The resistance of a $0.2 \, M$ electrolyte solution is $50 \, \Omega$. The specific conductivity of the solution is $1.3 \, S \, m^{-1}$. If the resistance of a $0.4 \, M$ solution of the same electrolyte is $260 \, \Omega$,what is its molar conductivity?

Which among the following aqueous salt solutions is used in a conductivity cell to determine the cell constant?

The molar conductivities of $HCl$,$NaCl$,$CH_{3}COOH$,and $CH_{3}COONa$ at infinite dilution follow the order:

$0.2\% (w/v)$ solution of $NaOH$ is measured to have resistivity $870.0 \ m\Omega \ m$. The molar conductivity of the solution will be $........ \times 10^2 \ mS \ dm^2 \ mol^{-1}$. $(Nearest \ integer)$

$\Lambda_{m}^0$ for $NaCl$,$HCl$ and $NaAc$ are $126.4 \ S \ cm^2 \ mol^{-1}$,$425.9 \ S \ cm^2 \ mol^{-1}$ and $91.0 \ S \ cm^2 \ mol^{-1}$ respectively. Calculate $\Lambda^0$ for $HAc$.

When a certain conductivity cell was filled with $0.1 \ M \ KCl$,it had a resistance of $85 \ \Omega$ at $25 \ ^oC$. When the same cell was filled with an aqueous solution of $0.052 \ M$ unknown electrolyte,the resistance was $96 \ \Omega$. Calculate the molar conductivity of the unknown electrolyte at this concentration ............. $\Omega^{-1} \ cm^2 \ mol^{-1}$ (Given: Specific conductance of $0.1 \ M \ KCl = 1.29 \times 10^{-2} \ \Omega^{-1} \ cm^{-1}$)