USH59H - Process for converting magnesium fluoride to calcium fluoride - Google Patents
Process for converting magnesium fluoride to calcium fluoride Download PDFInfo
- Publication number
- USH59H USH59H US06/685,100 US68510084A USH59H US H59 H USH59 H US H59H US 68510084 A US68510084 A US 68510084A US H59 H USH59 H US H59H
- Authority
- US
- United States
- Prior art keywords
- caf
- calcium
- fluoride
- mgf
- magnesium fluoride
- Prior art date
- Legal status (The legal status is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the status listed.)
- Abandoned
Links
Classifications
-
- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01F—COMPOUNDS OF THE METALS BERYLLIUM, MAGNESIUM, ALUMINIUM, CALCIUM, STRONTIUM, BARIUM, RADIUM, THORIUM, OR OF THE RARE-EARTH METALS
- C01F11/00—Compounds of calcium, strontium, or barium
- C01F11/20—Halides
- C01F11/22—Fluorides
Definitions
- the invention relates generally to a process for converting magnesium fluoride (MgF 2 ) to a useable product and more specifically to the conversion of MgF 2 to calcium fluoride (CaF 2 ) using calcium hydroxide (Ca(OH) 2 ), calcium oxide (CaO) or calcium carbonate (CaCO 3 ) and is a result of a contract with the United States Department of Energy.
- MgF 2 magnesium fluoride
- CaF 2 calcium fluoride
- CaO calcium oxide
- CaCO 3 calcium carbonate
- MgF 2 slag In the reduction of uranium tetrafluoride to uranium metal with magnesium for use at various DOE facilities, large quantities of MgF 2 slag are produced.
- this magnesium fluoride is processed through one of two routes depending on whether it contains enriched or depleted uranium. If the slag is produced from reduction of enriched uranium it is processed by leaching with nitric acid for uranium solubilization and recovery. The uranium barren slag is neutralized with lime, filtered, placed in drums and eventually dried for long term storage. Some of the magnesium fluoride, from both depleted and enriched uranium, is recycled as liner material for future reductions.
- the process is generally the conversion of MgF 2 to CaF 2 by mixing either CaO, Ca(OH) 2 , or CaCO 3 with MgF 2 and heating the mixture to at least 1,600° F. for not less than two hours.
- the reactions that take place are:
- the solid by-product, MgO, is removed from CaF 2 using an acid leach and filtration to separate the solution from the solid CaF 2 .
- This CaF 2 cake is dried to provide CaF 2 powder.
- the other by-products, CO 2 and H 2 O, are gases and naturally depart as such. Since HNO 3 , HCl, H 2 SO 4 or any organic acid will work for the acid leach, the preferred acid depends on economic considerations and the by-products desired.
- This method of converting MgF 2 to CaF 2 is advantageous because the resulting CaF 2 is useful in the manufacture of anhydrous HF whereas MgF 2 is of no known commercial use.
- the invention is a process whereby MgF 2 , particularly MgF 2 slag formed in the reduction of UF 4 with Mg, is converted to CaF 2 using either CaO, Ca(OH) 2 or CaCO 3 .
- the three compounds were tested, each giving especially satisfactory results yielding better than 90% conversion from MgF 2 slag, so the choice of the calcium compound is discretionary.
- the MgF 2 slag containing small amounts of uranium (2-2.5%), magnesium oxide (1-1.5%), and water (0.1-0.5%) is milled to increase its surface area and mixed with either calcium oxide, calcium hydroxide or calcium carbonate using stoichiometric amounts or slight excesses of the calcium containing compounds.
- This mixture is placed in a furnace and heated to at least 1,600° F. for two hours or more to form CaF 2 and the by-products. After the reaction is complete the by-products are separated from the CaF 2 by leaching with an acid solution.
- Sufficient acid must be used for stoichiometric reaction with the MgO and uranium which is present.
- the acid can be HCl, HNO 3 , H 2 SO 4 or any organic acid.
- the chosen acid must be dilute enough to keep the resulting magnesium salts in solution. In tests, a 7-8 N HNO 3 solution was used with excellent results.
- the acid solution containing the by-products is filtered from the solid CaF 2 leaving a CaF 2 cake that contains approximately 50% water.
- the cake is dried with heat, yielding a product of better than 90% CaF 2 .
- the impurities are MgF 2 and less than 500 ppm uranium.
- the CaF 2 produced is of sufficient purity to be used in the industrial manufacture of anhydrous HF. This is a considerable advantage since the MgF 2 from which it is made has no use and creates a significant disposal or storage problems.
- the by-product MgO can be converted to Mg metal, however, known processes are not economically feasible under present industrial conditions. Although incomplete, procedures are being developed to convert the MgO to magnesium metal which could be used or perhaps sold, thus eliminating the burdensome storage problem.
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- Chemical & Material Sciences (AREA)
- Organic Chemistry (AREA)
- Life Sciences & Earth Sciences (AREA)
- Geology (AREA)
- Inorganic Chemistry (AREA)
- Compounds Of Alkaline-Earth Elements, Aluminum Or Rare-Earth Metals (AREA)
Abstract
This invention is a process for the conversion of magnesium fluoride to calcium fluoride whereby magnesium fluoride is decomposed by heating in the presence of calcium carbonate, calcium oxide or calcium hydroxide. Magnesium fluoride is a by-product of the reduction of uranium tetrafluoride to form uranium metal and has no known commercial use thus its production creates a significant storage problem. The advantage of this invention is that the quality of calcium fluoride produced is sufficient to be used in the industrial manufacture of anhydrous hydrogen fluoride, steel mill flux or ceramic applications.
Description
The invention relates generally to a process for converting magnesium fluoride (MgF2) to a useable product and more specifically to the conversion of MgF2 to calcium fluoride (CaF2) using calcium hydroxide (Ca(OH)2), calcium oxide (CaO) or calcium carbonate (CaCO3) and is a result of a contract with the United States Department of Energy.
In the reduction of uranium tetrafluoride to uranium metal with magnesium for use at various DOE facilities, large quantities of MgF2 slag are produced. Presently this magnesium fluoride is processed through one of two routes depending on whether it contains enriched or depleted uranium. If the slag is produced from reduction of enriched uranium it is processed by leaching with nitric acid for uranium solubilization and recovery. The uranium barren slag is neutralized with lime, filtered, placed in drums and eventually dried for long term storage. Some of the magnesium fluoride, from both depleted and enriched uranium, is recycled as liner material for future reductions. The slag from depleted uranium production, when not recycled, is placed in below ground pit storage, but the procedure of burying materials can threaten underground water sources. It is preferred to minimize the amount of slag requiring storage, therefore a project was begun to develop a process converting the magnesium fluoride slag to usable, recyclable and possibly saleable material.
An attempt was made to use the MgF2 to make anhydrous hydrogen fluoride (HF) but the reaction proved to be very slow and incomplete and resulted in a need for storage of voluminous quantities of magnesium sulfate contaminated with residual uranium. Since anhydrous HF is usually made from CaF2, investigation were begun to study the possibility of converting MgF2 to CaF2 but the literature was not encouraging, Mellor's A Comprehensive Treatise on Inorganic and Theoretical Chemistry specifically states that CaO does not react with MgF2 ; that MgF2 is decomposed by alkali carbonates, not mentioning alkaline earth carbonates (such as CaCO3); and is silent on the use of Ca(OH)2 in such a process. Nevertheless work was begun to see if MgF2 would be decomposed using CaO, CaCO3 or Ca(OH)2.
In view of the above-mentioned need, it is an object of this invention to provide a process for the conversion of MgF2 to CaF2.
It is another object of this invention to solve the problem of storage of large quantities of MgF2.
It is further object of this invention to convert MgF2 to a useable substance.
Additional objects, advantages and novel features of the invention will be set forth in part in the description that follows, and in part will become apparent to those skilled in the art upon examination or may be learned by practice of the invention. The objects and advantages of the invention may be realized and attained by means of instrumentalities and combinations particularly pointed out in the appended claims.
To achieve the foregoing and other objects, the process is generally the conversion of MgF2 to CaF2 by mixing either CaO, Ca(OH)2, or CaCO3 with MgF2 and heating the mixture to at least 1,600° F. for not less than two hours. The reactions that take place are:
MgF.sub.2 (solid)+CaO(solid)→CaF.sub.2 (solid)+MgO(solid)
MgF.sub.2 (solid)+Ca(OH).sub.2 (solid)→CaF.sub.2 (solid)+MgO(solid)+H.sub.2 O(gas)
MgF.sub.2 (solid)+CaCO.sub.3 (solid)→CaF.sub.2 (solid)+MgO(solid)+CO.sub.2 (gas)
The solid by-product, MgO, is removed from CaF2 using an acid leach and filtration to separate the solution from the solid CaF2. This CaF2 cake is dried to provide CaF2 powder. The other by-products, CO2 and H2 O, are gases and naturally depart as such. Since HNO3, HCl, H2 SO4 or any organic acid will work for the acid leach, the preferred acid depends on economic considerations and the by-products desired.
This method of converting MgF2 to CaF2 is advantageous because the resulting CaF2 is useful in the manufacture of anhydrous HF whereas MgF2 is of no known commercial use.
The invention is a process whereby MgF2, particularly MgF2 slag formed in the reduction of UF4 with Mg, is converted to CaF2 using either CaO, Ca(OH)2 or CaCO3. The three compounds were tested, each giving especially satisfactory results yielding better than 90% conversion from MgF2 slag, so the choice of the calcium compound is discretionary.
The MgF2 slag containing small amounts of uranium (2-2.5%), magnesium oxide (1-1.5%), and water (0.1-0.5%) is milled to increase its surface area and mixed with either calcium oxide, calcium hydroxide or calcium carbonate using stoichiometric amounts or slight excesses of the calcium containing compounds. This mixture is placed in a furnace and heated to at least 1,600° F. for two hours or more to form CaF2 and the by-products. After the reaction is complete the by-products are separated from the CaF2 by leaching with an acid solution. Sufficient acid must be used for stoichiometric reaction with the MgO and uranium which is present. The acid can be HCl, HNO3, H2 SO4 or any organic acid. The chosen acid must be dilute enough to keep the resulting magnesium salts in solution. In tests, a 7-8 N HNO3 solution was used with excellent results.
The acid solution containing the by-products is filtered from the solid CaF2 leaving a CaF2 cake that contains approximately 50% water. The cake is dried with heat, yielding a product of better than 90% CaF2. The impurities are MgF2 and less than 500 ppm uranium.
Since the literature stated that treatment of MgF2 with CaO would not yield CaF2 and also suggested that using CaCO3 and Ca(OH)2 would be unsuccessful, it was surprising that all three gave such impressive results.
The CaF2 produced is of sufficient purity to be used in the industrial manufacture of anhydrous HF. This is a considerable advantage since the MgF2 from which it is made has no use and creates a significant disposal or storage problems. The by-product MgO can be converted to Mg metal, however, known processes are not economically feasible under present industrial conditions. Although incomplete, procedures are being developed to convert the MgO to magnesium metal which could be used or perhaps sold, thus eliminating the burdensome storage problem.
The foregoing description of a preferred embodiment has been presented to explain the invention and enable others skilled in the art to best utilize it in a particular application. Obviously, many modifications are possible and one versed in the art will be able to determine the most suitable process conditions for any given set of circumstance without resorting to undue experimentation.
Claims (2)
1. A process for the conversion of MgF2 to CaF2 comprising:
mixing MgF2 with a stoichiometric amount or slight excess of a calcium-containing compound selected from the group CaO, Ca(OH)2, and CaCO3 ;
heating said mixture to 1,600° F. or higher for two hours or longer to convert said magnesium fluoride and said calcium-containing compound to CaF2 and by-products;
leaching said CaF2 and said by-products with an acid solution of sufficient concentration to dissolve said by-products;
removing said acid and by-product solution from said CaF2 resulting in wet CaF2 that contains approximately 50% water; and
drying said wet CaF2 to produce CaF2.
2. The process of claim 1 wherein said acid is selected from the group HNO3, HCl, H2 SO4 and all organic acids.
Priority Applications (1)
| Application Number | Priority Date | Filing Date | Title |
|---|---|---|---|
| US06/685,100 USH59H (en) | 1984-12-21 | 1984-12-21 | Process for converting magnesium fluoride to calcium fluoride |
Applications Claiming Priority (1)
| Application Number | Priority Date | Filing Date | Title |
|---|---|---|---|
| US06/685,100 USH59H (en) | 1984-12-21 | 1984-12-21 | Process for converting magnesium fluoride to calcium fluoride |
Publications (1)
| Publication Number | Publication Date |
|---|---|
| USH59H true USH59H (en) | 1986-05-06 |
Family
ID=24750777
Family Applications (1)
| Application Number | Title | Priority Date | Filing Date |
|---|---|---|---|
| US06/685,100 Abandoned USH59H (en) | 1984-12-21 | 1984-12-21 | Process for converting magnesium fluoride to calcium fluoride |
Country Status (1)
| Country | Link |
|---|---|
| US (1) | USH59H (en) |
Cited By (4)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| US5207999A (en) * | 1991-08-13 | 1993-05-04 | Cameco Corporation | Generation of fluorine via thermal plasma decomposition of metal fluoride |
| US5516496A (en) * | 1995-06-01 | 1996-05-14 | Advanced Recovery Systems, Inc. | Metal and fluorine values recovery from fluoride salt matrices |
| WO1996038380A1 (en) * | 1995-06-01 | 1996-12-05 | Advanced Recovery Systems, Incorporated | Metal and fluorine values recovery from fluoride salt matrices |
| US5851500A (en) * | 1997-08-22 | 1998-12-22 | United States Enrichment Corporation | Removal of uranium contamination from magnesium fluoride slag |
-
1984
- 1984-12-21 US US06/685,100 patent/USH59H/en not_active Abandoned
Non-Patent Citations (2)
| Title |
|---|
| D.F. Othmer et al., "Metal Ordering by Choline Affinity for Oxides", Metallurgical Society of AIME Light Metals Committee Proceedings of the Sessions, vol. 1, 1973, pp. 271-298. |
| L. F. Grantham, R. L. Gay, D. E. McKenzie, The Decontamination of Magnesium Fluoride Waste From Uranium Production: Process Evaluation and Preliminary Economics, Apr. 30, 1985, prepared for U.S. Department of Energy under contract DE-AT03-835F11948 by Rockwell International. |
Cited By (6)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| US5207999A (en) * | 1991-08-13 | 1993-05-04 | Cameco Corporation | Generation of fluorine via thermal plasma decomposition of metal fluoride |
| US5516496A (en) * | 1995-06-01 | 1996-05-14 | Advanced Recovery Systems, Inc. | Metal and fluorine values recovery from fluoride salt matrices |
| WO1996038380A1 (en) * | 1995-06-01 | 1996-12-05 | Advanced Recovery Systems, Incorporated | Metal and fluorine values recovery from fluoride salt matrices |
| US5881359A (en) * | 1995-06-01 | 1999-03-09 | Advanced Recovery Systems, Inc. | Metal and fluorine values recovery from fluoride salt matrices |
| US5851500A (en) * | 1997-08-22 | 1998-12-22 | United States Enrichment Corporation | Removal of uranium contamination from magnesium fluoride slag |
| FR2767520A1 (en) * | 1997-08-22 | 1999-02-26 | Us Enrichment Corp | PROCESS FOR THE TREATMENT OF A MAGNESIUM FLUORIDE DAIRY CONTAMINATED WITH URANIUM |
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