The resistance of a conductivity cell containing $0.001 \ M \ KCl$ solution at $298 \ K$ is $1500 \ \Omega$. What is the cell constant if the conductivity of $0.001 \ M \ KCl$ solution at $298 \ K$ is $0.146 \times 10^{-3} \ S \ cm^{-1}$?

For a strong electrolyte,a plot of molar conductivity against (concentration)$^{1/2}$ is a straight line,with a negative slope. The correct unit for the slope is:

$\wedge_{AgCl}^{\infty}$ can be obtained by:

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. . . . . .

The resistance of a decimolar solution of $NaCl$ is $30 \ \Omega$. Calculate the conductivity of the solution if the cell constant is $0.33 \ cm^{-1}$.

When the molar conductivity of a weak electrolyte is plotted against the square root of its concentration $(\sqrt{C})$,which of the following is observed?