A 100.0-mL sample of 0.2 M (CH₃)₃N (K_b = 5.3 * 10^-⁵) is titrated with 0.2 M HCl. What is the pH at the equivalence point?

Question

Quizplus · Accepted Answer

At the equivalence point, the solution contains the conjugate acid of (CH₃)₃N, which is (CH₃)₃NH⁺. The pH is determined by the hydrolysis of this ion. Using the Kb of (CH₃)₃N, we can find the Ka of (CH₃)₃NH⁺ and calculate the pH, which is approximately 5.4.

A 1000-ML Sample of 0