Final answer:
The question lacks necessary information, such as the volume of the solution and the pKa of acetic acid, to accurately calculate the pH of the sodium acetate solution.
Step-by-step explanation:
The student is asking to calculate the pH of a solution prepared by dissolving 1.15 g of sodium acetate. To calculate the pH, we need to know the concentration of the sodium acetate in solution, the ionization constant (Ka) for acetic acid, and then use the Henderson-Hasselbalch equation for a buffer solution. However, the question does not provide the volume of the solution or the pKa of acetic acid. Normally, to find the pH of a buffer solution, like the one formed by sodium acetate and acetic acid, you would use the formula:
pH = pKa + log ([A-]/[HA])
where [A-] is the concentration of the acetate ion and [HA] is the concentration of acetic acid. If we assume that the sodium acetate completely dissociates in water, it will produce sodium ions Na+ and acetate ions CH3COO-. Assuming that the volume is 1 L, the moles of sodium acetate would be equal to its molarity. Because we do not have the necessary information to solve this problem, such as the volume of the solution and the pKa of acetic acid, we cannot provide the exact pH without making some assumptions. Therefore, we cannot accurately answer this question or select the correct multiple-choice answer.