Question

consider the following chemical reaction in equilibrium.
ch₃cooh ⇌ ch3coo⁻(aq) + h⁺(aq)
what will happen to the chemical equilibrium if mgcl₂ is added?
the chemical equilibrium of the system will be unaffected.
the chemical equilibrium of the system will shift to the right to favor the forward reaction.
the chemical equilibrium of the system will shift to the left to favor the reverse reaction.
the chemical equilibrium of the system will be damaged irreversibly.

Explanation:

1. Analyze the ions from \(MgCl_2\): When \(MgCl_2\) dissolves in water, it dissociates into \(Mg^{2 +}(aq)\) and \(Cl^-(aq)\) (\(MgCl_2(aq)

ightarrow Mg^{2+}(aq)+2Cl^-(aq)\)).

1. Check interaction with equilibrium species: The equilibrium reaction is \(CH_3COOH

ightleftharpoons CH_3COO^-(aq)+H^+(aq)\). The ions \(Mg^{2+}\) and \(Cl^-\) from \(MgCl_2\) do not react with \(CH_3COOH\), \(CH_3COO^-\), or \(H^+\) in a way that would change the concentrations of the species involved in the acetic acid dissociation equilibrium. According to Le Chatelier's principle, a change in equilibrium occurs when the concentration of reactants or products (or other factors like pressure, temperature for gas - phase reactions) changes. Since \(MgCl_2\) addition does not alter the concentrations of \(CH_3COOH\), \(CH_3COO^-\), or \(H^+\) (as it doesn't react with them), the equilibrium remains unaffected. Also, chemical equilibria are dynamic and can adjust, and there's no irreversible damage as equilibria can be re - established under different conditions. And since there's no change in the concentrations of the species in the acetic acid equilibrium, the equilibrium does not shift left or right.

Answer:

The chemical equilibrium of the system will be unaffected.