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 $cm^{-1}$)

The resistivity of a $0.8 \ M$ solution of an electrolyte is $5 \times 10^{-3} \ \Omega \ cm$. Its molar conductivity is $..... \times 10^4 \ \Omega^{-1} \ cm^2 \ mol^{-1}$. (Nearest integer)

The resistance of a $0.01\, M$ solution of an $Hg_2Cl_2$ electrolyte was found to be $210\, \Omega$ at $298\, K$ using a conductivity cell with a cell constant of $0.63\, m^{-1}$. The equivalent conductance of the solution is:

$A$ conductivity cell dipped in $0.05 \ M$ $KCl$ has a resistance of $600 \ \Omega$. If the conductivity is $0.0015 \ \Omega^{-1} \ cm^{-1}$,what is the value of the cell constant (in $cm^{-1}$)?

What is the molar conductivity of $0.02 \text{ M}$ $KI$ solution if its conductivity is $4.37 \times 10^{-4} \text{ }\Omega^{-1} \text{cm}^{-1}$?

Calculate the degree of dissociation of $0.01 \ M$ acetic acid at $25^{\circ} C$ given that the molar conductivity at concentration $c$ is $\Lambda_{c} = 15.0 \ \Omega^{-1} \ cm^2 \ mol^{-1}$ and the limiting molar conductivity is $\Lambda_0 = 300 \ \Omega^{-1} \ cm^2 \ mol^{-1}$.