Consider the following equilibrium: Ag⁺(aq) + Cl^-(aq) ⇌ AgCl(s) Use Le Châtelier's principle to predict how the amount of solid silver chloride will change when the equilibrium is disturbed by: (d) Removing Cl^-; also account for the change using the reaction quotient Q_c

Verified step by step guidance

1. Identify the initial equilibrium condition for the reaction: Ag^+(aq) + Cl^-(aq) ⇌ AgCl(s).
2. Understand that removing Cl^- from the system will disturb the equilibrium.
3. Apply Le Châtelier's principle: The system will shift to counteract the disturbance, which means it will shift to the right to produce more Cl^- ions.
4. Recognize that as the equilibrium shifts to the right, more AgCl(s) will form, increasing the amount of solid silver chloride.
5. Use the reaction quotient Q_c to confirm the shift: Q_c = [Ag^+][Cl^-]. Removing Cl^- decreases Q_c, making it less than K_c, thus the reaction shifts right to restore equilibrium.

Key Concepts

Le Châtelier's Principle

Le Châtelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust to counteract the change and restore a new equilibrium. This can involve changes in concentration, pressure, or temperature. In the context of the given equilibrium, removing Cl^- ions will shift the equilibrium to the left, favoring the formation of more reactants to compensate for the loss.

Equilibrium Constant (K)

The equilibrium constant (K) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. For the reaction Ag⁺(aq) + Cl^-(aq) ⇌ AgCl(s), K is defined in terms of the concentrations of Ag⁺ and Cl^-. Changes in concentration of reactants or products will affect the position of equilibrium but not the value of K itself.

Reaction Quotient (Q_c)

The reaction quotient (Q_c) is calculated using the same formula as the equilibrium constant but with the current concentrations of the reactants and products, regardless of whether the system is at equilibrium. By comparing Q_c to K, one can determine the direction in which the reaction will shift to reach equilibrium. If Q_c is less than K, the reaction will shift to the right, while if Q_c is greater than K, it will shift to the left.