To prepare a buffer solution with a pH of 3.21, using one of the weak acid/conjugate base systems listed, you combine 1.00 L of a 0.430 M solution of weak acid with a 0.307 M potassium hydroxide solution.### Weak Acid and Conjugate Base Systems- **HNO₂ / NO₂⁻** - \( K_a = 4.5 \times 10^{-4} \) - \( pK_a = 3.35 \)- **HClO / ClO⁻** - \( K_a = 3.5 \times 10^{-8} \) - \( pK_a = 7.46 \)- **HCN / CN⁻** - \( K_a = 4.0 \times 10^{-10} \) - \( pK_a = 9.40 \)### TaskCalculate the volume in liters of the potassium hydroxide solution required to achieve the desired buffer pH with your chosen weak acid solution.

Answered: Consider how to prepare a buffer…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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To prepare a buffer solution with a pH of 3.21, using one of the weak acid/conjugate base systems listed, you combine 1.00 L of a 0.430 M solution of weak acid with a 0.307 M potassium hydroxide solution.

### Weak Acid and Conjugate Base Systems

- **HNO₂ / NO₂⁻**
- \( K_a = 4.5 \times 10^{-4} \)
- \( pK_a = 3.35 \)

- **HClO / ClO⁻**
- \( K_a = 3.5 \times 10^{-8} \)
- \( pK_a = 7.46 \)

- **HCN / CN⁻**
- \( K_a = 4.0 \times 10^{-10} \)
- \( pK_a = 9.40 \)

### Task

Calculate the volume in liters of the potassium hydroxide solution required to achieve the desired buffer pH with your chosen weak acid solution.

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Step 1: Defining buffer solution

Answer:

Buffer solution is a type of solution that resists the change in its pH on adding small quantity of acid or base. The solution of weak acid and its conjugate base can act like a buffer solution.

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