For an electrolytic solution,specific conductance is $9.2 \times 10^{-2} \ \Omega^{-1} \ m^{-1}$,then calculate the value of molar conductance for a solution having a concentration of $0.02 \ M$.
- A$4.6 \times 10^{-3} \ S \ m^2 \ mol^{-1}$
- B$4.6 \times 10^2 \ S \ m^2 \ mol^{-1}$
- C$9.2 \times 10^{-2} \ S \ m^2 \ mol^{-1}$
- D$4.6 \times 10^{-5} \ S \ m^2 \ mol^{-1}$
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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 $.......... \, \times 10^{-3} \, cm^{-1}$.
The resistance of $0.01 \ M$ $KCl$ solution at $298 \ K$ is $1500 \ \Omega$. If the conductivity of $0.01 \ M$ $KCl$ solution at $298 \ K$ is $0.1466 \times 10^{-3} \ S \ cm^{-1}$,the cell constant of the conductivity cell in $cm^{-1}$ is:
DifficultKCET 2021
View SolutionThe unit of cell constant is
Easy
View SolutionFor which of the following electrolytes does the graph of $\Lambda_m$ vs $\sqrt{C}$ give a negative slope?
$0.01\, S\, m^2\, mol^{-1} = $ ....... $S\, cm^2\, mol^{-1}$
Medium
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