122 DR. B. D. STEELE, DR. D. McINTOSH AND DR. E H. ARCHIBALD 



(a) Hydrogen chloride 



Bromine, potassium iodide, thionyl chloride, sulphuryl chloride, and 

 uranium nitrate (very slight increase), phosphorus pentachloride, 

 pentabromide, and oxychloride (considerable increase) ; 



(b) Hydrogen bromide 



Phosphorus oxychloride (considerable increase) ; 



(c) Hydrogen iodide- 



Iodine, sulphuric acid, carbon disulphide, and phosphorus oxychloride 

 (slight increase) ; 



(d) Sulphuretted hydrogen- 



Phosphorus pentachloride, and sulphuryl chloride (slight increase). 



The following substances did not cause an increase in the conductivity of either of 

 the solvents : 



Sodium, sodium sulphide, sodium biborate, sodium acid phosphate, sodium nitrate, 

 sodium sulphide, sodium thiosulphate, sodium arsenate, chromic acid, the following 

 salts of potassium : the nitrate, hydroxide, chromate, sulphide, acid sulphate, 

 ferrocyanide, ferricyanide ; ammonium fluoride and carbonate ; rubidium and caesium 

 chlorides ; 



Magnesium sulphate, calcium fluoride, strontium chloride, barium chloride, oxide, 

 nitrate and chromate ; copper sulphate, mercuric chloride, zinc sulphate, boron 

 trichloride, aluminium chloride, and sulphate ; carbon dioxide, stannous chloride, lead 

 peroxide, nitrate, and cyanide ; phosphorus tribromide, bismuth nitrate, tartar emetic, 

 manganese chloride, ferric chloride, ferrous sulphate, nickel sulphate, and cadmium 

 sulphate. 



In addition to the organic ammonium bases, we have, in conjunction with 

 Dr. J. W. WALKER,* examined the conductivity of solutions of about 80 organic 

 substances in each of the foregoing solvents. 



The only substances which form conducting solutions in H 2 S are the ammonium 

 bases and a few alkaloids such as nicotine and pyridine. On the other hand, many 

 ethers, ketones, esters, nitrites, and, generally speaking, substances containing oxygen 

 or nitrogen, form conducting solutions in hydrogen chloride, bromide, and iodide. 

 The hydrocarbons, although in some cases soluble in all proportions, do not conduct. 

 We have noticed that the solution of those substances which conduct is accompanied 

 by a considerable evolution of heat, while little or no heat is evolved in the case of 

 other substances. 



This indicates chemical interaction between the conducting solute and the solvent, 

 and many of the resulting compounds have been isolated and analysed.! It has been 



* 'Journal of the Chemical Society,' 1904, 85, p. 1098. 

 t ARCHIBALD and MC!NTOSH, ' J. C. S.,' 1904, 85, p. 919. 



