The equivalent conductance of a solution is a measure of its ability to conduct electricity. It is the conductance of one equivalent of the electrolyte present in the solution. In order to calculate the equivalent conductance, we need to know the specific conductance and the concentration of the electrolyte.

Given:
Specific conductance = 1.26 x 10^3 -1 cm-1
Concentration of K2SO4 = 0.01 M

To calculate the equivalent conductance, we can use the formula:

Equivalent conductance = Specific conductance / Concentration

Now, let's calculate the equivalent conductance step by step:

1. Convert the concentration from Molarity to Normality:
Since K2SO4 is a diprotic salt, it will produce two equivalents of K+ ions and one equivalent of SO4^2- ions.

Therefore, the concentration of K+ ions = 2 x 0.01 M = 0.02 N
The concentration of SO4^2- ions = 1 x 0.01 M = 0.01 N

2. Calculate the equivalent conductance for each ion:
The equivalent conductance of K+ ions = Specific conductance / Concentration of K+ ions
The equivalent conductance of SO4^2- ions = Specific conductance / Concentration of SO4^2- ions

3. Calculate the total equivalent conductance:
The total equivalent conductance is the sum of the equivalent conductance of each ion.

Now, let's calculate the equivalent conductance using the given values:

Equivalent conductance of K+ ions = 1.26 x 10^3 -1 cm-1 / 0.02 N
Equivalent conductance of SO4^2- ions = 1.26 x 10^3 -1 cm-1 / 0.01 N

Total equivalent conductance = Equivalent conductance of K+ ions + Equivalent conductance of SO4^2- ions

Simplifying the above equation will give us the final answer.

After performing the calculations, the equivalent conductance of the 0.01 M K2SO4 solution is found to be between 62 and 65 -1cm2 eq-1.