Measurement of the Conductivity of Ionic Solutions

The resistance of a conductivity cell containing 0.001 M KCI solution at 298 K is 1500  $\Omega .$  The cell constant would be (if the conductivity of 0.001 M KCI solution at 298 K is  $0.146\times {10}^{-3}\text{S}{\text{cm}}^{-1}$  ):  

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 $0.146\times {10}^{-3} {\mathrm{Scm}}^{-1}.$

If the resistance of $0.1\mathrm{M} \mathrm{KCl}$ solution in a conductance cell is $300 \mathrm{\Omega }$ and conductivity is $0.013 \mathrm{S}.{\mathrm{cm}}^{-1},$ then the value of cell constant is $\_\_\_\_\_\_\_\_\_$

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 _____.

Quantity of electricity required to reduced $0.1$ mole of ${\mathrm{Cr}}_2{\mathrm{O}}_7^{-2}$ to ${\mathrm{Cr}}^{+3}$ completely is:-

What is a conductivity cell?

What are the electrodes of a conductivity cell generally coated with?

How many electrode/electrodes are present in a conductivity cell?

Which of the following relations are not correct ?

A weak electrolyte having the limiting equivalent conductance of $400 \mathrm{S} {\mathrm{cm}}^{2 }\mathrm{g} {\mathrm{equivalent}}^{-1}$at $298 \mathrm{K}$ is $2\%$ ionized in its $0.1 \mathrm{N}$ solution. The resistance of this solution (in ohms) in an electrolytic cell of cell constant $0.4 {\mathrm{cm}}^{-1}$ at this temperature is

The units of cell constant are:

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

What is cell constant? What is its unit? How is it determined?

The unit of cell constant is-

The specific conductivity of 0.1 N KCl solution is 0.0129 ${\mathrm{\Omega }}^{-1}{\mathrm{c}\mathrm{m}}^{-1}.$ The resistance of the solution in the cell 100Ω. The cell constant of the cell (in cm^-1) will be

What is the cell constant of a cell of KCl containing N/50 solution, if the conductivity and resistance of cell is ${\text{0.002765 S cm}}^{-1}$ and 400 ohm respectively.