Chemistry
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ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![### Determining the pH Change in a Buffer Solution
**Problem Statement:**
A buffer solution contains two components with the following molar concentrations:
- **0.452 M KHSO₃**
- **0.273 M Na₂SO₃**
Our goal is to determine the pH change when **0.109 mol KOH** is added to **1.00 L** of this buffer solution.
**Equation Setup:**
\[ \text{pH after addition} - \text{pH before addition} = \text{pH change} = \_\_\_\_ \]
To find the pH change, you will need to understand the chemistry of the buffer and how the added KOH (a strong base) interacts with the components of the buffer. This involves understanding:
- Buffer equations
- Acid-base equilibria
- The Henderson-Hasselbalch equation (for easy calculation of pH before and after addition).
**Explanation of Buffer Interaction:**
1. **Initial Condition:**
The buffer contains weak acid (KHSO₃) and its conjugate base (Na₂SO₃).
2. **Reaction with KOH:**
\[ \text{KHSO₃} + \text{KOH} \rightarrow \text{K₂SO₃} + \text{H₂O} \]
3. **Understanding pH Calculation:**
After adding KOH, the concentrations of KHSO₃ and Na₂SO₃ will change based on the stoichiometry of the reaction. The new concentrations will be used to find the new pH using the Henderson-Hasselbalch equation:
\[ \text{pH} = \text{pKa} + \log \left(\frac{[\text{Conjugate Base}]}{[\text{Acid}]}\right) \]
**Note:**
- Calculate the pH before and after addition.
- Subtract the initial pH from the final pH to find the pH change.
Insert the calculated value in the space provided to quantify the pH change.
Understanding this process is fundamental for controlling reactions in various scientific and industrial applications, ensuring the solution maintains its buffering capacity upon the addition of acids or bases.
---
**Interactive Diagrams:**
- Although there are no diagrams or graphs in the provided image, diagrams illustrating the reaction mechanism and pH changes in](https://content.bartleby.com/qna-images/question/03ba95c9-584b-483d-8f8a-8f0f9c4c55b7/722b04f8-3aad-4c9f-a71b-0d8a503100e6/ks399j_processed.png)
Transcribed Image Text:### Determining the pH Change in a Buffer Solution
**Problem Statement:**
A buffer solution contains two components with the following molar concentrations:
- **0.452 M KHSO₃**
- **0.273 M Na₂SO₃**
Our goal is to determine the pH change when **0.109 mol KOH** is added to **1.00 L** of this buffer solution.
**Equation Setup:**
\[ \text{pH after addition} - \text{pH before addition} = \text{pH change} = \_\_\_\_ \]
To find the pH change, you will need to understand the chemistry of the buffer and how the added KOH (a strong base) interacts with the components of the buffer. This involves understanding:
- Buffer equations
- Acid-base equilibria
- The Henderson-Hasselbalch equation (for easy calculation of pH before and after addition).
**Explanation of Buffer Interaction:**
1. **Initial Condition:**
The buffer contains weak acid (KHSO₃) and its conjugate base (Na₂SO₃).
2. **Reaction with KOH:**
\[ \text{KHSO₃} + \text{KOH} \rightarrow \text{K₂SO₃} + \text{H₂O} \]
3. **Understanding pH Calculation:**
After adding KOH, the concentrations of KHSO₃ and Na₂SO₃ will change based on the stoichiometry of the reaction. The new concentrations will be used to find the new pH using the Henderson-Hasselbalch equation:
\[ \text{pH} = \text{pKa} + \log \left(\frac{[\text{Conjugate Base}]}{[\text{Acid}]}\right) \]
**Note:**
- Calculate the pH before and after addition.
- Subtract the initial pH from the final pH to find the pH change.
Insert the calculated value in the space provided to quantify the pH change.
Understanding this process is fundamental for controlling reactions in various scientific and industrial applications, ensuring the solution maintains its buffering capacity upon the addition of acids or bases.
---
**Interactive Diagrams:**
- Although there are no diagrams or graphs in the provided image, diagrams illustrating the reaction mechanism and pH changes in
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