Calculate the molar conductivity of a $0.02 \, M$ solution if its conductivity is $2.06 \times 10^{-3} \, S \, cm^{-1}$.

Calculate the cell constant of a conductivity cell containing $0.01 \ M \ AgNO_3$ solution having a resistance of $1440 \ \Omega$ and a conductivity of $0.001262 \ \Omega^{-1} \ cm^{-1}$. (in $cm^{-1}$)

In a conductivity cell,the electrodes are separated by a distance of $2 \ cm$ and have a cross-sectional area of $4 \ cm^2$. If the conductivity of pure water is $8 \times 10^{-7} \ S \ cm^{-1}$,then the resistance of the water is:

Which of the following expressions for conductivity of a solution of an electrolyte is $NOT$ correct?

What is the ionic mobility of $Ag^{+}$? Given $\lambda^{Ag^{+}} = 5 \times 10^{-4} \ \Omega^{-1} \ cm^{2} \ eq^{-1}$.

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:
$\lambda^{\infty}_{CH_3COONa} = 91.0 \ S \ cm^2 \ eq^{-1}$
$\lambda^{\infty}_{HCl} = 426.25 \ S \ cm^2 \ eq^{-1}$
What additional information/quantity is needed to calculate $\lambda^{\infty}$ of an aqueous solution of acetic acid?