Explain the variation of molar conductivity with concentration for strong and weak electrolytes.

Explanation

(1) Molar conductivity is the conductance of all the ions produced from one mole of an electrolyte. The molar conductivity of both, strong and weak electrolytes increases with dilution or the decrease in concentration of the electrolytic solution.
As the dilution increase , the dissociation of the electrolyte increases, hence the total number of ions increases, therefore, the molar conductivity increases.
(3) Molar conductivity `^^_(m)` is given by `^^_(m) = (k)/(C) = k xx V` where k is conductivity and C or V are concentration or dilution of the solution respectively.
(4) On dilution, the molar conductivity of strong electrolytes increase rapidly and approaches to a maximum limiting value at infinite dilution or zero concentration and respresented as `^^ oo` or `^^_(0)` or `^^_(m)^(0)` .
(5) In case of weak electrolytes, the molar condutivity is low and condutivity is low and increase slowly in high concentration region but incerease rapidly at low concentration or high dilution since the extent of dissocitate inrease with dilution rapily.
For strong electrolytes, the linear variation of molar conductivity (Am) with the concentration is represented by Kohlrausch relation, `^^_(m) = ^^_(0) - a sqrt(c)` where a is a constant .
`^^_(0)` values for strong electrolytes can be obtained by extrapolating the linear graph to zero concentration (or infinite dilution). However A, for the weak electrolytes cannot be obtained by this method, since the graph increases exponentially at very high dilution and does not intersect `^^_(m)` axis,