Acetic acid is a weak acid that dissociates into the acetate ion and a proton in aqueous solution: HC₂H₃O₂ (aq) C₂H₃O₂^- (aq) + H⁺ (aq)
At equilibrium at 25 °C a 0.100 M solution of acetic acid has the following concentrations: and The equilibrium constant,K_eq,for the ionization of acetic acid at is ________.

Question

Acetic acid is a weak acid that dissociates into the acetate ion and a proton in aqueous solution: HC₂H₃O₂ (aq)

Acetic acid is a weak acid that dissociates into the acetate ion and a proton in aqueous solution: HC<sub>2</sub>H<sub>3</sub>O<sub>2</sub> (aq) C<sub>2</sub>H<sub>3</sub>O<sub>2</sub><sup>-</sup> (aq) + H<sup>+</sup> (aq) At equilibrium at 25 °C a 0.100 M solution of acetic acid has the following concentrations: and The equilibrium constant,K<sub>eq</sub>,for the ionization of acetic acid at is ________. A) 5.71 × 10<sup>4</sup> B) 0.100 C) 1.75 × 10<sup>-7</sup> D) 1.79 × 10<sup>-5</sup> E) 5.71 × 10<sup>6</sup>

C₂H₃O₂^- (aq) + H⁺ (aq)
At equilibrium at 25 °C a 0.100 M solution of acetic acid has the following concentrations:

and

The equilibrium constant,K_eq,for the ionization of acetic acid at

is ________.

Quizplus · Accepted Answer

The equilibrium expression for the ionization of acetic acid is as follows: K_eq = [C₂H₃O₂^-]/[H⁺][C₂H₃O₂ (aq)] Substituting the given equilibrium concentrations: K_eq = [(0.0472)(0.0472)]/[0.0528] = 1.79 × 10^-5 Therefore, the answer is D, 1.79 × 10^-5.

Acetic Acid Is a Weak Acid That Dissociates into the Acetate