10 ABSTRACTS OF CHEMICAL PAPERS. I n o r g a n i c Chemistry. Liquefaction of Oxygen. By RAO UL P I c TE T (Chein. News, xxxvi, 281).-This gas has been liquefied under a pressure of 300 atmo- spheres at the temperature produced by the rapid evaporation of liquid carbon dioxide in a vacuum. By a double circulation of sulphur di- oxide and carbon dioxide, this latter gas was liquefied a t a tenipernture of -65" and a pressure of 4 to 6 atmospheres. The liquid carbon dioxide was passed along a tube about 4 meters long, communicating with two air-pumps. When a vacuum is produced by these pumps the carbon dioxide solidifies. In the interior of the tube is a smaller one, through which passes a current of oxygen, produced in a strong vessel. The whole apparatus can stand a pressure of 800 atmospheres.With this apparatus oxygen was liquefied at a pressure of about 300 atmospheres, a jet of liquid oxygen escaping from the tube when the pressure was taken off. c. w. w.INORGANIC CHEMISTRY. 11 Liquefaction of Nitrogen Dioxide. By C A I L L E T E T (Cornpi. rend., lxxxv, 1017).-This gas was liquefied at a pressure of 104 at- mospheres, and a temperature of -11". It is still liquid a t +8" and 270 atmospheres. Methane a t 7" and a pressure of 180 atmospheres gives a cloudy appearance, similar to that produced when the pressure is suddcnly On Iodine Chlorides, Iodine Bromide and Bromine Chlo- ride, and their Reaction with Water. By W. BORNENAPU" (Liebig's AnnaZen, clxxxix, 183--213).-The main results of the author's experiments are as follows :- (1.) Pure iodine chloride, ICI, remains liquid in a sealed tube, but solidifies on opening the tube.(2.) I n presence of iodine trichloride the monochloride crystallises even in a sealed tube. (3.) By distillation, and by long exposure to air, iodine chloride is partially decomposed into iodine and trichloride. (4.) Iodine chloride is not soluble in water without decomposition ; it dissolves in dilute hydrochloric acid without separation of iodine. (5.) If iodine be suspended in water and chlorine be passed through the liquid, the greater the quantity of water present, the greater is the amount of chlorine required for complete solution of the iodine. Complete conversion of the iodine into iodic acid is accomplished only when a minimum of 10 parts water to 1 part iodine is maintained.Iodic acid then separates out, and iodine trichloride may be obtained from the liquor. (6.) Iodine bromide is a crystalline body resembling iodine ; it may be distilled with partial decomposition; it dissolves in water with separation of but little iodine. taken off liquid carbonic acid. c. w. w. (7.) No hydrate of the composition BrI.5Hz0 exists. (8.) Bromine chloride is a red-brown liquid, stable only at tempera- tures under + 10". (9.) BrCl + 5Hz0 does not exist : the crystalline mass obtained by decomposing bromine chloride with water-if a true compound a t all -is represented by the formula, BrC1.lOHzO. Preparation of Iodine Trioxide. By J. OGIER (Corrqt. rend., lxxxv, 957-959).-By the action of a mixture of ozone and oxygen on the vapour of iodine, an exceedingly light yellow dust is obtained in small quantities, which is decomposed by water, with formation of iodic acid and separation of iodine. It is very deliquescent, and when heated between 125-130".decomposes into iodine and oxmzen. I t R M. M. P. ill. .I '2 analysis gives numbers corresponding with the formula, 1203. L. T. 0's. Boric Acid. By M. L. DIEULAFA~T (Ann. Chim. Phys. [5], xii, 318--354).-Tn complex saline solutions, the only trustworthy methods of detecting boric acid are by spectrum analysis and by the green colour imparted to a Bunsen's flame. A drop of the solution under examination is placed on a ball of magnesia, prepared by dipping a platinum wire in a saturated aqueous solution of magnesium chloride,12 ABSTRACTS OF CHEMICAL PAPERS. drying the wire in the gas-flame, and repenting the operation untiI 8 spongy mass of magnesia four millimeters in diameter is obtained.This ball impregnated with the solution is heated in a non-luminous flame, which is examined through a, spectroscope. I n this way m$m grm. of boyon can be detected. A mixture of the substance with strong sulphuric acid held on the loop of a thick platinum wire imparts a distinct green colour to the flame, when i,&,BDB grm. of boron is present. The wire should be placed from two t o four millimeters from the outer edge of the visible flame, so that the temperature is not high enough to volatilize the sodium salts. Sea-water contains appreciable quantities of boric acid, and on evaporation the boric acid collects in the last mother-liquors. I n the Stassfurt salt beds boric acid occum in the top layers with magnesium chloride and other deliquescent salts, The Mediterranean contains 0.2 grrn.of boron or 1.73 grms. of sodium borate per cubic meter. The saline deposits of the trias and tertiary formations have been formed by the evaporation of sea-water ; hence they must contain con- siderable quantities of boric acid. It is to these salt-beds of the tertiary formation that the boric acid in the Tuscan lagoons owes its origin, and not to the action of steam on boron nitride or sulphicie, as was formerly supposed. Volcanic heat volatilizes the water in the salt beds, and partly decomposes the magnesium chloride with which the boric acid is probably associatcd ; hydrochloric acid is thereby set free, which in its turn liberates boric acid.w. c. w. Synthesis of Ultramarine. By J. F. PLICQUE (COWL@. rend. lxxxv, 749-752) .-A silico-aluminate of sodium prepared by mixing equivalent parts of sodium silicate and sodium aluminate in solution, was heated in a current of carbon disulphide vapour, when a yellowish- white ccrrnpound was obtained, which rapidly absorbed oxygen from the air, with evolution of sulphuretted hydrogen, the colour changing t o blue. This compound heated in a current of sulphur dioxide absorbed large quantities of it, free sulphur separating out. The blue com- pound thus obtained contained 41.3 per cent. of sodium snlphate, but no free sulphur. The author’s conclusions are (1) that ultramarine contains no nitrogen ; and (2) ultramarine-blue is a compound of sulphur dioxide with sodium and aluminium.The sulphur in the carbon disulphide replaces part of the oxygen in the silico-aluminate of soda, forming sodium sulphide, which, with sulphur dioxide, forms sodium sulphate, with liberation of sulphur. By substituting the corresponding selenium-compounds for those Nitroxylsilver, or Silver Hyponitrite. By W. 2; o n N ( Deut. Chem. Ges. Ber., x, 1306) .--The author entirely corroborates the state- ments of Divers that silver hyponitrite, NOAg, is formed when sodium- amalgam acts on solution of potassium nitrate, and the product is neutraiised with acetic acid and precipitated by silver nitrate. Divers of sulphur, a red compound was obtained. L. T. 073.INORGANIC CHEMISTRY.13 did not obtain the silver salt perfectlypure, as shown by his analytical numbers, and by the greenish-yellow colour of his product ; the author has obtained it quite pure by solution in dilute nitric acid, and careful neutralisation by ammonia: it then forms a pure yellow substance soluble in nitric acid and in ammonia, and capable of being dried in a vacuum over sulphuric acid without decomposition ; when dry it under- goes no change at 100'. The yield is about 15 per cent. of the nitrate employed, about the same result being obtained if a nitrite be employed instead. Silver hyponitrite is readily acted on even in the cold by methyl, ethyl, normal propyl, normal secondary butyl, tertiary butyl, and hexyl iodides, silver iodide being formed with evolution of heat ; the products of these actions are under investigation.Amount of Water in Hydroauric Chlorides. By JIJLIUS THOMSEN (Deut. CYhem. Ges. Ber., x, 1633).-The author finds t h t this substance in the dry state, as obtained by drying the crystals over quick-lime, contains 4 mol. of water. Its formula is, thercfore, duC14H + 4H20. J. R. Tin Phosphide. By S. NATANSON and G. VORTMANN (Dezct. Chem. G'es. Ber,, x, 1459-1461) .-The authors have analysed certain varieties of tin phosphide prepared by the following methods : (1.) By heating together glacial phosphoric acid, 3 parts ; charcoal, 1 part, and tin 6 parts. (2.) By fusing together glacial phosphoric acid and metallic tin. (3.) By passing phosphorus vapour in a stream of hydro- gen over melted tin ; and (4.) By adding phosphorus t o mclted tin.Prepared according to the above methods, the phosphide was silvery- white, of leafy crystalline structure, and soluble in hydrochloric acid with evolution of phosphuretted hydrogen. C. R. A. W. The analytical results in each case are as follows :- (1.) Sn 97.97, P 1.52, and 1.37 per cent. ; when heated to redness in a current of hydrogen, a loss of 0,997 per cent. of phospliorus was estimated. (2.) P 0.746, and 0.827 per cent. (3.) Sn 96.551. P 2,856. (4;) This variety resembled the preceding. The two commercial varieties of the phosphide, which are also silverv-white and exhibit a leafy fracture, were found to contain : (No. 6) 95.904 per cent. Sn. ("b. 1) 98.9 per cent. Sn. c. I?. c. Barium Oxysulpharsenite. By L.F. NILSON (J. pr. Chen2. [a], xvi, 93--96).-From the mother-liquors of barium sulpliar- senite, 2BaS.As2S3 + 5Hz0 (J. pr. Cheru~. [2], xiv, 48), the author obtains by boiling a yellow crystalling precipitate, to which he lizd formerly given the formula, 5BaS.2As2S3 + 6H20. ]Further analytical results lead him t o attribute t o it the composition 5RaS.2hs2S,0 + 6H20. This formula is also supported by the observation that from the mother-liquors a barium sulphersenit-arsenate, 5BaS { f: + 8H20 separates out, owing its formation to that of the oxisuiphar- senite, as by this the necessary sulphur is set free, The author attributes the following constitution to this oxysulpharsenite :-14 ABSTRACTS OF CHTMICAL PAPERS. Ba< >As-S-Ba-S-As-S-Ba-S-As-S-Ba-S-As< 0 >Ba.l S / Two analogous arsenic compounds are known, viz., the bisulph- arsenic acid in the salt of Cloez, K,O.As,S,O, + 2H,O, and the bisulph- arsenic acid, As,S302 prepared by the author (J. pr. Chern. [2], xii, 297). P. P. 13. On the Atomic Weight of Molybdenum and certain Phos- phomolybdates. By C. RAM M E L s B E R G (Deut. Che?n. Qes. Ber., x, 1776-1780) .-Prior to his investigation of the phosphomolybdates, the author has made a determination of the atomic weight of molyb- denum, by reduction of the anhydridc to metal in a stream of hydrogen. The experimental number thus obtained was 96-18 : molybdenum is therefore taken as 310 = 96. Ammonizsnz and Potassium Phosj~lmn olybdate.--To the well known yellow ammonium salt and the corresponding potassium compound, the author assigns the formula : 3Rf2O.P2O5.22MoO3.12Aq.By the action of a small quantity of potash-solution, the yellow potassium salt is converted into a white insoluble modification : FjK,0.P,05.15Mo03. On boiling the alkaline filtrate from this salt, a flocculent precipitate of K2Mo3OI0 is obtained. By dissolving this compound in a small quantity of potash-solution and adding phosphoric acid, a salt is obtained in white shining prisms of the composition, 5K,0.2P205 10MoO3.20Aq. By fusing 1 mol. K2C0, with XvIoO,, dissolving in water, and adding phosphoric acid to the solution, a compound crystallising in large colourless octohedrons is obtained. The formula of this salt, 3K,O.Pz05.5M003.7Aq, exactly corresponds with that assigned by Zenkcr to the colourless compound obtained from the solution of the yellow ammonium phos- Osmium Oxysulphides. By E.VON MEYER (J. pr. Chenz. [2], xri, 77-86) .-The author has shown that oxidised platinic sulphide is a hydrate of platinum sulphoxide, PtSO (J. p r . Chew [el, xiv, 1). He finds that by treating an aqueous solution of osmium tetroxide Kith sulphuretted hydrogen, a precipitate is formed, which, when sus- pended in water, and submitted to the further action of sulphuretted hydrogen, yields a loosely crystalline body, easily oxidised on exposure t o air, and having the formula, Os3S706.2H,0. The oxidation of this body by air at 70-SO" yields an unstable, odourless, and insoluble body, having the composition (OsSO,) .3H,O. Further exposure to air yields osmium tetroxide.The presence of sulphur in these bodies renders the oxygen more easily removed than in osminm tetroxide, and produces a tendency to form hydrates, which the latter does not. For the method of analysing these unstable bodies, the original paper must be consulted. P. P. B. phomolybdate in ammonia. c. 3'. c.10 ABSTRACTS OF CHEMICAL PAPERS.I n o r g a n i c Chemistry.Liquefaction of Oxygen. By RAO UL P I c TE T (Chein. News,xxxvi, 281).-This gas has been liquefied under a pressure of 300 atmo-spheres at the temperature produced by the rapid evaporation of liquidcarbon dioxide in a vacuum. By a double circulation of sulphur di-oxide and carbon dioxide, this latter gas was liquefied a t a teniperntureof -65" and a pressure of 4 to 6 atmospheres.The liquid carbondioxide was passed along a tube about 4 meters long, communicatingwith two air-pumps. When a vacuum is produced by these pumps thecarbon dioxide solidifies. In the interior of the tube is a smaller one,through which passes a current of oxygen, produced in a strong vessel.The whole apparatus can stand a pressure of 800 atmospheres.With this apparatus oxygen was liquefied at a pressure of about300 atmospheres, a jet of liquid oxygen escaping from the tube whenthe pressure was taken off. c. w. wINORGANIC CHEMISTRY. 11Liquefaction of Nitrogen Dioxide. By C A I L L E T E T (Cornpi.rend., lxxxv, 1017).-This gas was liquefied at a pressure of 104 at-mospheres, and a temperature of -11". It is still liquid a t +8" and270 atmospheres.Methane a t 7" and a pressure of 180 atmospheres gives a cloudyappearance, similar to that produced when the pressure is suddcnlyOn Iodine Chlorides, Iodine Bromide and Bromine Chlo-ride, and their Reaction with Water.By W. BORNENAPU"(Liebig's AnnaZen, clxxxix, 183--213).-The main results of theauthor's experiments are as follows :-(1.) Pure iodine chloride, ICI, remains liquid in a sealed tube, butsolidifies on opening the tube.(2.) I n presence of iodine trichloride the monochloride crystalliseseven in a sealed tube.(3.) By distillation, and by long exposure to air, iodine chloride ispartially decomposed into iodine and trichloride.(4.) Iodine chloride is not soluble in water without decomposition ;it dissolves in dilute hydrochloric acid without separation of iodine.(5.) If iodine be suspended in water and chlorine be passed throughthe liquid, the greater the quantity of water present, the greater is theamount of chlorine required for complete solution of the iodine.Complete conversion of the iodine into iodic acid is accomplishedonly when a minimum of 10 parts water to 1 part iodine is maintained.Iodic acid then separates out, and iodine trichloride may be obtainedfrom the liquor.(6.) Iodine bromide is a crystalline body resembling iodine ; it maybe distilled with partial decomposition; it dissolves in water withseparation of but little iodine.taken off liquid carbonic acid.c. w. w.(7.) No hydrate of the composition BrI.5Hz0 exists.(8.) Bromine chloride is a red-brown liquid, stable only at tempera-tures under + 10".(9.) BrCl + 5Hz0 does not exist : the crystalline mass obtained bydecomposing bromine chloride with water-if a true compound a t all-is represented by the formula, BrC1.lOHzO.Preparation of Iodine Trioxide.By J. OGIER (Corrqt. rend.,lxxxv, 957-959).-By the action of a mixture of ozone and oxygenon the vapour of iodine, an exceedingly light yellow dust is obtainedin small quantities, which is decomposed by water, with formation ofiodic acid and separation of iodine. It is very deliquescent, and whenheated between 125-130". decomposes into iodine and oxmzen. I t RM. M. P. ill..I '2 analysis gives numbers corresponding with the formula, 1203.L. T. 0's.Boric Acid. By M. L.DIEULAFA~T (Ann. Chim. Phys. [5], xii,318--354).-Tn complex saline solutions, the only trustworthy methodsof detecting boric acid are by spectrum analysis and by the greencolour imparted to a Bunsen's flame. A drop of the solution underexamination is placed on a ball of magnesia, prepared by dipping aplatinum wire in a saturated aqueous solution of magnesium chloride12 ABSTRACTS OF CHEMICAL PAPERS.drying the wire in the gas-flame, and repenting the operation untiI 8spongy mass of magnesia four millimeters in diameter is obtained.This ball impregnated with the solution is heated in a non-luminousflame, which is examined through a, spectroscope. I n this waym$m grm. of boyon can be detected.A mixture of the substance with strong sulphuric acid held on theloop of a thick platinum wire imparts a distinct green colour to theflame, when i,&,BDB grm.of boron is present. The wire should beplaced from two t o four millimeters from the outer edge of the visibleflame, so that the temperature is not high enough to volatilize thesodium salts.Sea-water contains appreciable quantities of boric acid, and onevaporation the boric acid collects in the last mother-liquors. I n theStassfurt salt beds boric acid occum in the top layers with magnesiumchloride and other deliquescent salts, The Mediterranean contains 0.2grrn. of boron or 1.73 grms. of sodium borate per cubic meter.The saline deposits of the trias and tertiary formations have beenformed by the evaporation of sea-water ; hence they must contain con-siderable quantities of boric acid.It is to these salt-beds of the tertiaryformation that the boric acid in the Tuscan lagoons owes its origin,and not to the action of steam on boron nitride or sulphicie, as wasformerly supposed. Volcanic heat volatilizes the water in the saltbeds, and partly decomposes the magnesium chloride with which theboric acid is probably associatcd ; hydrochloric acid is thereby set free,which in its turn liberates boric acid. w. c. w.Synthesis of Ultramarine. By J. F. PLICQUE (COWL@. rend.lxxxv, 749-752) .-A silico-aluminate of sodium prepared by mixingequivalent parts of sodium silicate and sodium aluminate in solution,was heated in a current of carbon disulphide vapour, when a yellowish-white ccrrnpound was obtained, which rapidly absorbed oxygen fromthe air, with evolution of sulphuretted hydrogen, the colour changingt o blue.This compound heated in a current of sulphur dioxide absorbedlarge quantities of it, free sulphur separating out.The blue com-pound thus obtained contained 41.3 per cent. of sodium snlphate, butno free sulphur.The author’s conclusions are (1) that ultramarine contains nonitrogen ; and (2) ultramarine-blue is a compound of sulphur dioxidewith sodium and aluminium.The sulphur in the carbon disulphide replaces part of the oxygen inthe silico-aluminate of soda, forming sodium sulphide, which, withsulphur dioxide, forms sodium sulphate, with liberation of sulphur.By substituting the corresponding selenium-compounds for thoseNitroxylsilver, or Silver Hyponitrite.By W. 2; o n N ( Deut.Chem. Ges. Ber., x, 1306) .--The author entirely corroborates the state-ments of Divers that silver hyponitrite, NOAg, is formed when sodium-amalgam acts on solution of potassium nitrate, and the product isneutraiised with acetic acid and precipitated by silver nitrate. Diversof sulphur, a red compound was obtained. L. T. 073INORGANIC CHEMISTRY. 13did not obtain the silver salt perfectlypure, as shown by his analyticalnumbers, and by the greenish-yellow colour of his product ; the authorhas obtained it quite pure by solution in dilute nitric acid, and carefulneutralisation by ammonia: it then forms a pure yellow substancesoluble in nitric acid and in ammonia, and capable of being dried in avacuum over sulphuric acid without decomposition ; when dry it under-goes no change at 100'.The yield is about 15 per cent. of the nitrateemployed, about the same result being obtained if a nitrite be employedinstead. Silver hyponitrite is readily acted on even in the cold by methyl,ethyl, normal propyl, normal secondary butyl, tertiary butyl, andhexyl iodides, silver iodide being formed with evolution of heat ; theproducts of these actions are under investigation.Amount of Water in Hydroauric Chlorides. By JIJLIUSTHOMSEN (Deut. CYhem. Ges. Ber., x, 1633).-The author finds t h tthis substance in the dry state, as obtained by drying the crystals overquick-lime, contains 4 mol. of water. Its formula is, thercfore,duC14H + 4H20.J. R.Tin Phosphide. By S. NATANSON and G. VORTMANN (Dezct.Chem. G'es. Ber,, x, 1459-1461) .-The authors have analysed certainvarieties of tin phosphide prepared by the following methods : (1.)By heating together glacial phosphoric acid, 3 parts ; charcoal, 1 part,and tin 6 parts. (2.) By fusing together glacial phosphoric acid andmetallic tin. (3.) By passing phosphorus vapour in a stream of hydro-gen over melted tin ; and (4.) By adding phosphorus t o mclted tin.Prepared according to the above methods, the phosphide was silvery-white, of leafy crystalline structure, and soluble in hydrochloric acidwith evolution of phosphuretted hydrogen.C. R. A. W.The analytical results in each case are as follows :-(1.) Sn 97.97, P 1.52, and 1.37 per cent.; when heated to rednessin a current of hydrogen, a loss of 0,997 per cent. of phospliorus wasestimated.(2.) P 0.746, and 0.827 per cent. (3.) Sn 96.551. P 2,856.(4;) This variety resembled the preceding.The two commercial varieties of the phosphide, which are alsosilverv-white and exhibit a leafy fracture, were found to contain :(No. 6) 95.904 per cent. Sn. ("b. 1) 98.9 per cent. Sn. c. I?. c.Barium Oxysulpharsenite. By L. F. NILSON (J. pr. Chen2. [a], xvi, 93--96).-From the mother-liquors of barium sulpliar-senite, 2BaS.As2S3 + 5Hz0 (J. pr. Cheru~. [2], xiv, 48), the authorobtains by boiling a yellow crystalling precipitate, to which he lizdformerly given the formula, 5BaS.2As2S3 + 6H20. ]Further analyticalresults lead him t o attribute t o it the composition 5RaS.2hs2S,0 +6H20.This formula is also supported by the observation that fromthe mother-liquors a barium sulphersenit-arsenate, 5BaS { f: +8H20 separates out, owing its formation to that of the oxisuiphar-senite, as by this the necessary sulphur is set free, The authorattributes the following constitution to this oxysulpharsenite :14 ABSTRACTS OF CHTMICAL PAPERS.Ba< >As-S-Ba-S-As-S-Ba-S-As-S-Ba-S-As< 0 >Ba.l S /Two analogous arsenic compounds are known, viz., the bisulph-arsenic acid in the salt of Cloez, K,O.As,S,O, + 2H,O, and the bisulph-arsenic acid, As,S302 prepared by the author (J. pr. Chern. [2], xii,297). P. P. 13.On the Atomic Weight of Molybdenum and certain Phos-phomolybdates.By C. RAM M E L s B E R G (Deut. Che?n. Qes. Ber., x,1776-1780) .-Prior to his investigation of the phosphomolybdates,the author has made a determination of the atomic weight of molyb-denum, by reduction of the anhydridc to metal in a stream of hydrogen.The experimental number thus obtained was 96-18 : molybdenum istherefore taken as 310 = 96.Ammonizsnz and Potassium Phosj~lmn olybdate.--To the well knownyellow ammonium salt and the corresponding potassium compound,the author assigns the formula : 3Rf2O.P2O5.22MoO3.12Aq.By the action of a small quantity of potash-solution, the yellowpotassium salt is converted into a white insoluble modification :FjK,0.P,05.15Mo03. On boiling the alkaline filtrate from this salt, aflocculent precipitate of K2Mo3OI0 is obtained.By dissolving this compound in a small quantity of potash-solutionand adding phosphoric acid, a salt is obtained in white shining prismsof the composition, 5K,0.2P205 10MoO3.20Aq.By fusing 1 mol. K2C0, with XvIoO,, dissolving in water, and addingphosphoric acid to the solution, a compound crystallising in largecolourless octohedrons is obtained. The formula of this salt,3K,O.Pz05.5M003.7Aq,exactly corresponds with that assigned by Zenkcr to the colourlesscompound obtained from the solution of the yellow ammonium phos-Osmium Oxysulphides. By E. VON MEYER (J. pr. Chenz. [2],xri, 77-86) .-The author has shown that oxidised platinic sulphideis a hydrate of platinum sulphoxide, PtSO (J. p r . Chew [el, xiv, 1).He finds that by treating an aqueous solution of osmium tetroxideKith sulphuretted hydrogen, a precipitate is formed, which, when sus-pended in water, and submitted to the further action of sulphurettedhydrogen, yields a loosely crystalline body, easily oxidised on exposuret o air, and having the formula, Os3S706.2H,0. The oxidation of thisbody by air at 70-SO" yields an unstable, odourless, and insolublebody, having the composition (OsSO,) .3H,O. Further exposure toair yields osmium tetroxide. The presence of sulphur in these bodiesrenders the oxygen more easily removed than in osminm tetroxide,and produces a tendency to form hydrates, which the latter does not.For the method of analysing these unstable bodies, the original papermust be consulted. P. P. B.phomolybdate in ammonia. c. 3'. c