The ph of a 1.4m solution of acetic acid (hch3co2) is measured to be 2.30. calculate the acid dissociation constant of acetic acid. round your answer to significant digits.

Ka = 1.8 × 10⁻⁵

Explanation:

Acetic acid is a weak acid that dissociates according to the following equation.

HCH₃CO₂(aq) ⇄ CH₃CO₂⁻(aq) + H⁺(aq)

The concentration of the acid is Ca = 1.4 M.

The pH is 2.30. The concentration of H⁺ is:

pH = -log [H⁺]

[H⁺] = anti log (-pH) = anti log (-2.30) = 5.01 × 10⁻³ M

We can find the acid dissociation constant (Ka) using the following expression.

[H⁺] = √(Ca × Ka)

Ka = [H⁺]²/Ca

Ka = (5.01 × 10⁻³)²/1.4

Ka = 1.8 × 10⁻⁵

explanation: it gains negative electrons, therefore becoming negatively charged. as charge cannot be created, nor destroyed, only transferred, this leaves the wool positive. now that they have opposite charges, the two items attract.