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Proceedings of the Chemical Society, Vol. 30, No. 429 |
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Proceedings of the Chemical Society, London,
Volume 30,
Issue 429,
1914,
Page 131-154
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摘要:
PROCEEDINGS OF THE CHEMICAL SOCIETY. ~ Vol. 30 No.429. Thursday, May 7th, 1914, at 8.30 p.m., Professor W. H. PERKIN, LL.D., F.R.S., President, in the Chair. Certificates were read for the first time in favour of Messrs.: Alfred Archibald Boon, D.Sc., Heriot-Watt College, Edinburgh. John Verne11 Cutler, Rose Cottage, Farringdon Lane, Ribbleton, Preston. Galstaun Slianazar Galstaun, B.A., Abbotsholme, Derbyshire. James Mylam Gittins, BLSc., South Lynn, Limes Road, Folkestone. Alfred Holt, 32, Britain Street, Bury. John Cyril Jennings, Rosindell, Fairlop Road, Leytonstone, N.E. Hashinat Rai, B.A., M.Sc., Chemical Buildings, Government College, Lahore, India. Frederic Robinson, M.Sc.Tech., The Hollies, Mile End, Stock-port. Walter Edward Rowbottam, 23, Darville Road, Stoke Newing- ton, N.Alfred John White, B.Sc., Hawes Down, West Wickham, Kent. Messrs. W. Sloan Mills and P. C. Austin were elected Scrutators, and a ballof-for the election of Fellows was held. The following were subsequently declared as duly elected : Abdel Hameecl Ahinad, 13.S~. Arthur Baxter, B. Sc. Charles Frank Armstrong. Frederick Stanley Btlxter. Raymond Foss I3aeo11, RSc., M.A., Robert Reginald Baxter, B.A. Ph. D. Charles Wesley Rayley. 132 Robert Ode11 Bishop. 13irendranath Msitrn, M. Sc. Edward Godfrey Bryant, B.A., TI.&. Ynsuf Ismail Mulla. Albert Coulthnrd, B.Sc., Ph. I>. IYilliani Whalley hlytltlleton, 31. Sc. Robert Barclay Craig. Arthur Ulysses Newton, B.Sc. Robinson Percy Poulds, 11.Sc.Jnnies Itiddick Partington, B. Sc. Hugh Miller Galt, B.Sc., M.B , 1j.P.H. Walter Ryley Pratt, H.Sc. Brojendranath G hosh, M. Sc. Henry Ratcliffe. Clifford Girdlestone Gill. Walter William Reeve, B.Sc. Alfred Cornwall Harrison. Herbert Corner Reynard, 13.Sc. Richard Selwyn Haskew. John Rogers. Jnroslav Heyrovsky’, R. Sc. Percy Charles Rundell. Arthur Bertram Hobson, M. Qc. La11 Behary Seal. Trevor Edward Hodges. Max Herbert Tagg, B.Sc. Lawson John Hudleston. Norman Cecil White, B. A., K.Sc. Ralph Waldo Emerson MacIvor. Albert Wntkins Mtlggs Wintle. Of the following papers, those marked * were read: *115. “ Besearches on santalin. Part 11.” By John Cannell Cain, John Lionel Simonsen, and Clarence Smith. -4s a result of determinations of the molecular weight of certain derivatives of santalin by Barger’s method, the authors are of the opinion that the formula previously assigned to this colouring matter should be doubled, and hence should be CNH280,,.The presence of four benzene rings in the santalin molecule appears also to be indicated by the facts that (1) the monomethyl ether yields, on oxidation, a mixture of anisic and veratric acids, and (2) nitrosantalin dimethyl ether yields four different benzenoid acids on oxidation. Santalin yields anthracene on distillation with zinc dust (Grand- mougin), and the authors suggest that it is probably a dianthracene derivative. DIscus SION. Dr. TURNERsuggested that the low molecular-weight values found for santalin in phenol might be due to combination with the solvent.Of the other solvents employed, ether was most likely to lead to the simplest (or normal) molecular weight. *116. ‘(The nature of molecular association. Its relation to chemical cornbination.” By William Ernest Stephen Turner and Solomon English. The term “association” is frequently used to denote both the phenomenon of the formation of complexes of similar molecules and of dissimilar molecules (formation of molecular compounds). 133 Further, views have been expressed to the effect that the forma- tion of molecular compounds is a natural consequence of molecular association in the component Substances. In order to test how far these views are truly founded, the subject was investigated by a review of the different classes of substances which form molecular compounds and by an investiga- tion of the behaviour in benzene, bromof orm, chloroform, and water of mixtures of (1) alkyl and aryl haloids, (2) associated organic substances, (3) associated organic substances and alkyl or aryl haloids, (4) salts, (5) salts and alkyl or aryl haloids, (6) salts and associated organic substances, (7) alkyl or aryl haloids and iodine, (8) salts and iodine, (9) associated organic substances and iodine.A study was also made of the mixture of a-naphthylamine and phenol, in which combination is known to occur. It was shown that whilst associated substances have a marked tendency to form molecular compounds, mixtures of associated substances can often be obtained without chemical combination, and, on the other hand, molecular compounds are also produced by non-associated substances.Mixtures of salts in bromoform, so far from dissociating each other, actually produce increased association. In one or two, cwe9 inve&gated the increased association passes through a maximum at a certain concentration, and then diminishes to zero. Similar behaviour is found in chloroform, and also in water, but in the latter to a less eatent. Benzoic and acetic acids have but little effect on one another, but iii some other cases of organic associated substances, each constituent influences the d,her, probably by combination. Alkyl or aryl haloids and iodine, and organic associated sub- stances and iodine have but little effect on one another; a nitrate in bromoform solution acts with iodine to some extent, but not nearly so much as chlorides, bromides, and iodides, which form periodides, these in turn apparently becoming associated. *117.‘(The action of diastase on starch granules. Part I.” Julian Levett Baker and Henry Francis Everard Hulton. Brown and Morris (T., 1890, 57, 510) have stated that when precipitated malt diastase is allowed to act at the ordinary tem- perature on the granules of barley starch, the whole of the optically active substance produced is maltose. Later Morris (T., 1901, 79, 1085) confirmed the observation in the case of malt extract, but when precipitated diastase was used a smaller yield was obtained, and the product was stated to consist of a mixture 134 of maltose and dextrin. No experimental evidence was adduced in support of this assertion.The authors bring forward experimental evidence to show that the similarity to maltose of the specific rotatory power and the cupric reducing power of the products so formed at temperature varying between 15.5 and 37.5 is fortuitous. On submitting the products of such action to fermentation, alcoholic fractionation, and dialysis, a dextrin was isolated which had a molecular weight exceeding 1500, an [aIn of 177O, and a cupric reducing power varying between 11 and 20 per cent. of maltose. This dextrin, which is not identical with the ‘‘ stable dextrin” of Brown and Millar (T., 1899, 75, 315), constitutes about 1 /5th of the conversion products, from which crystalline malt,ose was also isolated, and a dextrin or dextrins of the sane molecular weight and optical activity as maltose, but of much lower cupric reducing power.When the time of conversion exceeds three or four days dextrose is produced. DISCUSSION. Dr. PLIMMERpointed out that French observers consider that starch granules consist of two constituents. The formation of small quantities of dextrose by the action of malt diastase might arise from one of these two constituents, and not from the other, which yields only maltose on hydrolysis. In reply, Mr. BAKERsaid that he did not think that Maquenne and ROUX’S differentiation of the starch granule into amylocellulose and amylopectin affected the question of the formation of dextrose.If the dextrose were derived directly from one or other of these substances, it would be reasonable to expect its production at once, but the experimental evidence was against this. It was more prob- able that the dextrose was formed by the slow hydrolysis of some of the dextrins of low molecular weight present in the conversion products. “118. The atomic weight of lead from Ceylon thorite,” (I By Frederick Soddy and Henry Hgman. Recent; results in radioactivity suggest that the lead derived from a mineral rich in thorium and poor in uranium may have an appreciably higher atomic weight than that of ordinary lead. If the end products of both uranium and thorium are, as is supposed, the isotopes of lead, the former should have an atomic weight of 206 and the latter of 208‘4,.whilst the accepted value for ordinary lead is 207.1. Ceylon thorite is uniquely suited for an experi-mental test of the question. The original analysis (W. R. Dunstan, Ceylou .iiii~erulogicnl Survey Report, March 31st, 1904) gave 58.24 per cent. of thorium, 0.38 per cent. of uranium, and no lead. The authors’ analysis gave 0.35 per cent. of lead and 54.5 per cent. of thorium. Whereas tlie chemical estimation of the uranium gave 0.72 per cent., a later preliminary estimation of tlie radium by the emanation method showed more uraiiium, namely, 1.6 per cent., and this is probably the more accurate.Owing to its greater rate of change, uranium will be about three times as effective in producing lead as thorium, so that if the lead in Ceylon thorite is entirely of radioactive origin, and if both isotopes are stable, the atomic weight, should be 208.2. Rather more than a gram of the finally purified lead chloride was obtained from about a kilogram of the mineral, and used in the determinations. Exactly similar estimations with it and with ordinary lead chloride, purified by an identical series of processes, have showii that tlie thorite lead has distinctly the higher atomic weight. The determinations are purely relative, the atomic weight of ordinary lead being taken as 207.1. The method adopted followed, in part, that of Baxter and Wilson.The lead chloride was fused in liydrcgen chloride befcre weighing, and its solution titrated with silver nitrate solution, the end point being determined without an indicator by the cloud method. Two separate deter- minations showed a difference of between 0.4 and 0.5 per cent. in ’ tlie volumes of the silver nitrate solution required by equal weights of the two chlorides, whereas the errors of the estimation do not probably exceed 0.1 per cent. The relative atomic weight of the thorite lead calculated from the results is 208.4. The cletermina- tioiis so far carried out do not suffice to settle the question, but they show clearly a difference in the expectgd direction of the right order of magnitude. From a preliminary examination with the Fgry spectrograph, the spark spectra of the two specimens of lead, between 6656.3 aiid 2170, appear to be identical, except for the line 4760.1, wiiich is much weaker iii the thorite lead than in crdinary lead.“119. A criticism of the hypothesis that neutral salts increase the dissociation of weak acids and bases.” By James William McBain and Frederick Charles Coleman. It was shown that if the hypothesis of Acree, Bredig, Snethlage, etc., is accepted, namely, that undisscciated hydrochloric acid catalyses the inversion of sucrose better than hydrogen ion, and if, further, the data of A. A. Koyes and his collaborators are employed, not only do the data of Arrlienius (1899) fcs the accelera- tion caused by adding a neutral salt to a weak acid fail to prove 136 that the dissociation-constant of the weak acid is enhanced by the presence of the neutral salt, but they niay even be adduced as strong evidence against the existence of such an effect.It was further pointed out that iiiucli of the evidence brought in support of the enhancement hypothesis is derived from methods often subject to grave systematic errors, involving, for instance, colour changes in colloidal or electrolytic colloidal systems, or dis-tribution data-methods wliicli are kiiown in some cases to give highly distorted results. Here the results are conflicting in order of magnitude, and even in sign. The evidence of electromotive force measurements is also uiif avourable to the hypothesis.The authors conclude, therefore, that on the whole there is no experimental evidence for the supposed increase in the dissociation- constant of weak acids and bases caused by the presence of neutral salts. 120. Studies in substituted. quaternary azonium compounds containing an asymmetric nitrogen atom. Part 11. Resolution of phenglbenzylmethglazonium iodide into optically active components.” By Bawa Hartar Singh. The author, in continuation o€ his work (T., 1913, 103,604), has prepared externally compeiisated pheiiylbenzylmethylazonium iodide by two different methods, namely, (i) by the action of mekhyl iodide on plienylbeiizylhydraziiie, and (ii) by the action of benzyl iodide 011 phenylmetliylhydrazine. In the second reaction there is also produced, owing to substitution having taken place, benzyldimethplazoiiium iodide, (C,H,)(CH,),(NH2)NI. The resolution was effected with the aid of cl-camphor-P-sulphonic and d-a-bromocamplior-j3-suIphoiiic acids.In each case the first fractions consisted of pure dBdA corripoiieiit ; in the last fractions ths two component salts dEdA and tBdA formed solid solutions. The lBdA component could not therefore be obtained in a pure state, and the process of resolutioii was very slow and partial. KO mutarotation was observed in the case of aiiy of the com-pounds obtained. Several salts of the externally compeiisated and optically active azonium base were described. 121. ‘.Contributions to the chemistry of the terpenes. Eart XVII. The action of hypochlorous acid on camphene.” By George Gerald HBnderson, Isidor Morris Heilbron, and Matthew Howie. When treated with dilute aqueous hypochlorous acid camphene gives a quantitative yield of a chlorohydrin, C,,H,,Cl*OH, a crystalline solid.m. p. 93O. This compound reacts readily with 157 aqueous or alcoholic alkalis, yielding isocamphenilallaldehyde, and by the action of phosphorus pentachloride is converted into cam-phene dichloride, C30H16C12. isoBorneol is obtained by the action of zinc and alcohol on the chlorohydrin, which therefore is a chloroisoborneol. On oxidation with chromium trioxide the chloro- hydriii is converted into a crystalline chlorolteto~ie,C,H,,Cl:CO, m. p. 133O, which gives camphor when heated with zinc and alcohol.122. ‘‘Reactions by trituration ” By Leslie Henry Parker. It has been shown by Carey Lea (Phil. Xog., 1892, [v], 34, 46; 1893, 36,351; 1894, 37,31, 470) that shearing stress is capable of “ disrupting the molecule ” of many endothermic compounds, being far more efficient in this respect than simple pressure of enormous magnitude. This fact, combined with the results of Spring’s work on the sulphates and carbonates of sodium and barium (Bull. SOC.chin>., 1885, fiii], 44, 166; 1886, 46, 299>, was the cause of the present investigation into the interaction of various salt pairs, presumably in the solid state, by trituration. Various pairs of salts were thoroughly dried, and ground together in a dry atmosphere.In most cases mutual action took place very easily, but not always. It was noticed that those substances which reacted most easily under the pestle were those which were easily fusible in ordinary circumstances, and vice versa. and the author arrives at the same conclusion as Johnston and Adams (Amer. J.Sci., 1913, [iv], 35, 305‘).that shearing stress, or (‘non-uniform ” pressure, C~USPSlocal or surface fusion of the substance to which it is applied-. It call also be sliowii that the action of shearing stress is funda- inelitally different from that of simple pressure, the chief difference lying in the fact that the products of any reaction occasioned by shearing stress are not necessarily denser than the reacting sub- stances. Experiments ha.ve also been conducted with the object of determining whether the trituration caused any ionisation of the atmosphere round the ground substances, but without success.123. ‘‘The reaction between dilute acid solvents and soil phosphates.” By James Arthur Prescott. The author has investigated tlie action of dilute acid solvents on soil with respect to tlie ainount of phosphoric oxide extracted. The extractions were inatie at’ constant tenperatnre fcr varying lengths of time, and with initial co:~centratioiis of from 0.06 to 0.3 equivalents of acid per litre. The amount of phosphoric oxide extracted is approxiniately pro- portional to the initial strength of the extracting acid. With nitric, hydrochloric, and sulpliuric acids, an increase in the time of extraction brings about a decrease in the amount of pliosplioric oxide extracted.With citric acid the reverse is the case. The amount of acid neutralised by the soil increases with tlie time of extraction, but an excess of acid always remains, large in proportion to the amount of phosphoric oxide preseiit. The greatest diminution in the quantity of pliospliate extracted with increase in time of extraction occurs with soils containing the highest proportion of clay. It is difficult to account for the removal of the phosphoric oxide from the solution on chemical grounds in view of the large excess of acid present, and the pheiio- mena were therefore studied from tlie point of view of adsorption. The results obtained by Hall and Amos (T.,1905, 89, 205) were found to agree with tlie adscrption relationsliip established by Freundlicli : Y/ltr=KC' 1') where Y =amount adsorbed by a quantity 21 of adsorbent, and C=equilibrium concentration of the solution.For the Saxmundliam soil p=O-58; for the Broadbalk soils (5 and 8) p=1*63; for tlie Hoos soil (2AI4) p=1.414. In these results, a correctioii has to be made for the amouiit of phosphate still left in the soil. The author has further investigated this point by adding known amounts of phosphate to a soil, and the curves obtained led to tlie conclusion that tlie amount of phosphate originally present in the soil, and soluble in liydrocliloric acid, tvvas the same as tliat soluble in citric acid. For a soil from Agdell field, which had already been extracted twice with dilute acid, 1) was found to be 1.96 for hydrochloric acid, 0.06 ec,uivalent per litre, and 0.485 €or citric acid of the same acidity.The same soil was also extracted seven times iii succession with 2 per cent. sodium hydroxide, and was found to contaiii no phos-phate soluble in dilute acid solvents. Adsorption experiments could therefore be carried out without any correction whatever. The Freundlicli law was found to hold, giving a value of p=2-32 for hydrochloric acid and 2.08 for citric acid. 139 124. “Influence of the dilution of hydrogen peroxide on the velocity of precipitation of manganese from ammoniacal solutions in presence of zinc.” By Andrew Jamieson Walker and Walter Parmer.A study of the effect of dilution of the hydrogen peroxide on the accuracy of the results obtained in Jannasch’s method for the separation of manganese and zinc in ammoiiiacal solution has shown that with a time-limit-of thirty ~ninutes precipitation of the man- ganese as MnO(OH)2 is complete with solutions of hydrogen per- oxide of 2.5 per cent. strength. More concentrated solutions of the peroxide, tip to 6 per cent., are equally efficacious. When the concentration is beiow 2.5 per cent., the manganese is not com-pletely precipitated within the time indicated, the percentage error increasing in a marked degree with increase in the dilution. With snch dilute solutions the mmganese is precipitated as carbonate along with the zinc, so that under these conditions the percentage results obtained for zinc are too high.The influence of the dilu- tion can be graphically represented by plotting curves with the percentages of hydrogen peroxide as abscissze, and the percentage yields of inangano-manganic oxide and of zinc carbonate as ordinates. The table gives the results obtained in a series of nine experi- ments. 0.4142 Grain of >~nS0,,4H20should give 0‘1417 gram of 31n304, and 0.4142 gram of ZnS04,7H20 should gl.;e 0.1806 gram of ZnCO,. This quantity of the salts was eiiiployed in each deter- mination. The experimental error is much magnified by transla- tion into percentage yield. Percentagestrengthof H,O,. Mn, 0,. Gram. Percentageyield of Ah<0,.ZnCO,. Gram. Percentageyield of ZnCO,,. 6.0 0.141 1 99-69 0.1815 100-53 5.0 0.1410 99.51 0.1815 100.53 4.0 0.1410 99-51 0.1815 100.53 3-0 0.1410 99.51 0-1816 100.59 2.0 0.1409 99.42 0.1817 100.61 1.0 0.1381 97.51 0.1861 103.99 0.76 0.1345 94.93 0.1915 105.99 0.5 0.3 0.1297 0-1151 91.56 81.25 0.1995 0,2206 110.49 122.19 The zinc carbonate precipitated in the 6-2 per cent. separations was quite white. As the dilution was increased, it developed a distinct light-brown tint, due to the presence of manganese. Within the limits of experimental error, the deficiency in the per- centage yields for manganese is balanced by the excess in the corresponding yields for zinc. The results indicate that in the separation of manganese and zinc 140 in amnioniacal solution, hydrogen peroxide of not less than 2.5 per cent.strength can be employed with satisfactory results (compare Jannasch and MacGregory, J. pr. Chem., 1891, [ii], 43, 402; Jannasch and Niederhofheim, BPT.,1891, 24, 3945 ;Jannasch and von Cloedt, Zeitsch. otiorfy. Chetn., 1895, 10,405; Jannascli and Lehnert, ibid., 1896, 12, 134 ; Jannascli, “ Gewichtsanalyse,” Leipzig, 1897, 43). 125. “ Additive and substitutive compounds of mercuric nitrite with organic thio-derivatives, Part I.” By Prafulla Chandra Rly. Mercuric nitrite yields with methyl and ethyl mercaptans com-pounds of the type (R-S-HgNO,),,Hg( NO,),,H,O, where R repre-sents an alkyl group. With the substituted carbamides it forms compounds of the general formula : NIIROC(: NII ) -SoHg NO,, 2HgS,HgO ; with thioacetamide and beiizamide, nitribs of the type : CR( :NH)*S-HgNO,,HgS,HgO (R=alkyl or aryl) ; and with thioacetic acid a salt of the formula : CH,*CO*SH,Hg(NO,),,HgS,HgO.The compound with thiosemi-carlnazide has the formula : 2NH,.NH*C(:NH)*S*HgNO,,HgO,R,O, and that with dithiocarbamic acid NH:C(S-HgKO,),,HgS. With the thiocarbimides, also, compounds having the general formula R.N:C~*Hg(N02!,,2HgS,~~~0have been obtained ; that with ethyl thioether has the formula 2Et&3Hg(NO2),.It is found that whenever a thio-compound tautomerises giving the thiol group [for example, CH,*CS-NH, -+CH,*C(SH):NH] the first reaction is as follows : *SH+ Hg(NO,), = =S-HgNO,+ NHO,. 126.‘‘ The reactivity of antimony haloids with various types of unsaturated compounds. Part I.” By Ernest Vanstone. The eight 6inary systems formed by s-diphenylethane (dibenzyl), stilbene, azobenzene and bend, and antimony trichloride and tri- bromide respectively have been investigated by thermal analysis. s-l)iplienyletliane forms the compounds 4SbC1,,C,,Hl4, 2SbCI,,C,,H,, and 4SbBr,,C,,H,,. Stilbene forms the compounds 2SbCl,,Cl,H14 and 2SbBr3,C,,H,,. The compounds with s-diphenylethane are stable ; those with stilbene are unstable, and difficult to obtain. The tendency is to give a thermal diagram, showing a single eutectic point. Azobenzene forms the compounds 4SbCI3,C,,H,,N, and 4SbBr,,C,,H1,N,.These compounds can only be obtained by seeding the fused mixture with some of the compound which had been prepared previously. Benzil does not combine with antimony haloids. The order of diminishing reactivity with antimony haloids is s-diphenylethane, azobenzene, stilbene, benzil. It was shown that the magnitude of the optical exaltation increases in the same order. The effect of increasing the number and position of phenyl groups and also of carbonyl groups on the reactivity with antimony haloids was discussed, and shown to be in agreement with the exaltation of molecular refractive power. In all cases conjugation diminishes the reactivity with antimony haloids and increases the exalt’ation. Thermal analysis thus provides a useful method of tracing the conjugation of the residual aflinity of the unsaturated atoms and groups CH:, N:, CO, with tlie phenyl groups in compounds of the type Ph .a.a.Ph.127. (( The absorption spectra of various substances containing two,three, and four benzene nuclei.” By John Edward Purvis. The author has carried out an investigation of substances containing two, three, and four benzene nuclei united either with simple aliphatic residues or with inorganic radicles or elements, to see how far and in what directions the vibrations of the various centres influence the absorption phenomena, and particularly as regards the effect on tlie benzene bands. The sub-stances examined were : s-and os-diphenylcarbamides, s-dibenzyl- carbamide, s-diphenylthiocarbaniide, triphenylguanidine, phenyl diphenylcarbamate, tribenzylamine, diphenyl phthalate, triphenyl- acetic acid, tribenzoin, triphenylphosphine, triphenpl phosphate, tri-o-tolyl phosphate, tri-p-t oly1 phosphate, and tetrap heny lsilicane.128. &‘ Kinetics of the decomposition of acyl derivatives of phenols by means of alcohol in presence of acids and alkalis.” (Pre-liminary note.) By Xarian Jones and Arthur Lapworth. The abstract of a paper by McCombie and Scarborough on “The velocity of saponification of the acyl derivatives of the substituted phenols” has recently appeared (this vol., p. 107). The present authors have been engaged for more than a year on certain aspects of the subject, having taken up the work primarily with the object of throwing further light on the mechanism of the acid hydrolysis of esters.142 Phenyl acetate has been most closely studied, special attention having been paid to the catalytic influence of acids and alkalis on the decomposition which it undergoes in alcoholic solution. With both agents the main reaction in the first instance consists in the irreversible formation of free phenol (or alkali phenoxide) and et\hyl acetate, so that complete saponification is largely the result of two successive reactions, the second being saponification of ethyl acetate complicated by the formation of phenoxide. The present authors have studied only the speed at which the first reaction takes place, by estimating the amount of phenol (or phenoxide) formed after varying periods.The influence of free phenol or phenoxide in excess has also been examined. Both acids and alkalis greatly accelerate the speed of the first reaction, and the relative influence of the two types of agent is of the same order of magnitude as in the case of tlie hydrolysis of alkyl esters, and there is therefore no reason to suppose that the mechanism of hydrolysis is different in phenyl and alkyl esters. As phenyl is not detached from oxygen unless under conditions of exceptional severity, it must be concluded that hydrolysis of an ester, whether by acids or alkalis, involves the severance of the molecule at the point (l),and not at (2): X*CO-0-A1 k, (1) and the analogy to ainides and allied compounds is complete.It is now fairly generally agreed that during hydrolysis and esterification by acid catalysts a complex (ionised or non-ionised) of catalyst and the two principal reacting components is formed which may decompose so as to yield carboxylic acid and alcohol or ester and water (and catalyst) on tlie other. The symmetry of the reactions, combined with all the data now available, suggests that the hydrogen atom in the ‘I polymolecule” is labile, in the intramolecular sense, and ma.y be regarded as influenced by all three oxygen atoms. The authors venture to suggest that the symbol -which is not inconsistent with modern views on valency, is the most satisfactory one that can at present be devised for the hypo- thetical. complex obtained during the hydrolysis of ethyl acetata by aqueous hydrochloric acid.The work on the kinetics of the decomposition of phenyl acetate is being continued by one of the authors (M. J.), and examina- tion is also being made of the applicability of phenyl acetate as an acetylating and dehydrating agent. 129. The alloys of aluminium and silicon.” By Charles Edward Roberts. A re-investigation of the thermal diagram of the aluminium- ailicon alloys in order to determine the possibility of the existence of either a compound of the two elements dissociating at high temperaturzs on an allotropic form of silicon stable above 1200°, resulted in a complete confirmation of the results arrived at by Fraenkel (Z~ifsch.utzorg.Chem., 1908, 58, 154), that the alloys form a simple eutectiferous seriee, tlie eutectic melting at 578O. 130. “The constitution of camphene. Part XI. Experiments on the synthesis of several degradation products of camphene.” By Walter Noxmm Haworth and Albert Theodore King. An account was given of the condensation of ethyl oxalate with ethyl as-dimethylsucciiiate in the presence of potassium or sodium ethoxide, and of tlie synthesis of the lactonic acid (IV) through the following st ages : 9H2*COCl yH,=CO*C)H(C0,Er )B vH2-C( 0H )( C0,Ec ) CH (C0,E t)2 CMP,*CO,Et CBfe2*C0,Kt CRIe,*CO,Et (1.1 (11.) (IIr.) yH2*C(CO,H)(CH,*CO,H)CMe; --CO>O. (IV.) Attention was directed to tlie fact that a coiiiylete synthesis of campliene has now been realised by the combined experiments of several independent workers.Caniplienic acid and cainphenilone having now been synthesised (Uer., 1914, 47, 871, 934), this, con- sidered along with the earlier work of Rloyclio and Zienkowski (BET.,1905, 38,2461 ; ,1nircileu, 1905, 340, 58) on the preparation of camphene from camphenilone, establishes finally the constitution of this terpene as represented by Wagner’s forinula. 131. L6 Action of nitrous acid on dimethylpiperazine.” By Prafulla Chandra Rty. In continuation of previous investigations on the amine nitrites, attempts have been made to isolate an aniine dinitrite. When ethylenediainine hydrochloride or hydrobromide was treated with silver nitrite, it was noticed that even during the initial stages of 144 reaction slight decomposition often set in, with evolution of nitrogen and formation of glycol and ethylene oxide.The aqueous filtrate, on evaporation in a vacuum, gave a non-crystalline residue, which did not dissolve to a clear solution, and on evaluation by the Crum-Frankland and “ urea ” methods, respectively, gave, as a rule, an appreciable excess of gas by the former, proving the conversion of a certain proportion of nitrite into nitrate. In two preparations, however, the nitrogen, as estimated by both the processes, agreed well : (1) 0.0214 gave 2.1 C.C. N,(“nitritic”) at. 24O and 760 mni. N=11*0. (2) 0.025 gave 3.6 C.C. h’,(“nitritic”) at. 23O and 760 mm. N =11-34 The result.approximates to a mononitrite, C,H,( NH,)2,1XN0, which requires N(“ nitritic ”) =13.08 per cent. That the per-centage of nitrogen actually found is lower is easily accounted for by the fact that there is always a slight insoluble residue. It has already been shown (P., 1912, 28, 258) that whilst benzyl- ethylammonium nitrite can be isolated in a crystalline forin, the corresponding methyl compound decomposes even in aqueous solu- tion, mainly into the nitroso-derivative, and that after some time equilibrium sets in, thus : C,Hi-NHMe,HNO, C,Hi*NMe*NO+ H,O. It has now been found that by using an alcoholic solution of the aniine hydrocliloride, this reverse change is completely ari ested. The alcoholic solution, when evaporated in a vaciiuiii over sulphuric acid, yields a crystalline inass, which is Z, c )I z?/?niet ltyL ammonium nityite : 0.0294 gave 2.46 C.C.N,(“nitritic”) at 33O and 76G mm. JS =8.94. C,H,,N,HNO, requires N =8-33 per cent. An alcoholic solution of piperazinium chloride, when similarly treated! gave a salt approxiniatiiig to a dinitrite. It was thought that dimethylpiperazine might yield better results, and this ex-pectation has been realised. The base chosen was a-2 : 5-dimethyl-piperazine, which Pope and Read’s recent investigations prove to have the tmizs-configuration (T., 1912, 101, 2325 ;1914, 105, 219). The aqueous solution of the hydrochloride, on treatment. with silver nitrite and evaporation of the filtrate in a vacuum, gave a crystalline salt, which was fouiid to be ?zitrosoctintethy?kipel.nzi,2ium nitrite, ~o*h-<CHBfe*CHCH,*CHMe”>KH,HNO,. 0.0286 gave 7.3 C.C.NO at 26O and 760 mm. by the Crum Frankland method, whereas the “urea ” test liberated only half the amount of nitrogen (compare T., 1913, 103, a), whence N =14.66. C6Hl3OX3,HKO2requires N =14.74 per cent. It should be mentioned that the aqueous solution of piperaziiiium chloride, by treatment as above, gave dinitrosopiperazine in the first two or three crops. The introduction of the two methyl groups in the ring had the desired effect of diminishing the tendency towards the formation of the nitroso-derivative. Dirnethylpiperazinium chloride in alcoholic solution was nest treated with finely powdered silver nitrite.Although both the reacting substances are very sparingly soluble in alcohol, the in- creased solubility of silver nitrite in the presence of an ainine nitrite (due, no doubt, to the formation of a double salt) facilitates the double decomposition. The alcoholic filtrate was evaporated in a vacuum, and the crystalline salt which was thus obtained was found to be a dinitrite, as both by the Crum-Franklaiicl and the ((urea” process it yielded the sanie amount of nitrogen: 0.023 gave 2.7 C.C.N2(“nit\ritic”) at 30° and 760 inin. N=13*33, 0.0764 (by combustion) gave 18.0 C.C. N2 at. 26O and 760 inin, N=26.41. C6H,,N,,2HT(LT0, requires N(“ nitritic ”) =13.46, and K(tota1) = 26.92 per cent. Conductivity measurements also bear out that the one is the nitrite of a nitroso-aerivative and the other a dinitrite (compare T., 1912, 101, 1555).ili’itrosodinz e thylpipernzitiiu m nitrite : v.......... t.4 .......... 252.1 93’5 504.2 102.7 1008.4 114’5 2016,s 120’7 In this case there are only two univalent ions. Dirnet hylpiperaziniu1tL ditLit rite : V.......... 200.3 400.6 801‘4 1602.4 p. ......... 210.3 225-4 237.2 241.1 Evidently there are three ions in solution. The measureinents were conducted at 25O. 132. ‘(Partially methylated glucoses. Part 111. Monomethyl, glucose.” By James Colquhonn Irvine and Thomas Percival Hogg. Monomethyl glucose has been prepared from glucosediacetoae on a sufficiently large scale to permit of the a-and B-modifications being isolated in pure stereochemical forms. 9s the inter- 146 conversion a /3 proceeds extremely slowly in pure methyl alcohol, it lias been possible to determine the initial specific rota- tion of each form of the sugar with a high degree of accuracy.The mutarotatory chaiiges observed were : a-Form (ni. p. 160.5-161°). @Form (m. p. 133*5--135O). Initial [aID+ 10'7*Go--f 68*5O, 68.3O +-+ 24.4O initial [aID. L.4 The difference of tlie molecular rotations of the a-and &forms thus equals 16141, and as tlie corresponding value for glucose is 16200, the result agrees with Hudson's rule (J. An!rr. Chenz. SOC., 1909, 31,66) within the limits of experimental error. It lias been found that moiiometliyl glucose yields few character- istic derivatives, and its metliylglucosides, in view of the spatial distribution of the liydroxyl groups, fail to enter into condensa- tion with either acetone or benzaldehyde.A well-defined mono-methyl glzicosea?iilide was, however, isolated (m. p. 154-155O). This coinpound shows suspended mutarotation in a remarkable degree, and the optical change [a]D-108*50 + -50-3O was only promoted by traces of acids, and not by alkalis. The constitution previously assigned to nionoiiiethyl glucose has been confirmed, as, on oxidat-ion with nitric acid, the sugar is con-verted into nioiioineth,t/l //litcoirolnctotie, thus indicating that the rnethoxyl group is attached to a terminal carbon atom. The sugar is not' fermented by living yeast, or by yeast' extract, and is UM-affected by most bacteria wliicli attack glucose.The action of B. Clocrcae (Jordan), however, resulted in the formation of both acid and gas, but tlie reaction proceeded mucli more slowly than in the case of glucose. 133. ('Studies in the diphenyl series. Part VI. The configuration of diphenyl and its derivatives." By John Cannell Cain and Frances Mary Gore Micklethwait. It lias been found that benzidiiie and tolidiiie condense with reagents for ortho-diamines, sucli as benzil and glyoxal, to form compounds of tlie type (&H,*N:YR C,,H4=N:CR (where R=H or C,H,). This reaction appears to prove that Kaufler's stereocliemical con- figuration of meiiibers of the diplieiiyl series is correct.134. “Studies in the diphenyl series. Part VII. Isomeric 0-and m-dinitro-0-tolidines.” By John Cannell Cab and Frances Mary Gore Micklethwait. In addition to the o-dinitrotolidine (m. p. 270O) described by Gerber, the authors have obtained, by the nitration of diacetyl-tolidine, a new isomeric o-cliiiitrotolidirie (m. p. 202-203°). By the nitration of tolidine sulphate or dipl~thalyltolidine there are formed, in addition to Gerber’s m-dinitrotolidine (m. p. 217O ; obtained by him from tolidinem sulphate), three new m-dinitro-tolidiires, melting at 205--206O, 263O, and 284O respectively. These four bases are represented by the plane formulze: (-4.) (Cj (D.) and the possibility of-the separate existence of A and B and of C and D, as well as of the two isomeric o-dinitrotolidines, is readily explained by means of Kaufler’s stereochemical formula for diphenyl.135. (( Thio-derivatives of P-naphthylamine.” By William Reeve and Samuel Smiles. The substances here described were obtained in some experiments which had been undertaken with the object of synthesising afl-naphthathiophen. The results are now published, since the scheme has been abandoned on account of the extremely poor yields of the essential products. Binzet hyl-fi-tiophthylamiii e siilphide, NR;Ie,*C,,H,= S*C“,,H,*NMe,, was obtained by treating three molecular proportions of dirnethyl-P-naphthylamine dissolved in light petroleum with one molecular proportion of sulphur chloride. The. insoluble hydrochloride of dimetlryl-P-naphthylamine separated, and when this had been re-moved the required substance was isolated by spontaneous svapora- tion of the solution.After recrystallisation from hot alcohol, it was obtained in very pale yellow needles, which melted at 145O: FOU11d, S=8.4. N =7.2. C,,H,,N2S requires S=8.6 ;IS =7.5 per cent. 148 Di-/3-/jtrp?it?iglccnz it? e szclph ide, NH,*C,oH,*S*C,,H,*NH,, was obtained by treating B-iiaplitliylaiiiine in nitrobeiizeiie solution at 160° with sulphur iii tlie presence of lead oxide. The solvent. was removed in a current of steam, and the residue was dissolved in acetic acid. Kater was then added to this solution, and the amorphous precipitate which separated was collected and dissolved in ether.By spontaneous evaporation of the solvent the sulphide was deposited in ail impure condition. It separated froin solution in hot alcohol in colourless needles, wliicli melted at 166’: Fouiid, S=lO.O and 9.8. N=8*6 aiid S.7. C,,H,,N,S requires S =10.1; N =8.86 per cent. When dissolved in hot aqueous mineral acids, tlie substance was readily osidised by atmospheric oxygen, an insoluble, blue inaterial being formed. The yield of the sulphide obtained by this method varies coil- siderably, not only according to tlie cuaiitity of the reagents taken, but also according to other conditions, which have iiot yet been determined. In the majority of experiiiieiits the yield was extremely poor, aiid in these cases it is difficult to separate the substance from the polysulphides which are always formed.These compounds-the cli-and tri-sulpliides--have not been closely examined. 136. ‘‘The interaction of naphthasulphonium-quinoneand substances containing the thiol group.” By Brojendrmath Ghosh and Samuel Smiles. A description was given of the reaction of certain tliiol deriv- atives with P-iiaplitliacr_uiiioiie aid P-naplitliasulphoiiium-quinone. From the last-nained cjuiiioiie, thioI and tliioglycollyl derivatives of diuaphtliathioxin were obtained. The action of alkali with these substances and with hydroxydinaplitliatliiosili was examined in order to deteriiiiiie whether isomeric change could be induced, as in the case of the isosulphide of P-naphthol. The results were negative.137. “The formation of heterocyclic compounds from hydroxy- methylene ketones and cyanoacetamide.” (Preliminary note.)By Hemendra Kumar Sen-Gupta. 1ETyclrol;yiiiet~iyleiie-ketoiies condense readily with cyaiioacetamide in tlie presence of piperidine 0:’ diethylamine, giving rise to hetero- cyclic Coi~ipounds ; in the case of open-chain hydroxymethylene- ketones, liydrosypyridiiie derivatives are obtained, whilst with 149 hydrosynlethylene-cycloketones, substarices are produced which may be either quinoline or isoquinoline derivatives, according as to whether the condensation commences at the forinyl carbon atom or &he ketonic carbonyl of the hydroxymethylene compound. CH, CH /\/\ VH2Y $!H*CN CH, CO ClI,C Cd i-2HZO \/ \/\/ CH2 CH, N CH, CH /CN-CH, In addition to these coiidensatioii products whicli are formed by the eliiniiiation of two molecules of water, there is evidence of the formatioil of a second type iii which oiily one molecule of water is eliminated : CH, CH, C'H*OH /'\ /\/\7k1, YH*CHO y H2 - C;H2 ?!I 8 + H,O.+ CH, co CO CH, C C*OH \/ / \/\/UH, C"*C'H, CH, C*CN In some cases, this intermediate type lias been isolated by careful crystallisation.Since a well-defined acid is obtained by hydrolysiiig either of the coiidensation products thus produced, there is little doubt as to the similarity of their structures. In a few cases the final products which are deposited from the coiideiisiiig mixture have been found to be those condensation products which have lost two molecules of water.The following coinpouiids have been obtained : (1) Ethyl hydroxyiiiethylene-ethyl ketone, C,H,*CO-C(CH,) :CH*OH, gives with cyanoacetaniide a iiiisture of coiideiisation products which, on hydrolysing, yields an acid,C9H,,0,N (in. p. 278-279O) ; this evolves carbon dioxide on melting, and passes into the com-POZLILCZ, CSH,,ON (in. p. 136-138O). (3) Hydroxyllzethyleiiecyclohexanoiie yields the condensation products CloH100N2 (in. p. 250') and C,,HI2O,N2 (melting above 300O). Both conzpou~zds,on hydrolysis with SO per cent. sulpliuric acid, give the same acid, C,,H,,O,N (m. p. 265O), which evolves 150 carbon dioxide on melting, and passes into the compound CSHl1ON (m.p. 204O). (3) 2-Methylhydroxymetliylenecyclohexanone gives the com-pound, C,,H,,ON, (m. p. 242O), which, on hydrolysis, yields the‘ acid, C,,H130,N (m. p. 260O); this loses carbon dioxide, and forms the cornpozind, C,,H,,ON (ni. p. 142O). (4) 4-Methylhydroxymethylenecyc~oliexanone gives the com-pound, C,,H,,ON, (m. p. 228-229O), which is liydrolysed to the acid, CliH1303N (m. p. 284O), and the latter yields tlie CO~~OZCI~~, C,,H,,ON (m. p. 206--207O), with loss of carbon dioxide. Experiments with the object of elucidating the constitution of this class of compounds are in progress. 138. ‘(Studies of ammonium solutions.” A correction. By Roland Edgar Slade. In a former communication it was shown that the potential of an aminoniuni electrode at’ 25O was given by the equation: The value of e,was calculated to be -0.486 volt from twelve independent measurements. It has been pointed out.to tlie author by Prof. Auerbach that, in calculating these values of eo, tlie pressures of ammonia were, by mistake, expressed in mni. of mercury instead of in atmospheres. This mistake has now been corrected, and tlie values have been revised in accordance with the later value fur the potential of the. normal hydrogen electrode, The revised value of eo is -0.654 volt. This value has been compared with other data, and fcuiid to be in excellent agreement. 139. (( Thujin.” By Arthur George Perkin Roclileder and Kawalier (Fien. L41,ud.Uw., 1858, 29,10; J. pr-Ghem., 1858, 74, 8) isolated from the arbor vitz (Thttja occideii trtlis) in minute amount a glucoside, tliu jin, C2,H~,0,,, which by hydrolysis yielded dextrose and thu jigenin, Cl,41Tl,07,the latter subsequently passing into tliujetin, C,,H,,O,.Tliu jigenin and thu jetin are described as yellow, crystalline substances, soluble in alkalis with a green colour, and in alcoholic ammonia with a bluish-green coloration. A re-esaiiiination has now shown that thujin is, in reality, quercitrin contaminated with a trace of a second glucoside, and that tlie green tint of tlie alkaline solution of tlie free colouring matter clriginates from the latter compound. It is possibly a glucoside of myricetin (T., 1899, 75, 829), but the 151 amount present in the material now examined was far t~osmall for identification.Incidentally, it has been found that quercitrin melts at 183--185O, much higher than has been usually supposed (compare Herzig, Monatsk., 1885, 6, 877), that the formula C21H2201,, assigned to it previously, which it is found to possess when dried in the air or at 100°, is, in reality, C21H2,011,H,0, and that it niay be obtained in the anhydrous condition when heated at 160O. 140. The rotatory powers of d-and I-isoamarine and of their respective tartrates." By Henry Lloyd Snape. In a previous paper on "Racemic and optically active forms of amarine" (T., 1900, 77, 784; see also this vol., p. 7), the density was inadvertently omitted in the calculation of rotatory powers.Redeterminations were subsequently made, and the missing factor was included. As before, the bases were dissolved in ethyl acetate, and the tartrates in 90 per cent. alcohol. Each determination of the angle of rotation was made by taking the average of a number of rotations (which fluctuated slightly and irregularly-sometimes falling and then rising, and sometimes con- versely) measured at the same time on successive days. The follow- ing are the results obtained: Number of c. [u] de termiiia tious lhxtro-base (C,,H18N,) ......... 4.500 +69 06 3 Lcevo-base ....................... 4 '581 -68.23 2 Ihxtro-tartrate of dextro-base.. 1.357 + 113.95 2 79 laevo-base... 3.377 -93-31 3 As the only polarimeter which was at the author's disposal for the above experiments was a very simple one, and could not be trusted to give very exact measurements, Professor W.J. Pope very kindly undertook to determine [a] in specimens of the dextro- tartrates of d-and Zisoamsrine, and the following are his results, for which the author desires to express his thanks. In each of the following determinations the quantity of the sub- stance stated was dissolved at 20°, made up to 30 c.c., and the solution examined in a 4-dcm. tube at 20°. d-isoA marine d-tartrate, 0.9053 gram in absolute alcohol. Hg violet. Hg green. Hg yellow. Na yellow. a.......... +32.57" f16-56" + 14.18" +13 48" [u] ...... +270 + 137 +117 +112 = 2-4 16 ;Hgg,eeu/NayellowRotat,ory dispersions, Hgviolet/Nareellow = 1.228 ; €1 gyeIlow/Na\ellorv = 1f62.0.3097 in 90 per cent. alcohol by weight. a......... +12*34" +6 '29" +5 '38" +5'12" [u] ......+299 +152 +130 +124 152 Rotatory dispersions, 2.410, 1.229, and 1.051 respectively. 1-isoL4marine d-tartrate, 0.2390 gram in absolute alcohol. a. ........ -7.55" -3.68" -3.15" -3.0;" [u] ...... --237 -115 -98.8 -96 3 Rotatory dispersions, 2.459, 1.199, and 1.026 respectively. It will be observed that the corrected values for tlie 11 line for the tartrate of the dextro-base in 90 per cent. alcohol is 124, which is distinctly higher than was obtained with the imperfect apparatus. Similarly, the value for the tartrate of the lzvo-base in absolute alcohol is somewhat higher than was obtained from a solution in 90 per cent.alcohol. Probably, therefore, the values given abovo for the bases are, like those cited in t,he same table for the tartrates, only approximately correct. ADDlTLONS TO THE LIBRARY. I. Donations. Barger, George. The simpler natural bases. London 1914. pp. vii +215. 6s. net. (h'ecd. 30/4/14.) From the Publishers : Messrs. Longmans, Green & Go. Dunstan, Albert Erfaeut, and Thole, Ferdinand Bsmwd. The viscosity OF liquids. Llndon 1314. pp. viii+91. 3s. net. (Rzcl. 31/3/14.) I'rorn the Publishers : Messrs. Longmans, Green & Co. Hilditch, l'llozrias Percg. A third year course of organic chemistry. The heterocyclic compounds, carbohydrates, and terpenes. London 1914. pp. xii+411. 6s. (Reccl. 25/3/14.) From the Publishers : Messrs.Methuen & Co., Ltd. Imperial Institute, Selected reports from the Scientific and Technical Department. I-V. London 1909-1914. (Recd. 28/4/14.) Reports on the results of Mineral Surveys in Ceylou, SouL1ie:L'iiNigeria, Northern Nigeria, and Nyasaland. London 1905-1913. (IZecd. 28/4/14.) From the Director. Jones, Walter. Nucleic acids, Their chemical properties and physiological conduct. London 1914. PI). viii + 118. 39. 6d. net. (Recd. 30/4/14.) From the Publishers : Mesbrs. Longmans, Green & Go. Lagache, Henri. De l'appri!t, des tissus de laine peignee. Paris 1914. pp. viii+438. ill. 18 fr. (Recd. 4/5/14.) From the Publishers : MM. H. Dunod et E. Pinat. Pickard, Joseph Allen. Modern steel analysis. A selection of practical methods for the chemical analysis of steel.London 1914. pp. viii + 128. ill. 3s. 6d. net. (Recd. 2/4/14.) Prom the Publishers : Messrs. J. & A. Churchill. 153 11. By Purchase. Caspari, William Augustus. India-rubber lab Irntory practic.3. London 1914. pp. viiif 196. ill. 5s. net. (RecI. 24/3/14.} Deutsche Chemische Gesellschaft. Literatur-Register der organ- ischen Chemie geordnet nach N.M.Richter's Formelsystem Edited by Robert Stelzner. Vol. I. 1910-1911. Braunechweig 1913. pp. XI + 1286. (Reference.) Groasmann, H. Die Bestimmungsmet hoden des Nickels uod Kobalts und ihre Trennung von den anderen Elementen. (Die chemiache Analyse, Vol. XVI.) Stuttgart 1913. pp. 140. B4.5.-. (Reference.) Sheppard, SanzueE Edward.Photo-chemistry. London 19 14. pp. xii +46l. ill. 12s. 6d. (Recd. 6/3/14.) Smith, Ernest A. The sampling and assay of the precious metitlh : comprising gold, silver, platinum and the platinum group metals in ores, bullion, and products. London 1913. pp. xv+460. ill. 158. net. (Recd. 11/2/14.) Soddy, Frederick. The chemistry of the radio-elements. Part 11. The radio-element.; and the periodic law. London 1914. pp. iv + 46. ill. 2s. net'. (Eecd. 6/1/14.) Stahler, A?*tl~ur.Handbuch der Arbeitsmethoden in der anorg.\11-ischen Chernie. Vol. 111, Part 1. Leipig 1913. pp. x+ 692. iii. R1.25.-. (Rpference.) Thomson, Sii* Joseph John. Knys of positive electricity and tlicir. :tpplication to chemical analyses. London 1913. pp. viii + 132.ill. 5s. net. (Recd. 13/3/14.) Vanino, Ludwig. [Editor.J Handbuch der praparativen Cheuiic . Vol. I. Anorgauircher Teil. Stuttgart 1913. pp. xx+ 670. 111. h1.18.-. (Idecd. 13/3/14.) Wolbling, H. Die Bestimmungsmethoden des Arsene, Antimotis uiid Zinns uhd ilire Trennuog von den anderen Elernenten. (Die cherrribche Ansly be, Vol~.XVI and XVII.) lap. 377. M. I:<.-. (Il-fe7.e )I ce.) TEE FARADAY LEG rURE. The Faraday Lecture, entitled " Electrolytic Dissociation," will be delivered by Professor Dr. Svante Arrlienius, F.R.S., on Monday, May 25th, at 6 p.m. The Lecture will be given, by the kind permission of the Managers, in the theatre of the Royal Institution, 21, Albeinarle Street, W. Admission will be by ticket only. Each Fellow of the Society is entitled to two tickets, which may be obtained on application to the Assistant Becretary, Chemical Society, Burlington House, W.154 RESEARCH FUND. A meet4ing of the Research Fund Committee will be held in June next. Applications for grants, to be made on forms which can be obtained from the Assistant Secretary, must be received on or before Monday, June lst, 1914. All persons who received grants in June, 1913, or in June of any previous year, whose accounts have not been declared closed by the Council, are reminded that reports must be in the hands of the Honorary Secretaries by June 1st. The Council wish to draw attention to the fact that the income arising from the donation of the Worshipful Company of Gold-smiths is more or less especially devoted to the encouragement of research in inorganic and metallurgical chemistry.Furthermore, that the income due to the sum accruing from the Perkin Memorial Fund is applied to investigations relating to problems connected with the coal-tar and allied industries. At the next Ordinary Scientific Meeting, on Thursday, May 21st, 1914, at 8 30 p.m., the following papers will be communicated : “Ionisation and the law of mass action. Part 111. Utilisation of the osmotic data and a new dilution law.” By W. R. Bousfield. (‘The influence of nitro-groups on the reactivity of substituents in the benzene nucleus.” By J. Kenner. I‘ Some indazole derivatives.” By R. Curtis and J. Kenner. “ The viscosity of sugar solutions.” By H.Green. “ Compounds of phenantliraquinone with metallic salts.” ByJ. Knox and H. R. Innes. “ Quinone-ammonium derivatives, Part 111. Dihaloid, mono-azo-, bisazo-, nitrotriazo-, and bistriazo-compounds. Attempts to prepare derivatives containing an asymmetric, quinquevalent nitrogen atom.” By R. Meldola and W. F. Hollely. ERRATA. PROCEEDINGS,1914. Pap. Line. 6 2 for “Arthur James Meads ” rend “John Arthur Meads.” ‘‘ e>’35 16 77 yead L‘ &’”. 1IX dy R. CLAY AND SONS. LTD.. BRUNSWICP ST., STAMFORD ST., S.E., AND BUNQAI, SUFFOLP.
ISSN:0369-8718
DOI:10.1039/PL9143000131
出版商:RSC
年代:1914
数据来源: RSC
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