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
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Identify the initial equilibrium reaction: Ag+ (aq) + Cl- (aq) ⇌ AgCl(s). This reaction shows the formation of solid silver chloride from its ions in solution.
Understand Le Châtelier's principle: When a system at equilibrium is disturbed, it will adjust to minimize the disturbance and re-establish equilibrium.
For part (a), adding NaCl increases the concentration of Cl- ions in the solution. According to Le Châtelier's principle, the equilibrium will shift to the right to reduce the increased concentration of Cl- ions, resulting in the formation of more AgCl(s).
For part (b), adding AgNO3 increases the concentration of Ag+ ions in the solution. Similarly, the equilibrium will shift to the right to reduce the increased concentration of Ag+ ions, leading to the formation of more AgCl(s).
Conclude that in both scenarios, the addition of either NaCl or AgNO3 will result in an increase in the amount of solid silver chloride, AgCl(s), due to the shift in equilibrium to the right.
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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 system will adjust to counteract the change and restore a new equilibrium. This principle helps predict how the concentrations of reactants and products will shift in response to changes such as concentration, pressure, or temperature.
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. It provides insight into the extent of the reaction and helps determine the direction in which the equilibrium will shift when disturbed.
The common ion effect refers to the decrease in solubility of a salt when a common ion is added to the solution. In the context of the given equilibrium, adding NaCl introduces Cl<sup>-</sup> ions, which shifts the equilibrium to the left, favoring the formation of reactants and reducing the amount of solid AgCl produced.
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