Which of the following solutions has the maximum conductivity?

At $291 \ K$,a saturated solution of $BaSO_4$ was found to have a specific conductivity of $3.648 \times 10^{-6} \ \Omega^{-1} \ cm^{-1}$ and that of the water used is $1.25 \times 10^{-6} \ \Omega^{-1} \ cm^{-1}$. If the ionic conductances of $Ba^{2+}$ and $SO_4^{2-}$ are $110$ and $136.6 \ \Omega^{-1} \ cm^2 \ mol^{-1}$ respectively,the solubility of $BaSO_4$ at $291 \ K$ will be (Atomic masses: $Ba=137, S=32, O=16$)

The resistance of a $0.1 \ N$ solution of acetic acid is $250 \ \Omega$ and the cell constant is $1.15 \ cm^{-1}$. The equivalent conductance of $0.1 \ N$ acetic acid in $\Omega^{-1} \ cm^2 \ eq^{-1}$ is:

Which of the following has maximum molar conductivity?

For a salt $XY$, which is a strong electrolyte, the plot of $\Lambda_m$ versus $\sqrt{C}$ has a slope of $-90.0 \ S \ cm^2 \ mol^{3/2} \ L^{1/2}$ at $298 \ K$. At $0.01 \ M$ concentration of $XY$, the value of $\Lambda_m$ is $145.5 \ S \ cm^2 \ mol^{-1}$. The limiting molar conductivity of $Y^-$ ion ($\lambda^\circ_{Y^-}$, in $S \ cm^2 \ mol^{-1}$) at $298 \ K$ will be (Given $\lambda^\circ_{X^+} = 74.0 \ S \ cm^2 \ mol^{-1}$) (in $.0$)

What happens when the solution of an electrolyte is diluted?