What is the pH of 1.00 L of a buffer that is 0.120 Mnitrous acid (HNO2) and 0.150 MNANO2? (pKa of HNO2 = 3.40) 1st attempt See Periodic Table pH =
What is the pH of 1.00 L of a buffer that is 0.120 Mnitrous acid (HNO2) and 0.150 MNANO2? (pKa of HNO2 = 3.40) 1st attempt See Periodic Table pH =
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 Statement:**
Calculate the pH of 1.00 L of a buffer solution containing 0.120 M nitrous acid \((\text{HNO}_2)\) and 0.150 M sodium nitrite \((\text{NaNO}_2)\). Given that the \(pK_a\) of \(\text{HNO}_2\) is 3.40.
**Solution:**
1. **Components of the Buffer:**
- **Weak acid:** Nitrous acid \((\text{HNO}_2)\)
- **Conjugate base:** Sodium nitrite \((\text{NaNO}_2)\)
2. **Henderson-Hasselbalch Equation:**
\[
\text{pH} = pK_a + \log \left(\frac{[\text{Conjugate base}]}{[\text{Weak acid}]}\right)
\]
3. **Substitute Values:**
- \( pK_a = 3.40 \)
- \([\text{HNO}_2] = 0.120 \, M\)
- \([\text{NaNO}_2] = 0.150 \, M\)
4. **Calculations:**
\[
\text{pH} = 3.40 + \log \left(\frac{0.150}{0.120}\right)
\]
5. **Interactive Component:**
- Enter the calculated pH value in the blank provided.
**Graph/Diagram Explanation:**
None present in the image.
For further reference, use the "See Periodic Table" link provided to view element details as needed.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdc588db3-fded-406e-895e-07daf210bf42%2Faeb645b2-81a5-44de-b805-7df9aeaf7d1f%2F6d9nacw_processed.png&w=3840&q=75)
Transcribed Image Text:**Buffer Solution pH Calculation**
**Problem Statement:**
Calculate the pH of 1.00 L of a buffer solution containing 0.120 M nitrous acid \((\text{HNO}_2)\) and 0.150 M sodium nitrite \((\text{NaNO}_2)\). Given that the \(pK_a\) of \(\text{HNO}_2\) is 3.40.
**Solution:**
1. **Components of the Buffer:**
- **Weak acid:** Nitrous acid \((\text{HNO}_2)\)
- **Conjugate base:** Sodium nitrite \((\text{NaNO}_2)\)
2. **Henderson-Hasselbalch Equation:**
\[
\text{pH} = pK_a + \log \left(\frac{[\text{Conjugate base}]}{[\text{Weak acid}]}\right)
\]
3. **Substitute Values:**
- \( pK_a = 3.40 \)
- \([\text{HNO}_2] = 0.120 \, M\)
- \([\text{NaNO}_2] = 0.150 \, M\)
4. **Calculations:**
\[
\text{pH} = 3.40 + \log \left(\frac{0.150}{0.120}\right)
\]
5. **Interactive Component:**
- Enter the calculated pH value in the blank provided.
**Graph/Diagram Explanation:**
None present in the image.
For further reference, use the "See Periodic Table" link provided to view element details as needed.
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