What is the Normality of a 0.5 solution of H2SO4. Use the equation M × valence

To calculate the normality (N) of a solution using the formula \( N = M \times \text{valence} \), where:

- \( M \) is the molarity of the solution.
- The valence (also known as the equivalence factor) is the number of hydrogen ions (H⁺) or hydroxide ions (OH⁻) that the acid or base can donate or accept in a reaction.

For sulfuric acid (H₂SO₄), it can donate two hydrogen ions (H⁺), so the valence is 2.

Given:
- Molarity \( M = 0.5 \, \text{M} \)
- Valence \( = 2 \)

Now, using the formula:
\[
N = 0.5 \, \text{M} \times 2 = 1.0 \, \text{N}
\]

So, the normality of the 0.5 M solution of H₂SO₄ is 1.0 N.

Would you like more details or have any questions?

Here are 5 related questions for you:
1. How do you determine the valence of other acids or bases?
2. What is the normality of a 0.25 M solution of H₂SO₄?
3. How would you calculate the normality of a base like NaOH?
4. What is the significance of normality in titration experiments?
5. How does normality differ from molarity in chemical reactions?

**Tip:** Normality is especially useful in titration because it directly relates to the reactive capacity of a solution.

Learn how to calculate the normality of a 0.5 M sulfuric acid (H₂SO₄) solution using the normality formula. Understand the concept of valence in acid-base chemistry and its role in determining normality. Suitable for advanced chemistry students in Grades 11-12.

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