The solubility of AgCl will be maximum in:

0.01 M C a C l_{2}

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pure water

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0.001 M A g N O_{3}

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0.01 M N a C l

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Solution

The correct option is B pure water
When a soluble compound with a common ion to the precipitate is added, the solubility of ppt. decreases this effect is Known as Common Ion Effect.
All the options will perform Common Ion Effect with $A g C l$ , thus, decreasing its solubility except for pure water which is a weak electrolyte.

Hence, $A g C l$ will be maximum soluble in Pure water.

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A g C l

E_{A g / A g +}^{0} = - 0.799 V

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The Solubility $s$ of $A g C l (s)$ in pure water and in $0.1 M$ $N a C l$ at $25^{\circ} C$ respectively are:

$K_{s p} (A g C l)$ = $2.8 \times 10^{- 10}$

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