The conductivity of $0.012 \ M$ $NaBr$ solution is $2.67 \times 10^{-4} \ S \ cm^{-1}$. What is its molar conductivity?

The equivalent conductance at infinite dilution $\wedge^0$ for electrolytes $BA$ and $CA$ are $140$ and $120 \ S \ cm^2 \ eq^{-1}$,respectively. The equivalent conductance at infinite dilution for $BX$ is $198 \ S \ cm^2 \ eq^{-1}$. The $\wedge^0$ (in $S \ cm^2 \ eq^{-1}$) of $CX$ is:

For which electrolyte the molar conductivity at infinite dilution cannot be obtained graphically?

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 $\lambda_{CH_3COO^{-}}^{\infty} = 40.9 \ S \ cm^2 \ mol^{-1}$]

The specific conductance of a saturated solution of silver bromide is $\kappa \ S \ cm^{-1}$. The limiting ionic conductances for $Ag^{+}$ and $Br^{-}$ are $x$ and $y$ $S \ cm^2 \ mol^{-1}$ respectively. Then the solubility of silver bromide (in $g/L$) will be $(Ag = 108, Br = 80)$.

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