Certainly! Below is the transcription and explanation suitable for an educational website.---**Buffer Solution pH Calculation****a.** What is the pH of a buffer solution that is 0.18 M \( \text{NH}_3 \) and 0.18 M \( \text{NH}_4^+ \)? The \( K_b \) for \( \text{NH}_3 \) is \( 1.8 \times 10^{-5} \).**pH =** [blank space for answer]*Explanation:* To calculate the pH of the buffer solution, use the Henderson-Hasselbalch equation:\[ \text{pH} = \text{pKa} + \log\left(\frac{[\text{base}]}{[\text{acid}]}\right) \]**b.** What is the pH if 41 mL of 0.13 M hydrochloric acid is added to 425 mL of this buffer?**pH =** [blank space for answer]*Explanation:* When adding an acid to the buffer, the pH changes depending on the buffer capacity. Adjust the concentration of \( \text{NH}_3 \) and \( \text{NH}_4^+ \) in the Henderson-Hasselbalch equation to find the new pH. Consider the volume change due to the addition of the acid.---This transcription provides a clear view of the problem and hints at the method needed to solve the questions.

Answered: a. What is the pH of a buffer solution…

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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Certainly! Below is the transcription and explanation suitable for an educational website.

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**Buffer Solution pH Calculation**

**a.** What is the pH of a buffer solution that is 0.18 M \( \text{NH}_3 \) and 0.18 M \( \text{NH}_4^+ \)? The \( K_b \) for \( \text{NH}_3 \) is \( 1.8 \times 10^{-5} \).

**pH =** [blank space for answer]

*Explanation:* To calculate the pH of the buffer solution, use the Henderson-Hasselbalch equation:
\[ \text{pH} = \text{pKa} + \log\left(\frac{[\text{base}]}{[\text{acid}]}\right) \]

**b.** What is the pH if 41 mL of 0.13 M hydrochloric acid is added to 425 mL of this buffer?

**pH =** [blank space for answer]

*Explanation:* When adding an acid to the buffer, the pH changes depending on the buffer capacity. Adjust the concentration of \( \text{NH}_3 \) and \( \text{NH}_4^+ \) in the Henderson-Hasselbalch equation to find the new pH. Consider the volume change due to the addition of the acid.

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This transcription provides a clear view of the problem and hints at the method needed to solve the questions.

Expert Solution

Step 1

a.) To calculate pH, we would use Henderson Hasselbalch equation.

b.) First we need to calculate moles of all species. Then hydrochloric acid will react with basic part of buffer, so we need to write a reaction and draw ICE table to calculate the equilibrium moles of all species.

Then we can use Henderson Hasselbalch equation to calculate pH.

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