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Proceedings of the Chemical Society, Vol. 27, No. 386 |
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Proceedings of the Chemical Society, London,
Volume 27,
Issue 386,
1911,
Page 117-130
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PROCEEDINGS OF THE CHEMICAL SOCIETY. Vol. 27. No. 38%. Thursday, May 4th, 1911, at 8.30 p.m., Professor PERCYF. FRANK-LAND, LLD., F.R.S., President, in the Chair. Nessrs. J. Bate and R. Hurst were formally admitted Fellows of the Society. Certificates were read for the first time in favour of Messra. : Arthur Owen Blackhurst, Downing, Broughton, Preston. Ganesh Dat,ts, B.A., Dera Ismail Ehan, N.W.F.P., India. Joges Chandra Ghose, M.A., Bhagalpur, Beha, India. Herbert Jame,s Ling, Hankow, China. Felix Gabriel Paul, No. 64, 38th Street, Rangoon, Burma. William Keighley Walton, Beechwood, Upper Rushton Road, Thornbury, Bradford. The PEESIDENTannounced that a general discussion on the subject of "High Temperatures " would take place at a meeting of the Faraday Society to be held on Tuesday, May 23rd, 1911.A ballot for the election of Fellows was held, and the following were subsequently declared duly elected : John Ernest Roux Adendorff. Arthur Stewart Bowyer, M.Sc. Samuel James Manson ,4uld,D.Sc., Ph. D. John Eric Collington. Ernest Carr Eennison. Clement Arthur Crook. Bichard Charles Bowden, B.Sc. Cecil Reginald Crymble, B. Sc. 118 Atulchandra Datta, N.9. Leonard Owen Newton. William Henry Dickinson, M.B.,Ch.B. Idris Larkby Owen, M.Sc. Oliver Statham Douse, B. Sc. John Lawrence Robinson Pastfield, B.A. Alfred Thomas Eggington, B.Sc. Richard Garnet Penny. Arthur Alfred Eldridge, B.Sc. George Arncliffe Percival. Algernon John Elkington. Albert Cherbury David Rivott, B.A., Alfred Walker Empson.B.Sc. Ralph Roscoe Enfield, B.A. Robert Robison, Ph.D., B.Sc. Thomas Grantham Giddy. Eric Everard Walker. Henry Francis Harwood, M. Sc., Ph.D. Henry Hough Watson. Edwin Burnhope Hughes. Alfred Henry Finniss- Wheldon. Thomae Riley Lncas. William Arthur Reginald Wilks, M. A. Roney Forshaw Messervy. William Wood. Oswald Mansell-Moullin,’ B.A. Robert Wright, M.A. Of the following papers, those marked * were read: *112. The constituents of bryony root.’’ By Frederick Belding Power and Charles Watson Moore. The material employed for this investigation consisted of the freshly collected roots of Bryonk dioica,Linne. The roots were‘found to contain an enzyme, which was obtained in the form cf a light brown powder.This product slowly hydro- lysed the glucosidic constituent of the root, and also effected the hydrolysis of amygdalin and salicin. An alcoholic extract of the root, when distilled in steam, yielded a small amount of a pale yellow essential oil. From the portion of the extract which wm soluble in water, and contained a quantity of sugar, there were isolated: (i) a colourless, neutral substance (m. p. 220--222°), which appears t,o possess the formula C20H3005, and has [a],,+58.6* ;(ii) an amorphous glucosidic product, having a bitter taslte, which, on hydrolysis, yielded a brown resin and a sugar, from which d-phenylglucoaazone (m. p. 208--210°) was prepared ; (iii) an amorphous alkaloidal principle, possessing an intensely bitter taste, which was apparently incapable of forming any crystalline salt.The portion of extract which was insoluble in water consisted of a dark brown, viscid resin, amounting to about 2 per cent. of the weight of dried root employed. From this material the follow- ing compounds were isolat’ed : (i) a phytosterol, C2,H4;0(m. p. 137O), which was optically inactive; (ti) a new dihydric alcohol, bryonol, C2z13202(OH)2, melting at. 210--212°, and yielding a diacetyl derivative, melting at 152O. Bryonol belongs to a group of dihydric alcohols possessing the general formula CnH2n-304,which comprise5 the following additional compounds ipurganol, C2,H3,0,(OH), ; 119 grindelol, C,3H,0,(OH), ;and cucurbitol, C,,H3,0,(OH),; (iii) oleic, linolic, palmitic, and stearic acids.The activity of the root appears to reside chiefly in its resinous and alkaloidal constituents, and the secalled “ bryonin ” of previous investigators has been shown to aonsist of a complex mixture, which was not entirely glucosidic, *113. “Reactivity of the halogens in organic compounds. Part VI. The mechanism of negative catalysis.” ~y George Senter and Alfred William Porter. The kinetics of the reaction of silver nitrate with bromoacetic and a-bromopropionic acids respectively in absolute ethyl alcohol have been measured at 49’9O. The reactions are retarded by nitric acid to an even greater extent than in aqueous solution. A formula which represents the results fairly satisf actorily was given. A formula which reprewnts accurately the decomposition of .a-bromopropionic acid by water has been derived on the assumption that both the anions and the non-ionised acid react with water. It was shown that the usual formula which represents negative catalysis as a difference between two factors is not in accord with the available experimental data.An empirical formula, based on the assumption that the rate of reaction is inversely proportional to the concentration of the negative catalyst, was shown to represent the experimental results very closely. The mode in which accurate formulz representing negative catalysis may be derived was indicated, and the connexion between the accurate and the empirical formulae pointed out. *114. fc The constitution of scopoletin.” By Charles Watson Moore.Scopcletin, a fluorescent substance obtained from ScopoZia japonica and several other plants, has been shown to be 4-hydroxy- 5-methoxycoumarin, since by prolonged boiling with aqueous potassium hydroxide it is converted into 2 :4-dihydroxyanisole. When, however, the alkali hydroxide is allowed to act for a few minutes only on scopoletin, 2 :4-dihydroxy-5-methoxycinnun~icacid is formed. In connexion with the investigation, the following compounds have also been prepared and characterised : 2 :4-Diacet-oxyanisole (m. p. 62-64O) ; 2 :5-diacetoxyanisole (m. p. 94O) ; 2 :4:5-trimethoxycinnamic acid (m. p. 163-165O) ; 2 :4-dihydroxy-5-methoxy-P-phenyZlrropionic acid (m. p. 69O); the Lactone of 2 :4-di’hydroxy-5-methoxy-P-phenylpropionicacid (m. p.155O);the Zactone of 2-hydi.os y-4-acetoxy-5-methoxy-~-phenylpropionicacid 120 (m. p. 135O) ;2 :4 :5-t~il7~ethoxy-~-phenylpropzonicacid (m. p. 96O) ; and methyl 2 :4 :3-ti.irnet~oxy-P-phenylpropionate(m. p. 54O). 115. ‘‘Note on the action of hydrogen dioxide on thiobenzanilide.” By Harold Leete and Edward de Barry Barnett. It has been shown previoudy (Jacobson, Ber., 1886, 19, 1068) that 1-phenylbenzothiazole is produced when thiobenzanilide is oxidised in alkaline solution with potassium ferricyanide. The authors now find that when the oxidation is brought about by hydrogen dioxide in alkaline solution, sulphur is eliminated as. sulphuric acid, and benzanilide is formed.In neutral solution, however, a, compound, C,,H,,ONS, is also formed, and this is the sole product when the oxidation t.akes place in acid solution. As a similar product is not obtained from benzanilide, it would seem that the oxygen is taken up by the sulphur atom, and this receives confirmation from the insolubility of the substance in alkali. No sulphinic acid appears to be formed, its is the case when hydrogen dioxide acts on thiocarbamide in neutral or alkaline solution (Barnett, I‘rans., 1910, 97, 63). In order to bring about the oxidation, the thiobenzanilide (20 grams) was dissolved in alcohol or acetone, a few C.C. of dilute sulphuric acid added, and then 20 grams of a 30 per cent. aqueous solution of hydrogen dioxide. Considerable heat was evolved, and on cooling the oxidation product separated out.This was crystallised from alcohol, and dried in a vacuum over concentrated sulphuric acid : 0.2140 gave 0.5322 CO, and 0.0958 H,O. C=67.8; H=4.93. 0.3252 ,, 17.2 C.C.N, at 17O and 746 mm. N=6.02. 0.3042 ,, 0.3118 BaSO,. S= 14.07. 0.1544 in 15.4 naphthalene gave At= -0’325O. M.W.=216. C,,H,,ONS requires C =68*1; H=4*80;N=6.11; S=13*97 percent. M.W. =229. T?riobemzanilide oxide forms pale yellow, microscopic needles, which, when rapidly lieated; melt at 126%-l%7q 6ut decompose at a considerably lower temperature on prolonged heating. It is readily soluble in hot alcohol or benzene, or in warm aniline or nitrobenzene, but is insoluble in water or ether. 116. ‘‘Purification of acetic acid.” By Kennedy Joseph Previte Orton, llduriel Gwendolen Edwards, and Harold King.Chlorine and bromine do not react with pure acetic acid when light is excluded. Fall in the titre of a solution of bromine in, 121 acetic acid, especially if diluted, shows the presence of certain impurities, which are found in the majority of commercial acetic acids, Both fractional distillation and fractional freezing give but, small proportions of pure acetic acid. Distillation from phosphoric oxide, on the other hand, yields 85-90 per cent. of the acid free from these impurities. With the proper precautions only traces, 0.009-0*04 per cent., of acetic anhydride are produced in this treatment. 117. “The detection and estimation of small quantities of acetic anhydride in acetic acid.’’ By Muriel Gwendolen Edwards and Kennedy Joseph Previt6 Orton.A method of detecting and estimating small quantities of acetic anhydride in aqueous acetic acids was described. The method is based on the fact that certain anilines, notably 2 :4-dichloroaniline, react with acetic anhydride with great rapidity. The anilide can be separated accurately from the aniIine, and then indirectly eetimated in the form of chloroamine. 118. Tetramethylammonium hyponitrite and its decomposition by heat.” By Prafulla Chandra R$y and Hemendra Kumar Sen. A solution of tetramethylarnrr?onium hyponitrite when evaporated in it vacdum over sulphuric acid undergoes partial hydrolysis, resulting in the formation of a ba.sic hyponitrite of the quaternary base.Nitrous oxide, trirnethylamine, nitrogen, and methyl ether are the gaseous products of decomposjition of tetramethylammonium hyponitrite; a small fraction of the hyponitrite is also converted into nit1 ate. 119. “The second and third dissociation constants of ortho-phosphoric acid.” By Edmund Brydges Rudhall Prideaux. A complete account of the changes in hydrogen ion concentration during the neutralisation of the second and third hydrogen ions of orthophosphoric acid has been prepared, partly from the measure ments of Sdm (Zeitsch. physikal. Chem., 1907, 57, 492), and partly from new results. The former results were checked by preparing the solutions in a different way. Equations have been deduced 122 connecting the hydrogen ion concentration of salts of weak polybasic acids with the dissociation constants of these acids.The second and t’hird dissociation constants of orthophosphoric acid as found by Abbott and Bray (J. Amer. Chiern. SOC.,1909, 31,730) have been tested by means of these results and equations. The value k,=2*0 x 10-7 has been confirmed, but instead of k,= 3.6 x 10-13, k, =3.0x 10-12 should be substituted as a result of the present work. The revised constants have been used to construct a general equation which it is hoped will be useful to all who require the standards in question. 120. ‘‘Experiments on tautomerism. Part I. The tautomerism of the syetem X*CHR.CR:CR*X, showing the identity of the a-and 7-positions in the glutaconic acid molecule.” By Ferdinand Bernard Thole and Jocelyn Field Thorpe.The elimination of a carbethoxy-group as ethyl carbonate in several instances already published has led to the general conclusion that when the terminal hydrogen atoms in systems of the above type are all replaced the tendency for the compound to acquire the hydrogen atom necessary to enable it to react in its tautomeric form is such that any group capable of replacement by hydrogen is at once eliminated in the presence of a suitable reagent. Numer-ous experiments in support of this view were described. It was also shown that a-methylglutaconic acid, C02H CHMe*CH:CH*CO,H, and y-methylglutaconic acid, CO,H*CH,*CH:CMe*CO,H, are identical, as are also a-methyl-y-ethylglutaconic acid, C02HCHMe*CH CEt* CO,H, and y-me th y 1-a-et h ylglut acon ic acid, CO,H-CHEto CH:CMe*C0,H.It was suggested that the cause of the identity of the a- and y-positions in the molecule of glutaconic acid is of the same order as that determining the equality of the metapositions in the benzene ring. 121. ‘‘Nitrites of the alkylammonium bases : ethylammonium nitrite, dimethylammonium nitrite, and trimethylammonium nitrite.” By Prafulla Chandra R8y and Jitendra Nath Rakshit. These nitrites are prepared by the interaction of silver nitrite arid the corresponding amine hydrochloride. Ethylammonium nitrite, when heated, decomposes according to the equation 2XEtH3*NO2=Nz+ 3H20+ h’Et2*N0.123 Dimethylammonium nitrite is mainly converted into nitroso-dimethylamine, and the decomposition oftrimethylammonium II it I 1I e is represented by the equation : 3NMe3H*N0,=NMe3H*N03+2N0 +2NMe3+ H,O. 122. “The relation of position isomerism to optical activity. Part IX. The rotation of the menthyl esters of the isomeric fluoro- and iodo-benzoic acid8 and of the halogen derivatives of the fatty acids.” By Julius Berend Cohen. In a former paper the apparently anomalous optical relation of the ortho-, met&, and para,-iodobenzoic esters was referred to, and in view of the important effect of temperature, to which attention was drawn, it was decided to re-investigate the rotation of these three, compounds (previously determined at 20.) at higher tem-peratures. This has now been done, and the temperaturerotation curves have been plotted at 20° intervals up to looo.At 20° the rotations of the three isomerides are identical, [a], -61*5O, whilst at looo there is a slight diminution in the case of the orth0-isomeride, [aID -61.2*, which is greater in the case of the meta-, [a], -60m40, and greatest in that of the parar, [aJD -58O. The three menthyl fluorobenzoates show among themselves a similar relation to that observed among the chlorine and bromine derivatives, the molecular rotations at 20° of the halogen derivatives being as follows : Menthyl ester. F. c1. Br. I. Ortho ............ -194 -5 -195 -205 -237 Meta............... 236 237 239 237 Para ...............239 %37 239 237 In order to determine the effect of the halogens on optical activity in the aliphatic series, a large number of halogen fatty esters have been prepared; but apart from the fact that the effect on rotation generally increases with the increasing mass or number of the halogen atoms, no satisfactory generalisation was arrived at. 123. (( The constitution of dehydro-/l-naphthol sulphide and the interaction of sulphuric acid and aromatic o-hydroxysulph- oxides.” By Thomas Percy Hilditch and Samuel Smiles. The investigation of t.he action of sulphuric acid on the sulphoxides of pcresol and p-chlorophenol has been continued. It is found that the primary products are isomeric with the original 124 sulphoxides, but contain the cyclic thioxin system.The formation of these substances is explained by assuming the production of a sulphonium-quinone from the o-hydroxy-sulphoxide in the same way that the sulphonium-quinones are formed from the o-sulph- oxides of diphenylmethane and diphenylamine by the action of acids. This hypothesis is further confirmed by the behaviour of dehydro-P-naphthol sulphide, which has been formerly obtained by alkaline oxidatioii of P-nanhthol sulphide. It was shown that this substance has the sulphonium-quinone structure, 0:C,,H6: S:Ci,$&j:O, and that it very readily yields na.phthathioxin when treated with alcoholic alkali hydroxide. 124. ‘‘ The action of steam on iron at high temperatures.’’ By John Albert Newton Friend, Thomas Ernest Hull, and Joseph Mallam Brown.The authors have studied the action of steam on iron at various temperatures up to and including 950O. At 500° the reaction was found to be too slow to admit of being carried to completion. The most favourable temperatures for study were found to lie between 650° and 820O. After five hours’ heating at 820°, pieces of iron, 0.05 mm. in thickness, were completely converted into f erroso-ferric oxide. At lower temperatures equilibrium appeared to be obtained between the steam and mixtures of ferrous and ferroseferric oxide in varying proportions. The explanatdon that naturally suggests itself is that the outer layers of the metal have been converted into ferroseferric oxide, and the rate of diffusion is so slow at the temperatures under consideration that a practically infinite time is required for the oxidation of the interior portions.It was pointed out, however, that this is not the only explanation. It may be that definite mixtures of ferrous oxide and ferroso-ferric oxide are produced, having a lower dissociation pressure than f errowf erric oxide, but higher than ferrous oxide, the mixtures being in equi- librium with the steam at the various temperatures corresponding therewith. 125. ‘LAromati~antimony compounds. Part 11. The action of the chlorides of antimony on aniline and its derivatives.’’ By Percy May. The action of antimony trichloride on aniline has been referred to by Schiff (Compt. rend., 1863, 56, 1095) and by Leeds (Amer.Chem. J., 1882, 3,137), but their observations are meagre and 125 contradictory, so that a more detaiied investigation has now been made. Primary aryl derivatives of antimony, such as pamino-phsnyldichlorostibine, NH,*C,H,*SbCl,, do not appear to be produced, but various additive compounds are formed. The following cumpounds have been isolated by the action of antimony trichloride on the corresponding amines under various conditions : Trianiline antimony pentachlode, SbC1,,3NH2Ph ; o-toluidine antimony trichloride, SbCl,,C,H, *NH,; p-t oluidine antimo’ny t?.ir chloride, and p-chloroaniline antimony trichloride, SbCl,,C,H,Cl-NH,. 17zr and p-Nitroanilines do not combine with antimony trichloride under the experimental conditions employed.The above-mentioned compounds dissolve in hydrochloric acid, being thereby dissociated into their constituents. The solutions so obtained yield insoluble, crystalline diazo-compounds of the type R*N,Cl,SbCl, on treatment with nitrous acid. Antimony pentachloride reacts violently with aniline, even when both substances are in dilute chloroform solution. It also reacts very vigorously with benzene, toluene, and xylene. In all these cases, partial chlorination of the aromatic compound takes place, the remainder then forming additive products with the antimony h?ic=hhlc!ridi?, 126. ci Synthetical experiments in the group of the isoquinoline alkaloids. Part I. Anhydrocotarninephthalide.” By Edward Hope and Robert Robinson. An account was given of the preparation and propertiw of anhydrocotarninephthalide, and of a number of its derivatives.127. “The solubility of electrolytes in aqueous solutions, Part I. Solubility of salts in the corresponding acids.” By James Irvine Orme Masson. Determinations have been made at 30° of the solubilities of sodium chloride and of barium chloride in aqueous hydrochloric acid, and of barium nitrate and of silver nitrate in aqueous nitric acid. The concentrations of acid were such that the solubilities of the salts ranged from 100 per cent. to about 3 per cent. of the values in pure water. It has been found that the relation of acid concentration to solubility is well expressed by a simple linear differential equation of the first order.The formula also expresses satisfactorily Engel’s results for the solubilities of numerous chlorides in hydrochloric 126 acid at Oo (Compt. rend., 1886, 102, 619; 1887, 104, 433; Ann, Chtim. Yhys., 1888, [vi], 13,132). Study of the specific gravities shows that the molecular volumes of water, acid, and salt in saturated solution are to be regarded as constant in a given case; that is, they are independent of the proportions in which t’he constituents are mixed. By means of equations embodying this, the specific gravities of the solutions can be calculated with considerable accuracy. 128. ‘‘ The effect of temperature and of *pressureon the equilibrium %COZXO,+C.” By ‘Thomas Fred Eric Rhead and Richard Vernon Wheeler.In Le Chatelier’s general formula for equilibrium in gaseous systems : the effect of pressure, measured in atmospheres, is given by the expression (Ar‘ -R)logeP. Using 5 method of experiment at constant volume different from that previously employed by them (Trans., 1910, 97, 2182), the authors find that this formula holds for the system 2C0 CO,+ C at all pressures between 0.5 and 3 atmospheres for temperatures between 1073O and 1373O Abs. The value of k, however, increases linearly from 59-85 to 20.15 over this range of temperature when the value of L (the total heat of the reaction) is regarded as constant and equal to 39,000 calories, as in their previous communication. The introduction of a value I,, =I,, + 2.025“-0-0031-T2,calculated from the difference between the molecular heats at constant volume of the factors and products of the system, gives the constant a permanent value, 18.74, I,, (the total heat of the reaction at absolute zero) being calcula.ted as equal to 38,055 calories.Le Chat’elier’s equation therefore becomes, for the system under consideration : from which the percentage of carbon dioxide and carbon monoxide in equilibrium over excess of carbon can be calculated for any temper ature and pressure. The rate of attainment of equilibrium is extremely slow at temperatures below 1073O Abs. 127 129. Nitrites of the benzylammonium series : benzylammonium nitrite and dibenzylammonium nitrite, and their sublimation and decomposition by heat.” By Prafulla Chandra Ray and Rasilr La1 Datta.By the interaction of silver nitrite and mono- and di-benzylamine hydrochlorides respectively in aqueous solution, and evaporation in a vacuum of the filtrate, the corresponding nitrites are obtained. The nitrites of this series are more stable than the corresponding ones of the aliphatic series. 130. The conductivity and viscosity of aqueous solutions of aniline hydrochloride at 25O.” By Nevil Vincent Sidgwick and Bernard Howell Wilsdon. These properties were measured for solutions from N/lO to more than 4N. With increasing concentration the product of conduc-tivity a.nd viscmity first falls, reaching a minimum at about 23,. and then remains nearly constant, with a slight tendency to rise.The product of the conductivity and the two-thirds power of the viscosity falls continuously. 131. “The solubility of aniline in aqueous solutions of its hydro- chloride.” By Nevil Vincent Sidgwick, Percival Pickford, and Bernard Howell Wilsdon. Aniline is miscible in all proportions with water at 168O, and with 4’5N-hydrochloric acid at 30°. The authors have measured the solubility in solutions of various strengths, at temperatures up to complete miscibility. They have also determined at 25O the partition-coefficient (concentration in water /concentration in aniline) of the salt between the two layers. This falls rapidly with increas- ing concentration, being 20 for a .%’,’lo-(aqueous) solution, and 0.9 for a l*SN-solution.The bearing of this on the shape of the solubiiity curves was discussed. Some measurements have also been made of the conductivity and viscosity of solutions of the hydrochloride in mixtures of aniline and water. The results appear to indicate that the conductivity for a given concentration of salt is propoftional to the amount of water in the solvent. 129 132. ‘I Some reducing actions of mercury.” By David Bornr. The action of mercury on solukions of a number of substances has been examined with the following results : (1) Potassium permanganate is reduced to potassium hydroxide and manganese dioxide, the mercury being oxidised to mercuric oxide. (2) Potassium dichromate in neutral solution is not reduced. In the presence of hydrochloric acid, however, chromium chloride and mercurous chloride are formed.(3) Ferric salts in the presence of hydrochloric acid are reduced to the ferrous state. The experiments showed that mercury may be used as reducing agent for ferric compounds in the estimation of iron. (4) Potassium persulphate is reduced to potassium sulphate, the mercury being converted into a basic sulphate. (5) Copper sulphate in the presence of hydrochloric acid is reduced to cuprous chloride. (6) Nitrobenzene in the presence of hydrochloric acid is reduced to aniline to asmall extent. (7) Solutions of potassium nitrate, potassium chlorate, and sodium peroxide are not acted on by mercury to any appreciable extent. 133. Note on the preparation of P-hydrindone.” By Jocelyn Field Thorpe.In a previous paper (Moore and Thorpe, Trans., 1908, 93, 165) a process was described by which o-phenylenediacetonitrile, which is derived from o-xylylene dibromide by the action of potassium cyanide, could be quantitatively transformed into /3-imino-a-cyano- hydrindene by the action of sodium ethoxide, thus : It was also shown that P-imino-a-cyanohydrindene could be converted, through the corresponding carboxylic acid, into P-hydrindone : Since that time it has been found that P-imino-a-cyanohydrindene can be directly converted into P-hydrindone by a much simpler process, and, as the yield by the newer method is 90 per cent. of the theoretical, the preparation of this ketone from o-xylene is now an easy matter.Twenty grams of P-iminea-cyanohydrindene are dissolved in 50 C.C.of cold concentrated sulphuric acid, and the clear solution is kept at the ordinary temperature €or one hour. It is then poured into six times its volume of water, and distilled in a current of steam, a large flask being used for the purpose, as much frothing occurs. P-Hydrindone passes over with the steam, and solidifies in the receiver. The semicarbuzone of P-hyarindone, which does not appear to have been prepared previously, separates as a white precipitate when a solution of semicarbazide hydrochloride in aqueous sodium acetate is added to a solution of the ketone in dilute alcohol. It crystallises from hot absolute alcohol, in which it is only sparingly soluble, as slender needles, which melt and decompose at 218O: 0.1803 gave 0-4209 CO, and 0.0904 H,O.C=63.66; €I=5*57. Cl,H1,0N2 requires C =63.5 ;H =5.8 per cent. Jn the previous paper (loc. cit., p. 174) it was stated that @-hydrindone prepared by this method does not alter on keeping, and it was suggested that the unstable character of this compound when prepared by other methods must be due to the, presence of some impurity. This statement was written after the ketone had been under observatim for three to four months prior tol the publi- catiou of the paper. A specimen of P-hydrindone prepared by this method was found, however, to have been completely transformed into rz brown, viscid resin after having been kept in a well-stoppered bottle for eighteen months.RESEARCH FUND. A meeting of the Research Fund Committee will be held in Juns next. Applicat.iona for grints, to be made on forms which can be obtained from the Assistant Secretary, must be received on, or before, Monday, June 5th, 1911. All persons who received grants in June, 1910, or in June of any previous year, whose accounts have not been declared closed by the Council, are reminded that reports must be in the hands of the Hon. Secretaries not later than Thursday, June 1st. The Council wish to draw special attention to the fact that the income arising from the donation of the Worshipful Company of Goldsmiths is to be more or less especially devoted to the encourage ment of research in inorganic aud met.allurgica1 chemistry.Furthermore, that the income due to the sum accruing from the Perkin .Memorial Fund is to be applied to investigations relating to problems connected with the coal-tar and allied industries. 130 FARADAY LECTURE. The Faraday Lecture will be delivered by Professor Theodore W. Richards, of Harvard University, on Wednesday, June 14th, 1911, at 8 p.m. The Lecture will be given, by the kind permission of the Managers, in the theatre of tbo Royal Institution, 21, Albemarle Street, W. Admission will be by ticket only. Full particulars Will be announced in the next number of the Proceedings.”I‘ ,4t the next Ordinary Scientific Meeting on Thursday, May 18th, 1911, at 8.80 p.m., the following papers will be communicated: ‘‘ Some reactions of w-bromomethylfurfuraldehyde.” By W.F. Cooper and W. H. Nuttall. “The course of chemical change in quinol under the action of radiant energy.” By W. N. Hartley and 0. H. Little. “A method for the accurate volumetric determination of the oxygen in the air.” By H. E. Watson. “ Electrolytic reduction. Part IV. Aromatic aldehydes.” By H. D. Law. “Mannitoboric acid.” By 5. J. Fox and A. J. H. Gauge. The Synthesis of ammonia by heat.” By J. S. Cardell and F. Thomas. R CLAY AND SON$, LlD., HHU>sWILK bT., 5TAYFORD ST., S.E., Ahl> HrhbAY’, SCFIOLK.
ISSN:0369-8718
DOI:10.1039/PL9112700117
出版商:RSC
年代:1911
数据来源: RSC
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