Organic Chemistry: A Guided Inquiry
2nd Edition
ISBN:9780618974122
Author:Andrei Straumanis
Publisher:Andrei Straumanis
Chapter4: Polar Bonds, Polar Reactions
Section: Chapter Questions
Problem 28CTQ: For the previous four questions, label each molecule that appears in the question or your answer...
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Question
![**Problem Statement:**
What is the pH of a 0.120 M solution of aniline (C₆H₅NH₂, Kb = 4.3 × 10⁻¹⁰)?
---
**Explanation:**
To find the pH of the solution, follow these steps:
1. **Identify the given information:**
- Concentration of aniline solution: 0.120 M
- Base dissociation constant (Kb) of aniline: 4.3 × 10⁻¹⁰
2. **Determine the concentration of OH⁻ ions:**
- Use the formula for base dissociation:
\[
Kb = \frac{[C₆H₅NH₃⁺][OH⁻]}{[C₆H₅NH₂]}
\]
3. **Assume x is the concentration of OH⁻ ions at equilibrium:**
- Substitute in the formula:
\[
4.3 \times 10^{-10} = \frac{x^2}{0.120 - x}
\]
- Since Kb is small, assume \(0.120 - x \approx 0.120\), then solve for x:
\[
x^2 = 4.3 \times 10^{-10} \times 0.120
\]
- Calculate x.
4. **Calculate pOH:**
- Use the formula:
\[
\text{pOH} = -\log[OH⁻]
\]
5. **Determine pH:**
- Use the relationship between pH and pOH:
\[
\text{pH} = 14 - \text{pOH}
\]
By following these steps, you can find the pH of the aniline solution.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Faeef920a-b7fc-42c4-a405-16f92aebf3b1%2Fe822e5ee-95dd-4ccf-bf55-2463193a9b39%2Fkh4z0xe_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
What is the pH of a 0.120 M solution of aniline (C₆H₅NH₂, Kb = 4.3 × 10⁻¹⁰)?
---
**Explanation:**
To find the pH of the solution, follow these steps:
1. **Identify the given information:**
- Concentration of aniline solution: 0.120 M
- Base dissociation constant (Kb) of aniline: 4.3 × 10⁻¹⁰
2. **Determine the concentration of OH⁻ ions:**
- Use the formula for base dissociation:
\[
Kb = \frac{[C₆H₅NH₃⁺][OH⁻]}{[C₆H₅NH₂]}
\]
3. **Assume x is the concentration of OH⁻ ions at equilibrium:**
- Substitute in the formula:
\[
4.3 \times 10^{-10} = \frac{x^2}{0.120 - x}
\]
- Since Kb is small, assume \(0.120 - x \approx 0.120\), then solve for x:
\[
x^2 = 4.3 \times 10^{-10} \times 0.120
\]
- Calculate x.
4. **Calculate pOH:**
- Use the formula:
\[
\text{pOH} = -\log[OH⁻]
\]
5. **Determine pH:**
- Use the relationship between pH and pOH:
\[
\text{pH} = 14 - \text{pOH}
\]
By following these steps, you can find the pH of the aniline solution.
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