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