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pH the Power of H

Assumed CaOH2...

Question

Assumed $C a (O H)_{2}$ to be completely ionized the $p H$ of 0.01 M molar aqueous solution of calcium hydroxide is approximately:

10.5

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11.8

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13.7

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12.3

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Solution

The correct option is D 12.3
Since $C a (O H)_{2}$ is a strong base , it will ionize completely. $C a (O H)_{2} (a q .) + H_{2} O ⟶ C a^{2 +} (a q .) + 2 O H^{-} (a q .) I n i t i a l : C 00 E q u i l i b r i u m : 0 C 2 C$
$[O H^{-}]_{e q b} = 2 \times [C a (O H)_{2}]_{i n i t i a l l y} = 2 \times C = 0.02 M p O H = - log [O H^{-}] p O H = - log (0.02) = 2 - 0.3 = 1.7 p H + p O H = 14 p H = 14 - 1.7 = 12.3$

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