JEE Mains · Chemistry · STD 11 - 6.2. Equilibrium - II (icon Equilibrium)
If the solubility product of \(AB _{2}\) is \(3.20 \times 10^{-11}\, M ^{3}\), then the solubility of \(AB _{2}\) in pure water is......... \(\times 10^{-4}\) \(mol\) \(L ^{-1}\). [Assuming that neither kind of ion reacts with water]
- A \(8\)
- B \(4\)
- C \(2\)
- D \(10\)
Answer & Solution
Correct Answer
(C) \(2\)
Step-by-step Solution
Detailed explanation
\(\begin{array}{*{20}{c}} {A{B_2}\left( S \right) \rightleftharpoons A_{\left( {aq.} \right)}^{ + 2} + 2B_{\left( {aq.} \right)}^ - \,:\,{K_{sp}}} \\ {\,\,\,\,\,\,\,\,\,\,S\,\,\,\,\,\,\,\,\,\,\,\,2s} \end{array}\) \(K _{ SP }= S ^{1} \times(2 s )^{2}=4 s ^{3}\)…
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