The cell constant of a cell is $0.5 \ cm^{-1}$ and the resistance $R = 50 \ \Omega$. If the normality is $1 \ N$,then the equivalent conductivity of the electrochemical cell is ...... $\Omega^{-1} \ cm^2 \ (g \ eq)^{-1}$.

The molar conductivity for electrolytes $A$ and $B$ are plotted against $C^{1/2}$ as shown below. Electrolytes $A$ and $B$ respectively are:

Calculate the concentration of silver nitrate solution if molar conductivity and conductivity of silver nitrate at $25 \text{ }^\circ\text{C}$ are respectively $120 \text{ ohm}^{-1} \text{cm}^2 \text{mol}^{-1}$ and $0.0024 \text{ ohm}^{-1} \text{cm}^{-1}$. (in $\text{ M}$)

Specific conductance of $0.1 \, M$ nitric acid is $6.3 \times 10^{-2} \, \Omega^{-1} cm^{-1}$. The molar conductance of the solution is ............... $\Omega^{-1} cm^2 mol^{-1}$.

Given below is the plot of the molar conductivity vs $\sqrt{concentration}$ for $KCl$ in aqueous solution. If,for the higher concentration of $KCl$ solution,the resistance of the conductivity cell is $100 \ \Omega$,then the resistance of the same cell with the dilute solution is '$x$' $\Omega$. The value of $x$ is $............$ ($Nearest$ $integer$)

Limiting molar conductivity of $CH_3COOH$ (i.e.,$\Lambda^o_{m(CH_3COOH)}$) is equal to: