Calcium hydroxide is a strong base. Compute [Ca²⁺] and [OH^–] for a solution that is prepared by dissolving 0.60 g of Ca[OH]₂ in enough water to make a 1500 mL of solution [Atomic weights : Ca = 40, O = 16, H = 1]

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8.1×10^–3, 8.1×10^–3

5.4×10^–3, 5.4×10^–3

5.4×10^–3, 1.08×10^–2

5.4×10^–3, 9.1×10^–13

answer is B.

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Detailed Solution

$[Ca (OH)_{2}] = \frac{0.6}{74 \times 1.5} = [{Ca}^{+ 2}] = 5.4 \times 10^{- 3}$

$[{OH}^{-}] = \frac{2 \times 0.60}{74 \times 1.5} = 1.08 \times 10^{- 2}$

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