1. What is Normality?

Normality (N) is a measure of concentration that expresses the number of equivalents of solute per liter of solution. It's particularly useful in acid-base and redox reactions where the concept of equivalents is important.

2. How Does the Calculator Work?

The calculator uses the normality equation:

Where:

• \( N \) — Normality (equivalents per liter)
• \( mass \) — Mass of solute in grams
• \( EW \) — Equivalent weight of solute (g/equivalent)
• \( V \) — Volume of solution in liters

Explanation: The equation calculates how many equivalents of solute are present in each liter of solution.

3. Importance of Normality Calculation

Details: Normality is crucial in stoichiometric calculations for acid-base and redox reactions, where the concept of equivalents is more relevant than moles.

4. Using the Calculator

Tips: Enter mass in grams, equivalent weight in g/equivalent, and volume in liters. All values must be positive numbers.

5. Frequently Asked Questions (FAQ)

Q1: What's the difference between molarity and normality?
A: Molarity is moles per liter while normality is equivalents per liter. Normality accounts for reactive capacity in specific reactions.

Q2: How do I determine equivalent weight?
A: For acids, EW = molar mass / H+ ions donated. For bases, EW = molar mass / OH- ions donated. For redox, EW = molar mass / electrons transferred.

Q3: When should I use normality instead of molarity?
A: Use normality for acid-base titrations, redox reactions, and precipitation reactions where equivalents are important.

Q4: Can normality be greater than molarity?
A: Yes, if each molecule can donate/accept multiple equivalents (e.g., H2SO4 has normality = 2 × molarity in acid-base reactions).

Q5: Is normality temperature dependent?
A: Like molarity, normality is slightly temperature dependent because volume changes with temperature, but this is usually negligible for dilute solutions.