Resistance of a conductivity cell filled with 0.1 M `KCl` solution is 100 ohms. If the resistance of the same cell when filled with 0.02 M `KCl` solution is 520 ohms, calculate the conductivity and molar conductivity of 0.02 M `KCl` solution. (The conductivity of 0.1 M `KCl` solution is 1.29 `Sm^(-1)`).

The resistance of a conductivity cell when filled with 0.05M solution of an electrolyte x is 100 Omega at 40^(@)C . The same conductivity cell filled with 0.01M solution of electrolyte y has a resistance of 50 Omega . The conductivity of 0.05 M solution of electrolyte x is 1.0 xx 10^(-4) S cm^(-1) . Calculate (i) cell constant (ii) conductivity of 0.01 M solution (iii) molar conductivity of 0.01 M solution

A cell when dipped in 0.5M sucrose solution has no effect, but when the same cell will be dipped in 0.5 M NaCl solution, it will:

If specific conductivity of N// 50 KCl solution at 298 K is 0.002765 Omega^(-1) cm^(-1) and resistance of a cell contaning this solution is 100 Omega , calculate the cell constant.

The specific conductivity of an N//20 solution of KCI at 25^@ C is 0.002765 mhos. If the resistance of the same solution placed in the cell is 2000 ohm, what is the cell constant ?

The resistance of a conductivity cell containing 0.001 M KCl solution at 298 K is 1500 Omega . What is the cell constant if the conductivity of 0.001 M KCl solution at 298 K is 0.146 xx 10^(-3) S cm^(-1) ?

The specific conductivity of 0.1 N kCl solution is 0.0129 ohm^(-1) cm^(-1) . The resistance of the solution in the cell is 100ohm . The cell constant of the cell is

The conductivity of 0.20 M solution of KCl at 298 K is 0.248S cm^(-1) . Calculate its molar conductivity.

At a certain temperature the specific conductance of 0.40M KCl solution is 4.96xx10^-2 ohm^-1cm^-1 . Calculate its molar conductance.