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
Chapter14: Acids And Bases
Section: Chapter Questions
Problem 10RQ: For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen...
Related questions
Question
![**Buffer Solution Calculation Example**
A buffer solution is prepared with the following concentrations:
- 0.372 M (Molar) of NaHC₂O₄
- 0.323 M (Molar) of Na₂C₂O₄
Given the acid dissociation constant \( K_a \) for HC₂O₄⁻ is \( 6.4 \times 10^{-5} \).
**Question:** What is the pH of this buffer solution?
This exercise involves the use of the Henderson-Hasselbalch equation for calculating the pH of a buffer solution:
\[ \text{pH} = pK_a + \log \left( \frac{[\text{Conjugate Base}]}{[\text{Weak Acid}]} \right) \]
**Explanation:**
1. \( K_a \) is provided, and from \( K_a \), \( pK_a \) can be found using the equation:
\[ pK_a = -\log(K_a) \]
2. Substitute the concentrations of the conjugate base \( [\text{Na}_{2}\text{C}_2\text{O}_{4}] \) and the weak acid \( [\text{NaHC}_2\text{O}_{4}] \) into the Henderson-Hasselbalch equation.
The given information is used to find the pH of the buffer through proper calculation steps involving logarithms and the provided constants.
Use this example to understand the practical application of acid-base chemistry in buffer systems and the importance of accurate calculations in determining pH levels.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2acc7fbd-793a-490d-a2b4-11bc81b4299f%2Fa3ecd244-4f01-43fd-94ba-d10ac33f7dba%2Fi2nk4jr_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Buffer Solution Calculation Example**
A buffer solution is prepared with the following concentrations:
- 0.372 M (Molar) of NaHC₂O₄
- 0.323 M (Molar) of Na₂C₂O₄
Given the acid dissociation constant \( K_a \) for HC₂O₄⁻ is \( 6.4 \times 10^{-5} \).
**Question:** What is the pH of this buffer solution?
This exercise involves the use of the Henderson-Hasselbalch equation for calculating the pH of a buffer solution:
\[ \text{pH} = pK_a + \log \left( \frac{[\text{Conjugate Base}]}{[\text{Weak Acid}]} \right) \]
**Explanation:**
1. \( K_a \) is provided, and from \( K_a \), \( pK_a \) can be found using the equation:
\[ pK_a = -\log(K_a) \]
2. Substitute the concentrations of the conjugate base \( [\text{Na}_{2}\text{C}_2\text{O}_{4}] \) and the weak acid \( [\text{NaHC}_2\text{O}_{4}] \) into the Henderson-Hasselbalch equation.
The given information is used to find the pH of the buffer through proper calculation steps involving logarithms and the provided constants.
Use this example to understand the practical application of acid-base chemistry in buffer systems and the importance of accurate calculations in determining pH levels.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 2 steps
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning