The limiting molar conductivities $\wedge ^0$ for $NaCl$,$KBr$,and $KCl$ are $126$,$152$,and $150 \ S \ cm^2 \ mol^{-1}$ respectively. The $\wedge ^0$ for $NaBr$ is ............ $S \ cm^2 \ mol^{-1}$.

If the resistivity of a $0.8 \ M \ KCl$ solution is $2.5 \times 10^{-3} \ \Omega \ cm$,calculate the molar conductivity of the solution.

At $25^o C$,the molar conductivity of a $0.1 \, N \, CH_3COOH$ solution is $80 \, S \, cm^2 \, mol^{-1}$ and the molar conductivity at infinite dilution is $400 \, S \, cm^2 \, mol^{-1}$. What is the degree of dissociation $(\alpha)$ of $CH_3COOH$?

At $298 \text{ K}$,the molar conductivity of $x\% \text{ (w/w)}$ $MX$ solution (aqueous) is $123.5 \text{ S cm}^2 \text{ mol}^{-1}$. The conductance of the same solution is $1.9 \times 10^{-3} \text{ S}$. The value of $x$ is . . . . . . $\times 10^{-2}$. (Given: cell constant = $1.3 \text{ cm}^{-1}$; molar mass of $MX$ is $75 \text{ g mol}^{-1}$,density of aqueous solution of $MX$ at $298 \text{ K}$ is $1.0 \text{ g mL}^{-1}$)

Metallic and ionic conductivity depends on which factors?

The specific conductance $(k)$ of $0.02 \ M$ aqueous acetic acid solution at $298 \ K$ is $1.65 \times 10^{-4} \ S \ cm^{-1}$. The degree of dissociation $(\alpha)$ of acetic acid is: [Given: $\lambda_{H^{+}}^{\infty} = 349.1 \ S \ cm^2 \ mol^{-1}$ and $\lambda_{CH_3COO^{-}}^{\infty} = 40.9 \ S \ cm^2 \ mol^{-1}$]