ou need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (pKa = 4.20) and 0.180 M odium benzoate. Cow many milliliters of each solution should be mixed to prepare this buffer? enzoic acid: 68.93 Incorrect odium benzoate: 31.07 Incorrect mL mL
ou need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (pKa = 4.20) and 0.180 M odium benzoate. Cow many milliliters of each solution should be mixed to prepare this buffer? enzoic acid: 68.93 Incorrect odium benzoate: 31.07 Incorrect mL mL
Chemistry
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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
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You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (p?a=4.20) and 0.180 M sodium benzoate.
How many milliliters of each solution should be mixed to prepare this buffer?
![### Preparation of a Buffer Solution
To prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (pKa = 4.20) and 0.180 M sodium benzoate, calculate the required volumes of each component.
#### Problem Statement:
You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (pKa = 4.20) and 0.180 M sodium benzoate.
**Question:**
How many milliliters of each solution should be mixed to prepare this buffer?
#### Incorrect Answers Provided:
**Benzoic acid:**
- 68.93 mL
*Status: Incorrect*
**Sodium benzoate:**
- 31.07 mL
*Status: Incorrect*
### Explanation:
When preparing a buffer solution, you should use the Henderson-Hasselbalch equation to determine the correct ratio of acid and conjugate base:
\[ \text{pH} = \text{pKa} + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \]
Where:
- pH is the desired pH of the buffer solution.
- pKa is the acid dissociation constant of benzoic acid.
- \([\text{A}^-]\) is the concentration of the conjugate base (sodium benzoate).
- \([\text{HA}]\) is the concentration of the acid (benzoic acid).
By setting up and solving this equation correctly, you can find the appropriate volumes for each solution needed to create the buffer with the desired pH.
In this problem, the calculated volumes provided are 68.93 mL for benzoic acid and 31.07 mL for sodium benzoate, both of which are incorrect. Therefore, re-evaluating the calculation using the appropriate method is necessary.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F85650e2f-17ad-4aa4-9d56-acd675fbc675%2F214d3758-c583-4a5e-8792-c79fec23e77a%2Ff88idld_processed.png&w=3840&q=75)
Transcribed Image Text:### Preparation of a Buffer Solution
To prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (pKa = 4.20) and 0.180 M sodium benzoate, calculate the required volumes of each component.
#### Problem Statement:
You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (pKa = 4.20) and 0.180 M sodium benzoate.
**Question:**
How many milliliters of each solution should be mixed to prepare this buffer?
#### Incorrect Answers Provided:
**Benzoic acid:**
- 68.93 mL
*Status: Incorrect*
**Sodium benzoate:**
- 31.07 mL
*Status: Incorrect*
### Explanation:
When preparing a buffer solution, you should use the Henderson-Hasselbalch equation to determine the correct ratio of acid and conjugate base:
\[ \text{pH} = \text{pKa} + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \]
Where:
- pH is the desired pH of the buffer solution.
- pKa is the acid dissociation constant of benzoic acid.
- \([\text{A}^-]\) is the concentration of the conjugate base (sodium benzoate).
- \([\text{HA}]\) is the concentration of the acid (benzoic acid).
By setting up and solving this equation correctly, you can find the appropriate volumes for each solution needed to create the buffer with the desired pH.
In this problem, the calculated volumes provided are 68.93 mL for benzoic acid and 31.07 mL for sodium benzoate, both of which are incorrect. Therefore, re-evaluating the calculation using the appropriate method is necessary.
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