K_sp of Mg(OH)2 is 1.2 x 10^-11. Its solubility in pure water (ignoring OH^- from water) in mol L^-1 is

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$K_{s p}$ of $Mg (OH) X_{2}$ is $1.2 \times 1 0^{- 11}$ . Its solubility in pure water (ignoring $OH X^{-}$ from water) in $mol L^{- 1}$ is

K_{s p} = 4 s^{3}

, so

s = (K_{s p} /4)^{1/3} = (3.0 \times 1 0^{- 12})^{1/3} = 1.4 \times 1 0^{- 4} M