Electrolyte Conductivity Quiz

As a strong electrolyte solution is diluted (concentration decreases), its molar conductivity:

• decreases

• increases

• remains constant

• first increases then decreases

Which of the following correctly describes a weak electrolyte in solution?

• It completely dissociates into ions even at high concentration.

• It partially dissociates into ions, with a degree of dissociation that increases on dilution.

• Its molar conductivity is independent of concentration.

• It has a higher conductivity than a strong electrolyte at the same concentration.

The limiting molar conductivity (Λ_m⁰) of an electrolyte is defined at:

• room temperature

• infinite dilution (very low concentration)

• the boiling point of the solvent

• the saturation point of the solution

For a weak electrolyte, the plot of molar conductivity (Λ_m) versus √c (where c is concentration) is:

• a straight line

• a curved line that increases sharply at low concentrations

• a horizontal line

• an exponential decay curve

For a weak monoprotic electrolyte, the degree of dissociation α is given by:

• Λ⁰ / Λ

• Λ / Λ⁰

• (Λ_m⁰ - Λ_m) / Λ_m⁰

• √(Λ_m / Λ_m⁰)

In the conductometric titration of a strong acid with a strong base, the conductance versus volume curve typically:

• monotonically increases

• monotonically decreases

• decreases to a minimum at the equivalence point, then increases

• remains constant up to the equivalence point, then increases

In a conductometric titration of a strong acid by a weak base , the solution's conductivity as titrant is added:

• increases continuously

• decreases to a minimum at the equivalence point and then remains constant

• decreases continuously without a minimum

• remains nearly constant up to the equivalence point and then decreases

Describe the conductometric titration of a strong acid by a weak base. How does the conductance change before, at, and after the equivalence point.

define Strong electrolytes and give example

Draw and explain the conductometric titration between a strong acid with a weak base.