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The molar conductivity of 0.05 M of solution of an electrolyte is 200 Ω-1 cm2 mol-1. The resistance offered by a conductivity cell with cell constant (1/3 cm-1) would be _______Ω.
    Correct answer is '33.33'. Can you explain this answer?
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    Calculation of Resistance Offered by a Conductivity Cell:

    Given:

    - Molar conductivity of the electrolyte solution = 200 -1 cm2 mol-1
    - Concentration of the electrolyte solution = 0.05 M
    - Cell constant of the conductivity cell = 1/3 cm-1

    Formula:

    - Molar conductivity (λ) = K / C
    - Resistance (R) = 1 / G
    - Conductance (G) = K / L

    Where,

    - K = conductivity of the solution
    - C = concentration of the solution
    - L = distance between the electrodes of the cell

    Calculation:

    - Molar conductivity (λ) = 200 -1 cm2 mol-1
    - Concentration (C) = 0.05 M

    Therefore, the conductivity (K) of the solution can be calculated as:

    K = λ x C
    = 200 x 0.05
    = 10 S cm-1

    - Cell constant (L) = 1/3 cm-1

    Therefore, the conductance (G) of the solution can be calculated as:

    G = K / L
    = 10 / (1/3)
    = 30 S

    - Resistance (R) = 1 / G
    = 1 / 30
    = 0.0333 Ω

    Therefore, the resistance offered by the conductivity cell is 33.33 Ω.
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    The molar conductivity of 0.05 M of solution of an electrolyte is 200 Ω-1 cm2 mol-1. The resistance offered by a conductivity cell with cell constant (1/3 cm-1) would be _______Ω.Correct answer is '33.33'. Can you explain this answer?
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