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.

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**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.
Transcribed Image Text: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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