What is the pH of a buffer solution made by adding 0.41 g of NaC2H3O2 to 100. mL of 0.10 M HC2H302? Molar mass of NaC2H3O2 = 82.0 g/mol Ka of HC2H302 = 1.8×10-5 pH of buffer pH of Buffer = [?] Enter
What is the pH of a buffer solution made by adding 0.41 g of NaC2H3O2 to 100. mL of 0.10 M HC2H302? Molar mass of NaC2H3O2 = 82.0 g/mol Ka of HC2H302 = 1.8×10-5 pH of buffer pH of Buffer = [?] Enter
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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
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![**Determining the pH of a Buffer Solution**
To calculate the pH of a buffer solution, consider the following scenario:
**Problem Statement:**
What is the pH of a buffer solution made by adding 0.41 g of NaC₂H₃O₂ to 100. mL of 0.10 M HC₂H₃O₂?
**Given Data:**
1. Mass of NaC₂H₃O₂ added: 0.41 g
2. Volume of HC₂H₃O₂ solution: 100. mL (0.10 L)
3. Concentration of HC₂H₃O₂: 0.10 M
4. Molar mass of NaC₂H₃O₂: 82.0 g/mol
5. Acid dissociation constant (Kₐ) of HC₂H₃O₂: 1.8 × 10⁻⁵
**Objective:**
Find the pH of the buffer solution.
**Calculation:**
1. **Determine the moles of NaC₂H₃O₂ (sodium acetate):**
\[
\text{Moles of NaC₂H₃O₂} = \frac{\text{Mass (g)}}{\text{Molar mass (g/mol)}} = \frac{0.41 \text{ g}}{82.0 \text{ g/mol}} = 0.005 \text{ mol}
\]
2. **Calculate the concentration of NaC₂H₃O₂ in the solution:**
- Note: The volume of the solution remains 0.10 L
\[
\text{Concentration of NaC₂H₃O₂} = \frac{\text{Moles of NaC₂H₃O₂}}{\text{Volume of solution (L)}} = \frac{0.005 \text{ mol}}{0.10 \text{ L}} = 0.05 \text{ M}
\]
3. **Apply the Henderson-Hasselbalch equation:**
\[
\text{pH} = \text{p}Kₐ + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right)
\]
Where:
- \([\text{A](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F74ff972a-42b6-478c-a012-297da9a07acf%2Ff718a825-cd15-46a7-a878-de087bde8079%2F03ekcmb_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Determining the pH of a Buffer Solution**
To calculate the pH of a buffer solution, consider the following scenario:
**Problem Statement:**
What is the pH of a buffer solution made by adding 0.41 g of NaC₂H₃O₂ to 100. mL of 0.10 M HC₂H₃O₂?
**Given Data:**
1. Mass of NaC₂H₃O₂ added: 0.41 g
2. Volume of HC₂H₃O₂ solution: 100. mL (0.10 L)
3. Concentration of HC₂H₃O₂: 0.10 M
4. Molar mass of NaC₂H₃O₂: 82.0 g/mol
5. Acid dissociation constant (Kₐ) of HC₂H₃O₂: 1.8 × 10⁻⁵
**Objective:**
Find the pH of the buffer solution.
**Calculation:**
1. **Determine the moles of NaC₂H₃O₂ (sodium acetate):**
\[
\text{Moles of NaC₂H₃O₂} = \frac{\text{Mass (g)}}{\text{Molar mass (g/mol)}} = \frac{0.41 \text{ g}}{82.0 \text{ g/mol}} = 0.005 \text{ mol}
\]
2. **Calculate the concentration of NaC₂H₃O₂ in the solution:**
- Note: The volume of the solution remains 0.10 L
\[
\text{Concentration of NaC₂H₃O₂} = \frac{\text{Moles of NaC₂H₃O₂}}{\text{Volume of solution (L)}} = \frac{0.005 \text{ mol}}{0.10 \text{ L}} = 0.05 \text{ M}
\]
3. **Apply the Henderson-Hasselbalch equation:**
\[
\text{pH} = \text{p}Kₐ + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right)
\]
Where:
- \([\text{A
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