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AP Chemistry Practice Quiz: Solubility

Written by AP Content Team, Verified for 2026 AP Exams, Last updated: May 2026

Test your understanding with short quizzes. This quiz has 7 questions to check your progress.

Question 1 of 7

Which statement best summarizes the general principle for predicting whether one substance will dissolve in another?

All Questions (7)

Which statement best summarizes the general principle for predicting whether one substance will dissolve in another?

A) Substances with similar molar masses tend to be soluble in one another.

B) Substances with similar intermolecular interactions tend to be soluble in one another.

C) Ionic compounds are only soluble in nonaqueous solvents.

D) Molecular compounds are only soluble in aqueous solvents.

Correct Answer: B

This is a direct restatement of the 'like dissolves like' principle provided in the content, which states that substances with similar intermolecular interactions tend to be miscible or soluble in one another.

A molecular compound that exhibits strong dipole-dipole interactions is most likely to be soluble in which type of solvent?

A) A nonpolar solvent with only London dispersion forces.

B) An aqueous solvent with strong hydrogen bonding.

C) A metallic solvent composed of a sea of electrons.

D) Any solvent, regardless of its intermolecular forces.

Correct Answer: B

According to the 'like dissolves like' principle, substances with similar intermolecular interactions are soluble in one another. A molecular compound with strong dipole-dipole interactions is polar. An aqueous solvent with hydrogen bonding is also highly polar. Therefore, the polar solute is most likely to dissolve in the polar solvent.

An ionic compound, such as potassium chloride (KCl), readily dissolves in water. This observation implies that the intermolecular interactions between the solute and solvent particles are:

A) Weaker than the interactions holding the ionic lattice together.

B) Similar to the interactions found in nonpolar, nonaqueous solvents.

C) Strong enough to overcome the forces within both the ionic compound and the solvent.

D) Primarily based on London dispersion forces.

Correct Answer: C

For an ionic compound to dissolve in an aqueous solvent like water, the new ion-dipole interactions formed between the ions and polar water molecules must be strong enough to overcome the ion-ion attractions in the crystal lattice and the hydrogen bonds between water molecules. This aligns with the principle that solubility is governed by the interplay of intermolecular interactions.

Which of the following solutes is expected to be most soluble in a nonaqueous solvent composed of nonpolar molecules?

A) An ionic salt with strong electrostatic attractions.

B) A polar molecular compound with hydrogen bonding capabilities.

C) A nonpolar molecular compound with only London dispersion forces.

D) A network covalent solid with strong covalent bonds.

Correct Answer: C

The principle of 'like dissolves like' dictates that nonpolar solutes dissolve best in nonpolar solvents. A nonpolar molecular compound has intermolecular interactions (London dispersion forces) that are similar to those of a nonpolar solvent, leading to high solubility. Ionic and polar compounds have very different interactions and would be largely insoluble.

A student observes that a particular molecular compound is highly soluble in water but nearly insoluble in hexane, a nonpolar solvent. What is the most reasonable conclusion about the intermolecular interactions of this compound?

A) The compound's particles interact primarily through weak London dispersion forces.

B) The compound is likely ionic, and its solubility is an exception to the rule.

C) The compound's particles are polar and form strong interactions with polar water molecules.

D) The compound has a very high molar mass, which prevents it from dissolving in hexane.

Correct Answer: C

Based on 'like dissolves like', high solubility in polar water and low solubility in nonpolar hexane indicates that the compound itself must be polar. Its polar intermolecular interactions are similar to those of water, facilitating dissolution, but dissimilar to the weak forces in hexane, preventing dissolution.

Which of the following pairs of substances is LEAST likely to be miscible?

A) A polar molecular compound and an aqueous solvent.

B) An ionic compound and an aqueous solvent.

C) A nonpolar molecular compound and a nonaqueous, nonpolar solvent.

D) An ionic compound and a nonaqueous, nonpolar solvent.

Correct Answer: D

Miscibility is governed by the 'like dissolves like' rule. An ionic compound consists of charged ions held by strong electrostatic forces. A nonaqueous, nonpolar solvent consists of neutral molecules with weak London dispersion forces. The intermolecular interactions are very dissimilar, making them least likely to be miscible.

The solubility of a substance is fundamentally a result of the competition between solute-solute, solvent-solvent, and solute-solvent interactions. For a molecular compound to dissolve readily in an aqueous solvent, which relationship between the particle interactions must be true?

A) The solute-solute interactions must be significantly stronger than all other interactions.

B) The solvent-solvent interactions must be negligible.

C) The solute-solvent interactions must be comparable in strength to the solute-solute and solvent-solvent interactions.

D) The solute must be nonpolar to minimize interactions with the polar solvent.

Correct Answer: C

Dissolution occurs when the energy required to break existing solute-solute and solvent-solvent interactions is compensated by the energy released from forming new solute-solvent interactions. This happens when the new interactions are of a similar type and comparable strength to the ones being broken, which is the essence of the 'like dissolves like' principle.