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 $400 \ S \ cm^2 \ mol^{-1}$.

The specific conductance $(k)$ of $0.02 \ M$ aqueous acetic acid solution at $298 \ K$ is $1.65 \times 10^{-4} \ S \ cm^{-1}$. The degree of dissociation $(\alpha)$ of acetic acid is: [Given: $\lambda_{H^{+}}^{\infty} = 349.1 \ S \ cm^2 \ mol^{-1}$ and $\lambda_{CH_3COO^{-}}^{\infty} = 40.9 \ S \ cm^2 \ mol^{-1}$]

What will be the concentration of $NaCl$ solution,if the molar conductivity and conductivity of $NaCl$ solution are $124.3 \ \Omega^{-1} \ cm^{2} \ mol^{-1}$ and $1.243 \times 10^{-4} \ \Omega^{-1} \ cm^{-1}$ respectively?

At $298 \ K$,the resistance of a $0.01 \ N$ electrolyte solution is $210 \ \Omega$. If the cell constant of the conductivity cell used is $0.66 \ cm^{-1}$,what is the equivalent conductivity of the solution in $mho \ cm^2 \ eq^{-1}$?

The resistivity of a $0.8 \ M$ solution of an electrolyte is $5 \times 10^{-3} \ \Omega \ cm$. Its molar conductivity is $..... \times 10^4 \ \Omega^{-1} \ cm^2 \ mol^{-1}$. (Nearest integer)

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: