Consider the following equilibrium: AgCl_{(s) | vedclass

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(C) The given equilibrium is $AgCl_{(s)} + 2NH_{3(aq)} \rightleftharpoons [Ag(NH_3)_2]^+_{(aq)} + Cl^-_{(aq)}$.When $HNO_3$ is added,it reacts with $N

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aqueous $HNO_3$

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(C) The given equilibrium is $AgCl_{(s)} + 2NH_{3(aq)} ightleftharpoons [Ag(NH_3)_2]^+_{(aq)} + Cl^-_{(aq)}$.When $HNO_3$ is added,it reacts with $NH_3$ to form $NH_4^+$ ions: $NH_{3(aq)} + H^+_{(aq)} 	o NH_{4(aq)}^+$.This decreases the concentration of $NH_3$,which shifts the equilibrium to the left according to Le Chatelier's principle.Consequently,the complex ion $[Ag(NH_3)_2]^+$ dissociates,releasing $Ag^+$ ions,which then react with $Cl^-$ ions to precipitate $AgCl_{(s)}$.The overall reaction is: $[Ag(NH_3)_2]^+_{(aq)} + Cl^-_{(aq)} + 2H^+_{(aq)} 	o AgCl_{(s)} + 2NH_{4(aq)}^+$.Thus,adding $HNO_3$ causes the white precipitate of $AgCl$ to reappear.

Consider the following equilibrium: $AgCl_{(s)} + 2NH_{3(aq)} \rightleftharpoons [Ag(NH_3)_2]^+_{(aq)} + Cl^-_{(aq)}$. $A$ white precipitate of $AgCl$ appears on adding which of the following?

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