Chapter 12: Solutions and Types of Mixtures

Vocabulary practice flashcards covering types of mixtures, solution processes, and concentration measures from Chapter 12 chemistry lecture slides.

Heterogeneous Mixture

A mixture in which the parts are noticeably different from one another, such as sand, salsa, or chocolate chip cookie dough.

Homogeneous Mixture

A mixture in which the substances are so evenly distributed that it is difficult to distinguish one substance from another.

Solution

A homogeneous mixture of two or more substances in a single phase.

Solute

The substance that is dissolved in a solution.

Solvent

The dissolving medium in a solution.

Suspension

A heterogeneous mixture containing particles over $1000\,nm$ in diameter that will settle out upon standing unless constantly stirred or agitated.

Colloid

A mixture containing intermediate-sized particles between $1\,nm$ and $1000\,nm$ that remain dispersed and will not settle out upon standing.

Emulsion

A heterogeneous system consisting of at least one immiscible liquid phase intimately dispersed throughout a second phase in the form of droplets or globules.

Brownian Motion

The movement of colloidal particles in an irregular and complicated zigzag pathway caused by random collisions with molecules of the dispersion medium.

Tyndall Effect

The scattering of light by dispersed colloidal particles, producing a visible path for a beam of light passing through a colloidal mixture.

Electrolyte

A substance that dissolves in water to give a solution that conducts electric current due to mobile separated positive and negative ions.

Nonelectrolyte

A substance that dissolves in water to give a solution that does not conduct electric current because its neutral solute molecules do not form mobile charged particles.

Immiscible

Describes liquids that do not dissolve in each other, such as oil and water.

Miscible

Describes liquids that dissolve freely in one another in any proportion to form a solution.

Solvation

The process in which solvent particles surround solute particles to form a solution.

Hydration

The solution process in which water is the solvent and polar water molecules attract and surround solute ions or molecules.

Solubility

The amount of a solute required to form a saturated solution with a specific amount of solvent at a specified temperature and pressure.

Saturated Solution

A solution that contains the maximum amount of dissolved solute possible for a given quantity of solvent at constant temperature and pressure.

Unsaturated Solution

A solution that contains less dissolved solute than a saturated solution under the same conditions.

Supersaturated Solution

A solution that contains more dissolved solute than a saturated solution contains under the same conditions.

Solution Equilibrium

The physical state in which the opposing processes of dissolution and crystallization of a solute occur at equal rates.

Henry's Law

States that at a given temperature, the solubility ($S$) of a gas in a liquid is directly proportional to the pressure ($P$) of the gas above the liquid ($\frac{S_1}{P_1} = \frac{S_2}{P_2}$).

Enthalpy of Solution

The net amount of energy absorbed or released as heat by a solution when a specific amount of solute dissolves in a solvent.

Molarity ($M$)

A unit of concentration defined as the number of moles of solute dissolved in one liter of solution ($\text{Molarity} = \frac{\text{moles of solute}}{\text{liters of solution}}$).

Molality ($m$)

A unit of concentration defined as the number of moles of solute dissolved per kilogram of solvent ($\text{Molality} = \frac{\text{moles of solute}}{\text{kilograms of solvent}}$).