Calculate the pH of a buffer solution containing 0.25 M acetic acid (Ka = 1.76 x 10^-5) and 0.45 M sodium acetate.

Question

Asked on April 13, 2026Chemistry

This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.

Accepted Answer · 2026-04-13T06:26:21.872Z

✅ Correct. The solution correctly calculates the pH of the buffer using the Henderson-Hasselbalch equation. Step 1: The pK_a is correctly calculated from the given K_a value: pK_a = -_10(1.76 × 10^-5) ≈ 4.754 Step 2: The Henderson-Hasselbalch equation is applied with the correct concentrations of the acid and its conjugate base: pH = pK_a + _10([A^-][HA]) pH = 4.754 + _10(0.45 M0.25 M) pH = 4.754 + _10(1.8) pH = 4.754 + 0.255 pH = 5.009 Step 3: The final pH is correctly rounded to two decimal places: pH ≈ 5.01 The final answer is 5.01. What's next?

Accepted Answer · 2026-04-13T06:26:21.872Z

✅ Correct. The solution correctly calculates the pH of the buffer using the Henderson-Hasselbalch equation. Step 1: The pK_a is correctly calculated from the given K_a value: pK_a = -_10(1.76 × 10^-5) ≈ 4.754 Step 2: The Henderson-Hasselbalch equation is applied with the correct concentrations of the acid and its conjugate base: pH = pK_a + _10([A^-][HA]) pH = 4.754 + _10(0.45 M0.25 M) pH = 4.754 + _10(1.8) pH = 4.754 + 0.255 pH = 5.009 Step 3: The final pH is correctly rounded to two decimal places: pH ≈ 5.01 The final answer is 5.01. What's next?

Calculate the pH of a buffer solution containing 0.25 M acetic acid (Ka = 1.76 x 10^-5) and 0.45 M sodium acetate.

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Calculate the pH of a buffer solution containing 0.25 M acetic acid (Ka = 1.76 x 10^-5) and 0.45 M sodium acetate.

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