In the equilibrium reactionAgCl_{(s)} + 2NH_3 | vedclass

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(B) According to Le Chatelier's principle,if the concentration of a product in an equilibrium reaction is increased,the equilibrium shifts in the dire

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$AgCl_{(s)}$ to precipitate

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(B) According to Le Chatelier's principle,if the concentration of a product in an equilibrium reaction is increased,the equilibrium shifts in the direction that consumes the added substance.In the reaction $AgCl_{(s)} + 2NH_3(aq.) \rightleftharpoons [Ag(NH_3)_2]^+ (aq.) + Cl^{-} (aq.)$,increasing the concentration of $Cl^{-} (aq.)$ (a product) will cause the reaction to shift to the left.This shift to the left results in the formation of more reactants,specifically causing $AgCl_{(s)}$ to precipitate.

In the equilibrium reaction
$AgCl_{(s)} + 2NH_3(aq.) \rightleftharpoons [Ag(NH_3)_2]^+ (aq.) + Cl^{-} (aq.)$
Increase in the concentration of $Cl^{-} (aq.)$ causes

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In the equilibrium reaction$AgCl_{(s)} + 2NH_3(aq.) \rightleftharpoons [Ag(NH_3)_2]^+ (aq.) + Cl^{-} (aq.)$Increase in the concentration of $Cl^{-} (aq.)$ causes