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.

Resistance of a conductivity cell filled with a solution of an electrolyte of concentration $0.1 \, M$ is $100 \, \Omega .$ The conductivity of this solution is $1.29 \, S \, m^{-1}.$ Resistance of the same cell when filled with $0.2 \, M$ of the same solution is $520 \, \Omega .$ The molar conductivity of $0.2 \, M$ solution of electrolyte will be..........$\times 10^{-4} \, S \, m^2 \, mol^{-1}$

$\Lambda_m^0(NH_4OH)$ is equal to:

Which among the following aqueous salt solutions is used in a conductivity cell to determine the cell constant?

The graphical variation of molar conductivity $(\Lambda_m)$ against the square root of molar concentration $(\sqrt{c})$ for a certain electrolyte '$X$' is linear with an intercept on the y-axis. Identify '$X$' from the following.

Write a note on the difficulties associated with the measurement of resistivity of an ionic solution.