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Issued 1/6/ 1897. PROCEEDINGS OF THE CHEMICAL SOCIETY. EDITED BY THE SECRETARIES, No. 180. Session 1896-2. ____~___ May 20th, 189’7. Professor Dewitr, F.R.S,, President, in the Chair. Messrs. H. E. Gardner, William Barlow and Paul Thomas White were formally admitted Fellows of this Society. Certificates were read for the first time in favour of Messrs. Walter Harry Barlow, 152, Osbaldiston Road, Stoke Newington, N. ; Ernest Stuart Cameron, 5 1, Pembroke Road, Dublin ;Medwin Caspar Clutter- buck, B.Sc., Ph.D., 61, Beaconsfield Villas, Brighton ;Frank William Harbord, Egham ;B. J. Harrington, Ph.D., McGill College, Montreal ; A. G. Kidston Hunter, Princes Street, Dunedin, N.Z.; John Edwin Mackenzie, B.Sc., Ph.D., 7, Ramsay Garden, Edinburgh ; Lionel Walter Kennedy Scargill, B.A., 14, Brunswick Place, W.Brighton ; James Porter Shenton, 34, Lansdowne Road, W. Didsbury, Man- Chester. Of the following papers, those marked * were read :-*60. ‘I The theory of osmotic pressure and the hypothesis of electro-lytic dissociation.” By Holland Crompton. The author applies the results obtained by Guye, Ramsay and Shields, and others in their investigations on the molecular complexity of liquids to the theory of osmotic pressure. It is found that Van’t Hoff’s view, that the osmotic pressure of the dissolved substance is in dilute solution equal to the pressure which the substance would exercise in the same volume if in the gaseous state, is applicable when both the dissolved substance and the solvent form normal or monomolecular liquids.It may also apply if both liquids are associated. But if the 110 dissolved substance is associated and the solvent is monomolecular, the osmotic pressure is then smaller than the theoretical, and becomes inversely proportional to the factor of association x1 of the dissolved substance. If the solvent is associated and the dissolved compound is monomolecular, the osmotic pressure is greater than the theoretical, and is directly proportional to the factor of association xof the solvent. If the solvent has also an abnormal vapour density, the factor of association of the vapour being a, the osmotic pressure is directly pro-portional to x/u. By application of the above conclusions, it is shown that the latent heat of fusion r, melting point on the abso1ut.e scale T, and density at the melting point, d, of a liquid are connected by the expression rd/T=const.in the case of monomolecular liquids, or rdxJTa= const. in the case of associated liquids. The mean value of the constant is 0,099, or roughly 0.1. This formula is exactly similar to the Trouton formula, which connects the latent heat of vaporisation, gaseous density, and boiling point on the absolute scale of liquids. The molecular reduction of the freezing point for monomolecular substances in monomolecular solvents is given by Van’t Hoff’sformula, E =0.01976 T2/r, or by the derived formula E =0.2 Td. If, however, the dissolved substance or the solvent are associated, this formula no longer applies, but E =0.01976 T2x/mxl, or E =O*2Td/x1.Excep-tions to Van’t Hoff’sformula for the molecular reduction of the freezing point appear, therefore, whenever association of either the dissolved substance or the solvent takes place, and it is shown that those excep- tions observed in the case of electrolytes in aqueous solution are in perfect keeping with the view that electrolytes are monomolecular compounds in solution in an associated solvent, e.g., water. The hypothesis of electrolytic dissociation is not only unnecessary in expla- nation of these exceptions, but is inconsistent with what is now known of the molecular character of liquids. A connection is supposed to exist between the specific inductive capacity of a liquid and its power of promoting electrolytic dissociation.The author shows that it is only associated liquids that have high specific inductive capacities, and that the specific inductive capacity is approximately proportional to the cube of the factor of association of a liquid. It is therefore not on the degree of electrolytic dissociation of the dissolved substance, but on the degree of association of the solvent, that the conductivity depends, and the view is taken that electrolytes are salts in the monomolecular fluid state in solution in associated solvents. 111 "61. bb Molecular rotations of optically active aalts." By Holland Crompton. A fact which is usually quoted as strong evidence in favour of the hypothesis of electrolytic dissociation, is that salts which contain a common optically active ion-either positive or negative-exhi bit, in sufficiently dilute aqueous solution, the same equivalent rotatory power.If, however, electrolytes are salts in the monomolecular fluid condition (preceding paper), the observed regularities indicate that monomolecular salts which contain a common optically active radicle have the same equivalent rotation. Those peculiarities which have been observed in the case of the equivalent rotations of optically active electrolytes in aqueous solution, are shown by' the author to be also exhibited by the amylic salts of certain organic acids, when these are examined in the free state and not in solution in any solvent.As electrolytic dissociation is in this case entirely out of the question, the hypothesis becomes an unnecessary one in other instances, and the behaviour of optically active electrolytes is merely in keeping with that of other optically active monomolecular salts. "62. "Heats of neutralisation of acids and bases in dilute aqueous solution." By Holland Crompton. The constancy of the heat of neutralisation of an acid by a base is usually explained in accordance with the electrolytic dissociation hypo- thesis by the assumption that the acid, base, and the resulting salt are all in a dissociated state, and that the only change occurring in the system is the formation of water from its ions. In this paper, the author calls attention to the fact that from Thornsen's Thermoclzernische Untewuchungen, Band IJ?, it may be inferred that the replacement in any monomolecular organic compound RK of the H atom by one and the same radicle M, is attended with a constant heat change, which is independent of the character of R, and that for monomolecular com- pounds the heat of the reaction RH -H +35 is constant if M is constant and indeperdent of variations in R. From this it also follows that the heat of the reaction ROH -OH +M is constant. In the neutralisation of an acid RH by a base MOH, we have the changes M -OH, R -H, M +R, H +OH.If M is kept constant then two terms in the reaction will be constant, M -OH and H +OH. The only variation is then in R -H and M +R. But as shown above, for monomolecular com-pounds RH-H +M is attended with a heat change that is independent of R, and hence if acids and bases in dilute aqueous solution are mono- molecular compounds, the heat of neutralisation of any acid by one and the same base is a constant quantity.It may be shown in similar 112 manner that the heat of neutralisation of any base by one and the same acid is constant, and hence the heats of neutralisation of acids by bases are always the same. The hypothesis of electrolytic dissociation is unnecessary in explanation of the observed phenomena, if it be granted that the dissolved electrolytes are monomolecular compounds. In the above, since OH is simply another negative radicle R, the heat of the reactions M -OH and H + OH might be expected to exactly balance that of the reactions H -R and M +R.This is probably the case when the reactions do not occur in dilute aqueous solution. But in solution while the acid, base, and salt are in a condition com-parable with that of their vapours, the water which is formed in the reaction must be transformed from that state to the liquid state of the solvent by which it is surrounded. This implies that the heat of neu-tralisation of an equivalent of an acid by an equivalent of a base in aqueous solution contains as main factor the heat of condensation of a molecule of water. This latter quality has a value of about 10,800 cal., and the mean value of the heat of neutralisation is 13,500 cal. The difference between the two values is to be mainly attributed to the state of partial association of the base.DISCUSSION. Mr. PICKERINGsaid whether Mr. Crompton had established his views or not, he had succeeded in throwing much new light on the subject under examination, and had given us further evidence that the theory of dissociation was not the only one through which we might look for an explanation of the phenomena of dissolution. By way of criticism, the speaker suggested that the means of recog- nising a liquid to be of the associated or non-associated class at the freezing temperatures was somewhat imperfect, and might, in many cases, lead to erroneous conclusions. He doubted, also, whether the numbers obtained showed that the same solvent indicated consistently the same degree of association when pitted against various mono-molecular solutes, as should be the case, and whether the same associated solute, when pitted against various monomolecular solvents, gave simi- larly consistent results.A stronger objection, however, might be raised in the behaviour of diatomic and triatomic electrolytes in water. According to Mr. Crompton’s views, these should both give values of 55.2 for the depression of the freezing point when in extreme dilution; the triatomic electrolytes do so, but diatomic electrolytes give values which show little or no tendency to surpass 3’7, which is only double instead of three times the ‘normal’ value. As regards the heat of neutralisation, the speaker considered Mr.113 Crompton’s application of a general principle which has been estab- lished in organic transformations to similar transformations in inor- ganic solutions to be both legitimate and ingenious. The simplicity of the principle for organic substances, no doubt, depends on the fact that these substances are nearly saturated compounds, and in dilute solutions of inorganic compounds we are probably also dealing with saturated compounds. Some years ago, the speaker brought before the Society an explanation of the constancy of the heat of neu-tralisation which was based on chemical grounds, without recourse to the theory of dissociation. Residual affinity was the explanation which was offered, and Mr. Crompton’s explanation could be improved by taking residual affinity into consideration.Mr. Crornpton accounts for the heat evolved on neutralisation by the condensation of the molecule of water formed ;this condensation should certainly be recog- nised (a fact which the speaker had overlooked in his own communica- tion on the subject), but the heat evolved by it falls short of that of neutralisation by some 3000 cal., and it seems probable that this excess may be accounted for by the salt formed becoming, in the presence of water, more fully saturated than either the acid or the alkali. Each of these latter contains a radicle, H and OH, which is identical with one of the radicles in water itself, and such compounds would, therefore, probably not have their residual affinity entirely saturated by the water, whereas this is not so with the salt, and there is nothing in its case to prevent complete saturation.Mr. W. C. D. WHETHAMsaid that although it was impossible to criticise such an interesting paper without having considered its details, he would like to ask Mr. Crompton how he would explain the phenomena of electrical conductivity. On the theory that the ions were free from each other, the observed fact that the conductivity of a dilute solution varied as the concentration was at once explained. The alternative supposition, that the ions worked their way through the solution by means of a continual series of interchanges between the opposite parts of molecules at the instants of collision, would lead to a different result, for the frequency with which such collisions would occur, and therefore the ionic velocities, must vary as the square of the concentration, and since the conductivity depended on the product of the number of ions and their average velocity, it would be proportional to the cube of the concentration. Then, again, the fact that the velocity of an ion in dilute solution was independent of the other ion present, not only as calculated from the conductivity, but also as directly observed, seemed to favour the idea of dissociation, and was of greater weight than other additive relations, since it involved the properties of the ions when in motion.The successful calculation of potential differences at the contact of 114 two solutions on the assumption that the faster-travelling ion moved independently of the other, and so diffused more quickly, must also be remembered.Such phenomena as these must be explained before the dissociation theory could be abandoned. No doubt the theory presented many difficulties, and a successful attempt to explain the facts in some other way would be of extreme interest; but at present the evidence in favour of the dissociation theory seemed very strong. Dr. SHIELDS,after referring to the difIiculty of discussing the paper until all the details were before them, stated that he was not satisfied that Mr. Crompton had made out his case that abnormally large osmotic pressures were due to the association of the solvent.According to the well-known equation, the osmotic pressure, x, of a solution containing r/~molecules of dissolved substance in N molecules of solvent is repre- sented thus : n . RZ'l000px=T M where M denotes the molecular weight of the solvent, p the specific gravity of the solution, 2' the absolute temperature, and Ris a constant, viz., 0.0819 litre-atmospheres, when we express the osmotic pressure in atmospheres and the volume of the solution containing 1 g-molecule in litres. In the above equation, the product NM is the weight in grams of the solution containing n g-mols. of the dissolved substances. If me make up a dilute solution to contain, by intention, n, g-mols. of dissolved substance in Ng-mols. of a solvent supposed, in the first instance, to be normal or monomolecular, then we get a certain definite value for the osmotic pressure.If, however, the solvent is associated, and x is a measure of its molecular complexity, then instead of having weighed out Ng-mols. of solvent, we have in reality only N/x, and since the weight of .the solution remains the same, the osmotic pressure must be 92 RTlOOOpx=-. NIX XM or in other words remain uninfluenced by the degree of association of the solvent. As regards aqueous salt solutions, Dr. Shields thought Mr. Crompton would encounter serious difficulties in attempting to explain why dilute solutions of binary compounds, such as potassium chloride, had a maximum osmotic pressure of twice the theoretical value, whilst com-pounds like calcium chloride gave three times the pressure one mould expect.Dr. Shields also called attention to the fact that associated liquids such as water become less associated as the temperature is raised, and asked whether when the particular temperature were reached at which 115 water becomes ‘normal,’ salt solutions also become ‘normal,’ i.e., show the theoretical osmotic pressure corresponding to that temperature and otherwise behave like indifferent substances or non-electrolytes. Mr. CROMPTON,in reply, explained that in assigning to a-particuIar liquid a monomolecular or an associated character the general results of the work of Guye, Ramsay and Shields and others had as far as possible been adhered to. That the molecular reduction of the freezing point of water by electrolytes was in certain cases, even in the most dilute solutions, below the value required for monomolecular compounds, indicated that the salt was originally associated and that the complex molecules only broke down slowly with rising dilution.Similar in- stances could be observed in the case of solutions of associated com-pounds in other solvents, e.g., benzene. Alcohol, which in concentrated solution in benzene gave a molecular weight far higher than the normal, would be found to give correct values in very dilute solution. On the other hand, acetic acid gave even in very dilute solution in benzene a molecular weight of about 110 in place of 60, the splitting up of the associated molecules taking place apparently with greater difficulty in the case of this compound than in that of alcohol.The adequacy of the dissociation hypothesis to explain the electrical properties of salt solutions had not been called in question, but it had been shown that the hypothesis gave no true account of certain other properties of salt solutions which it had hitherto professed to explain. ‘The additive character of the molecular conductivities of dilute salt solutions was merely in keeping with the additive character of nearly all the properties of monomolecular compounds in the fluid condition, as, for example, the molecular volumes, the molecular refractions, the molecular viscosities. If a dissociation hypothesis were adopted to explain additive properties in one case, this would have to be extended to all, and such a thing as a monomolecular fluid compound would be non-existent. *63.(‘A comparative crystallographical study of the normal selenates of potassium, rubidium, and caesium.” By A. E. Tutton. The main conclusions of this investigation, which is analogous to the one formerly presented concerning the corresponding sulphates (Trans, 1894, 65,628), are as follows. 1. The order of solubility bf the three salts follows that of the atomic weights of the three respective metals contained. 2. The values of the morphological angles of the crystals of rubidium selenate are without exception intermediate between those of the analogous angles of the potassium and casium salts. The angles are therefore a function of the atomic weight of the metal present. 116 3.The morphological axial ratios of rubidium selenate are likewise intermediate. 4. The usual habits of the crystals of the three salts exhibit a pro-gressive development of the primary forms, following the progressive change in atomic weight. 5. The directions of cleavage are identical. 6. The relative density and molecular volume increase when a lighter is replaced by a heavier alkali metal. The increase in density is greater when potassium is replaced by rubidium than when the latter is replaced by czesium, and the increase in molecular volume is, on the contrary, greater when rubidium is replaced by cesium. The replacement of sulphur in the sulphates by selenium is accompanied by an increase of molecular volume varying from 6.5 to 6.7 inversely as the weight of the initial molecule. 7.The replacement of potassium by rubidium, and of the latter by cssium, is accompanied in each case by an increase in the separation of the centres of contiguous units of the homogeneous crystal structure, along the directions of each of the morphological axes, the influence of the nature of the alkali inetal becoming relatively greater as the atomic weight rises. An extension of volume in all directions also accompanies the replacement of sulphur by selenium. 8. An increase of refractive index is observed to accompany an in- crease in the atomic weight of the alkali metal, and the increase be- comes relatively greater as the atomic weight rises.The replacement of sulphur by selenium is also accompanied by an increase of refractive index, and such increase diminishes in amount as the weight of the initial molecule increases. 9. If the closed optical ellipsoidal figures, the optical indicatrices, of the three salts were constructed about the same origin, the indicatrix of the cesium salt would contain within it that of the rubidium salt, and this again would contain that of the potassium salt. The indicatrix of the rubidium salt mould lie nearer to that corresponding to the potassium salt. 10. The replacement of one alkali metal by another of higher atomic weight is accompanied by a diminution of the already feeble double refraction. In the convergence of the axial values of the optical indicatrix towards unity the c value proceeds much more rapidly than the others.11. The latter fact causes a reversion of the sign of double refraction from positive to negative on attaining the cesium salt. 12. The optic axial angles are precisely such as would naturally follow from the progressive development of the optical indicatrix ; a change of direction of the acute bisectrix and of the optic axial plane occurs 117 when the caesium salt is reached, as the direct result of tlhe continuity of the progression according to atomic weight. 13. The optical properties of the selenates exhibit marked specific differences from those of the sulphates, owing to the progressively different effect of replacing sulphur by selenium in the three sulphates, but the whole of the relationships of these optical properties exhibited by the three salts of each group are of a precisely parallel nature, being functions in each case of the atomic weight of the alkali metal which they contain.14. Progressive changes occur in the optical properties on raising the temperature, following, even to the least detail, the order of the atomic weights. An interesting direct consequence is that a 60" prism of czesium selenate whose vibration-directions are parallel to b and c affords at 90"C. only one image of the spectrometer slit, the two images usually observed coinciding at this temperature, the crystal being then apparently uniaxial.15. A further consequence of the foregoing is that the crystals of czesium selenate exhibit unique interference phenomena in convergent polarised light when their temperature is raised, including crossed axial plane dispersion, and two reversals of the sign of double refraction. Section-plates perpendicular to all three axes in turn require to be em- ployed in order to follow the optic axial changes even as far as 28OOC. 16. The whole of the molecular optical constants of rubidium selenate are intermediate between those of potassium and czsium selenates. The replacement of sulphur by selenium is acompanied by an increase of molecular refraction of 3.4-3-8 Lorenz or 6-2-6.7 Gladstone units, according to the direction chosen for comparison.The relations of the three salts of each group as regards molecular refraction are identical, but the actual differences are slightly greater in the selenate group than in the sulphate group. 17. The molecular refraction of each of the three selenates for the state of solution in water is approximately the same as the mean of the three values for the crystal. When potassium selenate is dissolved in water, its refraction equivalent rises by 2.8 per cent ; in the case of rubidium sulphate, a less rise of 1.0 per cent. is observed, while for czesium selenate there is no longer a rise but a decrease, to the extent of 0.5 per cent. These slight differences, due to change of state, thus exhibit a progression varying directly as the specific refractive energy and inversely as the atomic weight of the alkali metal contained in the salt.After subjecting Kanonnikoff's value for dissolved potassium sulphate to revision, precisely similar differences €or the two states are shown to exist in the sulphate group, 18. The author finally concludes as regards the selenates that- The whole of the morphologicccl and physical properties of the crystals 118 oj the rhombic normal selenates of potassium, rubidium, ccnd ccesium a9.e functions of the atomic weight of the alkali metal yvesent. 19. It is shown that the joint results of the investigations of the sulphates and selenates agree with the assumption that- The characters of the cvystals of isomorphous series arefunctions of the atomic weight of the interchangeable elenzents, belonging to the same fc6mily group, which give rise to the series.DISCUSSION. Dr. GLADSTONEremarked that everyone recognised in a general way that in groups of analogous elements there is a gradual progression in the properties, the middle member of the group being intermediate, not only in atomic weight, but also in other respects. The value of Mr. Tutton’s elaborate papers, is, that he has proved this up to the hilt quantitatively in the case of two similar, well defined groups of salts, and that with regard to a large number of properties. The change in the specific refraction of the selenates of the alkalis in their crystal- line and their dissolved condition is especially instructive, as it involves the change’ from plus in potassium and rubidium to minus in czsium.The correction of Kanonnikoff’s number for the potassium sulphate which Mr. Tutton has made brings the atomic refraction back to a figure practically identical with that published in Dr. Gladstone’s paper of 1870, viz., 33.11. “64. The platinum-silver alloys ; their solubility in nitric acid.” By John Spiller. Referring to the published statements in the text-books, and particu- larly to those in Percy’s L%i?etcclZzc~~g~and Bloxam’s C‘hernistyy, according to which 5 or even 9 per cent. of platinum followed the silver into solution when their alloys were treated with nitric acid, the author investigated the properties of ten graduated alloys constituted as follows :-Series I, containing 12, 9 and 5 per cent. of platinum ; series 11, containing 2, 1.5, 1 and 0.75 per cent.of platinum ; series 111, con-taining 0.5, 0.4 and 0.25 per cent. of platinum. These alloys were prepared by fusion of the requisite proportions of silver and platinum under a gas-air blow-pipe flame in shallow porcelain cups, and then attacked by nitric acid of three different strengths, when it was found that the ordinary concentrated acid of 1-42 sp. gr., warmed, proved the best solvent, but that even under the most favourable conditions no more than 0.75 to 1-25, mean 1 per cent. of platinum, could be dissolved along with the silver. When diluted nitric acid of 1.2 sp. gr. was employed, the maximum 119 amount of platinum taken up was only about 0.25 per cent.; whilst the highly concentrated acid of 1-50 sp.gr. proved altogether inappro- priate, giving a bulky, insoluble product consisting of platinum black, intermixed with nearly the whole of the silver nitrate formed. It would appear, then, that Berthier’s account, quoted by Percy, and the statement in Bloxam’s Cliemistyy are incorrect. DISCUSSION. Mr. VERNON suggested that the composition of the alloys HARCOURT of platinum and silver might vary with the temperature at which they were formed, and that Mr. Spiller should determine the solubility of alloys formed at higher temperatures than those he had employed. Mr. FRISWELLthought that impurities in the nitric acid might account for some of the discrepant statements on record.65. ‘‘Dalton’s law in solutions. The molecular depression of mix-tures of nonelectrolytes.” By Meyer Wilderman, Ph.D. Since Van’t Hoff has shown that the generalisations arrived at by Boyle and Guy-Lusssc in the cases of gases are equally applicable to dissolved substances in dilute solutions, the conclusion must be drawn that the third gaseous law, the law of Dalton, holds for dilute solutions also, this being a necessary consequence of the nature of osmotic pressure. Following up the thermodynamic considerations of Planck, the equations for mixtures of two or more electrolytes and the ex- perimental proof of them are given. 66. ‘‘The action of bromdiphenylmethane on ethyl sodacetoacetate,” By G. G).Henderson D.Sc., M.A.,and M.A. Parker, B.Sc. While bromtriplienylmethane and ethyl sodacetoacetateinteract to give a disubstituted derivative, (CPh,),: CAc*CO,Et, and ethyl acetoacetate, bromdiphenylmethane, on theother hand,appears to yield only a inonosub- stituted ester, ethyl a-cccetyZ-P-di~~~e.Zp~.opion~te,CHPh,. CHAc* C0,Et. This substance was prepared by heating bromdiphenylmethane (1 mol.) and ethyl sodacetoacetate (1 mol.) in presence of pure dry benzene or xylene till the reaction was completed,filtering from sodium bromide, con- centrating the benzene solution, and purifying the crystals, which then separated, by recrystallisation from alcohol. It crystallises in shining, colourless needles, m. p. 85O, is sparingly soluble in alcohol but readily in benzene, and decomposes almost entirely when distilled.On hydrolysis of this ester with cold dilute aqueous potash, a small quantity of a-ccce5?/1-P-di~~enyZpropioniccccid, CHPh,,CHAc*COOH, was obtained in the form of extremely unstable crystals, which melt 120 about 90' and decompose at a slightly higher temperature. The salts of this acid are also very unstable. /3-diphenyZethyZrnethylketone, CHPh,*CH,. CO-CH,, was prepared by hydrolysing the ester with hot dilute alcoholic potash. It crystallises in colourless prisms which melt at 87.5" and distils with almost no decomposition at 315'. It is fairly readily soluble in alcohol, and very readily in benzene. The oxirne, CHPh,. CH,* C(CH,) :N*OH, forms small, colourless crystals, m.p. 86-87'. It is sparingly soluble in alcohol but readily soluble in ben- zene. The senzicccrbcmow,e,CHPh,-CH,. C(CH,) :N*NH-COONH,, crystal- lises from alcohol in small, white clusters of minute crystals, which melt at 181O. It is sparingly soluble in alcohol and in benzene. ADDITIONS .TO THE LIBRARY. I. By Purchccse. Behrens, H. Anleitung zurMikrochemischen Analyse. Pp. xi +224, mit 92 figuren im text. 8vo. Leipsig 1895. Grandeau, L. Trait6 d'hnalyse des Matihres agricoles. 3rd edition. Tome I. Pp. viii +560. Tome 11. Pp. 6 14. Svo. Paris 1897. Griffen, R. B., and Little, A. D. The Chemistry of Papermaking, Pp. vi+517. New York 1894. Lewin, L. Lehrbuch der Toxikologie, zweite auflage. Pp. x +509.Wien und Leipzig 1897. Prior, Eugen. Chemie und Physiologie des Malzes und des Bieres. Pp. x+ 597. Leipzig, 1896. Stillman, T. B. Engineering Chemistry, a Manual of Quantitative Chemical Analysis. Pp. xxiii +523. Easton, Pa., U.S.A., 1897. Roth, E. ;Heinzerling, C. ; Helbig, Dr. ; Goldschmidt, F. ;Weyl, Th. Hygiene der Chemischen Grossindustrie. Pp. 629-9 10, init 38 abbildungen im text. Jena 1896. (Vol. 8. Pt. 4 of Weyl's Hand- buchs der Hygiene.) Wiley, H. W. Principles and Practise of Agricultural Analysis. Vol. 111. Agricultural Products. Pp. xii + 665. Enston 1897. 11. Donrctions. Clarke, F. W. The Constants of Nature. Part V. A Recalculation of the Atomic Weights. New edition, revised and enlarged. Wash-ington 1897. 8vo. Pp. vi +370.From Smithsonian Miscellaneous Collections, 38. (Number 1075.) Cohen, J. B. The Air of Towns. Washington 1896. 8vo. Pp. 41, 121 21 plates of illustrations. From Smithsonian Miscellaneous Collec- tions, 39. (Number 1073.) Duclaux, E. Atmospheric Actinometry and the Actinic Constitu- tion of the Atmosphere. Washington 1896. 4to. Pp. iii +48. From Smithsonian Contributions to Knowledge, 29. (Number 1034.) Gray, Thomas. Smithsonian Physical Tables. Washington 1896. 8vo. Pp. xxxiv + 301. From Smithsonian Collections, 35. (Number 1038.) Holden, Edward S. Mountain Observatories in America and Europe. Washington 1896. 8vo. Pp. vi + 77. From Smithsonian Miscella- neous Collections, 37. (Number 1035.) McAdie, A. Equipment and Work of an Aero-physical Observatory.Washington 1897. 8vo. Pp, 30. From Smithsonian Miscellaneous Collections, 39. (Number 1077.) Russell, F. A. R. The Atmosphere in Relation to Human Life and Health. Washington 1896. 8vo. Pp. 148. From Smithsonian Mis- cellaneous Collections, 39. (Number 1072.) Varigny, Henry de. Air and Life. Washington 1896. 8vo. Pp. 69. From Smithsonian Miscellaneous Collections, 39. (Number 1071.) From the Smithsonian Institution. Griffiths, A. B. Respiratory Proteids Researches in Biological Chemistry. Pp. viii + 126. London 1897. From the Author. RESEARCH FUND. A meeting of the Research Fund Committee will be held in June. Applications for grants, accompanied by full particulars, should be sent to the Secretaries before June 8th.LIST OF FELLOWS. A new list of Officers and Fellows of the Chemical Society being in course of preparation, it is requested that Fellows will send any altera- tion of address, without delay, to the Assistant Secretary, Burlington House, London, W. At the next meeting, on Thursday, June 3rd, the following Papers will be received. The authors of those marked with an asterisk have announced their intention of being present. * “On the thermal phenomena attending the change of rotatory power of freshly-prepared solutions of certain carbohydrates ; with some remarks on the cause of multirotation.” By Horace T. Brown, F.R.S., and Spencer Pickering, F.R.S. * ‘(On the thermo-chemistry of carbohydrate-hydrolysis : (I.)The hydrolysis of starch by vegetable and animal diastase.(11.)The hydrolysis of cane-sugar by invertase.” By Horace T. Brown, F.R.S., and Spencer Pickering, F.R.S. * I‘ Optical inverson of camphor.” By Frederic Stanley Kipping, Ph.D., D.Sc., and William Jackson Pope. Q (‘Derivatives of camphoric acid. Part 11. Optically inactive derivatives.” By F. Stanley Kipping, Ph.D., D.Sc., and William Jackson Pope. * ‘‘Racemism and Pseudoracemism. F. Stanley Kipping, Ph.D., D.Sc., and William Jackson Pope. * ‘‘ Note on some new gold salts of the Solanaceous alkaloids.” By H. A. D. Jowett, D.Sc. CERTIFICATES OF CANDIDATES FOR ELECTION. N.B.-The names of those who sign from ‘‘General Knowledge ’’ are printed in italics. The following have been proposed for election.A ballot will be held on Thursday, June 17th. Ackroyd, William, 9, Grandsmere Place, Halifax, Yorks. Analyst. Public Analyst and Gas Examiner for Halifax. Fellow of the Institute of Chemistry, &c. Author of “The Old Light and the New ; dealing with the Chemistry of Colour and the New Photo- graphy.” During the last 20 years has published papers on Chemistry and Physics in the Phil. Mag., Chew. AGews, Pyoceedings of the Phys. Soc. Lond., and the Royal SOC.Edin. R. Meldola. Arthur Smithells. Alfred H. Allen. A. G. Green. C. Rawson. G. W. Slatter. Walter Leach. Barlow, Walter Harry, 152, Osbaldeston Road, Stoke Newington, N. Analytical Chemist. Associate of the Institute of Chemistry. Cer-tificated Student of Finsbury Technical College, 1890-95.Fourteen months Assistant Chemist at Gas Light and Coke Co.’s Works, Beckton. At present Assistant to Dr. Attfield, F.R.S. R. Meldola. John Attfield. R. C. T. Evans. J. Theo. Hewitt. Arthur J. Chapman. Brothers, William Malam, Beechwood House, Prestmich, near Manchester. Chemist. Studied Chemistry and Physics for the past six years at Bury Grammar School under Mr. W. French, M.A., F.I.C. For the past two years have been Chemist to Higher Clews Chemical Works, R.awtenstal1. At present studying under Mr. French for the Honours Chemistry of South Kensington and Institute of Chemistry, and 124 desirous of obtaining the Jou~nalfor the current literature of the subject. William French. Edward Haworth.Wm. Hesketh. Christopher Wilson. W. H. Bcwr. Brown, Gerald Noel, 8, The Esplanade, Plymouth, Analytical Chemist and illetallurgist. Associate of the Royal College of Science (Chemistry), 1894. Associate of the Royal School of Mines (Metallurgy), 1895. Chapman Jones. T. E. Thorpe. W. Palmer Wynne. Henry C. Jenkins. Boverton Redwood. W. C. RobertsAusten. William A. Tilden. Cameron, Ernest Stuart, 51, Pembroke Road, Dublin. Demonstrator of Chemistry in the Royal College of Surgeons of Ireland, and Public Analyst for the County of Dublin. Bernard Dyer. James Dewar. Alfred Smetham. Otto Hehner. AlJq*ed Godon Salanzon. Bovwton Redwood. Sydney Steel. J. R H. GiZ6aad. Clutterbuck, Medwin Caspar, 6 1, Beaconsfield Villas, -Brighton.Lecturer on Chemistry to the Municipal School of Science and Art, Brighton. B.Sc. Lond., Ph.D. Strassburg, late Chemical Scholar of Un. Coll., Bristol. Joint Author with Prof. Fittig of an original research on tetrolic acid. Two years manager of Dallan Chemical Works, Burton-on-Trent. For the last three years Lecturer on Chemistry to the Municipal School of Science and Art, Brighton. William Ramsay. G. Harris Morris. Sydney Young. S. F. Dufton. John Shields. Cranfield, William, 5, Second Avenue, Halifax. Teacher of Chemistry. Now and for several years past chief teacher of Chemistry at the Higher Grade Board School, Halifax. Studied at the Westminster Training College under S. Parrish, Esq., F.C.S., and at the Yorkshire College, Leeds.Arthur Smitbells. John &I. Thomson. S. Parrish. J. B. Cohen. Herbert Ingle. Gorness, A. F. Bilderbeck, 848,Alfred Place West, South Kensington. Medical. Late Assistant Pathologist, St. George's Hospital (includ- ing 3athological Chemistry). Passed final examination R.C.P., i.e., the Medical portion of the Conjoint Scheme L.R.C.P., M.R.C.S. Gave demonstration at the International Congress (with Professor Delipine) for the prevention of air pollution with some of the products of combustion of coal. Samuel ICideal. William Henry Walenn. H. E. Roscoe. Frank Scudder. Henry E. Armstrong. Grundey, Frederick Roscoe, 20, Derby Road, Douglas, Isle of 31nn. Science Teacher (Chemistry and Physics). Bachelor of Science (Vict.), Chemistry and Physxs.Student in Owens College, Alan- Chester, for 3 years. Teacher of Chemistry and Physics in the Organised Science School, Douglas, Isle of Man. H. B. Dixon. E. Haworth. A. Harden. TV. H. Perkiii, jun. G. H. Bailey. Halliwell, Edward, Alexandra Crescent, Demsbury. Analytical Chemist and Associate of the Institute of Chemistry. Gained a Scholarship at the Yorkshire College, Leeds, for 3 years, 1891-4, and took full courses in Chemistry, Physics and certain Art Subjects. In 1894 passed the ''Institute of Chemistry " examina-tion for A.I.C., and have since been engaged in general analytical and clmnical work in the laboratory of Mr. T. Fairley, Leeds. Arthur Smithells. J. J. Hummel. Wyndham R.Dunstan. Thomas Fairley. Herbert Ingle. Julius B. Cohen. Sydney Young. B. A. Burrell. Harbord, Frank William, Egham, Surrey. Analytical Chemist. Assoc. R.S. Mines, Fellow of Institute of' Chemistry. For 7 years Chemist to the Staffordshire Steel Co. Two years Chemist and Steel Works Manager to Messrs. Hatton, Sons & Co., Bilston, Staffs. For last 5 years Analytical Chemist to Indian Gorernmcnt, R.I. Engincering College, Cooper's Hill, Staines. Herbert McLeod. Bennett H. Brough. F. E. Mat'thewP. W. R. Hodgkinson. A. H. Churcb. 126 Harman, Harold, Brewers Sugar Co., Greenock. Chemist to Brewers Sugar Co., Greenock. Studied Chemistry at the Royal College of Science, South Kensington. Research Chemist in Mr. Lawrence Briant's Laboratory.Now Chemist to the Brewers Sugar Co., Greenock. Lawrence Briant. Arthur J. Starey. Thos. Stevenson. Cuthbert Vaux. Chapman Jones. Williunz Crookes. Williccm Briggs. Harrington, B. J., Montreal. Professor of Chemistry McGill College, F.R.S.C., F.G.S., Pli.D., &c. Author of a number of original papers in the 17rccn.sccction,s of the Royal Society of Canada, the Brneyican Journcci of Science and others, more especially on the chemistry of rare and new minerals. William A. Tilden. TIV. C. Roberts-Austen. 'v7rilliam Ramsay. TPilliarrz Crookes. J. $1,Glriclstone. Hunter, A. G. Kidston, Colonial Mutual Buildings, Prince's St., Dunedin, N. Zealand. Professor of Chemistry. Studied under the late Prof. Dittmar, Glasgow and West of Scotland Technical College.Author of ('Ex-amination of a Potable Water from LZ Ijacteriological and Chemical point of view " (Paper read at Intercolonial Medical Congress, Dunedin, 1896). At present Professor of Chemistry in, and Principal of, Otago College of Pharmacy, Dunedin, New Zealand. Public analyst, &c. James XI. Mason. John McArthur. G. G. Henderson. A. Humboldt Sexton. Jccnzes Robson. Matthew A. Piwkey. Johnston, George Lawson, Kingswood, Xydenham Hill. Director Ijovril Limited. Attended Course Organic Chemistry Lectures,-Royal College of Science, Kensington. Three years' analytical work under H. R. Gregory, F.I.C., and in private laboratory (analysis of foods particularly). Member of Chemical Industrial Society.Playf air. A. Searl. Wm. Harkness. S. Arch. Vasey. Jccmes Dewnr. R.Bannistey. J.Woodwa9*cl. c. f?'OCtOT. Mackeneie, John Edwin, 7, Ramsay Garden, Edinburgh. Ph. D. (Strassburg), B.Sc. (Edin.) Assistant Professor of Chemistry, Heriot-Watt College, Edin. (‘Diwiethoxydiphenylmethane and some of its Homologues.” Chem. Xoc. J.; 1896, 987. ap-und &Penten- saure,” Liebig’s Anncdern der Chem., 283,82. With A. G. Perkin, “ Action of Nitric Acid upon Anthracene,” Chem. Xoc. J., 1892, 865. With W. H. Perkin, jun., Ph.D., “Synthesis of Hexahydroterephthalic Acid,” Chem. Xoc. J., 1892, 172. With F. S. Kipping, Ph.D., D.Sc., 4‘ Ethyl-aa’-Dimethyl-aa’-diacetylpimelateand some of its Decomposition Products,” C‘hem.Soc.J., 1891, 569. Alex. Crum Brown. J. Gibson. ’CV. H. Perkin, jr. A. G. Perkin. F. Stanley Kipping. Pollock,William Robertson, Kirkland, Bonhill, Dumbnrtonshire. Assistant Manager in Turkey Red Dye-Work. Three years a chemical student in the Glasgom Technical College under Profs. Dittmar, Henderson, and Mills; engaged in a calico print works for 18 years; for two years and at present on the staff of llessrs. Archibald Orr Ewing & Go., Dillichip; Bronze and Silver Medallist of the City and Guilds of London Institute. Edmund J. &Tills. G. G. Henderson. A. Humboldt Sexton. R. R. Tatlock. 57 L. Pattewon. Scargill,Lionel Walter Kennedy, 14, Brunswick Place, West Brighton. Schoolmaster. Honours in the Final School of Natural Science, Oxford.For the past year Science Teacher in the Langport Grammar School. John Conroy. D. H. Nagel. P. Elford. Tp. JJ? Pk7~er. V,H. Yeleg. Shenton, James Porter, 34, Lansdowne Road, West Didsbury, Jfanchester. Analytical Chemist. A pupil of Mesers. Crace Calvert and Thomson, Royal Institution Chemical Laboratory, Manchester, from 1887 to 1890. Junior Assistant in the same laboratory from 1890 to June, 128 1894. Senior Sssistant in the same laboratory from June, 1894, up to the present time. William Thonison. J. Carter Bell. C. Estcourt. P. Anderson Estcourt. Alfred H. Allen. Chades E. Cassd. Otto Hehze~. I’honaccs Faidey. Taverner, William, 1, Stapenhill Road, Burton-on-Trent, Brewers’ Chemist, in the employ of 1Slessrs. Worthington & Coo: Burton-on-Trent.I have for three years held the position of Chief Chemist to the above-mentioned firm, having previously worked for five years as Assistant Analyst in the Inland Revenue Laboratory, Somerset House. I received my chemical training first at the Uni- versity College, Dundee, and afterwards at the Royal School of n%ines, South Kensington, and the Somerset House Laboratory. R. Bannister. H. J. Helm E. Grant’HoOi3er. C. Proctor. J. Wooclwa1-11. J. H. Robbins. RICHARD CLAY AND SONS, LIMITED, LONDON AND BUNCAY.

ISSN:0369-8718    

DOI:10.1039/PL8971300109

出版商:RSC    

年代:1897

数据来源: RSC