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...
Related questions
Question
![### Calculating the pH of a Buffer Solution
#### Problem Statement:
Calculate the pH of a buffer solution that is **0.339 M** in **NH₃ (ammonia)** and **0.143 M** in **NH₄Cl**.
#### Solution:
To calculate the pH of a buffer solution, you can use the Henderson-Hasselbalch equation:
\[ \text{pH} = \text{p}K_{\text{a}} + \log \left( \frac{[\text{Base}]}{[\text{Acid}]} \right) \]
In this problem:
- The base (\( \text{NH}_3 \)) concentration (\( [\text{Base}] \)) is **0.339 M**
- The conjugate acid (\( \text{NH}_4^+ \), provided by \( \text{NH}_4\text{Cl} \)) concentration (\( [\text{Acid}] \)) is **0.143 M**
Here, the \( \text{Kb} \) for ammonia (\( \text{NH}_3 \)) can be used to find the \( \text{pKa} \) of its conjugate acid, ammonia (\( \text{NH}_4^+ \)).
\[ \text{p}K_{\text{a}} = 14 - \text{p}K_{\text{b}} \]
Assuming \( \text{p}K_{\text{b}} \) of ammonia is approximately 4.75:
\[ \text{p}K_{\text{a}} = 14 - 4.75 = 9.25 \]
So, the Henderson-Hasselbalch equation becomes:
\[ \text{pH} = 9.25 + \log \left( \frac{0.339}{0.143} \right) \]
#### Graphs and Diagrams:
In this example, no graphs or diagrams were provided. However, if there were, the explanation would include descriptions of axes, data points, and any significant trends or patterns observed within the graph or diagram.
You can input these values into the equation and calculate the log term to find the pH of the buffer solution. The final pH will be determined numerically.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2acc7fbd-793a-490d-a2b4-11bc81b4299f%2F0cb8ec65-3a90-4966-9d77-d376dbac9e9e%2Fk3pw5vv_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Calculating the pH of a Buffer Solution
#### Problem Statement:
Calculate the pH of a buffer solution that is **0.339 M** in **NH₃ (ammonia)** and **0.143 M** in **NH₄Cl**.
#### Solution:
To calculate the pH of a buffer solution, you can use the Henderson-Hasselbalch equation:
\[ \text{pH} = \text{p}K_{\text{a}} + \log \left( \frac{[\text{Base}]}{[\text{Acid}]} \right) \]
In this problem:
- The base (\( \text{NH}_3 \)) concentration (\( [\text{Base}] \)) is **0.339 M**
- The conjugate acid (\( \text{NH}_4^+ \), provided by \( \text{NH}_4\text{Cl} \)) concentration (\( [\text{Acid}] \)) is **0.143 M**
Here, the \( \text{Kb} \) for ammonia (\( \text{NH}_3 \)) can be used to find the \( \text{pKa} \) of its conjugate acid, ammonia (\( \text{NH}_4^+ \)).
\[ \text{p}K_{\text{a}} = 14 - \text{p}K_{\text{b}} \]
Assuming \( \text{p}K_{\text{b}} \) of ammonia is approximately 4.75:
\[ \text{p}K_{\text{a}} = 14 - 4.75 = 9.25 \]
So, the Henderson-Hasselbalch equation becomes:
\[ \text{pH} = 9.25 + \log \left( \frac{0.339}{0.143} \right) \]
#### Graphs and Diagrams:
In this example, no graphs or diagrams were provided. However, if there were, the explanation would include descriptions of axes, data points, and any significant trends or patterns observed within the graph or diagram.
You can input these values into the equation and calculate the log term to find the pH of the buffer solution. The final pH will be determined numerically.
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 4 steps with 1 images
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
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY