A buffer solution is made up of 1.0 M NH3 and 1.0 M NH4CI. = 1.8 x 10-5 K₂NH3 What is the pH when 20 mL of 0.60 M NaOH is added to 25. mL of the buffer? pH after base added [?] pH Enter
A buffer solution is made up of 1.0 M NH3 and 1.0 M NH4CI. = 1.8 x 10-5 K₂NH3 What is the pH when 20 mL of 0.60 M NaOH is added to 25. mL of the buffer? pH after base added [?] pH Enter
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter15: Acid–base Equilibria
Section: Chapter Questions
Problem 51P
Related questions
Question
![**Buffer Solution pH Calculation**
A buffer solution is composed of 1.0 M ammonia (NH₃) and 1.0 M ammonium chloride (NH₄Cl).
Given:
- \( K_b \) for NH₃ = \( 1.8 \times 10^{-5} \)
**Problem Statement:**
What is the pH when 20 mL of 0.60 M sodium hydroxide (NaOH) is added to 25 mL of the buffer solution?
The equation to determine the new pH is:
\[ \text{pH after base added} = \text{[?]} \]
### Steps to Solve:
1. **Determine the moles of NH₄⁺ and NH₃ initially in the buffer:**
- Volume of buffer = 25 mL → 0.025 L
- Molarity of NH₄Cl = 1.0 M
- Moles of NH₄⁺ = 0.025 L * 1.0 M = 0.025 moles
- Moles of NH₃ = 0.025 L * 1.0 M = 0.025 moles
2. **Determine the moles of NaOH added:**
- Volume of NaOH = 20 mL → 0.020 L
- Molarity of NaOH = 0.60 M
- Moles of NaOH = 0.020 L * 0.60 M = 0.012 moles
3. **Calculate the changes in moles after NaOH addition:**
- NaOH reacts with NH₄⁺ to form NH₃:
\[ \text{NH₄⁺} + \text{OH⁻} → \text{NH₃} + \text{H₂O} \]
- Moles of NH₄⁺ after reaction = 0.025 moles - 0.012 moles = 0.013 moles
- Moles of NH₃ after reaction = 0.025 moles + 0.012 moles = 0.037 moles
4. **Use the Henderson-Hasselbalch equation to find the new pH:**
\[ \text{pH} = \text{pKa}](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F12ff4d7f-8404-42ec-b494-33d871f3212a%2Ffc92ea4d-182f-4f53-be14-75360a2da608%2Fqf6nh8_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Buffer Solution pH Calculation**
A buffer solution is composed of 1.0 M ammonia (NH₃) and 1.0 M ammonium chloride (NH₄Cl).
Given:
- \( K_b \) for NH₃ = \( 1.8 \times 10^{-5} \)
**Problem Statement:**
What is the pH when 20 mL of 0.60 M sodium hydroxide (NaOH) is added to 25 mL of the buffer solution?
The equation to determine the new pH is:
\[ \text{pH after base added} = \text{[?]} \]
### Steps to Solve:
1. **Determine the moles of NH₄⁺ and NH₃ initially in the buffer:**
- Volume of buffer = 25 mL → 0.025 L
- Molarity of NH₄Cl = 1.0 M
- Moles of NH₄⁺ = 0.025 L * 1.0 M = 0.025 moles
- Moles of NH₃ = 0.025 L * 1.0 M = 0.025 moles
2. **Determine the moles of NaOH added:**
- Volume of NaOH = 20 mL → 0.020 L
- Molarity of NaOH = 0.60 M
- Moles of NaOH = 0.020 L * 0.60 M = 0.012 moles
3. **Calculate the changes in moles after NaOH addition:**
- NaOH reacts with NH₄⁺ to form NH₃:
\[ \text{NH₄⁺} + \text{OH⁻} → \text{NH₃} + \text{H₂O} \]
- Moles of NH₄⁺ after reaction = 0.025 moles - 0.012 moles = 0.013 moles
- Moles of NH₃ after reaction = 0.025 moles + 0.012 moles = 0.037 moles
4. **Use the Henderson-Hasselbalch equation to find the new pH:**
\[ \text{pH} = \text{pKa}
Expert Solution
![](/static/compass_v2/shared-icons/check-mark.png)
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 1 images
![Blurred answer](/static/compass_v2/solution-images/blurred-answer.jpg)
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
![Principles of Modern Chemistry](https://www.bartleby.com/isbn_cover_images/9781305079113/9781305079113_smallCoverImage.gif)
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
![Principles of Modern Chemistry](https://www.bartleby.com/isbn_cover_images/9781305079113/9781305079113_smallCoverImage.gif)
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning