The specific conductance (conductivity) of a solution is $0.2 \ \Omega^{-1} cm^{-1}$ and its conductance is $0.04 \ \Omega^{-1}$. The cell constant would be .............. $cm^{-1}$.

$0.5 \ N$ solution of a salt placed between two platinum electrodes $2.0 \ cm$ apart and of area of cross section $4.0 \ cm^2$ has a resistance of $25 \ \Omega$. Calculate the equivalent conductivity of solution ................. $\Omega^{-1} \ cm^2 \ eq^{-1}$

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

Given the limiting molar conductivities at $25^{\circ}C$ for the following electrolytes in $S \, cm^{2} \, mol^{-1}$:
$KCl = 149.9$
$KNO_{3} = 145.0$
$HCl = 426.2$
$NaOAc = 91.0$
$NaCl = 126.5$
Calculate $\Lambda^{\infty}_{HOAc}$ using the Kohlrausch law of independent migration of ions.

The increase in equivalent conductance of an electrolyte solution with dilution is due to the increase in

$A$ solution of concentration $C \ g \ equiv/L$ has a specific resistance $R$. The equivalent conductance of the solution is