Question

ways in which the equilibrium concentration of $A{g}^{+}$ can be reduced in a solution of $N{a}^{+}$, $C{l}^{-}$, $A{g}^{+}$ and $N{O}_3^{-}$, in contact with solid $AgCl.$
$N{a}^{+}\left(aq\right)+C{l}^{-}\left(aq\right)+A{g}^{+}\left(aq\right)+N{O}_3^{-}\left(aq\right)\rightleftharpoons AgCl\left(s\right)+N{a}^{+}\left(aq\right)+N{O}_3^{-}\left(aq\right)\Delta H=-65.9kJ$

• A. Add $NaCl$ or some other salt that produces $C{l}^{-}$ in the solution.
• B. Cool the solution.
• C. Heat the solution
• D. Add HCL

Answer 1

Answer: (A), (B)

The correct options are
A Add $NaCl$ or some other salt that produces $C{l}^{-}$ in the solution.
B Cool the solution.

the equilibrium concentration of $A{g}^{+}$ can be reduced in a solution of $N{a}^{+}$, $C{l}^{-}$, $A{g}^{+}$ and $N{O}_3^{-}$, in contact with solid $AgCl.$ by the following methods.
(A) Add $NaCl$ or some other salt that produces $C{l}^{-}$ in the solution. Since, the chloride ion concentration increases, the equilibrium $A{g}^{+}+C{l}^{-}\rightleftharpoons AgCl\downarrow$ will shift to the rise and the $A{g}^{+}$ ion concentration will decrease.
(B) Cool the solution. The solubility of AgCl (and hence, $\left[A{g}^{+}\right]$) will decrease.