Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![**Question:**
What is the pH of a 0.240 M solution of aniline (C₆H₅NH₂, Kb = 4.3 × 10⁻¹⁰)?
**Explanation:**
To find the pH of aniline, which is a weak base, you can use the formula for the base dissociation constant (Kb) to determine the concentration of hydroxide ions (OH⁻). Then, convert the OH⁻ concentration to pOH, and finally to pH.
1. **Calculate OH⁻ Concentration:**
For a weak base like aniline (C₆H₅NH₂), use the equation:
\[
Kb = \frac{[C₆H₅NH₃⁺][OH⁻]}{[C₆H₅NH₂]}
\]
Assume that the change in concentration \([OH⁻] = x\), then:
\[
Kb = \frac{x^2}{[0.240 - x]} \approx \frac{x^2}{0.240}
\]
Solve for \( x \) knowing \( Kb = 4.3 \times 10^{-10} \).
2. **Calculate pOH:**
\[
pOH = -\log[OH⁻]
\]
3. **Calculate pH:**
\[
pH = 14 - pOH
\]
Use these steps to find the pH of the solution.](https://content.bartleby.com/qna-images/question/3523b6f7-3769-45b8-98d5-cc26f8ce7a3b/05067b64-354d-4ac0-8fbd-1f25643cf5e4/wo3smgo_processed.jpeg)
Transcribed Image Text:**Question:**
What is the pH of a 0.240 M solution of aniline (C₆H₅NH₂, Kb = 4.3 × 10⁻¹⁰)?
**Explanation:**
To find the pH of aniline, which is a weak base, you can use the formula for the base dissociation constant (Kb) to determine the concentration of hydroxide ions (OH⁻). Then, convert the OH⁻ concentration to pOH, and finally to pH.
1. **Calculate OH⁻ Concentration:**
For a weak base like aniline (C₆H₅NH₂), use the equation:
\[
Kb = \frac{[C₆H₅NH₃⁺][OH⁻]}{[C₆H₅NH₂]}
\]
Assume that the change in concentration \([OH⁻] = x\), then:
\[
Kb = \frac{x^2}{[0.240 - x]} \approx \frac{x^2}{0.240}
\]
Solve for \( x \) knowing \( Kb = 4.3 \times 10^{-10} \).
2. **Calculate pOH:**
\[
pOH = -\log[OH⁻]
\]
3. **Calculate pH:**
\[
pH = 14 - pOH
\]
Use these steps to find the pH of the solution.
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