Normality and Equivalents Calculator
Calculate normality, equivalents, and equivalent weight for acids, bases, and redox reagents.
Includes N₁V₁ = N₂V₂ for volumetric analysis.
Normality (N) is a concentration unit that accounts for the reactive capacity of a substance.
Definition:
N = M × n_eq
where M = molarity and n_eq = number of equivalents per mole (the “n-factor”).
Equivalent weight:
Eq. weight = Molar mass / n_eq
Equivalents:
Equivalents = mass / Eq. weight = mass × n_eq / M
N-factor (n_eq) for different reaction types:
- Acids: n_eq = number of H⁺ ions donated per formula unit
- HCl: n_eq = 1, H₂SO₄: n_eq = 2, H₃PO₄: n_eq = 3
- Bases: n_eq = number of OH⁻ ions per formula unit
- NaOH: n_eq = 1, Ca(OH)₂: n_eq = 2, Al(OH)₃: n_eq = 3
- Redox: n_eq = change in oxidation state × number of atoms
- KMnO₄ in acid (Mn goes from +7 to +2): n_eq = 5
- K₂Cr₂O₇ (Cr goes from +6 to +3, two Cr atoms): n_eq = 6
Volumetric analysis formula:
N₁V₁ = N₂V₂
This is the fundamental equation for acid-base and redox titrations. At the equivalence point, equivalents of acid = equivalents of base.
Normality vs Molarity: Normality is older and less commonly used in modern chemistry. However, it remains useful in medical/clinical labs (e.g., serum electrolytes in mEq/L) and in some titrimetric analyses.
Example: 1 L of 1 M H₂SO₄ contains 1 mole of H₂SO₄ but 2 equivalents of H⁺. Therefore N = 2 N. It will neutralize 2 L of 1 N NaOH (N₁V₁ = 2×1 = N₂V₂ = 1×2).