The pH of a 0.018 M aqueous solution of 3,5-dimethylpyridine (C7H9N) is 9.20. Calculate Kb. (Assume Kw = 1.00 ✕ 10−14.)
use:
pH = -log [H+]
9.2 = -log [H+]
[H+] = 6.31*10^-10 M
use:
[OH-] = Kw/[H+]
Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC
[OH-] = (1.0*10^-14)/[H+]
[OH-] = (1.0*10^-14)/(6.31*10^-10)
[OH-] = 1.585*10^-5 M
C7H9N dissociates as:
Kb = [C7H9NH+][OH-]/[C7H9N]
Kb = x*x/(c-x)
Kb = 1.585*10^-5*1.585*10^-5/(0.018-1.585*10^-5)
Kb = 1.397*10^-8
Answer: 1.40*10^-8
The pH of a 0.018 M aqueous solution of 3,5-dimethylpyridine (C7H9N) is 9.20. Calculate Kb. (Assume...
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