Molar conductivities at infinite dilution $\wedge_{m}^{\circ}$ for $Ba(OH)_2$,$BaCl_2$ and $NH_4Cl$ are $457.0$,$240.6$ and $213.0 \ S \ cm^2 \ mol^{-1}$ respectively. The $\wedge_{m}^{\circ}$ for ammonium hydroxide (in $S \ cm^2 \ mol^{-1}$) is (in $.2$)

The conductivity of an electrolytic solution decreases on dilution due to

The resistance of a conductivity cell containing $0.001 \ M \ KCl$ solution at $298 \ K$ is $1500 \ \Omega$. What is the cell constant if the conductivity of $0.001 \ M \ KCl$ solution at $298 \ K$ is $0.146 \times 10^{-3} \ S \ cm^{-1}$?

What will be the concentration of a solution of an electrolyte if its molar conductivity and conductivity are respectively $230 \ \Omega^{-1} \ cm^2 \ mol^{-1}$ and $0.0115 \ \Omega^{-1} \ cm^{-1}$ at $298 \ K$ (in $M$)?

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..........$\times 10^{-4} \, S \, m^2 \, mol^{-1}$

What is the resistance of $0.01 \ M \ KCl$ solution if its conductivity is $200 \ \Omega^{-1} \ cm^{-1}$ and cell constant is $1 \ cm^{-1}$?