Let the solubility of an aqueous solution of | vedclass

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(A) The dissociation of $Mg(OH)_2$ in an aqueous solution is represented as: $Mg(OH)_2(s) \rightleftharpoons Mg^{2+}(aq) + 2OH^-(aq)$ If the solubilit

Vedclass · Accepted Answer

$4x^3$

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(A) The dissociation of $Mg(OH)_2$ in an aqueous solution is represented as: $Mg(OH)_2(s) \rightleftharpoons Mg^{2+}(aq) + 2OH^-(aq)$ If the solubility is $x$,then the concentration of ions at equilibrium will be: $[Mg^{2+}] = x$ $[OH^-] = 2x$ The solubility product constant $K_{sp}$ is given by: $K_{sp} = [Mg^{2+}][OH^-]^2$ Substituting the values: $K_{sp} = (x)(2x)^2 = (x)(4x^2) = 4x^3$ Therefore,the correct option is $A$.

Let the solubility of an aqueous solution of $Mg(OH)_2$ be $x$,then its $K_{sp}$ is:

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