Question

consider the chemical equilibrium of the reaction
agcl(s) ⇌ ag⁺(aq) + cl⁻(aq)
what will happen to the chemical equilibrium if agno₃ is added?
there is no shift in the chemical equilibrium of the system.
the chemical equilibrium of the system shifts to the right.
the chemical equilibrium of the system shifts to the left.
the chemical equilibrium of the system is destroyed.

Explanation:

1. First, analyze the reaction and the added substance: The given reaction is $\ce{AgCl(s)

ightleftharpoons Ag^{+}(aq) + Cl^{-}(aq)}$. When $\ce{AgNO_{3}}$ is added, $\ce{AgNO_{3}}$ dissociates in solution as $\ce{AgNO_{3}(aq) -> Ag^{+}(aq) + NO_{3}^{-}(aq)}$, which increases the concentration of $\ce{Ag^{+}}$ ions in the solution.

1. Then, apply Le Chatelier's principle: Le Chatelier's principle states that if a stress is applied to a system at equilibrium, the system will shift in a direction that relieves the stress. In this case, the increase in the concentration of $\ce{Ag^{+}}$ (a product of the dissociation of $\ce{AgCl}$) is a stress on the equilibrium. To relieve this stress, the system will shift in the direction that consumes the excess $\ce{Ag^{+}}$ ions.
2. Finally, determine the direction of the shift: The reverse reaction of the dissociation of $\ce{AgCl}$ (i.e., $\ce{Ag^{+}(aq) + Cl^{-}(aq) -> AgCl(s)}$) consumes $\ce{Ag^{+}}$ ions. So, the equilibrium will shift to the left (towards the reactant, $\ce{AgCl(s)}$) to reduce the increased concentration of $\ce{Ag^{+}}$ ions. Also, chemical equilibrium is a dynamic state and is not destroyed by the addition of a substance; it just shifts to re - establish equilibrium under the new conditions. And since the concentration of a product is increased, the equilibrium cannot shift to the right (which would produce more products) or remain unchanged.

Answer:

The chemical equilibrium of the system shifts to the left.