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On what factors the electrical conductan...

On what factors the electrical conductance of an aqueous solution of electrolyte depends ?

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The electrical conductance of an equeous solution of electrolyte depends on
i) The nature of the electrolyte
ii) Size and solvation of the ions formed in the dissociation of the electrolyte.
iii) The nature and viscosity of the solvent.
iv) Concentration of the electrolyte
v) Temperature
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Knowledge Check

  • The equivalent conductance of 1N solution of an electrolyte is nearly

    A
    Same as its specific conductance
    B
    `10^(-3)` times its specific conductance
    C
    `10^(2)` times more than its specific conductance de
    D
    `10^(3)` times more than its specific conductance

  • Conductors allow the passage of electric current through them. Metallic and electrolytic are the two types of conductors. Current carriers in metallic and electrolytic conductors are free electrons and free ions respectively. Specific conductance or conductivity of the electrolyte solution is given by the following relation: K= cx (l)/(A) where, c=1/R is the conductance and 1/A is the cell constant, Molar conductance (^^_m) and equivalence conductance (^^_e) of an electrolyte solution are calculated using the following similar relations: ^^_m = K xx (1000)/(M) ^^_(e) = K xx (1000)/(N) where, M and N are the molarity and normality of the solution respectively. Molar conductance of strong electrolyte depends on concentration : ^^_m = ^^_m^(0) - b sqrt(C) ^^_m^(0) = molar conductance at infinite dilution C = concentration of the solution b = constant The degrees of dissociation of weak electrolytes are calculated as alpha = (^^_m)/(^^_m^(0)) = (^^_e)/(^^_e^(0)) Which of the following decreases on dilution of electrolytic solution?

    A
    Equivalent conductance
    B
    Molar conductance
    C
    Specific conductance
    D
    Conductance

  • Conductors allow the passage of electric current through them. Metallic and electrolytic are the two types of conductors. Current carriers in metallic and electrolytic conductors are free electrons and free ions respectively. Specific conductance or conductivity of the electrolyte solution is given by the following relation: K= cx (l)/(A) where, c=1/R is the conductance and 1/A is the cell constant, Molar conductance (^^_m) and equivalence conductance (^^_e) of an electrolyte solution are calculated using the following similar relations: ^^_m = K xx (1000)/(M) ^^_(e) = K xx (1000)/(N) where, M and N are the molarity and normality of the solution respectively. Molar conductance of strong electrolyte depends on concentration : ^^_m = ^^_m^(0) - b sqrt(C) ^^_m^(0) = molar conductance at infinite dilution C = concentration of the solution b = constant The degrees of dissociation of weak electrolytes are calculated as alpha = (^^_m)/(^^_m^(0)) = (^^_e)/(^^_e^(0)) For which of the following electrolytic solution ^^_m and ^^_e are equal ?

    A
    `BaCl_2`
    B
    `KCl`
    C
    `Al_2(SO_4)_3`
    D
    `CaCl_2`

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    Conductors allow the passage of electric current through them. Metallic and electrolytic are the two types of conductors. Current carriers in metallic and electrolytic conductors are free electrons and free ions respectively. Specific conductance or conductivity of the electrolyte solution is given by the following relation: K= cx (l)/(A) where, c=1/R is the conductance and 1/A is the cell constant, Molar conductance (^^_m) and equivalence conductance (^^_e) of an electrolyte solution are calculated using the following similar relations: ^^_m = K xx (1000)/(M) ^^_(e) = K xx (1000)/(N) where, M and N are the molarity and normality of the solution respectively. Molar conductance of strong electrolyte depends on concentration : ^^_m = ^^_m^(0) - b sqrt(C) ^^_m^(0) = molar conductance at infinite dilution C = concentration of the solution b = constant The degrees of dissociation of weak electrolytes are calculated as alpha = (^^_m)/(^^_m^(0)) = (^^_e)/(^^_e^(0)) Which of the following equality holds good for the strong electrolytes?

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