Neutralization

Neutralization is a reaction in which an acid and a base react, commonly forming water and a salt. In aqueous solution, its net ionic form is often hydrogen ions reacting with hydroxide ions to form water.

Brønsted–Lowry acid–base theory: A theory in which acids donate protons and bases accept them. Proton transfer explains neutralization for acids and bases that do not produce hydroxide ions directly.
Arrhenius acid: A substance that increases hydrogen-ion concentration in aqueous solution. This definition describes the acid reactant in the familiar aqueous neutralization model.
Acid–base titration: A quantitative method that determines an acid’s or base’s concentration by reacting it with a measured standard solution. A titration tracks neutralization to determine an unknown concentration.
Hydrolysis (chemistry): A reaction in which a compound reacts with water, often producing new chemical species. Salt hydrolysis can alter the pH after neutralization rather than leaving the solution neutral.
pH: A logarithmic measure of hydrogen-ion activity in a solution. The solution’s pH records how neutralization changes its acidity.
Hydrogen ion: A positively charged hydrogen species; in water, it is present chiefly as hydronium. Acidic solutions supply the hydrogen ions consumed during aqueous neutralization.
Arrhenius base: A substance that increases hydroxide-ion concentration in aqueous solution. This definition supplies the hydroxide ions in the simplest neutralization equation.
Indicator (chemistry): A substance that changes a measurable property, often color, over a particular chemical range. Color-changing indicators can signal a titration endpoint near neutralization’s equivalence point.
Buffer solution: A solution that resists pH change when small amounts of acid or base are added. Buffers resist large pH shifts instead of simply consuming a fixed amount of acid or base.
Equivalence point pH: The pH measured at the stoichiometric equivalence point of an acid–base titration. Its value can differ from 7 when the reacting acid or base is weak.

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