The solubility of a sparingly soluble salt $A_{x} B_{y}$ in water is $S$ moles per litre. The solubility product has the value:

S^{2}

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x^{y} y^{x} . S^{x + y}

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x^{x} y^{y} S^{x + y}

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S^{x + y}

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Solution

The correct option is C $x^{x} y^{y} S^{x + y}$
When S represents the molar solubility of $A_{x} B_{y}$ , the molar solubilities of the ions $A^{y +}$ and $B^{x -}$ will be xS and yS respectively.
The expression for the solubility product will be $K_{s p} = [A^{y +}]^{x} [B^{x -}]^{y} = (x S)^{x} (y S)^{y} = x^{x} y^{y} S^{x + y}$

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