A buffer solution with a pH of 4.31 is prepared with and The Ka of H is A)0.37 B)0.74 C)4.2 × 10^-6 D)8.8 × 10^-10 E)0.18

Question

Quizplus · Accepted Answer

To calculate the pH of a buffer solution, we can use the Henderson-Hasselbalch equation:
pH = pKa + log([base]/[acid])
where [base] is the concentration of the basic component (in this case, the acetate ion), and [acid] is the concentration of the acidic component (in this case, acetic acid).
We are given the pH (4.31) and the pKa (4.76) of the buffer, so we can rearrange the Henderson-Hasselbalch equation to solve for the ratio of [base]/[acid]:
4.31 = 4.76 + log([base]/[acid])
-0.45 = log([base]/[acid])
Antilog[-0.45] = [base]/[acid]
0.37 = [base]/[acid]
Therefore, the concentration of the acetate ion (the basic component) is 0.37 times the concentration of acetic acid (the acidic component).

A Buffer Solution with a PH of 4