Question 5 of 7 What quantity in moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer with a pH of 4.30? (Ka for HF is 6.8 x 104)
Question 5 of 7 What quantity in moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer with a pH of 4.30? (Ka for HF is 6.8 x 104)
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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![**Buffer Preparation Question**
**Question:**
What quantity in moles of NaOH needs to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer with a pH of 4.30? (Ka for HF is 6.8 × 10⁻⁴)
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**Explanation:**
To solve this problem, use the Henderson-Hasselbalch equation:
\[ \text{pH} = \text{pKa} + \log \left( \frac{\text{[A⁻]}}{\text{[HA]}} \right) \]
Where:
- pH is the desired pH of the buffer.
- \(\text{pKa} = -\log(\text{Ka})\) for HF.
- \([\text{A⁻}]\) is the concentration of the conjugate base (F⁻).
- \([\text{HA}]\) is the concentration of the weak acid (HF).
Calculate the pKa of HF and rearrange the equation to find the moles of NaOH needed to achieve the desired pH.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3523b6f7-3769-45b8-98d5-cc26f8ce7a3b%2F39b3b9a7-d3af-4b0c-9138-185e21a1f9a0%2F8liphm7_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Buffer Preparation Question**
**Question:**
What quantity in moles of NaOH needs to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer with a pH of 4.30? (Ka for HF is 6.8 × 10⁻⁴)
---
**Explanation:**
To solve this problem, use the Henderson-Hasselbalch equation:
\[ \text{pH} = \text{pKa} + \log \left( \frac{\text{[A⁻]}}{\text{[HA]}} \right) \]
Where:
- pH is the desired pH of the buffer.
- \(\text{pKa} = -\log(\text{Ka})\) for HF.
- \([\text{A⁻}]\) is the concentration of the conjugate base (F⁻).
- \([\text{HA}]\) is the concentration of the weak acid (HF).
Calculate the pKa of HF and rearrange the equation to find the moles of NaOH needed to achieve the desired pH.
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