Specific conductance or conductivity of the electrolyte solution is given by the following relation: $\mathrm{K}=\mathrm{G}\cdot \mathrm{\ell }/\mathrm{A}$ where, G=1/R is the conductance and l /A is the cell constant, Molar conductance (${\wedge }_{\mathrm{m}}$) and equivalent conductance (${\wedge }_e$) of an electrolyte solution are calculated using the following similar relations: ${\wedge }_{\mathrm{m}}=\mathrm{K}.1000/\mathrm{M};{\wedge }_{\mathrm{e}}=\mathrm{K}.1000/\mathrm{N}$ where, M and N are the molarity and normality of the solution respectively. Molar conductance of strong electrolyte depends on concentration : ${\wedge }_{\mathrm{m}}={\wedge }_{\mathrm{m}}^0-\mathrm{b}\sqrt{\mathrm{C}}$ where, ${\wedge }_{\mathrm{m}}^0$ = molar conductance at infinite dilution; C = concentration of the solution b = constant. $\mathrm{\alpha }={\wedge }_{\mathrm{m}}/{\wedge }_{\mathrm{m}}^0={\wedge }_{\mathrm{e}}/{\wedge }_{\mathrm{e}}^0$