Ostwald Dilution Law

The strength of elctrolytes is expressed in terms of degree of dissociation alpha For strong electrolyte alpha is close to one and for weak electrolytes alpha is quite small. According to Ostwald Dilution Law alpha=sqrt((K)/(C)) For an acid [H^(+)] = sqrt(K_(a)C) For a base [OH^(-)] =sqrt(K_(b)C The relative strengths of acids or bases can be compared in terms of the square roots of their K_(a) " or " K_(b) values. A monoprotic acid in 0.1 M solution ionises to 0.001 % . Its ionisation constant is :

Ionic Equilibrium - Ostwald'S Dilution Law

Arrhenius Theory OF Electrolytic Dissociation|| Ostwald's Dilution Law

Classification OF Substance (Electrolyte and Non - electrolyte) || Arrhenius Theory OF Electrolytic Dissociation || Strong and Weak Electrolyte || Ostwald’s Dilution Law || Factors Affecting Degree OF Dissociation

State and derive Ostwaid dilution law for a weak electrolyte.