Final answer:
The pH of a 0.2 M acetate buffer can be calculated using the Henderson-Hasselbalch equation. Given a pKa of 4.77 and twice as much acid as conjugate base, the pH is approximately 4.469.
Step-by-step explanation:
To calculate the pH of the acetate buffer, we need to consider the Henderson-Hasselbalch equation:
pH = pKa + log([Base]/[Acid])
Given that the pKa is 4.77 and the buffer contains twice as much acid as conjugate base, we can set up the equation as follows:
pH = 4.77 + log(1/2)
Simplifying, pH = 4.77 - log(2)
Calculating log(2), pH = 4.77 - 0.3010
Therefore, the pH of the acetate buffer is approximately 4.469.