At equilibrium,if HCl gas is passed through a | vedclass

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

Question

(C) The dissolution of $NaCl$ is represented as: $NaCl_{(s)} ⇌ Na^+_{(aq)} + Cl^-_{(aq)}$.When $HCl$ gas is passed through the solution,it dissociates

Vedclass · Accepted Answer

Ionic product of $NaCl$ becomes greater than its ${K_{sp}}$

Vedclass · Answer

(C) The dissolution of $NaCl$ is represented as: $NaCl_{(s)} ⇌ Na^+_{(aq)} + Cl^-_{(aq)}$.When $HCl$ gas is passed through the solution,it dissociates as: $HCl_{(g)} ⇌ H^+_{(aq)} + Cl^-_{(aq)}$.This increases the concentration of $Cl^-$ ions in the solution (Common Ion Effect).According to Le Chatelier's principle,the equilibrium shifts to the left,and the ionic product $[Na^+][Cl^-]$ exceeds the solubility product constant ${K_{sp}}$ of $NaCl$,causing precipitation.

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

Similar Questions

On addition of ammonium chloride to a solution of ammonium hydroxide,what happens to the concentration of $OH^{-}$ ions?

The solubility (in $mol \ L^{-1}$) of $AgCl$ $(K_{sp} = 1.0 \times 10^{-10})$ in a $0.1 \ M \ KCl$ solution will be

Which is not an example of common ion effect?

Aqueous ammonia is used instead of an aqueous solution of $NaOH$ to precipitate $Al^{+3}$ ions as $Al(OH)_3$ because:

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

Vedclass Test Series

Exam Paper Generator

Online Exam Module