Unit 8 Solutions Study Guide

Flashcards based on key concepts from the Solutions unit, including types of mixtures, solubility, and properties of solutions.

What is a heterogeneous mixture?

A mixture with an uneven distribution throughout.

What characterizes a suspension?

A heterogeneous mixture with large particles that settle out unless stirred.

Define colloid.

A heterogeneous mixture that appears homogeneous, with particles larger than those in a solution, identifiable by the Tyndall effect.

What is the Tyndall effect?

The scattering of light by colloidal particles dispersed in a transparent medium.

What is a homogeneous mixture?

A mixture with an even distribution throughout.

What is a solution?

A homogeneous mixture of 2 or more substances that are uniformly dispersed.

What is a solute?

The substance that is dissolved in a solution.

What is a solvent?

The substance that is doing the dissolving; the dissolving medium.

Differentiate between immiscible and miscible liquids.

Immiscible liquids do not dissolve in each other, while miscible liquids dissolve freely in one another.

What is solubility?

A measure of how well one substance dissolves in another.

What is a strong electrolyte?

Any compound whose aqueous solutions conduct electricity well due to presence of dissolved compound as ions.

Define weak electrolyte.

Any compound whose aqueous solutions conduct electricity poorly due to presence of a small amount of dissolved ions.

What is a nonelectrolyte?

A substance that dissolves in water creating a solution that cannot conduct electric current.

What does Henry’s Law state?

The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas.

What is the difference between dissolution and dissociation?

Dissolution is the process where the solute separates and is surrounded by solvent; dissociation is the separation of ions from an ionic compound.

How does temperature affect solubility?

For most solutes, higher temperatures increase solubility due to greater kinetic energy.

What is a saturated solution?

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

What factors affect the solubility of a substance?

Surface area of solute, agitation of the solution, heating the solvent, and pressure changes (for gases).

What are colligative properties?

Properties dependent on the concentration of solute particles but not on their identity.

How do colligative properties differ from non-colligative properties?

Colligative properties depend on the number of solute particles, while non-colligative properties depend on the identity of the substance.