Limiting molar conductivity of $CH_3COOH$ (i.e.,$\Lambda^o_{m(CH_3COOH)}$) is equal to:

The molar conductance of an infinitely dilute solution of ammonium chloride was found to be $185 \ S \ cm^2 \ mol^{-1}$ and the ionic conductance of hydroxyl and chloride ions are $170$ and $70 \ S \ cm^2 \ mol^{-1}$,respectively. If molar conductance of $0.02 \ M$ solution of ammonium hydroxide is $85.5 \ S \ cm^2 \ mol^{-1}$,its degree of dissociation is given by $x \times 10^{-1}$. The value of $x$ is $...........$ $(Nearest \ integer)$

Molar conductivity of $0.02 \ M$ weak acid is $7.92 \ \Omega^{-1} \ cm^2 \ mol^{-1}$ and its molar conductivity at infinite dilution is $232.7 \ \Omega^{-1} \ cm^2 \ mol^{-1}$. Calculate the degree of dissociation of the weak acid.

At $298 \ K$,the limiting molar conductivity of a weak monobasic acid is $4 \times 10^2 \ S \ cm^2 \ mol^{-1}$. At $298 \ K$,for an aqueous solution of the acid,the degree of dissociation is $\alpha$ and the molar conductivity is $y \times 10^2 \ S \ cm^2 \ mol^{-1}$. At $298 \ K$,upon $20$ times dilution with water,the molar conductivity of the solution becomes $3y \times 10^2 \ S \ cm^2 \ mol^{-1}$. $(1)$ The value of $\alpha$ is. . . . . . $(2)$ The value of $y$ is. . . . . .

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?

Conductivity of a saturated solution of a sparingly soluble salt $AB$ at $298 \ K$ is $1.85 \times 10^{-5} \ S \ m^{-1}$. Solubility product of the salt $AB$ at $298 \ K$ is. Given $\Lambda_{m}^{\circ}(AB) = 140 \times 10^{-4} \ S \ m^{2} \ mol^{-1}$.