528 
CHEMISTRY: D. A. M'INNES 
TABLE I 
Calculation of the Liquid Junction Potential and Electrode Potentials (in 
Millivolts) of Chloride Concentration Cells With Silver — 
Silver Chloride Electrodes 
SUBSTANCE 
MOLS PER 
LITER 
TRANSFERENCE 
NUMBER 
E. M. F. OF 
CELL E 
LIQUID JUNC- 
TION 
POTENTIAL, £l 
ELECTRODE 
POTENNTIAL 
AVERAGE 
DEVLATION 
FROM MEAN 
HCl 
0.01665 
0.833 
— 92.35 
—36.94 
— 55.41 
0.001665 
NaCl 
0.01673 
0.396 
-43.60 
+ 11.46 
-55.06 
0.24 
0.001674 
KCl 
0.01670 
0.496 
-54.24 
+00.44 
-54.69 
0.001674 
HCl 
0.03330 
0.833 
-91.62 
-36.64 
-54.98 
0 . 003329 
0.25 
KCl 
0.03347 
0.496 
-54.03 
+0.43 
-54.47 
0.003347 
HCl 
0.008315 
0.833 
-64.87 
-25.95 
-38.92 
0.001665 
NaCl 
0.008364 
0.396 
-30.73 
+ 8.08 
-38.81 
0.04 
0.001674 
KCl 
0.008329 
0.495 
-38.44 
+ 0.39 
-38.83 
0.001670 
HCl 
0.006686 
0.833 
-56.14 
-22.45 
-33.79 
0.001665 
NaCl 
0.006686 
0.396 
-26.53 
+ 6.97 
-33.49 
0.08 
0.001674 
KCl 
0.006700 
0.495 
-33.30 
+0.34 
-33.64 
0.001670 
It will be observed that in each group of cells in which the solutions 
of electrolytes have the same concentrations, the calculated sum of the 
electrode-potentials has the same value within a few tenths of a milli- 
volt. This is true even though the liquid- junction potential in the 
case of the hydrochloric acid cells is 40% of the total electromotive 
force, and of opposite sign to that in the case of the sodium chloride so- 
lutions. The agreement is as close as can be expected from our knowl- 
edge of the transference-numbers. Calculations based on other work 
by the same author show a similar agreement. 
