US3207571A - Process for preparing cesium compounds from cesium alum - Google Patents
Process for preparing cesium compounds from cesium alum Download PDFInfo
- Publication number
- US3207571A US3207571A US185833A US18583362A US3207571A US 3207571 A US3207571 A US 3207571A US 185833 A US185833 A US 185833A US 18583362 A US18583362 A US 18583362A US 3207571 A US3207571 A US 3207571A
- Authority
- US
- United States
- Prior art keywords
- cesium
- hydroxide
- sulfate
- water
- solution
- 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.)
- Expired - Lifetime
Links
Classifications
-
- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01D—COMPOUNDS OF ALKALI METALS, i.e. LITHIUM, SODIUM, POTASSIUM, RUBIDIUM, CAESIUM, OR FRANCIUM
- C01D17/00—Rubidium, caesium or francium compounds
Definitions
- This ore can be represented by various formulae from Cs Al Si O -H O to Cs Na Al Si O -yH O where x is a number from to 15 and y is usually 1 or less than 1. When x is 16 the mineral is termed analcite.
- More than this quantity of Water may be added if necessary to keep the ore-acid paste in stirrable condition, since, as the reaction progresses, the originally thin paste thickens to a very stiff, hard-to-stir paste unless water is added to restore it to a fluid consistency.
- Using less than the above mentioned quantity of one-fourth the ore Weight of water results in a decreased recovery of cesium values from the ore.
- the water may be added with the acid to the powdered ore if desired or part of the water can be so added and the remainder during the acid treatment period. To ensure maximum acid-ore contact the ore is finely ground, usually to minus 200- mesh.
- M is any one of the alkali metals.
- the alkali metals and aluminum may not be present as oxides in the ore and this method of dealing with them is for simplicity; it has proven to be reliable.
- Pollucite the mineral, occurs in association with other minerals. For example, a petrographic examination of Bikita pollucite ore showed the presence of albite, lepidolite and quartz in addition to pollucite.
- the quantity of acid used to form cesium alum has been found to be critical. In contrast to classical methods heretofore described, we have found an excess of acid decreases the yield rather than increasing it as would be expected. We have found that about a 10% increase over the stoichiometric quantity of acid required is all that can or should be used. A 50% increase over the stoichiometric acid requirement lowers the cesium recovery by as much as 13%, all other reaction conditions being the same. If a 100% excess of acid is used, the cesium recovery is decreased by 45%, maintaining other reaction conditions the same.
- the cesium alum then is crystallized a number of times and further processed to form the desired cesium salt.
- the purified cesium alum is then added to a hot slurry of calcium hydroxide in distilled or demineralized water to yield a solution of cesium sulfate and a solid residue of calcium sulfate hydrate and aluminum hydroxide.
- the calcium hydroxide is added in amount suflicient to stoichiometrically convert substantially all of the cesium alum to cesium sulfate and aluminum hydroxide.
- the solution of cesium sulfate is separated from the solid material by filtration, centrifugation, sedimentation or any combination of these.
- Pure cesium sulfate can be recovered by evaporating the solution to dryness and calcining the salt so obtained at about 300 F. to remove the last traces of water.
- Conversion of cesium sulfate into other cesium salts can be accomplished by adding an aqueous barium hydroxide mixture to the cesium sulfate liquor obtained as above. The resulting mixture of cesium hydroxide and barium sulfate is separated by filtration, centrifugation, sedimentation, or a combination of these to yield a solution of cesium hydroxide. Cesium hydroxide can then be converted into the desired cesium salt by acidification with the desired acid.
- Another way of obtaining cesium salts other than the sulfate or hydroxide is to treat the cesium sulfate solution with a barium salt of the desired acid such as barium chloride or barium nitrate.
- the barium sulfate precipitate is again removed as before and the solution of the desired cesium salt is concentrated and evaporated to dryness.
- Example 1 One hundred pounds of minus ZOO-mesh Bikita pollucite ore was charged to :a 15 gal. cast iron kettle equipped with a motor driven agitator and a steam jacket. Both high pressure p.s.i.g.) and low pressure (35 p.s.i.g.) steam were piped into the heating jacket with appropriate valving so that either heat source could be used.
- the Bikita pollucite ore used contained 25.5% Cs O. A total of 64.5 pounds of 102% H 80 was slowly mixed remove entrainment.
- a batch of 115 pounds of cesium alum prepared as described above was slurried in 50 gallons of hot (200 F.) distilled water and a slurry of 24 pound-s of calcium hydroxide in 10 gallons of distilled water was slowly added. After digesting for 30 minutes the slurry was filtered in vertical pressure filters, and the cake was Washed with 40 gallons of hot distilled water. A total of 140 pounds of wet calcium sulfate-aluminum hydroxide hydrate cake containing 0.19% residual cesium oxide was dumped from the filters. A cesium recovery of 99% was obtained in this operation.
- the cesium sulfate solution obtained as just described was combined with additional cesium sulfate solution to yield va total of 158 gallons of liquor containing 46.7 pounds of cesium oxide.
- This solution was treated with 70.0 pounds of barium hydroxide octahydrate dissolved in about gallons of distilled water to convert the cesium sulfate to cesium hydroxide and form a precipitate of barium sulfate.
- the slurry was filtered on a Sweetland filter and the cake washed with 35 gallons of hot distilled water. A total of 74 pounds of wet barium sulfate cake was obtained containing 0.75% cesium oxide.
- Example 2 A reaction vessel loaded with 1750 pounds of pollucite ore and 75 gallons of 102% sulfuric acid was run in. Sufficient water was run in to maintain a workable slurry while ore decomposition was in progress.
- reaction vessel contents of the reaction vessel were dumped into 2000 gallons of hot 200 F. water, leached under agitation for 30,minutes, and filtered.
- the filter cake was thoroughly washed with 800 gallons of hot (200 F.) water. Analysis of the washed residue indicated a cesium extraction of 90.5%.
- the filtrate and wash water were cooled to 90 F. to crystallize out about 2000 pounds of cesium alum. This cesium alum was then recrystallized four times, using about 1000 gallons of water for each recrystallization to yield a 99.9% pure product.
- the purified alum then was dewatered and the cesium alum was dumped into 800 gallons of hot (180 F.) deionized water containing 375 pounds of calcium hydrox- 'ide. After about 3 hours digestion at 180 F., the slurry temperature was lowered to 150 F., and the slurry was filtered. The calcium sulfate-aluminum hydroxide hydrate filter cake was Washed with deionized water to The residual cesium oxide content of the filter cake was 0.67%. At this point, the over-all recovery of cesium values from the ore was 84.8%.
- the resulting cesium sulfate solution was concentrated to reduce the volume to about 800 gallons, and to it was added a hot solution of 530 pounds of barium hydroxide octahydrate in 250 gallons of deionized water. This slurry of barium sulfate in cesium hydroxide solution was then filtered and the barium sulfate cake was washed with 500 gallons of hot deionized water. The residual (absorbed) cesium oxide of this filter cake was 1.47%. Following this filtration, the cesium hydroxide solution was carbonated and concentrated to yield a cesium carbonate liquor which was then polish-filtered to remove barium carbonate and dried. A total yield of 424 pounds of 99.9% cesium carbonate was obtained, corresponding to an overall yield of 77%.
- the process for preparing cesium sulfate which comprises treating cesium alum with calcium hydroxide in an aqueous medium, the calcium hydroxide being employed in an amount sufiicientto stoichiometrically convert the cesium alum to a mixture containing a solution of cesium sulfate and insoluble aluminum hydroxide and insoluble calcium sulfate, and separating a soluble cesium sulfate solution consisting essentially of water and cesium sulfate.
- the process for preparing cesium compounds which comprises treating cesium alum with calcium hydroxide in an aqueous medium, the calcium hydroxide being employed in an amount sufficient to stoichiometrically convert substantially all of the cesium alum to :a mixture containing a solution of cesium sulfate, insoluble aluminum hydroxide and insoluble calcium sulfate, said solution consisting essentially of water and cesium sulfate, treating said cesium sulfate solution with barium hydroxide to form an aqueous mixture containing soluble cesium hydroxide and insoluble barium sulfate, and separating an aqueous solution of soluble cesium hydroxide consisting essentially of water and cesium hydroxide.
- the process for preparing cesium compounds which comprises treating cesium alum with calcium hydroxide in an aqueous medium, the calcium hydroxide being employed in an amount sufficient to stoichiometrically convert substantially all of the cesium alum to a mixture containing a solution of cesium sulfate, insoluble aluminum hydroxide and insoluble calcium sulfate, said solution consisting essentially of water and cesium sulfate, treating said cesium sulfate solution with barium hydroxide to form an aqueous mixture containing soluble cesium hydroxide and insoluble barium sulfate, said cesium hydroxide being dissolved 1111a solution consisting essentially of water and cesium hydroxide, and carbonating the aqueous solution of cesium hydroxide to form a solution consisting essentially of water and soluble cesium carbonate.
Landscapes
- Chemical & Material Sciences (AREA)
- Organic Chemistry (AREA)
- Engineering & Computer Science (AREA)
- Materials Engineering (AREA)
- Inorganic Chemistry (AREA)
- Compounds Of Alkaline-Earth Elements, Aluminum Or Rare-Earth Metals (AREA)
Description
United States Patent ()fi ice 3,207,571 Patented Sept. 21, 1965 3,207,571 PRGCESS FGR PREPARING CESKUM COMPOUNDS FRGM CESIUM ALUM Cornelius E. lBerthold, Trona, Calif, assignor, by mesne assignments, to San Antonio Chemicals, Inc., a corporation of Deiaware No Drawing. Filed Apr. 9, 1962, $91. No. 185,833 4 Claims. (Cl. 23-33) This invention relates to the recovery of cesium values as cesium salts from cesium aluminosilicate ore, pollucite. This ore can be represented by various formulae from Cs Al Si O -H O to Cs Na Al Si O -yH O where x is a number from to 15 and y is usually 1 or less than 1. When x is 16 the mineral is termed analcite.
Heretofore, it has been necessary to subject this ore to long and severe chemical treatment to decompose it and provide the cesium value in a recoverable form. For example, processes described in Inorganic Synthesis, vol. IV, pp. 69, McGraw-Hill (1953), utilize approximately four times the stoichiometric amount of sulfuric hydrochloric acid theoretically required by the alkalies and aluminum in the ore. The ore-acid solution is heated to boiling and refluxed for periods of up to 30 hours to enable a 90% recovery of the cesium contained in the ore as cesium alum or cesium aluminum chloride. Multiple leaches are also employed to increase the cesium recovery. After digesting the ore-acid mixture for the required period, one is faced with the problem of conveying, pumping, and filtering a hot, very corrosive, abrasive slurry. The demands upon materials of construction by such a combination are very severe, with the result that operating costs and maintenance requirements are both very high.
I have discovered a new and novel method of treating pollucite ore which obviates these heretofore severe treatment methods and affords a simple, economical, and relatively rapid means of recovering cesium salts from the ore. In addition, it eliminates the need for handling a hot, strongly acidic and very corrosive, abrasive slurry with its attendant problem.
I have found that, if a mixture of finely ground pollucite ore and the stoichiometric quantity of sulfuric acid required for reaction with the alkali metals and aluminum present in the ore be heated to a temperature of about 150 C. for a period of about four hours, and a weight of water equal to at least one-fourth the weight of the pollucite ore used be added to the ore-acid mixture during this period, substantially complete extraction of cesium values as cesium alum from the ore results. More than this quantity of Water may be added if necessary to keep the ore-acid paste in stirrable condition, since, as the reaction progresses, the originally thin paste thickens to a very stiff, hard-to-stir paste unless water is added to restore it to a fluid consistency. Using less than the above mentioned quantity of one-fourth the ore Weight of water results in a decreased recovery of cesium values from the ore. The water may be added with the acid to the powdered ore if desired or part of the water can be so added and the remainder during the acid treatment period. To ensure maximum acid-ore contact the ore is finely ground, usually to minus 200- mesh.
In arriving at the quantity of acid one can take into account the alkali metals and the aluminum present as oxides:
where M is any one of the alkali metals. The alkali metals and aluminum may not be present as oxides in the ore and this method of dealing with them is for simplicity; it has proven to be reliable. One must deal with ore composition for it is the ore which must be decomposed. Pollucite, the mineral, occurs in association with other minerals. For example, a petrographic examination of Bikita pollucite ore showed the presence of albite, lepidolite and quartz in addition to pollucite.
It has been found convenient to operate the ore-acid reaction within a temperature range of about C. to about 180 C. Temperatures lower than 100 C. require longer reaction times while at temperatures above about 180 C. too much water is lost from the reaction mixture, thereby necessitating frequent addition of water or operation under reflux and so increasing the cost of the reactor vessel.
The quantity of acid used to form cesium alum has been found to be critical. In contrast to classical methods heretofore described, we have found an excess of acid decreases the yield rather than increasing it as would be expected. We have found that about a 10% increase over the stoichiometric quantity of acid required is all that can or should be used. A 50% increase over the stoichiometric acid requirement lowers the cesium recovery by as much as 13%, all other reaction conditions being the same. If a 100% excess of acid is used, the cesium recovery is decreased by 45%, maintaining other reaction conditions the same.
The cesium alum then is crystallized a number of times and further processed to form the desired cesium salt. The purified cesium alum is then added to a hot slurry of calcium hydroxide in distilled or demineralized water to yield a solution of cesium sulfate and a solid residue of calcium sulfate hydrate and aluminum hydroxide.
In general, the calcium hydroxide is added in amount suflicient to stoichiometrically convert substantially all of the cesium alum to cesium sulfate and aluminum hydroxide.
The solution of cesium sulfate is separated from the solid material by filtration, centrifugation, sedimentation or any combination of these.
Pure cesium sulfate can be recovered by evaporating the solution to dryness and calcining the salt so obtained at about 300 F. to remove the last traces of water.
Conversion of cesium sulfate into other cesium salts can be accomplished by adding an aqueous barium hydroxide mixture to the cesium sulfate liquor obtained as above. The resulting mixture of cesium hydroxide and barium sulfate is separated by filtration, centrifugation, sedimentation, or a combination of these to yield a solution of cesium hydroxide. Cesium hydroxide can then be converted into the desired cesium salt by acidification with the desired acid.
Another way of obtaining cesium salts other than the sulfate or hydroxide is to treat the cesium sulfate solution with a barium salt of the desired acid such as barium chloride or barium nitrate. The barium sulfate precipitate is again removed as before and the solution of the desired cesium salt is concentrated and evaporated to dryness.
The practice of the invention is further illustrated by the following examples.
Example 1 One hundred pounds of minus ZOO-mesh Bikita pollucite ore was charged to :a 15 gal. cast iron kettle equipped with a motor driven agitator and a steam jacket. Both high pressure p.s.i.g.) and low pressure (35 p.s.i.g.) steam were piped into the heating jacket with appropriate valving so that either heat source could be used.
The Bikita pollucite ore used contained 25.5% Cs O. A total of 64.5 pounds of 102% H 80 was slowly mixed remove entrainment.
in with the ore and sufficient water added to yield a thin slurry. The steam was slowly turned on in the jacket and the paste mixed for a period of 5 hours. During the reaction period, the temperature of the pot contents ranged from 250 F. (121 C.) to 300 F. (149 C.). Several times during the reaction period, the reaction became violent and the charge foamed badly so that the steam pressure was reduced or shut off entirely to allow the reaction mixture to cool down. After the 5-hour reaction period was completed, the charge was dumped into 100 gallons of hot (200 F.) water in an agitated stainless steel tank. The slurry was leached for one hour and then filtered in two vertical, plastic-lined, pressure filters. The filter cakes were washed with two -gallon portions of hot (200 F.) water to remove as much of the soluble cesium values as possible. A total of 97.5 pounds of cesium alum containing 23.5% Cs O was obtained for an 89.8% cesium recovery.
A batch of 115 pounds of cesium alum prepared as described above was slurried in 50 gallons of hot (200 F.) distilled water and a slurry of 24 pound-s of calcium hydroxide in 10 gallons of distilled water was slowly added. After digesting for 30 minutes the slurry was filtered in vertical pressure filters, and the cake was Washed with 40 gallons of hot distilled water. A total of 140 pounds of wet calcium sulfate-aluminum hydroxide hydrate cake containing 0.19% residual cesium oxide was dumped from the filters. A cesium recovery of 99% was obtained in this operation.
The cesium sulfate solution obtained as just described was combined with additional cesium sulfate solution to yield va total of 158 gallons of liquor containing 46.7 pounds of cesium oxide. This solution was treated with 70.0 pounds of barium hydroxide octahydrate dissolved in about gallons of distilled water to convert the cesium sulfate to cesium hydroxide and form a precipitate of barium sulfate. Following this step, the slurry was filtered on a Sweetland filter and the cake washed with 35 gallons of hot distilled water. A total of 74 pounds of wet barium sulfate cake was obtained containing 0.75% cesium oxide. By difference, there was 46.2 pounds of cesium oxide remaining in the filtrate for a recovery of 98.8% in this openation. This dilute cesium hydroxide solution was then concentrated and carbonated to convert it to cesium carbonate liquor and also to precipitate any excess barium hydroxide as barium carbonate. An over-allrecovery of 87.8% of the cesium values in the ore was obtained as a 98.5% pure cesium carbonate. Example 2 A reaction vessel loaded with 1750 pounds of pollucite ore and 75 gallons of 102% sulfuric acid was run in. Sufficient water was run in to maintain a workable slurry while ore decomposition was in progress.
Thereafter, the contents of the reaction vessel were dumped into 2000 gallons of hot 200 F. water, leached under agitation for 30,minutes, and filtered. The filter cake was thoroughly washed with 800 gallons of hot (200 F.) water. Analysis of the washed residue indicated a cesium extraction of 90.5%. The filtrate and wash water were cooled to 90 F. to crystallize out about 2000 pounds of cesium alum. This cesium alum was then recrystallized four times, using about 1000 gallons of water for each recrystallization to yield a 99.9% pure product.
The purified alum then was dewatered and the cesium alum was dumped into 800 gallons of hot (180 F.) deionized water containing 375 pounds of calcium hydrox- 'ide. After about 3 hours digestion at 180 F., the slurry temperature was lowered to 150 F., and the slurry was filtered. The calcium sulfate-aluminum hydroxide hydrate filter cake was Washed with deionized water to The residual cesium oxide content of the filter cake was 0.67%. At this point, the over-all recovery of cesium values from the ore was 84.8%.
' The resulting cesium sulfate solution was concentrated to reduce the volume to about 800 gallons, and to it was added a hot solution of 530 pounds of barium hydroxide octahydrate in 250 gallons of deionized water. This slurry of barium sulfate in cesium hydroxide solution was then filtered and the barium sulfate cake was washed with 500 gallons of hot deionized water. The residual (absorbed) cesium oxide of this filter cake was 1.47%. Following this filtration, the cesium hydroxide solution was carbonated and concentrated to yield a cesium carbonate liquor which was then polish-filtered to remove barium carbonate and dried. A total yield of 424 pounds of 99.9% cesium carbonate was obtained, corresponding to an overall yield of 77%.
I claim:
1. The process for preparing cesium sulfate which comprises treating cesium alum with calcium hydroxide in an aqueous medium, the calcium hydroxide being employed in an amount sufiicientto stoichiometrically convert the cesium alum to a mixture containing a solution of cesium sulfate and insoluble aluminum hydroxide and insoluble calcium sulfate, and separating a soluble cesium sulfate solution consisting essentially of water and cesium sulfate.
2. The process of claim 1 in which the separated soluble cesium sulfate solution is evaporated to dryness to recover anhydrous cesium sulfate.
3. The process for preparing cesium compounds which comprises treating cesium alum with calcium hydroxide in an aqueous medium, the calcium hydroxide being employed in an amount sufficient to stoichiometrically convert substantially all of the cesium alum to :a mixture containing a solution of cesium sulfate, insoluble aluminum hydroxide and insoluble calcium sulfate, said solution consisting essentially of water and cesium sulfate, treating said cesium sulfate solution with barium hydroxide to form an aqueous mixture containing soluble cesium hydroxide and insoluble barium sulfate, and separating an aqueous solution of soluble cesium hydroxide consisting essentially of water and cesium hydroxide.
4. The process for preparing cesium compounds which comprises treating cesium alum with calcium hydroxide in an aqueous medium, the calcium hydroxide being employed in an amount sufficient to stoichiometrically convert substantially all of the cesium alum to a mixture containing a solution of cesium sulfate, insoluble aluminum hydroxide and insoluble calcium sulfate, said solution consisting essentially of water and cesium sulfate, treating said cesium sulfate solution with barium hydroxide to form an aqueous mixture containing soluble cesium hydroxide and insoluble barium sulfate, said cesium hydroxide being dissolved 1111a solution consisting essentially of water and cesium hydroxide, and carbonating the aqueous solution of cesium hydroxide to form a solution consisting essentially of water and soluble cesium carbonate.
References Cited by the Examiner UNITED STATES PATENTS OTHER REFERENCES Jacobson: Encyclopedia of Chemical Reactions, vol. II 1948 p. 657.
Mellor: Comprehensive Treatise on Inorganic and Theoretical Chemistry, vol. 2, Longmans, Green and Co., N.Y., 1922, p. 725.
MAURICE A. BRINDISI, Primary Examiner.
Claims (1)
- 4. THE PROCESS OF PREPARING CESIUM COMPOUNDS WHICH COMPRISES TREATING CESIUM ALUM WITH CALCIUM HYDROXIDE IN AN AQUEOUS MEDIUM, THE CALCIUM HYDROXIDE BEING EMPLOYED IN AN AMOUNT SUFFICIENT TO STOICHIOMETRICALLY CONVERT SUBSTANTIALLY ALL OF THE CESIUM ALUM TO A MIXTURE CONTAINING A SOLUTION OF CESIUM SULFATE, INSOLUBLE ALUMINUM HDROXIDE AND INSOLUBLE CALCIUM SULFATE, SAID SOLUTION CONSISTING ESSENTIALLY OF WATER AND CESIUM SULFATE, TREATING SAID CESIUM SULFATE SOLUTION WITH BARIUM HYDROXIDE TO FORM AN AQUEOUS MIXTURE CONTAINING SOLUBLE CESIUM HYDROXIDE AND INSOLUBLE BARIUM SULFATE, SAID CESIUM HYDROXIDE BEING DISSOLVED IN AN SOLUTION CONSISTING ESSENTIALLY OF WATER AND CESIUM HYDROXIDE, AND CARBONATING THE AQUEOUS SOLUTION OF CESIUM HYDROXIDE TO FORM A SOLUTION CONSISTING ESSENTIALY OF WATER AND SOLUBLE CESIUM CARBONATE.
Priority Applications (1)
| Application Number | Priority Date | Filing Date | Title |
|---|---|---|---|
| US185833A US3207571A (en) | 1962-04-09 | 1962-04-09 | Process for preparing cesium compounds from cesium alum |
Applications Claiming Priority (1)
| Application Number | Priority Date | Filing Date | Title |
|---|---|---|---|
| US185833A US3207571A (en) | 1962-04-09 | 1962-04-09 | Process for preparing cesium compounds from cesium alum |
Publications (1)
| Publication Number | Publication Date |
|---|---|
| US3207571A true US3207571A (en) | 1965-09-21 |
Family
ID=22682629
Family Applications (1)
| Application Number | Title | Priority Date | Filing Date |
|---|---|---|---|
| US185833A Expired - Lifetime US3207571A (en) | 1962-04-09 | 1962-04-09 | Process for preparing cesium compounds from cesium alum |
Country Status (1)
| Country | Link |
|---|---|
| US (1) | US3207571A (en) |
Cited By (19)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| US3489509A (en) * | 1967-05-18 | 1970-01-13 | Kewanee Oil Co | Process for recovery of cesium compounds of high purity |
| US4447406A (en) * | 1983-07-12 | 1984-05-08 | Carus Corporation | Process for recovering cesium from cesium ore |
| US4466950A (en) * | 1983-07-12 | 1984-08-21 | Carus Corporation | Process for recovering cesium from cesium alum |
| US4469670A (en) * | 1983-07-12 | 1984-09-04 | Carus Corporation | Process for recovering cesium from cesium alum |
| USRE32556E (en) * | 1983-07-12 | 1987-12-08 | Process for recovering cesium from cesium alum | |
| US4938934A (en) * | 1989-05-16 | 1990-07-03 | Carus Corporation | Recovery of cesium chloride from pollucite ore |
| DE4313480C1 (en) * | 1993-04-24 | 1994-04-14 | Metallgesellschaft Ag | Prepn. of water-soluble caesium salt from caesium-aluminium alum - by reaction with calcium hydroxide and soluble calcium salt in amts. equimolar to aluminium and caesium in water, without adding barium cpd. |
| WO1994011303A1 (en) * | 1992-11-11 | 1994-05-26 | Metallgesellschaft Aktiengesellschaft | Process for producing a high-density caesium and rubidium salt solution |
| WO1995013986A1 (en) * | 1993-11-16 | 1995-05-26 | Metallgesellschaft Aktiengesellschaft | Method of preparing a caesium and rubidium salt solution |
| WO1996031435A1 (en) * | 1995-04-06 | 1996-10-10 | Cabot Corporation | Process for the production of cesium compounds |
| US6015535A (en) * | 1995-04-06 | 2000-01-18 | Cabot Corporation | Process for producing purified cesium compound from cesium alum |
| WO2002079089A1 (en) * | 2001-04-02 | 2002-10-10 | Cabot Corporation | Methods of making cesium salts and other alkali metal salts |
| WO2004106564A2 (en) * | 2003-05-23 | 2004-12-09 | Cabot Corporation | Method for recovering at least one metallic element like cesium from ore |
| WO2006079514A1 (en) * | 2005-01-27 | 2006-08-03 | Chemetall Gmbh | Methods for producing cesium hydroxide solutions |
| US20060239900A1 (en) * | 2005-04-20 | 2006-10-26 | Cabot Corporation | Methods of forming an alkali metal salt |
| CN101774613B (en) * | 2010-02-04 | 2011-11-30 | 江西东鹏新材料有限责任公司 | Novel technology of producing cesium carbonate by pollucite |
| WO2015084416A1 (en) * | 2013-12-03 | 2015-06-11 | Cabot Corporation | Methods to recover cesium formate from a mixed alkali metal formate blend |
| EP2075066B1 (en) | 2007-12-10 | 2016-08-17 | Honeywell International Inc. | Method for making catalyst compositions of alkali metal halide-doped bivalent metal fluorides and a process for making fluorinated olefins |
| US20190048437A1 (en) * | 2016-01-29 | 2019-02-14 | Cascadero Copper Corporation | Recovery of cesium from epithermal mineral deposits |
Citations (8)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| US513001A (en) * | 1894-01-16 | Process of making alkali salts | ||
| US1948887A (en) * | 1932-04-22 | 1934-02-27 | Louise D Sanders | Method of manufacturing alumina |
| US1951443A (en) * | 1932-04-22 | 1934-03-20 | Louise D Sanders | Method of manufacturing alumina hydrate and valuable sulphates from compounds of alumina |
| US2021988A (en) * | 1934-01-20 | 1935-11-26 | Grasselli Chemical Co | Production of lithium compounds |
| US2516109A (en) * | 1948-09-16 | 1950-07-25 | Metalloy Corp | Method of extracting lithium values from spodumene ores |
| US3000699A (en) * | 1957-10-18 | 1961-09-19 | Pechiney Prod Chimiques Sa | Purifying lithium salts |
| CA629452A (en) * | 1961-10-17 | Muller Jurgen | Process for the decomposition of pollucite for recovery of caesium values therefrom | |
| US3099527A (en) * | 1959-04-23 | 1963-07-30 | Basic Atomics Inc | Purification of leach liquor containing lithium values |
-
1962
- 1962-04-09 US US185833A patent/US3207571A/en not_active Expired - Lifetime
Patent Citations (8)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| US513001A (en) * | 1894-01-16 | Process of making alkali salts | ||
| CA629452A (en) * | 1961-10-17 | Muller Jurgen | Process for the decomposition of pollucite for recovery of caesium values therefrom | |
| US1948887A (en) * | 1932-04-22 | 1934-02-27 | Louise D Sanders | Method of manufacturing alumina |
| US1951443A (en) * | 1932-04-22 | 1934-03-20 | Louise D Sanders | Method of manufacturing alumina hydrate and valuable sulphates from compounds of alumina |
| US2021988A (en) * | 1934-01-20 | 1935-11-26 | Grasselli Chemical Co | Production of lithium compounds |
| US2516109A (en) * | 1948-09-16 | 1950-07-25 | Metalloy Corp | Method of extracting lithium values from spodumene ores |
| US3000699A (en) * | 1957-10-18 | 1961-09-19 | Pechiney Prod Chimiques Sa | Purifying lithium salts |
| US3099527A (en) * | 1959-04-23 | 1963-07-30 | Basic Atomics Inc | Purification of leach liquor containing lithium values |
Cited By (47)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| US3489509A (en) * | 1967-05-18 | 1970-01-13 | Kewanee Oil Co | Process for recovery of cesium compounds of high purity |
| US4447406A (en) * | 1983-07-12 | 1984-05-08 | Carus Corporation | Process for recovering cesium from cesium ore |
| US4466950A (en) * | 1983-07-12 | 1984-08-21 | Carus Corporation | Process for recovering cesium from cesium alum |
| US4469670A (en) * | 1983-07-12 | 1984-09-04 | Carus Corporation | Process for recovering cesium from cesium alum |
| EP0132656A2 (en) * | 1983-07-12 | 1985-02-13 | Carus Corporation | Process for recovering cesium from cesium alum |
| EP0132656A3 (en) * | 1983-07-12 | 1985-04-17 | Carus Corporation | Process for recovering cesium from cesium alum |
| USRE32556E (en) * | 1983-07-12 | 1987-12-08 | Process for recovering cesium from cesium alum | |
| US4938934A (en) * | 1989-05-16 | 1990-07-03 | Carus Corporation | Recovery of cesium chloride from pollucite ore |
| AU669770B2 (en) * | 1992-11-11 | 1996-06-20 | Chemetall Gmbh | Production of high-density caesium and rubidium salt solution |
| WO1994011303A1 (en) * | 1992-11-11 | 1994-05-26 | Metallgesellschaft Aktiengesellschaft | Process for producing a high-density caesium and rubidium salt solution |
| US5593650A (en) * | 1992-11-11 | 1997-01-14 | Metallgesellschaft Aktiengesellschaft | Method for producing a high-density saline cesium and rubidium solution |
| WO1994025422A1 (en) * | 1993-04-24 | 1994-11-10 | Metallgesellschaft Aktiengesellschaft | Method of preparing caesium salts from caesium aluminium alum |
| DE4313480C1 (en) * | 1993-04-24 | 1994-04-14 | Metallgesellschaft Ag | Prepn. of water-soluble caesium salt from caesium-aluminium alum - by reaction with calcium hydroxide and soluble calcium salt in amts. equimolar to aluminium and caesium in water, without adding barium cpd. |
| US5605669A (en) * | 1993-04-24 | 1997-02-25 | Metallgesellschaft Aktiengesellschaft | Process of preparing cesium salts from cesium aluminum alum |
| AU679528B2 (en) * | 1993-04-24 | 1997-07-03 | Chemetall Gmbh | Method of preparing caesium salts from caesium aluminium alum |
| US5900221A (en) * | 1993-11-16 | 1999-05-04 | Metallgesellschaft Aktiengesellschaft | Process of preparing a solution of cesium and rubidium salts |
| WO1995013986A1 (en) * | 1993-11-16 | 1995-05-26 | Metallgesellschaft Aktiengesellschaft | Method of preparing a caesium and rubidium salt solution |
| AU691206B2 (en) * | 1993-11-16 | 1998-05-14 | Chemetall Gmbh | Method of preparing a caesium and rubidium salt solution |
| WO1996031435A1 (en) * | 1995-04-06 | 1996-10-10 | Cabot Corporation | Process for the production of cesium compounds |
| AU709994B2 (en) * | 1995-04-06 | 1999-09-09 | Cabot Corporation | Process for the production of cesium compounds |
| US6015535A (en) * | 1995-04-06 | 2000-01-18 | Cabot Corporation | Process for producing purified cesium compound from cesium alum |
| US6436879B1 (en) | 1995-04-06 | 2002-08-20 | Cabot Corporation | Process for producing a predetermined cesium compound |
| EP1254942A3 (en) * | 1995-04-06 | 2011-07-27 | Cabot Corporation | Drilling fluid containing caesium compounds |
| EP1254942A2 (en) * | 1995-04-06 | 2002-11-06 | Cabot Corporation | Drilling fluid containing caesium compounds |
| CN1106345C (en) * | 1995-04-06 | 2003-04-23 | 卡伯特公司 | Production of cesium compounds |
| WO2002079089A1 (en) * | 2001-04-02 | 2002-10-10 | Cabot Corporation | Methods of making cesium salts and other alkali metal salts |
| US6652820B2 (en) | 2001-04-02 | 2003-11-25 | Cabot Corporation | Methods of making cesium salts and other alkali metal salts |
| NO343675B1 (en) * | 2001-04-02 | 2019-05-06 | Cabot Corp | Processes for the preparation of cesium salt |
| US20040253157A1 (en) * | 2003-05-23 | 2004-12-16 | Bakke Bart F. | Methods for recovering at least one metallic element from ore |
| WO2004106564A3 (en) * | 2003-05-23 | 2005-05-19 | Cabot Corp | Method for recovering at least one metallic element like cesium from ore |
| WO2004106564A2 (en) * | 2003-05-23 | 2004-12-09 | Cabot Corporation | Method for recovering at least one metallic element like cesium from ore |
| US7323150B2 (en) | 2003-05-23 | 2008-01-29 | Cabot Corporation | Methods for recovering at least one metallic element from ore |
| NO339341B1 (en) * | 2003-05-23 | 2016-11-28 | Cabot Corp | Process for the recovery of cesium and / or rubidium. |
| US20080166281A1 (en) * | 2005-01-27 | 2008-07-10 | Harms Gerd J | Methods for Producing Cesium Hydroxide Solutions |
| JP2008528422A (en) * | 2005-01-27 | 2008-07-31 | ヒェメタル ゲゼルシャフト ミット ベシュレンクテル ハフツング | Method for producing cesium hydroxide solution |
| WO2006079514A1 (en) * | 2005-01-27 | 2006-08-03 | Chemetall Gmbh | Methods for producing cesium hydroxide solutions |
| US20060239900A1 (en) * | 2005-04-20 | 2006-10-26 | Cabot Corporation | Methods of forming an alkali metal salt |
| EP2075066B1 (en) | 2007-12-10 | 2016-08-17 | Honeywell International Inc. | Method for making catalyst compositions of alkali metal halide-doped bivalent metal fluorides and a process for making fluorinated olefins |
| CN101774613B (en) * | 2010-02-04 | 2011-11-30 | 江西东鹏新材料有限责任公司 | Novel technology of producing cesium carbonate by pollucite |
| WO2015084416A1 (en) * | 2013-12-03 | 2015-06-11 | Cabot Corporation | Methods to recover cesium formate from a mixed alkali metal formate blend |
| US9452966B2 (en) | 2013-12-03 | 2016-09-27 | Cabot Corporation | Methods to recover cesium formate from a mixed alkali metal formate blend |
| US20160355406A1 (en) * | 2013-12-03 | 2016-12-08 | Cabot Corporation | Methods To Recover Cesium Formate From A Mixed Alkali Metal Formate Blend |
| US9573821B2 (en) * | 2013-12-03 | 2017-02-21 | Cabot Corporation | Methods to recover cesium formate from a mixed alkali metal formate blend |
| CN105960444B (en) * | 2013-12-03 | 2018-12-11 | 卡博特公司 | The method for collecting cesium formate from mixed alkali metal formates blend |
| CN105960444A (en) * | 2013-12-03 | 2016-09-21 | 卡博特公司 | Methods to recover cesium formate from a mixed alkali metal formate blend |
| US20190048437A1 (en) * | 2016-01-29 | 2019-02-14 | Cascadero Copper Corporation | Recovery of cesium from epithermal mineral deposits |
| US10738370B2 (en) * | 2016-01-29 | 2020-08-11 | Cascadero Copper Corporation | Recovery of cesium from epithermal mineral deposits |
Similar Documents
| Publication | Publication Date | Title |
|---|---|---|
| US3207571A (en) | Process for preparing cesium compounds from cesium alum | |
| US4119698A (en) | Reclamation treatment of red mud | |
| US3780158A (en) | Process for recovering high purity free flowing crystalline manganese dioxide from impure manganese nitrate solutions | |
| CA1066025A (en) | Method of treating alunite ore | |
| US3489509A (en) | Process for recovery of cesium compounds of high purity | |
| US1792410A (en) | Max btjchnee | |
| US2354133A (en) | Process for producing alumina from clay | |
| US1956139A (en) | Process for treating argillaceous material | |
| US3112171A (en) | Lithium carbonate production | |
| US3383166A (en) | Process for producing iron-free aluminum nitrate solutions | |
| US2467271A (en) | Process for production of ammonium alum from acid liquors | |
| US4366129A (en) | Process for producing alumina and ferric oxide from aluminium carriers with high iron and silicon content | |
| US4100264A (en) | Process for the preparation of calcium carbonate for use in fluorescent lamp phosphors | |
| US4195070A (en) | Preparation of a MgCl2 solution for Nalco's MgCl2 process from MgSO4 and other MgSO4 salts | |
| US2384009A (en) | Process for recovering magnesium salts | |
| JPS58151303A (en) | Manufacture of calcium hypochlorite | |
| US2862788A (en) | Process for purifying impure solid-phase kainite | |
| US2758912A (en) | Process for producing a substantially sulfate-free and potassium-free magnesium chloride solution | |
| US3111376A (en) | Production of magnesium hydroxide | |
| US2940820A (en) | Process for recovering alkali metal values from lepidolite | |
| US1389862A (en) | Manufacture of potassium sulfate | |
| US3547579A (en) | Removal of sulfates from brines | |
| US3314747A (en) | Recovery of chromate from chrome mud wastes | |
| US2531182A (en) | Process for the manufacture of boric acid | |
| US2924507A (en) | Process for recovering lithium values |
