Conductance is the reciprocal of electrical resistance. Unit for conductance is mho or siemens (S) [1 S = 1 ohm^-1]. Specific conductivity (κ) is defined conductance of solution of 1 cm length and having 1 cm² area or conductance of 1 cm³ of the solution of electrolyte.

Specific conductance = Measured conductance (ohm^-1) × Cell constant (cm^-1) -------------------- eq (i)

Equivalent conductance at dilution V cm³ is defined as the conductance of all ions produced from one-gram equivalent electrolyte dissolved in V cm³ when the distance between the electrodes is one and electrodes are so large that the whole solution is contained between them. Molar conductivity of solution at dilution V cm³, is the conductance of all the ions from one mole of electrolyte dissolved in V cm³ when the distance between the electrodes is one and electrodes are so large that the whole solution is contained between them.

Λ_m = κ × 1000 / Molarity -------------------- eq (ii)

Λ_eq = κ × 1000 / Normality -------------------- eq (iii)

Degree of dissociation (α) is the ratio of equivalent conductance (Λ_eq) to the conductance at infinite dilution (Λ_∞).

α = Λ_eq / Λ_∞ -------------------- eq (iv)

Λ_∞ = ν_A Λ_∞⁺ + ν_B Λ_∞^- (Kohlrausch’s law) -------------------- eq (v)

Where ν_A and ν_B is the number of ions dissociated from molecule cation and anion respectively.

Degree of dissociation α can be expressed as, α = Λ / Λ₀

Dissociation constant (K_d) for acetic acid could be given by the following formula

K_d = Cα² / (1 − α) -------------------- eq (vi)

where, C is the concentration. Graphically, dissociation constant can be determined by plotting the graph of (α² / (1 − α)) vs. 1 / Concentration.