Common Ion Effect and Equilibrium

The video tutorial explains the common ion effect, demonstrating it with a saturated solution of potassium chloride. By adding hydrochloric acid, which shares a common ion, the equilibrium shifts, causing potassium chloride to precipitate. This process is explained in detail, highlighting its applications in laboratory settings and classroom discussions.

What is the common ion effect?

• The addition of a compound with a different ion to a solution.

• The addition of a compound with the same ion to a saturated solution.

• The removal of ions from a solution.

• The dilution of a solution.

Why is it important for the solution to be saturated in the common ion effect?

• To ensure there are no ions present.

• To allow the solution to dissolve more solute.

• To maintain a dynamic equilibrium.

• To prevent any chemical reaction.

What happens when hydrochloric acid is added to a saturated solution of potassium chloride?

• The potassium chloride dissolves completely.

• The solution remains unchanged.

• The chloride ions increase, causing precipitation.

• The solution becomes unsaturated.

What is the concentration of the saturated potassium chloride solution used in the demonstration?

• 15 to 16 molar

• 10 to 12 molar

• 4 to 5 molar

• 1 to 2 molar

What is the role of chloride ions in the precipitation of potassium chloride?

• They dissolve the potassium chloride.

• They cause the potassium chloride to precipitate.

• They increase the solubility of potassium chloride.

• They have no effect on potassium chloride.

How does Le Chatelier's principle apply to the common ion effect?

• It indicates no change in equilibrium.

• It predicts the dissolution of solids.

• It explains the shift in equilibrium to form more solid.

• It suggests the removal of ions from the solution.

What is the result of adding a common ion to a saturated solution?

• The solubility of the solute increases.

• The solution becomes more dilute.

• The solute precipitates out of the solution.

• The solution becomes acidic.

In what scenarios can the common ion effect be applied?

• In the formation of precipitates.

• In the formation of gases.

• In the heating of solutions.

• In the dilution of solutions.

Why might precipitates form in a laboratory setting?

• Due to the addition of a common ion.

• Because of an increase in temperature.

• Because of the removal of a solvent.

• Due to a decrease in pressure.

What principle is used to explain the shift in equilibrium in the common ion effect?

• Avogadro's Law

• Le Chatelier's Principle

• Dalton's Law

• Boyle's Law