First slide

Solubility product(KSP)

Question

The $K_{SP} of Mg {(OH)}_{2}$ is $1 \times 10^{- 12} .$ 0.01 M $Mg {(OH)}_{2}$ will precipitate at the limiting pH

Moderate

A

3
B

9
C

5
D

8

Solution

$[{Mg}^{2 +}] {[{OH}^{-}]}^{2} = 10^{- 12} 0.01 \times {[{OH}^{-}]}^{2} = 10^{- 12} [{OH}^{-}] = 10^{- 5} M ∴ [H^{+}] = 10^{- 9} M and pH = - \log [10^{- 9}] = 9$

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