Limitations of Arrhenius Theory
Following are the limitations to the Arrhenius’s theory:
- This theory does not apply to non-aqueous or gaseous processes of acids and bases; it is only relevant to their aqueous solutions.
- Only compounds with the formulas HA for acids or BOH for bases can use this theory. As the acidic characteristics of CuSO4, AlCl3, CO2, and SO2 cannot be represented by the formula HA, the theory is unable to explain them. Similarly, because amines, Na2CO3, and NH3 cannot be represented by the formula BOH, the theory is unable to explain their fundamental features.
- This hypothesis is unable to account for the basic and acidic properties of NH3 and HCl in non-aqueous media such as acetone, benzene, and gaseous states.
- The Arrhenius hypothesis states that protons (H+) are free to exist in aqueous solutions. H+ ions, on the other hand, are constantly hydrated and exist as hydronium ions (H3O+) in aqueous solutions.
Arrhenius Theory
Arrhenius Theory introduced in 1887 by Swedish scientist Svante Arrhenius, is used to describe the behavior of acids and bases in aqueous solutions. This theory states that a material that releases hydroxide ions (OH–) in water is an Arrhenius base, and a substance that releases hydrogen ions (H+) in water is an Arrhenius acid.
This article will thoroughly explain the Arrhenius theory, along with instances of Arrhenius bases, Arrhenius acids and Arrhenius theory of electrolytic dissociation.
Table of Content
- What is Arrhenius Theory?
- Arrhenius Theory of Acid and Base
- Reaction Between Arrhenius Acid and Base
- Arrhenius Theory of Electrolytic Dissociation
- Limitations of Arrhenius Theory