Neutralisering

Neutralisering, or neutralisation, is the process by which the acidity or basicity of a solution is reduced by a reaction between an acid and a base. The net result is the formation of a salt and water, moving the mixture toward a more neutral pH. The term is used in chemistry as well as in other contexts where substances are rendered less reactive or active.

In chemistry, acid-base neutralization is the most common form. A typical reaction is HA + BOH → AB + H2O, where an acid (HA) and a base (BOH) react to give a salt (AB) and water. Neutralization is usually exothermic. The equivalence point is reached when the amounts of acid and base are stoichiometrically equal; the pH at this point depends on the strengths of the reacting acids and bases. For strong acids and bases, the equivalence point is near pH 7, while weak acids or bases yield different pH values at equivalence. Titration and pH monitoring are standard methods to study and utilize neutralization.

Applications span laboratory work and industry. In environmental and wastewater treatment, neutralization is used to adjust pH, for example by adding lime to acidic mine drainage, which can also precipitate dissolved metals as hydroxides. In food processing and cleaning, neutralization helps control acidity and corrosion. It is important to manage heat release and salt formation, as these can influence solution properties and safety.

Neutralization also appears in biology and medicine, where it describes the inactivation of pathogens by antibodies. Neutralizing antibodies block infection, and neutralization assays assess immune protection or therapeutic efficacy.

See also: acid-base reaction, pH, titration, buffer.