Equivalent conductivity (Λ): The conductance of that volume of solution containing one equivalent of an electrolyte is known as equivalent conductivity. It is denoted by Λ. 

Let us consider the V cm³ of solution containing one equivalent of an electrolyte. Its conductance is equal to equivalent conductance, Λ. 

Also we know that the conductance shown by 1 cm³ solution containing this electrolyte is called specific conductance, κ.

i.e., the conductance of V cm³ --------- Λ 

the conductance of 1 cm³ --------- κ 

Therefore: Λ = κ.V ---------- equation (3) 

We know that the normality (N) of a solution is given by the equation:

N = n_e/V(in cc) x 1000

For above electrolytic solution, no. of equivalents, n_e = 1. 

Hence

V(in cc) = 1000/N

By substituting the above value in the equation (3), we can now write:

Λ = k 1000/N

Units of Λ: 

= Ohm^-1 cm^-1/ equivalents cm³

= cm² . ohm^-1 . equiv^-1 = cm² . mho. equiv^-1 

or m² . Siemens. equiv^-1

Molar conductivity (Λ_m or μ): The conductance of that volume of solution containing one mole of an electrolyte is known as molar conductivity. It is denoted by Λ_m or μ. 

It is related to specific conductance, κ as:

μ = κ.V 

or

μ = k 1000/M

 Where 

M = molarity of the electrolytic solution. 

Units of μ: 

= cm² . ohm^-1 . mol^-1 = cm² . mho. mol^-1 

or 

m² . Siemens. mol^-1 

The relation between equivalent conductance, Λ and molar conductance, μ can be given by: 

μ = Λ x equivalent factor of the electrolyte