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The volume of water required to dissolve 0.1 g PbCl$_2$ to get a saturated solution (in mL) is (Given K$_{sp}$(PbCl$_2$) = $3.2 \times 10^{-8}$; Atomic mass of Pb = 207u)

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For a sparingly soluble salt of type $A_x B_y$, the relationship between $K_{sp}$ and molar solubility (s) is $K_{sp} = (xs)^x (ys)^y = x^x y^y s^{x+y}$. For PbCl$_2$, it's type $AB_2$ (x=1, y=2), which gives $K_{sp} = 1^1 2^2 s^{1+2} = 4s^3$.

Updated On: Mar 30, 2026

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The Correct Option is D

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The volume of water required to dissolve 0.1 g PbCl\(_2\) to get a saturated solution (in mL) is (Given K\(_{sp}\)(PbCl\(_2\)) = \(3.2 \times 10^{-8}\); Atomic mass of Pb = 207u)

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The Correct Option is D

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