Calculate the cell constant of a conductivity cell containing $0.1 \ M$ $KCl$ solution having a resistance of $60 \ \Omega$ and a conductivity of $0.014 \ \Omega^{-1} \ cm^{-1}$ at $25^{\circ} \ C$. (in $cm^{-1}$)

Match List-$I$ with List-$II$:

List-$I$ (Parameter)	List-$II$ (Unit)
$a$. Cell constant	$i$. $S\, cm^{2}\, mol^{-1}$
$b$. Molar conductivity	$ii$. Dimensionless
$c$. Conductivity	$iii$. $m^{-1}$
$d$. Degree of dissociation of electrolyte	$iv$. $\Omega^{-1}\, m^{-1}$

Choose the most appropriate answer from the options given below:

Write a note on molar conductivity $(\Lambda_{m})$ of a solution.

Conductivity of a saturated solution of a sparingly soluble salt $AB$ at $298 \ K$ is $1.85 \times 10^{-5} \ S \ m^{-1}$. Solubility product of the salt $AB$ at $298 \ K$ is. Given $\Lambda_{m}^{\circ}(AB) = 140 \times 10^{-4} \ S \ m^{2} \ mol^{-1}$.

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

The molar conductivity of $0.1 \ M$ $BaCl_2$ solution is $106 \ \Omega^{-1} \ cm^2 \ mol^{-1}$ at $25^{\circ} C$. What is its conductivity?