The specific conductance of a 0.1 M KCl solution at 23$°\mathrm{C}$ is 0.012 ${\mathrm{\Omega }}^{-1}{\mathrm{cm}}^{-1}$.
The resistance of the cell containing the solution at the same temperature
was found to be 55 $\mathrm{\Omega }$. The cell constant will be:

1. 0.142 cm^-1
2. 0.66 cm^-1
3. 0.918 cm^-1
4. 1.12 cm^-1

The $k=$ $4.95$ $\times$ ${10}^{-5}S$ $c{m}^{-1}$ for a 0.00099 M solution. The reciprocal of the degree of dissociation of acetic acid, if ${\wedge }_m^0$ for acetic acid is 400 S $c{m}^{2}mo{l}^{-1}$ will be:

The conductivity of 0.20 M solution of KCl at 298 K is 0.0248 S cm^–1. The molar conductivity will be -

The molar conductivity of a 0.5 mol/dm³ solution of AgNO₃ with electrolytic conductivity of 5.76 x 10^-3 S cm^-1 at 298 K is:

1. 11.5 S cm²/mol
2. 21.5 S cm²/mol
3. 31.5 S cm²/mol
4. 41.5 S cm²/mol

The unit of specific conductance is:

The cell constant of a conductivity cell-

Consider the following graph.

The strong electrolyte in the above graph is represented by:

1. X

2. Y

3. Both X and Y

4. Data given is not sufficient to predict.

At 25 °C molar conductance of 0.1 molar aqueous solution of ammonium hydroxide is 9.54 Ω^-1 cm² mol^-1 and at infinite dilution its molar conductance is 238 Ω^-1 cm² mol^-1. The degree of ionisation of ammonium hydroxide at the same concentration and temperature is :

The incorrect statement about the solution of electrolytes is:

Limiting molar conductivities, for the given solutions, are :

${\lambda }_m^0\left(H_{2}S{O}_4\right)= x$ $\mathrm{S }c{m}^2$ $mo{l}^{-1}$

${\lambda }_m^0\left(K_{2}S{O}_4\right)= y$ $\mathrm{S }c{m}^2$ $mo{l}^{-1}$

${\lambda }_m^0\left(C{H}_{3}COOK\right)= z$ $\mathrm{S }c{m}^2$ $mo{l}^{-1}$

From the data given above, it can be concluded that \(\lambda_m^0 \) in (\(S\ cm^2\ mol^{-1}\)) for CH₃COOH will be :