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To solve the problem of determining the concentration of sulfuric acid remaining after neutralization, we need to follow these steps:

1. **Write the balanced chemical equation:**
   \[ \text{H}_2\text{SO}_4 + 2\text{KOH} \rightarrow \text{K}_2\text{SO}_4 + 2\text{H}_2\text{O} \]

2. **Calculate the moles of \(\text{H}_2\text{SO}_4\) and \(\text{KOH}\):**
   - Moles of \(\text{H}_2\text{SO}_4\):
     \[ \text{Moles of H}_2\text{SO}_4 = 0.950 \, \text{L} \times 0.470 \, \text{M} = 0.4465 \, \text{moles} \]
   - Moles of \(\text{KOH}\):
     \[ \text{Moles of KOH} = 0.900 \, \text{L} \times 0.280 \, \text{M} = 0.252 \, \text{moles} \]

3. **Determine the limiting reagent:**
   From the balanced equation, 1 mole of \(\text{H}_2\text{SO}_4\) reacts with 2 moles of \(\text{KOH}\). 
   - Moles of \(\text{KOH}\) required to react with all of \(\text{H}_2\text{SO}_4\):
     \[ 0.4465 \, \text{moles H}_2\text{SO}_4 \times 2 = 0.893 \, \text{moles KOH} \]

   Since we only have 0.252 moles of \(\text{KOH}\), \(\text{KOH}\) is the limiting reagent.

4. **Calculate the amount of \(\text{H}_2\text{SO}_4\) that reacts:**
   - Moles of \(\text{H}_2\text{SO}_4\) that react with 0.252 moles of \(\text{KOH}\):
     \[ \frac{0.252 \, \text{moles KOH}}{2} = 0.126 \, \text{moles H}_2\text{SO}_4 \]

5. **Calculate the remaining moles of \(\text{H}_2\text{SO}_4\):**
   \[ 0.4465 \, \text{moles H}_2\text{SO}_4 - 0.126 \, \text{moles H}_2\text{SO}_4 = 0.3205 \, \text{moles H}_2\text{SO}_4 \]

6. **Calculate the total volume of the solution after mixing:**
   \[ 0.950 \, \text{L} + 0.900 \, \text{L} = 1.850 \, \text{L} \]

7. **Calculate the concentration of the remaining \(\text{H}_2\text{SO}_4\):**
   \[ \text{Concentration} = \frac{0.3205 \, \text{moles H}_2\text{SO}_4}{1.850 \, \text{L}} = 0.1732 \, \text{M} \]

Therefore, the concentration of sulfuric acid remaining after neutralization is **0.1732 M**.

Would you like more details on any part of this process or have any questions?

Here are five relative questions to expand your understanding:
1. How do you determine the limiting reagent in a chemical reaction?
2. What is the significance of the stoichiometric coefficients in a balanced chemical equation?
3. How does the concept of molarity help in calculating concentrations in reactions?
4. What are the steps to calculate the remaining concentration of a reactant in a neutralization reaction?
5. Can you provide another example where you need to calculate the concentration of a reactant after a reaction?

**Tip:** Always ensure the chemical equation is balanced before performing any calculations, as the stoichiometric coefficients are crucial for accurate computations.

Suppose 0.950 L of 0.470 M H2SO4 is mixed with 0.900 L of 0.280 M KOH. What concentration of sulfuric acid remains after neutralization?

Find out how to calculate the concentration of sulfuric acid remaining after a neutralization reaction between 0.950 L of 0.470 M H2SO4 and 0.900 L of 0.280 M KOH. This problem involves key concepts in stoichiometry and molarity calculations, making it suitable for Grades 10-12.

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