxide is formed during the hydrolysis process.
13. The process of claim 12 wherein the amorphous titanium oxide comprises thin film membrane spheres having a diameter between about 1 and about 100 μm and a membrane thickness between about 30 nanometer and about 1000 nanometer.
14. The process of claim 1 wherein the feed solution is first concentrated by vacuum evaporation under conditions to avoid hydrolysis of the titanium chloride.
15. The process of claim 1 wherein the calcining is conducted at a temperature between about 450° C and about 1100° C.
16. The process of claim 1 wherein the calcining is conducted at a temperature between about 600° C and about 900° C.
17. A process for producing ultrafine titanium dioxide having a particle size less than about 100 nanometer from an aqueous titanium chloride solution comprising: a. adding a chemical control agent to the titanium chloride solution to form a feed solution; b. hydrolyzing the solution in a controlled temperature, total evaporation process at a temperature higher than the boiling point of the solution but lower than the calcination temperature of the product; c. calcining the hydrolyzed product; and, d. milling the calcined product to liberate the elemental nano-sized particles
18. The process of claim 1 wherein the hydrolyzing step successively evaporates part of the solution, hydrolyzes the titanium in solution to form TiO2, and evaporates the remainder of the solution.
19. The process of claim 17 wherein the hydrolyzing step includes forming hydrochloric acid and removing water.
20. The process of claim 19 wherein the hydrochloric acid and water are recovered.
21. The process of claim 17 wherein the hydrolyzing is effected by a spray dryer.
22. The process of claim 21 wherein the spray dryer temperature is between about 120° C and about 350°C.
23. The process of claim 21 wherein the spray dryer temperature is between about 200° C and about 250°C.
24. The process of claim 17 wherein the chemical control agent is selected from the group consisting of chloride salts, fluoride salts, sulfate salts, carbonate salts, phosphate salts of a metal, phosphoric acid, and mixtures thereof.
25. The process of claim 17 wherein the chemical control agent is selected from the group consisting of chloride salts, carbonate salts, fluoride salts, sulfate salts, phosphate salts of sodium, potassium, aluminum, tin, zinc, and mixtures thereof.
26. The process of claim 17 wherein the chemical control agent is selected from the group consisting of organic acids selected from the group consisting of oxalic, citric, stearic, a lithium, sodium, potassium, or ammonium salt of these organic acids, polyacrylates, glycols, siloxanes, and mixtures thereof.
27. The process of claim 26 further including a chemical control agent selected from the group consisting of organic acids selected from the group consisting of oxalic, citric, stearic, a lithium, sodium, potassium, and ammonium salt of these organic acids, polyacrylates, glycols, siloxanes, and mixtures thereof.
28. The process of claim 17 where a thin film of amorphous titanium oxide is formed during the hydrolysis step.
29. The process of claim 28 wherein the amorphous titanium oxide comprises hollow spheres or parts of spheres having a diameter between about 1 and about 100 μm and a membrane thickness between about 30 nanometer and about 1000 nanometer.
30. The process of claim 17 wherein the feed solution is concentrated by vacuum evaporation under conditions to avoid hydrolysis of the titanium chloride.
31. The process of claim 17 wherein the calcining is conducted at a temperature between about 450° C and about 1100° C.
32. The process of claim 17 wherein the calcining is conducted at a temperature between about 600° C and about 900° C.
33. The process of claim 17 wherein the average diameter of the titanium dioxide is between about 10 and about 60 nanometer.
PCT/US2000/016355 1999-06-24 2000-06-14 Processing aqueous titanium chloride solutions to ultrafine titanium dioxide WO2001012555A2 (en)

Priority Applications (5)

Application Number Priority Date Filing Date Title
CA002375623A CA2375623C (en) 1999-06-24 2000-06-14 Processing aqueous titanium chloride solutions to ultrafine titanium dioxide
DE60015763T DE60015763T2 (en) 1999-06-24 2000-06-14 METHOD FOR TREATING AQUEOUS TITANTETRACHLORIDE SOLUTIONS FOR THE PREPARATION OF ULTRAFINE TITANIUM DIOXIDE
AU19128/01A AU769225B2 (en) 1999-06-24 2000-06-14 Processing aqueous titanium chloride solutions to ultrafine titanium dioxide
JP2001516860A JP4653916B2 (en) 1999-06-24 2000-06-14 Method for producing ultrafine titanium dioxide from aqueous titanium chloride solution
EP00982051A EP1194380B9 (en) 1999-06-24 2000-06-14 Processing aqueous titanium chloride solutions to ultrafine titanium dioxide

Applications Claiming Priority (8)

Application Number Priority Date Filing Date Title
US14111499P 1999-06-24 1999-06-24
US14105799P 1999-06-24 1999-06-24
US60/141,114 1999-06-24
US60/141,057 1999-06-24
US09/500,207 2000-02-07
US09/500,207 US6375923B1 (en) 1999-06-24 2000-02-07 Processing titaniferous ore to titanium dioxide pigment
US09/503,365 2000-02-14
US09/503,365 US6440383B1 (en) 1999-06-24 2000-02-14 Processing aqueous titanium chloride solutions to ultrafine titanium dioxide

Publications (2)

Publication Number Publication Date
WO2001012555A2 true WO2001012555A2 (en) 2001-02-22
WO2001012555A3 WO2001012555A3 (en) 2001-10-11

Family

ID=27495454

Family Applications (1)

Application Number Title Priority Date Filing Date
PCT/US2000/016355 WO2001012555A2 (en) 1999-06-24 2000-06-14 Processing aqueous titanium chloride solutions to ultrafine titanium dioxide

Country Status (7)

Country Link
US (1) US6440383B1 (en)
EP (1) EP1194380B9 (en)
JP (1) JP4653916B2 (en)
AU (1) AU769225B2 (en)
CA (1) CA2375623C (en)
DE (1) DE60015763T2 (en)
WO (1) WO2001012555A2 (en)

Cited By (10)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
WO2002006159A1 (en) * 2000-07-17 2002-01-24 Industrial Research Limited Titanium-containing materials
US6689716B2 (en) 2000-10-17 2004-02-10 Altair Nanomaterials Inc. Method for producing catalyst structures
KR100420275B1 (en) * 2001-04-06 2004-03-02 (주)아해 Preparation of TiO2 fine powder from titanium tetrachloride with inorganic acid
US6974566B2 (en) 2000-09-05 2005-12-13 Altair Nanomaterials Inc. Method for producing mixed metal oxides and metal oxide compounds
US6982073B2 (en) 2001-11-02 2006-01-03 Altair Nanomaterials Inc. Process for making nano-sized stabilized zirconia
US7482304B2 (en) 2003-12-10 2009-01-27 Altair Nanomaterials Inc. Method for producing structures
CN1898160B (en) * 2003-11-13 2011-06-22 阿尔泰纳米材料公司 Process to make rutile pigment from aqueous titanium solutions
US8182602B2 (en) 2007-08-16 2012-05-22 Sachtleben Pigments Oy Method of preparing a well-dispersable microcrystalline titanium dioxide product, the product, and the use thereof
EP2460830A2 (en) 2003-11-12 2012-06-06 Abbott Laboratories IL-18 binding proteins
CN101676215B (en) * 2008-09-19 2012-11-07 范莉 Method for preparing titanium dioxide nanosphere by using synergistic action of hydrochloric acid and macromolecular compound

Families Citing this family (60)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
EP1033347B2 (en) * 1997-09-02 2012-06-20 Ishihara Sangyo Kaisha, Ltd. Hollow fine powder, flaky fine titanium oxide powder prepared by pulverizing said hollow fine powder, and process for preparing the both
ATE285379T1 (en) * 2001-07-20 2005-01-15 Altair Nanomaterials Inc METHOD FOR PRODUCING LITHIUM TITANATE
EP1282180A1 (en) * 2001-07-31 2003-02-05 Xoliox SA Process for producing Li4Ti5O12 and electrode materials
JP4340160B2 (en) * 2002-03-08 2009-10-07 アルテアナノ インコーポレイテッド Method for producing nano-sized and sub-micron sized lithium transition metal oxides
CA2494787A1 (en) * 2002-08-07 2004-03-25 Ishihara Sangyo Kaisha, Ltd. Titanium dioxide pigments,method for production thereof and resin composition comprising the same
KR100475551B1 (en) * 2002-10-08 2005-03-10 (주)아해 Preparation of Nanosized brookite-phase Titanium Dioxide Powder from Titanium Tetrachloride and Aqueous Hydrochloric Acid
US7140567B1 (en) * 2003-03-11 2006-11-28 Primet Precision Materials, Inc. Multi-carbide material manufacture and use as grinding media
US7407690B2 (en) * 2004-03-23 2008-08-05 Altair Nanomaterials Inc. Process for surface modifications of TiO2 particles and other ceramic materials
US7368523B2 (en) * 2004-11-12 2008-05-06 Eastman Chemical Company Polyester polymer and copolymer compositions containing titanium nitride particles
US20070269522A1 (en) * 2004-08-20 2007-11-22 Wold Chad R Transdermal Drug Delivery Device with Translucent Protective Film
CN101006016A (en) * 2004-08-26 2007-07-25 三井化学株式会社 Ultrafine particle of rutile-type titanium oxide
US20060110557A1 (en) * 2004-09-03 2006-05-25 Zhiyong Xia Polyester polymer and copolymer compositions containing metallic tungsten particles
US20060051542A1 (en) * 2004-09-03 2006-03-09 Zhiyong Xia Polyester polymer and copolymer compositions containing metallic molybdenum particles
US7662880B2 (en) * 2004-09-03 2010-02-16 Eastman Chemical Company Polyester polymer and copolymer compositions containing metallic nickel particles
KR100888559B1 (en) * 2004-10-14 2009-03-16 토쿠센, 유.에스.에이. 인코포레이티드 Method of production of high purity silver particles
WO2006044495A1 (en) * 2004-10-14 2006-04-27 Tokusen U.S.A., Inc. Method for synthesizing nano-sized titanium dioxide particles
JP5241994B2 (en) * 2004-11-05 2013-07-17 戸田工業株式会社 Titanium oxide particle powder and photocatalyst
US20070287193A1 (en) * 2004-11-09 2007-12-13 Monogen, Inc. Vial Assembly, Sampling Apparatus And Method For Processing Liquid-Based Specimens
JP2008519750A (en) * 2004-11-11 2008-06-12 バーゼル・ポリオレフィン・イタリア・ソチエタ・ア・レスポンサビリタ・リミタータ Production of TiO2 powder from waste liquid containing titanium compound
EP1807352A1 (en) * 2004-11-11 2007-07-18 Basell Poliolefine Italia S.r.l. Preparation of tio2 powders from a waste liquid containing titanium compounds
US7300967B2 (en) * 2004-11-12 2007-11-27 Eastman Chemical Company Polyester polymer and copolymer compositions containing metallic titanium particles
KR100627621B1 (en) * 2004-11-19 2006-09-25 한국화학연구원 Rutile Titania Nano Sol, and Process for Preparation Its
US20060122300A1 (en) * 2004-12-07 2006-06-08 Zhiyong Xia Polyester polymer and copolymer compositions containing steel particles
US20060177614A1 (en) * 2005-02-09 2006-08-10 Zhiyong Xia Polyester polymer and copolymer compositions containing metallic tantalum particles
DE102005022076A1 (en) * 2005-02-25 2006-09-07 Heubach Gmbh Pastel white, doped rutile pigment, useful e.g. in polymers, building materials and paints, has reduced photoactivity and specific particle size distribution, prepared from crude or synthetic rutile
US20060210798A1 (en) * 2005-03-16 2006-09-21 Clemens Burda Doped metal oxide nanoparticles and methods for making and using same
US7326399B2 (en) * 2005-04-15 2008-02-05 Headwaters Technology Innovation, Llc Titanium dioxide nanoparticles and nanoparticle suspensions and methods of making the same
KR101304263B1 (en) * 2005-06-03 2013-09-05 후지필름 가부시키가이샤 Pigment-containing thermal-curable composition, color filter, image-recording material, and method of producing color filter
US8557950B2 (en) 2005-06-16 2013-10-15 Grupo Petrotemex, S.A. De C.V. High intrinsic viscosity melt phase polyester polymers with acceptable acetaldehyde generation rates
CN100445209C (en) * 2005-07-28 2008-12-24 同济大学 Preparation method of new type nano-titanium dioxide powder
US7655746B2 (en) 2005-09-16 2010-02-02 Eastman Chemical Company Phosphorus containing compounds for reducing acetaldehyde in polyesters polymers
US7776942B2 (en) * 2005-09-16 2010-08-17 Eastman Chemical Company Polyester polymer and copolymer compositions containing particles of titanium nitride and carbon-coated iron
US7745512B2 (en) * 2005-09-16 2010-06-29 Eastman Chemical Company Polyester polymer and copolymer compositions containing carbon-coated iron particles
MX2008005136A (en) * 2005-10-21 2008-10-31 Altairnano Inc Lithium ion batteries.
US7247200B2 (en) * 2005-11-01 2007-07-24 E. I. Du Pont De Nemours And Company Titanium dioxide finishing process
US20070260002A1 (en) * 2006-05-04 2007-11-08 Zhiyong Xia Titanium nitride particles, methods of making them, and their use in polyester compositions
US20080058495A1 (en) * 2006-09-05 2008-03-06 Donna Rice Quillen Polyester polymer and copolymer compositions containing titanium and yellow colorants
WO2008036176A1 (en) * 2006-09-21 2008-03-27 Tokusen U.S.A., Inc. Low temperature process for producing nano-sized titanium dioxide particles
US8114377B2 (en) * 2006-11-02 2012-02-14 E.I. Du Pont De Nemours And Company Process for producing titanium dioxide particles having reduced chlorides
EP2111370A1 (en) * 2006-12-28 2009-10-28 E. I. Du Pont de Nemours and Company Processes for the flux calcination production of titanium dioxide
JP2010524179A (en) * 2007-03-30 2010-07-15 アルテアーナノ，インコーポレーテッド Method for making a lithium ion cell
US7704470B2 (en) * 2007-04-24 2010-04-27 Haydock Consulting Services, Lc Removal of contaminants from by-product acids
US7858066B2 (en) * 2007-05-08 2010-12-28 E.I. Du Pont De Nemours And Company Method of making titanium dioxide particles
EP2245112A1 (en) * 2007-12-27 2010-11-03 E. I. du Pont de Nemours and Company Method of making photoluminescent samarium-doped titanium dioxide particles
JP5126783B2 (en) * 2008-03-24 2013-01-23 日揮触媒化成株式会社 Method for producing rutile type titanium oxide fine particles
KR100987825B1 (en) * 2008-05-26 2010-10-18 한국화학연구원 Anatase Type Titanium dioxide Nanorods and Its Preparation Method
EP3017986B1 (en) 2008-06-27 2022-11-09 Proterra Operating Company, Inc. Vehicle battery systems and method
US20100111818A1 (en) * 2008-10-29 2010-05-06 Haydock Frederick J Removal of contaminants from by-product hydrochloric acid
CN101922044B (en) * 2010-09-11 2012-02-15 天津大学 Method for doping nano-Ag particles in TiO2 nanotubes
EP2522373A1 (en) 2011-05-11 2012-11-14 Dentsply IH AB Biocompatible component
US8932556B2 (en) * 2013-03-15 2015-01-13 Cristal Usa Inc. Rutile titanium dioxide nanoparticles and ordered acicular aggregates of same
CN111994949A (en) 2014-07-08 2020-11-27 阿瓦塔纳有限公司 Extraction of products from titaniferous ores
US10988828B2 (en) 2017-11-21 2021-04-27 Scandium Intrenational Mining Corporation Extraction of scandium values from copper leach solutions
US10480047B1 (en) 2018-06-28 2019-11-19 Argex Titanium Inc. Process for recovering titanium dioxide from titanium containing materials
CN109354062A (en) * 2018-11-26 2019-02-19 昆明冶金研究院 A kind of nanometer anatase titania and the preparation method and application thereof
US11673812B2 (en) 2019-08-15 2023-06-13 Scandium International Mining Corporation Countercurrent process for recovering high purity copper sulfate values from low grade ores
US11821057B2 (en) 2020-03-06 2023-11-21 Scandium Internatlonal Mlning Corporatlon Recovery of critical metals from SX-EW copper raffinate and other solutions derived from leaching ores with sulfuric acid
KR102411275B1 (en) * 2021-09-15 2022-06-23 주식회사 한내포티 Method for producing anatase-type titanium dioxide using titanium-containing hydrochloric acid solution and titanium dioxide crystal control method using titanium-contained hydrochloric acid solution
WO2023043095A1 (en) * 2021-09-15 2023-03-23 주식회사 한내포티 Method for extracting waste denitrification catalyst-containing valuable metals
CN113860364B (en) * 2021-09-29 2023-03-03 李礼 Method for regulating and controlling crystal transformation process of nano titanium dioxide

Citations (5)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
GB481892A (en) * 1936-09-18 1938-03-18 Titan Co Inc Improvements in and relating to the production of titanium dioxide pigments
GB497694A (en) * 1936-11-06 1938-12-23 Titan Co Inc Improvements in and relating to the decomposition of titanium salt solutions by hydrolytic precipitation
GB2166126A (en) * 1984-10-25 1986-04-30 Mitsubishi Mining & Cement Co Production of a ceramic powder
WO1997010185A1 (en) * 1995-09-15 1997-03-20 Rhodia Chimie Titanium dioxide-based photocatalytic coating substrate, and titanium dioxide-based organic dispersions
DE19725616C1 (en) * 1997-06-17 1998-11-19 Max Planck Gesellschaft Production of nano-crystalline titanium di:oxide

Family Cites Families (85)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US4065544A (en) * 1970-05-11 1977-12-27 Union Carbide Corporation Finely divided metal oxides and sintered objects therefrom
US3967954A (en) 1971-04-09 1976-07-06 Benilite Corporation Of America Pre-leaching or reduction treatment in the beneficiation of titaniferous iron ores
CA949331A (en) 1971-09-01 1974-06-18 National Research Council Of Canada Spherical agglomeration of ilmenite
NL7315931A (en) 1972-12-04 1974-06-06
US3903239A (en) 1973-02-07 1975-09-02 Ontario Research Foundation Recovery of titanium dioxide from ores
JPS5080298A (en) 1973-11-20 1975-06-30
US3966455A (en) 1974-02-19 1976-06-29 Paul Franklin Taylor Process for ilmenite ore reduction
GB1489927A (en) * 1974-08-10 1977-10-26 Tioxide Group Ltd Titanium dioxide carrier
US3935094A (en) 1974-10-10 1976-01-27 Quebec Iron And Titanium Corporation - Fer Et Titane Du Quebec, Incorporated Magnetic separation of ilmenite
US4183768A (en) 1975-03-03 1980-01-15 American Cyanamid Company Anatase pigment from ilmenite
US4085190A (en) 1975-04-29 1978-04-18 Chyn Duog Shiah Production of rutile from ilmenite
US4082832A (en) 1975-05-06 1978-04-04 Solex Research Corporation Treatment of raw materials containing titanium
US3996332A (en) 1975-12-02 1976-12-07 The United States Of America As Represented By The Secretary Of The Interior Synthesis of rutile from titaniferous slags
US4269619A (en) 1976-05-14 1981-05-26 Kerr-Mcgee Chemical Corporation Ilmenite beneficiation process and a digester method
US4097574A (en) 1976-06-16 1978-06-27 United States Steel Corporation Process for producing a synthetic rutile from ilmentite
US4089675A (en) 1976-10-05 1978-05-16 American Cyanamid Company Combination beneficiation ilmenite digestion liquor reduction process
US4120694A (en) 1977-09-06 1978-10-17 The United States Of America As Represented By The Secretary Of The Interior Process for purifying a titanium-bearing material and upgrading ilmenite to synthetic rutile with sulfur trioxide
US4107264A (en) 1977-11-14 1978-08-15 Allied Chemical Corporation Recovery of TiO2 from ilmenite-type ore by a membrane based electrodialysis process
US4168297A (en) 1977-11-14 1979-09-18 Allied Chemical Corporation Recovery of TiO2 from ilmenite-type ore using an organophosphoric acid extractant for impurity iron removal
US4174274A (en) 1978-01-12 1979-11-13 Uop Inc. Separation of rutile from ilmenite
US4158041A (en) 1978-02-21 1979-06-12 Uop Inc. Separation of ilmenite and rutile
FR2418773A1 (en) 1978-03-02 1979-09-28 Thann & Mulhouse METHOD OF USING FERROUS SULPHATE IN THE MANUFACTURE OF PIGMENTAL TITANIUM BIOXIDE BY THE SULPHURIC VOICE
US4152252A (en) 1978-05-04 1979-05-01 Uop Inc. Purification of rutile
US4199552A (en) 1978-05-26 1980-04-22 Kerr-Mcgee Corporation Process for the production of synthetic rutile
US4178176A (en) 1978-07-19 1979-12-11 Uop Inc. Recovery of iron and titanium metal values
US4175952A (en) 1978-07-19 1979-11-27 Uop Inc. Recovery of iron and titanium metal values
US4172878A (en) 1978-07-21 1979-10-30 Uop Inc. Recovery of titanium metal values
US4174963A (en) 1978-07-31 1979-11-20 Uop Inc. Recovery of titanium metal values
US4175110A (en) 1978-08-22 1979-11-20 Uop Inc. Recovery of titanium metal values
US4230542A (en) 1978-10-13 1980-10-28 Oronzio De Nora Impianti Elettrochimici S.P.A. Electrolytic process for treating ilmenite leach solution
US4214913A (en) 1979-03-05 1980-07-29 E. I. Du Pont De Nemours And Company Process for producing rutile TiO2
US4288418A (en) 1979-08-10 1981-09-08 Nl Industries, Inc. Process for manufacturing titanium dioxide
US4288417A (en) 1979-08-10 1981-09-08 Nl Industries, Inc. Process for manufacturing titanium dioxide
US4269809A (en) 1979-12-19 1981-05-26 Uop Inc. Recovery in titanium metal values by solvent extraction
DE2951746A1 (en) 1979-12-21 1981-07-02 Bayer Ag, 5090 Leverkusen DIGESTION OF TERNAER RAW MATERIAL MIXTURES
DE2951799A1 (en) 1979-12-21 1981-07-02 Bayer Ag, 5090 Leverkusen METHOD FOR PRODUCING A HYDROLYZABLE TITANYL SULFATE SOLUTION
US4384883A (en) 1980-08-19 1983-05-24 Ici Australia Limited Reduction of ferrotitaniferous materials
US4401467A (en) 1980-12-15 1983-08-30 Jordan Robert K Continuous titanium process
US4359449A (en) 1980-12-15 1982-11-16 Occidental Research Corporation Process for making titanium oxide from titanium ore
US4390365A (en) 1980-12-15 1983-06-28 Occidental Research Corporation Process for making titanium metal from titanium ore
US4468248A (en) 1980-12-22 1984-08-28 Occidental Research Corporation Process for making titanium metal from titanium ore
US4389391A (en) 1981-06-28 1983-06-21 Dunn Jr Wendell E Process for beneficiating titaniferous ores
JPS5815031A (en) 1981-07-15 1983-01-28 Taijiro Okabe Manufacture of high purity titanium dioxide
JPS60215506A (en) * 1984-04-12 1985-10-28 Mitsubishi Mining & Cement Co Ltd Preparation of ceramic powder and device therefor
AU5051985A (en) 1984-12-10 1986-06-19 Grampian Mining Co. Limited T102 pigment from ilmenite using chloride route with regeneration of hcl from fecl2
EP0214308B1 (en) * 1985-03-05 1993-07-28 Idemitsu Kosan Company Limited Method for preparing super-fine spherical particles of metal oxide
DE3524053A1 (en) 1985-07-05 1987-01-08 Bayer Antwerpen Nv METHOD FOR PRODUCING HIGH QUALITY TITANIUM DIOXIDE BY THE SULFATE METHOD
US5192443A (en) 1987-03-23 1993-03-09 Rhone-Poulenc Chimie Separation of rare earth values by liquid/liquid extraction
US4944936A (en) * 1987-04-10 1990-07-31 Kemira, Inc. Titanium dioxide with high purity and uniform particle size and method therefore
US5104445A (en) 1987-07-31 1992-04-14 Chevron Research & Technology Co. Process for recovering metals from refractory ores
CH672633A5 (en) 1987-11-23 1989-12-15 Escher Wyss Ag
US5061460A (en) 1988-08-19 1991-10-29 Solex Research Corporation Of Japan Method for manufacturing titanium oxide
GB8829402D0 (en) * 1988-12-16 1989-02-01 Tioxide Group Plc Dispersion
NZ231769A (en) 1988-12-20 1991-01-29 Univ Melbourne Production of tif 4 from ore containing tio 2
US4923682A (en) * 1989-03-30 1990-05-08 Kemira, Inc. Preparation of pure titanium dioxide with anatase crystal structure from titanium oxychloride solution
NZ237273A (en) 1990-03-02 1992-02-25 Wimmera Ind Minerals Pty Ltd Upgrading titaniferous ore to produce a synthetic rutile
FI103033B (en) 1990-07-25 1999-04-15 Anglo Amer Corp South Africa Process for the recovery of titanium
AU649441B2 (en) 1990-08-30 1994-05-26 Almeth Pty Ltd Improved process for separating ilmenite
US5135652A (en) 1990-10-25 1992-08-04 Cominco Ltd. Method for the solvent extraction of zinc
WO1992014851A1 (en) 1991-02-21 1992-09-03 The University Of Melbourne Process for the production of metallic titanium and intermediates useful in the processing of ilmenite and related minerals
US5106489A (en) 1991-08-08 1992-04-21 Sierra Rutile Limited Zircon-rutile-ilmenite froth flotation process
US5490976A (en) 1991-08-26 1996-02-13 E. I. Du Pont De Nemours And Company Continuous ore reaction process by fluidizing
DE4211560A1 (en) * 1992-04-07 1993-10-14 Merck Patent Gmbh Composite pigment prodn. - by spraying drying aq. suspension of substrate particles and fine pigment free from additive, used in plastics, lacquer, ink and cosmetics
US5378438A (en) 1992-11-30 1995-01-03 E. I. Du Pont De Nemours And Company Benefication of titaniferous ores
EP0612854B1 (en) 1993-02-23 1998-12-30 Boc Gases Australia Limited Process for the production of synthetic rutile
WO1994026944A1 (en) 1993-05-07 1994-11-24 Technological Resources Pty Ltd Process for upgrading titaniferous materials
DE4329129A1 (en) 1993-08-30 1995-03-02 Merck Patent Gmbh Photostabilisation of titanium dioxide sols
CA2169947A1 (en) 1993-09-13 1995-03-23 Andrzej Calka Ilmenite processing using cold milling
US5441712A (en) 1993-10-15 1995-08-15 Bhp Minerals International Inc. Hydrometallurgical process for producing zinc oxide
US5399751A (en) 1993-11-05 1995-03-21 Glitsch, Inc. Method for recovering carboxylic acids from aqueous solutions
ES2224104T3 (en) * 1993-12-13 2005-03-01 Ishihara Sangyo Kaisha, Ltd. ULTRAFIN PARTICLES OF TITANIUM DIOXIDE TYPE RUTILO CONTAINING IRON AND PROCEDURE FOR PREPARATION.
EP0741802A4 (en) 1994-03-08 1997-05-21 Rgc Mineral Sands Ltd Leaching of titaniferous materials
US5698177A (en) * 1994-08-31 1997-12-16 University Of Cincinnati Process for producing ceramic powders, especially titanium dioxide useful as a photocatalyst
AU4764796A (en) 1995-02-10 1996-08-27 Bhp Minerals International, Inc. Processing ilmenite ore to tio2 pigment
DE19543204C2 (en) * 1995-11-20 1997-09-18 Bayer Ag Process for the production of nanodisperse titanium dioxide and its use
FR2744914B1 (en) 1996-02-15 1998-03-20 Rhone Poulenc Chimie TITANIUM DIOXIDE DISPERSION, TITANIUM DIOXIDE POWDER, THEIR USE IN COSMETIC FORMULATIONS
US5679131A (en) 1996-03-13 1997-10-21 Photran Corporation Method for producing titanium oxide from ore concentrates
JPH09272815A (en) * 1996-04-02 1997-10-21 Merck Japan Kk Composite metal oxide fine particle and production of the same
US5833892A (en) 1996-07-12 1998-11-10 Kemira Pigments, Inc. Formation of TiO2 pigment by spray calcination
JP3524342B2 (en) * 1996-08-30 2004-05-10 昭和電工株式会社 Titanium dioxide sol and thin film for thin film formation
US5730795A (en) 1996-09-24 1998-03-24 E. I. Du Pont De Nemours And Company Process for manufacturing titanium dioxide pigment having a hydrous oxide coating using a media mill
JP4018770B2 (en) * 1997-02-28 2007-12-05 チタン工業株式会社 Fan-shaped titanium oxide, method for producing fan-shaped or plate-shaped titanium oxide, and use thereof
KR100696225B1 (en) * 1998-05-14 2007-03-20 쇼와 덴코 가부시키가이샤 Titanium oxide sol, thin film, and processes for producing these
JP4154515B2 (en) * 1998-06-02 2008-09-24 株式会社村田製作所 TiO2 powder manufacturing method
KR100277164B1 (en) * 1998-07-16 2001-01-15 장인순 A preparing method for crystalline micropowder of Titania from aqueous Titanium(Ⅳ) chloride by homogeneous precipitation process at low temperature

Patent Citations (5)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
GB481892A (en) * 1936-09-18 1938-03-18 Titan Co Inc Improvements in and relating to the production of titanium dioxide pigments
GB497694A (en) * 1936-11-06 1938-12-23 Titan Co Inc Improvements in and relating to the decomposition of titanium salt solutions by hydrolytic precipitation
GB2166126A (en) * 1984-10-25 1986-04-30 Mitsubishi Mining & Cement Co Production of a ceramic powder
WO1997010185A1 (en) * 1995-09-15 1997-03-20 Rhodia Chimie Titanium dioxide-based photocatalytic coating substrate, and titanium dioxide-based organic dispersions
DE19725616C1 (en) * 1997-06-17 1998-11-19 Max Planck Gesellschaft Production of nano-crystalline titanium di:oxide

Cited By (11)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
WO2002006159A1 (en) * 2000-07-17 2002-01-24 Industrial Research Limited Titanium-containing materials
US6974566B2 (en) 2000-09-05 2005-12-13 Altair Nanomaterials Inc. Method for producing mixed metal oxides and metal oxide compounds
US7713504B2 (en) 2000-09-05 2010-05-11 Altair Nanomaterials, Inc. Method for producing mixed metal oxides and metal oxide compounds
US6689716B2 (en) 2000-10-17 2004-02-10 Altair Nanomaterials Inc. Method for producing catalyst structures
KR100420275B1 (en) * 2001-04-06 2004-03-02 (주)아해 Preparation of TiO2 fine powder from titanium tetrachloride with inorganic acid
US6982073B2 (en) 2001-11-02 2006-01-03 Altair Nanomaterials Inc. Process for making nano-sized stabilized zirconia
EP2460830A2 (en) 2003-11-12 2012-06-06 Abbott Laboratories IL-18 binding proteins
CN1898160B (en) * 2003-11-13 2011-06-22 阿尔泰纳米材料公司 Process to make rutile pigment from aqueous titanium solutions
US7482304B2 (en) 2003-12-10 2009-01-27 Altair Nanomaterials Inc. Method for producing structures
US8182602B2 (en) 2007-08-16 2012-05-22 Sachtleben Pigments Oy Method of preparing a well-dispersable microcrystalline titanium dioxide product, the product, and the use thereof
CN101676215B (en) * 2008-09-19 2012-11-07 范莉 Method for preparing titanium dioxide nanosphere by using synergistic action of hydrochloric acid and macromolecular compound

Also Published As

Publication number Publication date
DE60015763T2 (en) 2005-03-31
DE60015763D1 (en) 2004-12-16
US6440383B1 (en) 2002-08-27
AU1912801A (en) 2001-03-13
EP1194380B9 (en) 2005-06-08
CA2375623A1 (en) 2001-02-22
WO2001012555A3 (en) 2001-10-11
JP2003507300A (en) 2003-02-25
EP1194380A2 (en) 2002-04-10
CA2375623C (en) 2009-05-12
EP1194380B1 (en) 2004-11-10
JP4653916B2 (en) 2011-03-16
AU769225B2 (en) 2004-01-22

Similar Documents

Publication Publication Date Title
US6440383B1 (en) Processing aqueous titanium chloride solutions to ultrafine titanium dioxide
US6548039B1 (en) Processing aqueous titanium solutions to titanium dioxide pigment
AU2002319587B2 (en) Process for making lithium titanate
KR101396803B1 (en) Low temperature process for producing nano-sized titanium dioxide particles
JPH092818A (en) Production of crystalline titania powder from solution of titanium salt in water/alcohol mixed solvent
ZA200603777B (en) Process to make rutile pigment from aqueous titanium solutions
AU776394B2 (en) Processing aqueous titanium solutions to titanium dioxide pigment
JP5553601B2 (en) Method for producing titanium oxide powder
JP4177920B2 (en) Method for producing high-purity titanium oxide powder
CN114751450A (en) Method for preparing gas-phase nano titanium dioxide by high-temperature plasma combustion method
JPH08333117A (en) Production of porous globular titanium oxide particle
Sun et al. Preparation of nano rutile titania powders with high photocatalytic properties
KR20000075055A (en) Method for production of titanium dioxide ultrafine powders with rutile phase from titanium sulfate
JP2001151510A (en) Method of producing titanium oxide fine particle
KR100396085B1 (en) A Titanium Dioxide powder and The method for preparation thereof

Legal Events

Date Code Title Description
AK Designated states

Kind code of ref document: A2

Designated state(s): AE AG AL AM AT AU AZ BA BB BG BR BY CA CH CN CR CU CZ DE DK DM DZ EE ES FI GB GD GE GH GM HR HU ID IL IN IS JP KE KG KP KR KZ LC LK LR LS LT LU LV MA MD MG MK MN MW MX MZ NO NZ PL PT RO RU SD SE SG SI SK SL TJ TM TR TT TZ UA UG UZ VN YU ZA ZW

AL Designated countries for regional patents

Kind code of ref document: A2

Designated state(s): GH GM KE LS MW MZ SD SL SZ TZ UG ZW AM AZ BY KG KZ MD RU TJ TM AT BE CH CY DE DK ES FI FR GB GR IE IT LU MC NL PT SE BF BJ CF CG CI CM GA GN GW ML MR NE SN TD TG

121 Ep: the epo has been informed by wipo that ep was designated in this application
DFPE Request for preliminary examination filed prior to expiration of 19th month from priority date (pct application filed before 20040101)
AK Designated states

Kind code of ref document: A3

Designated state(s): AE AG AL AM AT AU AZ BA BB BG BR BY CA CH CN CR CU CZ DE DK DM DZ EE ES FI GB GD GE GH GM HR HU ID IL IN IS JP KE KG KP KR KZ LC LK LR LS LT LU LV MA MD MG MK MN MW MX MZ NO NZ PL PT RO RU SD SE SG SI SK SL TJ TM TR TT TZ UA UG UZ VN YU ZA ZW

AL Designated countries for regional patents

Kind code of ref document: A3

Designated state(s): GH GM KE LS MW MZ SD SL SZ TZ UG ZW AM AZ BY KG KZ MD RU TJ TM AT BE CH CY DE DK ES FI FR GB GR IE IT LU MC NL PT SE BF BJ CF CG CI CM GA GN GW ML MR NE SN TD TG

ENP Entry into the national phase

Ref document number: 2375623

Country of ref document: CA

Ref country code: CA

Ref document number: 2375623

Kind code of ref document: A

Format of ref document f/p: F

WWE Wipo information: entry into national phase

Ref document number: 19128/01

Country of ref document: AU

ENP Entry into the national phase

Ref country code: JP

Ref document number: 2001 516860

Kind code of ref document: A

Format of ref document f/p: F

WWE Wipo information: entry into national phase

Ref document number: 2000982051

Country of ref document: EP

WWP Wipo information: published in national office

Ref document number: 2000982051

Country of ref document: EP

REG Reference to national code

Ref country code: DE

Ref legal event code: 8642

WWG Wipo information: grant in national office

Ref document number: 19128/01

Country of ref document: AU

WWG Wipo information: grant in national office

Ref document number: 2000982051

Country of ref document: EP