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Proceedings of the Chemical Society, Vol. 14, No. 190 |
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Proceedings of the Chemical Society, London,
Volume 14,
Issue 190,
1898,
Page 49-60
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摘要:
Issued 10/3/1898. PROCEEDINGS OF THE CHEMICAL SOCIETY. EDITED BY THE 13‘ECRETARIES. No. 190. Session 1897-8. &€arch 3rd, 1898. Professor Dewar, F.R.S., President, in the Chair. Mr. Cecil J. Brooks was formally admitted a Fellow of the Society. Certificates were read for the first time in favour of Messrs. Joseph Brierley B.Sc., Ashton Road, Failsworth, Manchester ;Arthur William Cowburn, Fernroyd, Bowdon, Cheshire ; Charles Ben jamin Dudley, Ph.D., Attoona, Penn., U.S.A. ; Arthur Leonard Harry Garside, c/o C. Lawes and Co., Barking Creek ; Lawrence Hislop, Gas- works, Uddingston ; F. Hurter, Ph.D., Holly Lodge, Cressington Park, Liverpool ; Samuel Morton Jessop, 12 Hanson Terrace, Wake- field ; George Henry Masson, M.D., M.S., 22 Lauriston Place, Edin- burg ; Walter Charles Cross Paters, 14 Trinity Square, S.E.; Francis Pitt Smith, B.Ph., 77 Woodland Avenue, New Rochelle, N.Y., U.S.A. ; Thomas de Smith, B.A.Eastbourne College, Eastbourne ; William Thomas Newton Spivey, M. A., 5 Trumpington Street, Cambridge ; John Alexander Williamson, 81 Cheverton Road, Upper Hollo way, N ; Thomas Barlow Wood, M.A., Caius College, Cambridge. Of the following papers those marked * were read :-*24,. ‘‘ Preparation of anhydrous hydrogen cyanide and carbon monoxide.’’ By John Wade, B.Sc., and Laurence C. Panting, M.B. On allowing a cold mixture of equal volumes of sulphuric acid and water to drop on to 98 per cent. “lump ” potassium cyanide, hydrogen cyanide, accompanied by traces of water only, is evolved in almost theoretical amount, and with the aid of suitable condensing apparatus is readily collected in quantity.With concentrated sulphuric acid, on 50 the other hand, but still at the ordinary temperature, nearly pure carbon monoxide is evolved, also in quantity approaching the theoretical; provided certain precautions are taken, it is free from dioxide, and is accompanied only by small quantities of hydrogen cyanide. In discussing the mechanism of the formation of the monoxide, ex-periments are described showing that part of the water required for the hydrolysis is derived either from the sulphuric acid itself or from the potassium hydrogen sulphate formed in the course of the action, and that consequently the sulphuric acid acts at the mme instant both as a hydrolyst and as a dehydrating agent. "25."Production of some nitro- and amido-oxylutidines." By J. N. Collie, Ph.D., F.R.S., and Thomas Tickle. In a former paper (Frans., 1897,71, 838) one of the authors drew attention to the fact that various nitro- and amido-derivatives of pyridine could be obtained by the ordinary process of nitration and reduction of certain oxypyridine compounds. These substances cor-respond in the pyridine series to nitro- and amido-phenols in the benzene series, and as some of the reactions (especially those with various oxidising agents) of the amido-oxypyridines resemble those of alkaloids, the investigation has been continued. Pseudolutidostyril (ay-dimethyl-a'-oxypyridine)gave on nitration a &tropseudoZutit yril, C5HNMe,(OH)N0,.It crystallises in light yellow needles that melt with much decomposition at about 250O. The hydroxyl and nitro-groups are in the ortho-position to one another, but the substance is not volatile with steam. With alkalis, it forms brilliant, yellow compounds. When the nitro-compound is reduced with tin and hydrochkoric acid, an amidopseudolutidostyril is produced. The hydrochloride of this base, C,HNMe,( OH)NH,HCl, crystallises in needles which de- compose without melting at 235-240O. By the action of sodium bicarbonate, the free base can be obtained in the form of a bulky mass of fine needles, m. p. 205' (corr.). The base is very soluble in hot water, but much less so in cold.It oxidises readily, and an aqueous solution on boiling turns brown. This solution reduces silver nitrate at once. With ferric chloride, it gives first a red and then a br5ght green colour, and when dissolved in strong sulphuric acid, if a drop of fuming nitric acid be added, a brilliant purple colour is momentarily produced. It forms a platinichloride and an acetyl derivative, m. p. 255' (corr.). By nitrating ethylic pseudolutidostyrilcarboxylate(m. p. 137-138') a nitro-derivative was formed, C,N*Me,(OH)(CO,Et)NO,. This sub- stance, m. p. 215' (corr.), crystallises in yellow needles. On hydrolysis, 51 it yielded the corresponding acid, m. p. 260° (cprr.), which when pure is almost colourless, but forms bright yellow salts.The acid on heating loses carbon dioxide and the same nitro-pseudolutidostyril (m. p. about 250') was obtained. acidAm~do~eudolzctido~~y~~carboxylicwas prepared from the corresponding nitro-acid by reduction. Its hydrochloride crystallises from water in needles with 2 molecules of water. The amido-acid melt8 at 275' (corr.), and contains 1molecule of water of crystalha-tion ;above its melting point it decomposes, yielding amido-pseudo- lutidostyril (m. p. 205O corr.). Its salts reduce silver nitrate solution, and with ferric chloride give a green coloration. *26. Production of some nitro- and amido-oxylutidines. Part 11." By Miss L. Hall and J. Norman Collie, Ph.D., F.R.S. Lutidone, aa'-dimethyl-y-oxypyridine,when warmed with nitric acid, does not yield a nitro-derivative (2'kms., 1897, 71,838), but a nitrate of lutidone.If, however, a mixture of strong nitric and sulphuric acids are employed, the ' nitro-compound is formed, C,H,NO +HNO, = C$18NO*N02+H,O. This nitrolutidone is a pale yellow, crystalline compound, possessing a strong acid reaction, and dissolving in alkalis with an intense yellow colour; it is not volatile in steam. When reduced with tin and hydrochloric acid, it yields an amido-lutidone, C7HsNO*N02+ 3H2=C,H,NONH, +2H20. This amidolutidone, un- like amidodioxypicoline and amidopseudolutidostyril, does not give characteristic colours with oxidising agents, but acts as a strong re-ducing agent. It forms both a monohydrochloride and a dihydro-chloride.The platinichloride is unstable ;it undergoes reduction when dissolved in water and warmed, but if its hydrochloric acid solution is boiled, a very insoluble platinichloride separates, which seems to Me*g*NH2be the salt of propine diamine, HC.NH, BHCI*PtCI,, the decom-Y position having been brought about by hydrolysis, C7H,,N20 +3H,O = C,H8N2+2C,H402. This breaking down of the pyridine ring is of considerable interest, and, in a substance like lutidone, is hardly to be expected, since the nitrogen atom is bound to two carbon atoms, neither of which are united to oxygen, and, moreover, lutidone is not the anhydride of an amido-acid. DISCUSSION. Mr. LINGpointed out that certain anilides give, when treated with oxidising agents in acid solution, colour reactions similar to thorse obtained with alkaloids (Tafel, Bey., 1892, 25,412; Schar, Archie, Pharm., 1894, 232,249).52 Prof. COLLIE, pointed out thatin reply to suggestions of Dr. WYNNE, it was impossible in the case of lutidone to obtain more than one mono- nitro-derivative. In nitrating pseudolutidostyril, the position of the entering nitro-group had been determined with certainty by the fact that pseudolutidostyrilcarboxylic acid, after nitration and subsequent heating, yielded the same nitro-compound as had been obtained from pseudolutidostyril itself. *27. “On benzene hexabromide.” By F. E. Matthews, Ph.D. In this paper, the author describes his failure to isolate the second modification of benzene- hexa br omide, obtained, in mi nute quantity, by Orndorf and Howells (Arne?..Chem.Journ., 1896, 18,312-319) even from considerable quantities of the crude hexabromide ;also the failure to prepare either the hexachloride or hexabromide of bromobenzene ; in the former case owing to the displacement of chlorine by bromine, and in the latter to the substitution of bromine taking place more readily than direct addition, The action of alcoholic soda upon benzene hexabromide is also described, the product of the action being a mixture of paradibromo-and tribromobenzene (1 :2 :a), possibly mixed with a small amount of one of the other dibromobenzenes. Benzene obtained from the hexa- bromide by nascent hydrogen in acid alcoholic solution yields both modifications of the hexachloride on treatment with chlorine.DISCUSSION. Professor TILDENwas glad that Dr. Matthews had resumed work on these interesting compounds. He had repeated some of Dr. Xatthews’ experiments, and had satisfied himself that the hexachloride was obtainable very readily and in very large proportion. It was some- what remarkable that the corresponding bromide should be formed so much less readily. Dr. MATTEEWSstated that he had always worked with material spontaneously precipitated from the mixture of benzene, bromine, and water, and not with the substance left after evaporating the mixture to dryness, as was the case with Orndorf and Howells. *28. “Note on the action of bromine on benzene.” ByJ. Norman Collie, Ph.D., F.R.S., and Colin C.Frye. The authors have repeated the work of Ador and Rilliet (Bey., 1875, 3, 1286) who stated that when bromine was allowed to act on excess of benzene in sunlight, dibromo-addition products were produced, which, after treatment with zinc ethyl and subsequent oxidation with chromic 53 acid, yielded metabromo- and metaphthalic acids, together with benzoic acid, parabromobenzoic, and terephthalic acid, but they were unable to obtain any ortho-com6ounds. The authors have succeeded in proving the presence of ortho-compounds, and at the same time have confirmed the observations of Ador and Rilliet, having isolated para-bromobenzoic acid and metaphthalic acid. DISCUSSION. Dr. MATTHEWSsaid that he had made several attempts to isolate di- and tetra-chlorine and bromine addition-compounds of benzene, both by the action of the halogens upon excess of benzene and also by decomposition of the hexabromide and hexachlorides of benzene, but always without finding a trace of any di- or tetra-halogen addition- derivative. ”29.Note on manganic salts.” By C. E. Rice, B.A. The author shows that the decomposition of manganic chloride in solution into manganous chloride and chlorine is reversible, the velocity of the reverse change being very small. He also describes the pro- duction and analysis of two double manganic chlorides, 2KC1*MnCI,,H20 and 2NH4C1*MnCI,,H,O, but obtains no evidence of the existence of any compound of the formula MnC1,. DISCUSSION.Professor CLOWESasked which of the manganese hydroxides was precipitated by the action of water upon the crystalline hydrated double chloride ;it would be interesting to know whether a hydroxide corresponding to the formula MnC1, could exist. Professor TILDENremarked that the manganese tetrachloride seemed to be now finally disposed of, and in representing the production of chlorine by the usual process we should have to write a new equation. Mr. RICE,in reply, said that he had not considered it necessary to investigate the point, since Pickering had shown that when the solu- tsion obtained by dissolving any of the higher oxides of manganese (Mn203,Mn304,MnO,) in hydrochloric acid is diluted, the precipitate consists of a mixture of these hydrated oxides in varying proportions.*30. Some chemical properties of concentrated solutions of certain salts. Part I. Potassium carbonate.” By W. Colebrook Reynolds. When the salts of certain other metals are added to a concentrated solution of potassium carbonate, double salts are formed which are some- times, as in the cases of iron, copper, nickel, and cobalt, soluble in the 54 solution, instead of the normal or basic carbonates which are formed when a dilute solution is employed. These double salts and their solutions are decomposed by pure water. To obtain them, the chloride, nitrate, or preferably the acetate, is added to a concentrated solution of potassium carbonate (sp. gr. 1-55}, and the liquid left to crystallise.The author has isolated the following double salts in well defined crystalline form :-cuK2(c03)2, CuK2(C03)2,H20, CuK,(c03)2,4H20, MnK2(C03),,4H20, FeK2(CO,),,4H2O, CaK2(CO3),, Bi2OK4(CO3),,H2O, CoK,(C0&4H,O, NiK2(C0J2,4H2O, MgK2(C03),,4H20, AgKCO,. The last four salts have been previously obtained by other chemists. DISCUSSIOX; Professor TILDENsaid that Mr. Reynolds had been led to the study of these compounds in the course of enquiring into the production of the recently discovered percarbonates. In dilute solution, potassium carbonate appeared to be resolvable into the ions 2K and CO,, while in a saturated solution it behaved as though made up of K and KCO,. Mr. Reynolds had omitted to point out that in the formulae of all his new double carbonates, the heavy metal seemed to be associated with a proportion of KCO, corresponding to its valency.Perhaps this was only a coincidence, but it seemed to deserve notice. Mr. A. G. BLOXAMremarked that if carbonic acid was regarded as a hydroxy-acid the formation of a deep blue coloured solution by mixing a concentrated solution of potassium carbonate with a solution of copper sulphate became of interest as bringing carbonic acid into line with other hydroxy-acids, all, or nearly all, of which were known fo give deep blue coloured solutions with copper sulphate and alkali sufficient to satisfy both the acidic and phenolic or alcoholic hydroxyl groups. Such solutions, however, were more stable than the potassium copper carbonate solution of Mr.Reynolds, and this might be due to a comparatively unstable condition of potassium carbonate in solution ; if a strong solution of this salt was partly decomposed on dilution, potassium hydroxide and bicarbonate being formed, a corresponding decomposition of the copper compound would be expected. He would be glad to learn from Mr. Reynolds whether addition of potassium hydroxide hindered the precipitation of copper carbonate on dilution. Mr. W. P. BLOXAMasked whether the formation of these salts was attended with the evolution of carbon dioxide. Had the author taken into account the hydrolysis of potassium carbonate which took place in aqueous solution? According to a paper published by Senderens, the action of a non-metallic element (sulphur) upon solution of potas-sium carbonate could be explained by regarding the salt as hydrolysed thus, H2C)+ K2C0, = KHCO, + KOH ; and experiments made by the 55 speaker showed that even a concentrated solution of the salt must be regarded as possessing this constitution.The presence of more oxygen in the double carbonate of bismuth than that present in the acid groups would be explained by the action of the hydroxide groups present in the carbonate solution. The same reaction would also explain the difficulty of obtaining manganous and ferrous double carbonates. Mr. REYNOLDS,in reply, stated that it was possible to represent the formation of these compounds as taking place in accordance with such an equation as, for instance, MnCI, + 2K*KCO,=Mn(KCO,), + 2KC1, and this view was strengthened by the fact that some of the salts, as, for instance, copper acetate, dissolved immediately without forming a precipitate which subsequently redissolved.In the case of the double succinates, however, where exactly the same phenomena occurred, the composition of the copper compound was CuK,(C4H,O,),,2H2O, and this could not be represented by a similar equation, He had, therefore, not introduced such views into the present paper, as they did not appear to be generally applicable. The author did not think that any of the phenomena supported the view that the solution contained potassium hydroxide and potas- sium bicarbonate, as no effervescence occurred, except in the case of normal bismuth salts, when basic salts were formed.31. “The colonring matters of the Indian dyestuff Delphinium zalil.” By A. G). Perkin and J. A. Pilgrim. lCAsbarg ’’ consists of the dried flowers and fldwering stems of the Delrpinizcm xalil, found in great quantity in Afghanistan, and which is much used in India for the production of a yellow colour on alum rnordanted fabrics. The flowering stems are nearly devoid of dyeing property. For the supply of material we are indebted to the authori- ties of the Imperial Institute. Three colouring matters exist in this plant in the form of glucosides. The sparingly soluble colouring matter, C16H1207, forms glistening yellow needles, soluble in alkalis with a yellow colour.Fused with alkali it yielded phloroglucinol and protocatechuic acid, and by means of hydriodic acid it yielded quer- cetin with the evolution of 1 mol. of methylic iodide. By rnethylation it was converted into quercetintetramethyl ether, and by ncetylation into a tetracetyl derivative of the formula Cl,H,07( C,H,O),, colour-less needles, m, p. 195-196’. It was evidently isorhamnetin, a quer-cetinmonomethyl ether, recently isolated from the yellow wallflower, Gheii*arzthzcs Cheiri (Trans., 1896, 69,1650). As by oxidation in 56 alkaline solution this yields vanillic acid, it has most probably the constitution represented by this formula. With alumina as mordant it dyes a purer yellow than quercetin, The chief constituent of the more soluble portion was recognised to be identical with quercetin, the colouring matter of quercitron bark.The residual colouring matter, present only in small quantity, was not obtained in a pure condition. It resembled quercetin in percent- age composition, and in its decomposition products, but differed from it in not reacting with alcoholic potassium acetate, and the melting point of its acetyl derivative. ‘‘Asbarg ” resembles quercitron bark in dyeing property, but has only 35 per cent. the tinctorial power of this dyestuff. It contains, when freed from the flowering stalks, 3.47 per cent. of colouring matter (not as glucoside). 32. ‘‘Some metallic salts of natural yellow colouring matters.’’ By A. (3. Perkin and P. J. Wood. That certain colouring matters decompose alkaline carbonates with the formation of acid salts has been previously demonstrated.Thus of morin, Hlasiwetz and Pfaundler describe salts of this description, and of quercetin (Juhreshericht, 1864, 560). Further, from gentisin, Hlasiwetz and Habermann (A. 1875, 1’75,73)obtained analogous com- pounds. Among other instances is bixin, the colouring matter of Annatto, which Etti describes (Bei-.,1878, 11,864) as giving a sodium and a potassium salt, and rottlerin, from which one of us obtained similar compounds (Trans., 1895, 6’7,230). Owing probably to the formation of acid salts these alcoholic alkaline solutions are not readily neutrnlised completely by acetic acid, and as it appeared that some of the fortnuke of the above compounds must be incorrect, this reaction was studied.It was found that in alcoholic solution, quercetin, morin, fisetin, and myricetin decompose potassium and sodium acetates with the formation of sparingly soluble salts, Potassium pwercetin, C,,H90,K (Found K = 11.46. Theory requires I(= 11*47),forms minute orange-yellow prismatic needles, insoluble in cold water and but slowly decomposed by boiling dilute acetic acid, Sodium quercetin, C15H907Na, closely resembles the above salt. Potas-(Found I(= 11.97. Theory requires K =11-47>,sium moTin, C15H907*K separates as glistening, orange-coloured needles, and is closely resem- 57 bled by sodium movin, C,,H,OI;Na (Found Na= 6-89, Theory 7.09). Morin reacts with magnesium and ammonium acetates, though from quercetin salts have not been obtained in this way.Ammonium morin and magrtesium morin separate in the form of long needles in a similar way (Found Mg = 3.52. Theory requires Mg-3.83 per cent.). Fisetin and myricetin apparently yield analogous derivatives, and on the other hand luteolin, apigenin, chrysin, and gentisin do not appear to react with alkaline acetates. With the exception of bixin and rottlerin, as yet but little examined, the above colouring matters are known to contain no carboxyl group, and it is thus of interest to study this reaction in which only one of the numerow hydroxyls present takes part. It appears probable that some analogy exists be- tween these salts and the acid compounds of the colouring matters described by one of us (Trans., 1896, 69, 1439).33. ‘‘ The interaction of magnesium and solution of copper sulphate.” By Edward Divers, M.D., F.R.S. Neither Clowes and Caven nor Tilden, in their communications made to the Society in November last, seem to the writer to have recognised the significance of the results of the interaction of magnesium metal and a solution of copper sulphate. Remarkable as these results are, it is to be remembered that a closely analogous case had long been known, even when Commaihle in 1866 observed them, namely, that of zinc immersed in a solution of an alum. Here, also, there is free evolution of hydrogen and precipitation of basic sul- phate, and, when chromium alum replaces the aluminium salt, there is also reduction of some of the chromic sulphate to chromous sulphate.The only part of the change which finds no parallel in the action of zinc upon chr,ome alum is that of the deposition of a little copper, but this deposition is quite in accordance with the general behaviour of copper salts. The formation of basic salt and hydrogen is a change independent of that of reduction, as is clearly shown by the same formation taking place, without that of reduction, when aluminium sulphate or common alum is concerned. Now, since the alum solution is dialysable into sulphuric acid and basic aluminium or chromium sulphate (besides potassium sulphate), and is also strongly acid in reaction, it will be admitted by all that the action in the case of an alum is really that of dilute sulphuric acid upon the zinc.The gradual precipitation of the previously soluble basic salt as the zinc dissolves in the solution is just what happens when zinc sulphate is dissolved in a dialysed solution of aluminium, or chromium hydroxide, or basic sulphate. These two points being admitted, it will be very difficult to doubt that 58 similar changes occur between copper sulphate and magnesium, or, in a less degree, zinc ;for the solution is here also very acid in reaction and needs only a little boiling to make it deposit basic sulphate; be-sides, too, it will unquestionably show largely that hydrolysing action upon cane-sugar which Long (J.Amer. Chem. Xoc., 1896, 18, 120) has recently shown so many metallic salts possess, and this property is evidence that, like aluminium sulphate, it is partly hydrolysed into sulphuric acid and soluble basic sulphate, which will be precipitated as magnesium goes into the solution.Caven and Clowes have pointed out the inadequacy of the action of the magnesium-copper couple to account for the large evolution of hydrogen. Their unsupported sug- gestion that the hydrogen is formed by the combined action of copper sulphate (as such) and magnesium upon water, has likewise little claim to consideration in presence of the fact that (hydrolysed) aluminium sulphate acts in the same way as copper sulphate. Coming now to the production of cuprous oxide, a separate reaction, or set of reactions, there would be nothing in this unlike that of the reduction of ferric or chromic sulphate by zinc or magnesium, could cuprous salt only be found in solution.When, in place of the sulphate, cupric chloride is used, then, as every one knows, there is just this looked-for reduction to cuprous salt. But the peculiarity of copper is that oxylic cuprous salts are apparently unable to exist. It is, however, not so improbable that in dilute solution and in presence of much cupric sulphate ct little cuprous sulphate may exist for a very short time. According, indeed, to Rose, from roasted copper sulphide water extracts, along with cupric sulphate, a little cuprous sulphate, which then gradually decomposes into metal and cupric salt, just as a mer-curous salt in water will change into metal and mercuric salt (AnnaZen, 1841, 39,109).However that may be, and the observation admits of another interpretation, it does seem to the writer that the precipitation of cuprous oxide during the action of magnesium upon cuprous sul- phate is a fact highly favourable to the view that cuprous sulphate is actually formed, part of it then quickly decomposing into cupric sul- phate and metallic copper, and the rest of it being decomposed by the basic cupric salt into normal cupric sulphate and cuprous oxide. With certainty he can state that, when finely divided copper is acted upon by nitrogen peroxide, nitric oxide and a copper nitrate are formed, and no nitrite, and that this copper nitrate, when touched with water, decom- poses into cupric nitrate and bright metallic copper, thus proving, ap- parently, that in absence of water cuprous nitrate can exist, .and, therefore, by analogy, other oxylic cuprous salts.There remains only to notice Tilden’s suggestion that some of the hydrogen reduces cupric to cuprous oxide. Hydrogen is known not to have such an action, and therefore the usual assumption of there 59 being a more active 'nascent ' hydrogen has to be made, but also without the least foundation in experience. In the present case, it may be pointed out, firstly, that in the reduction of chromic sulphate to chromous sulphate by zinc, hydrogen continues to be evolved, although very great excess of chromic salt is always in contact with the zinc; and, secondly, that in the reduction of ferric salts by zinc it has been established that this takes place much more rapidly when claan zinc dust is put into the ferric solution in the absence of excess of acid, than when, as is usual, an excess of acid is added to generate hydrogen.It may, therefore, with great probability be assumed that the reactions are 2CuS0, +Mg =Cu,SO, +MgSO, and Fe,(SO,), +Zn =D'eSO, +ZnSO,, hydrogen having nothing to do in the matter. ADDITIONS TO THE LIBRARY. I. By Purchase. Groth P. Tabellarische ubersicht der Mineralien nach ihrn krystallo- graphisch-chemischen beziehungen. Vierte auflage. Pp. viii +184. Braunschweig 1898. Wollny, Ewald. Die zersstzung der organischen stoffe und die humusbildungen mit riicksicht auf die bodencultur.Pp. x +479. Heidelberg 1897. 11. Donations. Bailey, G. H. The Tutorial Chemistry. Part 11. Metals. Bp vi + 295. London 1898. From the Author. Roscoe, €3. E., und Classen, A. Lehrbuch der anorganischen Chemie Zweiter band. Dritte ganzlich umgearbeitete auflage des infriiheren adlagen von Roscoe und Schorlemmer bearbeiteten werkes. Braun-schweig 1897. From Sir H. E. Roscoe. Pamphlets. Louis, D. A. The Iron Industry of Hungary. (Reprinted from the Jolurnal of the Iron and Eteel Inst. No. II., for 1897). Sachs, E. 0. What is fire protection? A study by. Pp. 37. Fire prevention, some American opinions on. Pp. 16. Sachs, E. 0. Paris Charity Bazaar Fire. A paper by. Pp. 52.(Publications of the British Fire Prevention Committee, Nos. 1, 2, and 3.) Spring, W. Sur le role des composes ferriques et des matihres humiques les ph6;omhe de la coloration des eaux et sur 1'6limination 60 de ces substances sous l’influence de la lumih solaire. Bruxelles 1897. Observations sur l’hydrolyse du chlorure ferrique. hide 1897. Sur le spectre d’absorption de quelques corps organiques incolores et ses relations avec la structure mol6culaire. Bruxelles 1897. Sur la couleur et le spectre d’wbsorption de quelques corps organiques. Genbve 1896. De la temperature b laquelle les courants de convection commencent A produire l’opacite d’une colonne d’eau d’une longueur donn6e. Bruxelles 1896. ’ Sur la transparence des solutions des sels incolores.Genhve 1896. De l’influence du temps sur l’agglutinntion de la craie comprim6e. Bruxelles 1895. Sur la couleur des alcools cornparbe b la couleur de l’eau. GenBve. 1896. Sur le role des courants de convection calorifique dans le phenomhne de l’illumination des eaux limpides. Genbe 1896. Sur un hydrate de trisulfure d’arsenic et sa dkcomposition par la compression. Bruxelles 1895. Spring, W., et Romanoff, L. Sur la solubilit6 reciproque du bismuth et du plomb dans le zinc existence d’une tempbratrue critique. Bruxelles I896. Spring W. Uber die physikalischen veranderungen, die gewisse schwefelverbindungen unter dem einfluss der temperatur erleiden. Leipzig 1895. Notice bibliographique. Bruxelles 1896. Woods, Hugh. Bther, its nature and place in the universe. London 1898. At the next meeting, on Thursday, March 17th, the following papers will be communioated. The reduction of bromic acid and the law of mass action.” ByWinifred Judson, B.Sc.,and J. Wallace Walker, M.A., Ph.D ‘‘The action of ferric chloride on the ethereal salts of ketone acids.” By R. S. Morell, M.A., Ph.D., and J. M. Crofts, B.A., Ph.D. ‘‘ Note on the volatility of sulphur.’’ By T. C. Porter. ‘6 Action of ammonia and substituted ammonias on acetylurethane.” By George Young, Ph.D., and Ernest Clark. RICHARD CLAY AND SONS, LIMITED, LONDON AND BUNGAY.
ISSN:0369-8718
DOI:10.1039/PL8981400049
出版商:RSC
年代:1898
数据来源: RSC
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