Solubility product of silver sulphide is 3.2 × {10^{ - 11}}. Its solubility at experimental tempera

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6-2.Equilibrium-II (Ionic Equilibrium)

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The solubility product of silver sulphide is $3.2 \times {10^{ - 11}}.$ Its solubility at the experimental temperature is

A

$2 \times {10^{ - 4}}$ moles per litre

B

$6 \times {10^{ - 6}}$ moles per litre

C

$1.2 \times {10^{ - 5}}$ moles per litre

D

$8 \times {10^{ - 4}}$ moles per litre

Solution

(a) $A{g_2}S \rightleftharpoons 2A{g^ + } + {S^{ – \,\, – }}$

${K_{sp}} = 4{S^3}$

$S = \sqrt[3]{{\frac{{{K_{sp}}}}{4}}}$$ = \sqrt[3]{{\frac{{3.2 \times {{10}^{ – 11}}}}{4}}} = 2 \times {10^{ – 6}}$

Standard 11

Chemistry

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