A conductivity cell dipped in 0.0005 M NaCl gives at `25^@C` resistance of 13710 ohms.If the electrode of the conductivity cell are 0.7 cm apart and the area of cross section of the electrode is `0.82cm^2`,what is the molar conductivity of the solution at `25^@C`?

The distance between the electrodes of a conductivity cell is 0.98 cm and area of cross section of theeletrodeis 1.3cm^2 . Calculate the cell constant for the cell.

Two electrodes are fitted in conductance cell 1.5 cm apart while the area of cross-section of each electrode is 0.75 cm^(2) . The cell constant is

a conductivity cell, the distance between two electrodes is 0.62 cm and the area of cross section of the electrode is 1.15 cm^2 . Find the cell constant of the cell.

The electrodes of a conductivities cell are 3 cm apart and have a cross-sectional area of 4 cm^(2) . The cell constant of the cell (in cm^(-1) ) is _________

A conductivity cell has two electrodes 50 mm apart and of cross section area 2.5 cm^2 . Find the cell constant.

Conductivity of, a solution is 6.23 xx 10^(-5) Omega^(-1) cm^(-1) and its resistance is 13710 Omega . If the electrode are 0.7 cm apart, calculate the cross-sectional area of electrode.

A conductivity cell dipped in 0.01 M AgNO_3 solution at 25^@C gives a resistance of 1442 ohms. If the molar conductivity of 0.01M AgNO_3 solution is 124.8 Omega^(-1) cm^2 mol^(-1) , what is the cell constant?

A conductivity cell filled with 0.02M H_2SO_4 at 25^@C gives a resistance of 122ohms. If the molar conductivity of 0.02M H_2SO_4 is 618 Omega^(-1) cm^2 mol^(-1) , what is the cell constant?

A conductivity cell filled with 0.01M KCl gives at 25^@C gives the resistance of 604 ohms. The conductivity of KCl at 25^@C is 0.00141Omega^(-1) 1cm^(-1) . The same cell filled with 0.001M AgNO_3 gives a resistance of 6529 ohms. Calculate the molar conductivity of 0.001M AgNO_3 [Conductivity of 0.01M KCl at 25^@C is 0.00141 Omega^(-1) cm^(-1) ]