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Publication numberUS1371741 A
Publication typeGrant
Publication dateMar 15, 1921
Filing dateMar 20, 1914
Priority dateMar 20, 1914
Publication numberUS 1371741 A, US 1371741A, US-A-1371741, US1371741 A, US1371741A
InventorsDietsche Otto
Original AssigneeSiemens & Co Geb
Export CitationBiBTeX, EndNote, RefMan
External Links: USPTO, USPTO Assignment, Espacenet
Process of manufacturing compounds of metals of the rare earths
US 1371741 A
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Description  (OCR text may contain errors)




1,371,741. No Drawing. Application filed March 20, 1914,

Specification of Letters Patent.

Patented Mar. 15, 1921.

T 0 all whom it may concern:

Be it known that I, O'r'ro DIETSCHE, a German citizen, and resident of Berlin- Lichtenberg, Germany, have invented certain new and useful Improvements in Processes of Manufacturing Compounds of Met: als of the Rare Earths, of whichthe following is a specification. 7

The present invention relates to the production of compounds of the rare earth metals and more especially to a method for producing such compounds from solutions containing a rare earth metal.

The invention is based upon the fact hitherto unknown that those mineral con taining salts of the metals of the alkali metal group (and also the alkaline earth metals and aluminum) which are little or not at all soluble in water, will, upon being added to a hot solution of a rare earth metal, precipitate the rare earth metal from such solution.

Besides those minerals which contain the ordinary insoluble or little soluble salts of calcium. strontium, barium, or aluminum also thosewhich contain the insoluble complex salts of the alkali metals proper, such as titano potassium fluorid, boro potassium fluorid, silico potassium fiuorid, may be used. The use of natural fluorids in general, but also of natural phosphates and tungstates is advantageous, and special ad vantages are obtained if finely comminuted natural minerals such a fluor-spar or apatite are employed as precipitating agents. According to whether a fluorid, a phosphate or a tungstate be present in the mineral used for precipitating, the respective rare earth metal is obtained under the form of a fiuorid, phosphate, or tungstate, the respectiv salt settling down very quickly as a homogeneous precipitate which can be easily treated further.

The solution of the rare earth metals may contain the chlorid or any other soluble salt of the metal, and it is possible according to v the present invention, to precipitate the salts from waste liquors resulting for instance in the manufacture of thorium or from decomposed monazite sand or from cerite solutions. 7

An addition of some suitable mineral acid,

such as hydrochloric acid, will prove advantageous in many cases, especialy so when fluor-spar is used as a precipitant, inasmuch as the reaction is expedited thereby.

Instead of the fluorids the double fluorids of the rare earth metal and of the precipitating agent may be produced, such double the difference in the respective specific weights. Moreover the compound obtained is absolutely insoluble in acid. By causing a solution of rare earth metals to act upon such double fluorid it may be decomposed, the single fluorids of the rare earth metals being then formed.

- It has been ascertained further that the tendency to form double fluorids is especially great in the presence of an acid of the oxalic acid series such as for instance oxalic acid, the acid having either been added by design or being present as an impurity. In

this ase the rare earth metal solution may either be mixed with the oxalic acid and fluor-spar and the mixture then heated, or else the metal-solution and the acid may be allowed to react with each other, oxalates of the metals being formed, and fluor-spar added afterward. Of oxalic acid not more than about 5'per cent. of the quantity of rare earth metals contained in the solution need be used.

The principal advantage offered by the method according to the present invention, as compared with the older methods practised up to this day lies in the very favorable qualities owned by the precipitates thus obtained.

Heretofore the rare earth metal solutions were precipitated as a rule withacids or easily soluble salts of an alkali, such as hydrofluoric acid or sodium fluorid. 'The precipitates thus obtained, however, are in a state of extremely fine division and settle down very slowly, thus offering great difliculties with regard to purification. This is probably due to the fact that the finely d1- vided precipitate contains besides rare earth metal fluorids, also double fluorids of a rare earth metal and an alkali. However thls may be, thedeposit will retain most tenaciously the alkali compound serving as a precipitating agent as well as all other 1mpurities. In contradistinction thereto the precipitate obtained with fiuor-s ar and with other compounds of the alkaline earth metals including magnesium andaluminum settles down'ver quickly and allows of being purified with the greatest ease. Moreover the danger connected with the use of hydrofluoric acid both as regards the operators and the apparatus used is totally avoided. The precipitate obtained according to the new method offers the further advantage of not sintering when being calcined, in contradistinction to the products obtained with hydrofluoric acid. or alkali metal fluorids. This is of the greatest importance in thecase where the product must be heated-in order to increase its density, such as in themanufacture of luminous admixtures for are light electrodes; The product obtained" according to the present invention, upon being strongly heated, gets denser without however forming solid stone-like masses, and need not, therefore, be ground. A quantitative output is obtained and there are no losses caused by complicated washing operations, as in the former methods. p

- The double fluorids obtained in accordance with the'method described above are coarsely Igrained and can be washed out easily. owever, if it is desired to obtain the ordinary fluorids, the solution of' rare earths containing the double fluorids need only be heated, thus yielding the simple fluoridsin the form of a grained substance, unlike the amorphous powder obtained after the old methods.

In practising my invention'I may for instance proceed as follows E ma/mple I 7.5 kgs.

precipitate formed is washed with water,

filtered and dried. 12.1 kgs. of dry fluorid are obtained, this being 96 per cent. of the theoretical quantity.

Example I].

To 100 kgs. of a neutral solution of rare earth metals, saidsolution containing 10.5 per cent. of metallic oxids, 10 kgs. of cal.- cium phosphate are added, the solution being heated and stirred all the while. After a few minutes the reaction will be completed; the rare earth metal phosphates are deposited asheavy flakes and can easily be washed. The quantative output of 15 kgs. is obtained. I

' Example I I I quantity.

' Example 1 V.

13.5 kgs. of rare earth metal oxide of the greatestpossible purity are dissolved in the least possible-quantity of hydrochloric acid or nitric acid, water being added .to make it 100 kgs. To this slightly acid solution l kg. of a saturated oxalic acid solution is added. A light precipitate will form, but be dissolved again upon the solution being heated. As soon as the boiling point is reached, 9.6 kgs. fluor-spar are added and boiling is proceeded with for about two hours. 15.6 kgs. of dry fluorid, equal to 96 per cent. of the theoretical quantity are obtained. I

In the same manner freshly precipitated pure oxalates of the rare earth metals can be made to react with the required quantit of fluor-spar in the presence of some aci It is true that in this case the reaction will take some more time but the fluorids of the rare earth metals are of better quality and more coarse-grained. I

I The. term alkali group .used in the claims shall include, besides the alkali metals proper, the alkaline earth metals, and


The term not easily soluble as used in the claims is meant to comprise little soluble as well-as practically insoluble salts.

I claim 1. The process which consists in causing a dissolved rare earth metal compound to react with a mineral containinga not easily soluble fluorid of a metal of the alkali group.

2. The process which consists in causing a dissolved rare earth metal compound to react easily soluble salt of a metal of the alkali group in the presence of an acid of the oxalic acid series.

4. The process which consists in causinga dissolved rare earth metal compound to react with. a mineral containing a fluorid of a metal of the alkali group and interrupting the reaction at the point where a double salt ofthe rare earths and the precipitating medium has formed. 7 5. The process which consists in causing a dissolved rare earth metal compound to react with a mineral containing a not easily s0luble fluorid of a metal :of the alkali group and interrupting the reaction at the point where a double fiuorid of the rare earths and the precipitating medium has formed.

In witness whereof I have hereunto set my signature in the presence of two subscribing witnesses.




Referenced by
Citing PatentFiling datePublication dateApplicantTitle
US2425573 *Nov 12, 1941Aug 12, 1947Frederick SoddySeparation of thorium and the rareearth group from minerals
US3049403 *Aug 25, 1958Aug 14, 1962Pawel KrumholzProcess for precipitating readily filterable rare earth hydroxides
US4769353 *Nov 4, 1986Sep 6, 1988General Electric CompanyClosed pore, polycrystalline
US5732367 *Jun 14, 1996Mar 24, 1998Sevenson Environmental Services, Inc.Reduction of leachability and solubility of radionuclides and radioactive substances in contaminated soils and materials
US5994608 *Oct 17, 1997Nov 30, 1999Sevenson Environmental Services, Inc.Reduction of leachability and solubility of radionuclides and radioactive substances in contaminated soils and materials
US6291736 *Oct 25, 1999Sep 18, 2001Sevenson Environmental Services, Inc.Contacting material with phosphoric acid to produce a mixture; curing mixture; wherein concentration of leachable radioactive substances in material so treated is decreased and non-leachable solid materials are formed
US6635796Jul 9, 2001Oct 21, 2003Sevenson Environmental Services, Inc.By converting to low-temperature phosphatic apatite type that are insoluble, nonleachable, nonzeolitic and pH stable, by contacting with a halide, sulfate, hydroxide, or silicate source and phosphate ion
U.S. Classification423/263, 423/600, 423/304, 423/491, 423/594.15, 423/472
International ClassificationC01F17/00
Cooperative ClassificationC01F17/0062, C01F17/0031
European ClassificationC01F17/00D5, C01F17/00J2