[1903 McBain ABSTRACT 6 1 



The existence of "copper-, cobalt-, and nickel-phosphites" 

 {('. <,>•., Na.CuPO,) is deduced from the movement of the heavy- 

 metal toward the anode. 



The movement toward the anode of the green solution of 

 chromic hydroxide in strong alkali demonstrates the existence 

 of chromites ; the chromic hydroxide is not merely dissolved as 

 colloid, for it can diffuse through parchment into alkaline solu- 

 tion. Similarly the zinc in potassium zincate becomes more 

 concentrated at the anode. 



1903. S. C Lind. 



The Constitution of Potassium Ruthenium Nitroso-chloride in Aqueous 

 Solution. Jour.j^m. Chem. Soc, 2j, 928. 



A 0.025 m solution was connected by siphons containing 

 0.05 m potassium chloride solution solidified by agar agar with 

 anode and cathode compartments containing Pt electrodes sur- 

 rounded by hydrochloric acid and potassium hy^drate respec- 

 tively. A pink color moved toward the anode while no color 

 change occurred in the cathode siphon. This shows that ru- 

 thenium is contained in an anion, presumably RuCl^NO" ; the 

 author further concluded that it proved that no cation contains 

 ruthenium. 



1903- J- W. McBain, 



Electrolytic Migration in Solutions of the Weak Acids. This paper has not 

 been published in full; abstracts have appeared in Trans. Roy. Soc. Canada, 

 May, 1903, and 1904, and in Trans. Am. Electrochem. Soc, 4, 184. (1903). 



Apparatus : many forms, mostly pairs of U tubes ; capacity 

 40-350 c.c. ; Pt. electrodes ; o.04g Ag ; diaphragms of cloth or 

 bundles of small tubes ; 2-5 middle portions, the real one un- 

 changed within 0.00 to 0.05 c.c. of decinormal alkali. 



The author eliminated the irregular and uncontrollable reac- 

 tions occurring at the electrodes during the electrolysis of acetic 

 and propionic acids, which would otherwise have discredited 

 the results, by surrounding the electrodes with long columns of 

 solutions of sodium sulphate, sulphuric acid, hydrochloric acid, 

 etc. This made the apparatus complicated and the manipula- 

 tion difficult. The electrode solutions were carefully tested for 

 in the middle portions, but were usually altogether absent, and 

 in no case present in quantity sufficient to cause an error of 20 

 percent in the result. An experiment with hydrochloric acid, 



