In which direction will the following equilibrium shift when solid sodium fluoride is added to an aqueous solution of acetic acid? CH3COOH â CH3COOâ + H+ A. The equilibrium shifts to the right, to form more products. B. The equilibrium shifts to the left, to form more reactants. C. There is no change; the system is still at equilibrium.

A. The equilibrium shifts to the right, to form more products.

Explanation:

When sodium fluoride, NaF, is added to an aqueous solution, some HF is produced:

NaF + H₂O ⇄ OH⁻ + Na⁺ + HF.

That is, some H⁺ reacts decreasing its concentration.

Now, the equilibrium of the acetic acid is:

CH3COOH ⇄ CH3COO⁻ + H⁺

As the concentration of H⁺ decreases:

A. The equilibrium shifts to the right, to form more products.

In order to restore the initial equilibrium.

im pretty sure its b