A) \[4\times {{10}^{-2}}\]
B) \[4\times {{10}^{-3}}\]
C) \[0.4\times {{10}^{-2}}\]
D) \[0.4\times {{10}^{-3}}\]
Correct Answer: A
Solution :
Key Idea: Let solubility of \[A{{g}_{2}}S=x\,g/L\] \[\underset{Concentration}{\mathop{A{{g}_{2}}S}}\,\,\,\xrightarrow{{}}\underset{2x}{\mathop{A{{g}^{+}}}}\,+\underset{x}{\mathop{{{S}^{2}}}}\,\] \[{{K}_{sp}}={{[A{{g}^{+}}]}^{2}}[{{S}^{2-}}]\] \[={{(2x)}^{2}}(x)\] \[=4{{x}^{3}}\] Given, \[{{K}_{sp}}=256\times {{10}^{-6}}\] \[\therefore \] \[256\times {{10}^{-6}}=4{{x}^{3}}\] or \[x=\sqrt[3]{\frac{25\times {{10}^{-6}}}{4}}\] \[=4\times {{10}^{-2}}\]
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