1. What is Normality?

Normality (N) is a measure of concentration equal to the gram equivalent weight per liter of solution. For NaOH, normality equals molarity because each mole of NaOH provides one equivalent of OH⁻ ions.

2. How Does the Calculator Work?

The calculator uses the simple equation:

Where:

• \( N \) — Normality (eq/L)
• \( M \) — Molarity (mol/L)

Explanation: Since NaOH has one reactive hydroxide group per molecule, its normality is numerically equal to its molarity.

3. Importance of Normality Calculation

Details: Normality is particularly important in acid-base chemistry as it accounts for the number of reactive units in solution, making it useful for titration calculations.

4. Using the Calculator

Tips: Enter the molarity of your NaOH solution in mol/L. The calculator will automatically compute the normality.

5. Frequently Asked Questions (FAQ)

Q1: Why is normality equal to molarity for NaOH?
A: Because NaOH has only one hydroxide group (OH⁻) that can react with H⁺ ions, so each mole provides one equivalent.

Q2: When should I use normality vs molarity?
A: Use normality for acid-base reactions and titrations, while molarity is more general for stoichiometric calculations.

Q3: Does this work for other bases?
A: No, this simple 1:1 relationship only applies to monoprotic bases like NaOH. For bases like Ca(OH)₂, the factor would be 2.

Q4: What are typical NaOH normality values?
A: Common lab solutions range from 0.1N to 1N, though concentrated NaOH can be up to 19N.

Q5: How precise should my measurement be?
A: For most applications, 2-3 significant figures are sufficient, but analytical work may require higher precision.