For the equilibrium reaction involving acetic acid, which can be described by the reaction below, describe the effect of adding a strong base to the solution, adding more acetic acid to the solution, and adding more water to the solution.

Question

For the equilibrium reaction involving acetic acid, which can be described by the reaction below, describe the effect of adding a strong base to the solution, adding more acetic acid to the solution, and adding more water to the solution.

CH3COOH(aq) + H2O(l) ↔ CH3COO-(aq) + H3O+(aq)

Answer 1

Adding a strong base to the solution will shift the equilibrium to the left, decreasing the concentration of CH3COO- and H3O+.

Adding more acetic acid to the solution will shift the equilibrium to the right, increasing the concentration of CH3COO- and H3O+.

Adding more water to the solution will have no effect on the equilibrium since water is a product of the reaction.