What You Need to Know

Key Concept Diagram

A saturated solution contains as much dissolved solute as the solvent can hold at a given temperature

Dynamic equilibrium exists when the rate of dissolution equals the rate of precipitation

The solubility product Ksp is the equilibrium constant for a sparingly soluble ionic compound

Adding a common ion decreases solubility (the common ion effect), shifting equilibrium toward precipitation

Temperature affects solubility: most solids dissolve more readily at higher temperatures, but gases dissolve less

Key Vocabulary

Saturated solution

A solution containing the maximum amount of dissolved solute at a given temperature

Solubility product (Ksp)

The equilibrium constant for the dissolution of a sparingly soluble ionic compound

Common ion effect

The decrease in solubility of a compound when a common ion is added to the solution

Dynamic equilibrium

A state where forward and reverse reactions occur at equal rates, maintaining constant concentrations

Knowledge Check

Select the correct answer for each question. Click "Check Answer" to see if you are right.

Question 1

In a saturated solution of silver chloride (AgCl), dynamic equilibrium means:

No silver chloride is dissolving or precipitating All the silver chloride has dissolved The concentration of ions is continually increasing Dissolution and precipitation occur at equal rates

Question 2

Adding NaCl to a saturated solution of AgCl will:

Decrease the solubility of AgCl due to the common ion effect Have no effect on AgCl solubility Increase the solubility of AgCl Dissolve all remaining AgCl

Question 3

Most solids become more soluble as temperature increases. What is the trend for gases in water?

Gases also become more soluble at higher temperatures Gas solubility decreases as temperature increases Temperature has no effect on gas solubility Gases only dissolve below 0°C

Solubility and Equilibrium