What is the pH of 0.25 M aqueous acetate ion? (K_b of CH₃CO₂^- = 5.6 × 10^-10)

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Quizplus · Accepted Answer

The pH of the solution can be calculated using the hydrolysis of the acetate ion (CH3COO-) and the given Ka value for acetic acid (CH3COOH). The Ka value for acetic acid is given as 5.6 × 10^-10. Since acetate is the conjugate base of acetic acid, we can find the Kb for acetate using the relation Kw = Ka × Kb, where Kw is the ion-product constant for water (1.0 × 10^-14 at 25°C). Kb = Kw / Ka = (1.0 × 10^-14) / (5.6 × 10^-10) = 1.79 × 10^-5. The pH can then be calculated from the pOH using the formula pOH = 1/2(pKw - log[Kb] - log[base concentration]), where pKw = 14 at 25°C. After finding the pOH, pH = 14 - pOH. The calculations will show that the pH is closer to 9.07, indicating that the solution is basic, as expected for a solution of a conjugate base (acetate ion) in water.

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