CA1042629A - Recovery of gallium oxide from solutions - Google Patents
Recovery of gallium oxide from solutionsInfo
- Publication number
- CA1042629A CA1042629A CA216,510A CA216510A CA1042629A CA 1042629 A CA1042629 A CA 1042629A CA 216510 A CA216510 A CA 216510A CA 1042629 A CA1042629 A CA 1042629A
- Authority
- CA
- Canada
- Prior art keywords
- solution
- gallium
- gallium oxide
- sodium aluminate
- alumina
- 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
Links
Classifications
-
- Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
- Y02—TECHNOLOGIES OR APPLICATIONS FOR MITIGATION OR ADAPTATION AGAINST CLIMATE CHANGE
- Y02P—CLIMATE CHANGE MITIGATION TECHNOLOGIES IN THE PRODUCTION OR PROCESSING OF GOODS
- Y02P20/00—Technologies relating to chemical industry
- Y02P20/141—Feedstock
Landscapes
- Compounds Of Alkaline-Earth Elements, Aluminum Or Rare-Earth Metals (AREA)
Abstract
ABSTRACT OF THE DISCLOSURE
Method for recovery of gallium from sodium aluminate solutions by co-precipitation of alumina and gallium oxide, followed by introducing sodium aluminate into the resultant solution to co-precipitate further alumina and gallium oxide.
The specification discloses a process in which carbon dioxide is fed into gallium-containing sodium aluminate solutions in sufficient amount to co-precipitate alumina and part of the gallium as gallium oxide and form sodium bicarbonate in the solutions, after which sodium aluminate is fed into the resultant solution, whereby further alumina and gallium oxide are co-precipitated from the solution. The respective degrees to which dissolved gallium is precipitated by gassing the solution with carbon dioxide, and by adding sodium aluminate to the gassed solution, as described above, ordinarily depends on the relative economy of those respective procedures in the recovery of gallium oxide. Normally, it is economically feasible to precipitate the major portion of the gallium by gassing the solution with carbon dioxide and forming at least 90 grams per liter of sodium bicarbonate in the solution, prior to adding sodium aluminate to recover further gallium oxide from the solution.
Method for recovery of gallium from sodium aluminate solutions by co-precipitation of alumina and gallium oxide, followed by introducing sodium aluminate into the resultant solution to co-precipitate further alumina and gallium oxide.
The specification discloses a process in which carbon dioxide is fed into gallium-containing sodium aluminate solutions in sufficient amount to co-precipitate alumina and part of the gallium as gallium oxide and form sodium bicarbonate in the solutions, after which sodium aluminate is fed into the resultant solution, whereby further alumina and gallium oxide are co-precipitated from the solution. The respective degrees to which dissolved gallium is precipitated by gassing the solution with carbon dioxide, and by adding sodium aluminate to the gassed solution, as described above, ordinarily depends on the relative economy of those respective procedures in the recovery of gallium oxide. Normally, it is economically feasible to precipitate the major portion of the gallium by gassing the solution with carbon dioxide and forming at least 90 grams per liter of sodium bicarbonate in the solution, prior to adding sodium aluminate to recover further gallium oxide from the solution.
Description
1~42629 ~his invention relates to the recovery of gallium fr.om sodium aluminate solutions.
. ~ ., - - .
In the well known Bayer process for the recovery of alumina from aluminas;, such as bauxite, by digesting the ore in hot caustic soda solution to form a sodium aluminate solution, followed by precipitation of alumina hydrate from the solution and recycling the resultant caustic soda-con-taining "spent liquor" to digest further bauxite, gallium values in the ore are dissolved and accumulate in the solution in repeated digests until an equilibrium is reached, usually at about 0.1-0.2 grams of gallium per liter of solution.
- Also, sodium aluminate solutions containing a low concentration of dissolved gallium can be produced by digesting in hot caustic soda solution of gallium-containing anode alloy from the well known 3-layer process for the purification of aluminium.
U.S. patents 2,574,008 and 2,~82,376 disclose recovering gallium values from sodium aluminate solutions by co-~recip-itating gallium oxide and alumina by feeding carbon dioxide into the solution, after preliminarily precipitating alumina and thercby decreasing the ratio of alumina to gallium in the solution, In effecting co-~recipitation of gallium oxide and alùmina in that manner, especially when the co-precipitation is accomplished slowly from solutions containing low concen-trations of yallium, it is uneconomical to recover all of the 1~4Z6Z9 gallium from the solution, despite feeding enough carbon dioxide that the solution contains a substantial proportion of sodium bicarbonate. Such unprecipitated gallium represents an economic loss.
It is an object of this invention to provide an economical and convenient process for precipitating further gallium oxide following co-precipitation of alumina and gallium oxide from sodium aluminate solutions by introducing carbon dioxide into the solution.
In accordance with the invention, carbon dioxide is fed into gallium-containing sodium aluminate solutions in sufficient amount to co-precipitate alumina and part of the gallium as gallium oxide and form sodium bicarbQnate in the solutions, after which sodium aluminate is fed into the resultant solution, whereby further alumina and gallium oxide are co-precipitated from the solution. The respective degrees to which dissolved gallium is precipitated by gassing the solution with carbon dioxide, and by adding sodium aluminate to the gassed solution, as described above, ordinarily depends on the relative economy of those respective procedures in the recovery of gallium oxide. Normally, it is economically feasible to precipitate the major portion of the gallium by gassing the solution with carbon dioxide and forming at least 90 grams per liter of sodium bicarbonate in the solution, prior to adding sodium aluminate to recover further gallium oxide from the solution.
In carrying out the abovementioned procedure of co-precipitating alumina and gallium oxide by adding sodium aluminate to the solution, the sodium aluminate employed may be either in solid form or in solution, but preferably in the foxm of a solution. The amount of sodium aluminate added depend~ on ~uch factors as the amount of gallium oxide to be 1~426Z9 precipitated, and the proportion of the dissolved gallium present which it is desired to precipitate.
Circulating the co-~recipitated alumina and gallium oxide through the solution for an extended time by agitation of the solution and precipitate is effective in promoting precipitation of additional gallium oxide, and whether that procedure is to be used is also a factor to take into consideration in determining the amount of sodium aluminate to be added to the solution. Such agitation can be effected by well-known means for stirring slurries.
The following example illustrates the practice of the invention:
Carbon dioxide was fed into a solution containing 4.6 grams per liter of alumina, 12.7 grams per liter of total caustic and 0.169 grams per liter of dissolved gallium, such gassing ~eing continued over a period of 21 hours, by which time sufficient alumina and gallium oxide had been co-precipi-tated that the resultant solution contained only 0.091 grams per liter of dissolved gallium, and less than 0.02 grams per liter of alumina, together with 88.7 grams per liter of sodium bicarbonate. Thereafter a portion of the solution, designated Portion A, was stirred continuously for 48 hours.
Sodium aluminate solution was fed into a second portion (designated Portion B) of the solution resulting from the abovementioned gassing step, in sufficient amount to add
. ~ ., - - .
In the well known Bayer process for the recovery of alumina from aluminas;, such as bauxite, by digesting the ore in hot caustic soda solution to form a sodium aluminate solution, followed by precipitation of alumina hydrate from the solution and recycling the resultant caustic soda-con-taining "spent liquor" to digest further bauxite, gallium values in the ore are dissolved and accumulate in the solution in repeated digests until an equilibrium is reached, usually at about 0.1-0.2 grams of gallium per liter of solution.
- Also, sodium aluminate solutions containing a low concentration of dissolved gallium can be produced by digesting in hot caustic soda solution of gallium-containing anode alloy from the well known 3-layer process for the purification of aluminium.
U.S. patents 2,574,008 and 2,~82,376 disclose recovering gallium values from sodium aluminate solutions by co-~recip-itating gallium oxide and alumina by feeding carbon dioxide into the solution, after preliminarily precipitating alumina and thercby decreasing the ratio of alumina to gallium in the solution, In effecting co-~recipitation of gallium oxide and alùmina in that manner, especially when the co-precipitation is accomplished slowly from solutions containing low concen-trations of yallium, it is uneconomical to recover all of the 1~4Z6Z9 gallium from the solution, despite feeding enough carbon dioxide that the solution contains a substantial proportion of sodium bicarbonate. Such unprecipitated gallium represents an economic loss.
It is an object of this invention to provide an economical and convenient process for precipitating further gallium oxide following co-precipitation of alumina and gallium oxide from sodium aluminate solutions by introducing carbon dioxide into the solution.
In accordance with the invention, carbon dioxide is fed into gallium-containing sodium aluminate solutions in sufficient amount to co-precipitate alumina and part of the gallium as gallium oxide and form sodium bicarbQnate in the solutions, after which sodium aluminate is fed into the resultant solution, whereby further alumina and gallium oxide are co-precipitated from the solution. The respective degrees to which dissolved gallium is precipitated by gassing the solution with carbon dioxide, and by adding sodium aluminate to the gassed solution, as described above, ordinarily depends on the relative economy of those respective procedures in the recovery of gallium oxide. Normally, it is economically feasible to precipitate the major portion of the gallium by gassing the solution with carbon dioxide and forming at least 90 grams per liter of sodium bicarbonate in the solution, prior to adding sodium aluminate to recover further gallium oxide from the solution.
In carrying out the abovementioned procedure of co-precipitating alumina and gallium oxide by adding sodium aluminate to the solution, the sodium aluminate employed may be either in solid form or in solution, but preferably in the foxm of a solution. The amount of sodium aluminate added depend~ on ~uch factors as the amount of gallium oxide to be 1~426Z9 precipitated, and the proportion of the dissolved gallium present which it is desired to precipitate.
Circulating the co-~recipitated alumina and gallium oxide through the solution for an extended time by agitation of the solution and precipitate is effective in promoting precipitation of additional gallium oxide, and whether that procedure is to be used is also a factor to take into consideration in determining the amount of sodium aluminate to be added to the solution. Such agitation can be effected by well-known means for stirring slurries.
The following example illustrates the practice of the invention:
Carbon dioxide was fed into a solution containing 4.6 grams per liter of alumina, 12.7 grams per liter of total caustic and 0.169 grams per liter of dissolved gallium, such gassing ~eing continued over a period of 21 hours, by which time sufficient alumina and gallium oxide had been co-precipi-tated that the resultant solution contained only 0.091 grams per liter of dissolved gallium, and less than 0.02 grams per liter of alumina, together with 88.7 grams per liter of sodium bicarbonate. Thereafter a portion of the solution, designated Portion A, was stirred continuously for 48 hours.
Sodium aluminate solution was fed into a second portion (designated Portion B) of the solution resulting from the abovementioned gassing step, in sufficient amount to add
2.5 grams per liter of alumina to the solution, and the slurry was stirred continuously for 48 hours at the same rate as was employed in stirring Portion A. At the end of 16 hours alumina and gallium oxide had precipitated from both portions A and B, but in the case o~ Portion A the solution still contained 0.073 gram~ per liter of dissolved gallium, whereas, Porti~n B contained only 0.~04 grams per liter of dissolved gal~ium. 4
Claims
1. The method of precipitating gallium oxide from sodium aluminate solutions containing dissolved gallium, comprising feeding into the solution sufficient carbon dioxide to co-precipitate alumina and part of the gallium oxide from the solution and produce sodium bi-carbonate in the solution, and thereafter co-precipitating further alumina and gallium oxide from the resultant solution by feeding sodium aluminate into that solution.
Priority Applications (1)
Application Number | Priority Date | Filing Date | Title |
---|---|---|---|
CA216,510A CA1042629A (en) | 1974-12-20 | 1974-12-20 | Recovery of gallium oxide from solutions |
Applications Claiming Priority (1)
Application Number | Priority Date | Filing Date | Title |
---|---|---|---|
CA216,510A CA1042629A (en) | 1974-12-20 | 1974-12-20 | Recovery of gallium oxide from solutions |
Publications (1)
Publication Number | Publication Date |
---|---|
CA1042629A true CA1042629A (en) | 1978-11-21 |
Family
ID=4101908
Family Applications (1)
Application Number | Title | Priority Date | Filing Date |
---|---|---|---|
CA216,510A Expired CA1042629A (en) | 1974-12-20 | 1974-12-20 | Recovery of gallium oxide from solutions |
Country Status (1)
Country | Link |
---|---|
CA (1) | CA1042629A (en) |
-
1974
- 1974-12-20 CA CA216,510A patent/CA1042629A/en not_active Expired
Similar Documents
Publication | Publication Date | Title |
---|---|---|
JP4895454B2 (en) | Nickel-containing laterite ore leaching method | |
EP0547744A1 (en) | Process for recovering metal from oxide ores | |
US4097575A (en) | Roast-neutralization-leach technique for the treatment of laterite ore | |
US4489043A (en) | Manufacture of manganous sulfate solutions | |
JPS5983933A (en) | Manufacture of alumina from aluminum-containing ore | |
NZ200320A (en) | Reducing iron content of aluminous material by leaching with hydrochloric acid | |
EP0028638B1 (en) | Method for producing cobalt metal powder | |
US4395278A (en) | Method for producing cobalt metal powder | |
US3933976A (en) | Nickel-cobalt separation | |
US2728636A (en) | Separation of nickel and cobalt | |
US3383166A (en) | Process for producing iron-free aluminum nitrate solutions | |
CA1042629A (en) | Recovery of gallium oxide from solutions | |
US4071422A (en) | Process for concentrating and recovering gallium | |
US4329169A (en) | Method for producing cobalt metal powder | |
US4804407A (en) | Method for recovering cobalt from hexammine cobaltic (111) solutions | |
US2867503A (en) | Cobalt and nickel recovery using carbon dioxide leach | |
US3751558A (en) | Process of separating cobalt from nickel by means of ammonia | |
US4612039A (en) | Production of pure cobalt metal powder | |
JPH09143589A (en) | Method for concentrating, separating and recovering rare earth metal | |
US3796789A (en) | Removal of iron from sodium aluminate liquor | |
US4594230A (en) | Recovery of cobalt | |
Scott | Alumina by acid extraction | |
US3856920A (en) | Recovery of gallium oxide from solutions | |
US4091071A (en) | Process for digesting goethite-containing bauxites according to the Bayer technology | |
US4743347A (en) | Production of pure MgCl2 solution suitable for the production of magnesium metal from an impure magnesite ore or concentrate |