The molar conductivity of $0.007 \ M$ acetic acid is $20 \ S \ cm^{2} \ mol^{-1}$. What is the dissociation constant of acetic acid? (In $\times 10^{-5} \ mol \ L^{-1}$)
$[\Lambda_{H^{+}}^{\circ}=350 \ S \ cm^{2} \ mol^{-1}, \Lambda_{CH_{3}COO^{-}}^{\circ}=50 \ S \ cm^{2} \ mol^{-1}]$

The resistance of a conductivity cell containing $0.01 \, M \, KCl$ solution at $298 \, K$ is $1750 \, \Omega$. If the conductivity of $0.01 \, M \, KCl$ solution at $298 \, K$ is $0.152 \times 10^{-3} \, S \, cm^{-1}$,then the cell constant of the conductivity cell is $.......... \, \times 10^{-3} \, cm^{-1}$.

Resistance of a decimolar solution between two electrodes $0.02 \ m$ apart and $0.0004 \ m^2$ in area was found to be $50 \ \Omega.$ Specific conductance $(\kappa)$ is .......... $S \ m^{-1}$

The equivalent conductance of $NaCl$ at concentration $C$ and at infinite dilution are $\lambda_C$ and $\lambda_{\infty}$ respectively. The correct relationship between $\lambda_C$ and $\lambda_{\infty}$ is given as: (Where the constant $B$ is positive)

Resistance of $0.1\, M\, KCl$ solution in a conductance cell is $300\, \Omega$ and conductivity is $0.013\, S\, cm^{-1}$. The value of cell constant is

Assertion : On increasing dilution,the specific conductance keeps on increasing.
Reason : On increasing dilution,the degree of ionization of a weak electrolyte increases and the mobility of ions also increases.