a-x-m-solution-of-methylamine-a-weak-organic-base-has-a-ph-of-x-what-is-the-kb-a

Question

A 3.93×$$10^{–5} M $$solution of methylamine, a weak organic base, has a pH of 9.56. What are the K_{b} and pK_{b} for this base?

Accepted Answer

K_{b} = 4.4×$$10^{–4}$$, pK_{b} = 3.36

Answer

K_{b} = 1.3×$$10^{–9}$$, pK_{b} = 8.88

Answer

K_{b} = 2.8×$$10^{–10}$$, pK_{b} = 9.56

Answer

K_{b} = 1.9×$$10^{–15}$$, pK_{b} = 14.71

A 3.93×10–5 M solution of methylamine, a weak organic base, has a pH of 9.56. What are the Kb and pKb for this base?