Chem 8-3 Solubility Basics

Open Ended

Describe what happens at the molecular level when a solute dissolves in a solvent, using water as an example.

Multiple Choice

Why is solubility an important concept in chemistry?

• It helps us understand how substances interact in solutions.

• It determines the color of a compound.

• It is only relevant for gases.

• It is unrelated to chemical reactions.

Multiple Choice

Which of the following statements best describes an insoluble substance?

• A substance that does not dissolve in water and forms a precipitate.

• A substance that dissolves completely in water.

• A substance that evaporates quickly.

• A substance that reacts with water to form a gas.

Multiple Choice

What is an example of a soluble ionic compound?

• NaCl

• AgCl

• CO2

• C6H12O6

Multiple Select

Which of the following statements are true about polar substances and ionic compounds dissolving in water?

• They attract water molecules directly.

• They always dissolve in water.

• Water forms hydration shells around them.

• They never dissolve in water.

Multiple Choice

Why do many nonpolar substances not dissolve in water?

• They stick better to each other than to water.

• They react with water to form a precipitate.

• They form hydration shells easily.

• They are always gases.

Open Ended

Explain how scientists use solubility rules to determine whether an ionic salt will dissolve in water.

Multiple Select

Based on the solubility curves, which substances show an increase in solubility as temperature rises?

• NaCl

• NaNO3

• NH3

• KBr

Multiple Choice

Which of the following statements best explains the effect of temperature on the solubility of ammonia in water?

• As temperature increases, ammonia's solubility in water increases.

• As temperature increases, ammonia's solubility in water decreases.

• Ammonia's solubility in water is unaffected by temperature.

• Ammonia becomes a solid at higher temperatures.

Open Ended

Explain how pressure affects the solubility of gases compared to liquids and solids.

Multiple Choice

Which of the following is an example of a weak electrolyte?

• Glucose

• Acetic acid

• KBr

• NaCl

Multiple Choice

Which product will dissolve and which will form a precipitate when potassium sulfate reacts with calcium chloride?

• Potassium chloride will dissolve, calcium sulfate will precipitate

• Calcium chloride will dissolve, potassium sulfate will precipitate

• Both products will dissolve

• Both products will precipitate

Multiple Select

Which of the following ions are present in the complete ionic equation for the reaction between K2SO4 and CaCl2?

• K+

• SO4^2-

• Ca^2+

• Cl-

Open Ended

Explain the difference between a complete ionic equation and a net ionic equation in precipitation reactions.

Open Ended

Write the net ionic reaction for the precipitation reaction that occurs when sodium chloride is mixed with silver nitrate. What precipitate forms?

Open Ended

Explain why scientists use complete ionic equations when describing precipitation reactions.

Multiple Choice

Which of the following is the correct net ionic equation for the reaction between potassium sulfate (K2SO4) and calcium chloride (CaCl2)?

• SO4^2- (aq) + Ca^2+ (aq) -> CaSO4 (s)

• K2SO4 (aq) + CaCl2 (aq) -> 2 KCl (aq) + CaSO4 (s)

• 2 K^+ (aq) + SO4^2- (aq) + Ca^2+ (aq) + 2 Cl^- (aq) -> 2 K^+ (aq) + 2 Cl^- (aq) + CaSO4 (s)

• Ag^+ (aq) + Cl^- (aq) -> AgCl (s)

Multiple Choice

When a solute dissolves in water, what happens to the solute particles?

• They remain unchanged and settle at the bottom.

• They are surrounded by solvent molecules forming hydration shells.

• They evaporate into the air.

• They combine to form larger particles.

Open Ended

Reflecting on today's lesson about solubility, what is one concept you found most interesting or would like to learn more about?