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Proceedings of the Chemical Society, Vol. 25, No. 364 |
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Proceedings of the Chemical Society, London,
Volume 25,
Issue 364,
1909,
Page 299-313
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[Issued 30/12/09 PROCEEDINGS CHEMICAL SOCIETY. ~~__ Vol. 25. No.304. ~~ Thursday, December lGth, 1909, at S.30 p.m., Professor HAROLD B. DIXON,F.R.S., President, in the Chair. Referring to the loss sustained by the Society in the death of Dr. Ludwig Mond, the PRESIDENTstated that the Council had that afternoon passed the following resolution : '' The Council of the Chemical Society desire to place on record their profound regret at the death of Dr. Ludwig Mond-a man distinguished no less for his life- long researches in pure and applied Chemistry than for his wise beneficence for the advancement of Science. Dr. Mond was elected a Fellow of this Society in 1872, and served as a member of Council in 1885-6 and as Vice-president from 1887 to 1890, and again from 1894 to 1898.In the present year he was invited by the Council to accept nomination for the Presidency : unfortunately, ill-health prevented his acceptance. The industrial processes which Dr. Mond established and gradually perfected presented chemical and engineering problems only to be solved by a rare combination of scientific insight and of practical skill. The faith of Dr. Mond in well-guided research as the fertiliser at the root of a nation's industry wits shown again and again when he applied his wealth to aid original investigation. Among his generous benefactions to the cause he had at heart, two stand out conspicuously -the fund which enabled the Royal Society to publish its catalogue of scientific papers, and the creation and endowment of the splendid Davy-Faraday Research Laboratory. To his adopted country Dr.Mond's work has been a help and an inspiration; we, his Chemical colleagues, who know what that work was, desire to convey to his famiIy our sense of the loss that science and the country have sustained.” It was further announced by the PRESIDENTthat in view of the completion of fifty years’ Fellowship by the Past Presidents the Rt. Hon. Sir Henry Roscoe, Sir William Crookes, Dr. Hugo Miiller, and Dr. A, Vernon Harcourt, it has been resolved by the Council hhat the Society hold a dinner some time at the end of May or beginning of June, 1910, and that these gentlemen be entertained as guests of the Society. 31r.Harold Baron was formally admitted a Fellow of the Society.Certificates were read for the first time in favour of Messrs. : Percival Frederick Adams, Sl, Rock Avenue, Gillingbam. Alexander Charles Gumming, D.Sc., 39, Viewforth, Edinburgh. Arthur Ernest Everest, B.Sc., Clifton House, Shrewsbury. Aquila Forster, B.Sc., 156, Coatsworth Road, Gateshead-on-Tyne. Charles Wright Meanwell, 15, Woodlands Crescent, Muswell Hill, N. Certificates have been authorised by the Couiicil for presentation to ballot under Bye-lam I (3) in favour of Messrs. : Tarak Nath Das, B.Sc., 31, Bhaironath, Benares City, India. John William McBeath, West End, Kimberley, S. Africa. Of the following papers, those marked * mere read : *285. The pr.oduction of para-diazoimides from alkyl- and aryl-sulphonyl-para-diamines.A general reaction.” By Gilbert T.Morgan and Joseph Allen Pickard. Earlier experiments having shown that many arylsulphonyl-p-diamines yield arylsulphonyl-p-diazoirnideson treating their diazonium salts with aqueous sodium acetate, a further selection of these acylated diamines containing very dissimilar alkyl- and aryl-sulphonyl groups has been examined, with the result that this condensation has been found to be a general one. Benzene-1:3 :5-trisdphonyltri-p-phenyZenediamirze, UGH,(S0,*NHoC6H,.NH~),, was taken as a typical example of a p-aminophenylamide derived from au aromatic polysulphonic acid. When successively diazotised and treated with aqueous sodium acetate, it gives rise to the complex p-diazo- imide, benzene-1;3 :5 -trisuZ~hon.yZtri-p-~~~~~~a~Ze~aed~a~o~m~de, CaH,(SO,*N.CsH;N,),.I I 301 As a type of a diamine containing a mixed aromatic alkylsulphonyl group, toluene-a-suZphonyI -p-phsnylenedic~mine, C,H,*CH, =SO,*NH*C,H,*NH,, was prepared ; it readily yields toluene-o-sulphontyl-p-p?~n~~e~edic~-imide, CSH5*CH2*S02*N*C,H4=N,.1-I The general character of this condensation mas finally demonstrated by preparing the two simplest members of the series of alkylsulphonyl-p-diazoimides, namely, ~etha~sul~hoizyl-p-phenylenedicl~oirnide, CH,*S0,*N*(3,H40N2, I-_ -I and metha~edis.ulp~onyZbis-p-pJ~enylsnediaxoimide, CH,(SO,*N*C,H,=N,),,I 1-obtained respectively from methccnesuZphonyZ-p-phenyleotediamine, CH,*S0,*NH*C,H4*NH2, and methanedisulphonylbiss-p-phenglenediamine, CH,(SO,*NH*C,H,*NH,),.DrscussroN. Dr. MORGAN,in reference to Prof. Armstrong’s expression of opinion that the para-diazoimides mere cquilibrat ed mixtures, said that he should be inclined to regard this serieg, and also the closely allied para-diazo-oxides, as having alternately para-cyclic and para-quinonoid structures : N*SO,Ph AII /I\//\N=N (1). (11.1 were it not for tbe fact that these compounds closely resemble in physical and chemical properties the naphthylene-1 :8-diazoimides (111) and 1 :8-diazo-oxides (IT)respectively. In the absence of evidence concerning the properties of peri-( 1 :8)-naphthaquinone or its derivatives, it seems preferable to regard these 1 :S-naphthylene-diazoimides and diazo-oxides as being cyclic compounds with 6-membered rings (I11 and IT),and thence by analogy to accept formula (I)as representing the structure of the para-diazoimides, lf=N-y S0,Ph Y=N-p C cc HC\/II \ // \c/\II (111.) (IT.) 308 In answer to Dr. Hewitt’s question as to the constitution of non-aromatic diazonium salts, he was of opinion that so long as one of the three phases of the diazonium oscillation could be formulated, the existence of the diazonium salt was possible, although such a corn-pound with only one phase would be less stable than the aromatic diazonium salt with three phases. The dynamic hypothesis of the constitution of diazonium salts would be overthrown by the diazotisation of an amino-derivative of a fully saturated organic complex, but this result had never yet been reslised experimentally.“286. ‘(Organic derivatives of antimony. Part I. Tricamphoryl-stibine chloride and triphenylstibine hydroxynitrate and hydroxysulphate.” By Gilbert T. Morgan, Frances M. G. Micklethwait, and George Stafford Whitby. Comparative experiments on the interaction of sodium camphor and the trichlorides of phosphorus, arsenic, and antimony have shown that, in the last case, the principal product is trica~~~horylstibinechloi-ide, (C,oHI,O),SbC1,, a substance which, although stable in the presence of mineral acids, is readily hydrolysed by aqueous alkalis, and even by moiht silver oxide, into hydrochloric and antimonic acids and camphor.This product is, therefore, much less stable than triphenylstibine chloride, which under similar conditions yields triphenylantinionic oxide. When triphenylstibine chloride is warmed with alcoholic silver nitrate, it loses both its chlorine atoms, and gives rise to triphenyl- stibine nitrate, which is partly hydrolysed by hot water to triphenyl-stibine hydroxynitrate, (C6H&Sb( OH)*NO,, this product crystallising unchanged from boiling aqueous solutions and also from benzene. Triphenylstibine hydroxysulphate, (C,H,),Sb( OH)*SO,*Sb(C6H,),*OH, is similarly obtained by adding tripheny lstibine chloride dissolved in alcohol to a hot aqueous solution of silver sulphate. *287. Lc The constituents of Rumex Ecklonianus.” By Frank Tutin and Hubert William Bentley Clewer. Rumex Ecklonianus, Meisner, is an herb indigenous to South Africa, where it is reputed to possess medicinal properties.An alcoholic extract of this plant yielded, together with resinous products and a small amount of essential oil, the following compounds : Ceryl alcohol ; a phytosterol, C,,H,,O, apparently identical with rhamnol ; palmitic, stearic, oleic, linolic, and isolinolenic acids ;a small amount of ipuranol, C,,H,,O,(OH), ; kaempferol ;chrysophanic acid ;emodin ; 303 and emodin monomethpl ether; together with traces of other crystalline substances and large amounts of inorganic salts. A sugar which yielded d-phenylglucosazone was also present in small amount, hut no evidence could be obtained of the presence of a glucoside.The emodin monomethyl ether which mas isolated was identical with that obtained by Perkin and Hummel from Yentilago madraspchtancc (Trccns., 1894, 65, 932), and with that prepared synthetically by Jowett and Potter (Trans., 1903, 77, 1330). The dinaethyl ether of clbysophanic mid was prepared, and obtained in yellow prisms, melting at 190'. "288. '( The influence of non-electrolytes on the solubility of carbon dioxide in water." By Francis Lawry Usher. The solubility of carbon dioxide in solutions of the following sub- stances was measured at 20' : sucrose, mannite, dextrose, glycine, pyrogallol, thiocarbamide, antipyrine carbamide, acetic acid, catechol, urethane, n-propyl alcohol, acetamide, quinol, and resorcinol.The solutions mere all N/2, with the exception of sucrose, which was examined at four different concentrations. It was found that the change in the solubility of carbon dioxide produced is a linear function of the quantity of sucrose present, for solutions more dilute than N/2, on the volume-normal basis of calculation. Of the fifteen substances enumerated above, the first twelve depress the solubility of carbon dioxide, the magnitude of the effect decreasing in the order given, from 26 per cent. in the case of sucrose to 1 per cent. in that of n-propyl alcohol. Acetamide, quinol, and resorcinol produce a slight elevation of solubility. The results were discussed from the standpoint of the theory recently advanced by Philip (Trans., 1907, 91, 711), which is found to be inadequate to account €or the majority of the observations.Jahn's formula, C,/C,=l, mas also shown to be inapplicable to tho data hitherto available. It is suggested, in common with Rothmund and others, that the phenomena observed can at present only be referred to mutual interaction of the molecules. DISCUSSIOX. Dr. PHILIPsaid that when he presented to the Society his com-inunication dealing with this matter, he had expressed the view that too little attention had been paid to the influence of non-electrolytes on the solubility of gases. Experiments were now in progress bearing on this point. 304 One important piece of evidence in favour of the hydration theory with which the author had not dealt was the fact that in the great a -a’majority of cases __ increases with dilution, a and a’ being the N absorption coefficients of the gas in water and soIution respectively, and N being the number of gram-equivalents of the dissolved substance per litre.This fact showed that the cause responsible for the lowering of the solubility of a gas was most potent in dilute solution. The assumption made in his (Dr. Philip’s) paper (Zoc. cit.), that the dissolved substance takes no part in the absorption of gas, shonld not be indefinitely extended. Obviously, there were many cases, for instance, the aqueous solution of acetic acid used by Mr. Usher, in which the dissolved substance had considerable solvent power for the gas.Mr. USHERreplied that, as was expected, the equivalent depression of solubility was found to increase with dilution. The strongest argument against any explanation depending on the assumption that neither the dissolved substance nor the water which might be combined with it had no solvent action was, in his opinion, the observation that, with the majority of the substances examined, the solubility of carbon dioxide in the water of the solutions was in excess of its normal solubility in pure water. *289. The condensation of benzaldehyde with resorcinol.” By Frank George Pope and Hubert Howard. Benzaldehyde and resorcinol in the presence of aqueous solutions of the alkali hydroxides condense to form 2 : 4-dihydroxybenzhydrol.The latter compound also condenses with phenols and with aminea in the presence of zinc chloride to yield substituted xanthsnes and hydro- scridines, thus : 0 NH 305 290. (‘Ethyl a-hydroxyisobutyrate.” By William Parry. Ethyl a-hydroxyisobutyrate may be conveniently prepared from pure acetone by converting the latter into its cyanohydrin, hydrolyaing this, and isolating the resulting acid in the form of its zinc salt, Anhydrous zinc a-hydroxyisobutyrate (100 grams) is then mixed with alcohol (200 c.c.) and sulpfiuric acid (35 c.c.), and heated on the water-bath for eight hours. After addition of water and extraction with ether, the solution is washed, dried, and the ether distilled. Fractionation of the residual liquid gives ethyl a-hydroxyisobutyrate, boiling at 145-150’.Sfter distillation over phosphoric oxide, it boils at 148-150°, and the yield is about half the weight of acetone employed. The author is studying the action of Grignard’s reagents on this ester and on others of similar type. 291. ‘‘ The action of hydrogen dioxide on thiocarbamides.” By Edward de Barry Barnett. The action of hydrogen dioxide on thiocarbamide and some of its derivatives in neutral and alkaline solution has been studied, and evidence was brought forward to show that under these conditions sulphinic acids are formed. 292. ‘‘ Chlorination and bromination of acylanilides. Part I1 The action of the halogen acids on chloro- and bromo-acyl- aminobenzenes.” (Preliminary note.) By Kennedy Joseph Previt6 Orton and William Jacob Jones.In glacial acetic acid solution, hydrobromic acid and acylchloro- aminobenzenes and hydrochloric acid and acylbroaoaminobenzenes react quantitatively, yielding identical solutioiis : Ar*NClAc+ HBr = Ar-NHAc + BrCl and Ar*NBrdc+ HCI = Ar*NHAc+ BrC1 (Brit. Assoc. Reports, Winnipeg, 1909). These solutions have been shown tin tometrically and by aspiration (compare Orton and Jones, Trans., 1909, 95, 1456) to contain bromine chloride, which has been found to exist nearly free from bromine and chlorine in this and other anhydrous solvents at 16’. In mixtures prepared by each of these ways, or from the anilide and bromine chloride, a rapid bromination of the anilide occurs, the speed of the reactions being the same in each case.In dilute acetic acids analogous reactions take place, but now 306 differences appear, and complications are caused by the hydrolysis of the bromine chloride. Hydrobromic acid and an acylbromoamine react thus : Ar-NBrAc+ HBr =Ar*NHAc+ Brg. The interaction has been shown by a tinto-metric method to be quantitative for glacial and dilute acetic acids. The mixtures are identical (except for the presence of hydrochloric acid) with those prepared from equivalent quantities of the corre-sponding chloroamine and two equivalents of hydrobromic acid : Ar*NGlAc+ 2HBr = Ar-NHAc +Br2+HCl. Moreover, the speed of bromination in these two mixtures is the same, and also equal to the speed of bromination in the system prepared from anilide and bromine.The velocity of bromination is now, however, very much smaller than in the systems above described, where bromine chloride is present. If an equilibrium exists between hydrobromic acid, the bromo-amine, anilide sncl bromine in acetic acid solution analogous to that found by the authors (Zoc. cit.) to exist between the chloroamine and bydrochloric acid, the bromoemine and hydrobromic acid are at very small concentration. In such solvents as chloroform and carbon tetrachloride, chloroamines and bromoamines cannot be shown to exist in detectable quantities in the presence of hydrogen chloride and bromide. The interaction of hydriodic acid and chloroamines in acetic acid solution has been investigated by a tintometric comparison with standard solutions of iodine chloride and iodine.When one molecular proportion of hydriodic acid is used, the reaction is quantitatively Ar-NClAc+ HI =IC1+ Ar-NHAc ; and with two molecular pro-portions of hydriodic acid : Ar-NCIAc + 2HI =Ar-NHAc+I, +HUl. Although in aqueous solution, iodine chloride is hydrolysed, the resulting hypoiodous acid then rapidly decomposing in the usual way, it possesses, even in 25 per cent. acetic acid, considerable stability. These results are in accord with the view suggested recently as to the process of conversion of chloro- or bromo-amines into the isomeric chloro-or bromo-acylanilides (Orton and Jones, this vol., p. 233), namely, that primarily the former react with the halogen acids to form anilide and halogen, which can then interact;, producing the C-halogen derivative.293. (‘A contribution to the study of the oxydases.” By Ross Aiken Gortner. The author has obtained a new variety of the tyrosine oxidising ferment, tyrosinase, obtained from the larva of Tene6ro molitor. This variety is distinguished from the known tyrosinases by its insolubility 307 in water, by its loss of vitality when treated with glycerol, or when subjected to drying, and by its inability to oxidise resorcinol, orcinol, quinol, or pyramidone. A chromogen has been isolated from the body contents of the larva of Tenebromolitor, which gives with tyrosinase, colour reactions identical with those given by tyrosine.Tyrosinase has also been identified in two examples of myripod5, Scalopocryptops sexpinoscc and Julius cunadensis (Kewp.), in the larva of Czccujzcs clavipes, in the colourless plant, Monotropa uniJlora, and ac observation has been made that extracts of almost all animal tissues possess the power of oxidising quinol. 294. ‘(Experiments on substituted allenecarboxylic acids. Part I.” By Arthur Lapworth and Elkan Wechsler. The authors have synthesised ay-dipheny2-y-l-n~p7ht?~yZulZen~-a-cnrb-oxylic acid, C,,H7*CPh:C:CPh*C0,H.It gives a very stable, crystal- line compound with ether, but its salts with active bases do not crystallise. The authors have not been successful in resolving the substance into its optically active constituents by any of the ordinary methods.295. ‘‘ Cyanocarone.” By Reginald William Lane Clarke and Arthur Lapworth. The preparation and properties of cyaszocaro?ie, and some of its derivatives were described. The cyano-ketone very readily gives up the elements of hydrogen cyanide, and is then at once converted into eucarvone. This confirms the usual view of the mechanism of the conversion of carvone into eucarvone, and indicates that the relative stabilities of carbon rings of different sizes may be inverted when a double linking is introduced. 296. “The influence of water on the availability of hydrogen chloride in alcoholic solution.” By Arthur Lapworth and James Riddick Partington. The influence of water on the availability of very dilute solutions of hydrogen chloride in absolute alcohol has been carefully examined. Several tintometric experiments were made with five different speci- mens of alcohol dried over excess of calcium, two different indicators being employed in all cases but one, involving a large variation in tho total concentration of the hydrogen chloride used.In each case, too, the change in the velocity of esterification of phenylacetic acid by the alcoholic hydrogen chloride, brought about by the addition of water, was estimated. The results prove that within the limits of experi-mental error, the availability of hydrogen chloride in very dilute alcoholic solption is proportional to concentration of HCI/T + concen-tration of water, r being identical with the constant used by Goldschmidt and Udby, and termed by them the “hydrolytic constant ” of ethyl alcohol hydrochloride, but which the present authors prefer to call the ‘‘ water-value ” of the alcohol.The value of 9-found was nearly 0.10 at 25’ in all cases (that is, 1 litre of alcohol at 25’ is equivalent to 0.10 gram-molecule of water), the discrepancy between this and the number 0.15 adopted by Goldschmidt and Udby being apparently clue, in the main, to the fact that in the former instance the hydrogen chloride was highly dilute and more fully ionised. The velocity of esterificntion of a carboxylic acid in a large quantity of alcohol containing varying small quantities of water is proportional to concentrc6tionof cnrboxy~~cacid x availability of the catalyst, and the curve only departs from the unimolecular type in so far as the water formed disturbs the availability of the catalyst.As the availability of an acid varies enormously with the solvent, even where its concentration and degree of dissociation are similar, the determination of the exact value of this quantity is of primary importance in all investigations connected with salt formation and catalysis in which acids take part. 297. Amides and imides of camphoric acid.” (Preliminary note.) By William Ord Wootton. In view of the recent publication of a paper by Abati and Notaris (Gaxzetta, 1909, 39, ii, 219), the author stated that he had been engaged for some time past in the examination of a number of deriv-ati ves of a-camphoramic acid of the type CO,H*C,R,,*CO=NHR, together with the corresponding imicles. Amongst the substances prepared are the acids and imides arising from the condensation of ca mphoric anhydride with e thy lamine, n-propylamine, n-butylamine, wamylarnine, .n-hexylamine, allylamine, 0-,m-,and ptoluidine, 0-, m-, and p-chloroaniline, 0-and nz-bromoaniline, m-nitroaniline, p-amino- phenol, p-phenetidine, a-and P-naphthylamine.In the majority of cases the conversion of the acid into the imide, a process involving ring-formation, is marked by considerable diminution in the specific rotation of the compound. 309 298. (‘The nomenclature of imino-compounds and of those compounds exhibiting imino-amino-isomerism.” By Jocelyn Field Thorpe.Some confusion exists owing to the present system of nomenclatura adopted for the imino-compounds. These substances, which possess the group C:KH, are obviously just as different from the secondary amines having the group g>NH as the ketones with the group C:O are different from the ethers with the group g>O, yet the general name of imine is applied to both these classes. It is suggested that as the compounds containing the group C:NH are in many respects analogous to the ketones, the general name ketimine should be applied to them, leaving the name imine to be applied to the secondary amines, thus : c:0 C:NH c,>r;H Ketone. Ketimine. Imine. Moreover, the well-established existence of tautomerism and desmo-tropism between compounds of the type : CH*C(:NH)*C and C:C(NH,)*C renders it advisable to apply some general term to this form of isomerism, similar to the phrase keto-enolic isomerism in use with the oxygen derivatives.It is proposed that the name ketimine-enarnic isomerism should be applied to this phenomenon. It is not proposed to alter the name of the ennn2ic individual, since such substances can evidently be classified as amino-compounds without entailing any confusion. Thus, in a compound showing ketimine-enanzic isomerism, the two forms would be: CH,*C(: NH)-CH(CN).CO,Et CH,*C(NH,):C( CK)-CO,EtEthyl 8-ketimino-a-cyanobutyrate Ethyl 8-amino-a-cyanocrotonste(ketimim form). (ename form). corresponding with CH,*CO*CK(CX)*CO,Et CH,*C(OH):C(CN)-CO,Et Ethyl B-keto-a-cyanobutyrate Ethyl P-hydroxy-a-cyanocrotonate(keto-form).(enol form). This nomenclature would be applicable to a number of other classes of compounds in which tautomerism of this kind has been shown to exist, such as the acid amides, the complex ureides, etc. 310 299. ‘(Dicamphorylphosphinic acid.” By Gilbert T. Morgan and W.R. Moore. Dicam~~or~Z~~~os~~hi?aicacid, (C,,H1,O),PO*OH, has been obtained by condensing soclium camphor and phosphorus trichloride, and extracting the product with aqueous alkali hydroxides. The study of this compound is in progress. 300. The combustion of naphthalene and other organic substances, and the atomic weight of carbon.” By Alexander Scott.Although Dumas and Stas (Ann. China. PAYS., 1841, [iiil, 1, 40) used the combustion of naphthalene, cinnamic and benzoic acids, and some other organic substances to justify their new value of C =12-00 in preference to that of 12.24, advocated by Berzelius, neither they nor anyone else seem to have recognised or utilised the advantages of such R substance as naphthalene for affording data for an accurate determination of the atomic weight of carbon. The experiments of Dixon, Baker, and others suggest that it is more than likely that the combustion of pure d~ycarbon in dry oxygen might lead to carbon monoxide escaping even with a large excess of oxygen. The combustion of a hydrocarbon would lessen any loss from such a cause enormously, as some trace at least of water may be assumed to be present t.hroughout the combustion.Each gram of naphthalene burnt ought to give 3.4359 grams of carbon dioxide if C =12.000 and H = 1.0075, but if c‘ = 12.018 only 3.4325 ought to be produced, hence for a difference of 0.018 in the atomic weight of carbon we get a difference of 3.4 milligrams in the carbon dioxide produced. Two series of conibustions have been carried out with naphthalene, one set in a glass tube and the other in a quartz tube, both in a current of oxygen. In all, six experiments were made, and 17.6175 grams of naphthalene gave 60.5355 grams of carbon dioxide, hence 1 gram of naphthalene gave 3.4361 grams of carbon dioxide, whence c= 11.999. Similarly, Kith cinnamic acid each gram ought to yield 2.67459 grams of carbon dioxide if C=12*000, but only 2.67276 if C=12*018.Two experiments have been made, giving together 8.61537 grams of cinnamic acid, which yielded 23.0413 grams of carbon dioxide, that is, 1 gram of cinoamic acid yielded 2.67444 grams of carbon dioxide, whence C = 12.0015. These results therefore agree with all other combustion and physical results in inciicating that C = 12.00. The cause of the discrepancy 311 between these results and those derived froin the alkylammoniurn bromides remains still to be discovered. It might be thought that the enormous number of combustions of organic compounds which are continually being made would have indicated whether C = 12.000 or C = 12.018 were the correct number.This is hardly likely, however, for if we calculate the percentage of carbon in naphthalene, taking C = 12-00 and C = 13*01S,this comes out 93.706 and 93.715 respectively, and both would be stated as 93.71 per cent. within the limits of experimental error. The weights given above are all corrected to vacuum standard. ADDITIONS TO THE LIBRARY. I. Boiacctions. Allen, Alfred Lienrg. Commercial organic analysis. A treatise or1 the properties, modes of assaying, and proximate analytical examina- tion of the various organic chemicals and products employed in the arts, manufactures, medicine, etc. With concise methods for the detection and estimation of their impurities: adulterations, and products of decomposition. 4th edition. Edited by Heizry Leffmann and V.A.Davis. Vol. I. pp. x+576. ill. London 1909. (Recd. 9/12/09.) From the Publishers : Nessrs. J. S= A. Churchill. Crookes, Siv 1VilZiccin. Diamonds. pp. xvi + 146. ill. London 1909. (Recd. 13/13/09.) From the Publishers : Blessrs. Harper 6. Brothers. Eijkman, J. F. Tafeln zum gebrauche bei cler Bestimmung von Brechiingsindices nach der hlethode der konstaa ten Deviation von 40". pp. [102]. Groningen 1909. (Recd. lO/l2/09.) From the Author. Gemmell, G'eorge Harrison. Chemical notes and equations, inorganic and organic. 2nd edition. pp. xiii+265. London 1909. (Red 10/12/09.) From the Publishers : Messrs. Baillihe, Tindall, and Cox. Morgan, J. Livingston R. Physical chemistry for electrical engineers.2nd edition. pp. xf249. New Tork 1909. (Recd. 1o/ I 2/09.) From the Publishers : Messrs. John Wiley & Sons. Thorpe, Sir Edward. History of chemistry, Vol. I. From the earliest times to the middle of the nineteenth century. pp. viii + 148. ill, London 1909. (ReccZ. 10/12/09.) From the Publishers : Messrs. Watts & Go. 312 Van Nostrand’s Chemical annual, 1909. A hand-book of useful data. Edited by John C. Olsen. pp. xii+580. London 1909. (Recd. 1O/12/09.) From the Publishers : Messrs. Constable and Company. 11. By PurcAccse. Konig, Frunx Jose$ Chemie der menschlichen Nahrungs-und Genussmittel. 4th edition. Vol. 111. Untersuchung von Nahrungs-, Uenussmitteln und Gebrauchsgegenstanden. Teil I. Allgemeine Untersuchungscerfahren.pp. xiv + 772. ill. Berlin [1909]. (Recd. 7/ 12/09.} Lunge, Gemage. The manufacture of sulphuric acid and alkali, with the collateral branchee. 3rd edition. Vol. 11. Sulphate of soda, hydrochloric acid, Leblanc soda, 2 vols. pp. xx + 490, xii + 493 to 1010. ill. London 1909. (Recd!.4/12/09.) JULIUS THOMSEN MEMORIAL LECTURE. The Julius Thomsen Memorial Lecture mill be delivered by Professor Sir EDWARDTHORPE, C.B., F.R.S., at the Ordinary Scientific Meeting on Thursday, February 17th, 1910, at 8.30 p.m. PRESENTATION TO PROFESSOR KOERNER. A Committee has been formed in Milan with the object of cele-brating the seventieth birthday of Professor Koerner. It is proposed to devote subscriptions to the following purposes : 1. Foundation of R prize for work in pnre and applied chemistry.2. Reprinting Professor Koerner’s works. 3. Presentation of a gold medal to Professor Koerner. The Treasurer of the Chemical Society will be glad to receive subscriptions, and will forward them to the Organising Committee, 313 TABLES OF INTERNATIONAL ATOMIC WEIGHTS, 1910. To encourage the use by Students of the Tables of Atomic Weights, as issued by the International Committee, the Couccil has decided to offer the Tables at the following prices : On Cards: 1/-per doz.; 4/-per 50; 7/6 per 100. On Paper : 4d. per doz. ; 1/-per 50 ;l/9 per 100. (Note: The Tables printed on paper are suitable for pasting into note-books. ) At the next Ordinary Scientific Meeting on Thursday, January 20th,1910, at 8.30p.m., the following papers will be communicated : “The alkaloids of ergot.Part 11.” By G. Barger and A. J. Ewins. “The constituents of colocynth.” By F. B. Power and C. M’. Moore. “The trihzo-group. Part XI. Substituted triazomalonic and phenyltriazoacetic acids.” By M.0. Forster and R. Muller. ‘I Iodobenzenemonosulphonic acids. Part 11. Esters and salts of di-and tri-iodobenzenesulphonic acids.” By Miss 31.Boyle. I‘ Organic derivatives of silicon. Part XII. Dibenxylethylpropyl-silicane and sulphonic acids derived from it.” By F. Challenger and F. S. Kipping. “ The absorption spectra of naphthalene and of tetramethyl-naphthalene.” By Miss A. Homer and J. E. Purvis. R. CLAY APID SONS, LTD., UKEAD ST. HILL, E.C., AND BUNOAY, BUE’L’OLK.
ISSN:0369-8718
DOI:10.1039/PL9092500299
出版商:RSC
年代:1909
数据来源: RSC
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