Define conductivity and molar conductivity for the solution of an electrolyte. Discuss their variation with concentration.

#### Solution

Conductivity of a solution is defined as the conductance of a solution of 1 cm in length and area of cross-section 1 sq. cm. The inverse of resistivity is called conductivity or specific conductance. It is represented by the symbol*κ*. If ρ is resistivity, then we can write:

`k = 1/rho`

The conductivity of a solution at any given concentration is the conductance (*G*) of one unit volume of solution kept between two platinum electrodes with the unit area of cross-section and at a distance of unit length.

ie `G= k a/l = k.l =k`

Since *a* = 1, *l* = 1)

Conductivity always decreases with a decrease in concentration, both for weak and strong electrolytes. This is because the number of ions per unit volume that carry the current in a solution decreases with a decrease in concentration.

**Molar conductivity:**

Molar conductivity of a solution at a given concentration is the conductance of volume V of a solution containing 1 mole of the electrolyte kept between two electrodes with the area of cross-section *A* and distance of unit length.

`Lambda_m = kA/l`

Now, *l* = 1 and *A* = V (volume containing 1 mole of the electrolyte).

`:.Lambda_m = kV`

Molar conductivity increases with a decrease in concentration. This is because the total volume V of the solution containing one mole of the electrolyte increases on dilution.

The variation of `Lambda_m` with `sqrtc` for strong and weak electrolytes is shown in the following plot: