87
In most instances, n was greater than, or equal to 3.
Standard deviations from the mean, a, are also included.
Deviations were generally within 5% to 10% of the averaged
values of Kg, which shows that the constancy over the
intervals selected is within acceptable limits for these
types of systems. As a rule, the lower the concentration
of background electrolyte, the greater the standard devia
tion. Similarly, the lower the charge density of the
cation of the supporting electrolyte, the greater the
standard deviation. For divalent metal electrolytes the
values of Kg were constant over nearly the entire accessible
range. In 0.010N MgfC^CCH^^' Kg varied from 1.32^ x 104 M 1
4 _i
to 1.21 x 10 M over the entire titration for an average
of 1.27 x 104 M-1 + 5%. In 6.3 x 10_4N Mg(0CCHo), K
2 3 2 s
4-1 4
went from a low of 4.71 x 10 M to a high of 5.09 x 10
-1 4-1
M (average: 4.90^ x 10 M + 4%). The essentially in
variant apparent equilibrium association constants through
out the entire titrations, along with the single straight
line plots of log([BHP]/[BH]) vs. log([Pt/m]- q[BHP]), is
convincing evidence that only the effects of the surface
bound species are observed in these systems and that,
either intercalative binding is not taking place, or it
is being masked. On the other hand, in 0.15M CsHPO K
^ ~r S
varies from an average over the whole titration by + 25%
and by + 55% in 0.0025M CsI^PO^. The magnitudes of the
standard deviations over the range -0.8 < log([BHP]/[BH] <
0.2 are proportional to those given above for the entire