A solution of a weak monoprotic base B (0.50 M) and its salt BHCl (0.80 M) has a pH = 9.40. What is the value of Kb for this base, B?
use:
pH = 14 - pOH
9.4= 14 - pOH
= 4.6
use:
pOH = pKb + log {[conjugate acid]/[base]}
4.6= pKb + log {0.8/0.5}
pKb = 4.396
use:
pKb = -log Kb
4.396= -log Kb
Kb = 4.018*10^-5
Answer: 4.02*10^-5
A solution of a weak monoprotic base B (0.50 M) and its salt BHCl (0.80 M)...
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