Increasing order of solubility of AgCl in (i) | vedclass

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(A) The solubility of a sparingly soluble salt like $AgCl$ is affected by the common ion effect and the salt effect.$1$. In $H_2O$, the solubility is

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$CaCl_2 < NaCl < H_2O < NaNO_3$

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(A) The solubility of a sparingly soluble salt like $AgCl$ is affected by the common ion effect and the salt effect.$1$. In $H_2O$, the solubility is $S = \sqrt{K_{sp}}$.$2$. In $1 \ M \ NaCl$ and $1 \ M \ CaCl_2$, the common ion $Cl^-$ is present. Since $CaCl_2$ provides $2 \ M \ Cl^-$ ions and $NaCl$ provides $1 \ M \ Cl^-$ ions, the solubility is lowest in $CaCl_2$ due to the strongest common ion effect.$3$. In $1 \ M \ NaNO_3$, the solubility is slightly higher than in pure water due to the salt effect (or diverse ion effect), which increases the ionic strength of the solution.$4$. Therefore, the order of increasing solubility is: $CaCl_2 < NaCl < H_2O < NaNO_3$.

Increasing order of solubility of $AgCl$ in $(i) H_2O$, $(ii) 1 \ M \ NaCl \ (aq.)$, $(iii) 1 \ M \ CaCl_2 \ (aq.)$ and $(iv) 1 \ M \ NaNO_3 \ (aq.)$ solution.

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