A 0.214 M aqueous solution of a monoprotic base has a pH of 11.48.What is the ionization constant of this base? A)1.4 × 10^-2 B)4.3 × 10^-5 C)1.5 × 10^-11 D)5.1 × 10^-23 E)2.0 × 10^-6

Question

Quizplus · Accepted Answer

First, we need to find the pOH of the solution since we are given the pH:

pH + pOH = 14

pOH = 14 - 11.48 = 2.52

Next, we can use the relationship between the ionization constant (Kb) and the concentration of hydroxide ions ([OH-]):

Kb = [OH-]^2 / [base]

To find [OH-], we can use the fact that:

pOH = -log[OH-]

[OH-] = 10^-pOH

[OH-] = 10^-2.52 = 2.17 x 10^-3

Substituting into the Kb expression:

Kb = (2.17 x 10^-3)^2 / 0.214

Kb = 4.32 x 10^-5

Therefore, the answer is (B).

A 0214 M Aqueous Solution of a Monoprotic Base Has a a PH