Solutions and Their Properties

Comprehensive vocabulary flashcards covering the definitions and concepts of solutions, mixtures, solubility, and concentration methods based on the lecture notes.

Solution

A homogeneous mixture of 2 or more substances in a single phase where parts cannot be distinguished.

Solute

The substance that is being dissolved in a solution (e.g., salt).

Solvent

The dissolving medium in a solution (e.g., water).

Aqueous solution

A solution in which water is the solvent; water is known as the universal solvent.

Alloy

A solid solution, such as Brass ($Cu + Zn$).

Suspension

A mixture that appears uniform while being stirred but separates into different phases when agitation ceases.

Colloid

A heterogeneous mixture containing intermediate size particles evenly distributed through a dispersion medium.

Brownian Motion

The jerky, erratic movement of dispersed particles that prevents colloids from settling out.

Tyndall effect

The scattering of light by dispersed particles.

Soluble

A term describing a substance that dissolves in another substance, such as sugar in water.

Insoluble

A term describing a substance that does not dissolve in another substance, such as sand in water.

Miscible

Two liquids that are soluble in each other, such as alcohol and water.

Immiscible

Two liquids that are insoluble in each other and form layers, such as oil and water.

Solvation

The process where solvent particles surround solute particles to form a solution.

Hydration

Solvation that specifically uses water as the solvent.

Exothermic

A process that releases heat and causes the solution to get warm, such as mixing $NaOH$ and water.

Endothermic

A process that absorbs heat and causes the solution to get cool, such as mixing Barium Hydroxide and Ammonium Chloride.

Solubility

The maximum amount of solute that will dissolve in a given amount of solvent at a certain temperature.

Saturated Solution

A solution containing the maximum amount of dissolved solute for a given amount of solvent at a specific temperature and pressure.

Unsaturated Solution

A solution containing less than the maximum amount of solute, meaning more solute can still be dissolved.

Supersaturated Solution

An unstable solution containing more dissolved solute than a saturated solution at the same temperature; it may recrystallize if disturbed.

Henry's Law

A law relating the solubility of a gas to the pressure above the liquid.

Colligative Properties

Physical properties of solutions affected by the number, but not the identity, of dissolved solute particles, including Vapor Pressure Lowering, Boiling Point Elevation, Freezing Point Depression, and Osmotic Pressure.

Electrolytes

Substances that form ions in solution and conduct electricity, having a greater effect on colligative properties because they produce more particles.

Nonelectrolytes

Covalent substances that do not ionize or conduct electricity in solution, such as glucose ($C_6H_{12}O_6$).

Concentrated

A solution that contains a large amount of solute.

Dilute

A solution that contains a small amount of solute.

Molarity ($M$)

The number of moles of solute dissolved per liter of solution, calculated as $\text{Molarity (M)} = \frac{\text{moles solute}}{\text{liters solution}}$.

Molality ($m$)

The number of moles of solute dissolved in each kilogram of solvent, calculated as $m = \frac{\text{moles of solute}}{\text{kg of solvent}}$; it is independent of temperature.

Mole Fraction ($X$)

The ratio of the number of moles of one component to the total number of moles in the solution, calculated as $X = \frac{\text{moles of component}}{\text{total moles of sol'n}}$.