AP Chemistry 3.10 Solubility Questions

Practice AP Chemistry 3.10 questions on predicting solubility from matching intermolecular interactions, polarity, hydrogen bonding, and ionic interactions.

Exam points

Use molecular structure, polarity, and intermolecular forces to predict solubility and acid–base behavior in water.
Interpret particle interactions and equilibrium data to explain dissolution, precipitation, and composition.

Covered syllabus points

3.10.A—Explain the relationship between the solubility of ionic and molecular compounds in aqueous and nonaqueous…

[Maximum number: 2]

Answer the following questions about the compounds $\mathrm{NH}_{2} \mathrm{Cl}$ and $\mathrm{NCl}_{3}$ . The Lewis electron-dot diagrams of the two compounds are shown.

$\mathrm{NH}_{2} \mathrm{Cl}$ is highly soluble in water, whereas $\mathrm{NCl}_{3}$ is nearly insoluble. Explain this observation in terms of the types and relative strengths of the intermolecular forces between each of the solutes and water.

For the correct identification of intermolecular forces between each substance and water: 1 point Accept one of the following:

- Both $\mathrm{NH}_{2} \mathrm{Cl}$ and $\mathrm{NCl}_{3}$ can participate in hydrogen bonding with water.

- Both $\mathrm{NH}_{2} \mathrm{Cl}$ and $\mathrm{NCl}_{3}$ have dipole-dipole attractions to water.

For a correct explanation: 1 point The intermolecular forces between $\mathrm{NH}_{2} \mathrm{Cl}$ molecules and water are stronger than those between $\mathrm{NCl}_{3}$ molecules and water, which leads to the greater solubility of $\mathrm{NH}_{2} \mathrm{Cl}$ in water.

Total for part (b) 2 points

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Covered syllabus points

Question 1