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...
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![### Buffers: Buffers and Buffer Capacity
#### Laboratory Simulation
1) **Calculate the pH of a solution prepared by dissolving 1.60 g of sodium acetate, CH<sub>3</sub>COONa, in 50.0 mL of 0.15 M acetic acid, CH<sub>3</sub>COOH (aq)**.
Assume the volume change upon dissolving the sodium acetate is negligible. K<sub>a</sub> of CH<sub>3</sub>COOH is 1.75 x 10<sup>-5</sup>.
#### pH = [Input Box Here]
In this simulation, you will learn how to calculate the pH of a buffer solution. Proper understanding of buffer capacity and their calculation is essential for grasping buffer systems in chemistry.
A buffer solution typically contains a weak acid and its conjugate base. The sodium acetate (CH<sub>3</sub>COONa) dissolves in water to provide acetate ions (CH<sub>3</sub>COO<sup>-</sup>), which combine with the acetic acid (CH<sub>3</sub>COOH) to form a buffer system. Use the given data along with your knowledge of acid dissociation constants and the Henderson-Hasselbalch equation to compute the pH.
### Steps to Calculate the pH of the Buffer Solution:
1. **Identify the Weak Acid and its Conjugate Base:**
- Weak Acid: Acetic acid (CH<sub>3</sub>COOH)
- Conjugate Base: Acetate ion (CH<sub>3</sub>COO<sup>-</sup>)
2. **Calculate the Moles of Sodium Acetate and Acetic Acid:**
- Moles of Sodium Acetate: Calculate using its mass (1.60 g) and molar mass.
- Moles of Acetic Acid: Calculate using its volume (50.0 mL) and concentration (0.15 M).
3. **Set Up the Expression:**
- Using the Henderson-Hasselbalch equation:
\[
\text{pH} = \text{p}K_{a} + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right)
\](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F136a9916-8a5d-490b-a1c4-57e644d5608a%2Fec73378b-e081-4f60-a384-42a0523e1783%2F5z9o04r_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Buffers: Buffers and Buffer Capacity
#### Laboratory Simulation
1) **Calculate the pH of a solution prepared by dissolving 1.60 g of sodium acetate, CH<sub>3</sub>COONa, in 50.0 mL of 0.15 M acetic acid, CH<sub>3</sub>COOH (aq)**.
Assume the volume change upon dissolving the sodium acetate is negligible. K<sub>a</sub> of CH<sub>3</sub>COOH is 1.75 x 10<sup>-5</sup>.
#### pH = [Input Box Here]
In this simulation, you will learn how to calculate the pH of a buffer solution. Proper understanding of buffer capacity and their calculation is essential for grasping buffer systems in chemistry.
A buffer solution typically contains a weak acid and its conjugate base. The sodium acetate (CH<sub>3</sub>COONa) dissolves in water to provide acetate ions (CH<sub>3</sub>COO<sup>-</sup>), which combine with the acetic acid (CH<sub>3</sub>COOH) to form a buffer system. Use the given data along with your knowledge of acid dissociation constants and the Henderson-Hasselbalch equation to compute the pH.
### Steps to Calculate the pH of the Buffer Solution:
1. **Identify the Weak Acid and its Conjugate Base:**
- Weak Acid: Acetic acid (CH<sub>3</sub>COOH)
- Conjugate Base: Acetate ion (CH<sub>3</sub>COO<sup>-</sup>)
2. **Calculate the Moles of Sodium Acetate and Acetic Acid:**
- Moles of Sodium Acetate: Calculate using its mass (1.60 g) and molar mass.
- Moles of Acetic Acid: Calculate using its volume (50.0 mL) and concentration (0.15 M).
3. **Set Up the Expression:**
- Using the Henderson-Hasselbalch equation:
\[
\text{pH} = \text{p}K_{a} + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right)
\
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