Exhibit 16-1 The following question(s) refer to the same titration: a 50.00 mL sample of 0.0950 M acetic acid (K_a = 1.8 × 10^-5) is being titrated with 0.106 M NaOH.
Refer to Exhibit 16-1. What is the pH at the midpoint of the titration?

Question

Quizplus · Accepted Answer

At the midpoint of a titration of a weak acid with a strong base, the concentration of the acid equals the concentration of its conjugate base. The pH at this point is equal to the pKa of the acid. The pKa can be calculated using the formula pKa = -log(Ka), where Ka for acetic acid is given as 1.8 × 10^-5. Therefore, pKa = -log(1.8 × 10^-5) = 4.74.

Exhibit 16-1 the Following Question(s) Refer to the Same Titration