The pH of a weak monoacidic base is 11.2, and its OH– ion concentration is ______.

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The pH of a weak monoacidic base is 11.2, its OH– ion concentration is 1.585 $\times$ 10–3 mol dm–3. Explanation: pOH of the solution is given as: pOH = 14 – pH = 14 – 11.2 = 2.8 pOH = – log10[OH–] log10[OH–] = – pOH = – 2.8 = – 2 – 0.8 – 1 + 1 = – 3 + 0.2 = overline(3).2 [OH–] = antilog overline(3).2 = 1.585 $\times$ 10–3 mol/dm–3

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