Which of the following $M$ $KCl$ solutions has the lowest value of equivalent conductance?

The resistance of $0.1 \ M$ weak acid $HA$ in a conductivity cell is $2 \times 10^3 \ \Omega$. The cell constant of the cell is $0.78 \ cm^{-1}$ and $\lambda_{m}^{\circ}$ of acid $HA$ is $390 \ S \ cm^2 \ mol^{-1}$. The $pH$ of the solution is

What is the molar conductivity of $0.02 \text{ M}$ $KI$ solution if its conductivity is $4.37 \times 10^{-4} \text{ } \Omega^{-1} \text{cm}^{-1}$?

Calculate the molar conductivity of $NH_4OH$ at infinite dilution,given that the molar conductivities of $Ba(OH)_2$,$BaCl_2$,and $NH_4Cl$ are $523.28$,$280.0$,and $129.8 \ \Omega^{-1} \ cm^2 \ mol^{-1}$ respectively.

At $298 \ K$ the molar conductivities at infinite dilution $(\Lambda_m^{\circ})$ of $NH_4Cl, KOH$ and $KCl$ are $152.8, 272.6$ and $149.8 \ S \ cm^2 \ mol^{-1}$ respectively. The $\Lambda_m^{\circ}$ of $NH_4OH$ in $S \ cm^2 \ mol^{-1}$ and $\%$ dissociation of $0.01 \ M \ NH_4OH$ with $\Lambda_m = 25.1 \ S \ cm^2 \ mol^{-1}$ at the same temperature are

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