A saturated solution of ${\rm{Mg}}{\left( {{\rm{OH}}} \right)_2}$ in water at $25^\circ C$ contains $0.11\;{\rm{g}}\;{\rm{Mg}}{\left( {{\rm{OH}}} \right)_2}$ per litre of solution. The solubility product of ${\rm{Mg}}{\left( {{\rm{OH}}} \right)_2}$ is:

JEE CHEMISTRY MCQ: Equilibrium

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Application +4 | -1

A saturated solution of

\mathrm{Mg}{\left( {\mathrm{OH}} \right)_2}

in water at

25^\circ C

contains

0.11\;\mathrm{g}\;\mathrm{Mg}{\left( {\mathrm{OH}} \right)_2}

per litre of solution. The solubility product of

\mathrm{Mg}{\left( {\mathrm{OH}} \right)_2}

is:

View answer and explanation

Correct option: D

4 \times {\left( {0.11} \right)^3}/{\left( {58} \right)^3}

Option D (

4 \times {\left( {0.11} \right)^3}/{\left( {58} \right)^3}

) is correct because it correctly calculates the solubility product using the given solubility and molar mass.

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\mathrm{K}_1

\mathrm{K}_2

\mathrm{N}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})\quad\ldots

\mathrm{NO}(\mathrm{g}) \rightleftharpoons \frac{1}{2} \mathrm{~N}_2(\mathrm{~g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g})\quad\ldots

K{a_1},\,\,\,K{a_2}\,\,\,\mathrm{and}\,\,\,K{a_3}

\begin{array}{l} {H_2}S\leftrightharpoons{H^ + } + H{S^ - }\\ H{S^ - }\leftrightharpoons{H^ + } + {S^{2 - }}\\ {H_2}S\leftrightharpoons2{H^ + } + {S^{2 - }} \end{array}

K{a_1},\,\,K{a_2}\,,K{a_3}

\mathrm{pH}

0.1 \mathrm{~M}-\mathrm{N}_2 \mathrm{H}_4

\mathrm{N}_2 \mathrm{H}_4,

K_{{b}_1}=3.6 \times 10^{-6}, K_{{b}_2}=6.4 \times 10^{-12}, \log 2=0.3

\log 3=0.48

{\text{Ba}}{{\text{O}}_2}(s) \rightleftharpoons {\text{BaO}}(s) + {{\text{O}}_2}(g);\Delta H = - {\text{ve}}.

\text{O}_2