Find out the solubility of $M g (O H)_{2}$ in $0.1 M N a O H$ solution.
[Given that the solubility product of $M g (O H)_{2}$ is $1.8 \times 10^{- 11}$ ]

Q. The sparingly soluble salt

S r F_{2}

has a

K_{s p}

value of

2.45 \times 10^{- 9}

at room temperature. Calculate its solubility in

0.1 M

highly soluble

N a F

aqueous solution.

Q. If the solubility of

M g {(O H)}_{2}

in water is

1.4 \times 10^{- x}

K_{s p} = 1.2 \times 10^{- 11}

. Find out the value of

x

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Let the solubility of an aqueous solution of Mg(OH)2 is x then its Ksp is __________.

The correct option is A 4x3The solubility of Mg(OH)2 is x.The dissociation equilibrium is as given below.Mg(OH)2x⇌Mg2+x+2OH−2x.The expression for the solubility product is Ksp=[Mg2+][OH−]2Substitute values in the above expression.Ksp=x(2x)2=4x3.Option A is correct.

Let the solubility of an aqueous solution of $M g (O H)_{2}$ is x then its $K_{s p}$ is __________.