A substance used to show the presence of a chemical substance or ion by its colour. Acid–base indicators are compounds, such as phenolphthalein and methyl orange, that change colour reversibly, depending on whether the solution is acidic or basic. They are usually weak acids in which the un-ionized form HA has a different colour from the negative ion A−. In solution the indicator dissociates slightly
In acid solution the concentration of H+ is high, and the indicator is largely undissociated HA; in alkaline solutions the equilibrium is displaced to the right and A− is formed. Useful acid–base indicators show a sharp colour change over a range of about 2 pH units. In titration, the point at which the reaction is complete is the equivalence point (i.e. the point at which equivalent quantities of acid and base are added). The end point is the point at which the indicator just changes colour. For accuracy, the two must be the same. During a titration the pH changes sharply close to the equivalence point, and the indicator used must change colour over the same range.
Other types of indicator can be used for other reactions. Starch, for example, is used in iodine titrations because of the deep blue complex it forms. Oxidation-reduction indicators are substances that show a reversible colour change between oxidized and reduced forms. See also adsorption indicator.