**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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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 =

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Chapter1: Chemical Foundations

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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

**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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