"Electrolytic conductance, equivalent conductivity and molar conductivity increases with dilution whereas the specific conductiity of an elctrolytic solution decreases with ditution". Please explain.

The book says that on dilution more ions are produced in the solution and so the conductance should also increase. And the specific conductiity decreases because the number of ions per centimeter cube becomes less and less with dilution.

I am badly confused. Please help.... :D

Look at the comparison:
1.The conductivity (specific conductance) and specific conductivity are similar terms and are defined as conductance of one unit volume of the solution kept between two platinum electrodes with the unit cross-sectional area at a distance of unit length. Its SI unit is S m⁻¹ and symbol used is $\kappa$ .
For both weak and strong electrolytes, conductivity decreases with decrease in concentration or increase in dilution as the number of ions per unit volume carrying the current in a solution decreases

2. Equivalent conductivity is defined as conductance of solution containing 1 equivalents of the electrolyte, kept between two electrodes with the cross-sectional area of A and distance of unit length. It is denoted by Λ _e. It is given by the following relation
 Λ _e = κ / c​
Here the concentration is in gram equivalents per litre. As the dilution of solution increases, the concentration of solution decreases, results in increasing equivalent conductivity.

3.Molar conductivity of a solution at a given concentration is the conductance of solution containing 1 mole of the electrolyte, kept between two electrodes with the cross-sectional area of A and distance of unit length. It is denoted by Λ m. It is given by the follwoing relation :
 Λ _m = κ / c​​
Here the concentration is in moles per litre. As the dilution of solution increases, the concentration of solution decreases, results in increasing equivalent conductivity