Resistance of a conductivity cell filled with a solution of an electrolyte of concentration 0.1M is `100Omega `. The conductivity of this solution is `1.29 S m^(-1)` . Resistance of the same cell when filled with 0.02M of the same solution is 520 `Omega` . The molar conductivity of 0.02M solution of the electrolyte will be
A
the electrode material and the solution in both half-cells are composed of the same substances
B
only the concentrations of solutions of ther same substances is different
C
`E_(cell)^(@)=0`
D
the Nernst equations reduces to `E_(cell)=-((0.0591)/(n))` log Q at `25^(@)C`
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The correct Answer is:
A, B, C, D
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The conductivity of 0.1 M KCl solution is 1.29 S m^(-1) . If the resistance of the cell filled with 0.1 M KCl is 100 Omega , Calculate the cell constant.
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Resistance of a conductivity cell filled with 0.1 mol L^(-1) KCl solution is 100Omega . If the resistacne of the same cell when filled with 0.02 mol L^(-1) KCl solution is 520 Omega , calculate the conductivity and molar conductivity of 0.02 mol L^(-1) KCl solution . The conductivity of 0.1 mol L^(-1) KCl solution is 1.29 S/m.
(A) : The conductivity of 0.1M solutions of different electrolytes is same. (R) : The conductivity depends on the size of the ions.
The resistance of 0.01N solution of an electrolyte AB at 328K is 100 ohm. The specific conductance of solution is ( cell constant =1 cm^(-1) )
Define conductivity and molar conductivity for the solution of an electrolyte. Discuss their variation with concentration.
