If the molar conductivity of a solution is $1.26 \times 10^{2} \ \Omega^{-1} \ cm^{2} \ mol^{-1}$ and its molarity is $0.01 \ M$,what will be its specific conductivity?

The molar conductivity of a $0.02 \ M$ solution of an electrolyte is $124 \times 10^{-4} \ S \ m^2 \ mol^{-1}$. What is the resistance of the same solution (in ohms),kept in a cell with a cell constant of $129 \ m^{-1}$?

The conductivity of $0.20 \, M$ solution of $KCl$ at $298 \, K$ is $0.0248 \, S \, cm^{-1}$. Calculate its molar conductivity.

At $298 \text{ K}$, the molar conductivity of $x\% \text{ (w/w)}$ $MX$ solution (aqueous) is $123.5 \text{ S cm}^2 \text{ mol}^{-1}$. The conductance of the same solution is $1.9 \times 10^{-3} \text{ S}$. The value of $x$ is . . . . . . $\times 10^{-2}$. (Given: cell constant = $1.3 \text{ cm}^{-1}$; molar mass of $MX$ is $75 \text{ g mol}^{-1}$, density of aqueous solution of $MX$ at $298 \text{ K}$ is $1.0 \text{ g mL}^{-1}$)

What is the molar conductivity of $CH_3COOH$ at infinite dilution if the molar conductivities of $H_2SO_4$, $K_2SO_4$, and $CH_3COOK$ at infinite dilution are $x$, $y$, and $z$ $\Omega^{-1} \text{cm}^2 \text{mol}^{-1}$ respectively?

The conductivity of sodium chloride at $298 \ K$ has been determined at different concentrations and the results are given below:

Concentration $/ M$	$0.001$	$0.010$	$0.020$	$0.050$	$0.100$
${10^2} \times \kappa / S \, m^{-1}$	$1.237$	$11.85$	$23.15$	$55.53$	$106.74$

Calculate ${\Lambda _m}$ for all concentrations and draw a plot between ${\Lambda _m}$ and $c^{1/2}$. Find the value of $\Lambda _m^o$.