Common Ion Effect and Solubility

The video explains the common ion effect, where adding a common ion to a solution reduces the solubility of an ionic compound. Using examples like barium sulfate and lead chromate, it illustrates how equilibrium shifts according to Le Chatelier's principle. The video also discusses the solubility product constant (Ksp) and provides a practice calculation involving silver chloride.

What is the common ion effect primarily concerned with?

• Altering the color of a solution

• Decreasing the solubility of ionic compounds

• Increasing the solubility of ionic compounds

• Changing the temperature of a solution

When sodium sulfate is added to a saturated solution of barium sulfate, what happens to the equilibrium?

• It shifts to the right

• It remains unchanged

• It shifts to the left

• It dissolves completely

According to Le Chatelier's principle, what is the effect of adding a common ion to a solution?

• It increases the solubility of the compound

• It decreases the concentration of the common ion

• It increases the concentration of all ions

• It has no effect on the equilibrium

What happens to the concentration of barium ions when sodium sulfate is added to the solution?

• It increases

• It decreases

• It remains the same

• It doubles

How does the common ion effect influence the solubility product constant (Ksp)?

• It decreases the Ksp

• It doubles the Ksp

• It does not change the Ksp

• It increases the Ksp

What remains constant when the common ion effect is applied to a solution?

• The color of the solution

• The temperature

• The Ksp value

• The concentration of all ions

What is the effect of adding sodium chromate to a solution of lead chromate?

• It increases the solubility of lead chromate

• It decreases the solubility of lead chromate

• It changes the color of lead chromate

• It has no effect on lead chromate

In the practice calculation, what is the first step to find the concentration of silver ions?

• Determine the volume of the solution

• Measure the temperature of the solution

• Find the moles of sodium chloride

• Calculate the molarity of silver ions

Why can we assume that the chloride concentration is mainly due to sodium chloride in the practice calculation?

• Because sodium chloride is not present

• Because the solubility product constant of silver chloride is very small

• Because silver chloride is very soluble

• Because sodium chloride is insoluble

What is the final step in calculating the concentration of silver ions in the practice problem?

• Rearrange the Ksp equation

• Measure the temperature

• Add more sodium chloride

• Calculate the volume of the solution