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

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(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

Vedclass · Accepted Answer

aqueous $HNO_3$

Vedclass · Answer

(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?

Similar Questions

$A$ solution is $0.1 \ M$ with respect to $AcOH$ and $0.2 \ M$ with respect to $AcONa$. What is the concentration of $Ac^-$? (Given $x = 0.2$)

When $NH_4Cl$ is added to $NH_4OH$ solution,the dissociation of $NH_4OH$ is reduced. This is due to:

What concentration of $Ac^{-}$ ions will reduce $H_3O^{+}$ ion concentration to $2 \times 10^{-4} \ M$ in a $0.40 \ M$ solution of $HAc$ (in $M$)? Given $K_a (HAc) = 1.8 \times 10^{-5}$.

Among the following,the correct statement is

Which of the following,when added to a solution of acetic acid,will decrease the concentration of hydrogen ions?

Vedclass Test Series

Exam Paper Generator

Online Exam Module