WBJEE · Chemistry · Ionic Equilibrium
At \(25^{\circ} \mathrm{C}\), the solubility produet of salt of \(\mathrm{MX}_{2}\) type is \(3.2 \times 10^{-8}\) in water. The solubility (in \(\mathrm{mol} / \mathrm{L})\) of \(M X_{2}\) in water at the sume temperature will be
- A \(1.2 \times 10^{-3}\)
- B \(2 \times 10^{-3}\)
- C \(3.2 \times 10^{-3}\)
- D \(1.75 \times 10^{-3}\)
Answer & Solution
Correct Answer
(B) \(2 \times 10^{-3}\)
Step-by-step Solution
Detailed explanation
For \(M X_{2}\) type salt, Solubility product, \(K_{\mathrm{sp}}=4 s^{3} ; 3.2 \times 10^{-8}=4 \mathrm{s}^{3}\) or \(s=\sqrt[3]{\frac{3.2 \times 10^{-8}}{4}}=2 \times 10^{-3} \mathrm{mol} / \mathrm{L}\)
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