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Proceedings of the Chemical Society, Vol. 9, No. 127 |
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Proceedings of the Chemical Society, London,
Volume 9,
Issue 127,
1893,
Page 171-197
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Issued 19/8/1893. PROCEEDINGS OF THE CHEMICAL SOCIETY. No. 127. Session 1893-94. June 15th, 1893. Dr. Armstrong, President, in the Chair. Mr. T. H. Easterfield was formally admitted a Fellow of the Society. Certificates were read for the first time in favour of Messrs. Henry Ornisby Hale, B.A., Oundle School, Northamptonshire ; Thomas Heilhy Rawlins, 2, Leven Street, Pollockshields, Glasgow ; Herbert Sant,er, Albion Brewery, Caledonian Road, N. ; William Gilcbrist White, Lamb Roe, Whalley, Lancashire ; Edward Humphreys Winder, 37, Vincent Square, S.W. The following were duly elected Fellows of the Societ,y :-John Bateman, Henry Bailey, Douglas T. C. Berridge, Robert S. Cahill, John Henry Coste, S. W. &I.Davy, Arthur Henry Green, Ernest Albert Hancock, James John Howitt, John Walter Leather, Alexander Mitchell Martin, Charles Mills, Charles Alexander McKerrow, I(.P.McElroy, John Wat'son Napier, William Ridgely Orndorff, Alexander Orr, George Ritchie, Wilfred Sessions, Henry Thomas Sorrell, Frank Ernest Thompson, Claude Theodore Vautin, Edward Augustus Warmiagton, Thomas Whittaker, Sydney Wbally. Of the following papers those marked * were read :-"33. " Contributions to our knowledge of the aconite alkaloids. Part VI. Conversion of aconitine into isaconitine." By Wynd-ham R. Dunstan, M.A., F.R.S., and Francis H.Carr. In a previous communication it has been shown that the roots of Aconitunt Nupellus contain, besides the highly poisc;iious aconitine, an almost non-poisonous isomeride-isaconitinc.These alkaloids are 172 evidently intimately related, as both furnish aconine and benzoic acid on hydrolysis. The authors now show that when an aqueous solution of aconitine hydrobromide (m. p. 163") is heated, change very gradually takes place, the isomeric isaconitine hydrobrowaidp (m. p. 282') being produced. The change is facilitated by the addi- tion of a small quantity (1-2 per cent.) of hydrogen brotnide, biit is not assisted if sufficient is present to induce hydrolysis of a large proportion of aconitine. The isaconitine was identified not only by the high melting point of its Palts, but also by the formation and analysis OE the characteristic aachlorisaconitine. No similar change could be detected in the case of aconitine nitrate, either when neutral or acid solution was nsed, nor could the conversion be effected by heating nconitine with glacial acetic acid, although in this case anhydraconitine is produced if the heating be continued during 18 hours at 120".Aconitine may be dissolved in concentrated sulphuric acid, and the solution gently heated without the conversion into isaconitine taking place ; nor does aconitine sulphate undergo conversion into the isomeride when it is heated many hours in con-t:tct with very dilute sulphuric acid. No isaconitine seems to be produced diiring the hydrolysis of aconitine by cold soda solution. The authors are making further experiments in the hope of gaining information with regard to the mechanism of the conversion of acon- itine hydrobromide into isacoiiitine hydrobromide.*34. '' Contributions to our knowledge of the aconite alkaloids. Part VII. Some modifications of aconitine aurichloride." ByWyndham R. Dunstan, M.A.,F.R.S.,and H. A. D. Jowett. Certain irregularities having been observed in t'he melting point of sconitine aurichloride, C33H45N012,HAuC14 (see Part I)prepared under different conditions from pure aconitine, the subject was fully investi- gahd, the result being that three distinct isomeric modifications have been isolated differing in melting point and crystalline form. When auric chloride is added to a solution of aconitine hydrochlor- ide, a yellow, amorphous precipitate is thrown down from which tlirectly or indirectly the three crystalline modifications cam be oh- t,;Lined by employing different solvents. Aconitirce a-azcrichloride is niost readily produced in rosettes of needles by crystallisation from a mixture of acetone and water, or less readily and certainly in rect- :iiigular plates from dilute alcohol.The crystals melt at 135.5". When recrystallised from strong alcohol, this compound changes into the p-modification. AconitirLe /3-aiirichlow2e is obtained by crystnllising from strong alcohol. It forms rosettes of needle-shaped crystals which melt at 173 152". When this substarice is recryshllised from a mixture of chloroform and ether it changes into the ymodification, and when recrystdlised from a mixture of acetone and water it appears as the a-modificatioii. Aconitine y-aurichloride cannot apparently bo formed directly from the amorphous precipitate or from the a-aurichloride.It is, however, easily prepared by recrystallising the P-aurichloride from a mixture of chloroform and ether, when it separates in prisms melting at 176". When crystallised from strong alcohol, this substance is converted into needles of the B-aurichloride; and on crystallising it from a mixture of acetone and water, the a-modi6cation is obtained. When the p-and y-modifications are melted they pass into the a-aurichloride. From each of the modifications one and the same crystalline aconitine (.me p. 188-189") may be recovered. They behave, then, as true " physical " isomerides, no chemical difference being detectable be- tween them."35. "Note on the stereoisomerism of nitrogen compounds." By S. U. */ Pickering. Hantzsch and Werner's suggestion that the isomerism of some triad nitrogen compounds may be explained by referring them to a tetrahedron and assuming that the nitrogen occupies one corner in- stead of the centre is tantamount to representing one side only of the nitrogen atom as capable of entering into combination. It leads to further difficulties when the nitrogen becomes pentad, as, in order to preserve the tetrahedral form, the nitrogen atom has to be placed in the centre of the tetrahedron together with one of the monad atoms. An alternative explanation which has been offered is based on the supposition that the isomerides are produced according as one of the bonds of the nitrogen atoms inclines towards one or other of the groups in its vicinity, an explanation for which the study of compounds of other elements affords no justification.In suggesting an arrange- ment of atoms in space, our ignorance of the matter renders the simplest possible arrangement the only justifiable one. This, in the case of an atom combining with three or five others, is that three of these should be arranged in one plane at equal distances around the central atom, the other two being placed in a plane at right angles, sir that each of them is equidistant from the first three. This arrangement, though not symmetrical, is the most nearly symmetrical one possible.It affords, in the author's opinion, a perfect explanation of the stable 1:haracter of ammonia derivatives, and of the fact that in ammonium derivatives two of the groups can be very easily split off. It explains the isomerism found in the hydroximes and hydrazones by one of the 174 groups present being united by different bonds in the two cases (two of the five bonds being always free), just as in the isomerism of carbon compounds, and it agrees vie11 with the facts as to isomerism and opticd activity observed in the case of ammonium derivatives. Masover, as the nitrogen atom can form a, symmetrical compound with any two, as well HS with three, of its bonds occupied, it also affords an explanation of the existence of nitric oxide and peroxide.'36. "A study of the properties of some strong soluticns." ByS. U. Pickering. The depressions of the freezing points of the three solvents watey, acetic acid and benzene by a number of non-electrolytes (methyl, ethyl and propyl alcohols, diethylamine, pyridine, ethyl ether, carbon bi- sulphide, acetic anhydride) were examined, the determinations being extended to the strongest solutions possible. The results showed that the slight irregularities which are observable in the results aforded by weak solutions become one of the most marked features in the case of sfronB solutions, and any theory which attempts to explain the nature of solutions while ignoring the existence of these irregularities must necea~arilybe imperfect.The nature of the dissolved substance has an obvious effect on the character of the results, but it is impossible to ascribe this character to the nature of the dissolved substance only, as the peculiarities exhibited by a pai*t,icular substance in one solvent are often absent when another solvent is used ; these peculiarities would appear to be explicable only on the assumption that every solution contains substances peculiar to itself-Le., compounds of the solvent and substance-and does not consist merely of the juxtaposed free solvent and free substance. Jn the various series, 29 breaks were observed in the regions em- bracing fairly simple molecular proportions (1:4 to 4 : 1 mols.), and of these, 24 agree within experimental error with molecular proportions, the remaining 5being breaks whose existence or position was doubtful.Additional evidence is thus afforded as to the existlence and signi- ficance of these breaks, and their occurrence is shown not to be confined to cases in which the solvent is water. "37. "Studies on citrazinic acid." By W. J. Sell and T. H. Easterfield. A new method of preparing citrazinamide is described, which con- sists in fusing a mixture of citric acid and urea. The alkali salts of the nmide and the normal and acid alkali salts of the acid are de- scribed, and an account is given oE trichlorcitrazinic acid and its behaviour with phenylhydraxine. The authors find that the production of a blue colour when citrazinic 175 acid is warmed with dilnte solutions of potassium nitrite is due to the formation of a quinhydroketopyridine, a substance whose alkaline solution has an intense blue colour; this, however, is only the final stage of a series in which isonitrosocitrazinic acid is first formed.The isonitroso-compound is very uustable ; it is oxidised by nit& or nitrous acid and converted into a stable, yellow acid of the formula CsHzNz05*4Hz0; hence, if an excess of nitrite be employed in apply- ing the colour test for citrazinic acid, no blue colour results. The yellow acid is dibasic, and its solutions precipitate potassium or am-monium salts from solutions of the chlorides of those metals. By the action of dilute sulphuric acid or of reducing agents, iso- nitrosocitrazinic acid is converted into ap'-quinhydro- and a-keto- pyridine, which crystallises in lustrous, bronze-green coloured prisms.The same substance may be produced by reducing the yellow acid. The quinhydrone is easily converted by oxidation into the correspond- ing quinone, which resembles ordinarj quiiione in many of its pro-perties, arid may be reconverted by sulphurous acid and other reducing agents to the quinhjdrone. On reduction the quinhydrone gives a colourless solution which probably contains the quinol, as, OIL ex-posure to air, the liquid begins at once to deposit crystals of the quin- hydrone ; the qninol has not yet been isolated. A bright red coloured phenjlhydrazwitrazinic acid, corresponding to the above isonitroso-derivative, is obtained by the action of diazo-benzene chloride on citrazinic acid ; this substance forms character-istic salts.The following formuke are provisionally suggested for the substances described :-f:0,H ?O,H F02H C C C /\Hy YHZ, /\H? ?:NOH, -O*y /\?:NOH , H0.C CO H0.C CO -c co \/N \/N \/N Citrazinic acid. Isonitrosocitrazinic acid. Yellow acid, $ mol. CHCH CH Y\HY YO oc\./co 7 \#' N Quinhydroke topyridine. Quinoketopyridine. Phenplhydrazocitraz inic acid. 176 O,H C Cl?/\-/\yc1, -(717 y:N*NH*C,H,. H0.C CO H0.C CO \/ \/N N Trichlorcitrazinic acid. Chlorpbeny111ydmzociti.azinicacid (as salts). Discr; ss~o~. Dr. RIPPINGsaid the published statements regarding citrazinic acid agree in assigning to it the property of fluorescence, which, according to Dr.Armstrong’s views on the origin and nature of colour, it should not possess, assuming it to have the usually accepted constitution. At Dr. Armstrong’s suggestion, Mr. 0. F. Russell and himself under- took to settle, if possible, this question of fluorescence, and for this purpose they prepared citrazinic acid by two methods, of which that described by Behrmann and Hofmann was found to give the better results, the acid obtained by Ruhemann’s process from ethylic acetyl- citrate being difficult to purify, A freshly prepared alkaline solution of the crude product is highly fluQrescent, but when the acid is carefully purified by converting it into the ethylic salt and crystallisirig the latter from acetic acid, this is no longer the case.A small quantity of pure citrazinic acid dis- solved in concentrated soda gives a colourless solution without visible fluorescence; on shaking for a few minutes in contact with air a slight but gradually increasing blue fluorescence is observed, caused doubtless by the presence of some oxidation or decomposition product of the acid. A solution containing pure ethylic citrazinate together with sodium carbonate becomes fluorescent on exposnre to the air, but apparently more slowly than a solution of the acid. Some further experiments were made with citrazinic acid with the object of elucidating its constitution. Ethylic citrazinate gave with acetic anhydride a colourless, crptalline diacetyl derivative, CI2H1?NOa, the composition of which was determined by the ordinary methods and by direct estimation of the quantity of acetic acid produced on decomposition with sulphuric acid.Ahtempts to prepare a hydritzone and a hydroxime from citrazinic acid were unsuccessful. By SUR-pending citzazinic acid in wa?er and passing nitrous fumes into the ice-cold mixture, a substance of the composition CsHsNzOs.which is evidently identical with the authors’ isonitrosocitrazinic acid, was obtained ; this compound can be obtained in almost colourless crystals by recrystallisation from ethylic acetate and petroleum. The action 177 of potash and methyl iodide on citrazinic acid seems to be quite abnormal, but the nature of the product, which was of an uninviting character, was not determined.Citraziuic acid combines with dry bromine, yielding a crystalline substance which is readily soluble in water and ethylic acetate ;it is, however, unstable, and loses hydrogen bromide very readily, being converted into a yellowish powder which is practically insoluble in ethjlic acetate. "38; " The essential oil of hops. Preliminary notice." By Alfred C. Chapman. About 80 kilos. of hops, some of which had been grown in Burgundy, some in Alsnce, and the remainder in Kent and Sussex, were sub-mitked to steam distillation in quantities of about 1 kilo. at a time. When the greater part of the oil had been prepared the author was compelled, owing to pressure of other work, to discontinue its examination, and it was placed aside in a well-stoppered bottle, which it filled; at the end of about 10 or 11 months, the remainder of the oil (about 30 c.c.) vas prepared, and the whole was then twice steam distilled to free it, from resin ; about 140 C.C.were obtained. On sub-mitting the oil to distillation it commenced to boil at 17U", the thermometer rapidly rising to 230°, the greater part distilling over between 230" and 270". After several fractionations, finally ovei* sodium, about,40 C.C. of oil were obtained, boiling between 256"and 261" (uncorr.). This was found, on examination, to be a sesquiterpene, three combustions giving numbers closely agreeing with those required by the formula CI5H2(.Two vapour density determinations by Uofmann's method gave 6.91 and 7.1, the vapour density required by C15H2,being 7.1. The boiling point of the sesquiterpene corrected for the emergent mer- curial column was 261-265". Its relative density was found to be 0.8987 at 15";15", and 0 8955 at 20"/20"; when examined in a tube 100 mm. long at 20", it produced a rotasion of 1" 5' to the right, corresponding to a specific rotatory power of +1.2". Its index of refraction for the red hydrogen line, hHa was 1.4978, corresponding to a specific refractive energy of 0.555. Another freshly distilled sample of hop oil which was examined soon after its preparation was found to boil at much lower tempera- tures, and consisted of lower boiling point terpenes, together with ail oxygenated constituent, and contained but little of tmhe sesquiterpene.Itl is proposed both to continue the study of the sesquiterpene and tu examine in detail the other constituents of oil of hops, in the hope oc' gaining some insight into the nature of the changes which occur during the ageing of the essential oil. 178 "39. " The sulphides and polysulphides of ammonium." ByW.P. Bloxam. After calling attention to the uncertain state of our knowledge of the changes which solutions of ammonia saturated with hydrogen sulphide undergo when oxidised by exposure to the air, the author describes qualitative experiments from which he infers that in addi- tion to polysulphide such solutions contain t hiosulphnte, but never more than traces of sulphite, and that no sulphate is produced. These conclusions are based on the application of the method of test- ing recommended by Fresenius (QuaE.Anal., Eng. trans. of 15th German ed., p. 193), using cadmium chloride in place of zinc chloride fO remove sulphides, as this proved to be a more effective agent, but adding the latter salt as its presence was found to be essential to the production of the coloration characteristic of sulphite. It is pointed out that the presence o€ excess of ammonia enhances the delicacy of the test for sulphite. In order to follow with success the changes undergone by solutions of " ammonium sulphide " on oxidation, the author has endeavoured to prepared the various sulphides and polysulphides in a pure state, and describes the results of a large number of experiments.I11 analgsing the solutions of ammonium sulphides, the total sdphur was determined after oxidation by alkaline hypobromite ; to determine the polysulphide sulphur, the solutions were boiled with excess of chlorhydric acid to expel sulphuretted hydrogen, and the residual sulphur was then oxidised by hypobromite, &c. ; ammonia was esti- mated by boiling with excess of stnndardised chlorhydric acid, am1 then determining the amount of acid in excess. A concentrated solution of ammonia (d = 0.880) does not absorb the amount of hydrogen sulphide required to convert the whole of the ammonia into sulphydride, NH4*SH,a, solution saturated at air temperature taking up only about 75 per cent.of that amount, and having a composition which may be represented by the formula. (NH&S*BNH,-SH. Less concentrated solutions of ammonia absorb a larger proportion of hydrogen sulphide, a mixture of 1 volume of ammonia solution (0.880) with 4volumes ol water taking up sufficient to form a, solution of the composition corresponding with the formula NH4SH,the strongest solution of this substance which is obtainable containing only about 16 per cent. The author infers, however, from t,he results obtained on passing hydrogen sulphide into various mix-t u-res of water and ammonia solution cooled with ice water, that the Rolutions do not progressively take up more hydrogen sulphide as they become weaker, but that the amount absorbed is constant within certain well-defined limits, viz.:- 179 Ammonia sol. : Water. Composition of sol. 3 :1 (NHa)ZS,4NH,*SH 2 :1 ( NH,), S,8NH4*SH 1 :1 (NH4)zS,tlNH**SH 1 :2 (NH,jzS,18NH,*SK 1 :3 (NHJ)zS,18NH,.SH 1 :4 NH,.SH The author attributes this remarkable behaviour to the zctual formation of double snlphides, and states that he has obtained several such in crystals. Thus, by cooling, the solution having a composition corresponding with the formula (NH4)2S.SNH4*SH,crystals of this composition were obtained ; whereas a concentrated solution of am-monia, saturated at air temperature with hydrogen sulphide, then cooled to 0" and further saturated with the gas, gave highly hydrated crystals of the formula (NH4)zS*12NH4*SH; and a concentrated solution of ammonia, cooled to 0" and then saturated with hydrogen sulphide, gave well-defined crystals, the composition of which is repre-sented by the formula (NH,j,S-18NHt-SH.What appears to be ammonium sulphydride, NH4*SH,may be ob- tained in the solid state by passing the two gases into a vessel sur-rounded with ice, the hydrogen sulphide being maintained in slight excess ; compounds of the type (NH4)2S*zNHt*8Hare also formed if' the ammonia be in excess, By exercising great care in adjusting the volumes of the two gases and the rate of flow, operating at 18",ruicaceous crystals are obtained, which, when rapidly dissolved in ice-cold water, yield a solution the composition of which sufficiently approximates to that required bj- the fbrmula (NH,),S to justify the concluvion that they consist of this compound; but if a large excess of ammonia passes through the bottle, a more volatile sulphide is obtained in the form of an oil, which appears to be a compound of the formula (NH4),S*BNH,.When an alcoholic solution of ammonia is saturated with hydrogen sulphide, crystalline compounds of the formula (NH4),S*zNH4*SH, containing alcohol of crystallisation, are obtained, the value of x depending on the concentration, as in the case of aqueous solutions. The formation of definite polysulphides appears to be ahtended with considerable difficulty ; " ammonium sulphide " solutions dissolve, at most, the amount of sulphur required to form a polysulphide of the formula (NHJ8S9,and the author is inclined to regard the simpler polysulp hides as secondary products resulting from the decomposition of this compound or of analogous lower compounds.180 40. (ISarcolactic acid obtained by fermentation of inactive lactic acid.” By Percy Frankland, F.R.S., and J. MacGregor, M.A. The authors have submitted ordinary inactive calcium lactate to partial fermentation, and have recovered from the fermented liquid a lactic acid yielding lanorotatory salts, which was separated from the inactive acid still present by repeated crystwllisation of the zinc salts, the zinc salt of the inactive acid being less soluble than that of the active acid. The specific rotatory power of the active zinc salt was determined in several specimens and for several different concentrations, ant 1 results were obtained showing that the rotation on the whole dimin- ishes as the concentration increases and agrees fairly closely witli those given by Wislicenus (Annalen, 167, 332).The identity of the two salts was further established by converting some of the zinc into the calcium salt and determining the specific: rotatory power of the latter; the value found (C = 5.79) was [aJD= -548, that given by Widicenus (C = 5.35) being [a], = -5.25. The authors hope to render this method availabie for the prepara- tion of considerable quantities of sarcolactic acid, in the same way as has already been done by one of them in the case of active glyceric: acid.In the meantime, it is of interest to uote that, as in the case of the fermentation of calcium glycerate, the bacteria attacked by prefereuce the dextrorotatory salt. Similarly, Linossier (Ber., 24, 660) has shown that Penicilliuin g2nuc;um also first destroys the dextrorotatory lactate. 41. “Hexanitroxanilide.” By A. G. Perkin. It is shown that whereas di- and tetra-nitroxanilide are converted by ammonia into the corresponding nitraniline (cf. C.S.Trans., 1892, 4158),hexariitroxanilide not only yie,ds trinitraniline, but also trinitro- phenoxamide, C,H,(NO,),*NH*CO*CONH,, R substance which crps- tallises trom nitrobenzene in colourless, glistening needles melting at 257”; this compound exhibits acid properties, forming potassiuni, sodium and ammonium derivatives, e.g., C,H2(N02)3*Ntl.CZ03NH2, which crystallises in red leaflets exhibiting a magnificent goldeu lustre.When subjected to the action of a cold mixture of nitric and sulphuric acids, trinitrophenoxamide loses the elements of a molecule of ammonia, forming trinitrdxanil. Hexanitroxanilide is converted into 1 : 3 : 5-trinitrobenzene by heat,ing it with a mixture of nitric atid sulphuric acids ; tetraniti-oxalorthotoluidine in like manner yields 1: 3 : 5-dinitrotoluene, but the isomeric par&-derivative is converted into dinitrobenzoic acid. Hexanitrocarbanilide hits also been prepared by the author ; like 181 the corresponding nitroxanilide, it yields red potassium and sodium derivatives.42. “The constituents of the Indian dye-stuff kamda, (I).” ByA. G. Perkin. A description is given of six distinct substances extracted by ether from Kamala-rottlerin, the principal constituent, described by Anderson, in 1855 (Journ. Chem. Soc., 1855, 669) ; isorottlerin; two resins, one of low, the other of high melting point ; a wax, which is possibly cetylic cerotate ; and a yellow, crystalline colouring matter present in a minute proportion, the composition of which is yet to be determined. Bottlerin is best separated from the dye-stuff by means of cold carbon bisulphide, from which it crystallises in thin salmon-coloured plates melting at 191”; its composition is represented by the em-pirical formula CllH1003 already assigned to it by Anderson, but it is undoubtedly a substance of high molecnlar weight.It yields a diacetyl derivative. On boiling it with alkalis, an odour of benzaldehyde is apparent. When oxidised by cold nitric acid, it yields two acids represented by the formula c11H14Og and c~H~09, while boiling nitric acid converts it into a dibasic acid of the formula C13HKJOW Isorottlerin closely resembles rottlerin in appearance, but melts at 198-199” and is practically insolnble even in hot carbon bisulphide ; moreover, no odour of benzaldehyde is apparent when it is boiled with alkali. It yields the acid of the formula C,H,,O9 on oxidation. The resin of low melting point resembles rottlerin, with which it is evidently closely allied in most of its properties ; its composition is represented by the formula CI2H12O3 ; on oxidation, it yields the acid of the formula c13H10og.The resin of high melting point is a light-yellow coloured sub-stance represented by the formula CI3Hl2O4,and also resembles rottlerin in many of its properties, being converted into the acid of the formula Cl3Hl0O,when boiled with nitric acid. 43. “A quantitative method of separating iodine from chlorine and bromine By D. S. Macnair, Ph.D., B.Sc. The method is based on the fact that when treated with potassiuni bichromate and concentrat.ed sulp hhuric wid, silver iodide is com- pletely converted into silver iodate, whereas silver chloride and lmoruide are converted into sulphate. Two portions of a sollition containing the three halogens are precipitated with bilver nitrate : the one precipitate is weighed, the other is heated with the oxidking 182 mixture and the resulting iodate is then reduced by means of sulph-urous acid and the iodide is fillered off and weighed.The silver oi~iginally present as chloride and bromide contained in the filtrate from the iodide is precipitated and weighed as chloride. The method affords very accurate results. Addendum.-Since the paper was written, at the suggestion of Dr. Armstrong, I have used a Gooch crucible asbestos filter, instead of paper, and have found it advantageous both as regards speed and accnracy, as it is not necessary to use two portions ot the liquid when the chlorine and bromine are to be determined ; the precipitate of the mixed haloids may be dried at 120”, weighed, and then treated with sulphuric acid and potassium bichroniate as usual, along with the asbestos previously used in filtering.When the oxidat’ion is finished, the solution is diluted and sulphurous acid is added at once, withotLC previously filtering off the asbestos, which is collected along with the silver iodide. The weight of the asbestos used in the first filtration is necessarily deducted from that of tohe silver iodide. It is evident that this asbestos might be removed by filtering before adding sulphurous acid, but 1do not recommend this, a ssilver iodate is apt to separate out during the filtration, and unless this be completely re-dissolved-no easy matter-before the addition of sulphurous acid, it will escape reduction arid ths results will be unreliable.44. “Note on a form of burette for rapid titration.” By Llewellyn Garbutt, Assistant Masttr at WinchestLr College. The following arrangement will be found extremely convenient in volumetric operations with liquids. The liquid to be used in titrating is contained in the flask E, which may have a capacity ot 300 c.c., and is delivered from a pinch-cock or stop-cock C, at the bottom of t,he long siphon tube 1’. The tube D is connected by means of rubber tube to the gas burette G. The side tabe l3 is closed by a pinch-cock, and the graduation of G begins from the bottom. The pressure tube H, which contains water, moves freely upwards, but its downward movement is arrested by the cork A, fixed stiffly to the upper end of the tube H, and normally serving as a support to it.Before beginning the titration the pinch-cock B is opened for a moment to equalise the pressure. The quantity of water in the two tubes is adjusted once for all, so that whenever the pressure is equalised the water in G falls to zero on the scale. The titration is conducted from the cock C in the usual way, and the amount delivered is read by raising H until the liquids are at the same level in bcth tubes. The parallel lines drawn across the supporting board serve as a guide to the eye. The volume of the liquid delivered can then be read off from the 183 position of the water in G. To begin a new titration, all that is necessary is to let H slide back to its normil position, and open the pinch-cock ah B for a momeiit ; the water in G at once falls accurately to zero, and the new titration can be begun.If it is desired to use several different liquids, as many flasks, furnished with siphon and r connecting tubes, should be prepared and mounted ready on stands. They can then be connected in it moment with the rubber tube E. The advantages of this arrangement are- 1. Bxtreme rapidity and simplicity of adjustment to zero. 2. As much as 300 C.C. of the liquid may be available for a series of tit1.a tions. 3. The same burette is used with all liquids, and always starting from zero, so the graduation is constant. 4.If the burette and pressure tube are thoroughly clean, there is little trouble from tears or imperfect meniscus, as only pure water is used in it.The disadvantages are- 1. The titration must be conducted fairly rapidly (my within 5or 10 minutes), otherwise changes of temperature and pressure may appreciably affect the volume of the air. 2. The pressure cannot be perfectly equalised by means of the sliding tube H. The error of reading from this cause is practically id when F is full, but it might, a9 an extreme, amount to -zlvC.C. when F contains 300 C.C. of air. If it is only desired to to read to c.c., this will not matter much. Forr greater accuracy the flask must always be kept nearly full. It is convenient to be able to detach H completely from the board.Tf the water should get out of adjustment, so that it no ionger falls to zero on opening the pinch-cock at B. either a few drops of water may be added or the cork A moved a trifle along the tube H. 45. “The use of sodium peroxide as an analytical agent.” ByJ. Clark, Ph.D. Experiments are described showing that the sulphur rtnd arsenic in minerals may be rendered soluble by cautiously heating the powdered substank with sodium peroxide, aitd that the peroxide may, in like manner, be used in estimating chroniium in chrome ores and chromium alloys. An ammoniacal solu+ion of the peroxide may be used in separating manganese from zinc, nickel and cobalt, a single precipitation sufficing in the case of zinc. 46. “Stibiotantalite: a new mineral.” By G.A. Goyder. The note has reference to a mineral from the alluvial tin-field at Greenbushes, Western Australia, the assay values of which varied most unaccountably. It is shown to consist, in the main, of antimony and tantalum oxides ar,d a not inconsiderable proportion of niobic oxide ; the amounts found in one sample, for example, were Tn,O, = 51-13, Nb,05 = 7-56, Sb,O, = 40.23. 47. “The colouring matter of Drosera Whittakeri. (11.)” ByE. Rennie, M.A.,D.Sc. In a previous communication (C.X. T?-a?ts.,1889, 371), the authoy has described two colouring matters separated from 1). Whittakeri, which he believed to be derivat,ives of methylniiphthaquinone. He now confirms the formula C,,H,O, previously assigned to the less soluble and more abundant constituent ; a determination of its mole-ciilar weight, by Raoult’s cryoscopic method, gave the value 223, the calculated value being 220.When boiled with a solution of sodium 185 carbonate, this substance Tields reddisli-brown crystals of a mono-sodium derivative, C ,,H,O,Na*2H,O, from which the corresponding calcium derivative was prepared ; it also yields a disodium derivative. Two yellow crystalline acetyl derivatives were obtained from it, one melting at 154",the other at 138",the former being a triacetate, and the latter a compound of the trincetate with acetic acid. The formula CllH804previously assigned to the more soluble snb-stance is confirmed ; it Fields a diacetate. Hitherto this substance has always been obtained in red ci-ystals ; in an experiment.in which a small quantity was incompletely oxidised, a portion was recovered in the form of yellow crystals melting at Z78", and the author is therefore inclined to think that the pure substance is yellow. 48. 'I Preparation of mono-, di-and tri-benzylamine." By Arthur T.Mason, Ph.D. No good method having as yet been published for the preparation of the henzylamine bases, the author has carefully examined the interaction of ammonia and benzyl chloride in nlcoholic solution, and finds that it takes place without a.pplication of heat and is complete in four or five days. If the theoretical quantity of ammonia be used, tribenzylamine is the principal product, the primary and secondary nmines being formed in very sniall quantity ; whereas when a large excess of ammonia (20 mols.to 1mol. of chloride) is used, mono- and di-benzylamine form the chief products, tribenzylamine appearing in small quantity. The details of the process have been worked out', as also an easy method for the separation of the three amines based on the difference in solubility in water of the chlorhydrides. Di-benzylamine has been prepared for the first time by distillation under reduced pressure : it is a colourless liquid distilling withoiit under- going the slightest decomposition at 188-189" under 35 xm, pressure. 49. "Piazine (pyrazine) derivatives, (11.)" By Arthur T. Mason,Ph.D. A continuation of previous researches ((7.8.Tmts., 1889, 97 ; Ber., 20, 267), having reference to the constitution of the compounds resulting from the interaction of eth~-lenediamine and orthocli-ketones. The first product from benzil and etbylenediamine is not a true piazine, being easily recvnverted into its generators by dilute chlorhydric acid :--When heated above its melting point, this compound (so calle (2, 3) diphenylpiazine (5, ti) dihydride) yields two true piazine deriv- atives, which are not resolved into their generators bv dilute chlorhydric acid : one of these compounds is isomeric with t8hc (5, 6) dihydride, and is formed by a molecular transformation of that sub- stance : it contains two imide (NH) groups, and is a strong base, beiqg very soluble in dilute chlorhydric acid ; it is very easily oxidised, a.nd even when dissolved in chlorhydric acid saturated with carbon dioxide changes spontaneously into the final product of inter-action-( 2, 3) diphenylpiazine.In the author’s opinion, these facts can only be explained by assuming that the true piazines contain a para-bond, thus :-Ph C:N.CH2 Pl~.~*NH-CH Ph*C.N.C/H Ph*C:N*CH2’ P1i.C.NH.C: H ’ Ph*C*N*CH (5, 6) Uihydride. (1, 4) Dihydride. (2, 3) Diphenylpiazine. By the interaction of phenanthraquinone and ethylenediamine, only two compounds are obtained, neither of which, however, is reconverted into its generators by chlorhydric acid ; they are represented by the formulae C8Hd.C*NH*CH C,H,-C*T*CH C6HI*C*NH*CH and CsH,.C*N-CH’ Phenanthrapiazine (1, 4) Pheiianthrapiazine.dihydride.A series of analogous compounds prepared from other ketones of the phenanthrene (retene and chrysene quinones) series and ethylene- and propylene-diamine are described ; their general properties are shown to be similar to those of phenanthrapiazine (1,4)dihydride and phenanthrapiazine. 59. Piazine derivatives. (111.)” By Arthur T. Mason, Ph.D., and L. A. Dryfoos, Ph.D, Details are given of the mode of preparing (2, 3) diphenylpiazine (1,4) dihydride and of its dibenzoyl and diacetyl derivatives. An addition product obtained by the interaction of the (5, 6) dihydride and hydrogen cyanide in alcoholic solution is described; as this is converted into diphenylpiazine by alcoholic potash, it is to be supposed t.ha,t the cyanogen radicles are attached to the nitrogen atoms.The constitutional formula of the compound is very probably Ph$H-N( CN)*CE2PIi-CH*N(CN).CH,o An account is given of a new method of preparing (2, 3) diphenyl-piazine, which consists in heating the (5, 6) dihydride with alcoholic potash ; R small quantity of a complicated compound-tetraphenyl- dipiazine--is also formed, which is distinguished by its sparing salubility in the ordinary solvents. 187 The pr0duct.s of the interaction of dimethoxybenzil or anisil and ethylenediamine, viz., (2, 3) dimethoxyphenylpiazine (5,6) dihydride and (2, 3) dimethoxyphenylpiazine, are described. It is shown that, when submitted to the action of potassium cyanide, (2, 3) diphenylpiazine (5, 6) dihydride yields the amide of (2, 3) di-phenylpiazinecnrboxylic acid, and that the corresponding conipound is formed from dimet,hoxyphenylpiazine dihydride when it is similarly treated.51. “Condensation products from ethylenediamine and derivatives of acetoacetic acid. (IV.)” By Arthur T. Mason, Ph.D., and L. A. Dryfoos, Ph.D. The authors describe ethylic ethylene-/3-amidomethylcrotonnte, CH,*C*NH*CpH4*.NH*Q.CH, CEt*CO2Et CEt*CO,Et ’ obtained by the interaction of ethylic methylacetoacetste and ethylenediamine ; and also the copresponding compounds from ethylic ethylacetoacetate and methylic acetoacetate. 52. “Studies of the oxidation products of turpentine.” By S. B. Schryver, Ph.D., B.Sc. The author finds that on oxidising turpentine with chromic mix- ture, besides terebic and terpenylic acids, a, third acid is obtained having the same composition as camphoronic acid, C9Hl4O6,but differing from it in electric conductivity (0.0102 instead of 0.0175) ; it is contained in the mother liquors from which the other acids have been separated, and is isolated through the agency of an insoluble lead salt.The crude aoid fused at 125-160”, but after repeated crystallisation from nitric acid at 135-137”. With the object of determining the constitution of terpenylic acid, attempts were made to synthesise various heptolactones : eventually that prepared from the methylisopropyllactic acid of the formula PrCMe(OH)*CH,*COOH was found to be identical with the lactone prepared from teracrylic acid. On reducing terpenylic acid with iodhydric acid, an acid was obtained which is shown to be identical with /3-isopropylglutaric acid prepared synthetically by condensing isobutaldehyde and ethylic malonate, combining the product with ethylic sodiomalonate, and hydrolysing the resulting tetrethylic salt. The conclusion is arrived at that terpenylic acid is to be represented by the formula C0OH*CH,*yH.QHz MezC GO ‘0’ 188 53.“Addendum to note on the nature of depolarisers.” By Henry E. Armstrong. I am induced to somewhat extlend my recent note on depolarisers in order that the argument there made use of in considering the diesolution of metals such as magnesium in nitric acid may be clearly understood and its consequences more fully realised.It is one of the most noteworthy features of such interactions that when reduction is carried beyond the nitric oxide stage, it invariably proceeds to ammonia, and gives rise to a variety of products: so that whereas neither nitrous oxide nor nitrogen is evolved when metals such as silver and mercury are dissolved, these two gases are always obtained when more active metals are the agents. From this it would appear that there is a limit of (?) electromotive force which must be exceeded if it be desired to extend the reduction beyond the stage involving the formation merely of nitrogen dioxide and monoxide. A somewhat similar case is presented by the behaviour of sulph-uric acid solutioiis on electrolysis.Whereas, besides hydrogen, only oxygen is obtained under certain conditions, under others ozone, per- sulphuric acid and hydrogen peroxide are also produced. This apparently is a phenomenon of the same order, but in a measure the converse of thst presented by nitric acid, as oxygen-not hydrogen-is the active substance. Judging from McLeod’s observations (19.8. Tram., 1886, 591) ,it is clear that “ current density ” is an all-important factor in determining “peroxidation,” but it remains to be determined whether it is the sole factor : the individual influence of electromotive force, of current strength and of current density, in fact, all require careful study in this as in many other cases of electrolysis ; undoubtedly much depends on the concentration of the acid, The peroxidation may be regarded as the outcome of oxygen depolarisation, effected apparently in two ways : part of the oxygen becoming affixed to sulphuric acid, persulphuric acid is formed, which in part gradually undergoes hydrolysis, affording hydrogen peroxide-a non-electrolytic change ; while another part serves as oxygen depolariser, affording ozone.On this assumption, Ozone is not the product of the fortuitous concourse of three oxygen atoms, but of the interaction of oxygen atoms in circuit with per- sulphuric acid ;and if this be the origin of electrolytic ozone, it appears not improbable that the oxidation of phosphorus, which is attended by the formation of ozone, will also be.found to involve the formation of a peroxide hitherto undiscovered. In the case of a, metal such as magnesium dissolving in consider- able excess of nitric acid, if a plate be imagined to be undergoing attack and conversion into nitrate at any one point, the displaced hydrogen may, it would seem, “ travel along ” a very large number of paths to other points on the plate capable of acting as negative pole and of there meeting with nitric acid in sufficient amount to oxidise it, and it is scarcely conceivable, therefore, that it should escape if the nitric acid act directly as depolariser. It is also difficult to understand why one substance, an electrolyte, should act in two ways in the same circuit, and the difficulty appears to be equally great whether any form of Grothns’ hypothesis, or a dissociation hypothesis, be adopted in explanation of electrolysis.But these difficulties seemingly disappear if-as previously suggested-the active depolariser be a nitrous compound or derivative ; perhaps, at all events, at the initial stage, nitrogen dioxide. Moreover, it would appear to be possible in this manner to account also for the extension of the reduction to ammonia: in the case of a metal like silver the amount of depolariser must always tend to reach a, maximum value depending on the extent to which the reversible interchange ex-pressed by the equation NO + 2HN03 =3N02+ OH2is limited by the concentration and temperature; brit it is limited by these con-ditions alone.In the case of more active metals, it appears probable that the nitric oxide also functions as depolariser and is reduced to hydroxylamine and ultimately to ammonia. If such an action take place, it follows (from Ohm’s law) that the more active the metal the more rapidly will hydrogen be displaced by it, giving greater opportunity therefore for nitric oxide to undergo reduction and lead- ing to the production of an increased proportion of products of extended reduction. Any circumstance which would tend to diminish the proportion of nitrogen dioxide relatively tao monoxide present in solution would, therefore, promote the formation of such products, and, in point of fact, Acworth and I have noticed, even in the case of copper, that when the metal is dissolved in diluted nitric acid, it appears to be more “active,” i.e., to furnish a larger proportion of products of extended reduction, than when more concentrated acid is used : as the preseme of water must obviously favour the reversal of the interchange expressed by the equation NO + tLHN03=3N02 + H20, so that weaker would potentially contain a larger proportion of monoxide than stronger solutions of nitric acid, these observations would appear to be in harmony with the hypothesis here advocated.There is no evidence, be it remarked, that hyponitrous acid can be formed in acid solution, i.e., by direct reduction of nitric or even of nitrous acid, and the whole of the nitrous oxide which is evolved when metals are dissolved in nitric acid may result from the inter- action of nitrous acid and hydroxylamine.That reduction invariably extends to ammonia whenever hydroxylamine is formed is probably a consequence of the ex treme readiness with which hydroxylarnine 190 is itself reduced, so that, in fact, when rediiction once proceeds beyond the nitric oxide stage, it is to be supposed that there are necessarily a number of competing depolarisers present in solution-nitrogen dioxide and monoxide and hydroxylamine (and perhaps others), none of which, however, are electrolytes in the sense in which the term is ordinarily nnderstocd. And here it may be pointed out that the fact that a nitrate may be reduced in alkaline solution by sodium amalgam, or aluminium, or zinc, is no argument against the conclusion above arrived at that probably nitric acid does not directly act as depolariser, as in these cases the alkaline solution appears to be the electroly5e and the nitrate merely the depolaiaiser-- SO that the nitrate does not act in two ways.As nitrates may be wholly converted intc ammonia by reducing an alkaline solution, it would seem probable that in such cases hydroxylamine is not an in-termediate product, as nitrogen is obtained on boiling an alkaline solution of this snbstance. The argument here made use of would appear also to afford an explanation of the effect produced by varying the electromotive force, Le., by metals of different degrees of '' activity " :as increase of electro-motive force, other conditions remaining unchanged, would increase the current strength and consequently the rate of change ; and, as indicated above, an increase in the rate of change would doubtless involve an increase in the amount of products of extended reduction. It remains to bc pointed out that the objection made to the as-sumption that nitric acid can act in two ways is equally applicable to the case of sulphuric acid ; in other words, that it is not likely that sulphuric acid would act as electrolyte and as oxygen depolariser.It becomes necessary, therefore, to reconsider the manner in which solutions of this acid undergo electrolysis. On the one hand it is coiiceivable that the water molecule alone suffers pal-tition, not the sulphuric acid (HPSOC)molecule, as commonly supposed, and that under certain conditions the 'latter takes a direct part in the change, becoming osidised ; but this does not appear to be probable, especi- ally as there is reason to believe that the acid in conjunction with water actually functions as electrolyte.An alternative assnmption would be that the immediate product has been overlooked, and it can scarcely be gainsaid that there is much evidence in favour of this view. It is not improbable that the first products of electrolysis are hydrogen and persulphuric acid ;it may be supposed that under "ordin-ary " circumstances this latter substance is resolved at the electrode sarface into oxygen and sulphuric acid, but when the electrode surface is small much escapes unchanged, this being especially the case when the electrolyte is a somewhat concentrated acid-a condition which in itself favours the survival of persulphuric acid.Not only do recent 191 observations on the electrolysis of various sulphates support this con- tention, but it would seemingly also serve to explain the extraordinary character of the curve representing the change in conductivity of solutions of sulphnric acid on dilution. 54. ‘I The molecular complexity of liquids.” By William Ramsay, Ph.D., F.R.k., and John Shields, Ph.D., D.Sc. From tho ascent of a liquid in a capillary tube of known diameter and its relative density, the surface tension of the liquid may be calculated. The molecular volume of a, liquid, at any temperature, is proportional to the number of molecules contained in unit volume at that temperature ; and the two-thirds root of the number representing the molecular volume is proportional to the number of molecules distributed in unit surface, with the proviso that the mean distance between 2 mols.at the surface is equal to that between any 2 mols. in the interior. Multiplying the number representing surface tension by that representing molecular surface, the product may bt: termed “molecular surface energy.” By stating surface tension in degrees, and molecular surface in square centimetres, the product is expressed in ergs, and may be defined as the work required to pro-duce or to extend a surface on which equal numbers of molecules lie.This energy is nil at the critical temperature of the liquid, for there is no surface. It increases with fall of temperature, and after about 20” below the critical temperature, the rate of increase is practically a linear function of the temperature. The equation which exhibits this relation is ~(Mw)$= k(~-d), where the letters have the following definitions :-y, surface tension, k, a numerical constant, M, molecular weight, T, temperature measured down- 21, specific voliime, wards from the critical temperature, d, being a numerical constant equal to about 6. This equation is analogous to that which expresses volume energy in its relation to heat, viz., pv = RT. As a gas is said to be normal if, when u expresses the volume of its molecular weight taken in grams, and p is measured in atmospheres, R is constant between various limits of temperature, so a liquid may be said to be normal, i.e., to be composed of molecules of no greater degree of complexity than those which form its gas, if the value of k is const.ant between various limits of temperature.This affords a means, therefore, of investigating the molecular weights of liquids as such, and it is the first colligative property of liquids which has been discovered. In all 57 liquids have been investigated. They divide themselves into two groups: those of which the rriolecule~ are simple (36 in number), and those which, in the liquid state, consist of molecules composed of several gaseous molecules coalesced to form a complox.To the latter class belong the alcohols, the acids, water, phenol, and three others, nitroethane, acetonitrile and acetone. It is remarkable that, so far as our experiments have gone, no liquid shows a greater molecular complexity than that in which the molecu- lar weight of t'he gas is multiplied by the factor 4. Water at 0" has approximately the formula, HBO1,i.e., (H,O),; the degree of com-plexity, however, is altered by rise of tempel-ature, and the complex molecules gradually dissociate into more simple groups. A determination of molecular surface energy also permits of a close estimate of the critical tcmpomtures of " normal " liquids. The numbers representing these important data are given in the complete memoir.55. '' The preparation of active amyl alcohol and active valeric acid from fusel oil." By W:A. C. Rogers, The author has prepared the alcohol by a niodification of Le Bel's method communicated to him by Professor Odling and Mr. Narsh, which consists in heating the alcohol with a fuming aqueous solution of hydrogen chloride in closed tubes at loo", the ti-eatmeot being repeated until the rot,atory power of the product reached a maxin7um. Finally, from 16.2 litres of purified fusel oil, he obtained 250 C.C. of an alcohol rotating -8" 30' per 200 mm. at 22" (or [a]== -5.2"). By oxidising this alcohol, a T-aleric acid was obtained rotating 26" per 'LOO mm. at 22" ([a],,= 13.9"). The values thus obtained are practically identical with those given by Guye and Chavanne in a recent paper.RESEARCH FUND. A donation of SlOO to the Research Pund has been received from Mr. L. Mond, F.R.S., by the Treasurer since the meeting of the Society. 193 The following is the text of the address presented to Sir John Lnwes, Bart., &c., and Dr. Gilbert, on July 29th, on the occasion of the Rothamsted Jubilee :-We, the President and Officers of the Chemical Society of London, 011 behalf of the Council and Fellows generally, desire on this occa-sioii to express our sense of the extraordinary value of your labours in the field of agricultural science, our admiration of your researches, and our gratitude for the immense number of exact data which YOU have placed at the disposal of chemists.Few men have been able to conduct experimental researches during so long a period, and there is no parallel in the history of science to your achievement in carrying on a single research without interrup- tion during a period of over 50 years. The plan laid down at its commencement has throughout been most rigidly adhered to, which is evidence of the skill originally displayed in its inception, and gives to your work its peculiar value. While affording guidance to the agriculturist, your researches have elicited information which will ever serve as the foundation of a truly scientific knowledge of the correlation of plant gr0wt.h and manurial constituents of the soil, and will be of the utmost value in all discussions of the chemistry of plant life.Your researches on the feeding of animak, in like manner, are not only of practical importance, but also shed much light on the processes of animal life. Great, however, as is the actual value to agriculture and agricul- tural science of your work, the example your single-minded devotion to the cause of scientific truth and research has afforded to the world is unquestionably to be regarded as of far greater value. Yours is the model of all agricultural experimental stations, and the methods that you have introduced are everywhere regarded as classical. The rare and enlightened munificence which has led the one of you to institute and maintain such a series of enqniries having been sup-plemented by a provision for the future conduct of the experiments in order especially to make it possible to deal with the great question of the ultimate exhaustion of the soil, the debt of gratitude which scieiice owes to t8he founder of the Rothamsted experimental station is extended into the distant future.It is, consequently, with a full sense of the inadequacy of our expressions that we to-day offer to you our heartfelt thanks and our wai-mest congratulations on your having been able to achieve results of such magnitude and importance. 194 The following “ Circular concerning the Hodgkins Fund Prizes ’’ has bcen communicated to the Society by the Secretary of the Smith- sonian Institution :-In October, 1891, Thomas George Hodgkins, Esq., of Setauket, New York, made a donation to the Smithsonian Institution, the income from a part of which was to be devoted “to the increase and diffusion of‘ more exact knowledge in regard to the nature and pro- perties of atmospheric air in connection with the welfare of man.” With the intent of furthering the donor’s wishes, the Smithsonian Institution now announces the following prizes to be awarded on or after July 1, 1894, should satisfactory papers be ogered in com-petition :-1.A prize of $10,000 for a treatise embodying some new and im- portant discovery in regard to the nature or properties of atmospheric air. These properties may be considered in their bearing upon any or all of the sciences, e.g., not only in regard to meteorology, but in connection with hygiene, or with any department whatever of bio-logical or physical knowledge.2. A prize of $2,000 for the most satisfactory essay upon- (a) The known properties of atmospheric air considered in their relationships to research in every department of natural science, and the importauce of a study of the atmosphere considered in view of these relationships. (b) The proper direction of future research in connection with the imperfections of our knowledge of atmospheric air, and of the connections of that knowledge with other sciences. The essay, as a whole, should tend to indicate the path best calculated to lead to worthy results in connection with the future administration of the Hodgkins foundation. 3. A prize of $1,000 for the best popular treatise upon atmospheric air, its properties and relationships (including those to hygiene, physical and mental).This essay need not exceed 20,000 words in length ; it should be written in simple language, and be suitable for popular instruction. 4. A medal will be established, under the name of “ The Hodgkins Medal of the Smithsonian Institution,” which will be awarded annually or biennially, for important contributions to our knowledge of the nature and properties of atmospheric air, or for practical ap- plications of our existing knowledge of them to the welfare of man-kind. This medal will be of gold, and will be accompanied by a duplicate impression in silver or bronze. The treatises may be written in English, French, German or Italian, and should be sent to the Secretarj of the Smithsonian 195 Institution, Washington, before July 1, 1894, except those in competition for the first prize, the sending of which may be delayed until December 31, 1894.The papers will be examined: and prizes awarded, by a committee to be appointed as follows :-One member by the Secretary of the Smithsonian Institution, one member by the President of the National Academy of Sciences, one by the President, pro tempore, of the American Association for the Advancement of Science ; and the committee will act together with the Secretary of the Smithsonian Institution as member, ex qficio. The right is reserved to award no prize if,in the judgment of the committee, no contribution is offered of sufficient merit to warrant an award.An advisory committee of not more than three European men of science may be added at the discretion of the Committee of Award. If no disposition be made of the first prize at the time now an- nounced, the Institution may continue it until a later date, should it he made evident that important inrestigations relative to its object are in progress, the results of which it is intended to offer in coni- petition for the prize. The Smithsonian Institution reserves the right to limit or modify the conditions for this prize after Decemhey 1, 1894, should it be found necessary. Should any of the minor pyizes not be awarded to papers sent in before July 1,1894, the said prizes will be withdrawn from competition.A principal motive for offering these prizes is to call attention to the Hodgkins Fund, and the purposes for which it exists, and accord- ingly this circular is sent to the principal universities, ahd to all learned societies known to the Institution, as well as to representative men of science in every nation. Suggestions and recommendations in regard to the most effective application of this fund are invited. It is probable that special grants of money may be made to specialists engaged in original investigation upon atmospheric air and its properties. Applications for grants of this nature should have the indorsement of some recognised academy of sciences, or other insti- tution of learning, and should be accompanied by evidences of the capacity of the applicant, in the form of at least one memoir already published by him, based upon original investigation. To prevent misapprehension of the founder’s wishes, it, is repented that the discoveries or applications proper to be brought to the con- sideration of the Committee of Award, may be in the field of any science or any art without restriction ; provided only tliat they have to do with “the nature and properties of atmospheric air in connec-tion with the welfare of man.” Infor*mation of any kind desired by pemons intending to become cornpettitorswill be furnished on application.196 All communications in regard to the Hodgkins Fund, the Hodgkins Prizes, the Hodgkins Medals, and the Hodgkins Fund Publications, or applications for grants of money, should be addressed to S.P. Langley, Secretary of the Smithsonian Inst’itution, Washington, U.S.A. ADDITIONS TO THE LIBRARY. I. Donations. Trait6 pratique de calorimhtrie chimique, par M. Berthelot. Paris 1893. From the Author. Royal Society of London. Philosophical Transactions. Vol. 130 (1840). 4to. (To complete set.) From G. T. Holloway, Esq. 11. By Purchase. Lehrbuch der physiologiscben Chemie, von R. Neumeister. Erster Theil : Die Ernahrung. Jena 1893. Anleitung zur Harnanalyse, von W. F. Loebisch. Wien und Leipzig 1893. Die Wirkungsweise der Rectificir- und Destillir- Apparate, von E. Hausbrand. Berlin 1893. Procentische Zusammensetzung und Nahrgeldwerth der mensch- lichen Nahrungsmittel.Graphisch dargestellt., von J. Konig. 6ste Auflage. Berlin 1893. Die Leim- und Gelatine-Fabrikation, von F. Dawidowsky. Wien Pest und Leipzig 1893. L’alirnentation de l’homme et des animaux domestiques, par L. Grandeau. Tome I : la nutrition animale. Paris 1893. Molecularkra€te, von E. Seelig. ‘Lte Autlage. Berlin 1893. Handbuch der Chemischen Technologie, von F. Fischer (Zugleich 14te Auflage von W‘agner’s Chemischen Technologie) . Leipzig 1893. Trait6 pratiqne d’analyse chimique et de recherches toxicolo, ’ques, par G. GuBrin. Paris 1893. Die Verwerthung des Holzes auf chernischen Wege, von J. Bersch. Wien, Pest und Leipzig 1893. Royal Society of London. Philosophical Transactions. Vols. 43-129 (1’744-1889).Indexes-Vols. 1-70 (l655-1’780), and 71-110 (1781-1820). 95 VO~S. 4t0. 197 Lehrbuch der Allgemeinen Chemie, von W. Ostwald. Zweite Auflnge. Band 11, 1. Chemische Energie. Leipzig 1893. Das Kupfer, von Standpunkte der gerichtlichen Chemie, Toxi-cologie und Hygiene, von A. Tschirch. Stuttgart 1893. El6ments de Cristallographie physique, par C. Soret. Genhve et Paris 1893. Theoretische Chemie, vom Standpunkte der Avogadro’schen Regel und der Thermodynamik, von W. Nernst. Stuttgart 1893. Entwickelnngsgeschichte, und kritisch-experimenteller Vergleich der Theorien uber die Natur der sogenannten Knallsaure und ihrer Derivate, von R. Scholl. Miinchelr und Leipzig 1893. Die Thermodynamik in der Chemie, von J. J. van Laar. Amster-dam und Leipzig 1893. HARRISON AND SONS, PRINTERS IN ORDINAEY TO HER MAJESTY, ST. MARTIN’S LANE.
ISSN:0369-8718
DOI:10.1039/PL8930900171
出版商:RSC
年代:1893
数据来源: RSC
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