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Statement I : Solubility of AgCl in NH₃(aq) is greater than in pure water.

Statement II : When AgCl dissolve in NH₃(aq), complex ion formation $\large Ag\left( {N{H_3}} \right)_2^ +$ takes place and solubility equilibria of AgCl shifted in forward direction.

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Both statement - I and statement - II are False

Statement I is correct and Statement II is incorrect

Statement I and II are correct

Statement - I is incorrect and Statement II is correct

answer is A.

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Detailed Solution

$\large AgCl\left( s \right) \rightleftharpoons AgCl\left( {aq} \right)\xrightarrow{{}}A{g^ + }\left( {aq} \right) + C{l^ - }\left( {aq} \right)$

In presence of NH₃, Ag⁺(aq) ions are removed due to the formation of soluble complexes via the following complexation reactions.

$\large A{g^ + }\left( {aq} \right) + N{H_3} \rightleftharpoons {\left[ {Ag\left( {N{H_3}} \right)} \right]^ + };{K_1}$

$\large {\left[ {Ag\left( {N{H_3}} \right)} \right]^ + } + N{H_3}\rightleftharpoons\;\left[ {Ag{{\left( {N{H_3}} \right)}_2}} \right]^ + ;{K_2}$

According to Le-chateliar principle when product are removed the equilibrium shifts forward.

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