Molar conductance is used to define as the conducting power of all the ions produced by one mole of the electrolyte in the given solution. Λm=1000×KC Where, K = specific conductance, C = Molar concentration of the solution. At infinite dilution, each ion makes a definite contribution for the conductance of electrolyte. At infinite dilution, the molar conductance of an electrolyte is the sum of the ionic conductance of constituent ions. ΛAB∞m=xA∞++yA∞+ where,x and y are the number of cations and anions per formula unit of the electrolyte. By measuring the conductance we can measure degree of dissociation and dissociation constants. α=ΛCΛ∞;Ka=a2C(1−α);Kb=α2C(1−α) By conductance measurements we can calculate the solubility product of a sparingly soluble salt. For a sparingly soluble salt, the saturated solution will be an extremely dilute solution and AC is taken as A∞. Knowing A∞ (by Kohlrausch’s law) the concentration of saturated solution is calculated from which Ksp is calculated. The degree of dissociation of water will be (Λ0H+=3.458×10−2 Sm2 mol−1;Λ0OH−=1.98×10−2Sm2 mol–1;Ka of water=5.7×10−6 Sm−1)