common ion effect

Question

The solubility of AgCl decreases in the presence of:

RankGuru · Accepted Answer

The **Common Ion Effect** states that the addition of an ion already present in the equilibrium mixture will shift the equilibrium away from that ion.
- $AgCl(s) \rightleftharpoons Ag^+(aq) + Cl^-(aq)$
- **$HCl$** provides $H^+$ and $Cl^-$ ions.
- **$NaCl$** provides $Na^+$ and $Cl^-$ ions.
- In both cases, the concentration of $Cl^-$ (a common ion) increases. According to Le Chatelier's principle, the equilibrium shifts to the **left**, causing more $AgCl$ to precipitate.
- Consequently, the solubility of $AgCl$ decreases in both solutions.

Rank Guru

common ion effect

Select the correct option: