Normality
| Formula / Notation | N = (equivalents/L) = M × n; N = molarity × number of reactive units |
|---|---|
| Also Known As | Normal concentration, N (normality), equivalent concentration |
What is Normality?
A concentration unit defined as the number of equivalents of solute per liter of solution (N = eq/L). For acids, one equivalent contains one mole of H⁺; for bases, one equivalent contains one mole of OH⁻. Normality is useful in titration calculations where stoichiometry varies.
Formula & Notation
Other Names / Synonyms: Normal concentration, N (normality), equivalent concentration
Properties & Characteristics
Uses & Applications
Safety Information
Always consult the SDS/MSDS before handling any chemical. This information is for educational purposes only.
Key Facts
Frequently Asked Questions
A concentration unit defined as the number of equivalents of solute per liter of solution (N = eq/L). For acids, one equivalent contains one mole of H⁺; for bases, one equivalent contains one mole of OH⁻. Normality is useful in titration calculations where stoichiometry varies.
Normality is used in: titrimetric analysis (acid-base, redox, precipitation titrations), standardisation of solutions, pharmacology (expressing concentration of polyvalent electrolytes in blood: mEq/L = mmol/L × valence), and in industrial chemical specifications (normality of sodium hydroxide solut…
Normality can be misleading if the context of n is not specified (n depends on the reaction type). A 1 N H₂SO₄ solution (0.5 M) is less concentrated and less corrosive than 1 M H₂SO₄. Always specify the reaction context when using normality. Modern practice increasingly uses molarity for clarity.
The formula or notation for Normality is: N = (equivalents/L) = M × n; N = molarity × number of reactive units