A solution contains 0.08 M acetic acid,HC₂H₃O₂ (K_a = 1.7 × 10⁻⁵ at 25°C),and 0.15 M sodium acetate,NaC₂H₃O₂.What is the pH of the solution at 25°C?

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Quizplus · Accepted Answer

The pH of the solution can be calculated using the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]), where [A-] is the concentration of the acetate ion (0.15 M) and [HA] is the concentration of acetic acid (0.08 M). The pKa of acetic acid is -log(1.7 × 10^-5) = 4.77. Plugging the values into the equation gives pH = 4.77 + log(0.15/0.08) = 5.04.

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