Specific conductivity or conductivity of an electrolytic solution at any given concentration is the conductance of unit volume of solution kept between two platinum electrodes with unit area of cross section and at a distance of unit length. Conductivity decreases with decrease in concentration as the number of ions per unit volume that carry the current in a solution decrease on dilution. Molar conductivity of a solution at a given concentration is the conductance of the volume \(V\)

\(Ʌ_m\)

Here,

\(c\)

\(К\)

\(Ʌ_m\)

As the solution contains only one mole of electrolyte, the above equation can be modified as:

\(Ʌ_m\)

Molar conductivity increases with decrease in concentration as the total volume, \(V\)

**Variation of molar conductivity with concentration for strong electrolytes**: For strong electrolytes the molar conductivity increases slowly with the dilution. The plot between the molar conductivity and \(\frac{c_1}{2}\)

For strong electrolytes the molar conductivity increases slowly with the dilution. The plot between the molar conductivity and \(\frac{c_1}{2}\)

\(Ʌ_m\)

Where, \(-A\)

**Variation of molar conductivity with concentration for weak electrolyte:**

For weak electrolytes, the graph plotted between molar conductivity and \(\frac{c_1}{2}\)

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