What is the pH of a 0.035 M aqueous solution of barium hydroxide?

Question

Quizplus · Accepted Answer

Barium hydroxide, Ba(OH)2, is a strong base and completely dissociates in water to give Ba2+ and two OH- ions. The concentration of OH- ions in a 0.035 M solution of Ba(OH)2 can be calculated as follows:

[OH-] = 2 × 0.035 mol/L = 0.070 mol/L

The pOH of the solution is:

pOH = -log[OH-] = -log(0.070) = 1.15

The pH of the solution can be calculated using the relation:

pH + pOH = 14

Therefore, pH = 14 - pOH = 14 -1.15 = 12.85

Hence, the answer is A) 12.85.

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