What is the pH of a 0.030 M solution of oxalic acid? K_a for oxalic acid is 5.9 $\times$ 10^-2.

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Quizplus · Accepted Answer

Oxalic acid is a weak acid, so we can use the following equation to calculate the pH:```pH = -log[H+]= -log(K_a * [HA]/[A-])```where K_a is the acid dissociation constant, [HA] is the concentration of the acid, and [A-] is the concentration of the conjugate base.Substituting the given values into the equation, we get:```pH = -log(5.9 * 10^-5 * 0.030/0.030) = 1.66```Therefore, the pH of a 0.030 M solution of oxalic acid is 1.66.

What Is the PH of a 0 ×\times× 10-2

What Is the PH of a 0 $\times$ 10^-2