A 25.0 mL solution of HNO3 is neutralized with 25.4 mL of 0.250 M Ba(OH)2. What is the concentration of the original HNO3 solution?

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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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**Problem Statement:**  
A 25.0 mL solution of HNO₃ is neutralized with 25.4 mL of 0.250 M Ba(OH)₂. What is the concentration of the original HNO₃ solution?

**Explanation:**

To solve this problem, we need to use the concept of neutralization and the balanced chemical equation between HNO₃ and Ba(OH)₂:

\[ 2 \, \text{HNO}_3 + \text{Ba(OH)}_2 \rightarrow \text{Ba(NO}_3)_2 + 2 \, \text{H}_2\text{O} \]

### Steps to Solve:

1. **Calculate Moles of Ba(OH)₂:**
   - Volume of Ba(OH)₂ = 25.4 mL = 0.0254 L
   - Molarity of Ba(OH)₂ = 0.250 M
   
   \[
   \text{Moles of Ba(OH)₂} = \text{Molarity} \times \text{Volume} = 0.250 \, \text{mol/L} \times 0.0254 \, \text{L} = 0.00635 \, \text{mol}
   \]

2. **Use Stoichiometry to Determine Moles of HNO₃:**
   - According to the balanced equation, 1 mole of Ba(OH)₂ reacts with 2 moles of HNO₃.
   
   \[
   \text{Moles of HNO₃} = 0.00635 \, \text{mol Ba(OH)₂} \times 2 = 0.0127 \, \text{mol HNO₃}
   \]

3. **Calculate the Concentration of HNO₃:**
   - Volume of HNO₃ = 25.0 mL = 0.025 L
   
   \[
   \text{Concentration of HNO₃} = \frac{\text{Moles of HNO₃}}{\text{Volume of HNO₃}} = \frac{0.0127 \, \text{mol}}{0.025 \, \text{L}} = 0.508 \, \text{M}
   \]

**Summary:**

The
Transcribed Image Text:**Problem Statement:** A 25.0 mL solution of HNO₃ is neutralized with 25.4 mL of 0.250 M Ba(OH)₂. What is the concentration of the original HNO₃ solution? **Explanation:** To solve this problem, we need to use the concept of neutralization and the balanced chemical equation between HNO₃ and Ba(OH)₂: \[ 2 \, \text{HNO}_3 + \text{Ba(OH)}_2 \rightarrow \text{Ba(NO}_3)_2 + 2 \, \text{H}_2\text{O} \] ### Steps to Solve: 1. **Calculate Moles of Ba(OH)₂:** - Volume of Ba(OH)₂ = 25.4 mL = 0.0254 L - Molarity of Ba(OH)₂ = 0.250 M \[ \text{Moles of Ba(OH)₂} = \text{Molarity} \times \text{Volume} = 0.250 \, \text{mol/L} \times 0.0254 \, \text{L} = 0.00635 \, \text{mol} \] 2. **Use Stoichiometry to Determine Moles of HNO₃:** - According to the balanced equation, 1 mole of Ba(OH)₂ reacts with 2 moles of HNO₃. \[ \text{Moles of HNO₃} = 0.00635 \, \text{mol Ba(OH)₂} \times 2 = 0.0127 \, \text{mol HNO₃} \] 3. **Calculate the Concentration of HNO₃:** - Volume of HNO₃ = 25.0 mL = 0.025 L \[ \text{Concentration of HNO₃} = \frac{\text{Moles of HNO₃}}{\text{Volume of HNO₃}} = \frac{0.0127 \, \text{mol}}{0.025 \, \text{L}} = 0.508 \, \text{M} \] **Summary:** The
Expert Solution
Step 1: Given :

Volume of HNO3 = 25.0 ml 

Volume of Ba(OH)2 = 25.4 ml

molarity of Ba(OH)2 = 0.250 M

We need to calculate the concentration of the original HNO3 solution.

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