The Arrhenius theory of electrolytic dissociation
(1) Postulates of Arrhenius theory
(i) In the aqueous solution, molecules of an electrolyte undergo spontaneous dissociation to form the positive and negative ions.
(ii) The degree of ionization (alpha)
(iii) At the moderate concentrations, there is prevailing an equilibrium between the ions and undissociated molecules, like,
This equilibrium state is known as ionic equilibrium.
(iv) Each ion behaves as osmotically as the molecule.
(2) The factors which affect degree of ionisation
(i) At the normal dilution, value of alpha is nearly 1 for strong the electrolytes, while it is very less than 1 for the weak electrolytes.
(ii) Higher the value of dielectric constant of the solvent more is its ionising power. Water is most powerful ionising solvent as its dielectric constant is highest.
(iv) The degree of ionisation of an electrolyte in the solution increases with the rise in temperature.
(v) Presence of common ion : The degree of the ionisation of an electrolyte decreases in the presence of the strong electrolyte having a common ion.
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