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6-2.Equilibrium-II (Ionic Equilibrium)
medium
If the solubility product ${K_{sp}}$ of a sparingly soluble salt $M{X_2}$ at $25\,^oC$ is $1.0 \times {10^{ - 11}}$, the solubility of the salt in mole litre$^{-1}$ at this temperature will be
A
$2.46 \times {10^{14}}$
B
$1.36 \times {10^{ - 4}}$
C
$2.60 \times {10^{ - 7}}$
D
$1.20 \times {10^{ - 10}}$
Solution
(b) $M{X_2}⇌ \mathop {{M^ + }}\limits_{(S)\,\,\,} + \mathop {2{X^ – }}\limits_{{{(2S)}^2}\,\,} $;
${K_{sp}} = 4{S^3}$
$S = \sqrt[3]{{\frac{{{K_{sp}}}}{4}}} = \sqrt[3]{{\frac{{1 \times {{10}^{ – 11}}}}{4}}} = 1.35 \times {10^{ – 4}}$
Standard 11
Chemistry
