NOVEMBEE 14, 1913] 



SCIENCE 



713 



E. W. Washburn and S. J. Bates: The Electro- 

 chemical Equivalent of Iodine and the Value of 

 the Faraday. 

 H. C. P. Weber: The Reduction, of Chromium 



Chloride. 

 T. W. B. Welsh and H. J. Bkodeeson: Anhy- 

 drous Hydrazine as a Solvent. (Presented by 

 A. W. Browne.) 



The solubility of 120 elements and eompoimds 

 in anhydrous hydrazine was studied. Of the me- 

 tallic elements employed, the alkali metals are 

 the only ones appreciably acted upon and dis- 

 solved. The solubility of the halogen compounds 

 increases with increase in the atomic weight of the 

 halogen. The chlorides of the alkali metals are the 

 least soluble. Carbonates and oxides are, as a 

 rule, insoluble. Nitrates are generally soluble. 

 Sulphates and sulphides are insoluble. Ammonium 

 compounds are soluble with the exception of the 

 tertiary phosphate. The solution of ammonium 

 salts is accompanied by hydraeinolysis with evolu- 

 tion of ammonia. A large number of compounds 

 dissolve, and at the same time react with the sol- 

 vent. 



T. W. B. Welsh and H. J. Broderson: Chemical 

 Reactions in Anhydrous Hydrazine. (Presented 

 by A. W. Browne.) 



Metathetical reactions take place between sol- 

 uble salts of zinc, or cadmium, and hydrazine sul- 

 phide, with formation of the metallic sulphides. 

 In fact, solutions of these salts in anhydrous hy- 

 drazine may be titrated with solutions of hydra- 

 zine sulphide, using the brownish-yellow color of 

 the latter as indicator. By the action of the 

 hydrazo-iase, sodium hydrazide, upon zinc chloride 

 in hydrazine solution, a solid which is in all prob- 

 ability zinc hydrazide, is precipitated. Hydrazo- 

 bases are neutralized in hydrazine solution by 

 hydrazine salts, which under these conditions act 

 as acids. For example, sodium hydrazide reacts 

 with hydrazine chloride, yielding sodium chloride 

 and hydrazine. Metallic sodium will precipitate 

 metallic cadmium, zinc and iron, from solutions of 

 their salts. 



T. W. B. Welsh: Electrolysis of Solutions of 



Sodium Hydrazide in Anhydrous Hydrazine. 



(Presented by A. W. Browne.) 



Solutions of sodium hydrazide (prepared by the 



action of either sodium amide or metallic sodium 



upon hydrazine) in anhydrous hydrazine have 



been electrolyzed, in absence of air and moisture, 



under such conditions as to permit measurement 



and analysis of the gases evolved at the electrodes. 

 In general nitrogen and hydrogen were obtained 

 at both electrodes. For each gram atom of copper 

 deposited on the coulometer cathode, from 1.1 to 

 1.5 gram atoms of nitrogen were liberated at the 

 anode when the electrolyte was dilute, and from 

 2.1 to 2.6 when the concentration was higher. A 

 blue color due to metallic sodium was in some ex- 

 periments transitorUy observed at the cathode. A 

 characteristic yellow coloration was (reversibly) 

 obtained in the neighborhood of the cathode. 

 A. R. Hitch: Electrolysis of Silver Trinitride in 



Liquid Ammonia. 

 A. E. Hitch: Thermal Decomposition of Various 



Trinitrides. 

 Harold Eaton Rieggee: The System Hydrazine 



Trinitride, Hydrazine. (Presented by A. W. 



Browne.) 



It has been found possible to prepare hydrazine 

 trinitride (first prepared by Curtius) by each of 

 three methods: (a) Interaction of anhydrous hy- 

 drazine and ammonium trinitride, (6) interaction 

 of anhydrous hydrazine and anhydrous hydrogen 

 trinitride, and (c) interaction of alcoholic hydra- 

 zine and ethereal hydronitric acid. A convenient 

 method for the analysis of the compound has been 

 formulated, and certain of its properties and re- 

 actions have been studied, including the behavior 

 of the substance when heated in a sealed tube to 

 100°. The substance is very soluble in anhydrous 

 hydrazine, and soon deliquesces when exposed to 

 hydrazine vapor. A study of the solubility 

 (T, X) curve for the system hydrazine trinitride; 

 hydrazine yielded results that point toward the 

 existence of a monohydrazinate of the formula 

 N^H^N^ . N^H^, and to the probable existence of 

 at least one higher hydrazinate. 



W. J. Marsh: Action of Various Oxidising 

 Agents upon Hydrazine in Liquid Ammonia 

 Solution. 



The behavior of free hydrazine in liquid am- 

 monia at — 33° toward potassium permanganate, 

 manganese dioxide, mercuric oxide (yellow), am- 

 monium persulphate, sodium peroxide, ferric ox- 

 ide, potassium chlorate, potassium iodate and am- 

 monium perchlorate, respectively, has been studied 

 with the aid of a modified nitrometer. All but the 

 last three of these substances oxidize the hydra- 

 zine more or less rapidly, with formation of nitro- 

 gen and water as the oxidation products. Po- 

 tassium permanganate is quantitatively reduced 

 to manganous hydroxide and potassium hydroxide. 

 In several cases the gas was evolved in two distinct 



