Mixtures and Solutions Vocabulary

This set of vocabulary flashcards covers key terms and definitions for mixtures, solubility, concentration units, and colligative properties as discussed in the lecture.

Heterogeneous mixture

Mixture with an uneven distribution throughout

Suspension

Heterogeneous mixture with particles large enough to settle out unless stirred

Colloid

Heterogeneous mixture that appears homogeneous and shows the Tyndall effect

Tyndall effect

Scattering of light by colloidal particles

Homogeneous mixture

Mixture with an even distribution throughout

Solution

Homogeneous mixture of two or more substances

Solute

Substance being dissolved

Solvent

Substance doing the dissolving

Immiscible

Liquids that do not dissolve in each other

Miscible

Liquids that dissolve freely in one another

Solubility

Measure of how well one substance dissolves in another

Soluble

Capable of being dissolved

Hydrates

Ionic substances that form crystals with water molecules

Electrolyte

Substance that forms a solution that conducts electricity

Strong electrolyte

Solution conducts electricity well because most particles form ions

Weak electrolyte

Solution conducts electricity poorly because few particles form ions

Nonelectrolyte

Substance that dissolves without conducting electricity

Solubility curve

Graph showing how much solute dissolves at different temperatures

Henry's Law

Gas solubility in a liquid increases as pressure increases

Dissolution

Process where solute dissolves and becomes surrounded by solvent

Dissociation

Separation of ions from an ionic compound as it dissolves

Saturated solution

Contains the maximum amount of dissolved solute

Unsaturated solution

Contains less than the maximum amount of dissolved solute

Supersaturated solution

Contains more dissolved solute than normally possible

Concentration

Amount of solute in a given amount of solvent or solution

Molarity

Moles of solute per liter of solution

Molality

Moles of solute per kilogram of solvent

Colligative properties

Properties that depend on the number of solute particles

Nonvolatile solute

Substance with little tendency to become a gas

Vapor pressure

Pressure caused by gas molecules above a liquid

Osmosis

Movement of solvent through a semipermeable membrane

Osmotic pressure

Pressure needed to stop osmosis

Formula for Molarity

$$M = \frac{\text{moles of solute}}{\text{liters of solution}}$$

Formula for Molality

$$m = \frac{\text{moles of solute}}{\text{kilograms of solvent}}$$

Dilution Formula

$$M_1 V_1 = M_2 V_2$$

Like dissolves like

Polar dissolves polar, nonpolar dissolves nonpolar

Water as universal solvent

Water's polarity allows it to dissolve many substances

Factors affecting solubility

Surface area, stirring, temperature, and pressure for gases

Freezing-point depression

Adding solute lowers freezing point

Boiling-point elevation

Adding solute raises boiling point