14 ABSTRACTS OF OHEMICAL PAPERS, In o r g a n i c C h e m i s t r y , Properties of Liquid Chlorine. By R. KNIETSCH ( ~ n n a l e n , 253, 10U-l.L4).--l'he author has made a series of determinatims of the vapour teiisiori of ch1or;ne from -888" to 146", and of its specific gravity a t tempeiatures ranging from -80" to 77'; the result8 ale given i n tables wild as ciii-ves, and the methods and apparatus employed ale fully described with the aid of various diagrams. 1 he critical tempel ature of chlorine was found to be 146'. F. 8. K. Simple rhd Rapid Evolutron of Pure Gases. By H. HORN- WAGER (Ztit. unitl. C h w i . , 20, 412; see Absfr,, 1890, 849).--l'heINORGANIC CHEMISTRY. 15 productibn of chlorine from a mixture of blenching powder and sodium hrdrogen sulphate was patented by 0, Stuber, on April 5th, 1890.M. J. S. Atomic Weight of Fluorine. By H. MOISSAN (COn7pt. rend., 111, 570-572) .-Sodium carbonate, prepared hy the ammonia process fram carefully purified sadium chloride, was converted into fluoride bg the action of hydrofluoric acid from potassium hydrogen fluoride. The sodium fluoride was tlien converted into sulphate. The results of five determinations varied between 1' = 19.04 and F t 19.08 (Na = 23'05, S = 38.014, arid 0 = 16). Calcium fluoride, obtained in ti crystalline form by adding calcium chloride to a boiling dilute solution (0.2 per cent.) of potassium fluoride, was likowiae converted into sulphate ; P = 19'02 to 19.08. Barium fluoride, obtained by adding potassiuni fluoride to a boiling solution a€ barium chloride, wits treated in the same way; F = The actior, of sulphuric acid on barium fluoride is more difficult to regulate than in the first two cases, and the author regards these re- hults as less trustworthy, Taking the mean of the results with sodiunl and calcium fluorides, P I 19.05.19'05-19 09, C. H, B. Solubility of Oxygen and Hydrogen in Water and in Aloohol. By W. TIMOF~EFF (Zeit. physikal. Chem., 6 , 141-152). - The author, in his investigation, ernplcys an apparatus devised by Ostwald. It consists of an absorption-chamber which is simply a p;pette provided a t one end with a stopc.ock and a t the other with three-wuy tap, by means of which communication can be effected chither with the air or, throuqh a leaden capillary, with a gas burette. The pipette is filled completely with the boiled-out solvent, and a quantity of the gas to be dissolved is introduced into the gas burette and there measured.Coniriiuriicatioti is then made between the two vessels ; a weighed or measured amount o€ water is run out through the stopcock, which is then closed, and the absorber immersed in a vessel of water a t the requisite temperature, From time to time the absorber is taken out of the bath and shaken as vigorously as the flexibility of the lead tube will permit, Mercury is filled into the gas burette as required, in order that the pressure may remain ag nearly that of the atmosphere a8 po~sible. W heu no more absorption takes place, pressure and temperature are adjusted, and a fresh measurement made. The absorption coefficient of hydrogen in water as determined in the ahove way may be expressed by the formula U = 0.0215286 - 0~00019216S + 0.000001722-t2.Bunsen found = 0 4 1 9 ~ 0 with no temperature coefficient. For oxygen in water, the author obt&ns /j 3; OQ41408 at 6.4", and /I = 0.03(jQll a t 12.6", numbers which agree well with W inklcr's results. The values for hydrogen in alcohol a1-e fairly concordant with those of CRI~~US, /j a t 0" being 00676 (mean of two experinients). An iriterpolatiun formula for the absorp- t ~ o n coefficient of uxygen in alcohol of 99.7 per cent. strength is Q =E 0.235'7 - 0*00074,83t + O4U0O093288t2, The solubility of nitro-7G ABSTRACTS OF CRICMICAL PAPERS. Fen, oxygen, carbon monoxide, and methane in water increases about 80 per cent.between 0" a,nd 20" ; the increase in alcohol is much lgss. Hydrogen Nitride (Azoimide). By T. CURTIUS (Bey.., 23, J . W. 3023-2033). See p. 56. Catalytic Decomposition of Ammonium Nitrite. By 0, LOEW (Bey-., 23, 3018-3019). -On adding platinum black, prcpared in the manner described in a previous paper (Abstr., 1890. 453), to ;t 4 to 5 per ceut. solution of ammonium nitrite, an immediate evolution of gas takes place. The first portion consists of a mixture of nitrogen and nitrous oxide, but after a time nitrogen is tlie sole product. No noticeable alteration in the temperature of t8he sol ation occurs. J. B. T. Absorption of Carbonic Oxide by Earth. By BERTHELOT ((lontyt. r e d . , 111, 469--471).-The volume of carbonic oxide re- tained by air-dried clay soil is equal to the volume of air which i t (*an retain, and hence the retention of carbonic oxide by the eartti, after an explosion i n a mine, for example, is riot due to any specific ;tct,ion between the soil and the gas.C. H. B. Double Chloride and Dithionate of Barium. By A. F o c ~ and K. Kr,Css (Ber., 23, 3001--3003).-Wben equivalent cluantities of barium dithiouate, 13aS,0G + 2H20, and barium chloride, BaClz + 2 H r 0 , are mixed in aqueous solution. and the latter allowed to evapo- rate, barium dithionnte first separates, tben, after a time, the double salt, BaS,O,.BaCI, + 4H20, and finally barium chloride. The above double salt forms short, colourless prisms, which hare been obtained 7 mm. in length and 5.5 mm. i n thickness. and belong t o the asym- metric system (u : 7) : c = 0.6720 : 1 : 0.6398; a: = 107" 12', p = 98" ll', y = 90" 57' 30").H. G. C. Action of Hydrogen on Potassium Thallium Sulphide. By R. SCHNEIDER ( J . y7-. Chern. [el, 42, 305-327).-When the author first published his work on thio-salts (Ann,. Phys. Chew., 136, 138, 139), he showed that when potassium thallium sulpliide is heated in llydrogen it is decomposed with formation of hydrogen sulphide, potassium sulphide, and thallium sulphide. Kriiss and Solereder (Abstr., 1887, 1111, on the contrary, assert that the thallium is re- duced to the inetallic state, the potassium remaining a s sulphide. The author has reinvestigated the subject, and his experiments show that the decomposition takes place in t w o stages, according to 1,he temperature ; a t a dark-red heat, it is in accordance w i t h the equation which the author first gave, namely :- K,S,TI,S, +- 4H = 2H,S + K28 + T'1,S; at a prolonged, full, red heat, however, a part of the thallium is re- duced t o the metallic state according to the eqiistion B[K,S,Tl,S,] + 10H = 5HLS + 2&S + TIZS + TI, ;INORGANIC CHEMISTRY.17 hut at, no kemrerature at which the author has been able to obtaiil quantitative results is the whole of the thallium so reduced. Kruss ant1 Schmidt also assert (loc. c i f . ) that the salt of a thio-acid can be reduced by hydrogen when the thio-acid itself can be so re- duced. But ihis is not the case with sodium thioantinionate or Schlippe's salt and potassium indium sulphide, which cannoi; be re- duced by hydroeen notwithstanding t h a t both antimony and indium stilphides are easily reduced.Compare also the behaviour of potaG- si u m pl tl tino thiop 1 atinat e, K4Pt S4, and potassium pall ad ot h iopalladsi te, K,PdS, (this Jouriml, 1871, 317). The specific gravity of potassium thallium sulpliide has been reclc- termined ; it now stands a t 4.60. A . G. B. Researches on the Gadolinium of Marignac. By L. DE Bors- BAUDRAN C'or~ipt. rend., 111, 393-395). - Mariqnac's gadolinia (Abstr., 1869, 4:)6) was fractionated with dilute ammonia. T tie absorption spectra showed that there was a concentration of' samarium in the head fritctions and of didymiurn in the tail. On the other liand, the fluorescence Zp is much stronger in the head fractioiix, whilst the samarium fluorescence is ieeble in these fraction<, and i s not visible in the others. The spark spectrurn shows that all the fractions conhain gadoliniutn.Cleve finds that the greater part of gadolinia cannot be split up by ft.actionat,ion. The impurities, which atme difficult to eliminate, dis- tribute themselves unequally in the different fractions, without, how- ewr, materially affecting the equivalent of the oxide. The author obseived a remarkable terriporury solubility of the oxides of the rare earths in ammonium acettate solution containiug excess of ammoriiw. A solution of gadolitiium chloride, eqtiivslent to 0.5 gram of the oxide per litre, when mixed with acetic acid arid after- n.;rrds with ammonia in excess, remained transparent for a long time, but gradually became turbid, and precipitation was practically coni- ~!lete after a day or two. Heat accelerates precipitat'ion, but makes it iticomplete.Analogous phenomena are observed w i t h lanthat~um, 1-ttrium, and diclymium, especially the first, arid in a lower degreo with cerous chloride. c. H. B. Equivalent of Terbia. By L. DE ROISBAUDRAN (Compt. rend., 111, $74--475).-h previous determinations of the equivalent of the earth Zp (terbia with a v w y deep-Ilrown colonr), the quaiitity of oxygen existing in the earth in the form of peroxide, was uiicerhin. The author has repeated the determinations by the same method, that k, weighing the quantity of the sulpliate formed by a given quantity of oxide, b u t the oxide was previously calcined a t a white heat, and the small quantity of peroxide present was determined.The coloni- of the calcined oxide was much paler, although still very yellow ; i t contaitied 0.16 per cent. of oxygeii as peroxide. The mean equivalent of tbe terbia, is 122.32, which gives 159.48 for the atomic weight of the metal. C. H. U. YCL. LS. C18 ABSTRACTS OF CHEMICAL PAPERS. Ammonium Fluoroxymolybdates. By F. MACRO (Gazxettrr,, 20, 109-121~- Hexagonal ammonium j?uoroxym olyhdate, 3MoOzF,,5NH4F + HzO, prepared by dissolving the laminar fluoroxymolpbdate (Ahstr., 1889,106), or the compound Mo03,2NH4F, in hydrofluoric acid, crpstal- lises in minute, hexagonal prisms, which resenible those of the double salts of molybdenum and niobium of the type 3MnOF3,5NH4F + H,O, and are probably isomorphous with the crystals of hexagonal ammonium flnoroxyhyponioljbdate.The crystals are colourless and t,ransparent at first, but become opaque after prolonged exposure to the air ; they are not dehydrated by heating at 100" ; they dissolve in water, forming an acid solution, which loses hydrogen fluoride on heating, and if the temperature exceeds loo", ammonia is also evolved. Monamnioniurn Jluoroxymolybdate. Mo02F2,NH4F, is obtained in monoclinic crystals on allowing a solution of the preceding compound in hydrofluoric acid to evaporate over sulphuric acid ; a : b : c = 0.63019 : 1 : 1.42549, p = 85" 53'. Fa,ces observed: 010, 001, 110, 111, 337, 335, 667. Plane of twinning (307). The crystals, which are generally twinned, are colourless and transparent, but darken and timi green after st short exposure to the air ; they dissolve in water, yielding an acid solution.T'he crystals may be heated t o 120" without losiiig weight, but decom- pose at a higher temperikture. Delafontaine's acid fluoyomolybdate of ammonium appears t o be identical with the aut8hor's triammonium fluoroxpmolybdate, MoOzF2,3NH4F, and is not isomorphoils with the acid fluoroxytnng- state. S. B. A. A. Double Salts of Tungstic and Vanadic Acids. By F. ROTHEN- BACH (Ber., 23, 3050-3060).-0n adding sodium paraiunpstate to hydrated vanadic anhydride, sodium paratungsto-vanadate is formed, together with a cornpound which crystallises in dark-red octahedra, and has the formula 3(Naz0,4W0,),N~,0,3Vz05 + 38H20. The following salts were prepared from sodium paratungsto- vanadate by double decomposition :- The ammonium salt crystallises in orange-red octahedra of the formula 5 [ 5(NH4),0, 12 W 0 3 1 2 [ 7Vz05,3 (NH&O] + 58Hz0.The bariu,m salt is deposited in light, orange-coloured crystals, which are very sparingly soluble, and have t'he formula 3( 5Ba0,12WO3),2(5VZO5,2BaO) + 94Hzo. From the mother liquors cubical crystals are obtained, which contain sodium chloride, barium tungstate, and bariixm vanadate. The strontium salt crystztllises in orange-red cubes, 3(5Sr0,12WO3),2(5VZO5,2Sr0) + 12dHz0, and resembles the barium compound. The potassiicm salt crystallises iu aggregates of large, light orange-red plates, which have not get been analysed. By the action of magnesium sulphate on sodium para- tungstovanadate, a, componnd of the formula 5NaZ0,12W O3,3V,O5,MgO,N a,O + 42HzoINORGANIC CHEMISTRY.19 i s formed. crystallising in pale orange-yellow prisms. A similay com- pound is deposited from the mother liquors in lustrous, light orange- coloured plates. With sodium tungstovanadate, aluminiuiri sulphate gives a compound of the formula crystallising in dark garnet-red cubes. No coppr salt could be ob- tained. The water of crystallisation i n the above compounds was deter- mined by cautious ignition. The variadic acid and fiungstic acid were precipitated together by means of mercuric nitrate and mercuric oxide. The vanadic acid was determined separately by reduction and titration with potassium permanganate, and also by boiling with phosphoric acid, potassium bromide, and hydrochloric acid ; the bromine which is evolved is absorbed in potassium iodide solution, and the liberated iodine estimated in the usual manner.Bismuth Oxyiodide. By C. ASTRE (J. Pharm,. [ 5 ] , 22,193-200). -Various published methods for the preparation of this oxyiodide yielded products more or less contaminated with sub-nitrahe, with oxide, or with both these compounds. To obtain the pure product, 10 grams of bismuth potassium iodide is decomposed by the addition of 4 litres of water, and the product is washed until iodine is no l o n p r removed. The resulting compound contained Bi, 59.38, and 1, 36-30 per cent. The double iodide employed is best, obtained by triturat- ing normal bismuth nitrate (1 mol.) with potassium iodide (4 mols.), and 50 C.C. of water (sic), extracting with ethyl acetate, and sub- mitting the mixture to spontaneous evaporation.3(Al,0,,9Na,0,48W0~3) ,4( 9V205,A1,0,) + 504H20, J. B. T. J. T. Platinum Thiocarbide. By P. SCHUTZEKBERGER (Compt. ?-end., 1117391-393).-A current of nitrogen or hydrogen charged with the vapour of carbon bisulphide is passed over spongy platinum heated at 400-450”, and when the absorption of t,he bisulphide ceases, the somewhat finely divided black product is allowed to cool, and is powdered and submitted to the same treatment again. The product is a dense, black powder of the composition Pt,CS2. Under a micro- scope, it seems homogeneous, and it cannot be separated into different components by levigation. I t is not attacked by boiling concentrated nitric or hydrochloric acid, and is almost entirely unaffected by warm aqua regia.It is, therefore, not a mixture of platinum sulphide wit,h carbon, and it probably has the constitution S:Pt:C:Pt:S. When heated below redness iir dry oxygen, i t burns with incandescence, atrid yields carbonic anhydride. sulphuric anhydride, sulphurous anhydride, and a, residue of pnre platinum. The formation of this compound may be used f o r the separation, and even the estimation, of carbon bisulphide in any mixture of gases which is free from oxygen. The gaseous mixture is passed over the heated spongy platinum, and the product is afterwards heated in oxygen, the gases formed being absorbed in some oxidising liquid, and the sulphuric acid estimated in the usual way. C. H. l3. c 214 ABSTRACTS OF OHEMICAL PAPERS,In o r g a n i c C h e m i s t r y ,Properties of Liquid Chlorine.By R. KNIETSCH ( ~ n n a l e n ,253, 10U-l.L4).--l'he author has made a series of determinatims ofthe vapour teiisiori of ch1or;ne from -888" to 146", and of its specificgravity a t tempeiatures ranging from -80" to 77'; the result8 alegiven i n tables wild as ciii-ves, and the methods and apparatus employedale fully described with the aid of various diagrams.1 he critical tempel ature of chlorine was found to be 146'.F. 8. K.Simple rhd Rapid Evolutron of Pure Gases. By H. HORN-WAGER (Ztit. unitl. C h w i . , 20, 412; see Absfr,, 1890, 849).--l'hINORGANIC CHEMISTRY. 15productibn of chlorine from a mixture of blenching powder and sodiumhrdrogen sulphate was patented by 0, Stuber, on April 5th, 1890.M.J. S.Atomic Weight of Fluorine. By H. MOISSAN (COn7pt. rend., 111,570-572) .-Sodium carbonate, prepared hy the ammonia processfram carefully purified sadium chloride, was converted into fluoridebg the action of hydrofluoric acid from potassium hydrogen fluoride.The sodium fluoride was tlien converted into sulphate. The resultsof five determinations varied between 1' = 19.04 and F t 19.08(Na = 23'05, S = 38.014, arid 0 = 16).Calcium fluoride, obtained in ti crystalline form by adding calciumchloride to a boiling dilute solution (0.2 per cent.) of potassiumfluoride, was likowiae converted into sulphate ; P = 19'02 to 19.08.Barium fluoride, obtained by adding potassiuni fluoride to a boilingsolution a€ barium chloride, wits treated in the same way; F =The actior, of sulphuric acid on barium fluoride is more difficult toregulate than in the first two cases, and the author regards these re-hults as less trustworthy, Taking the mean of the results with sodiunland calcium fluorides, P I 19.05.19'05-19 09,C.H, B.Solubility of Oxygen and Hydrogen in Water and inAloohol. By W. TIMOF~EFF (Zeit. physikal. Chem., 6 , 141-152). -The author, in his investigation, ernplcys an apparatus devised byOstwald. It consists of an absorption-chamber which is simply ap;pette provided a t one end with a stopc.ock and a t the other withthree-wuy tap, by means of which communication can be effectedchither with the air or, throuqh a leaden capillary, with a gas burette.The pipette is filled completely with the boiled-out solvent, and aquantity of the gas to be dissolved is introduced into the gas buretteand there measured.Coniriiuriicatioti is then made between the twovessels ; a weighed or measured amount o€ water is run out throughthe stopcock, which is then closed, and the absorber immersedin a vessel of water a t the requisite temperature, From time to timethe absorber is taken out of the bath and shaken as vigorously asthe flexibility of the lead tube will permit, Mercury is filled into thegas burette as required, in order that the pressure may remain agnearly that of the atmosphere a8 po~sible. W heu no more absorptiontakes place, pressure and temperature are adjusted, and a freshmeasurement made.The absorption coefficient of hydrogen in water as determined inthe ahove way may be expressed by the formula U = 0.0215286 -0~00019216S + 0.000001722-t2. Bunsen found = 0 4 1 9 ~ 0 with notemperature coefficient.For oxygen in water, the author obt&ns/j 3; OQ41408 at 6.4", and /I = 0.03(jQll a t 12.6", numbers whichagree well with W inklcr's results. The values for hydrogen in alcohola1-e fairly concordant with those of CRI~~US, /j a t 0" being 00676(mean of two experinients). An iriterpolatiun formula for the absorp-t ~ o n coefficient of uxygen in alcohol of 99.7 per cent. strength isQ =E 0.235'7 - 0*00074,83t + O4U0O093288t2, The solubility of nitro7G ABSTRACTS OF CRICMICAL PAPERS.Fen, oxygen, carbon monoxide, and methane in water increases about80 per cent.between 0" a,nd 20" ; the increase in alcohol is much lgss.Hydrogen Nitride (Azoimide). By T. CURTIUS (Bey.., 23,J . W.3023-2033). See p. 56.Catalytic Decomposition of Ammonium Nitrite. By 0,LOEW (Bey-., 23, 3018-3019). -On adding platinum black, prcparedin the manner described in a previous paper (Abstr., 1890. 453), to ;t4 to 5 per ceut. solution of ammonium nitrite, an immediate evolutionof gas takes place. The first portion consists of a mixture of nitrogenand nitrous oxide, but after a time nitrogen is tlie sole product. Nonoticeable alteration in the temperature of t8he sol ation occurs.J. B. T.Absorption of Carbonic Oxide by Earth. By BERTHELOT((lontyt. r e d . , 111, 469--471).-The volume of carbonic oxide re-tained by air-dried clay soil is equal to the volume of air which i t(*an retain, and hence the retention of carbonic oxide by the eartti,after an explosion i n a mine, for example, is riot due to any specific;tct,ion between the soil and the gas.C. H. B.Double Chloride and Dithionate of Barium. By A. F o c ~and K. Kr,Css (Ber., 23, 3001--3003).-Wben equivalent cluantitiesof barium dithiouate, 13aS,0G + 2H20, and barium chloride, BaClz +2 H r 0 , are mixed in aqueous solution. and the latter allowed to evapo-rate, barium dithionnte first separates, tben, after a time, the doublesalt, BaS,O,.BaCI, + 4H20, and finally barium chloride. The abovedouble salt forms short, colourless prisms, which hare been obtained7 mm. in length and 5.5 mm.i n thickness. and belong t o the asym-metric system (u : 7) : c = 0.6720 : 1 : 0.6398; a: = 107" 12', p =98" ll', y = 90" 57' 30"). H. G. C.Action of Hydrogen on Potassium Thallium Sulphide. ByR. SCHNEIDER ( J . y7-. Chern. [el, 42, 305-327).-When the authorfirst published his work on thio-salts (Ann,. Phys. Chew., 136, 138,139), he showed that when potassium thallium sulpliide is heated inllydrogen it is decomposed with formation of hydrogen sulphide,potassium sulphide, and thallium sulphide. Kriiss and Solereder(Abstr., 1887, 1111, on the contrary, assert that the thallium is re-duced to the inetallic state, the potassium remaining a s sulphide.The author has reinvestigated the subject, and his experiments showthat the decomposition takes place in t w o stages, according to 1,hetemperature ; a t a dark-red heat, it is in accordance w i t h the equationwhich the author first gave, namely :-K,S,TI,S, +- 4H = 2H,S + K28 + T'1,S;at a prolonged, full, red heat, however, a part of the thallium is re-duced t o the metallic state according to the eqiistionB[K,S,Tl,S,] + 10H = 5HLS + 2&S + TIZS + TI, INORGANIC CHEMISTRY.17hut at, no kemrerature at which the author has been able to obtaiilquantitative results is the whole of the thallium so reduced.Kruss ant1 Schmidt also assert (loc. c i f . ) that the salt of a thio-acidcan be reduced by hydrogen when the thio-acid itself can be so re-duced. But ihis is not the case with sodium thioantinionate orSchlippe's salt and potassium indium sulphide, which cannoi; be re-duced by hydroeen notwithstanding t h a t both antimony and indiumstilphides are easily reduced.Compare also the behaviour of potaG-si u m pl tl tino thiop 1 atinat e, K4Pt S4, and potassium pall ad ot h iopalladsi te,K,PdS, (this Jouriml, 1871, 317).The specific gravity of potassium thallium sulpliide has been reclc-termined ; it now stands a t 4.60. A . G. B.Researches on the Gadolinium of Marignac. By L. DE Bors-BAUDRAN C'or~ipt. rend., 111, 393-395). - Mariqnac's gadolinia(Abstr., 1869, 4:)6) was fractionated with dilute ammonia. T tieabsorption spectra showed that there was a concentration of' samariumin the head fritctions and of didymiurn in the tail. On the otherliand, the fluorescence Zp is much stronger in the head fractioiix,whilst the samarium fluorescence is ieeble in these fraction<, and i snot visible in the others.The spark spectrurn shows that all thefractions conhain gadoliniutn.Cleve finds that the greater part of gadolinia cannot be split up byft.actionat,ion. The impurities, which atme difficult to eliminate, dis-tribute themselves unequally in the different fractions, without, how-ewr, materially affecting the equivalent of the oxide.The author obseived a remarkable terriporury solubility of theoxides of the rare earths in ammonium acettate solution containiugexcess of ammoriiw. A solution of gadolitiium chloride, eqtiivslent to0.5 gram of the oxide per litre, when mixed with acetic acid arid after-n.;rrds with ammonia in excess, remained transparent for a long time,but gradually became turbid, and precipitation was practically coni-~!lete after a day or two.Heat accelerates precipitat'ion, but makes ititicomplete. Analogous phenomena are observed w i t h lanthat~um,1-ttrium, and diclymium, especially the first, arid in a lower degreowith cerous chloride. c. H. B.Equivalent of Terbia. By L. DE ROISBAUDRAN (Compt. rend., 111,$74--475).-h previous determinations of the equivalent of theearth Zp (terbia with a v w y deep-Ilrown colonr), the quaiitity ofoxygen existing in the earth in the form of peroxide, was uiicerhin.The author has repeated the determinations by the same method, thatk, weighing the quantity of the sulpliate formed by a given quantityof oxide, b u t the oxide was previously calcined a t a white heat, andthe small quantity of peroxide present was determined.The coloni-of the calcined oxide was much paler, although still very yellow ; i tcontaitied 0.16 per cent. of oxygeii as peroxide. The mean equivalentof tbe terbia, is 122.32, which gives 159.48 for the atomic weightof the metal. C. H. U.YCL. LS. 18 ABSTRACTS OF CHEMICAL PAPERS.Ammonium Fluoroxymolybdates. By F. MACRO (Gazxettrr,, 20,109-121~- Hexagonal ammonium j?uoroxym olyhdate, 3MoOzF,,5NH4F + HzO, prepared by dissolving the laminar fluoroxymolpbdate (Ahstr.,1889,106), or the compound Mo03,2NH4F, in hydrofluoric acid, crpstal-lises in minute, hexagonal prisms, which resenible those of the doublesalts of molybdenum and niobium of the type 3MnOF3,5NH4F + H,O,and are probably isomorphous with the crystals of hexagonal ammoniumflnoroxyhyponioljbdate. The crystals are colourless and t,ransparentat first, but become opaque after prolonged exposure to the air ; they arenot dehydrated by heating at 100" ; they dissolve in water, formingan acid solution, which loses hydrogen fluoride on heating, and if thetemperature exceeds loo", ammonia is also evolved.Monamnioniurn Jluoroxymolybdate.Mo02F2,NH4F, is obtained inmonoclinic crystals on allowing a solution of the preceding compoundin hydrofluoric acid to evaporate over sulphuric acid ;a : b : c = 0.63019 : 1 : 1.42549, p = 85" 53'.Fa,ces observed: 010, 001, 110, 111, 337, 335, 667. Plane oftwinning (307).The crystals, which are generally twinned, arecolourless and transparent, but darken and timi green after st shortexposure to the air ; they dissolve in water, yielding an acid solution.T'he crystals may be heated t o 120" without losiiig weight, but decom-pose at a higher temperikture.Delafontaine's acid fluoyomolybdate of ammonium appears t o beidentical with the aut8hor's triammonium fluoroxpmolybdate,MoOzF2,3NH4F, and is not isomorphoils with the acid fluoroxytnng-state. S. B. A. A.Double Salts of Tungstic and Vanadic Acids. By F. ROTHEN-BACH (Ber., 23, 3050-3060).-0n adding sodium paraiunpstate tohydrated vanadic anhydride, sodium paratungsto-vanadate is formed,together with a cornpound which crystallises in dark-red octahedra,and has the formula 3(Naz0,4W0,),N~,0,3Vz05 + 38H20.The following salts were prepared from sodium paratungsto-vanadate by double decomposition :-The ammonium salt crystallises in orange-red octahedra of theformula 5 [ 5(NH4),0, 12 W 0 3 1 2 [ 7Vz05,3 (NH&O] + 58Hz0.Thebariu,m salt is deposited in light, orange-coloured crystals, which arevery sparingly soluble, and have t'he formula3( 5Ba0,12WO3),2(5VZO5,2BaO) + 94Hzo.From the mother liquors cubical crystals are obtained, which containsodium chloride, barium tungstate, and bariixm vanadate. Thestrontium salt crystztllises in orange-red cubes,3(5Sr0,12WO3),2(5VZO5,2Sr0) + 12dHz0,and resembles the barium compound. The potassiicm salt crystallisesiu aggregates of large, light orange-red plates, which have not getbeen analysed.By the action of magnesium sulphate on sodium para-tungstovanadate, a, componnd of the formula5NaZ0,12W O3,3V,O5,MgO,N a,O + 42HzINORGANIC CHEMISTRY. 19i s formed. crystallising in pale orange-yellow prisms. A similay com-pound is deposited from the mother liquors in lustrous, light orange-coloured plates. With sodium tungstovanadate, aluminiuiri sulphategives a compound of the formulacrystallising in dark garnet-red cubes. No coppr salt could be ob-tained.The water of crystallisation i n the above compounds was deter-mined by cautious ignition. The variadic acid and fiungstic acidwere precipitated together by means of mercuric nitrate and mercuricoxide. The vanadic acid was determined separately by reductionand titration with potassium permanganate, and also by boiling withphosphoric acid, potassium bromide, and hydrochloric acid ; thebromine which is evolved is absorbed in potassium iodide solution,and the liberated iodine estimated in the usual manner.Bismuth Oxyiodide.By C. ASTRE (J. Pharm,. [ 5 ] , 22,193-200).-Various published methods for the preparation of this oxyiodideyielded products more or less contaminated with sub-nitrahe, withoxide, or with both these compounds. To obtain the pure product,10 grams of bismuth potassium iodide is decomposed by the additionof 4 litres of water, and the product is washed until iodine is no l o n p rremoved. The resulting compound contained Bi, 59.38, and 1, 36-30per cent. The double iodide employed is best, obtained by triturat-ing normal bismuth nitrate (1 mol.) with potassium iodide (4 mols.),and 50 C.C. of water (sic), extracting with ethyl acetate, and sub-mitting the mixture to spontaneous evaporation.3(Al,0,,9Na,0,48W0~3) ,4( 9V205,A1,0,) + 504H20,J. B. T.J. T.Platinum Thiocarbide. By P. SCHUTZEKBERGER (Compt. ?-end.,1117391-393).-A current of nitrogen or hydrogen charged with thevapour of carbon bisulphide is passed over spongy platinum heatedat 400-450”, and when the absorption of t,he bisulphide ceases, thesomewhat finely divided black product is allowed to cool, and ispowdered and submitted to the same treatment again. The productis a dense, black powder of the composition Pt,CS2. Under a micro-scope, it seems homogeneous, and it cannot be separated into differentcomponents by levigation. I t is not attacked by boiling concentratednitric or hydrochloric acid, and is almost entirely unaffected by warmaqua regia. It is, therefore, not a mixture of platinum sulphide wit,hcarbon, and it probably has the constitution S:Pt:C:Pt:S. Whenheated below redness iir dry oxygen, i t burns with incandescence, atridyields carbonic anhydride. sulphuric anhydride, sulphurous anhydride,and a, residue of pnre platinum.The formation of this compound may be used f o r the separation,and even the estimation, of carbon bisulphide in any mixture of gaseswhich is free from oxygen. The gaseous mixture is passed over theheated spongy platinum, and the product is afterwards heated inoxygen, the gases formed being absorbed in some oxidising liquid,and the sulphuric acid estimated in the usual way. C. H. l3.c