$A$ conductivity cell has been calibrated with $0.01 \ M$ $1:1$ electrolyte solution (specific conductance, $k = 1.25 \times 10^{-3} \ S \ cm^{-1}$) in the cell and the measured resistance was $800 \ \Omega$ at $25^{\circ}C$. The cell constant will be (in $cm^{-1}$)

The conductivity of $0.001 \ M$ acetic acid at a certain temperature is $5.07 \times 10^{-5} \ S \ cm^{-1}$. If $\wedge_m^0$ of acetic acid at the same temperature is $390 \ S \ cm^2 \ mol^{-1}$,the dissociation constant of acetic acid at that temperature is:

What is the molar conductivity of $CH_3COOH$ at infinite dilution if the molar conductivities of $H_2SO_4$, $K_2SO_4$, and $CH_3COOK$ at infinite dilution are respectively $x$, $y$, and $z$ $\Omega^{-1} \text{ cm}^2 \text{ mol}^{-1}$?

At a certain temperature and at infinite dilution,the equivalent conductances of sodium benzoate,hydrochloric acid,and sodium chloride are $240$,$349$,and $229 \ \Omega^{-1} \ cm^2 \ equiv^{-1}$ respectively. The equivalent conductance of benzoic acid in $\Omega^{-1} \ cm^2 \ equiv^{-1}$ at the same conditions is

Molar conductivity of $0.01 \ M \ CH_3COOH$ is $19.5 \ \Omega^{-1} \ cm^2 \ mol^{-1}$. Calculate its degree of dissociation if molar conductivity at zero concentration is $390 \ \Omega^{-1} \ cm^2 \ mol^{-1}$.

If the molar conductivity of a solution is $1.26 \times 10^{2} \ \Omega^{-1} \ cm^{2} \ mol^{-1}$ and its molarity is $0.01 \ M$,what will be its specific conductivity?