### Table of Solution pH ValuesThe following table provides the pH values of various solutions after performing specific treatments. The pH scale is used to determine the acidity or basicity of a solution, with lower values indicating higher acidity and higher values indicating higher basicity.| Solutions | pH values ||----------------------|-----------|| H₂O (unboiled) | 3.5 || H₂O (boiled) | 7.0 || NaCl | 7.0 || NaC₂H₃O₂ | 9.1 || NH₄Cl | 4.5 || NaHCO₃ | 9.5 || Na₃PO₄ | 11.9 || Na₂CO₃ | 11.0 |### Explanation:1. **H₂O (unboiled)**: - pH: 3.5 - Unboiled water appears to be acidic.2. **H₂O (boiled)**: - pH: 7.0 - Boiled water has a neutral pH.3. **NaCl (Sodium Chloride)**: - pH: 7.0 - Sodium chloride solution is neutral.4. **NaC₂H₃O₂ (Sodium Acetate)**: - pH: 9.1 - Sodium acetate solution is basic.5. **NH₄Cl (Ammonium Chloride)**: - pH: 4.5 - Ammonium chloride solution is acidic.6. **NaHCO₃ (Sodium Bicarbonate)**: - pH: 9.5 - Sodium bicarbonate solution is basic.7. **Na₃PO₄ (Sodium Phosphate)**: - pH: 11.9 - Sodium phosphate solution is strongly basic.8. **Na₂CO₃ (Sodium Carbonate)**: - pH: 11.0 - Sodium carbonate solution is strongly basic.This data can be useful in educational contexts, for example, in chemistry experiments and practical lessons to demonstrate the properties of acids, bases, and neutral solutions. **Lab Report #2-2-3:****0.1 M Na₂CO₃ solution, using the given pH data, write expression for equilibrium constant (Ka or Kb):**- ○ Kb = [HCO₃⁻] [OH⁻] / [CO₃²⁻]- ○ Ka = [H₂CO₃] [OH⁻] / [CO₃²⁻]- ○ Ka = [HCO₃⁻] [OH⁻] / [CO₃²⁻]- ○ Kb = [H₂CO₃] [OH⁻] / [CO₃²⁻]

As the pH of Na2CO3 is 11.0 which means that it is basic in nature.

Answered: 0.1 M Na2CO3 solution, using the given…

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0.1 M Na2CO3 solution, using the given pH data, write expression for equilibrium constant (Ka or Kb):

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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Question

### Table of Solution pH Values

The following table provides the pH values of various solutions after performing specific treatments. The pH scale is used to determine the acidity or basicity of a solution, with lower values indicating higher acidity and higher values indicating higher basicity.

| Solutions | pH values |
|----------------------|-----------|
| H₂O (unboiled) | 3.5 |
| H₂O (boiled) | 7.0 |
| NaCl | 7.0 |
| NaC₂H₃O₂ | 9.1 |
| NH₄Cl | 4.5 |
| NaHCO₃ | 9.5 |
| Na₃PO₄ | 11.9 |
| Na₂CO₃ | 11.0 |

### Explanation:

1. **H₂O (unboiled)**:
- pH: 3.5
- Unboiled water appears to be acidic.

2. **H₂O (boiled)**:
- pH: 7.0
- Boiled water has a neutral pH.

3. **NaCl (Sodium Chloride)**:
- pH: 7.0
- Sodium chloride solution is neutral.

4. **NaC₂H₃O₂ (Sodium Acetate)**:
- pH: 9.1
- Sodium acetate solution is basic.

5. **NH₄Cl (Ammonium Chloride)**:
- pH: 4.5
- Ammonium chloride solution is acidic.

6. **NaHCO₃ (Sodium Bicarbonate)**:
- pH: 9.5
- Sodium bicarbonate solution is basic.

7. **Na₃PO₄ (Sodium Phosphate)**:
- pH: 11.9
- Sodium phosphate solution is strongly basic.

8. **Na₂CO₃ (Sodium Carbonate)**:
- pH: 11.0
- Sodium carbonate solution is strongly basic.

This data can be useful in educational contexts, for example, in chemistry experiments and practical lessons to demonstrate the properties of acids, bases, and neutral solutions.

**Lab Report #2-2-3:**

**0.1 M Na₂CO₃ solution, using the given pH data, write expression for equilibrium constant (Ka or Kb):**

- ○ Kb = [HCO₃⁻] [OH⁻] / [CO₃²⁻]
- ○ Ka = [H₂CO₃] [OH⁻] / [CO₃²⁻]
- ○ Ka = [HCO₃⁻] [OH⁻] / [CO₃²⁻]
- ○ Kb = [H₂CO₃] [OH⁻] / [CO₃²⁻]

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