If the conductivity of a $0.5 \ M \ KCl$ solution at $298 \ K$ is $0.024 \ S \ cm^{-1}$,then the molar conductivity of the solution would be $S \ cm^2 \ mol^{-1}$.

The resistance of a conductivity cell of $0.1 \ M$ $KCl$ solution is $120 \ \Omega$ and conductivity is $1.64 \times 10^{-4} \ S \ cm^{-1}$. What is the value of cell constant (in $cm^{-1}$)?

The electrical conductance of unit volume $(1 \ cm^3)$ of solution is called as

Kohlrausch's law states that at

Solutions of two electrolytes $A$ and $B$ are diluted. The $\Lambda_m$ of $B$ increases $1.5$ times while that of $A$ increases $25$ times. Which of the two is a strong electrolyte? Justify your answer.

The equivalent conductance at infinite dilution $\wedge^0$ for electrolytes $BA$ and $CA$ are $140$ and $120 \ S \ cm^2 \ eq^{-1}$,respectively. The equivalent conductance at infinite dilution for $BX$ is $198 \ S \ cm^2 \ eq^{-1}$. The $\wedge^0$ (in $S \ cm^2 \ eq^{-1}$) of $CX$ is: