Which of the following decreases on dilution of an electrolytic solution?

How does electrolytic conduction differ from metallic conduction?

The molar conductivity of $0.02 \ M$ $KCl$ solution is $410 \ \Omega^{-1} \ cm^2 \ mol^{-1}$ at $25^{\circ} C$. Calculate its conductivity?

What benefit do we get by forming a thin layer of $Pt$ particles on the electrodes of a conductivity cell?

Which of the following is the correct relationship between molar conductivity $(\Lambda_m)$,conductivity $(k)$,and molarity $(M)$ of a solution for an electrolyte?

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 $74.5 \; g \; mol^{-1}$.