Normality, given the symbol N, is closely related to molarity but counts reactive units instead of whole molecules. An equivalent is the amount of a substance that supplies or reacts with one mole of a defined reacting unit, usually one mole of hydrogen ions in acid-base chemistry or one mole of electrons in redox chemistry. Normality equals molarity multiplied by the number of equivalents each formula unit provides.
The number of equivalents depends on the reaction. For acids, it is the number of hydrogen ions that can be donated. Hydrochloric acid, HCl, donates one proton, so its normality equals its molarity.
Sulfuric acid, H2SO4, can donate two protons, so a 1 molar solution is 2 normal. For redox reagents, the number of equivalents is the number of electrons gained or lost per formula unit.
Normality is convenient in titrations because equivalents react in a simple one-to-one manner. At the equivalence point, the number of equivalents of acid equals the number of equivalents of base. This leads to the compact relationship N times V for the acid equals N times V for the base, which lets an analyst find an unknown concentration with one quick calculation.
Despite its convenience, normality has a drawback: it is not a fixed property of a solution. Because the number of equivalents depends on the specific reaction, the same solution can have different normalities in different reactions. For this reason, modern practice usually prefers molarity, which does not change with context.
Still, normality remains common in titration work, water testing, and clinical labs where reactive capacity is what matters.