The solubility product of AgCl is 1.8×10−10. Precipitation of AgCl will occur only when equal volumes of solutions of:

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The solubility product of $AgCl$ is $1.8 \times 10^{- 10}$ . Precipitation of $AgCl$ will occur only when equal volumes of solutions of:

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$10^{- 7} M {Ag}^{+}$ and $10^{- 7} {MCl}^{-}$ are mixed

$10^{- 5} M {Ag}^{+}$ and $10^{- 5} {MCl}^{-}$ are mixed

$10^{- 4} M {Ag}^{+}$ and $10^{- 4} {MCl}^{-}$ are mixed

$2 \times 10^{- 5} M {Ag}^{+}$ and $2 \times 10^{- 5} {MCl}^{-}$ are mixed

answer is A.

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Detailed Solution

${ppt}^{n}$ occurs when $k_{i p} > k_{s p}$ . For each option,

$(a) [k_{i p} = \frac{10^{- 8}}{4} > k_{s p}]$

$(b) [k_{i p} = \frac{10^{- 14}}{4} < k_{s p}]$

$(c) [k_{i p} = \frac{10^{- 10}}{4} < k_{s p}]$

$(d) [k_{i p} = 10^{- 10} < k_{s p}]$

Thus, precipitation of $AgCl$ will occur only when equal volumes of solutions of $10^{- 4} M {Ag}^{+}$ and $10^{- 4} {MCl}^{-}$ are mixed.

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