Be sure to answer all parts. The pH of a 0.30 M solution of a weak...

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Question

Be sure to answer all parts. The pH of a 0.30 M solution of a weak base is 10.02. What is the Kb of the base? Kb = × 10

science chemistry

Answer 1

Answer #1

Let us consider weak base be BOH

BOH(aq) -------> B⁺(aq) + OH^-(aq)

pH + pOH = 14

pOH = 14-10.02 = 3.98

pOH = -log [OH^-] = 3.98

[OH^-] = 10^-3.98 = 0.000105 M

BOH(aq) -------> B⁺(aq) + OH^-(aq)

Initial Concentration : 0.3 0 0

Change in concentration :(0.3-0.000105) +0.000105 +0.000105

Equilibrium concentration : 0.299895 0.000105 0.000105

Kb = [OH^-] [B⁺]/[BOH] = (0.000105)²/0.299895 = 0.000000011/0.299895 = 3.67 X 10^-8

Answer 2

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