The equivalent conductance of a 0.2 n solution of an electrolyte was found to be `200Omega^(-1) cm^(2)eq^(-1)` . The cell constant of the cell is `2 cm^(-1)` . The resistance of the solution is

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 :

Calculate the resistance of 0.01 N solution of an electrolyte whose equivalent conductivity is 420 ohm^(-1) cm^(2) equiv^(-1) . (The cell constant of the cell is 0.88 cm^(-1) )

The resistance of 0.01 N solution of an electrolyte waw found to be 210 ohm at 298 K, when a conductivity cell with cell constant 0.66 cm^(-1) is used. The equivalent conductance of solution is:

The resistance of 0.01 N solution of an electrolyte was found to be 220 ohm at 298 K using a conductivity cell with a cell constant of 0. 88cm^(-1) . The value of equivalent conductance of solution is

The resistance of 0.15 M solution of an electrolyte is 50Omega . The specific conductance of the solution is 2.4 Sm^(-1) . The resistance of 0.5 N solution of the same electrolyte measured using the same conductivity cell is 480Omega . Find the equivalent conductivity of 0.5 N solution of the electrolyte.

The resistance of 0.1 N solution of a salt is found to be 2.5xx10^(3) Omega . The equivalent conductance of the solution is (Cell constant =1.15 cm^(-1) )

The resistance of 0.1 N solution of a salt is found to be 2.5xx10^(3) Omega . The equivalent conductance of the solution is (Cell constant =1.15 cm^(-1) )