Final answer:
The pH of a solution that is 0.75 M in sodium acetate and 0.50 M in acetic acid is around 5.00, calculated using the Henderson-Hasselbalch equation with the given concentrations.
Step-by-step explanation:
To determine the pH of a solution that is 0.75 M in sodium acetate and 0.50 M in acetic acid, we can use the Henderson-Hasselbalch equation, pH = pKa + log([A-]/[HA]), where pKa is the acid dissociation constant of acetic acid and [A-] and [HA] are the concentrations of the acetate ion and acetic acid, respectively. From the given information, we can assume the pKa of acetic acid to be approximately 4.76 (as given in the example of creating a buffer of pH 5.0). Plugging the numbers into the equation, we get pH = 4.76 + log(0.75/0.50), which simplifies to pH = 4.76 + log(1.5). Therefore, the calculated pH after solving this becomes 4.76 + 0.176 = 4.936, which means the closest answer would be option b) 5.00. Thus, the pH of the solution is around 5.00, indicating that the solution is slightly acidic.