The conductivity of a strong electrolyte is:

The conductivity of a solution containing $2.08 \ g$ of anhydrous barium chloride in $200 \ mL$ solution is $6 \times 10^{-3} \ \Omega^{-1} \ cm^{-1}$. The molar conductivity of the solution (in $\Omega^{-1} \ cm^2 \ mol^{-1}$) is $\underline{x} \times 10^2$. The value of $\underline{x}$ is (Atomic mass of $Ba=137, Cl=35.5$)

The resistance of $0.01 \ M$ $KCl$ solution at $298 \ K$ is $1500 \ \Omega$. If the conductivity of $0.01 \ M$ $KCl$ solution at $298 \ K$ is $0.1466 \times 10^{-3} \ S \ cm^{-1}$,the cell constant of the conductivity cell in $cm^{-1}$ is:

The metal which is the best conductor of electricity is

Molar ionic conductivities of a divalent cation and a divalent anion are $57 \ S \ cm^2 \ mol^{-1}$ and $73 \ S \ cm^2 \ mol^{-1}$ respectively. The molar conductivity of a solution of an electrolyte containing these ions will be:

The values of $\lambda^{\infty}_m$ for $NH_4Cl$,$NaOH$,and $NaCl$ are $129.8$,$248.1$,and $126.4 \ \Omega^{-1} \ cm^2 \ mol^{-1}$ respectively. Calculate $\lambda^{\infty}_m$ for $NH_4OH$ solution (in $\Omega^{-1} \ cm^2 \ mol^{-1}$).