306 JAMES GEERE DICKSON 
Table 2 
The Composition of the Normal Solution in Terms of Osmotic Concentration 
Salt 
Dissociation 
Factor 
Concentration 
Percent 
Volume Molecular 
Decimal 
Fraction 
Osmotic 
Ca(N03)2 
KNO3 
KH2PO4 
MgS04 
NaCl 
1.94 
1.90 
1.86 
1.87 
2.00 
0.0533 
0.0133 
0.0133 
0.0133 
0.0067 
0.00325 
0.00132 
0.00098 
O.OOIII 
0.001 14 
Ml 307.7 
Ml 758.4 
iW/l02I.8 
Ml 903.1 
Ml 872.5 
0.0063 
0.0025 
0.0018 
0.0022 
0.0023 
Total salts 
O.I 000 
0.00780 
Ml 128.2 
O.OI5I 
The dissociation of the salts, with the exception of monopotassium 
phosphate and monosodium phosphate, is considered as occurring in 
one step in each case as illustrated by the following equations: 
KNO3 = K + NO3, 
MgS04 = Mg + SO4. 
The two phosphate salts are considered as dissociating in four steps 
instead of one as shown in the following scheme, which illustrates the 
complexity of electrolytic dissociation in a solution of monopotassium 
phosphate, when the process is incomplete and proceeds by stages 
with increasing dilution. 
Stage I. KH2PO4. 
Stage II. (i) KH2PO4, (2) K, (3) H2PO4. 
Stage III. (i) KH2PO4, (2) K, (3) H2PO4, (4) H, (5) HPO4. 
Stage IV. (i) KH2PO4, (2) K, (3) H2PO4, (4) H, (5) HPO4, 
(6) H, (7) PO4. 
The algebraical method of calculation of the dissociation of these salts 
is explained in detail by Tottingham (1914). For practical purposes 
only the first two dissociation steps indicated above need be considered 
for monopotassium or monosodium phosphate. 
The effects of dissociation in a complex mixture of salts, even when 
very dilute, are not easily determined. In such a mixture, the in- 
fluence of one salt upon the dissociation of another should be taken 
into account in work of this character, but the problem becomes 
complicated by the difficulties attending calculations. It was not 
