Certainly! Here's a transcription of the text suitable for an educational website:---**Buffer Solutions and pH Analysis**Consider the following scenario involving buffer solutions composed of m-chlorobenzoic acid, \( \text{HC}_7\text{H}_4\text{ClO}_2 \), and its conjugate base.1. **Buffer #1 Preparation:** - **Components:** 40.0 mL of 0.1 M \( \text{HC}_7\text{H}_4\text{ClO}_2 \) and 60.0 mL of 0.1 M \( \text{C}_7\text{H}_4\text{ClO}_2^- \) - **Final Volume:** 100.0 mL - **Objective:** Determine the pH of this buffer solution.2. **Buffer #2 Preparation:** - **Components:** 60.0 mL of 0.1 M \( \text{HC}_7\text{H}_4\text{ClO}_2 \) and 40.0 mL of 0.1 M \( \text{C}_7\text{H}_4\text{ClO}_2^- \) - **Final Volume:** 100.0 mL - **Objective:** Determine the pH of this buffer solution.**Question: Why is Buffer #2 more acidic than Buffer #1?**- **Options:** - (1) It has a greater volume of base. - (2) It has a greater final volume. - (3) It was prepared after Buffer #1. - (4) It has a higher acid concentration. *(Correct Answer)*---This exercise helps illustrate the concept of buffer solutions and how variations in their composition can affect their pH.

The Henderson-Hasselbalch equation for the acidic buffer solution is: pH=pKa+logsaltacid ......(1)

of m-chlorobenzoic acid, HC7H4CIO2, is 1.5x 10-4. (a) Suppose buffer #1 is prepared using 40.0 mL 0.1 M HC7H4CIO2 and 60.0 mL 0.1 M C7H4CIO2 to give a final volume of 100.0 mL. What is the pH of this buffer? 4.0 (b) Suppose a buffer #2 is prepared using 60.0 mL 0.1 M HC7H4CIO2 and 40.0 mL 0.1 M C7H4CIO2 to give a final volume c 100.0 mL. What is the pH of this buffer? 4.0 (c) Why is buffer #2 more acidic than buffer #1? It has a greater volume of base. O It has a greater final volume. O It was prepared after buffer #1. It has a higher acid concentration.

of m-chlorobenzoic acid, HC7H4CIO2, is 1.5x 10-4. (a) Suppose buffer #1 is prepared using 40.0 mL 0.1 M HC7H4CIO2 and 60.0 mL 0.1 M C7H4CIO2 to give a final volume of 100.0 mL. What is the pH of this buffer? 4.0 (b) Suppose a buffer #2 is prepared using 60.0 mL 0.1 M HC7H4CIO2 and 40.0 mL 0.1 M C7H4CIO2 to give a final volume c 100.0 mL. What is the pH of this buffer? 4.0 (c) Why is buffer #2 more acidic than buffer #1? It has a greater volume of base. O It has a greater final volume. O It was prepared after buffer #1. It has a higher acid concentration.

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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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

Certainly! Here's a transcription of the text suitable for an educational website:

---

**Buffer Solutions and pH Analysis**

Consider the following scenario involving buffer solutions composed of m-chlorobenzoic acid, \( \text{HC}_7\text{H}_4\text{ClO}_2 \), and its conjugate base.

1. **Buffer #1 Preparation:**
- **Components:** 40.0 mL of 0.1 M \( \text{HC}_7\text{H}_4\text{ClO}_2 \) and 60.0 mL of 0.1 M \( \text{C}_7\text{H}_4\text{ClO}_2^- \)
- **Final Volume:** 100.0 mL
- **Objective:** Determine the pH of this buffer solution.

2. **Buffer #2 Preparation:**
- **Components:** 60.0 mL of 0.1 M \( \text{HC}_7\text{H}_4\text{ClO}_2 \) and 40.0 mL of 0.1 M \( \text{C}_7\text{H}_4\text{ClO}_2^- \)
- **Final Volume:** 100.0 mL
- **Objective:** Determine the pH of this buffer solution.

**Question: Why is Buffer #2 more acidic than Buffer #1?**

- **Options:**
- (1) It has a greater volume of base.
- (2) It has a greater final volume.
- (3) It was prepared after Buffer #1.
- (4) It has a higher acid concentration. *(Correct Answer)*

---

This exercise helps illustrate the concept of buffer solutions and how variations in their composition can affect their pH.

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