Test: Electrochemistry - 3 - Chemistry MCQ

The minimum equivalent conductance in fused state is shown by:

According to Kohlrausch law, the limiting value of equivalent conductivity of an electrolyte, A₂B is given by:

The molecular conductivity and equivalent conductivity are same for the solution of:

Variation of molar conductivity with concentration of strong electrolyte is given by Huckel-Onsager equation expressed as:

The molar conductivity of NaCl, HCl and CH₃COONa at infinite dilution are 126.45, 426.16 and 91 S cm² mol^–1 respectively. The molar conductivity of CH₃COOH at infinite dilution is:

The conductivity of N/10 KCl solution at 20°C is 0.0212 S cm^–1 and the resistance of cell containing this solution at 20°C is 55 ohm. The cell constant is:

The limiting molar conductivities of NaCl, KBr and KCl are 126, 152 and 150 S cm² cm^–1 respectively. Thefor NaBr is:

The equivalent conductivity o f 0.1 M weak acid is 100 times less than that at infinite dilution. The degree of dissociation of weak electrolyte at 0.1 M is:

Limiting molar ionic conductivities of uni-univalent electrolyte are 57 and 73. The limiting molar conductivity of the solution will be:

Which statement is not correct for Kohlrausch law:

Molar conductivity and equivalent conductivity for an electrolyte A_xB_y at any dilution are related as:

The charge on cation and anion of an electrolyte is n⁺ and v^- respectively. One molecule of electrolyte furnishes ‘c’ cations and ‘a’ anions. Which expression is not correct:

Which statement is correct about  (i.e., ionic conductivit ies):

Which is correct relation:

The conductivity k(in S m^–1) is related with molar conductivity(in S m² mol^–1) by the relation (M is molarity in mol m^–3)

Cell constant of a conductivity cell is generally obtained by measuring conductance of aqueous solution of:

The conductivity of 1 × 10^–3 M acetic acid is 5 × 10^–5 S cm^–1 and is 390.5 S cm^–1 mol^–1. The dissociation constant of acetic acid is:

Which of the following shows, the highest electrical conductance in aqueous solution:

AgNO₃(g) was added to an aqueous KCl solution gradually and the conductivity of the solution was measured. The plot of conductance () versus the volume of AgNO₃ is:

Resistance of 0.2 M solution of an electrolyte is 50 Ω. The specific conductance of the solution is 1.4 S m^–1. The resistance of 0.5 M solution of the same electrolyte is 280 Ω. The molar conductivity of 0.5 M solution of the electrolyte in S m² mol^–1 is:

The equivalent conductance of NaCl at concentration C and at infinite dilution are λ_C and λ_∞ respectively. The correct relationship between λ_C and λ_∞ is given is:

Resistance of a conductivity cell filled with a solution of an electrolyte of concentration 0.1 M is 100 ohm. The conductivity of this solution is 1.29 S m^–1. Resistance of the same cell filled with 0.02 M of the same solution if the electrolyte is 520 ohm. The molar conductivity of 0.02 M solution of electrolyte would be:

The mean ionic activity coefficient of 0.0005 mol kg^–1 CaCl₂ in water at 25°C is:

According to the Debye-Huckel limiting law, the mean activity coefficient of 5 × 10^–4 mol kg^–1 aqueous solution of CaCl₂ at 25°C is (the Debye-Huckel constant ‘A’ can be taken to be 0.509)]

According to the Debye-Huckel limiting law if the concentration of a dilute aqueous solution of KCl is increased 4-fold, the value of ln γ± (γ± is the molal mean ionic activity coefficient) will:

For a 1 molal aqueous NaCl solution, the mean ionic activity coefficient (γ±) and the Debye-Huckel limiting law constant (A) are related as:

Specific conductance of 0.01 M KCl solution is x ohm^–1 cm^–1. When conductivity cell is filled with 0.01 M KCl the conductance observed is y ohm^–1. When the same cell is filled with 0.01 M H₂SO₄, the observed conductance was Z ohm^–1 cm^–1. Hence specific conductance of 0.01 M H₂SO₄ is: