What is the cell constant,if two platinum electrodes in a conductivity cell are separated by $0.92 \ cm$ and the area of cross-section is $1.2 \ cm^2$ (in $cm^{-1}$)?

Calculate molar conductivity at infinite dilution for $NaBr$ if molar conductivity at infinite dilution for $NaCl$,$KBr$ and $KCl$ are $126$,$152$ and $150 \ \Omega^{-1} \ cm^2 \ mol^{-1}$ respectively.

The resistance of $0.1 \ M$ weak acid $HA$ in a conductivity cell is $2 \times 10^3 \ \Omega$. The cell constant of the cell is $0.78 \ cm^{-1}$ and $\lambda_{m}^{\circ}$ of acid $HA$ is $390 \ S \ cm^2 \ mol^{-1}$. The $pH$ of the solution is

If the resistance of a $0.01 \, M$ electrolyte in a cell is $40 \, \Omega$ and the cell constant is $0.4 \, \text{cm}^{-1}$,what is the molar conductivity in $\Omega^{-1} \, \text{cm}^2 \, \text{mol}^{-1}$?

The factor which is not affecting the conductivity of any solution is

What is the molar conductivity at infinite dilution of $CaCl_{2}$,if the molar conductivity of $Ca^{2+}$ ion and $Cl^{-}$ ion at infinite dilution is $119$ and $71 \ \Omega^{-1} \ cm^{2} \ mol^{-1}$ respectively?