A solution is 0.1 M in $\mathrm{Cl}^{-}$and 0.001 M in $\mathrm{CrO}_4^{-2}$.
Solid $\mathrm{AgNO}_3$ is gradually added to it
Assuming that the addition does not change in volume and $\mathrm{K}_{\mathrm{se}}(\mathrm{AgCl})=1.7 \times 10^{-10} \mathrm{M}^2$ and $\mathrm{Ksp}\left(\mathrm{Ag}_2 \mathrm{CrO}_4\right)=1.9 \times 10^{-12} \mathrm{M}^3$.
Select correct statement from the following:
Select the correct option:
A
AgCl precipitates first because its Ksp is high.
B
$\mathrm{Ag}_2 \mathrm{CrO}_4$ precipitates first as its Ksp is low.
C
$\mathrm{Ag}_2 \mathrm{CrO}_4$ precipitates first because the amount of $\mathrm{Ag}^{+}$needed is low.
D
AgCl will precipitate first as the amount of Ag+ needed to precipitate is low.
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