The solubility product of magnesium hydroxide | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(A) For $Mg(OH)_2 \rightleftharpoons Mg^{2+} + 2OH^-$,the solubility product $K_{sp} = [Mg^{2+}][OH^-]^2 = (s)(2s)^2 = 4s^3$. In pure water: $4s^3 = 1

Vedclass · Accepted Answer

$1.44 	imes 10^{-4} \ M, 4.8 	imes 10^{-9} \ M$

Vedclass · Answer

(A) For $Mg(OH)_2 ightleftharpoons Mg^{2+} + 2OH^-$,the solubility product $K_{sp} = [Mg^{2+}][OH^-]^2 = (s)(2s)^2 = 4s^3$. In pure water: $4s^3 = 1.2 	imes 10^{-11} \implies s^3 = 0.3 	imes 10^{-11} = 3.0 	imes 10^{-12} \implies s = \sqrt[3]{3.0} 	imes 10^{-4} \approx 1.44 	imes 10^{-4} \ M$. In $0.05 \ M$ $NaOH$,$[OH^-] \approx 0.05 \ M$. $K_{sp} = [Mg^{2+}][OH^-]^2 \implies 1.2 	imes 10^{-11} = s(0.05)^2 \implies s = \frac{1.2 	imes 10^{-11}}{2.5 	imes 10^{-3}} = 4.8 	imes 10^{-9} \ M$.

The solubility product of magnesium hydroxide $Mg(OH)_2$ is $1.2 \times 10^{-11}$. Calculate its solubility in pure water and $0.05 \ M$ $NaOH$.

Similar Questions

Sodium sulfate is soluble in water,whereas barium sulfate is sparingly soluble. Why?

Which of the following pairs of ions would be expected to form a precipitate when their dilute solutions are mixed?

What mass of $AgI$ will dissolve in $1.0 \ L$ of its saturated solution? [Given $: K_{sp}(AgI) = 1.0 \times 10^{-16} ; (At. \ wt. \ Ag = 108; I = 127)$]

At $298 \ K$,the solubility of silver chloride in water is $1.434 \times 10^{-3} \ g \ L^{-1}$. The value of $-\log K_{sp}$ for silver chloride is $........$ (Given: molar mass of $Ag = 107.9 \ g \ mol^{-1}$ and $Cl = 35.5 \ g \ mol^{-1}$)

Solubility of an $MX_2$ type electrolyte is $0.5 \times 10^{-4} \ mol/L$,then $K_{sp}$ of electrolyte is

Vedclass Test Series

Exam Paper Generator

Online Exam Module