The correct order of equivalent conductances at infinite dilution in water at room temperature for $H^{+}$, $K^{+}$, $CH_{3}COO^{-}$ and $HO^{-}$ ions is

If $x$ is the specific conductance (in $S \ cm^{-1}$) of an electrolyte solution and $y$ is the molarity of the solution,then $\Lambda_m$ (in $S \ cm^2 \ mol^{-1}$) is given by:

$A$ $KCl$ solution of conductivity $0.14 \, S m^{-1}$ shows a resistance of $4.19 \, \Omega$ in a conductivity cell. If the same cell is filled with an $HCl$ solution,the resistance drops to $1.03 \, \Omega$. The conductivity of the $HCl$ solution is $....... \, \times 10^{-2} \, S m^{-1}$. (Round off to the Nearest Integer).

What is the effect of dilution on the equivalent conductivity of a strong electrolyte?

In an aqueous solution,how does specific conductivity of electrolytes change with the addition of water?

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 $\Lambda^{0}_{HOAc}$?