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:

The variation of $\lambda_{m}$ of acetic acid with concentration is correctly represented as:

The molar conductivity of a $0.01 \text{ M}$ monobasic acid at $25^{\circ} \text{C}$ is $15 \text{ } \Omega^{-1} \text{cm}^2 \text{mol}^{-1}$. The molar conductivity of the same acid at infinite dilution is $375 \text{ } \Omega^{-1} \text{cm}^2 \text{mol}^{-1}$. Calculate the concentration of $[H^+]$ in the solution.

If $\Lambda^{0}_{NaOAc} = 91 \, S \, cm^{2} \, mol^{-1}$ and $\Lambda^{0}_{HCl} = 496.2 \, S \, cm^{2} \, mol^{-1}$,what additional value is required to calculate $\Lambda^{0}_{HOAc}$?

$A$ conductivity cell shows a resistance of $600 \ \Omega$. If the conductivity of $0.01 \ M \ KCl$ is $0.0015 \ \Omega^{-1} \ cm^{-1}$,what is the cell constant (in $cm^{-1}$)?

At $25\,^{\circ}C$,the molar conductivity at infinite dilution for electrolytes $KOH$,$KCl$ and $BaCl_2$ are $248 \times 10^{-4}$,$126 \times 10^{-4}$ and $280 \times 10^{-4}\,S\,m^2\,mol^{-1}$ respectively. Calculate $\Lambda _m^{\infty}$ for $Ba(OH)_2$ (in $S\,m^2\,mol^{-1}$).