Use Le Châtelier's Principle to predict how this equilibrium system will respond to the changes you will make: CH3COOH (aq) LaTeX: / Leftrightarrow⇔ CH3COO - (aq) + H + (aq) How will adding sodium acetate (CH3COONa) initially change the concentrations of CH3COOH, CH3COO-, and H+? How will the equilibrium system respond to this change?

Question

Chemistry

Cory Bailey

13 March, 16:30

Use Le Châtelier's Principle to predict how this equilibrium system will respond to the changes you will make: CH3COOH (aq) LaTeX: / Leftrightarrow⇔ CH3COO - (aq) + H + (aq) How will adding sodium acetate (CH3COONa) initially change the concentrations of CH3COOH, CH3COO-, and H+? How will the equilibrium system respond to this change?

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Answers (1)

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Emilee Chen · Answer 1

Answer: The equilibrium will shift to the left.

Explanation:

If sodium acetate is added to acetic acid, the dissociation of the acetic acid is suppressed. The equilibrium position shifts to the left and the hydrogen ion concentration decreases due to decreased ionization of the acid. This common ion solution becomes less acidic than pure acetic acid.

This is so because of common ion effect. The acetate ion already present from the dissociation of acetic acid is also present in the sodium acetate. The presence of a common ion usually shifts the equilibrium position towards the left.

NaCH3CO2 (s) → Na + (aq) + CH3CO2 - (aq)

CH3CO2H (aq) ⇌ H + (aq) + CH3CO 2 - (aq)