Final answer:
To determine the pH of the buffer, we need to calculate the concentrations of the CH₃COONa and CH₃COOH components and use the Henderson-Hasselbalch equation. The pH of the buffer is approximately 4.85.
Step-by-step explanation:
A buffer is a solution that resists changes in pH when small amounts of acid or base are added to it. To determine the pH of the buffer, we need to calculate the concentrations of the CH₃COONa and CH₃COOH components.
Given that the solution contains 0.13 mol of CH₃COONa and 0.10 mol of CH₃COOH in 1.0 L of solution, we can calculate the concentrations:
Concentration of CH₃COONa = 0.13 mol / 1.0 L = 0.13 M
Concentration of CH₃COOH = 0.10 mol / 1.0 L = 0.10 M
Next, we can use the Henderson-Hasselbalch equation to calculate the pH:
pH = pKa + log([A-]/[HA])
where pKa is the acid dissociation constant and [A-] and [HA] are the concentrations of the conjugate base and acid, respectively.
In this case, the pKa of CH₃COOH is 4.74 (given in the example). Plugging in the values, we get:
pH = 4.74 + log(0.13/0.10) = 4.74 + log(1.3) = 4.74 + 0.11 = 4.85
Therefore, the pH of the buffer is approximately 4.85.