A beaker contains 100. mL of the buffer solution. What is the resulting pH when 50.0 mL of 0.4 M HNO3 is added to the buffer? H₂PO; HPO2- 0.50 M; 0.50 M Кан,род pH after strong acid added = [?] = 6.23 x 10-8 pH of Soln w/ Acid Enter
A beaker contains 100. mL of the buffer solution. What is the resulting pH when 50.0 mL of 0.4 M HNO3 is added to the buffer? H₂PO; HPO2- 0.50 M; 0.50 M Кан,род pH after strong acid added = [?] = 6.23 x 10-8 pH of Soln w/ Acid Enter
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
Chapter1: Chemical Foundations
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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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### Buffer Solution pH Calculation Problem
**Problem Statement:**
A beaker contains 100. mL of the buffer solution. What is the resulting pH when 50.0 mL of 0.4 M HNO₃ is added to the buffer?
Buffer Components and Concentrations:
- \( \text{H}_2\text{PO}_4^- \)
- \( \text{HPO}_4^{2-} \)
- Concentrations: 0.50 M for both components.
Acid Dissociation Constant:
\[ K_{\text{a}_{\text{H}_2\text{PO}_4^-}} = 6.23 \times 10^{-8} \]
**Objective:**
Determine the pH after the strong acid (HNO₃) is added to the buffer.
**Given Equation:**
\[ \text{pH after strong acid added} = \;? \]
**Interactive Element:**
- *Text Box:* "pH of Soln w/ Acid"
- *Button:* "Enter"
**Explanation for Calculation Approach:**
1. **Determine the moles of HNO₃ added:**
\[ \text{Moles of HNO₃} = 0.4 \, \text{M} \times 50.0 \, \text{mL} = 0.4 \, \text{M} \times 0.050 \, \text{L} \]
2. **Calculate the initial moles of phosphate species in the buffer before the acid is added.**
3. **Use the moles of HNO₃ to determine the new equilibrium concentrations of \( \text{H}_2\text{PO}_4^- \) and \( \text{HPO}_4^{2-} \).**
4. **Apply the Henderson-Hasselbalch equation to find the new pH of the solution:**
\[ \text{pH} = \text{pKa} + \log \left( \frac{[\text{base}]}{[\text{acid}]} \right) \]
Where,
\[ \text{pKa} = -\log K_{\text{a}_{\text{H}_2\text{PO}_4^-}} \]
This example demonstrates the effect of adding a strong acid to a buffered system](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F74ff972a-42b6-478c-a012-297da9a07acf%2Ffd49b4e1-34ee-44d5-bd0b-af040b59ba13%2Ffjjl2as_processed.jpeg&w=3840&q=75)
Transcribed Image Text:---
### Buffer Solution pH Calculation Problem
**Problem Statement:**
A beaker contains 100. mL of the buffer solution. What is the resulting pH when 50.0 mL of 0.4 M HNO₃ is added to the buffer?
Buffer Components and Concentrations:
- \( \text{H}_2\text{PO}_4^- \)
- \( \text{HPO}_4^{2-} \)
- Concentrations: 0.50 M for both components.
Acid Dissociation Constant:
\[ K_{\text{a}_{\text{H}_2\text{PO}_4^-}} = 6.23 \times 10^{-8} \]
**Objective:**
Determine the pH after the strong acid (HNO₃) is added to the buffer.
**Given Equation:**
\[ \text{pH after strong acid added} = \;? \]
**Interactive Element:**
- *Text Box:* "pH of Soln w/ Acid"
- *Button:* "Enter"
**Explanation for Calculation Approach:**
1. **Determine the moles of HNO₃ added:**
\[ \text{Moles of HNO₃} = 0.4 \, \text{M} \times 50.0 \, \text{mL} = 0.4 \, \text{M} \times 0.050 \, \text{L} \]
2. **Calculate the initial moles of phosphate species in the buffer before the acid is added.**
3. **Use the moles of HNO₃ to determine the new equilibrium concentrations of \( \text{H}_2\text{PO}_4^- \) and \( \text{HPO}_4^{2-} \).**
4. **Apply the Henderson-Hasselbalch equation to find the new pH of the solution:**
\[ \text{pH} = \text{pKa} + \log \left( \frac{[\text{base}]}{[\text{acid}]} \right) \]
Where,
\[ \text{pKa} = -\log K_{\text{a}_{\text{H}_2\text{PO}_4^-}} \]
This example demonstrates the effect of adding a strong acid to a buffered system
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