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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![### Question:
What is the pH of a buffer containing 0.55 M HF (aq) and 0.55 M NaF (aq)?
### Possible Answers:
- ○ 1.70
- ○ 3.15
- ○ 0.26
- ○ 8.44
- ○ 10.85
### Explanation:
This question tests your understanding of buffer solutions and their pH calculations. A buffer is a solution containing a weak acid and its conjugate base, which resists changes in pH when small amounts of acid or base are added. For this problem, use the Henderson-Hasselbalch equation:
\[ \text{pH} = \text{pKa} + \log\left(\frac{\text{[A}^-]}{\text{[HA]}}\right) \]
Where:
- \(\text{pKa}\) of HF is approximately 3.17
- [A\(^-\)] is the concentration of the conjugate base, F\(^-\) from NaF
- [HA] is the concentration of the weak acid, HF
Since both concentrations are equal, the pH equals the \(\text{pKa}\).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F704a01f5-4824-48f7-9b88-5a0e03edcc36%2F90f0db86-4a9d-4564-9a17-d95d08f03af3%2Fxqybr1h_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Question:
What is the pH of a buffer containing 0.55 M HF (aq) and 0.55 M NaF (aq)?
### Possible Answers:
- ○ 1.70
- ○ 3.15
- ○ 0.26
- ○ 8.44
- ○ 10.85
### Explanation:
This question tests your understanding of buffer solutions and their pH calculations. A buffer is a solution containing a weak acid and its conjugate base, which resists changes in pH when small amounts of acid or base are added. For this problem, use the Henderson-Hasselbalch equation:
\[ \text{pH} = \text{pKa} + \log\left(\frac{\text{[A}^-]}{\text{[HA]}}\right) \]
Where:
- \(\text{pKa}\) of HF is approximately 3.17
- [A\(^-\)] is the concentration of the conjugate base, F\(^-\) from NaF
- [HA] is the concentration of the weak acid, HF
Since both concentrations are equal, the pH equals the \(\text{pKa}\).
Expert Solution
Step 1
Given that :
The concentration of HF (acid) = 0.55 M
The concentration of NaF (salt) = 0.55 M
We have to calculate the pH of the above buffer.
Step by step
Solved in 3 steps
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