What is the pH of a 0.020 M Ba(OH)₂ solution? A)1.40 B)1.70 C)12.30 D)12.60

Question

Quizplus · Accepted Answer

Ba(OH)2 completely dissociates in water to form Ba2+ and OH- ions. Hence, the hydroxide ion concentration will be twice the molarity of the Ba(OH)2 solution.

[OH-] = 2 x 0.020 M = 0.040 M

pOH = -log[OH-] = -log(0.040) = 1.40

pH + pOH = 14

pH = 14 - pOH = 14 - 1.40 = 12.60

Therefore, the pH of the solution is 12.60, which corresponds to option D.

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