Arrheniusteori

Arrhenius theory, proposed by Swedish chemist Svante Arrhenius in 1884, is a fundamental concept in chemistry that describes the dissociation of substances in solution or the ionization of substances in the gas phase. According to Arrhenius, a substance that dissociates in water or ionizes in the gas phase produces ions, which are atoms or molecules that have gained or lost electrons. These ions are responsible for the substance's electrical conductivity.

The theory is based on the principle that the degree of dissociation or ionization is proportional to the concentration of the substance and inversely proportional to the square root of its molecular weight. This relationship is expressed by the Arrhenius equation, which states that the degree of dissociation (α) is equal to the square root of the product of the concentration (C) and the dissociation constant (K), divided by the molecular weight (M) raised to the power of 1.5.

Arrhenius theory has been widely used to explain the behavior of electrolytes in solution and the ionization of gases. However, it has limitations, as it does not account for the effects of temperature, pressure, or the presence of other substances in the solution or gas phase. Despite these limitations, the Arrhenius theory remains an important concept in chemistry, as it provides a basic understanding of the behavior of ions in solution and the ionization of gases.