$A$ conductivity cell has two electrodes $18 \ mm$ apart and having cross-sectional area $2.0 \ cm^2$. What is the value of the cell constant (in $cm^{-1}$)?

The molar conductivity of a $0.04 \text{ M}$ $AB_2$ type salt solution at $300 \text{ K}$ is $200 \text{ } \Omega^{-1} \text{ cm}^2 \text{ mol}^{-1}$. Find the conductivity.

In infinite dilution,the equivalent conductances of $Ba^{2+}$ and $Cl^{-}$ are $127$ and $76 \ ohm^{-1} cm^2 eqv^{-1}$ respectively. The equivalent conductivity of $BaCl_2$ at infinite dilution is: (in $.5$)

The limiting molar conductivities of $X^{+}$ and $Y^{-2}$ ions are $45$ and $110 \ S \ cm^2 \ mol^{-1}$ respectively. The $\Lambda_{m}^{\infty}$ of $X_2Y$ is:

The molar conductivity of $KCl$ solutions at different concentrations at $298 \ K$ is given below:

$c / mol \ L^{-1}$	$\Lambda_m / S \ cm^2 \ mol^{-1}$
$0.000198$	$148.61$
$0.000309$	$148.29$
$0.000521$	$147.81$
$0.000989$	$147.09$

Show that a plot of $\Lambda_m$ versus $c^{1/2}$ is a straight line. Determine the values of $\Lambda_m^o$ and $A$ for $KCl$.

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