How does the conductivity of a strong electrolyte change upon dilution?

What is the conductivity of $0.01 \ M$ $NaCl$ solution if the resistance and cell constant of the $NaCl$ solution are $375 \ \Omega$ and $0.5 \ cm^{-1}$ respectively at $298 \ K$?

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.

What is the molar conductivity of $0.1 \ M$ $NaCl$ if its conductivity is $1.06 \times 10^{-2} \ \Omega^{-1} \ cm^{-1}$?

If the conductivity of a $0.5 \ M \ KCl$ solution at $298 \ K$ is $0.024 \ S \ cm^{-1}$,then the molar conductivity of the solution would be $S \ cm^2 \ mol^{-1}$.

The molar conductances of $Ba(OH)_2$, $BaCl_2$ and $NH_4Cl$ at infinite dilution are $523.28$, $280.0$ and $129.8 \ S \ cm^2 \ mol^{-1}$ respectively. The molar conductance of $NH_4OH$ at infinite dilution will be: