The electronic conductance does not depend on . . . . . . .

If the conductivity of $0.08 \ M$ $KCl$ solution is $2 \times 10^{-2} \ \Omega^{-1} \ cm^{-1}$,what is the molar conductivity of the solution?

The electrodes of a conductivity cell are $3 \text{ cm}$ apart and have a cross-sectional area of $4 \text{ cm}^2$. The cell constant of the cell (in $\text{cm}^{-1}$) is

Which solution of $NaCl$ will show the highest resistance during the passage of current (in $N$)?

Resistance of a conductivity cell (cell constant $129 \; m^{-1}$) filled with $74.5 \; ppm$ solution of $KCl$ is $100 \; \Omega$ (labelled as solution $1$). When the same cell is filled with $KCl$ solution of $149 \; ppm$,the resistance is $50 \; \Omega$ (labelled as solution $2$). The ratio of molar conductivity of solution $1$ and solution $2$ is i.e.,$\frac{\wedge_{1}}{\wedge_{2}} = x \times 10^{-3}$. The value of $x$ is (Nearest integer). Given,molar mass of $KCl$ is $74.5 \; g \; mol^{-1}$.

The number of correct statements from the following is $...........$.
$(A)$ Conductivity always decreases with decrease in concentration for both strong and weak electrolytes.
$(B)$ The number of ions per unit volume that carry current in a solution increases on dilution.
$(C)$ Molar conductivity increases with decrease in concentration.
$(D)$ The variation in molar conductivity is different for strong and weak electrolytes.
$(E)$ For weak electrolytes,the change in molar conductivity with dilution is due to decrease in degree of dissociation.