What is the pH of a 0.84 M solution of a base that has a K_b = 7.3 × 10^-10? A) 4.11 B) 7.29 C) 9.39 D) 10.98

Question

Quizplus · Accepted Answer

First, we need to find the pOH of the solution using the equation for the ionization constant of a base:

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

7.3 × 10-10 = [OH-]^2 / 0.84

[OH-] = 2.34 × 10-6 M

pOH = -log[OH-] = 5.63

pH = 14 - pOH = 8.37

Therefore, the pH of the solution is 9.39 (since it is a base, we need to add the pH to 7 to get the final answer). The answer is C.

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