Jennifer Kastner from A-Plus College Ready explains solubility equilibrium, focusing on the behavior of soluble salts in aqueous solutions. The video covers the formation of precipitates, the calculation of KSP from solubility, and the use of ICE tables. It also discusses the common ion effect and its impact on solubility, providing practice problems to reinforce learning.

What is the role of water molecules in solubility equilibrium?

• They have no effect on ions in a solution.

• They form a solid barrier around ions.

• They attract and surround ions, facilitating dissolution.

• They repel ions in a solution.

What happens when silver nitrate is added to sodium chloride in a solution?

• The solution remains clear.

• The solution turns blue.

• A precipitate of silver chloride forms.

• The ions dissolve completely.

Which of the following is not included in an equilibrium expression?

• Liquid solvents

• Aqueous ions

• Pure solids

• Gaseous reactants

How do you calculate KSP from a given molarity?

• Multiply the molarity by the volume.

• Square the molarity value.

• Use the molarity in the equilibrium expression.

• Divide the molarity by the number of ions.

What is the significance of the reaction quotient (Q) in solubility?

• It calculates the mass of the precipitate.

• It determines the color of the solution.

• It indicates the direction of the reaction shift.

• It measures the temperature of the solution.

When is a solution considered supersaturated?

• When Q is greater than KSP

• When Q is equal to KSP

• When Q is zero

• When Q is less than KSP

What effect does a common ion have on the solubility of a salt?

• It has no effect on solubility.

• It decreases the solubility.

• It increases the solubility.

• It changes the color of the solution.

Which ion is common in both potassium nitrate and potassium sulfate?

• Chloride

• Potassium

• Sulfate

• Nitrate

How does increasing the concentration of silver ions affect the equilibrium?

• It shifts towards the solid silver carbonate.

• It causes the solution to evaporate.

• It shifts towards more dissolution.

• It has no effect on equilibrium.

What is the relationship between temperature and solubility equilibrium?

• Temperature has no effect.

• Solubility decreases with temperature.

• Solubility is temperature dependent.

• Temperature only affects gaseous solutes.