Question

Acetic acid is a weak acid that dissociates into the acetate ion and a proton in aqueous solution: HC_2H_3O_2 (aq) C_2H_3O_2-(aq) + H+

At equilibrium at a 0.100 M solution of acetic acid has the following concentrations: The equilibrium constant, K, for the ionization of acetic acid at is __________.

A) [HC_2H_3O_2] = 0.0990 M
B) [C_2H_3O_2-] = 1.33 x 10^-3 M
C) [H+] = 1.33 x 10^-3 M.

Answer 1

The correct option is: (c) [H+] = 1.33 x 10^-3 M. The equilibrium constant, K, for the ionization of acetic acid is primarily determined by the concentration of H+ ions acetic acid is related to the concentrations of the reactants and products at equilibrium. In this case, the equation for the ionization of acetic acid.

Step-by-step explanation:

The equilibrium constant, K, for the ionization of acetic acid is related to the concentrations of the reactants and products at equilibrium. In this case, the equation for the ionization of acetic acid is:

CH3COOH(aq) → H+(aq) + CH3COO-(aq)

The equilibrium constant expression is:

K = [H+][CH3COO-] / [CH3COOH]

Based on the given concentrations, the value of K would be option C) [H+] = 1.33 x 10^-3 M.