Calculate the pH of a solution made by combining 10.0 mL of 17.5 M acetic acid with 5.54 g of sodium acetate and diluting to a total volume of 1.50 L.

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1. Calculate the moles of acetic acid (CH₃COOH) using its concentration and volume: \( \text{moles of CH}_3\text{COOH} = 17.5 \text{ M} \times 0.010 \text{ L} \).
2. Calculate the moles of sodium acetate (CH₃COONa) using its mass and molar mass: \( \text{moles of CH}_3\text{COONa} = \frac{5.54 \text{ g}}{\text{molar mass of CH}_3\text{COONa}} \).
3. Determine the concentrations of acetic acid and acetate ion in the final solution by dividing the moles of each by the total volume of the solution (1.50 L).
4. Use the Henderson-Hasselbalch equation to calculate the pH: \( \text{pH} = \text{pK}_a + \log \left( \frac{[\text{CH}_3\text{COO}^-]}{[\text{CH}_3\text{COOH}]} \right) \), where \( \text{pK}_a \) is the negative logarithm of the acid dissociation constant of acetic acid.
5. Substitute the concentrations of acetate ion and acetic acid into the Henderson-Hasselbalch equation to find the pH.