Question

Suggest two ways in which the equilibrium concentration of Ag+ can be reduced in a solution of Na+, Cl−, Ag+, and NO₃−, in contact with solid AgCl.

Na+(aq)+Cl−(aq)+Ag+(aq)+NO₃−(aq)⇌AgCl(s)+Na+(aq)+NO₃−(aq) ΔH=−65.9kJ

Answer 1

To decrease the Ag+ concentration in solution, adding more Cl- ions will shift equilibrium to form more solid AgCl, and lowering temperature favors product formation, including solid AgCl, thus reducing Ag+ concentration.

Step-by-step explanation:

To reduce the equilibrium concentration of Ag+ in a solution containing Na+, Cl−, Ag+, and NO3− that is in contact with solid AgCl, we can apply Le Chatelier's principle. Here are two ways to achieve this:

1. Add more Cl− ions to the solution. Since chloride ions are a reactant in the equilibrium reaction, AgCl(s) ⇌ Ag+ (aq) + Cl−(aq), adding more Cl− will shift the equilibrium to the left to form more solid AgCl, thus reducing the concentration of Ag+.
2. Lower the temperature of the system. Considering the reaction is exothermic (ΔH = −65.9 kJ), a decrease in temperature will favor the formation of products, including solid AgCl, by shifting the equilibrium to the right, which will decrease the Ag+ concentration in solution.