Question

Consider the following equilibrium, $AgCl\downarrow +2N{H}_3\rightleftharpoons \left[Ag\right(N{H}_3{)}_2{]}^{+}+C{l}^{-}$
White precipitate of $AgCl$ appears on adding which of following?

• A. $N{H}_3$
• B. Aqueous $HN{O}_3$
• C. Aqueous $N{H}_{4}Cl$
• D. Aqueous $NaCl$

Answer 1

The correct option is C Aqueous $N{H}_{4}Cl$

$AgCl\downarrow +2N{H}_3\rightleftharpoons \left[Ag\right(N{H}_3{)}_2{]}^{+}+C{l}^{-}$
On adding $N{H}_{4}Cl$ it gives $N{H}_4^{+}$ and $C{l}^{-}$ ions and according to Le-Chatelier's principle, the reaction will shift to left side. When the reaction shifts to left side white precipitate of $AgCl$ appears.