$A$ $5.0 \, mmol \, dm^{-3}$ aqueous solution of $KCl$ has a conductance of $0.55 \, mS$ when measured in a cell with a cell constant of $1.3 \, cm^{-1}$. The molar conductivity of this solution is ....... $mS \, m^{2} \, mol^{-1}$. (Round off to the Nearest Integer)

What is the molar conductivity of a $0.05 \ M$ solution of sodium hydroxide,if its conductivity is $0.0118 \ S \ cm^{-1}$ at $298 \ K$?

The molar conductivity of a conductivity cell filled with $10 \ moles$ of $20 \ mL$ $NaCl$ solution is $\Lambda_{m1}$ and that of another identical cell filled with $20 \ moles$ of $80 \ mL$ $NaCl$ solution is $\Lambda_{m2}$. If the conductivities $(\kappa)$ exhibited by these two cells are the same,the relationship between $\Lambda_{m2}$ and $\Lambda_{m1}$ is $........$

Suggest a way to determine the $\Lambda _m^o$ value of water.

Molar conductivity of $0.01 \ M \ CH_3COOH$ is $19.5 \ \Omega^{-1} \ cm^2 \ mol^{-1}$. Calculate its degree of dissociation if molar conductivity at zero concentration is $390 \ \Omega^{-1} \ cm^2 \ mol^{-1}$.

The variation of molar conductivity with concentration of an electrolyte $X$ in aqueous solution is shown in the given figure.
The electrolyte $X$ is :