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Issued 16/11/1896. PROCEEDINGS OF TEE CHEMICAL SOCIETY. EDITED BY TLTE SECRETARIES. The followin% are the abstrazts of pnp'rs reccived during the vacation, and published in the Transactions. 107. ''Contributions to the chemistry of phenol derivatives." ByR. Meldola, F.R.S.,G. H. Woolcott, and E. Wray. In this paper the authors describe a number of new derivatives of phenol, pyrocstechol, guaiacol, &c., which have been prepared inciden- tnlly in the course of an investigation into the methods of synthesis o€certain natural phevol derivatives such as eugenol, safrole, &c. 4-CliZwo-S-?iitropheiaoZ from the corresponding nitroaininophenol by Sandme! er's process. Whitish needles, m. p. !26-127". Beiizoyl delidive, m. p. 96-97'. Acetyl derirstive, m.p. F3--85". DiLccetllZ-o-anzi.IL~plzeizoZ(0-acetiniinophenyl acetate) prepared by heating o-aminoplienol with excess of acetic atilijdride and dry sodium acetate. 'i7rhite prismatic needles, m. p. IL3--124", or with l$HTLO,ni. p. 76-7'7O. The niti-o-deri vatire, obtaiiied by nitrating the diacetyl compound by a mixture of ordinary and fuming nitric acid, gives, on liydroljsis, 5-nitro-2-,zminophenol (Friedlander and Zeitlin, Eer., 1894, 27,196). t2-Cl,Zo~o-5-iiitropltenoZ,obtained from the last nitroaminophenol by Sandmeyer's process. White needles, m. p. 118-1 19". Benzoyl derivative, m. p. 127-1 25". .2-~~.onzo-4-iiitl.o-6-u?~~)~o~~~e~~~Z,obtained by reducing the broinc- dinitrophenol, m. p. 118-110°, of Laurent and Korner by means of ammonium sulphide.Whitish needles, soluble in hot water ; becomt s brown on exposure to air; rn. p. 16'2-163". Both acid and basic in properties. Acetyl derirative; 111. p. 194' iyith dccornposition, cm 164 be ma3e to decompose at 204' by rapidly heating. Anhydro-hsc ; by heating acetrl derivative with acetic nnhjilride, ni. p. 146-1 47'. Methjl ether (bromonitro-o-anisidine), yellow ncedle?, m. p. 120-131'. Dinzoxide ; yellow needles, decomposing point 152-153". 2-Ch201-0-4-dropheno I, obtdain ed fro m 4-nitro-2-aminoplien01 (Lau-rent and Gelahad t, Aniden, 1850, 75, 63) by Saizdmejer's process. Benzoyl derivative, m. p. 135". Acetyl tlerivative, m. p. 63'. 4-Nitr.o-2-a~ninoanisole,prepared by reducing 2 : 4-dinitroanisole in alcoholic solation with amnioniuni snlphide.Orange needles (from water), m. p. 11s'. Acet.yl derivative, In. p. 174-173'. 5-Nit~o-2-aminoa?aisoZe,prepared by hydrolysing the acet'yl deriva- ti1.e obtained by nitrating o-nitroacetanisiclo (Ndilhnuser, Annalev, 1881, 207, 242). Yellow needles (from water), m. p. 139-140", Acetyl derirstivc, in. p. 115-146". ~jtronnzi,zogztaiacul,obtained by reducing dinitroguniacol, in. p. 121" (Herzig, Uonatsh., 1SS2, 3,825) with ammoiiium sulphide ; brown needles, both acid and basic ; decomposing point 182". Acetyl derivn- tive ; decomposing point 224-226'. I.)iacetyl derivativc ; decom-posing point 204". Uiazoxitle ; orimge needles, exploding sharply at 149-170". constitution probably 4-nitro-G-amino-2-methoxyphenol. 5-Nilro-3-anzi~zo~~~rocateclz~1,obtained by seducing the dinitropyro-cateohol of m.p. 164O (Nietzki and Moll, Be).., 1894, 26, 2183) with ammotiiom sulphide ; acid and basic ochreous needles, m. p. 220-!%lo with decomposition. Diazoxide ; flat, goldcii needles, explodiiig sharply at 159--1603. Soluble in nlkrtli, with B purple colour. The authors point out tliat goliesally Ihe formation of diazoxides may be taken as evidence that thc amino-and hydrosp-groups are ortho with respect to cach other, and they consider klie formula of the compound to be 5-nitro-3-amino-2-hydroxyphcnol. 108. '' Action of light on amyl alcohol." By A. Richardson, Ph.D., and Emily C. Fortey, B.Sc. The nntliors have investigatcd the action of light on a number of alcohols in presenco Gf oxygen.The alcohols used -sere obtained from Kahlbaum, nncl carefully purificd by redistillation. It was fonncl that. wherens in the caw of methyl, ethyl, propjl, and butjli alcohols an exposure extending over many months failed to produce :my apparent change, thc alcoho?s reniaiuing neutral to litmus and cmtaiiiing 110 hydrogcii pcroxidc, nmji alcohol gavc strongly aci 1 wactioiis and contairiecl large quantities of hydrogen peroxide atter only a few dajs' exposure. A sidar cliaiige Deemed to take place in the case of octyl alcohol, but to a very much smaller extent. The action of light on amyl alcoliol was therefore studied in detail. Amy1 2lnoLol was exposrd to light in presence of excess of wrrtei- and of oxygen for a few dsys.A portion of the watir mas then tested with titanic ncici, when th2 preser-ce c€ hydragen pxaside was shown bj-a deep brown coloratiou. Another portion mas shaken mitli pure ether and patassium bichrornate, when the ether assumed an intensely blue colo~ir, lesving no doubt RS to the presmce of hydrogen peroxide in th, solution. In another experiment, liquid water was absent, amyl alcohol being exposed in presence of moist oxygen. Two days’ exposure sufficed to bring about tlie formation O€ hydrogen peroxide, as shown by the titanic acid test. A third experi- irieut was made with dry alcohol. A sample of amyl alcohol dried first from quizklime, then by distil1;ttion from so.li~rn,was s3aled in a hent tube coiitzining oxygen and phosphoi*us pentoxide (care being taken not to allow the liquid to met ths pentoxide), and kept in tlic dark for seven weeks.After cxposurc, the alcoliol was found to contain abundance of hydrogen peroxide. The other products formed were then examined. TLe acidity -was found to be due to tlie presence of ralerisnic acid, and the absence of carbon dioxide leads to the conclusion that the chanse is one of a comparatively simple nature, not involving the breaking clown of the iuolccule. It seeais, then, that the products formed by the oxidation of amyl alcohol in presence of sunlight aiid oxygen ody differ from those formed wlicn otlier oxidising agents arc used in that hydrogen peroxide is formed instead of water.The change imy, therefore, be represented by the follaming equation :--ZCjH,,OH + 30, = 2C,H,COOH -k 2H,O,. It was found that the presence of sunligIit was essential to the change, a saniplc of amyl alcohol kept in the dark st 1003for nine days reniaining neutral to lit~mus,and containing no liydrogen peroxide. 109, ‘‘Note on tbe action of light on ether.” By A. Richwdson, Ph.D I and Emily C. Fortey, B.Sc. Ether prepared from pure alcohol and pure sulpliuric acid, and tlien treated with potassium bichromate, was dried by repeated clistillation from phosphorus pentoxide in a specially constructed apparatus by means of which samples could be sealed for use without contact with air. The ether was then exposed in a tube containing osyge:i which had been dried by contact with phosphorus pentoxide for many weeks.After three days’ exposure, the liquid gaye a wcll u:a:l:eil peroxide reaction when tested with titanic acid. In oideii to iiivcatigate t!ie otlier prodiict3 formed, a snmi)le of ether JV~Yexposed for many weeks in presence o€ w:irei* a:id os~gcn-It was thcn rich in tiydrogcn peroxide, aiid gave an mid rcitctioll with 166 litmus. The neutmlised solution was distilled on the water bath. The distillate, consisting chiefly of et,hei-, wns also proved to contain aldehyde by its reducing action on animoniscal silver nitrate, and by its restoring the colour to rosaniline hydrochloride, decolorised by sulphurous acid. The residue in the distilling flask gave a distinct red colour with ferric chloride, and the clisracteristic smell of ethyl acetate on warming with alcohol and siilphuric acid, leaving no doubt as to the formation of acetic acid.No carbon dioxide was formed in the reaction, which may, therefore, probably be represented by the cquation 2(C,H5),0 + 502=4C,H,02 + f2HzO2,aldehyde being an intermediate product. Here, again, 11ydrogen peroxide takes the phce of the water which is formed when ordinary oxidising agcnts are used. 110 “The constitution of lapachol and its derivatives. Part 111. The structure of the amylene chain.” By Samuel C. Hooker, Experimental proof is lirouglit to show that the amylene chain mufit be written -CH,*CH:C(CH,),, and notl -CH:CH*CH(CH,),, as has been previously assumed.I11 accordance with this change, new formulae are proposed for various lapachol derivatives. 111. “Lomatiol.” By Samuel C. Hooker. The coloaring matter obhincd by Reniiie (Proc., 11, 150) is a hydroxyisolapachol. 112. “Contributions to the knowledge of the P-ket inic acids. Part 11.” By Si3gTriei Ruhemmn, Ph.D., M.A., and C. G. L. Wolf, B.A.,M.D. The authoys describe tlie products of the action of ethjlic chloro-fumarate on ethylic benzoyIacetute, and on tlie sodium derivative of ethylic methylacetoncetate ; of the hydrolrsis of etliylic methjlfur- furandicnrboxylate ; arid of the action of ethjlic sodioacetoacetate on ethylic a-chlorocrotonate. 113, ‘I Formation of pyrazolone derivatives from chlorofumaric acid.” By Siegfried Ruhemann, Ph.D., M.A.The author describes the products of the action of lijdrazine and plier,ylhjdrazine on e thylic chlorof urnatrate. In the former case, etiiylic 5-pyrazolone-3-car.box~latcis formed, identical with v. Rothec-burg’s compound (J. pr. Chenz., 1595, 51, 53), in the latter an tthere.11 salt of bis-phenylpyrazo!onecai~boxylic acid. Their pro-perties are described. 167 14. LL Studies of the terpenes and allied compounds. Note on ketopinic acid-a product of the oxidation of the solid hydrochloride (chloro- camphydrene) prepared from pinene.” By Henry E. Armstrong. The acid described has the formula C10H1403,and is obtained by the iiiteraction of chlorocamphydrene and the strongest nitric acid. It melts at 234’ (uncorr.).Bark, calcic, and metbylil: salts arc described, as well as a hydrazone (m. p. 146’) and a hjdroxime (m. p. 216’). Ketopinic acid appears to be a saturated keto-monocarboxg lic acid. 115. “Acid compounds of natural yellow colouring matters. Part 11.” By A. G. Perkin. In a previous communication by Perkin and Pate (Proc., 1895, 11, 126), it was shown that vhen treated with mineral acids in the presence of acetic acid, quercetin, rhamnetin, rhamnazin, fisetin, and morin, yielded crystalline Compounds, the formula of which is gener-ally represented as an addition product oE one molecule of acid to one molecule OF colouring matter. It has siiice been shown that luteolin and myricetin beliave similarly, and there can be little doubt that all these colonring matters belong to the so-called quercetin group. In this paper certain of these compounds not previously examined are described, vix.: Quercetia hydrochloride, C,,H,,O,*HCl ; inorin hydriodide ; C15H100,*HI,and lnteolin hydriodide, C1,Hl,06HI. It is also shown that whereas qucrcetin tetramethyl ether, resembles the mono-metlijl ether of rhamnetin in rzacting with sulph-uric acid, and not with the lialoid acids, dibromo-quercetin and tetrabromo-morin yield no compounds with mineral acids. The other known members of the yuercetin series are dioxyflavone (Fried- liinder and Rudt, Be,.., 2896, 878) and chrysin, the colouring matter of poplar buds. The former has been shown by its discoverers to yield acid compounds, but, on exarninaticn, tlie latter was found to be devoid of this property.Various members of the ketone group (gallacetophenone, alizarine, and maclurin), of tlie xan thone gt-oup (gentisin, euxanthone, datiscetin), and of the anthrsquinone group, were examined in this respect, but yielded no compounds with mineral acids. Catechin and kino‘in also, the latter a constituent of mslabar kino, did not react. For the constitution of the acid compounds two schemes are put forward, the first a similar one to that soggested by Nietzki and Schriiber (Bey., 1895, 50) for the phthaleine ea’lts, and a second depending upon the saturation of the ethyleue bond in the y-pyrone ring. It is considered probable that this reaction is characteristic of the quercetin group, and will thus be of sei~icefor distinguishing its menibers from the other classes of non-nitrogenous, yellow, mordnnt dye-stuffs which are at present known to exist.316. “Studies on citraziiiic acid. Part 18.” By W. J. Sell, M.A. The n3thor lias employed Tiemann and Reimer’s reaction (Bey., 1876, 9,423, S24) to introduce the aldehyde group into hydroxjl derivatives of pyridine, and has isolated niid analgwd the disodiu m salt of tbe monnldeliycie of citrazinic acid, the inonolciehjde acid, tlie oxime of tlie mo~inldehyde acid, and the phenjlliydrazlne salt of the hjdrazoi7P. 117. ‘I The action of certain acidic oxides on salts of hydroxy-acids.111.” By G. G. Henderson, D.Sc., M.A., and John M. Bm. By the prolonged boiling of antimonious oxide in an aqueous soln-tion of the primary inatlate, amnzoniunz cr?itinz012i0-17zaZntemi3 obtained, 25b,O (C4B,0,NH,),.Sb,O (C,H,O,) ,*20H,O, resembling the potassium salt already described (Trans., 1895,1030). It forms large, colour- less crystals, easily soluble in water, and decomposes when heated to about 115O, or when its aqueous solution is boiled for a short time, except in presence of excess of the oxide. Antimonious oxide dissolved slowly in a boiling soluticn of sodinm hjdrogen nislate, and, on adding alcohol, a syrup was precipitated, which consisted principally of tlie sodium compound. However, the pcre salt coulct not be obtained in a crystalline condition. While arscniQus oxide disaolved freely in solutioiis of primary sodium and 2inmonium malates, salts corrcspondiiig to the antimonio- malates could not be prepared in a pure state, owing to the insta-bility of the products, although an impurc ammonium compound was obtai n ed.Armioiiiim anti,iioizio-iiizicat~, S bO(X€1,)C413,0,.3H,0, was pre-pared by prolonged boiling of the oxide with a solution of the primary inucate and repeated recrystallisation of the product. It is a white, finely crystalline powder, sparingly soluble in cold, but fairl~casily soluble in lict water. In its otlier properties it closely resembles the potnssium salt already described (Zoc. cit.). The sodium salt, EbOK’aC4HbOs*3H,0,prepared similarly, is also a white crystalline powder, only differing from the others in its greater solu- bility in water.On zddition of barium acefate to a solution of the sodiuni salt what appeared to be a, lightly impure barium salt was gradually precipitated in the form of a white powder. Attempts to prepare wsenio-mucntes of sodium and ammonium were not successful, and failure also attended our edTorts to obtain coinpounds of the alkali salts of mandelic acid with antimonions and arsenioas oxides respectively. Salicylic and gallic acids mere then taken as examples OF plienol acicls, but experiment showed that xieither antimonious nor arsenious oxide entered into reaction with any of thc alkali salts of these acids. Molybdenum trioxide was found to dissolve in boiling aqueons solutions of primwy tartrates, forming compounds with them.Sod i(A. m mo7.yhdi-tartr(xtP, MOO,(NaC H40,),*3H,0, was obt ainecl i 11 the form OF a white cr~staflinepowder, easily soluble in cold water, and ciecomposed on exposure to light or to a tsmperature of 9Go,and also when its aqueous solution is b3iled for some time. The potas-siiim salt is also rz crystalline powder, very similar in properties to the sodium salt, but less stable. Ihe ammonium salt. mas only obtained in the form of n gelatinons prccipitate. Sodium tu itgsti-tartrate, WO,( NnC,H,O,) ,*5H,O, was prepared l)y dissolving tungsten trioxide in :I boiling aqiieous solution of the primary tartrate, excess of the lnttzr being used. It crystallises in white plates, easily soluble .in water, and decomposed when heated to about 110”,or when its aqueous solution is boiled for any length of time.The yotassizinz salt, WOz(KC4H,O,),*4~H.,O, and thc nmnionizcnt salt are also crjstalline, the former closely resembling the sodium salt in properties, the latter being very unstable in pre- sence of water. The Dn~iuiusalt, TV0,(C4H,0,)2Bn, is precipitated as n white, insoluble powder when barium acetate is added to a solu tion of the sodium salt’. Silicoli dioxide, used iu the form of gelatinous silicic acid, appa-rently does not react directly with primary tartrates, but titanium dioxide dissolves in solutions of these salts, yielding substances which me being examined. It remains to be triecl whether other acidic oxides also react with tartrates and salts of otlier hydroxF- acids.118. ‘I Mote on r-acetobutyric acid, CH:,.C0.CH,.CH,.CH2.COOH.”By W. H. Bentley and W. H. Perkin, Jun. l’hz properties of this acid were cxmfully investigated in order to enable the authors to compare it with a ketonic acid obtained from sulphocnmphylic acid. It mas prepared by the hydrolysis of ethylic acetjyl glutarate (kyolff, Amaleit, 1633, 216, lag), the method of preparation being improved in some respects, The oxime (m. p. 104-105’) and the semicarbazone (m. p. 174’) me the most characteristic derivatives ; when oxidised with nitric. acid, aceto-butyric acid yields succinic acid. 170 119. '' Some derivatives of propionic acid, of acrylic acid, and of glutaric acid." By W.H. Perkin, jun. tigation of acid, (CH,),.C:CH.COOH ; tfi??%ethyl-wrylic acid, isopropylacrtjlic acid, The ethorcal salt of the former acid, when digested in alcoholic solntio.-l with the sodium compound of ethplic malonate, yields ethylic dimsthyZpi-opanefricarboxylafe, (C 00C,H,),CH.C (CH,),.CII,*C 0OC,H, (coizpare AUWCI'S, Bey,, 189.3, 28, 1130; A~znaleu,2896, 292, 145), (b. p. 203", 60 mm.),from which, by hydrolysis and elimination o€ carbon dioxide, COOH.CH,.C(CfT,),.CH~~COOH,/jP-dirnethylgZuta7-ic: acid, was obtained. This acid melts at 101", and gives au anhy-dride melting at 124" and an aniiic acid melting at 1.34". Trinzethylacrylic acid, together with isip-opy7acs.ylic acid, results from the action of alkalis on ethylic a-bromo-xpp-ti.i~iethyl~ropionate, CH(CH3),.CBr(CH3).COOC,H5.The former is a crystalline com-pound which melts at 70-71", and froni which the following deriva- ti yes have been prepared. ap-Dibronzo-app-trimethylpropioiaic acid, CBt.Jle,.CBrMe*C 0OH (m. p. 188"). /?-Xromo-zpp-t rinz et JLylpropionic a cit7, CBr(CH3),*c!H(CH,) C0OH (m. p. 88"). ~-lodo-a~~-trinze~~i~l~rop~o~a~cacid, CI(C&),.CH( CH,) *COOH (m. p. 88"). When the mixed ethereal salts of trimethylacrylic and isopropyl- acrylic acids (as obtained by the action of quinoline on cthylic a-bromotrimethylpropionate)are digested mi th the sodium compound of ethplic mnlonate, the ethylic isopropylacrylate only elitera into tlie reaction with formation of ethylic isops.opyl.pi.opnnetricarboxylute, (COOC,H5)*CH,*CH,~C(COOC2H5),*CH*(CH3), (b.p. 208-210" at 45 mm.), the ethjlic trimethylacrylate remaining apparently un-attacked. (COOH) .CH2GH2*C(C 0OH),.CH (CH,),, isopopylpropane-tytcarboxylz'c acid, crystallises in colourless needles, which inelt at 265" with decomposition into carbon dioxide and isopopylglzitilric acid, COOH~C€12*CH,~CH(COOH)*CH(CH3)2.This acid melts at 95", and gives an alzhydde at 53" and an arrilic acid melting at 15s-159' ; its constitution is proved by its synthesis from ethylic isopropyl-malonate and ethylic a-iodopropionate. This paper contains also an account of a number OF experiments on the action of phenoxjethylbromide, C6H5*O*CHa*CH,Br, on the sodium compounds of ethylic dimethylpropaaetricarboxylate and ethrIic isopropylpro~anetrica~boxylate.171 120. “On the sction of chloroform and potash on metamidobenzoic acid.” By W.J. Elliott, M.A. By the action of aqueous potash and chloroform on metamido- benzoic acid, a, compound is obtained which is insoluble in all solvents, reduces Fehling’s solution, and gives with plienylhydrazine a red compound, which is not a hydrazone, but has the properties of an azo- compouiid. The compound has the cmpiricsl formula CsHiNO, aad the author THz YH.2 suggests the constitutionul forniuls C6H~-CH0H*CO*C6H3that,I600H COOH is di-amido-di-carboxy-benzoin.TVlieii boiled mitli water for some time, the compound is oxidised, jielding a solution of metamido-benzoic acid.Witli phenylhydrazinc, metamidobcnzoic acid and a compound having the empirical formula C7H6N2, are formed. The author suggests the formation of an osazoiie, wliich is reduced, by the hydrogen set free, to metamidobenzoic acid and a disazo-com-pound of the formula C6H,.N:~,CH:CH.N:I.CsHj. No\-ember 5th, 1S96. Mr. A. G. Vernon Harcourt?President, in tlre Chair. 3Iessrs. J. B. Knight, S. G. ltosenblum, J. A. Craw were formally admitted Fellotvs of the Society. The following certificates were read for the first time :-Henry Edward Ajlxojd, Ashwell, Toller Lane, Bradford ; William Ballingall, Ardarrock, Dundee ; Charles Uathurst, Junr., Lydney Park, Gloucestersliire ; Lauiitz Hansen Bay, The Grammar School, Carlisle ; Charles Edward Browne, 2, Hinton Villas, Cheltenham ; George Harold Cross, B.Sc., Balliol College, Oxford ; Williain Duncan, Ropal Dispensary, West Richmond Street,, Edinburgh ; Walter John Elliott, M.A., 5, Dover Place, Clifton, Bristol; John TI omas Fleet, Rugby, Warwickshirc ; George George, Regent Street, Kingswood, near Bristol ; Arthur Croft Hill, Trinity College, Cam-bridge ; Cbarla Alexander Hill, Hawthorns, South Road, Clapham Park ; John William Hinchley, Baggeholme Road, Lincoln ; William Trevor Lawrence, B.A., Ph.D., 57, Prince’s Gate, S.W.; Robert Dexter Littlefield, 23, Wightman Road, Hamingay, N.; Thomas Henry Lloyd, Penjgraig, Pontypridd ; Thomas TVilliam Lockwood, 172 Heclimondwike ; Edward Seaborn Marks, 111, Crornwell Road, S.W. ; Arthur Stanley Mayfair, Avenue House, Beverley Road, Hull ; William 31.Miller, Prye Estnte, Wellesley, Penang, Straits Settle- ments ; Landon Clarence Moore, 19, Mecklenburgh Square, W.C. ; Francis Ambrose Moss, Menzies, Western Australia ; Herbert William Moss, Broken Hill Proprietary Company, Limited, Port Pirie, South Australia ; Joseph Terreiice de la Mothe, Grand Bacolet Estate, St. Andrew’s Parish, Grenada, Wesi Indies ; Alexander Henry &fit- chell Muter, The Chbtelet, Horley, Surrey ; William Harrisou Pearsall, The School House, Dnlton-in-Furness ; Henry William Potts, Eiirca, Victoria ; Frederick Belding Power, 21, Queen Square, Bloomsbur*y,W.C. ; William Russell, Summerlie, Coatbridge, N.B. ; Herbert Cecil Seabrooke, The Echoes, Grczjs, Essex ; TVil!iam Horace Sodeau, B.Sc, 25, Shore Road, South Hackney, N.G.; Charles ‘l’honipson, Graminar School, Costham, Rcdcar ; William Henry Walker, Stafford Street, Willenhall, Staffs.; William Watson, M.A,, School House, Kingsbridge, South Devon ; EdKin Whitfield Wheel-wright, R.Sc., Ph.D., The Oaklands, Warley, Oldbury, near Birming-ham ; John Harrison Wiper, Ph.1>., 58, Breakspears Road, St. Joliii’s, S.E. Of the following papers, those marked * wore read. “121.“The constitution of the so-called nitrogen iodide. By F. D. Chattaway, M.A. From tbe beginning of the present century, the black explosive compound formed when a solution of ammonia acts upon iodine, has dmost continuously engaged the attention of chemists.No definite conclusion as to its constitution has, however, bcen arrived at, although, from time to time, different formulz have been assigned to it, while, on account of its apparently variable composition, several iiistiiict compounds have been supposed to exist. The formulx: N13, NI, NH2‘I,NH12,and NH3N13,have been adopted by various chemists, while others hare suggested that ;L series of different but allied substances exist, derived either from NH,, or a liypotliktical substance, H3N:NH3,by replacement of hydrogen. A number of experiments made with this substance with a, view to the spthesis of hydrazine derivatives having given negntire results, an investigation of the compound itself was undertaken. Nitrogen iodide cannot be obtained dry in a condition suitable for analysis, so that a11 experiments have to be conducted with an nnknomn quantity and in presence of water.It is Lest prepared by adding a solution of iodine in potassium iodide to an excess CE€ a 173 strong solution of ammonia, when it is precipikated as a soft black powder. Many anxlysm have shown that its composition does not T-ary according to the mode of preparation, provided thah sufficieut care is taken to remove unchanged ammonia, iodine, and the various pro- duets of the action. The substance always yields, on decomposition, ammonia and iodine, 1mol. of ammonia being set free to 2 atoms of iodine. The variations of composition which have been obscrved we probably due to the substance not having been properly freed from ammonia or iodine.or to a decomposition of greater or less extent having taken place during the treatment of the substance after pre- cipitation. If itl be continuously washed with water, all the nitrogen can be removed as ammonium salts, practically pure iodine alone being left. This seems n snfficient explanation of the apparent existence of a series of compounds, Nitrogen iodide has always been assumed to bc a substitution derivative, mainly on the gronnd that in its preparation a largc amount of ammonium iodide is formed. This, liowevcr, is not the sole other product,, nmmoniiim hypoiodite also being produced, and, forttier, more than half the total iodine employed can be obtained in the nitrogen iodide produced.This could not happen if it mere a substitution product. A number of other facts, also, seem to show that it cannot be ,z substituted ammonia ; for example, tlic invariable production of ammonia and never of any nitrogen compound containing oxygen in its deconiposition by various agents; its formation only from free ammonia, and never from ammonium salts ; the fact that iodine does not substitute in NH, groups, and the product,ion of ammonitim iodide when it explodes. Whenever it is decomposed, ammonia and iodine nre always liberated ; these may be free or partially combined together, or they rnay react with the agent effecting the decomposition. An excess of water decomposes the substance, yieldin<g, if light be excluded, animonium iodide and liypoiodite and free iodine.This action oxplains the decomposition of the compound by prolonged washing, and the consequent accumulation of iodine in the residue. The amrnoniium iodide and hypoiodite formed can dissolve a little of the liberated iodine, but a certain amount cannot thus be taken into solu-tion, and consequently remains behind mixed with the undecomposed compound. The pereentags of iodine in the residue therefore con- tinually increases, and ultimately only a smali quantity of practically pure iodine is left behind. Potash and soda very easily decompose the substance, liberating nn:monia and forming iodide and hgpoiodite, or if the solution be heated, iodide and iodate. The oxides of lead and silver sus-pended in water act similarly, ammonia is evolved, and iodide and iodate of the metal formed.Finely divided metals appear to assist the action of the water by combining with the liberated iodine. Acids, generally speaking, decompose the compound, liberating iodine and ammonia, with the latter of which they combine. The action of hydrochloric acid is peculiar; it seems to form, at first amnionium iodide and iodine chloride. All substaiices capable of reacting with iodine at once decompose nitrogen iodide, yielding, in addit.ion to ammonia, the same products that they yield with iodine itself. Sulphuretted hydrogen forms ammonium iodide and hydriodic acid, while sulphur is precipitated. Sulphurous acid gives hydriodic acid, and amriioniuni sulphate. Sodium thiosulphate liberates ammonia, and forms sodium iodide and sodium tetrathionate.The lower oxides of arsenic and antimony are converted into the higher, with libera- tion of ammonia and formation of hydriodic acid. Potassinm cyanide sets free ammonia, and forms potassium iodide and cyanogen iodide. On the whole, therefore, it seems that a single substance is formed by the action of ammonia on iodine, and that in this one atom of nitrogen is associated with two atoms of iodine. Whether the simplest formula that can be given to the substance is NHI, or NHJ, can only be finally settled by a very careful investigation of all its reactions under the most varied conditions; but at present the formula NH,I, seems best to accord with t’he reactions of the sub- stance and express the known facts regarding it.“122. “The carbohydrates of barley-straw.” By C. F. Cross, E.J. Bevan, and C. Smith. This is a continuation of investigations which were the subject of a recent comniiinication (Trans., 69, 804). Tile furfu~oid carbo- hydrates isolated by acid hydrolysis from the cereal celluloses afferded evidence of the existence of tl liexose-pentose series of tissue constituents with a definite transition form corresponding with a pentose monoformal, i.e., C,H,O,<O>0 CH, = C,Hl,05. The metliods lending to the recognition of this intermediate con- stitutional form have becn applied to the plant taken at various rstnges of growth dur:ng the season 1896. The fiirfuroids were similarly isolated, arid their constitution investigated by ( 1)osazones, (2) yeast fermentation, (3) t.he reaction with hydrogen peroxide pre- viously described (Zoc.cit.). The numbers obtained show a progrcssive variation. Thus, tbe 175 osazones aiv at first oE high melting point (180-190’); the fur furoids are entirely broken down (fermented) by past in the neutralised solution, and tlie peroxide treatment shows negativc results, i.e., no evolution of carbon dioxide. From the flowering stage onwards tlie oaazones fall in melting point ; there is increasing rasist- ance of tlie furfuroids to the action of yeaqt, and the characteristic reaction with hydrogeu peroxide is observed, with incrssing propor- tions of carbon dioxide formed.These results point to the gradual transferrnation of a hesose into a pentose derivative. At the same timc the evidence is reviewed uFon whieh these characteristic tissue constituents must be looked upon as having a special constitution or configuration ah hitio, i.e.: they are assimi- lated 01’ elaboratcd in the Erst instance with the constitutional features which determine their characteristic decompositions, viz., (1) to fu1*ful?iIl by the action of condensing acids, (2) to pentose derivatives as a normal incident of tlieir life history in the plant. “123. The direct union of carbon and hydrogen.” By William A. Bone, and David S.Jerdan. The author:, have continued and extended the experinleiits of which they gare some account to the Society six months ago (Proc., 162,Gl), and now arc in a position to discuss their results more fully.In their first communication they stated that they had produccd methane by passing a slow current of hydrogen, free from hpdrocm boil impurities. over purified carbon heated to bright redness in a p01.c~-lain tube placed iiiside it Fletcher injector furnace. The products of the union of carbon with hydrogen ah Ihe tern- peraturc of the electric arc have been more thoroughly studied. The electric arc mas formed between terminals of purified gas carbon in an atmosphere of dry hydrogen contained in a glass globe standing in a troagli over mercury. The arc was maintained in hydrogen for an hour or more, and samples of the gas were drawn off at the end of 5, 15, 30, 45,&c., minutes in each experiment.These were after- wards analysed in a modificd form of the McLeod gas-annl~-;is apparntu s. The gases almost always contained small amounts of hydrocyanic acid, due, no doubt, to the presence of a little nitrogen in the hydrogen employed. Acetylene was always present in considerable quantities, ancl, in addition to this and any other unsaturated hydrocarbon, appre- ciable quantities of methane were found. 176 “124. “The explosion of acctylene with less thm its own volume of oxygen.” By William A. Bone and John C. Cain. Continuing their earlier experiments (Proc., 142, liO), tlie authors have exploded mixtures of acetylcnc wit11 from 23 to 95 per cent.of its own volume of oxygen in a leaden coil, soxw 5 metres long, having an internal diatneter of 13 mm. The coil wm closed at each end by a steel tap, and at one end a stout ghss firing piece, into which two platinum wires were fused, was fixed betwecn the steel tap and the end of the coil. Tlic other end of tlie coil was connected with a mercu1.g manometer, so that tlie pressure change inside the coil after an explosion could be determined. The coil was immersed in a bucket of cold wi.n!cr, hicli served to rapidly cool the gases in the coil after an explosion. The coil was filled with the explosion mixture at tlie ordinsly atmospheric pressure by displacement; the mixture was tlicn fired by an electric spark passed across the wires at the firing piece.After the products of the explo- sion had cooled down to the temperature of the vr,ter surrounding the coil, the tap nearest the manometer W~~Sopened, arid the pressure of the gases inside the coil was read off. In :ill cases a considtixble increase in pressure, varying from 2GO lo 370 inm. of inercniy, according to the mixture exploded, occurred. Samples of the products of explosion were collected in eneh case, and these, together with the original mixtures of acetylene and oxygen, were carefully analysed in n modified form oE the l\lcI~eod apparatus. The products of explosion were found to consist chiefly of carbon monoxide and hydrogen, but in addition to these, small, but quite appreciable amouiits of acetylene and cerbon dioxide were invariably present.In their earlier experiments, the nut>horssuspected the presence of a small amount of methane among the products of explosion of certain mixtures of acetylene and oxygen ; a more rigid examination of the products has, however, shown that methane is not present in any appreciable qnantity. Further experiments indicate that although the main resultant reaction may be expressed by such equations as (u)CzH2+ 0, = 2CO + Hz; (b) ‘LC,H, + 0, = 2C0 + 3H, + ?C ; (c) 3C2H2+0, = 2CO + 3H, + 4C, yet some steam is formed ; this is evident froin the fact that the ratio of the hydrogen to the carbon inoiioxide ill the products is always less than the above equations require. Further, the presence of carbon dioxide in the products would be difficult to explain if no steam were produced. The small percentages of nitrogen in the products of explosion are due to nitrogen contained in the original niixtures fired.177 From these experiments, it is evident that when the electric are is passed between c3rbon terminals in an atmosphere of hydrogen, acetylene and metlinne are both produced. Further, that the rate of formation of these two gases is fairly rapid during the first 7 5 minutes o€ tbe experiment, after which the rate falls, and finally, after about half an hour, a state of equilibrium between the hydrogen, acetylene and methane is attained. This equilibrium depends, to some extent, on the voltage employed. These results led to tlie inference that methane and acetylene would both be decomposed by the electric arc, and that if the are is passed long enough a similar state o€ equilibrium would be arrived at.This conclusion was fully borne out by subsequent experiments, in which pure acet~lene or methane was subjected to the action of the electric :ire passed between carbon terminals in the same apparatus as tlist employed in the experiments with hydrogen. Both methane and acetylene are easily decomposed by the electric arc ; during the first 10 minutes of tlie experiment, the gas (methane or acetylene, as the czse might be) was very rapidly resolved into its elements, large flakes of carbon were formed in the neighbourhood OF the terminals, and fell to the surhce of the mercury below ; the gas in the globe underwent a great increase in yolume, much greater than could be accounted for by the mere expansion of the gas by tile hest oE the arc.A smoky flame rose from the terminals and Glled the upper part of tlie globe. At the end of about 10 minutw, this ex truordinary appearance subsided, after which the are presented the same appearance as in the case of the hydrogen experimunts. After the arc had passed for an hour, the experiment was stoppecl; Eamples of the gases were ther, collected and subsequently analysed. The principal product in each case was hydrogen with about 9 per ceiit. of acetylene, and small quantities of methane, nitrogen, arid hydrocyanic acid. In the experiment with acetylene, a minutc quan- tity oE naphthalene mas also formed.125. The refraction constants of crystalline salts.” By Willi3m Jackson Pope. Although a large inass of accurate data concerning the yefraction const ants and molecular volumes of crystalline substances possessing one, two, or three principal indices OE refraction has been collected, 110 successful attempt has hitherto been made to deduce a definite general relationship between the refraction constants and the com- position ol such salts. The author considers that thc method used by Tutton of calculating a single molecular refraction constant for biaxial crystalline substances as the arithmetic mean of the mole-cular refractions for the two extreme refractive indices is not a 178 Logical one, but that thc molecular refraction should be calcnlated from the mean of all three ref~active indices in such cases; the molecular refraction of uniaxial salts sbould be calculated from a refractive index which is one-third of the sum of the extraordinary index, and twice the ordinary refractiye index.Thc molecular refraction constants obtaineJ in tAis mag arc, within the limits oE experimental error, of an additive nature, so that it becomes possible to compile tdiles of atomic or eqiiivaleiit refrac- tions from which the molecular refraetion of solid salts may be cnlcu- lated additively in just the same way as is in general use for liquids. The rno!ecular refractions of some hundred or so salts have thus been calculated, both from the expeiimcntal data, and from the table of atomic refractions, and comparison show n good agreement between both sets of numbers.Tlie author shows that the molecular refraction of a solid salt, cal- culated as above described, is not quite the sxme as that of the salt in aqiieons solution. The influence of the solvent is ii:tturally elirninated by dealing with the solid salt alone, and nphysical method of deriving valuable information respecting the constitution of solid substances is thus obtained. 126. 'I Compounds of metallic hydroxides with iddiae." By Theodore Rettie, B.Sc. When iodine, dissolved in aqueous potassium iodide, is added to a solufion of a mngiicsiurn salt, and potash iq then carefully added to the mixed solukione, a dark brown precipitate is obtained. The an thor concludes that this and the somewhat similar precipitates obtained in an analogous manner with solutioiis of zinc, cadmium, and ser-era1 other salts consist of metallic hydrates with a variable quantity of iodine carried down with them, forming compound3 aesernblirig lakes.127."Economical preparation of hydroxylamine sulphat e." ByE. Divers, M.D.,F.-R.S., and T. Hags, D.Sc. Sodium ititri te yields nearly its own weiglit of hydroxylaminc sulphate when carefully sulpllonated, by the ndclition of sodium sulphite, and h~drolysed. In sulplionating, the solution must be kept slightly below O", and the sodium carbonate be closely in proportion to the nitrite of 1mol. to 2 mols. The hydrolysis in its second stage must not be carried out at 8 boiling hest, because then much hydroxjl- amine is destroyed.At 90-95" the hydrolysis is satisfactorily effected in two dais. After neutialisation, the sodium sulphate is separated, and the ltydroxjlamine sulphats crystillised out. It is a non-deliquescent salt, soluble in three-fourths of its weight of water at ZOO, and cryst,allises well. 179 133. ‘‘The reduction of nitrososulphates.” By E. Divers, M.D., F.R.S., and T. Haga, D.Sc. From a partly quantitative examination oE the products of reduc-tion of potassium nitrososulphate by Eodium amalgam, it has been ascertained tht they include hyponitrite, nitrous oxide, h ydrazine, ammonia, nitrogen (probably), sulphi te, sulphate, and arnidosnlpho- nate.Of 12 mols. of the salt it is estimated that six become amido- sulplionnt e and nitrous oxide, four become sulphite and hyponitrite, and two become sulphate and partly hydrazine, partly nitrogen. The occurrence of hj-drazine was discovered by Duden, in 1894; that of sulphate and amidosulphonate is new. The production of sul-phate by the sodium is regarded by the authors as another proof that nitrososulphates have not a sillphonic constitution. The forination of amidosulphonic acid is attributed to the salt being a srilphatc of a hydrogenisable radicle, and in this respect like no other known sulphate. 129. “Imidosulphonates. Part 11.” By E. Divers, M.D.,F.R.S.,and T. Haga, D.Sc. Through the kindness of Dr. Raschig, the authors have been able to compare the contents of Berglund’s Swedish papers on Imido- sulphoiiic acid and amidosulpl~onic acid with their own results, which appeared in the Journal, in 1892 (Trans., 61, 943). They find that they have succeeded fairly well in making their own work supple- mentary to his and not a, repetition of it.Where there has been overlapping, some interesting points are raised. The normal sodium salt had been preparecl by Berglund, bat only by indirect methods, not by the sulphonation oE sodium nitrite. The $ normal salt he did not prepare. There is disagreement as to the composition of the oxymercuric salt, and in the present paper new work is submitted, establishing fully, in the authors’ judgment, the correctness of their formula, which makes tho salt coiitain the bivalent group -HgOHgOHg-, found also in the oxymercuric bulphate, sulphite, and imidosulphonate9. What the authors have described as the calcium sodium salt, Berglund mistook for the normal calcium salt.Among the new salts described in this paper are the true normal calcium and the true normal strontium, as well as the + normal calcium salt. Berglund also mistook, it appears, the strontium sodium salt for the normal strontium salt. The mercuric sodium salt he duly recognised as such. The mercuric calcium salt has now been prepared, as also a compound of it with mercuric chloride, analogons to apatite, imidosulphonic acid holding the place of phosphoric acid. An oxymercurous salt described is of 180 interest on account of the contrast it s1iow.s between imidasulphonic acid and smidosulphonic acid, the latter, like amnionia, i.esolving mercurous salts iiiti metal and mercuric snltms.Lastly, mercurosic salts have been prepared, remarkab?e in exhibiting a substitution, to varying extent, of t’be mercurous radicles in the preceding salt by mercuric radicles. The limit of this substitution is expressed in thc following formule :-Hg2N(m&Hg?. Hq”N(SO,)zHgzO<Hg2N(SO,),Hg, ’ O<H~~W(SO,),H~. Oxymercurous salt. Oxymcrcurosic salt. 130. Amidosulphonic acid.” By E. Divers, M.D., F.R.S.,and T. Haga, D.Sc. Except in the field of organic chemistry, nearly all that is knowii of amidosulphonic acid and its salts we owe to its discoverer, Berglund.Outside his work, in 1876,there is oiily to be mentioned that Fock has described its crystals and Raschig discowred a simple and excellent, though costly, nietliod of preparing it by sulphonuting hjdroxylaminc. Of the additions now made by the authors to the knowledge of tliis acid, the following are the most prominent. Amidosulplionic acid is Iargely precipitated from its solutions by sulphnric acid. This fnci. makes the preparation of the acid from sodiuni nitrite vti’y easy. Its preparation fi-om this source is also very inexpensive ; for when the nitrite has been sulphonated, and the product hydrolysd, the solution nent~*alised,and sodium sulphate crystsllised out, there only remains to add some concentrated snlpl-iuric acid, in order to get nmidosnl- phonic acid almost pure, and in quantity equal in weight to at least three-fourths of the nitrite worked upon. Aniidosulphouic acid combines with mercnric oxide only to forni a basic, insoluble compound.The acid precipitates the sarric coni-pound from a r?olution of mercuric nitrate, which it can completely dmonipose, its mercui*y compound beirig insoluble iri cliliitc nitric acid. MorJ remarkable is the fact, that this compound is noluble in alkalis. In its degree of basicity it agrees with tlic oxymcrcuric: sulphate, sulphite, and imiclosnlybonates, and ma-j, theyefore, be foimulstcd as (H2NS0,HgO),Hg,2H,0. But, since potassium liyclr-oxide dissolves it without demmposing it, and tht, rt.gai*dingI its ninidosulphonic acid as an amine, it behaves exactly 1iL-ca mercnr-ammonium compound with Pesci’s reagent (ammonium bromide), it may be taken to be, in alkaline solution at least, a sulphmated mercuram monium hyd roxi cle, Hg,Nz(S0,K) (0€I ):,2 Li 0.Amidosnlphonic acid shows, again, a likeness to ammonitt in serving to prevent precipitation of silver nitrate by potwsium hyclr- 181 oxide. When the amidosulphonate is not in excess, a bright, ochre yellow, colloidal substaccc can be precipitated irom solutions of moderate dilntion. Much water decomposes itJ,and forms with it a collo’idal, brown Eolution (apparently OF dver oxide). Its composition seems to be expressed by the formula AgHNS03K. Double decom- position between silver nitrate and potassium amidosulphonate does not take place when their solutions are mixed. The normal silver salt is well known.The first action of heat upcn amidosulphonic acid is very interest- ing. It melts at 205O, but not without decomposing, to a liquid which solidifies to a transparent vitreous mass, on cooling. The properties of this mass, which is formed without gain or loss in weight to the acid, show it to be composed of ammonium pyro-sulphato and ammonium pyro-imidosulphonate in molecular pro-portions, along with 7-10 per cent. of unchanged acid. This transformation of the acid by heat is a striking example of intra-molecular decomposition and of cnmulative resolution in the direction of amtnor,ia and water for hydration and salt formation.The behaviour of the mixed pyro-salts, when further heated, is described in the author’s paper, but must be passed over here. Anhydrous salts of fimiilosulphonic acid are largely converted by heat into imidosulphonates and ammonia, but also into sulpliates and gases. The decoiiiposition of the barium salt, for instance, is nearly repre-sented by the equation 3Ba(SO3NH2),= 3BaS01 + HN(S03NH4)z + NH, f NS fN; but it is only this salt that yields nitrogen sulpliide. 131. ‘I Molecular conductivity of amidosulphonic acid.” By J. Sakurai. Thc mc*leculnr conductivity of amidosulpbouic acid 1)-asdetermined by means of a Kohlransch’s universal bridge ; the result shows tlint it is a strong rnonobssic acid, being nearly c:ornpi*abla with iodic arid.The author coinp)nres, at different dilutions, the dcgrc: OF KHdissocintion of amidoau1l)honic acid, 0,s<OHL, with that of sulph-H urons acid, O~S<oH, at the same dilutions, and shows that the former acid is much stronger than the latter. This result, lie points ont, is interesting from the fact that the influence of the NB,group upon the streiigth of organic acids generally is just of the oppositu character, as is vell known, and gives a confirmation of the view n1reacl-Y publishcd (Proc., 1894, 137)on the constitution of glycociri and othw orgmic amido-acids. The $act that organic nmido-acids are w-eaker than tlic non-amidated acids, mbils t amido-sulphonic acid is stronger than siilphurous acid, of which it is the arnido-derivative, shows that mere prcwnce of NH, does nct iliminis'i the strength of an acid. The difference c~n only b3 understood by assuming that, in the case of the former class of acids, the nitrogzn of the basic group, -R"*NH2, is in combination with the hydrogen of the acid group, -CO?H or -S03H, thus H,N.R"*CO0,or H,N*R"*S02*0,the L-J L-J dissociation oE these moleculcs into H, on the one hand, and H21S*R"*CO-0,or H2N*R"*S02*0,on the ot,lier, occurring to a much L--I L-J less extent than in the case of tltc non-aniicjatcd acids, which dis-sociate into 11 and R'*C02or R'*SOJ.Finally, the author considers the dilution formula of electrolytes recently proposed by Rudolphi (Zeit. phy4kaZ. Chem., 1895, 17, 385) and van't Hoff (Zed.physikaZ. Chenz., 1896, IS,300),2nd shows that his results are in agreement with thes2 formulze. 132. " The physiological action of a-idosulphonic acid." By Oscar Loew, Ph.D. Amidosulphonic acid, applied as its calcium or sodium salt, proves to be noxious to the life. of phmogamous plants, but not to algm, or to thc lower fungi. It is not poisonous to the lower aqutttic fornis of animal life, such as Infusoria, Itotatorin, Copepods ; and, from experi- ment,s made by Prof. 0.Takahashi,it proves to be also not poisoi~ous to vertebrate animals, such as the dog and the frog, That its poisonous action should be confined to flowering plants is a point of much interest. 133. ''HOWmercurous and mercuric salts change into each other." By S.Hada, B.Sc. By the results of numerous experiments, the ways are shown by which mercuric salts iii presence of water become mercurous, and mercurous salts become mercuric. Very much has been observed aiready by others concerning such a common subject, but the state- ments based on past experience have been unczrtain and even con-tradictory, and nearly every point has had to be worked out anew. It has now been ascertained tliat a cold solution of mercuric nitrate shaken with mercury is at once aud fully conrerted into one of meiwmous nitrate, one of mercuric acetate into mercuro~s acetate, and one of mercuric chloride iiito simple water and a precipitate of mercurous chloride. As was bctter known, moist mercuric sulphate or phosphate quickly becomes ail mercurous salt, with evolution of heat, when rubbed with mercury.Mercurous nitrate in boiling water becomes rnercuric nitrate and metallic mercury, which distils with the ,steam. Other mercurous 183 salts, solulule or insoluble, e.q., the chloride, behave aimilarly. This dissociation procceds also at lower temperatures, eren to a measur- able extent at 40°, in the case of the nitrate, on condition thaf, by a current of air, the mercury vapour is carried away. Mercurous salts, in solutioii or moist, are also all dissociated at the common temperalure by strong daylight, the acetate allowing the effects of dissociation to be very clearly observed. Mercurous nitrate, when free from its mother liquor, is a stable salt, unchanged in the air: if not exposed to bright light.I11 solution in tIic dark, in a closed 1-essel,it is also stable even in an atmosphere of osjgen. There is no evidence that this or any other mercurous salt, whether in solution or only moist, is oxidisable in the air at comrnoii or oiily moderately elevated tempertttuyes. What has been sapposed to be the effect of' oxidation, as iu MialhA's experiments, is the effect of dissociation. Mercurous oxide alone is oxidisable. Nercurous salts, in presence of watey, and best when in solut.ion, osidise in air or oxygen at a temperntnre of 150". Thus, mercurous chloride can be largely, if not wholly, changed by oxidation into mercuric chloride in presence of hydrochloric acid. When mercurous chloride, boiled with lijdrochloric acid under atmospheric pressure, becomes mercuric chloride, it does so by dissociation, not by appre- eiable osi2ation.Mercurous nitrate in water at the common temperature, but in strong daylight,, becomes mercuric salt by reduction of its own nitric acid to nitrous acid. Exposure in an open vessel, 01-to au attospEtere of mercury rapour, or even to undiluted oxygen, retards the progress of the change by keeping down the quantity of nitrous acid which ot'neiwise increases with time. An atmosphere of carbon dioxide favours, that is, does not impede, the change. Merciirous nitrate also freely becomes mercuric nitrate and nitrite when kept in solution at 150" under pressure. Mercurous oxide both oxidises and dissociates at the common tem- perature, as has been shown by Barfoed.Exposed to the air, it increases or lessens in weight, according to conditions. Shut up in an atmosphere of moist air, it gains in weight, dissociation being checked and oxidation Earourcd. Exposed with large surface to the open air, it loses in weight, for then dissociation and volatilisation of the mercury go on faster than oxidation of the undecomposed mer- C.UIOUS oxide. 134. "The Effect of heat on aqueous solutions of chrome alum." By Margaret D. Dougal. As is well known, the colour of an aqueous solut.ion of chrome alum, when heated, changes from violet or purple to grcen, and, 184 on evaporating, the green solution yields a green, non-crystalline mass.The a,uthor has made a seyies of observations on the relative rates of diffusion of green and violet solutions of the same initial strength which go to prove tliat tlic green diffusate contains less chromium and more sulphuric acid than the violet diffusate, 1~1i;ch is compatible with the assumption that the green solution contains a colloidai, and, therefore, slowly diffusing chromosulphuric acid. This conclusion is in harmony with the results recently arrived at by Monte, and inferred by Whitney, that when a solution OE chrome alum is heated it is resolved into a mixture of potassium sulphate, chrornjlsulphuric acid and free sulphuric acid, according to the following equation :-2[Cr2(S04)3*K2S04]i H20 = [Cr40(S0,),]X04 + 21.,S04+ H,SOs. Experiments have also shown that solutions of chrome alum, aftel.heating, are less dense than the unchsngcd or violet solutions, the expansion being due, in all probabilit?, to the pr.oduction of the free sulphuric acid. 135. '' On the hydrolysis of ethylic dicarboxylglutacoiiatbte." By H. W. Bolam, B.Sc., Ph.D. It was found impossi bla to prepare glutacoiiic acid in quantity from ethjlic dicarboxylglut~conate, following the directions of Conrad and Guthzeit (AnvaEeit, 222, 254). Attempts to pi-epre this acid from /?-oxyglutaric acid likewise failed. No oxyglntaric acid, such as v. Pechmann and Jenisch (Be?..,1891,24,3250) describe, could be isolated from the product of the reduction of acctoncciicarboxylic acid by means of sodium amalgam. It mas Pouiid that ethylic dica~boxylglutaconate nndern-mt, on boiling witli alkalis (baryta and caustic potash), a remarkable dec:oin-position, the products being nialonic acid and formic acid.The yields of glutaconic acid are still further reduced bx the action of alkali, it being shown that oxyglutarates (possibly p-) are formcd. Thc decomposition is effected on bohg with a cize per cent. solu-tion of harjtn; in the cold, on thc other hand, no such decom-position was observed with even a 20 pcr cent. solution of catustic potasli. On saponifying the etliylic dicarbosylglutncoriate with acids no such decomposition takes rlace ; here, liower-er, sjrupy pi-oducts, presumably 130th a-and /hoxTglntaric acids and the lnctone acid, butyrolactonc ca~*'uoxjlic acid, are formed, and these liiiider the crys-tnllisation of the glutaronic acid.Using 11 per cent. hydrochloric acid, and obserying certain precautions in boiling, aud 011 evaporation, yields of from 50 to 60 per cent.. of glutaconic acid are got. 33thylic benzyl dicarboxg Iglutacon,zte undergoes no decomposition on boiling with alkalis, nor does the benzylglutaconic acid thus formed show any tendency to form oxy-acids. It is supposed that other a1ky1 snbstitu ted e th ylic dicarbox ylgl utaconates behave sim i-larly, and it is suggested that an explanation of the decomposition of the simple ethylic dicarboxylglut’aconate is to be found in the presence oE the hydrogen atom replaceable by a metal, and that, further, only ethers having such a replaceable hydrogen atcjm may be expected to show an analogous deconlposition on boiling with alkalis.136. “The periodic law.” By R. M.Deeley. In this paper it is pointed out that the manner in which the elements poup themselves rnries according to the comparative im-portance which is attached to their several physical and chemical propert icb. The elements have generally been grouped in accordancc with their most shiking chemical properties. When thus grouped the author shows that many of them do not fall in with a regular periodic sjstcm, and the arrangement would seem to indicate that quite a numbcr of elements of small atomic weight remain to Le discovered. On the otlier hand, wLen they are grouped in accordance with the periodic changes in the values of many of their physical properties, the result is much more satisfactmy-.As an example, the refraction equivalents we instanced, helium being shown to fill :I blank for n missing element (pointed out in a previous paper), whilst argon falls most naturally between sodium and fluorine. The periodic arrangement proposed nmkcs tbc list of elements of smaller atomic weight than iodine complete, if we discount the pvssibility of the existence of a, whole group of inert elements of lower atomic weights respectively than Iiydrogen and the alkali metals. 137. The colouring matters occnrring in various British plants.”Part I. By A. G. Perkin and J. J. Hummel. Formerly numerous British plants mere employed in dyeing, and at present in remote districts, notablg the Highlands of Scotland, some are still used for this purpose.Many of these have been found sufficiently strong in colouririg matter to marrant toheir chemical 6 examination. The colouring matters of the yellow walljlower, Cheiranthus cheiri.- An aqueous extract of the flowers when digested with acid deposits a precipitate of colouring matter; this was found to consist of two mbstances which could be Eepnrated readily, owing to the difference of their solubilities in alcohol. The more soZuLEe product which was obtained a9 yellow needles, had the formula C,,H,,,O,, yielded an acetyl compound, C,,H,O,(C2HaO), ; colourless needle^, m. p. 189-191°; 186 when decomposed with fused a1kali, pratocatechuic acid and phloro- glucin were produced.It was found to be piercetiti. The sparingly solubIe colouring matter, Cl6Hl20,,minute, yellow needles, gave an acetj-1 compound, colourless needles, melting at 195-1‘36’, and when acted upon by lijdriodic acid, it yielded qrher-cetiii, and one molecule of methylic iodide. It was thus a qziemetin monometlryl ether. Though closely resembling rhamnetin it is not identical with it,for acetylrhamnetin melts at 184-lSfi0 ; and for it is proposed the name isorhanznstin. The cohritzg matter in white hawtliorn ~~OESOIIIS,Cretagus oxycantha, was obtained as yellow needles having the formiila Cl5HI007.Its acetyl compound, colourless needles, melted at 189-191°, and when fused P ith alkali, phloroglucin and protxatechuic acid were formed.There could be no doubt as to its identity nyith qzcercetiu. It is most probable that these colouring matters exist in the above plants as glucosides. This point will be studied at a later date. 133. ‘‘Position-isomerism and optical activity ; the comparative rotatory powers of the dibenzoyl and ditoluyltartrates.” By Percy Frank- land, Ph.D., F.R.S.,and Frederick Malcolm W harton, A.I.C. Thc authors have rzcently shown (Trans., 1896, 1309) that the rotatory effect of the pars-toluyl radicle is greater than that, of the meta-and this again greater than that of the ortho-tolupl group. This relationsliip, they hare pointed out, is in harmony with the relative position of the centre of grarity in these several groups, for :assuming that the centre of gravity of the benzene ring is the geo- metrical centre of a regular hexagon, it is obvious that in the ortho- arrangement of the toluyl group the centre of gravity is somewhat nearer, in the ineta-arrangement somewhat further, and in the para- zrrnngement still further than that geometrical ccntve from the carbonyl carbon atom by means of which the ring is iu each case attached to the asymmetric carbon atom of the tartaric acid. They have now investigated the relationship subsisting between the rota- tion OE these toluyl compounds and the corresponding benzoyl derivatives.To this end they have studied the rotation, over a wide range of temperature, of methylic and etliylic dibenzoyltartrate, with the result tbat they have found that the rotation of the benzoyl com- pound is iu each case intermediate between that of the corresponding ortho-aad meta-tolnyl derivative.This is also the relative position of the centre of gravity in the respective rings with regard to the carbonyl carbon atom hy means of which they are attached. Methylic and ethylic dibenzoyltartrates, like the corresponding ditoluyltartrates, were found to possess rotatior!s which are vtry sensitive to temperature, the high negative vnliie of the rotatioii 187 diminishing with rise of temperature. In this connection etliylic dibenzoyltartrate was found to exhibit the phenomenon of a maxi-mum rotation. This maximum is situated in the vicinity of its melting point, the rotation values diminishing more and more as it is examined in a state of superfusion at temperatures further and further below its melting point.139. "Researches on the terpenes. VII. Halogen derivatives of cam-phor." By J. E. Marsh and J. H. Gardner. When camphor is treated with a mixture of brdmine arid phos-phorus trichloride at the ordinary temperature, it yields a mixture of two isomeric compounds, of the formula CIOHIIB~*I, a-and /?-tribrorno- camphene hjdrobromides. The two compounds are separated by crjstal I ising from light petroleum . a-Tyibromocumphene hydro bromide crys tallises from chloroform in large colourlcss crystals; it melts at 1G8", and its specific rotatoy powcr [a]D = +90*3".p-Tribromocawphene hydyobromide mtlts at 143-144', and has the rchatory power [a],,= +7.6". When boiled with sodium methylate in methyl alcohol both the above mentioned compounds react in the sime way, losing hydro- bromic acid, and yielding the same trib,.o)5ioc~Z?iphene,C,0Hf313Hr3. Tribromocamphene melts at 75-76', and has the specific rotatory power [a]D = +33-5'. Tlie action of bromine and phosphorus trichloride on other sub- stances haq been examined. Borneo1 yields the same compound (m. p. i6SG) as camphor. Ordinary turpentine gives a new com-pound of the formula CIOHI4BrG,which crjstallises in colourless iieedles melting at 150'. When pentachloride of phosphorus acts OR camphor in the cold two isomcric chlorocampliene hydrochlorates are obtained, which may be sepamted by petroleum ether.One of these compounds, a-cklorocunzplzene hydrochloride, appears to bc in all respects identical with that originally described by Spitzer, having the melting point 155", and specific rotatory power = -9". p-Chlorocamphene hydrochlorate is very sligbtly soluble in petro- leum ether, and crystallises from the hot solution in large, co1ourles~, hard crptals, that obtained by Spitzer forms small, soft, binding crys- tals. %'be new isomeride melts at 16S0, and has the rotatory power [aJD = -27.7'. When boiled with zinc dust and glacial acetic acid it yields clilorocampkene, CIOHI5Cl,a colourless solid of lorn melting point, which distils at 202O, ar.d lias a sfecific rotatory power [aID = -29.7'.Spitzer’s compound also yields a chlorocarnphene by the Sams treatment, but it is difficult to say whether it is ideriticsl with or different,from the derivative of the /3-compound. It is usuaily con-taminated with higher chlorinated producls. When chlorocnmphene is acted on with strong sulphuric acid it dis-solyes, nith evolution of hydrcgen cliloride, and on pouring thc solution into water a liquid is obtained, which can be distilled ii: steam. It has a strung csmphorous smell, and burning taste. It, boils at f230°, and has the composition C,,H,,O. The examination of its properties is not completed? but it appears to be a saturated tertiary alcohol, aiid is probably a hydroxyl derivative of camphene.140. ‘‘Derivatives of cimphenesulphonic acids.” By Arthur Lapworth, D.Sc., and Frederic Stanley Kipping, Ph.D., D.Sc. This paper contains an account of the study of the two camplicne- sulphonic chlorides which are obtained as bje-products in the pre- paration of camphorsulphonic chloride ; the properties of these sub-stances, and those of a11 their more important derivatives, have been briefly described in previous notes (Proc., 2895, 57 ; 1896, 152). 141. Preparation of dimethylketohexamethylene and experiments on the synthesis of dimethylhexamethenylmalonicacid.” By F. Stanley Kipping, Ph.D., D.Sc., and W. B. Edwards. The appearance of a paper by Verwey on “ Peotainethenylmalonic acid and Pentamethenylaaetic acid,” in a recent number of the Berichfe (29, 1996) has led us to take the earliest opportunity of making known the results of some experiments which were com-menced last spring, and which were undertaken, partly with thc object of synthesising dimethylhexflmcthenylrllelonic acid and di-iiiethylhexamethenylacetic acid-liomo2ogues respectively of tbc compounds described by Verviey--and partly with the object of making a general study of hexaniethylene derivatives.To obtain these substances it ww necessary to prcparc dimethjl-ketohexainethylene (Trans., 1895, l349) and for, this purpose illargc quantity of dimethylpimelic acid ,~vasrequired ; in the first place, therefore, we endtavonred to find a better method for preparing this acid than the one previously adopted (Trans., 1891, SSS), and this we acconiplished in the following manner :--Tile acetyldimethyl-csproic acid which is formed, together with dirnethylpimelic acid, by the hydrolysis of ethylic: dimethyldiaoetylpimelate (Zoc.ca’t.), is.dis-solued in excess of aqueous sodium hydroxide arid bromine is then added, iu small quantities at a time, until bromoforui is 110 longer produced ; under these conditioiis the acetyldiinethylcaproic acid seems to bc converted quantitatively into dimetbylpimelic acid. This fact beiiig established, the crude mixture of acids directly obtained from etbylic dimethyldiacetylpimelato may be submittecl to oxidation in the above manner, the troublesonio separation of the two acids thus being atvoided.Having prepared a considerable quantity of dinlethyl piinelic nc;d in this way, we. converted it into dimethylketohexnmeth~le~eby dis-tilling its barium salt and laeduced tlie ketone with sodium in moist ctliereal solntion, thus obtaining the con-esponding nlcohol, which has been recently described by Zelinsky ; this alcohol mas then con-verted into dimethylhexametbplene bromide by treating it witli liydrobroniic acid. We then began to study the conditions uiider which ctliylic dimethylhexametlien~l~i~alonntecould be prepared by tlie interaction of dimethylhexamethylene bromide and cthylic sodiomalonate, but the experiments were interrupted by the summer vacation, slid have not yet been resumed ; as, liowevcr, they will bc continued at an ear1-j-data the publication of this note seemed desirable. The fact that Noyes (Ber., 1896, 2326) has lately obtained from ciihydrocampholytic acid (cis) R ketone which may be identical with di me thy 1ketohexani e t11J len e , e11 1~an c es the i 11 terest w hich is attachecl to the further study of this ccnipound.142. '' Sulphocamphylic acid <C9H,4S05>,with remarks on the constitution of camphoric acid and of camphoronic acid." Ey William HenryPerkin, jun, 'In two previous notices (Proc., 1893, 109 ; 189.5, 2:J), the autlior stated that when sulphocamphylic acid is fused with potash, the principal products of the reaction are two isomeric acids, C9H,?0, (or C,H,,~COOH),for which he proposes the names a-cnnipliyZic acid and /3-campl~yZicacid ; the homer melts at 148O, tlie latter at &out 105'.Besides these two acids, it lias sinc;3 been found that az-di~ethyZ-succinic acid, COOH*C(CH3),-CH2*COOH,and sniall quantities of dicunzphylic acid, C16H2z(COOH)2(m. p. 225") are formed during the fusion. The latter acid, which has not been very fully investigated, is decomposed on distillation, with formation of a-camphylic acid. a-Canqdzylic acid (m. p. 148") is readily acted on by phosphorus trichloride, with formation of a-camnphylie chloride, C,Hl,COC1 (b. p. about 13s-140" at GO mm., with decomposition). The anilide, C,Hl,CONHC,H5, melts at ill",and the ethylic salt, C8HllCOOC2Hj, is a colourless oil, which distils at 132' (i0 mm.). All thess derivatives yield a-camphylic acid again on Iiydrolysis, and not an isomeric acid (see below under P-cainphylic acid).a-CamphyZic ucid dibrowaide, C8H,lBr,~COOH,is formed when bromine is added to the solution of a-caniphglic acid in ch!oroform ; 190 it melts at l57", an13 wl en digested with glacial acetic acid, it is con-verted into bronzo-a-cawpfi ylic acid, C,H,,Br*COOH (m.p. l07'), with elimination of hydrogen bromide. a-Can?phylic acid dihydrobromide, C,€€l,Br2*COOH,is produced by dissolving a-camphylic acid in a saturated solution of hydrogen bromide in glacial ncetic acid. It melts at 156-157", and when boiled with water or digested with quinoliiie it is reconverted into a-camphylic acid. On reduction with sodium amalgam, a-camphyiic acid yields di?~ydl.o-x-can?p7aylicacid,C,H,,*COOR, a colourless oil, which distils at 1G5--170" ($0mm.) ; it is an unsaturated acid, and possibly idrn- tical with the dihydro acid obtained from p-camphylic acid by reduc- tion (see below).When oxirlised with potassium permanganate, a-cnmphglic acid is converted into it new monobaaic acid of the formula C,H,,O,*COOH (m. p. lW),and this acid, on oxidation with chromic acid, is decompose3, with formation of acetone, acetic acid, and other products which are at present under inrcstigation. /3-CnruphyZic acid, C,H,,.COOH (m. p. 105'), combines readily with bromine yielding P-camphylic atid dd?,rornide, C,H,,Br,COOH (m. p. about 177'), and this acid, when liested with glacial acetic acid, loses 1 mol.of hjdrogen bromide with formation of b~onzo-/3-cnmphylicacid, CeH,,Br*(COOH (m. p. 150°), in which the bromine atom is so firmly bound that the acid may be boiled with strong potash, or with zinc dust and acetic acid, for some time without decomposition. When digested with quinoline, there is no elimination of hydrogen bromide, but the acid is converted into G,H,,Br*COOH, isobronzo-p-canz~hylic acid (m. p. 168') ; probably these two bromo-P-campbylic acids are stereoisomeric. /3-CuwplyZic acid, hydrobromide, C,H,?Br*COOH, is produced when /3-camphjlic acid is dissolved in a fuming solution of hydrogen bromide in glacial acetic acid. It melts at 138-140°, and, when boiled with water or digested with quinoline, is reconverted into i3-catnphylic acid. When treated with sodium amalgam, P-camphylic acid yields an oily reduction product, C,H,,~COOH, which boils constantly at 190" (80 mm.) ;this oil is probably a mixture of isomeric dihydrocumphylic acids, as, under certain conditions, it deposits crystals of a dibydro-camphylic acid which melts at 130". Iso-/3-camnphyZic acid, C8HllCOOH, is formed when 13-camphyiic acid is digested with pliosphorous trichloride and the product, after fractionation, decomposed with water.It melts at 130°, and is prob-ably stereoisomeric with p-camphylic acid ; the chloride, C8H1,C0CI, distils with wry little decomposition at 135' (60 mm.) ; the ethylic salt, C8HllCOOC2H,,is a colourlcss oil which boils at 140' (60 mm.), 191 and ths anilide, CsH11CONHCdH5,crystallises in colourless needles and melts at 103d.i'lrhen oxidised, first with potassium permanganate and then with chromic acid, p-camphylio acid yields ax-dinzethlllsuccinic acid, C00HaC(CH3)2* CH,*C0 0 H (m. p. 140°), ax -dintethy IgIzc f ciric acid, COOH.C(CH3),.CH2*CH2*COOH,and a ketonic acid, CeH1103,which melts at about 50-51'. This latter acid gives a beau tifully crystalline sew icarbaaoue C9R,,N30, (m. p. 187') ; on oxidation with nitric acid, it gields ax-dirnethylsuccinic acid, and, wlien treated with bromine and potash, it is decomposed, with formation OE tetrabromometliane and act-di- methglglutaric acid; it is therefore exceedingly probable that it is of the foormnla CH3.CO*C(CH3),*C€I,*CH2*COOH,an acctyZdimethyZ-bihy-z'c acid, and very likely identical with an acid, CYNlt03,which Tiemann (Ber., 1895, 28,ZliC,) obtained by the oxidation of p rEi-h?ldr~xyd.il~yd,.ocr?np~o7e~~~cacid with chromic acid, and to which lie assigns tlie constitution given above.The Tarions decompositions of u-and p-camphylic acids, briefly stated above, as well as the results of a number of further experi- ments, which the author hopes soon to be able to communicate to the Society, throw much light on the constitut,ion of these acids, as well as on the constitution of sulphocamphylic acid, and indirectly on that of camphoric acid. In this short abstract it is, of course, not possible to enter into this matter in detail, but it may be stated that it is exceedingly difficult to account for the observed behaviour of thc;e substances on the assumption that the forinulm either of Bredt CT of Tiemann for camphoric acid are correct.If, however, camph- oric acid has the constitution represented by either oE the following forniu1;r:: (of nhich the author considers formula I the more probable), then riot, only the formation of acetyldimethyl butyric acid from sulpho- camphjlic acid, but also the various decompositions of the camphylic acids may be readily understood, and the author has furt.her satisfied himself that all the other reactions of camphoric acid are at least as readily, and, in most cases much more easiiy, explained with the help (Jf these formula than with that of any other formuls which hare, SO far, been suggested. The author hopes that the discussion of these new formulae will be reserved until he has been able to explain thpir 192 application in the detailed description of the experimental results indicated above.Campltoronic acid.-Bredt has assigned to this acid the foi*mul,z C0OH*CH2*C:(CH,),( COOH) CH,*CO0 H, and it seems very probable tliat this expression (which also follows from the formuh I and 11 given above) is the correcf one. Tiemanil (Ber., 1895, 28,lo@), 011 the other hand, represents camphoronic acid as COOH.CH(CHJ *C(CH,) L*CH(COOH),, and tvheii the paper putting forward this view appeared, the author pyit.ately suggested to Professor Tiemann that this expression could hardly be correct, since the acid, on heating, does not lose carbon &oxide, forming a corresponding dibasic acid, as would be the case if,as represented, the acid were a derivative of malonic acid.Tiemanil (Bey., 1895, 28, 2163) replied to this that the acid did .tlot decompose in this way, because it first loses wat,er, mid yields 7H(CHs)*C(CH,) 2.7 H.COOH , whichn11hyd roca rnp7io~onic acid, co-0-lieco considers would be stable at high temperatures. But au acid oE this CH2*CH,*$!HGOOHformula is similarly constituted to 0-co ,carbobutyro-1 lactonic acid, which, at 120”, very readily decomposes, with elimina- tion of carbon dioxide and formation of butyrolnctonc. In contact with witer, anbydrocamphoronic acid is at once con-vcrtcd into camphoronic acid, and it appeared to the author that the validity of Tiemann’s formula might be tested by heating an aqueous solution of camphorouic acid at high temperatures.The result of experiments on this point showed that camplioronic acid is not appreciitbly decomposed when heated with water in sealed tubes at 2‘15-235’ for two hours, a result which appears to the author to prove conclusively that Tiemann’s formula cancot be correct. In confirmation of this it may be mentioned that Bredt (AnFhaZciL, 292,131) lias lately shown that the triethylic salt of camphoronic acid, wliich according to Tiemann shoald contain the group -CH(C00C,H5)2, does not react Iviith sodium. 143. ‘‘ On Pettenkofer’s method for determining carbonic anhydride in air.” By Professor Letts, D.Sc., PhD., and R.F. Blake, F.I.C. The authors discuss the errors in the process of absorbing the car- bonic anhydride from a ?ample of air collected in a glass vessel by barytn, and titrating with acid, and show that, in addition to the more obvious sources of error, the zction of the alkaline absorbent, on thc glass is one of importance. In order to aroid it they coat both the receiver cohining the air 193 sample and the bottle holding tlie stock of standard solution of baryta with parafin was. By this means they at onc3 obtained more conccrdant results in a series of determinations. They then proceeded to test tlie degree, both of accuracy and of dslicacy, of Pettenkofer's process if carried out with all the available precautions which sug-gzsted themselves. For this purpose they employed paraffined re-ceiving vessels, an apparatus for performing the titrations in a yamurn, and burettes of special construction. In addition, an apparatus ~'RS used for delivering, rery accurately, measured volumes of pure car-bonic anhydride into known volumes of air previously freed from that gas.Experimenting with such niixtures of the two as occur in air, con-taining about 3 vols. carbonic anhydride in 10,000, the authors show that with careful work the mean error in the dcterminntions need not exceed -0.04 part. The actual quantityv of carbonic anhydride added to each receiver full of air, in R series OE five experiments, amountel to 0 927 C.C.; the mean amount, found to he 0 916 c.c., giving, tlierefitre, a mean erroi' of -0.011 C.C.They thus show that Pettenkofcr's process, if suitably performed, is one of great accuracy and delicacy. After giving tlie results of a series of determinations of carbo:iic anhydride in ordinary air, the authors comment 011 the method described by Messrs. Sgmons and Stephens (Trans, 1896, 869) for such determinations and some of the iesults obtainel by them. Sources o€ error in the process are pointed out, especially the intro- duction of smail quantities of carbonic anhydride with the steam used to reiider the receiving vessels vacuous. Ti1 siipport of this rontention they draw attention to an esperimciit described by Messrs. Symons and Stephens in which 0.2 C.C.of carbonic anliy-dritle were thus found in a flask of 3 litres capacity, an amount cor-responding with nearly 0.67 -i-olnnies in 1@,000supposing the flask to hare been filled with air, m-hich is iiearly one.fifth the total quail- titj usually found in '' fresh " air. Although awt'nre of the error thus introduc?d, Messrs. Symons rind Stephens di not (as far as the authors can judge from their paper) niake any correction for it in their su bseqnent. deterinittu- tions. 194 ’ ADDITIONS TO THE LIBRARY. 1. By Purchase. And&, L. E. Papier-Speciali taten. Praktische Anleitung zur Herstellung von, de=1 verschiedensten Zwecken dienendeii Pnpierfnbri- kanten, wie Pergnmentpnpiere. xvi +288 pp. Mit 48 Abbildungeu.\Vein, Pest, Leipzig 1896. Fiugge, Dr. C. Die Mikroorganismen. Mit besonderer Beriizk-sichtigung der Atiologie der Infektiouskrankheiten. Dritte, vollig umgcarbeitete Auflage. Erster Tlieil. xvi+ 596 pp. Rlit 57 Abbil-dungenim Text. Zweiter Theil. xxiit 751 pp. Nit 153 Abbildungen im Text. Leipzig 1896. Gatt,ermann, Ludwig. The Practical Methods of Organic Chemistry. Translated by William B. Shober. With numerous illustrations. xi+-330 pp. New York lS9G. 8\70. Helmholtz, H. v. Zwci Hydrodynamische Abhandlungen. Hernus-gcgeben von A. Wangerin. 79 pi?. Leipzig 1896. (Ostwald’s Klassiker der Exakten Wisserrschaften. No. 79.) Kahann Wilhelm. Kurze Anleitung zur Chemischen Untcr-suchung yon Rohstoffen und Produkten cler landwirtscliaftlichen Gewerbe und der Fettindustrie.x +133pp. Mit 3 Abbildungen iui Ttxt. Leipzig und Wicu 1896. Kohlrausch, F. Leitfaden der Praktischen Phjsik mi t einern Anhange des absolute hiIsss-system. Nit in den Tcxt geclruckten Figuren. Achte vermelirte Auflage. xusiv +492 pp. Leipzig 1896. Ohlmuller, W. Die Untersuchung des Wassers. Mit 75 Textab-bildungen und einer Lichtdrucktafel. Zwe:te durchgeseline Auflage. xi +178 pp. Svo. Berlin 1596. Scoffern, John. Chemistry no Mystery ; or a Lecturer’s Bequest. Arranged from the Original Manuscript, and revised by. vii+31Q pp-London 1839. Thomson, Thomas. The History of Chemistry. Second edition. 2 vols. in one. vii+ 349 +325 pp. London. Windisch, Karl. Die chemische Untersuchung und Beurtheilung des Weines.Mit 33 in den text gedruckten Figuren. xis+351 pp- Bcrlin 1896. 11. Donations. Ackroyd, William. The Old Light and tho New: Dealing with the Chemistry of Colour and the New Photography. 102 pp. Lon-don 1896. From the Author. Aikin, Arthur. A Nltnusl of Mineraloqy. Second edition, with additions and corrections. viii +263 pp. London 1815. From S. G. Rosenlluni, Esi. 196 Allen, Alfred H. Commercial Organic Analysis. Vol. 111,Part 111. xii +508. London 1896. From the Author. Brande, W. T. A Manual of Chemistry, containing the principal facts of the Science, arranged in the order in which they are dis-cussed and illustrated in the lectures at the Royal Institution of Great Britain. xlvii +652 pp. London 1819.From S. G. Rosenblum, Esq. The Chemist. Vols. I and 11. 1824-25. From S. G. Rosenblum, Esq. Clare, M., F.R.S. The Motion of Fluids, Natural and Artificial ; in particular that of the Air and Water. 369 pp. London 1737. From S. G. Rosenblum, Esq. Clowes, Frank, and Coleman, J. Bernard. Elementary Quantita- tive Chemical Analysis. xv+238 pp. London 1896. From the Authors. Clowes, Frank, and Redwood, Boverton. The Detection and Measurement of Inflammable Gas and Vapour in the L4ir. xii +206 pp. London 1896. From the Authors. Cumberland, Richard. An Essay towards the Recovery of the Jewish Measures and Weights, comprehending their Monies. 140 pp. London 1686. From S. 0.hosenblum, Esq. Dey Kanny Lall. The Indigenous Drugs of India.Second edition. xxxviii -+ 387 pp. Calcutta 1896. From the Author. Evans, J. Castell. A New Course of Experimental Chemistry, in- cluding the Principles of Qualitative arid Quantitative Analysis. T’hird edition. xi+244 pp. From the Publishers. Fresenius, Dr. C. Remigius. A System of Instruction in Quanti- tative Analysis. Second edition. Edited by J. Lloyd Bullock, F.C.S. xvi+624 pp. London 1854. From S. G. Rosenlolum, Esq. Gurney, Goldsworthy. A Course of Lectures on Chemical Science as delivered at the Surrey Institution. v+310 pp. London 1823. From S. G. Rosenblum, Esq. Hamilton, Hugh, D.D., F.R.S. Philosophical Essays on the fol- lowing subjects :-I. On the Ascent of Vapours, the Formation of Clouds, Rain, and Dew, and on several other Phenomena of Air and Water.11. Observations and Conjectures on the nature of the Aurora Borealis, and the Tails of Comets. 111. On the Principles of Mechanicks. Fourth edition. 172 pp. London 1783. From S. G. Rosenblum, Esq. Hoff, J. H. van’t. Studies in Chemical Dynamics. Revised and enlarged by Dr. Ernest Cohen. Translated by Thomas Ewan, M.Sc., Ph.D. vi+286 pp. With 49 figures in the text. London 1896. From the Translator. Kidd, J. Outlines of 3fineralog-y. vol. I. ix+255 pp. ; Vol. 11. viii +227. Appendix 39 pp. London 1809. From S. G. Rosenblum, Esq. Lavoisier. Elements of Chemistry in a new systematic order con- taining all the modern discoveries, illustrated by thirteen copper plates. Translated from the French by Robert Ken*.4th edition. xxxvi+592 pp. Edinburgh 1799. From S. G. Rosenblum, Esq. Liebig, Justus. Organic Chemistry in its application to Agricul- ture and Physiology. Edited from the manuscript of the aut8hor by Lyon Playfair, Ph.D. xvi+387 pp. London 1840. From S. G. Rosenblum, Esq. Liebig, Justus. Animal Chemistry or Organic Chemistry in its applications to Physiology and Pathology. Edited from the author’s manuscript by William Gregory, M.D. xix +354 pp. London 1842. From S. G. Rosenblum, Esq. Liebig, Justus. Lettres sur le Chimie et sur ses applications 8 l’hdustrie, 2la Phgsiologie et & 1’Agricalture. Traduites de 1’Alle- mand par le Dr. G. W. Bichon. xi+331 pp. Paris 1845. From S. G. Rosenbliim, Esq. Liebig, Justus. Nouvelles Lettres sur la Chimie, consid6r6e dam ses applicatioiis B l’Industrie, 8 la Physiologie et 1’Agriculture.Edition Fmnqaise publi6e par Charles Gerhardt. xii+330 pp. Paris 1852. Prom S. G. Rosenblum, Esq. Mead, Richard. A Mechanical Account of Poisons in several Essays. 175 pp. London 1702. From S. G.Rosenblum, Esq. Musschenbroek, Petro van. Institutiones Physic=. Conscript= in usus Academicos. 743 pp. Leyden 1748. From S. G. Roseiiblum, Esq. Orfila, M. P. Trait6 des Poisons tires des r6gucs mineral, vBg6ta1, et animal, OLI Toxicologie GAnArale, consid&& SOLIS les rapports de In Physiologie, do la Pathologio et de la Mbdicine LAgale. Seconcle Qdition. Vol. I. xxxii+ 658 pp. ; 11. xvi +703 pp. Paris 1818. From S. G. Rosenblum, Esq.Parkes, Samuel. The Chemical Catechism with notes, illustra- tions, and experiments. 7th edition. x+ 562 pp. Londoii 1816. From S. G. Rosenblum, Esq. Parkes, Samuel. The Chemical Catechism with notes, illustra- tions, and experiments. 8th editlion. xxv +618 pp. London 1818. B’rorn S. G. Rosenblum, Esq. Rontgen, Robert. Die Grundlehern der mechanischen Wiirme- theorie. Erster Theil. xiv$330 pp. Mit 49 eingedruckten Holz-schnitten. Jena 1871. From S. G. Rosenblum, Esq. Salmon, William. Supplement to the New hndon Dispensary in I11 Books. Containing a supplement I to the Materia Medics ; I1 to 197 the Internal Compound Medicaments ; 111to the External Compound Medicaments. 720 pp. London 16S3. Prom S. G. Rosenblum, Esq. Short, Thomas.An Essay towards a Natural, Experimental, and Medicinal History of the Principal Mineral Waters. xix+330 pp. Sheffield 1740. From S. G. Rosenblum, Esq. Sutton, Francis. A Systematic Handbook of Volumetric Ana- lysis ; or, the Quantitative Estimation of Chemical Substances by measure, applied to Liquids, Solids, and Gases. Seventh edition, enlarged and improved. xi + 587. London 1896. From the Author. Thorpe, T. E. Humphrey D~tvy,Poet and Philosopher. vii+240 pp. London 1896. From the Author. Tollens, B. Les Hydrates de Carbone. Traduit de l’Allemand par LQon Bourgeois. vi+770 pp. Avec 24 figures dans le texte. Paris 1896. From the Publishers. Whytt, Robert. An Essay on the Vital and Involuntary Motions of Animals. xf392 pp.Edinburgh 1751. From S. G. Rosenblum? Esy, At the next meeting on Thursday, Nov. 19t11, t>he fdlowing papers will be received :-“ Mercury hyponitrites.” By P. C. RBy, D.Sc. “ The nitrites of mercury and the conditions under which they are formed.” By P. C. RBy, D.Sc. “ The interaction of mercurous nitrite and the alkyl iodides.” By P. C.RBy, D.Sc. “ Crystallography of the monohydrated mercurous nitrite.” By T. H. Holland. “ Snlphocamphoric acid and other derivatives of camphorsulphonic acid.” By A. Lapworth, D.Sc., and F. S. Kipping, Ph.D., D.Sc. “ Solution and diffusion of certain metals and alloys in mercury. Part 11.” By W. J. Humphreys. “ Noteeon the heat of formation of the silver amalgam, Ag2Hg8.” By Fannie I. Littleton.“ On the identity of dextrose from different sources with special reference to the copper oxide reducing power.” By C. O’Sullivan, F.R.S., and A. L. Stern, D.Sc. LIST OF PUBLICATIONS WHICH MAT BE SEEN IN THE SOCIETY’S LIBRARY. Academia Nacional di Ciencias de Is Cordoba. Republica Argentina. Boletin. Academy of Natural Sciences of Philadelphia. Proceedings. Akademie (Kaiserlich-Leopoldinisch-Carolinisch-Deutsche) der Natur- forscher. Verbandlungen. (Also with the title : Nova acta AcademiE Csesareze Leopoldini-Carolinx: Germanicorum nsturze curiosorum.) 4to. Akademie (Kaiserliche) der Wissenschaften in Wien. Denkschriften. (Mathematisch-NaturwissenschaftlicheClasse.) .-Sitzungsberichte. (Mathematisch -Naturwissenschaftliche Classe.) Akademie (Koniglich-Preussische) der Wissenschaften zu Berlin.Monatsberichte. Akademie (Eoniglich-Bayerische) der Wiesenschnften in Miinchen. Abhandlangen (Mathematisch-Physikalische Classe). 4to. Sitzungsberichte. Akademie (Ungarische) der Wissenscliaften. Mathematische nnd Naturwissenschaf tliche Berichte aus Ungarn. American Chemical Journal. Remsen. 2 copies, American Journal of Pharmacjr. American Journal of Science and Arts. Silliman. 8vo. New haven. 2 copies. American Chemical Society. Journal. 2 copies. American Philosophical Society. Proceedings. 8v0, Transactions. Analyst. 2 copies. Annalen der Chemie und Pharmacie. 2 copies. Annalen der Physik und Chemie. Herausgegeben von J. C. Poggen-dorff. 8vo. Leipzig.2 copies. Annales Agronomiques. 2 copies. Annales de Chimie et de Physique. 8vo. Paris. 2 copies. Annales de 1’Institut F’asteur. Annales des Mines, 011 Recueil de MBmoires sur 1’Exploitation des Mines. RQdig6es par les IngBnieurs des Mines. Paris. Annali di Chemica e di Farmacologia. 199 Annuaire de 1’Acadhmie Royale des Sciences, des Lettres et des Beaux-Arts de Belgique. Apotheker Verein (Allgemeiner Dentscher). Archiv der Phar-macie. Archiv der Pharmacie. Archiv fiir Hygiene. Archiv fur die gesammte Physiologie voii Menschen und Thieren. Herausgegeben von F. Pfluger. Archiv fur Pathologische Anatomie und Physiologie und fiir Hli-nische Medicin. Herausgegeben von Rudolf Virchow. Archives Nkerlaiidaises des Sciences exnctes et naturelles.Army Medical Department. Reports. Asclepiad. Australasian Journal of Pharmacy. Berichte cler Deutschen Chemischen Gesellschaft zu Berlin. 8170. 1868. 2 copies. Biedermann’s Centralblatt fur Agrikulturchemie und rationellen Land wirthschaf ts-Be trieb. 2 copies. Birmingham Philosophical Society. Proceedings. Bulletin de 1’Acadhmie des Sciences, des Lettres et des Beaus Arts de Belgique. 8ro. Bruxelles. Bulletin de l’Acad6mie Imphriale des Sciences de St. Pktersbourg. Bulletin de l’bbsociatioa Belge des Chimistes. Bulletin de la Soci6th Chimique de Paris. 2 copies. Bulletin de la Soci6th Industrielle de Mnlhouse. Bulletin de la Soci6tk des Nataralistes de iJloscou. Bulletin International de l’Acad6mie des Sciences de Cracovie.Bureau International des Poids et Mesures. Travaux. Cambridge Philosophical Society. Transactions. Proceedings. Canada. Geological and Natural History Surrey. Reports. Carlsberg Laboratoriet. Centralblatt fur Bakteriologie. Series I and 11. Chemical News and Journal of Physical Science. 2 copies. Chemical Trades Journal. Chemiker Zeitung. Chemisches Centralblatt. Repertorium fur Reine, Pharmaceutische Physiologische und Tecliaische Chemie. 2 copies. Chemische Indnstyie. Ch emisch-Technisc hes Re pert orium. E. Jacobsen. Chemist and Druggist. Cimento (I1 Nuovo). Giornale di Fisica., Fisica Matematica, Chimica e Storia Naturals. Comptes rendns des S6ances de la SociBtk de Biologic, 200 Comptes rendus Hebdornadaires des S6ances de 1’Academie cles Sciences.2 copies. Cornwall Polytechnic Society’s Annual Reports. 8vo. Falmouth. Deutsche Chemiker Zeitung. Dingler (E. M.). Polytechnisches Journal. 8vo. Augsburg. Dorpat, Pharmakologischeii Institutes, Arbeiten des. Dublin Society (Royal). Sciefitific Transactions. I_-Scientific Proceedings. Electrical Engineer. E11ginee rin g. Fortschritte der Electrotechnik. Portschritte der Physik. Dargestellt von der Physikalischen Gesell- schaft zu Bcrlin. Fortschritte der T heerfarbenfabrikation. Porschungen suf dem Gebiete der Agricult ar Physik. Herausgege-ben von E. Wollny. Gazzetta Chimica Italiana. 2 copies. Geological Society. Quarterly Journal. Glasgow Philosophical Society. Proceedings.Industries and Iron. Jahrbuch d er Orgaiiisclien Chemie. Xinunni. Jahresbericht uber die Fortschritte auf dem Gesanimtgebiete der Agriculturchernie. Jahresbericht uber Pharmacognosie, Pharmacie, uiid Toxicologie, von G. Dragendorff (now Jahrbuch der Pharmacie). J nhresbericlit uber die Fortschritte der Chemie. Jahresbericht uber die Fortschritt e der Chemischen Technologie, fur Fabrikanten, Chemiker, Pharmaceuteu und Cameralisten. Herausgegeben von Dr. Johannes Rudolf v. Wagiier. Jahresbericht uber die Fortschritte der Thierchemie. Herausgegeben von Dr. hichard Xaly. J shresbericht uber Z uckerfabrikation. Herausgegcben von K. Stammer. . Journal of the Camera Club. Journal of the CoJlege of Science. Japan. Journal of the Franklin Institute.Philadelphia. Journal of the Iron and Steel Institute. 8vo. Lolidon. Journal de Pharmacie et de Chimie. 2 copies. Journal of Physical Chemistry, The. 2 copies. Journal fur Praktische Chemie. 2 copies. Journal of Gas Lighting. Journal of the Sanitary Institute. Journal of the Society of Arts. Journal of the Society of Dprs and Clolourists. 201 Journal of the Society of Chemical Industry. 2 copies. Journal of the Federated Institutes of Brewing. 2 copies. Journal of the Tokio Chemical Society. Kern. Bulletin. Kongliga Svenska Vetenskaps -4kademiens Handlingar. Ofversigt a€ Pordhandlingar. Svo. Landwirtschaftlichen Versucbs- Stationen. Organ fur Naturwissen- schaftliche Forschungen auf dem Gebiete der Landwirtschaft.Lincei. Memorie. Transunti. -.-Rendiconti. Liverpool Literary and Philosophical Society. Proceedings. L'Orosi. Local Government BocLrd. Medical Officer's Repcrts. Manchester Literary and Philosophical Society. Memoirs. Proceedings. JIineralogical Society of Great Britain and Ireland. Magazine and Journal. Uineralogische unil Pe trographische Nittheilungen. Herausgegeben von G. Tschermak. llIint (Royal). Annual Reports of the Deputy-Master. Monatshefte fur Chemie. 2 copies. Nonit eur Scien tifique. Nature. Naturhistorisch -Medicinischer Vereiii zu Heidelburg. Verhand-1 ungen. Neues Jahrbuch f iir Minerslogie, Geologie, und Palzontologie. 2 copies. Observatoire de Moutsouris. Annuaire. Pharxnaceut ical Journal of Australasia.Pharmaceutical Journal and Transactions. 8vo. London. 2 copies. Pharmaceutische Rundscliau (now Pharmaceutical Review). Philosophical Magazine. Photographic News. 2 copies. Physical uncl Chemical Society of Russia. Journal. Physical Society. Proceedings. Physikalisch-Medicinische Gesellschaft in Wiirzburg. Sitzungs-berichte. Verhandlungen. Physikali s ch-Technische Reichsanst a1t, Berlin. M'issenschaf tliche Abhandlungen. Q tiarterly Journal of Microscopical Science. Rccxeil des 'I'ravaux Chimiques des Pays-Bas. Repertorjum der Technischen Journal-Litteratnr. Berlin. 202 8-Report (Annual) of the Leeds Philosophical and Liteixry Society. Reports of the Meetings of the British Association for the Advance- ment of Science.Reports of the Meetings of the Australasian Association for the Advancement of Science. Roya1 Agricultural Society . Journal. Royal Astronomical Society. Memoirs. 4to. -Monthly Notices. 8170. London. Royal Institution of Great Britain. Proceedings. Royal Irish Academy of Sciences, Dublin. Proceedings.-Transactions. Royal Microscopical Society. Journal, Royal Photographic Society. Journal. Royal Physical Society of Edinburgh. Royal Scciety of Edinburgh. Transactions. Proceedings. Royal Society of Lordon. Philosophicd Transactions, -Proceedings. 2 copies. Royal Society, Sydney. Transactions. Science Progress. Smithsonian Contributions to Knowledge. Smithsonian Geports. --Miscellaneous Collections. Soap-maker and Perfumer.Stahl und Eisen. Stazioni sperimentali sgrarie italiane. Timehri. The Journal of the Royal Agricultural and Commercial Society of British Guiana. United States Geological Survey. I\IIonographs. Annnal Reports. Veyhandlungen der Nsturforschenden Gesellschaft zu Basel. Verslagen en Mededeelingen des Koninklijke Akademie van Weten-schappen (Af deeling Naturkunde) . Videnskabernes Selskab (Kongelige Danske). Oversigt over det Fordhandlinger. Kjobenhavn. Vierteljahresschrift der Cheniie der Nahrungs und Genussmittei Viertel jahresschrift der Naturforschenden Gesellschaft in Zurich. Year-Book of Pharmacy, and Transactions of the British Pharma- ceutical Conference. Yorkshire Philosophical Socioty. Annual Reports. Zeitschrift fur Analytische Chemie.Herausgegeben von C. Rernigius Fresenius, unter Mitwirkung von H. Fresenius. 2 copies. Zeitschrift fur angewandte Chemie. 2 copies. Zeitschrift fur Anorgsnische Chernie. 2 copies. 203 Zeitschrift fur Biologie. Zeitschrift fur Elektrochernie. Zeitschrift fur Hygiene. Zeitschrift fur Instrumentenkunde. Zeituchrift fur Krystsllogra phie und Mineralogie. Herausgegebea voa P. Groth. Zeitschrift fur Physiologische Chemie. Heransgegeben von F. Hoppe-Xeyler. Zeitschrift fiir Rubenzuckorindustrie. 2 copies. Zeitschrift fiir Physiknlische Chemie. 2 copies. Zeitschrift fur Zuckerindustrie in Bohmen. Journals, duplicate copies of which are in the Library, may be borrowed by Fellows. CERTIFICATES OF CANDIDATES 3’01; ELECTION AT THE NEXT BALLOT.N.B.-The names of those who sign from “ Geiioral Knowledge ’’ are printed in itcclics. The following Candidates will be balloted for on Thursday, December 3, 1896:-Aykroyd, Henry Edward, Ashwell, Tollen Lane, Bradford. One of Principals of Wm. Aykroyd 65 Sons, Oakwood Dye Works. Director of the Chemical and Tecliiiical Investigations at the Dye Works. Seven years private Stiident in B’. W. Richardson’s Analytical Laboratory. Honours Organio C‘lieniistry, Science and Art, 1892. Conjoint author of recent original pnpcrs on “ Sulphites, Snlphates, &c.”, ‘‘ Cachou de Lava1 ” (J.S.C.1). 3Iember of Com-mittee YorBs. See., S.C.I. F.W. Richardson. G. W. Slatter. Henry R. Procter. Arthur Smithclls.J. J. Huminel. C. Kawson. Ballingall, William. “ Ardarr oc h,” Dundee, Manager of Messrs. Ballingall & Son, Brewers, Dunclee. Studied .at University College, Dundee, under the late Dr.. Carnelley, arid .Dr. Percy Frankland, F.R.S. ; also the Chemistry of Brewing, under Mr. Lawrence Briant, F.C.S. E’.R.;?/I.S.,Mem. SOC.Pub. Anal., Master of Arts, St. Andrew’s University. Analytical Cheinist of Park and Pleasance Breweries, Dundee, for past six years. William Frew. Andrew Thornson. James E. Appleyard. Lawreiice Briant. Arthur J. Starey. John Foggie. Frank IT.Young. Bathurst, Charles, jun. Lydney Park, Gloucestershire. B .A. (Oxon), Barrister-at-Law, &c., &c. Gold Medallist and 205 Member of the Royal Agricultural College (by examination). Silver Medallist and Life Member of the Rojal Agricultural Society (by examination).Edward Kinch. Cecil Cooke Duncan. J. Augustus Voelcker. J. I-Ienry Gilbert. A. H. Chnrcb. George Embrey. T.A. Dickson. Bay, Lauritz Hansen. The Grammar School, Carlisle. Science Master at Carlisle Grammar School. Studied under Mr, John Howard, 1188 -1889, and litter under Professor Tilden, at tlie Royal College of Science, S.W. Formerly Science Master arid Lecturer in Chemistry under the Essex County Council, at Palmer’s School, GraTs. Have also lectured in Chemistry under the Derby shire County Council at Wirksworth and Matlock, while Science Master at Wil*ksworth Grammar School. At present attempting Research Work in private laboratory.William A. Tilden. W. Palmer Wynne. Chapman Jones. Arnold Eiloart. H. H. Slater. Browne, Charles Edward. 2, Hinton Villas, Cheltenham. Science Master, the Training College, Cheltenham. G~-aduatein Science (London). 1st Class Honours, Practical Chemistry, Science and Art Department. Science Master and head of Chemical Depart- ment. B. S. Gott, &LA.(Cantab.). A. X.Tutton. Frank Gossling. I?. Neldola. Robt. G. Grimwood. Cobb,Walter William, Hilton House, Atherstone. Assistant Schoolmaster. MA., Oxon, Science Master of the Atherstone Grttmrnar School. Late Junior Student of Christ Chui-ch, Oxford. Honours in Final School of Natural Science, Oxford, 1879. Registered Teacher of Science, under the Science and Art Depart- ment, South Kensington. Since 1879, the pupils of the candidate have gained about 200 certificates, chiefly in Chemistry, from the South Kensington Department.A pyivate pupil is now a Professor at the Royal College of Science, London ; another won 2nd Prize from the Warwick County Council in Chemistry in 1893. Other private pupils have a-on eight medals, including two gold ones for Chemistry, 206 from the Royal (Dick) Veterinai y College, Edinburgh. Candidate is now Lecturer on Chemistry to the Warmick County Council. A. Vernon Harcourt. Harold B. Dixon. T. C. Sharrott. W. TV. Pisiier. John Conroy. V. H. Veley. Cross, George Harold, B.Sc., Balliol College, Oxford. Selected candidate in the Indian Civil Service.Three years in the Chemical Laboratories, 0wens College, Manchester. B.Sc., with 1st Class Honours, in the Honours School of Chemistry, Victoria University. University Scholar in Chemistry, 1893. H. B. Dixon. G. H. Bailey. W. H. Perkin, jun. A. Harden. P. J. Hartog. Duncan, William, Edinburgh. Pharmaceutical Chemist and Teacher of Chemistry and Pharmacy. The candidate has been for 10 years Lecturer in Chemistry to pharmaceutical students, and in Materia Medica to medicid students, at the Royal Dispensary, Edinburgh; this course in the latter is accepted by the University Court. He has also condacted numerous investigations in Pharmaceutical Chemistry, particularly in regard to alkaloids, the resixlts of which have from time to time been published in the Plinmzacez&al Journal.31. Carteighe. Thomas T'yrer. Alex. Cram Brown. John httfield. Alex. Qunn. Peter MacEwan. Leonard Dobbin. Wyndham R. Dimstan. H. Eelbing. Fred. TV. Fletcher. Elliott, Walter John, 5, Dover Place, Clifton, Bristol. Schoolmaster. &LA. Cambridge. Senior Science Master in the Grammar School, Bris tol. Sydney Young. Arthur Richardson. Thomas 11. Easterfield. W. J. Sell. H. J. €3. Fenton. Fleet, John Thomas, Rugby, War wickshire. Analyst,. Examination of Seaweeds, &c., for Iodine. Examination of Blue Clays for Alumina and Iron. Chemical Toxicology. General 207 Analyst in Rugby. Student at Wolsingharn Grammar School. Technical College and Rutherford’s College, Ncwcastle-on-Tyne.Leopold M. Deane. W. F. Wyley. H. W. Jones. Bernard E. Smith. Fatson Smith. T.H. Dodd. G, Xtallard. George, George, Regent Street, Kingswood, near Bristol. Assistant Master, Merchant Venturers’ Technical College, Bristol. Inter. B.Sc. (Lond.). Second Class Honours in Physics. A.T.C. by Examination (January, 1896). Studied Chemistry at Merchant Venturers’ Technical College, Bristol, since September, 1889, under T. Coomber, Dr. Cook, H. J. Palmer, Dr. Tingle, Dr. Leicester, Professor Werthciner, and G. P. Darnell-Smith. Have done a good deal of commercial work in Analytical Chemistry. Am taking Final B.Sc. Examination (Lond.) in October next. J. Wertheimer. G. Y. Darnell-Smith. James Leicester. Ernest H.Cook. J. Bishop Tingle. Hill, Arthur Croft, Trinity College, Cambridge. B.A. (Cantab.) ; 1st class Natural Science Tripos, Parts I and I1 (special subjects, Physiology and Chemistrj). At present engaged in research in Pllysiological Chemistry. James Dewar. W. J. Sell. H. J. H. Fenton. Alexander Scott . A. Sheridau Lea. Hill, Charles Alexander, Hawth3rns, South Road, Clapham Park. Manufacturing Chemist. Studied at the school of the Pharma- ceutical Society ; worked at the Chemical Laboratory, St. Thomas’ Hospital, for one year ; and for one year in the Research Laboratory of the Pharmaceutical Society. Subsequently has been engaged in research work. Associate of the Institute of Cheniistry. Wyndham R. Dunstan. Percy F. Frankland. Herbert Mcleod.Otto Hehner. Francis H. Carr. Hinchley, John William, Batggeholme Road, Lincoln. Metallurgist. Associate of Royal School of Mines (1st class). Kational Scholar (1893). Whitworth Exhibition (1894) and Scholar (1896). 4-5 years in Laboratory at Lincoln School of Science 208 and Royal College of Science. Honours 1st class, Practical and Theoretical (2nd in Chcmistry, 1st in Metallnrgg) Chemistry and Theoretical and Practical Metallurgy, Science and Art Department. W. C. Roberts Austcn. William A. Tilden. John Hope Belcher. W. Palmer Wynne. M. 0. Fomter. J. S. S. Bmme. Lawrence, William Trevor, 57, Prince’s Gate, London, S.W. Private research. B.A., Oxford, Honour Schools, 1893. Ph.D. Berlin, 1896.Three years with Prof. Emil Fischer. NOWin Prof. Perkins’ Laboratory, Manchester. Published work, Die Veybin-dzcngen der Zuckerayten mit &!ereaptanen,Berlin, 1896. Henry E. Roscoe. E. Frankland. F. A.Abe1. M. Holzmann. W. Palmer Wynne. Littlefield, Robert Dexter, 23, Wightman Road, Harringay, N. Student oE Chemistcry. During the last three years have been studying Chemistry and Physics at University College, G-ower Street. Now Demonstrator iiz Chemistry in t’he Laboratory of the Pharma- ceu tical Society . William Ramsay. J. Norman Collie. Morris W. Travers. John Shields, Edward C. Cyril Baly. Arthur Lap worth . W.A I€. Naylor. Lloyd, Thomas Henry, Penygraig, Pontipridd. Analytical Chemist. I have been engaged at tlic Dowlais Iron Company’s laboratory for 3 years, and at Dr.Dykes’ Public Health Laboratory for one year; as Chemist to the Pottsville Iron Com-pany one year, and have worked for 2 years at University College, Cardiff. Claude M. Thompson, M.A., R. W. Atkineon. D.Sc., F.C.S. Robt. H. Owen. A. A. Read. E. P. Perman. Thomas Ihghes. Lockwood, Thomas William, Heckmondwike. Science Teacher. Studied Chemistry at the Dewsburg Technical School, the Royal College of Science, and the Yorkshire College. Studied Experimental and Chemical Physiology at the heeds Medical School. Obtained First Class Honours Inorganic and Honours Organic Chemistry, Science and Art Department, South Kensington. Teacher of Chemistry at the Batley and Liversedge Technical Schools.Science Teacher to the Heckmondwike School Board. Arthur Sinithelle. Henry R. Procter. I. Patchett. Julius B. Cohen. Thos. Ewm. Herbert Ingle. F. W. Bmnson. J. Willis Marshall. William A. Tilden. C hapman Jones. Alfred 11.Allefb. Marfin 0. Forster. G. X.Newth. Manners, Hugh, Academy House, Airdrie. Rector, Airdric Academy. Principal of Airdrie Science and Art School, Teacher of Chemistry, Airdrie Academy, and formerly one of the Science Masters, High School, Glaegow. MA., B.Sc. (Glaa. Univ.). First Class Honours, Practical Organic and Inorgaiiio Chemistry, Science and Art Department. John Ferguson. A. Humboldt, Sexton. J. T. Bottomley. Horatio Ballaiitync. G. G. Henderson. James J. DoEbie. Edzv. C. Stanford.James McCutcheon. Geo. Ritchie. Marks, Edward Seaborn, Astwood House, 111,Cromwell Road, S.W. Metallurgical Chemist. Have studied Chemistry (Theoretical and Practical) at the Royal School of Mines under Professor Thorpe; Physics under Professor Rucker, and Metallurgy under Professor Roberts-Austen, and am an Associate, in Metallurgy, of the Royal School of Mines. T.3;. Thorpe. W. Palmer Wynne. Henry C. Jenkins. Ernest A. Smith. Phi1ip Schidyowitz. Otto Rosenheim. Mayfield, Arthur Stanley, Avenue House, Beverley Road, Hull. Analyst with Messrs. S. Tudor & Co., Lead Woyks, Hull. Have passed Honours Practical Advanced Theory Inorganic. Analyst with Messrs. 8. Tudor & CO., Hull. Have studied at the Royal Institution, Hull, under Mr.G. Carr Robinson, F.R..S.E., F.I.C., F.C.S., and donc general Analytical work. Have made investiga- tions in the manufacture and composition of White Lead, &c. G. Carr Robinson. Allan T. Hall. Fred. E. Johnson. H. Irving Foster. John Pattinso11.. J. Carter Bell. 0. 0. Graham. 210 Miller, William M., Prye Estate, Wellesley Province, Penang, Straits Settlements. Chemist. Diploma and Gold Medal of the College of Science and Arts, Glasgow, 1884. Author of paper on Ruin Manufacture. “Therneri,” Improvements in Rum and Sugar Manufacture (Colonial). James Napier. John S. MacArthur. John Clark. R. R. Tatlock. Horatio Ballnntyne. Moore, Landon Clarence, 19, Mecklenhurgh Square, W.C., Student of Chemistry. Educated at University College School.Have been studying Chemistry for four years at the Birkbeck Institute, and am desirous of devoting myself ultimately to Chemical Research. Particularly wish to receive the Society’s Journal. Undergraduate of London University. J. Woodward. F. Gossling. E. G. Clayton. Temple Orme. Henry Bmlfd. J. Kear Cokuell. MOSS,Francis Ambrose, Menzies, Western Australia. Assayer and Consulting Metallurgist,. Certificated Assayer and Metallurgist. Four years chief Chemist B. H. P. Co.’s Refinery. Present engaged in private practice as Assayer and Consulting Metallurgist. W. T. Gronow. James C. Fi*aser. L. R,. Scammell. T. J. Greenway.T.C,Cloud. moss, Herbert William, Broken Hill Proprietary Co., Ltd., Port Pirie, South Aus-tralia.Metallurgist. Certificated Assayer and Metallurgist and Mine Surveyor. Five years Chemist and Assayer to the B. H. P, Co., Ltd. Present Assistant Superintendent B. H. P. Co., Ltd. W. T. Gronow. T. (3. Cloud. James C. Fraser. L. R. Scammell. T. J. Greenway. Mothe, Joseph Terrence de la, Grand Bacolet Estate, St. Andrew’s Parish, Grenada, West Indies. Agricultural Consulting and Analytical Chemist. Diploma in Agriculture of the Cambridge University. 1st Class Certificate of the Royal Agricultural Society of England. Diploma and Member- ship of the Highland and Agricultural Society of Scotland. Student 211 for over 3 years at Agricultural College, Aspatria. Pupil in Analyti- cal work under Prof. Lloyd since January, 1895.Fredk. J. Llojci. J. Augiistus Voelcker. Alexaiic1c.r Cameron. R. Buclmei-. John 31. Thomson. KerbP rt Jackson . Muter, Alexander Henry Mitchell, The Chhtelet, Horley, Surrey. Anrtlyt,ical Chemist. Three years course in King’s College under Professor Thompon. Subsequently pscd the Examination as Asso-ciate of the Institute of Chemistry, ancl now employed at the South London Public Laboratory. John &I.Thomson. John Muter. Herbert Jackson. Bernard Dyer. Leonard cle Koningh. Pearsall, William Harrison, The School House, Dalton-in-Furness. Priucipal of the Higher Grade School, Dalton-in-Furlless. Smith Me111 oriaI Sc hol ~trship f o1-Advanceci !L‘h eoretica1 3 nd Practica1 Clieniistry, Council Prize arid 4 Queeii’s Prizes (Science and Art Dept.), Birmingham, 18%.Lecturer in Cliemistry, Birmingham School Board. For ycars engaged in teaching the subject in the svlrool lubor(1tories, and also for the Technical Board under Science arid Art Dept. here and at Stoarbridge. Arthur hdams. Horace W. Crow ther. Alfred R. Gower. Charles Baj-liss. Arthur Hadley. Thos. TY. Berry. F. IT’. TVes/azoq. TV. J. Lancaster. 11. S. Xliorthoitse. Willin~tzW. Butlei,. Potts,Henry William, Euroa, Victoria. Analytical Cheoiist. Trained in the Government, Analytical Laboratorr, Quernslaud, u:ider Karl ‘I’heodor Staiger, Ph.D., F.L.S., &c., 1873acd 1874. Examinel*in Cliemistry to the Dental Board of Victoria, under Part)11, “ Medical Act,” 1890-1888--1892.-G~o~e?.)2.-inenf Giczette, Jlay llth, 1838.Analjst to the Xuron Butter, Cheese, and Ice Factory Company, Limited, at which the “ System of Pay-ment by Results ” was formulated and introduced, 1893. Author of several papers on “ Milk Testing, Preserving, &c.” Baron Percl. von Mueller, M.D. L. R. Scarlimell. J. Pond. C. R. Blackett. M. C‘itrteighe. A. W. Craig. 212 Power, Frederick Belding, 21, Queen Square, Bloomsbury, W.C. Director of “ the Wellcome Research Lahoratories,” 42, Snow Hill, E.C. Ph.D. of the University of Strassburg. Foiamerly Professor of Pharniaceutical Chemistry in tlie University of Wisconsin, U.S.A. Late Director of the American Laboratories of Schiminel ‘6Co. H. A. D. Jowett. Wyndham R. Dunstan. R. Meldola. David Howard.Atfred G. HmiLrd. Russell,William, Summerlie, Coatbridge, N.B. Analytical Chemist and Assayer. Pour years in Glasgow City Analysts’ Laboratory. Seven years Chemist to Summerlie & Mossend Iron and Steel Company. Four yeara Lecturer on Iletallurgy at Coat- bridge Technical School ;presently with the Cassel Gold Extracting Co., Glasgow. Robert R. Tatlock. Horatio fialiantpe. A1fred James. John S. Rfa.c.4rthur. Hugh Barclay. Alexandw If. A1 t letin. Saville, Arthur Edwin, 33, Richmond Terrace, Danven. Chemist and Assistant &Tanager of the Ilarwen Corporation Ga3 \Vorks. Has had experience at Gas Works, Sulplittte of Aninionia Works, and Tar Distillation Works, and is frilly qustlitied to tiikt. over management of any or all of these.Hiis a s miid, practical knowledge of Advanced Chemistiy, both Organic and Inorganic. Hy. Ellison, Jun. Thou. Dnxbury. Francis Henry ‘Fate. Geo. -1. JIilq~e. B. Hcttaor?h. Seabrooke, Herbert Cecil, The &hoes, Grays, Essex. Research Assistant. Three years student &’insbury Teoliiiical College. Two years with Dr. lforitz aid Dr. Morris, past 18 months as Research Assistant. Associate of the Jnstitute of Chemistry. G. Harris Illorris. E. R. Moritz. W. TV. Cheadle. Horace T. Brown. J. H. XZillar*. Shimomura, Kotaro, Dotemachi, Kioto, Japan. Professor of Chemistry, Harris School of Scieiicc, Kioto. S.H. (Worcester Polytechnic ILstitute, Worcester, Mass., U.S.A., 1888). Studied under Professor Ira Remsen, Johns Hopkius’ University, 1888-1889.Director and Professor of Chemistry in Harris Scliool 213 of Science, 1889-1896. Papers: ‘LOn the Theories in regard to the Formation and Composition of the ‘ Chemical Elements,’ ” 1888 ; experimental work “ On the Oxidation of certain Aromatic Isomeric Compounds,” submitted to Remsen, 1895. Watson Smith. R. J. Friswell. Edward Kiiich. Arthur J. Dickinson. Wil Ilia ti2 Banisay. Sodeau, William Horace, B .Sc. (Lond.), A.I.C., 25, Shore Road, South Hackney, N.E. Assistant Demonstrator of Chemistry, King’s College, London. Hducated at King’s College, London. Obtained the “ Ilaniell 8cholarship” in Chemistry at that College in 1S91. Passed the liitermediate Science Examination in 1893 wlt8h “ 1st Class Honours in Chemistry and Physics,” and “ Neil Arnott Medal ” in Physics.“ Honours in Chemistry and Physics ” at B.Sc. examination in 1895. John nil. Thomson. W. I>. Hailiburton. Herbert Jackson. Wyndhm R. Dunstan. Patrick H. Kirkaldy. A. K. Huntington. Thompson, Charles, Grammar School, Coatham, Redcar. Science Master. B.Sc. degree of London University in Chemistry, Physics, and Geology. A Teacher of Chemistry for five years. Holder of Honours Certificates in Chemistry from Science and Art 1 Iepzirtmen t. J. E. Stead. Jno. Archyll Jones. Alex. F. Hogg. Wni . Whit eho use. H. Fnmaklasd. E. H. Xa.iLiter. C. H. 12idstlale. H. E. Wright. Walker, William Henry. Stafford Street, Willenhall, Staffs. Xanufacturing Chemist. Four years Student of Cheniisti*y, Free Library Science School, Wolverharnpton.Six months Student in Laboratory of Mr. k’. H. Alcock, Y.I.C., Birmingham. 1st Class Hononrs Practical Chemistry (Science and Art Departmei!t). Xsso-ciate Pharmaceutical Society (lfiiior Examination, 1896). Wm. W hitehouse. Alfred Southall. F. H. Alcock, F.I.C. FV. F. Wyley. H. W. Jones. 1V. H. Richa~dson. Pewy F. FranIr7autl. -7. H. Hichefi., M.A. Watson, William, School House, Kingsbridge, S. Devou. Headmaster of Kingsbridge Grammar School. Student Cheriiical and Physical Laboratories, Oxford. M.A. Oxford. Science Xastei; 2 14 Cowbridge Grnnimar School, Glarnorganshire, 1881--1887. Tcnclier of Scsience under Devonsliire County Council, 1892-1896. Francis Jones. Arthur W.Clayclen. Heiiry T. Gerrnns. Ai*tliurE. Holme. R. L. Taylor. Wheelwright, Edwin Whitfield, The Oaklaiids, Warley, Oldbury, neai-Birmi~iqhnni. Research Chemist. Student of Chemistry in the Yorks. Coll., Leeds, 1884-4. Natural Science Scholar of Balliol College, Oxford, 1858. B.A. 1st Class Honours in Chemistry, Oxford, 1891. P1i.D. Munich, 1893. Geo. S. Albrighf. A. Vernon Harcourt. T. E. Tliorpe. John Conroy.. Arthur Smithells. Whimster, John Inctus, 12, Rutland Terrace, Stockton-on-Tees. Draughtsnian in a Gas Works Contractor’s Offlce. Student of Chemistry for 3 years in Sharp’s Institution, Perth, passing Advanced stage Theoretical and PInctical in the Solzth Kensingtoli Examinations. Oiie year with Professor Pel-cy Frankland and Dr. Thonisoii in University College, Dundee, where I was first in niy year in Theoretical, Prnctical, and Analytical Chemistry ; specially interested in the Chemistry of Gas Manufacture.Percy F. E’rankland. Andrew Thomson. John S. Lumsden. John Foggie. TVriItey Jtcrdine. Junzes R. Appleyard. Pled. ,J. Humbly. Wigner, John Harrison. 58, Breakspear Road, St. John’s, London, S.E. Student. Doctor of Philosophy and Student of Chemistry in Heidelberg University, where he is doing research work under Pro- fessor Jannasch. St?udied Clicmistry previously for three years at hyal Colleges of Science, London arid Dublin. Jocelyn F. Thorpe. Thomas Gray. Alex. 31. Iiellas. R. H. Hxrlaud. Bewznd Dyer. OtfoIfehaer. Wilcox, Alfred James, The Grammar School, Guisborough, Yorks. Tutor.Pupil (24 years) W. E’. Keating Stock, Esq., F.C.S,, F.I.C., Public Analyst for the County of Durham. Teacher (5 years) including Magdalen College School, Brackley, Northants, and Guisbor ough Grammar School. Organised Science School under S.K. Department. W. F. Keating Stock. S. A. Sadler. M. Smith. H. T,Sorreli. A. C. TVilson. HABRISOX AND SONS, Printers iu Ordinary to Her Majesty 8t. Martin’s Lane.

ISSN:0369-8718    

DOI:10.1039/PL8961200163

出版商:RSC    

年代:1896

数据来源: RSC