A 0.300 M solution of a weak base has a pH of 9.10. What is the base hydrolysis constant, Kb, for the weak base?
pH + pOH = 14
pOH = 14 - 9.10
pOH = 4.90
-Log[OH-] = 4.90 (pOH = - Log[OH-] )
[OH-] = 10-4.90
[OH-] = 1.26 * 10-6 M
And for weak bases,
[OH-] = (Kb*C)1/2
(1.26*10-6)2 = Kb * 0.300
Kb = 5.29*10-12
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