Conductance in Electrolytic Solutions

The molar conductivity of a 1.5 M solution of an electrolyte is found to be 138.9 S  $c{m}^2$  $mo{l}^{-1}.$  Calculate the conductivity of the solution.

The molar conductivity of a $1.5 \mathrm{M}$ solution of an electrolyte is found to be$138.9 \mathrm{S} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}$. Calculate the conductivity of the solution?

The resistance of a conductivity cell containing $0.001\mathrm{MKCl}$ solution at $298 \mathrm{K}$ is $1500 \mathrm{\Omega }$. What is the cell constant if the conductivity of $0.001\mathrm{MKCl}$ solution at $298 \mathrm{K}$ is $0.146\times {10}^{-3} {\mathrm{Scm}}^{-1}.$

The limiting molar conductivities of the given electrolytes at $298 \mathrm{K}$ follow the order

${\lambda }_{\left({\mathrm{K}}^{+}\right)}^{\circ }=735 \mathrm{S} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}, {\lambda }_{\left({\mathrm{Cl}}^{-}\right)}^{\circ }=763 \mathrm{S} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}, {\lambda }_{\left({\mathrm{Ca}}^{2+}\right)}^{\circ }=1190 \mathrm{S} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}, {\lambda }_{\left({\mathrm{SO}}_4^{2-}\right)}^{\circ }=160.0 \mathrm{S} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}$

At a fixed concentration, the molar conductance of aqueous sodium hydroxide at $298 \mathrm{K}$ is found to be$10 {\mathrm{ohm}}^{-1}.{\mathrm{cm}}^2.{\mathrm{mol}}^{-1}$$.$At infinite dilution and $298 \mathrm{K}$$,$ its molar conductance is found to be $242 {\mathrm{ohm}}^{-1}.{\mathrm{cm}}^2.{\mathrm{mol}}^{-1}$$.$ Find the degree of ionization of sodium hydroxide at the same concentration and temperature.

If the conductivity of a $0.5\mathrm{MKCl}$ solution at $298 \mathrm{K}$ is $0.024 \mathrm{S}.{\mathrm{cm}}^{-1},$ then the molar conductivity of the solution would be ____ $\mathrm{S}.{\mathrm{cm}}^2·{\mathrm{mol}}^{-1}$

The molar conductivities of $\mathrm{KCl}, \mathrm{NaCl}$ and ${\mathrm{KNO}}_3$ are $100, 120$ and $90{ \mathrm{cm}}^2·{\mathrm{mol}}^{-1},$ respectively. The molar conductivity of ${\mathrm{NaNO}}_3$ would be _____  ${\mathrm{cm}}^2·{\mathrm{mol}}^{-1}$

The conductivity of solutions of different electrolytes in the same solvent and at a given temperature differs due to charge and size of the _____.

Explain the effect of dilution on the molar conductivity of a strong electrolyte.

The degree of ionisation of a weak electrolyte increases

Among the following, the plot that correctly represents the conductometric titration of $0.05 \mathrm{M}$ ${\mathrm{H}}_2{\mathrm{SO}}_4$ with $0.1 \mathrm{M} {\mathrm{NH}}_4\mathrm{OH}$ is

The molar conductivity of $0.02 \mathrm{M} \mathrm{HCl}$ solution is $407.2 \mathrm{S} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}$ at $25 °\mathrm{C}$. Its conductivity will be:

The conductivity of $0.10\mathrm{M}$ solution of $\mathrm{KCl}$ at $298\mathrm{K}$ is $0.0129 \mathrm{S} {\mathrm{cm}}^{-1}$. Calculate its molar conductivity?

The $\mathrm{SI}$unit of molar conductivity is

The conductance of a $0.0015 \mathrm{M}$ aqueous solution of a weak monobasic acid was determined by using a conductivity cell consisting of platinised Pt electrodes. The distance between the electrodes is $120 \mathrm{cm}$ with an area of cross-section of $1 \mathrm{cm}$. The conductance of this solution was found to be $5\times {10}^{-7} \mathrm{S}$. The $\mathrm{pH}$ of the solution is $4$. The value of limiting molar conductivity $\left({{\mathrm{\Lambda }}^{°}}_{\mathrm{m}}\right)$ this weak monobasic acid in aqueous solution is $\mathrm{Z}\times {10}^{2 }\mathrm{S} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}$.The value of $\mathrm{Z}$ is

${\mathrm{AgNO}}_3 \left(\mathrm{aq}\right)$ was added to an aqueous $\mathrm{KCl}$ solution gradually and the conductivity of the solution was measured. The plot of conductance $\left(\mathrm{\Lambda }\right)$ versus the volume of ${\mathrm{AgNO}}_3$ is