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: (c) Adding NO₃, which reacts with Ag⁺ to form the complex ion Ag(NH₃)₂⁺

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Identify the initial equilibrium reaction: Ag^+ (aq) + Cl^- (aq) ⇌ AgCl(s).

Recognize that adding NO_3^- will not directly affect the equilibrium, but the formation of Ag(NH_3)_2^+ from Ag^+ and NH_3 will.

Understand that the formation of Ag(NH_3)_2^+ reduces the concentration of free Ag^+ ions in the solution.

Apply Le Châtelier's principle: the system will shift to counteract the change, meaning it will shift to the left to produce more Ag^+ ions.

Conclude that as the equilibrium shifts to the left, the amount of solid AgCl will decrease as it dissolves to release more Ag^+ ions.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Le Châtelier's Principle

Le Châtelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change. This means that if a reactant or product concentration is altered, the system will adjust to restore equilibrium, either by favoring the forward or reverse reaction.

Equilibrium Constant

The equilibrium constant (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. For the reaction Ag+ + Cl- ⇌ AgCl, the equilibrium constant expression is K = [AgCl]/([Ag+][Cl-]). Changes in concentration of reactants or products will affect the value of K and the position of equilibrium.

Complex Ion Formation

Complex ion formation occurs when a metal ion binds with one or more ligands, resulting in a new species. In this case, the addition of NO3 leads to the formation of the complex ion Ag(NH3)2+, which decreases the concentration of free Ag+ ions in solution. This shift in concentration affects the equilibrium position, potentially increasing the amount of solid AgCl formed.

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Textbook Question

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: (a) Adding NaCl (b) Adding AgNO₃

Textbook Question

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

Textbook Question

For the water–gas shift reaction CO1g2 + H2O1g2 ∆ CO21g2 + H21g2, ΔH° = - 41.2 kJ does the amount of H2 in an equilibrium mixture increase or decrease when the temperature is increased? How does Kc change when the temperature is decreased? Justify your answers using Le Châtelier's principle.

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: (c) Adding NO3, which reacts with Ag+ to form the complex ion Ag(NH3)2+

Verified video answer for a similar problem:

Key Concepts

Le Châtelier's Principle

Equilibrium Constant

Complex Ion Formation

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: (c) Adding NO₃, which reacts with Ag⁺ to form the complex ion Ag(NH₃)₂⁺