The resistance of a $0.5 \, M$ solution of an electrolyte in a cell was found to be $50 \, \Omega$. If the electrodes in the cell are $2.2 \, cm$ apart and have an area of $4.4 \, cm^2$,then the molar conductivity (in $S \, m^2 \, mol^{-1}$) of the solution is:

$\Lambda_{m(HAc)}^0$ is equal to . . . . . . .

The equivalent conductances of two strong electrolytes at infinite dilution in $H_2O$ (where ions move freely through a solution) at $25 ^\circ C$ are given below:
$\Lambda _{CH_3COONa}^o = 91.0 \ S \ cm^2 / equiv.$
$\Lambda _{HCl}^o = 426.2 \ S \ cm^2 / equiv.$
What additional information/quantity one needs to calculate $\Lambda ^o$ of an aqueous solution of acetic acid?

Which of the following statements regarding the solution of an electrolyte is not correct?

The conductivity of a centimolar solution of $KCl$ at $25^{\circ} C$ is $0.0210 \, \Omega^{-1} cm^{-1}$ and the resistance of the cell containing the solution at $25^{\circ} C$ is $60 \, \Omega$. The value of the cell constant is $......... \, cm^{-1}$.

$A$ $0.5\,M\,NaOH$ solution offers a resistance of $31.6\,\Omega$ in a conductivity cell at room temperature. What shall be the approximate molar conductance of this $NaOH$ solution if the cell constant of the cell is $0.367\,cm^{-1}$? (in $S\,cm^2\,mol^{-1}$)