Question

To the equilibrium reaction shown$:$
$AgCl\left(s\right)\rightleftharpoons A{g}^{+}+C{l}^{-}$
What will happen if concentrated $HCl\left(12M\right)$ is slowly added?

• A. More salt will go into solution, and the $K_{sp}$ will remain the same
• B. More salt will go into solution, and the $K_{sp}$ will increase
• C. Salt will come out of the solution, and the $K_{sp}$ will remain the same
• D. Salt will come out of the solution, and the $K_{sp}$ will decrease
• E. No change in concentration will occur, and the $K_{sp}$ will increase

Answer 1

The correct option is C Salt will come out of the solution, and the $K_{sp}$ will remain the same

Due to excess ${Cl}^{-}$ from $HCl$ (12M) common ion effect reverses ${eqb}^m$ to backward so no salt will be dissolved further and since $K_{SP}$ only depend on temperature ($\because$ it is an ${eqb}^m$ constant) it will be constant.