The graphical variation of molar conductivity $(\Lambda_m)$ against the square root of molar concentration $(\sqrt{c})$ for a certain electrolyte '$X$' is linear with an intercept on the y-axis. Identify '$X$' from the following.

The molar conductivity of $0.025 \ M$ methanoic acid is $46.1 \ S \ cm^2 \ mol^{-1}$. Calculate its degree of dissociation. Given: $\lambda^0(H^{+}) = 349.6 \ S \ cm^2 \ mol^{-1}$ and $\lambda^0(HCOO^{-}) = 54.6 \ S \ cm^2 \ mol^{-1}$.

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 $S\,m^2\,mol^{-1}$).

The specific conductance of $0.0025 \ M$ acetic acid is $5 \times 10^{-5} \ S \ cm^{-1}$ at a certain temperature. The dissociation constant of acetic acid is $...... \times 10^{-7}$. (Nearest integer) Consider limiting molar conductivity of $CH_3COOH$ as $400 \ S \ cm^2 \ mol^{-1}$.

Resistance of a cell containing $0.02 \ M \ KCl$ solution is $164 \ \Omega$. If the cell is filled with $0.05 \ M \ AgNO_3$,the resistance becomes $75.8 \ \Omega$. Calculate the following: [Conductivity of $0.02 \ M \ KCl = 2.768 \times 10^{-3} \ \Omega^{-1} \ cm^{-1}$] $(i)$ Conductivity of $0.05 \ M \ AgNO_3$ (ii) Molar conductivity of $AgNO_3$ solution.

Which of the following $M$ solutions of $KCl$ has the lowest value of specific conductivity?