What is the ionic mobility of $Ag^{+}$? Given $\lambda^{Ag^{+}} = 5 \times 10^{-4} \ \Omega^{-1} \ cm^{2} \ eq^{-1}$.

The specific conductance (conductivity) of a solution is $0.2 \ \Omega^{-1} cm^{-1}$ and its conductance is $0.04 \ \Omega^{-1}$. The cell constant would be .............. $cm^{-1}$.

Which of the following is the correct equation representing the change in molar conductivity with respect to concentration for a weak electrolyte,where the symbols carry their usual meaning?

The molar conductivity of $0.025 \ M$ methanoic acid is $46.1 \ S \ cm^2 \ mol^{-1}$. Calculate its degree of dissociation. Given: $\lambda^0(H^{+}) = 349.6 \ S \ cm^2 \ mol^{-1}$ and $\lambda^0(HCOO^{-}) = 54.6 \ S \ cm^2 \ mol^{-1}$.

The resistance of $0.1 \ M$ weak acid $HA$ in a conductivity cell is $2 \times 10^3 \ \Omega$. The cell constant of the cell is $0.78 \ cm^{-1}$ and $\lambda_{m}^{\circ}$ of acid $HA$ is $390 \ S \ cm^2 \ mol^{-1}$. The $pH$ of the solution is

The resistance of a $0.5 \, M$ solution of an electrolyte in a cell was found to be $50 \, \Omega$. If the electrodes in the cell are $2.2 \, cm$ apart and have an area of $4.4 \, cm^2$,then the molar conductivity (in $S \, m^2 \, mol^{-1}$) of the solution is: