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 $S \ cm^2 \ mol^{-1}$.

Which of the following cannot be used as a standard solution for the determination of the cell constant of a conductivity cell?

Molar conductivity of $0.02 \ M$ weak acid is $7.92 \ \Omega^{-1} \ cm^2 \ mol^{-1}$ and its molar conductivity at infinite dilution is $232.7 \ \Omega^{-1} \ cm^2 \ mol^{-1}$. Calculate the degree of dissociation of the weak acid.

With dilution,the conductivity of a solution $—$

Conductivity (unit $S$) is directly proportional to the area of the vessel $(A)$ and the concentration of the solution $(C)$ in it,and is inversely proportional to the length of the vessel $(l)$. The unit of the constant of proportionality is:

The dissociation constant of $n$-butyric acid is $1.6 \times 10^{-5}$ and the molar conductivity at infinite dilution is $380 \times 10^{-4} \ S \ m^2 \ mol^{-1}$. The specific conductance of the $0.01 \ M$ acid solution is