A litre of solution is saturated with AgCl. T | vedclass

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

Question

(B) The solubility equilibrium of $AgCl$ is given by: $AgCl(s) \rightleftharpoons Ag^{+}(aq) + Cl^{-}(aq)$.According to the solubility product constan

Vedclass · Accepted Answer

Less

Vedclass · Answer

(B) The solubility equilibrium of $AgCl$ is given by: $AgCl(s) ightleftharpoons Ag^{+}(aq) + Cl^{-}(aq)$.According to the solubility product constant expression,$K_{sp} = [Ag^{+}][Cl^{-}]$.When $NaCl$ is added,it dissociates completely: $NaCl(s) 	o Na^{+}(aq) + Cl^{-}(aq)$.This increases the concentration of $Cl^{-}$ ions in the solution.Due to the common ion effect,the equilibrium shifts to the left to maintain the constant value of $K_{sp}$.Consequently,the concentration of $[Ag^{+}]$ decreases compared to its initial value in the saturated solution.

$A$ litre of solution is saturated with $AgCl$. To this solution if $1.0 \times 10^{-4} \ mol$ of solid $NaCl$ is added,what will be the $[Ag^{+}]$ compared to the original concentration,assuming no volume change?

Similar Questions

The solubility of $AgI$ in $NaI$ solution is less than that in pure water because

When $H_2S$ is passed through a solution containing $HCl$ for qualitative analysis,it does not precipitate group $IV$ cations. Why is this?

Calculate the solubility of $AgCl(s)$ in $0.1 \ M \ NaCl$ at $25 \ ^oC$. Given ${K_{sp}}(AgCl) = 2.8 \times 10^{-10}$.

At equilibrium,if $HCl$ gas is passed through a saturated solution of $NaCl$,$NaCl$ gets precipitated because:

The following equilibrium exists in aqueous solution: $CH_3COOH \rightleftharpoons CH_3COO^{-} + H^{+}$. If dilute $HCl$ is added,without change in temperature,the:

Vedclass Test Series

Exam Paper Generator

Online Exam Module