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 value of ΛC for 0.001M aqueous solution of NH3 is (in S m2mol−2)

Molar conductance is used to define as the conducting power of all the

1.	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 value of ΛC for 0.001M aqueous solution of NH3 is (in S m2mol−2)
Answer» 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. $Λ m = \frac{1000 \times K}{C}$ 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. $Λ A B_{m}^{\infty} = x A_{+}^{\infty} + y A_{+}^{\infty}$ 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. $α = \frac{Λ^{C}}{Λ^{\infty}}; K_{a} = \frac{a^{2} C}{(1 - α)}; K_{b} = \frac{α^{2} C}{(1 - α)}$ 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 $A^{C}$ is taken as $A^{\infty}$ . Knowing $A^{\infty}$ (by Kohlrausch’s law) the concentration of saturated solution is calculated from which Ksp is calculated. The value of $Λ^{C}$ for 0.001M aqueous solution of $N H_{3}$ is (in $S m^{2} m o l^{- 2}$ )

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