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The cell constant of a conductivity cell...

The cell constant of a conductivity cell

A

changes with change of electrolyte.

B

changes with change of concentration of electrolyte.

C

changes with temperature of electrolyte.

D

remains constant for a cell.

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The correct Answer is:
D
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The resistance of a conductivity cell containing 0.001 M KCl solution at 298 K is 1500 Omega . What is the cell constant if conductivity of 0.001 M KCl solution at 298 K is 0.146 X 10^(-3) Scm^(-1) ?

The resistance of a conductivity cell filled with 0.1 M KCl solution is 100 Omega . If R of the same cell when filled with 0.02 M KCl solution is 520 Omega , calculate the conductivity and molar conductivity of 0.02 M KCl solution. The conductivity of 0.1 M KCl solution is 1.29 S m^(-1) .

(a) Explain why electrolysis of aqueous solution of NaCl gives H_2 at cathode and Cl_2 at anode. Write overall reaction. (b) The resistancee of a conductivity cell containing 0.000M KCl solution at 298K is 1500 Omega . Calculate the cell constant if conductivity of 0.001M KCl solution at 298K is 0.146 times 10^-3 S cm^-1 .

c) Resistance of a conductivity cell containing 0.1 M KCl solution is 100Omega . Cell constant of the cell is 1.29/cm. Calculate the conductivity of the solution at the same temperature.

The molar conductance of a 0.1 M solution of an electrolyte was found to be 400 ohm^(-1) cm^(2) "mol"^(-1) . The cell constant of the cell is 0.1cm^(-1) . The resistance of the solution is :

The resistivity of 0.5 N solution of an electrolyte in a conductivity cell was found to be 45 ohms. The equivalent conductance of the same solution is ... if the electrodes in the cell are 2.2 cm part and have an area of 3.8 cm^2

The cell constant is product of resistance and

Which of these is usually constant for a variety of cells?

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