**Lab Report #6-2-2:****Objective:**Determine the net-ionic equation for the hydrolysis of a 0.1 M Na₃PO₄ solution.**Instructions:**Using the given pH data, write the net-ionic equation for the hydrolysis reaction.**Options:**1. \( \text{Na}_3\text{PO}_4 + \text{H}_2\text{O} \leftrightarrow \text{Na}^+ + \text{HPO}_4^{2-} + \text{OH}^- \)2. \( \text{PO}_4^{3-} + \text{H}^+ \leftrightarrow \text{HPO}_4^{2-} \)3. \( \text{PO}_4^{3-} + \text{H}_2\text{O} \leftrightarrow \text{HPO}_4^{2-} + \text{OH}^- \)**Discussion of Options:**- Option 1 considers the complete dissociation of \( \text{Na}_3\text{PO}_4 \) in water followed by the interaction with water resulting in the formation of ions.- Option 2 describes the reaction of phosphate ions with hydrogen ions to form hydrogen phosphate, which does not represent the hydrolysis phenomenon.- Option 3 describes the hydrolysis process where the phosphate ion reacts with water to produce hydrogen phosphate and hydroxide ions.**Conclusion:**The correct net-ionic equation for the hydrolysis of a 0.1 M Na₃PO₄ solution, given the pH data, is represented by:\[ \text{PO}_4^{3-} + \text{H}_2\text{O} \leftrightarrow \text{HPO}_4^{2-} + \text{OH}^- \] ### pH Values of Different Solutions| 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 |This table lists the pH values of various solutions. 1. **H₂O (unboiled) has a pH of 3.5** - Unboiled water typically holds dissolved carbon dioxide, which forms carbonic acid, lowering the pH. 2. **H₂O (boiled) has a pH of 7.0** - Boiling water drives off dissolved gases such as carbon dioxide, bringing the pH to neutral.3. **NaCl has a pH of 7.0** - Sodium chloride (table salt) in solution is neutral and does not affect the pH of water.4. **NaC₂H₃O₂ has a pH of 9.1** - Sodium acetate is a salt of a weak acid and a strong base, resulting in a slightly basic solution.5. **NH₄Cl has a pH of 4.5** - Ammonium chloride dissolves in water to form a weak acid, lowering the pH.6. **NaHCO₃ has a pH of 9.5** - Sodium bicarbonate is mildly basic, often used as an antacid to neutralize stomach acid.7. **Na₃PO₄ has a pH of 11.9** - Sodium phosphate is strongly basic.8. **Na₂CO₃ has a pH of 11.0** - Sodium carbonate, also known as washing soda, is strongly basic and raises the pH of solutions.Understanding the pH values of different chemicals is crucial in various applications, such as chemistry experiments, pharmaceuticals, and even everyday household uses.

As the pH of Na3PO4 is 11.9 which indicates that it is basic in nature

Answered: 0.1 M NagPO4 solution, using the given…

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0.1 M NagPO4 solution, using the given pH data, write net-ionic equation for hydrolysis:

Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

**Lab Report #6-2-2:**

**Objective:**
Determine the net-ionic equation for the hydrolysis of a 0.1 M Na₃PO₄ solution.

**Instructions:**
Using the given pH data, write the net-ionic equation for the hydrolysis reaction.

**Options:**
1. \( \text{Na}_3\text{PO}_4 + \text{H}_2\text{O} \leftrightarrow \text{Na}^+ + \text{HPO}_4^{2-} + \text{OH}^- \)
2. \( \text{PO}_4^{3-} + \text{H}^+ \leftrightarrow \text{HPO}_4^{2-} \)
3. \( \text{PO}_4^{3-} + \text{H}_2\text{O} \leftrightarrow \text{HPO}_4^{2-} + \text{OH}^- \)

**Discussion of Options:**
- Option 1 considers the complete dissociation of \( \text{Na}_3\text{PO}_4 \) in water followed by the interaction with water resulting in the formation of ions.
- Option 2 describes the reaction of phosphate ions with hydrogen ions to form hydrogen phosphate, which does not represent the hydrolysis phenomenon.
- Option 3 describes the hydrolysis process where the phosphate ion reacts with water to produce hydrogen phosphate and hydroxide ions.

**Conclusion:**
The correct net-ionic equation for the hydrolysis of a 0.1 M Na₃PO₄ solution, given the pH data, is represented by:
\[ \text{PO}_4^{3-} + \text{H}_2\text{O} \leftrightarrow \text{HPO}_4^{2-} + \text{OH}^- \]

### pH Values of Different Solutions

| 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 |

This table lists the pH values of various solutions.

1. **H₂O (unboiled) has a pH of 3.5** - Unboiled water typically holds dissolved carbon dioxide, which forms carbonic acid, lowering the pH.

2. **H₂O (boiled) has a pH of 7.0** - Boiling water drives off dissolved gases such as carbon dioxide, bringing the pH to neutral.

3. **NaCl has a pH of 7.0** - Sodium chloride (table salt) in solution is neutral and does not affect the pH of water.

4. **NaC₂H₃O₂ has a pH of 9.1** - Sodium acetate is a salt of a weak acid and a strong base, resulting in a slightly basic solution.

5. **NH₄Cl has a pH of 4.5** - Ammonium chloride dissolves in water to form a weak acid, lowering the pH.

6. **NaHCO₃ has a pH of 9.5** - Sodium bicarbonate is mildly basic, often used as an antacid to neutralize stomach acid.

7. **Na₃PO₄ has a pH of 11.9** - Sodium phosphate is strongly basic.

8. **Na₂CO₃ has a pH of 11.0** - Sodium carbonate, also known as washing soda, is strongly basic and raises the pH of solutions.

Understanding the pH values of different chemicals is crucial in various applications, such as chemistry experiments, pharmaceuticals, and even everyday household uses.

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