The Common Ion Effect

The video tutorial explains the common ion effect, an application of Le Chatelier's principle, which helps predict and control precipitation in chemical equilibria. It uses examples like silver iodide and cadmium sulfide to illustrate how adding a common ion shifts equilibrium, promoting precipitation. The tutorial includes a quantitative analysis of cadmium sulfide's solubility in a cadmium bromide solution, demonstrating how the presence of a common ion reduces solubility and enhances precipitation.

What principle is the common ion effect an application of?

• Boyle's Law

• Le Chatelier's Principle

• Avogadro's Law

• Dalton's Law

How does adding potassium iodide affect the equilibrium of silver iodide?

• It dissolves the silver iodide completely.

• It shifts the equilibrium to the left, promoting precipitation.

• It has no effect on the equilibrium.

• It shifts the equilibrium to the right, increasing solubility.

What is the Ksp value of cadmium sulfide used in the example?

• 1 x 10^-5

• 1 x 10^-10

• 1 x 10^-28

• 1 x 10^-20

In the cadmium sulfide example, what is the initial concentration of cadmium ion from cadmium bromide?

• 0.001 M

• 0.0001 M

• 0.01 M

• 0.1 M

How does the presence of cadmium ions in solution affect the molar solubility of cadmium sulfide?

• It increases the molar solubility.

• It reduces the molar solubility, promoting precipitation.

• It has no effect on the molar solubility.

• It dissolves the cadmium sulfide completely.