212 THE ROYAL SOCIETY OF CANADA 



with CaS0^-3H._S0„ which contained SO3: 0.94H2SO,:0-07CaO 

 {Winter, 1910-1911). 



No. 11. W. D. Bonner: — Experimental determination of hinodal 

 curves, plait-points, and tie-lines, in fifty systems, each consisting of 

 water and two organic liquids. — As it was desired to study as many 

 different systems as possible, and as organic liquids are in general 

 costly, it was necessary to develop a method of working which would 

 not necessitate the use of more than a few grams of material in each 

 experiment. The difficulties of analysis were avoided by adopting 

 a modification of Bancroft's method of "quantitative synthesis," and 

 the positions of the tie-lines and plait-points were determined by a 

 graphic method described in the paper by Lash Miller and McPherson 

 referred to above. {Jour. Phys. Chem. 14, pp. 738-789, 1910). 



No. 12. W. IF. Evans: — The rate of propagation of /lames. — ^The 

 rate at which a flame spreads along a circular wick moistened with a 

 combustible liquid was determined by measuring the rate at which 

 a disc of millboard (dipping in the liquid) must be rotated in order 

 that the flame may remain stationary. For a standard size of flame, 

 occupying a fixed position on the wick, the rate was found to be a 

 linear function of the initial temperature of the liquid. 



Curves were obtained for 22 pure liquids and solutions, with 

 ''seconds per revolution" as ordinates, and initial temperatures as 

 abscissœ. All showed a slight concavity, most marked at temperatures 

 near the flash-points. {Winters 1910-1912). 



No. 13. Saul Dushman:—The behaviour of copper anodes in 

 chloride solutions. — Having found that it was possible to make copper 

 dissolve anodically in hydrochloric acid wholly as cupric or wholly 

 as cuprous salt or as a mixture of these in any desired proportions de- 

 pending on the concentration of acid, current density, rate of stirring 

 and rate of circulation of the electrolyte thi'ough the cell, a series of 

 quantitative measurements was undertaken to see whether there 

 was equilibrium at the electrode between the cupric salts, cuprous 

 salts, hydrochloric acid, and metallic copper. 



As the concentrations at the electrode were very different from 

 those in the l)()d3^ of the solution — sometimes they were twenty times 

 as gieat — they had to be calculated from the latter by allowing for 

 diffusion, and methods had to be devised for obtaining the constants 

 needed in these calculations. 



Electrolyses were carried out in which the concentration of the 

 hydrochloric acid, the current, the anode area and the rate of circu- 

 lation of the electrolyte through the cell were varied; the fiaction of 

 the copper dissolved as cuprous salt varied from 25% to 74 %, and 

 agreed within the expeiimental errors with the fraction calculated 



