デバイ–ハッケル–オンサーガーコンダクタンス方程式

The Debye-Hückel-Onsager equation applies specifically to uni-univalent electrolytes, which dissociate into one cation with a +1 charge and one anion with a –1 charge per formula unit. This limitation ensures the equation accurately predicts molar conductivity behavior for these specific electrolyte types in solution.

The asymmetry effect and electrophoretic effect both reduce molar conductivity by retarding ion movement in solution. The Debye-Hückel-Onsager equation quantifies their combined impact by multiplying their sum by the square root of concentration, showing how conductivity decreases as electrolyte concentration increases from infinite dilution.

Experimental data for uni-univalent electrolytes in water confirms a linear relationship between molar conductivity and the square root of concentration, with a slope of (60.2 + 0.229 Λ°m). This validates the Debye-Hückel-Onsager equation predictions up to concentrations around 0.02 M, though slight deviations occur at higher concentrations.

The Debye-Falkenhagen effect describes how conductance of a strong electrolyte solution increases with the frequency of applied alternating current. At higher frequencies, the ionic atmosphere remains symmetric around the central ion, eliminating the asymmetry-induced retarding effect and thereby enhancing overall conductance.

The Wien effect occurs at high potential gradients where ions move too rapidly for an ionic atmosphere to form, minimizing asymmetry and electrophoretic effects. This contrasts with the Debye-Falkenhagen effect, which operates at high alternating current frequencies, and both phenomena result in increased conductance of strong electrolytes.

At infinite dilution, concentration approaches zero, eliminating the retarding effects of the ionic atmosphere. Under these conditions, molar conductivity reaches its theoretical maximum value Λ°m, as predicted by the Debye-Hückel-Onsager equation, representing the conductivity when ions move completely unimpeded by surrounding ions.

The equation is verified by plotting molar conductivity versus the square root of concentration for uni-univalent electrolytes in water, which produces a straight line with slope (60.2 + 0.229 Λ°m). This linear relationship holds reliably up to approximately 0.02 M concentration, validating the theory of strong electrolytes.