The concentration of $KI\ and\ KCl$ in a certain solution containing both is 0.001 M each. If 20 mL of this solution is added to 20 mL of a saturated solution of $AgI$ in water. What will happen? ($K_{sp}\ AgCl = 10^{- 10},\ K_{sp}\ AgI = 10^{- 16}$)

Question

Dr. Abubacker · Accepted Answer

(a)
The saturated solution of $AgI$ means that
$\left\lbrack {Ag}^{+} \right\rbrack\left\lbrack I^{-} \right\rbrack = K_{sp}\ AgI$
Hence, in this solution, if a mixture of $KI + KCl$ is added, then the concentration of $\lbrack I^{-}\rbrack$ ions will increase quite a bit in the solution. Hence, now the ionic product of $AgI$ will be more than its solubility product and therefore, $AgI$ will precipitate out.

Q. The concentration of $KI\ and\ KCl$ in a certain solution containing both is 0.001 M each. If 20 mL of this solution is added to 20 mL of a saturated solution of $AgI$ in water. What will happen? ($K_{sp}\ AgCl = 10^{- 10},\ K_{sp}\ AgI = 10^{- 16}$)

Explanation

Reviewed by Dr. Abubacker

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