2. A buffer solution of volume 0.500 L contains 1.68 g NH3 and 4.05 g (NH);SOu. a) What is the pH of this solution? b) If 0.88 g NAOH is added to the solution, what will be the pH?
2. A buffer solution of volume 0.500 L contains 1.68 g NH3 and 4.05 g (NH);SOu. a) What is the pH of this solution? b) If 0.88 g NAOH is added to the solution, what will be the pH?
Chemistry
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Chapter1: Chemical Foundations
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I just need help on questions 2 and 3.
Transcribed Image Text:**Problem 2: Buffer Solution Chemistry**
A buffer solution of volume 0.500 L contains 1.68 g NH₃ and 4.05 g (NH₄)₂SO₄.
a) What is the pH of this solution?
b) If 0.88 g NaOH is added to the solution, what will be the pH?
**Explanation:**
- **Part a)** involves calculating the initial pH of a buffer solution, which consists of a weak base (NH₃) and its conjugate acid (NH₄⁺ from (NH₄)₂SO₄).
- **Part b)** requires determining the new pH after the addition of NaOH, a strong base, which will react with the NH₄⁺ ions, altering the buffer capacity.
This problem helps in understanding the application of the Henderson-Hasselbalch equation and the concept of buffer solutions in chemical equilibria.
![**Educational Content: pH Calculations and Acid-Base Equilibria**
1. **Buffer Solution Problem:**
- A buffer solution with a volume of 0.500 L contains 1.68 g of NH₃ and 4.05 g of (NH₄)₂SO₄.
- **a)** Determine the pH of this solution.
- **b)** If 0.88 g of NaOH is added to the solution, calculate the new pH.
2. **Propionic Acid Adjustment Problem:**
- You have 250.0 mL of 0.100 M CH₃CH₂COOH (propionic acid, Kₐ = 1.35 × 10⁻⁵).
- You need to adjust the pH by adding an appropriate solution:
- **a)** What volume of 1.00 M HCl is needed to lower the pH to 1.00?
- **b)** What volume of 1.00 M CH₃CH₂COONa is needed to raise the pH to 4.00?
3. **Titration Problem:**
- Determine the pH at each of the following points in the titration of 25.00 mL of 0.100 M CH₃CH₂COOH with 0.100 M NaOH:
- **a)** Before the addition of any NaOH.
- **b)** After the addition of 10.00 mL of 0.100 M NaOH.
- **c)** After the addition of 12.50 mL of 0.100 M NaOH.
- **d)** After the addition of 25.00 mL of 0.100 M NaOH.
- **e)** After the addition of 26.00 mL of 0.100 M NaOH.
4. **Sodium Phosphate Problem:**
- Sodium phosphate, Na₃PO₄, is used as a cleaning agent.
- What is the pH of 1.0 M Na₃PO₄ (aq)? [Refer to Table 7.4 "Stepwise Dissociation Constants for Several Common Polyprotic Acids."]
5. **Acidity and Basicity:**
- **a)** Is a 0.10 M solution of Na₂S](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbecc57bd-691c-44b9-b5ef-c7430b91fff8%2F1ce99540-9efd-4070-aa53-896279af1b83%2Fphqo4f_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Educational Content: pH Calculations and Acid-Base Equilibria**
1. **Buffer Solution Problem:**
- A buffer solution with a volume of 0.500 L contains 1.68 g of NH₃ and 4.05 g of (NH₄)₂SO₄.
- **a)** Determine the pH of this solution.
- **b)** If 0.88 g of NaOH is added to the solution, calculate the new pH.
2. **Propionic Acid Adjustment Problem:**
- You have 250.0 mL of 0.100 M CH₃CH₂COOH (propionic acid, Kₐ = 1.35 × 10⁻⁵).
- You need to adjust the pH by adding an appropriate solution:
- **a)** What volume of 1.00 M HCl is needed to lower the pH to 1.00?
- **b)** What volume of 1.00 M CH₃CH₂COONa is needed to raise the pH to 4.00?
3. **Titration Problem:**
- Determine the pH at each of the following points in the titration of 25.00 mL of 0.100 M CH₃CH₂COOH with 0.100 M NaOH:
- **a)** Before the addition of any NaOH.
- **b)** After the addition of 10.00 mL of 0.100 M NaOH.
- **c)** After the addition of 12.50 mL of 0.100 M NaOH.
- **d)** After the addition of 25.00 mL of 0.100 M NaOH.
- **e)** After the addition of 26.00 mL of 0.100 M NaOH.
4. **Sodium Phosphate Problem:**
- Sodium phosphate, Na₃PO₄, is used as a cleaning agent.
- What is the pH of 1.0 M Na₃PO₄ (aq)? [Refer to Table 7.4 "Stepwise Dissociation Constants for Several Common Polyprotic Acids."]
5. **Acidity and Basicity:**
- **a)** Is a 0.10 M solution of Na₂S
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