To answer this question, we need to consider the effect of adding [tex]\( AgNO_3 \)[/tex] on the given chemical equilibrium:
[tex]\[ AgCl (s) \Leftrightarrow Ag^{+} (aq) + Cl^{-} (aq) \][/tex]
1. Understand the Addition of [tex]\( AgNO_3 \)[/tex]:
- When [tex]\( AgNO_3 \)[/tex] is added to the solution, it dissociates completely in water into [tex]\( Ag^+ \)[/tex] and [tex]\( NO_3^- \)[/tex] ions:
[tex]\[ AgNO_3 (aq) \rightarrow Ag^+ (aq) + NO_3^- (aq) \][/tex]
2. Effect on the Equilibrium:
- The addition of [tex]\( AgNO_3 \)[/tex] increases the concentration of [tex]\( Ag^+ \)[/tex] ions in the solution.
- According to Le Chatelier's principle, if the concentration of one of the products is increased, the system will shift the equilibrium position to counteract this change, thus shifting the equilibrium towards the reactants to reduce the excess [tex]\( Ag^+ \)[/tex] ions.
3. Shift in Equilibrium:
- To counteract the increased [tex]\( Ag^+ \)[/tex] ion concentration, the equilibrium will shift to the left, favoring the formation of [tex]\( AgCl \)[/tex] (s) and reducing the concentration of [tex]\( Ag^+ \)[/tex] ions in the solution.
Based on this understanding, the correct outcome is that:
The chemical equilibrium of the system shifts to the left.
