Chapter 4 Lecture Flashcards: Chemical Reactions and Aqueous Solutions

Flashcards covering key terminology from Chapter 4, Lecture 1 on Chemical Reactions and Aqueous Solutions, including types of solutions, electrolytes, solubility, and acid-base definitions.

Solution

A homogeneous mixture of solute(s) and solvents.

Solute

The components of the mixture present in the smallest amount.

Solvent

The component of the mixture present in the largest amount.

Dilute solution

A solution with a small ratio of solute to solvent.

Concentrated solution

A solution with a large ratio of solute to solvent.

Aqueous solution

A solution where the solute is 'hydrated' (dissolved in water).

Unsaturated solution

Less solute is dissolved than possibly could be dissolved at a given temperature.

Saturated solution

The maximum amount of solute possible to dissolve at a given temperature is dissolved.

Supersaturated solution

More solute than is present in a saturated solution at a given temperature is dissolved.

Strong electrolytes

Substances that dissociate 100% to form ions in solution, leading to strong electrical conductivity.

Weak electrolytes

Substances that dissociate <5% to form ions in solution, leading to weak electrical conductivity.

Nonelectrolyte

A substance that does not form ions in solution and thus does not conduct electricity.

Precipitation Reaction

A chemical reaction that results in the formation of an insoluble ionic compound (a precipitate).

Solubility

The maximum amount of a solid that will dissolve in a given amount of water at a certain temperature.

Soluble ionic compound

A strong electrolyte where >1 g solid dissolves in 100 mL of water.

Insoluble ionic compound

A nonelectrolyte where <1 g solid dissolves in 100 mL of water.

Double Displacement Reaction

A reaction where ions change partners (partner swap), forming new product(s).

Complete molecular equation

A balanced chemical equation that shows all reactants and products in their unionized, molecular form.

Complete ionic equation

An equation showing all strong electrolytes as dissociated ions and non-electrolytes in their original molecular form.

Spectator ions

Ions that are present in both the reactant and product sides of a complete ionic equation and do not participate in the reaction.

Net ionic equation

An equation that shows only the species directly involved in the chemical reaction, after spectator ions have been removed.

Arrhenius acid

Any substance that produces H+ when dissolved in water.

Arrhenius base

Any substance that produces OH- when dissolved in water.

Proton (H+)

A term used interchangeably with hydrogen ion (H+(aq)) or hydronium ion (H3O+) in aqueous solution.

Hydronium ion (H3O+)

The hydrated form of a hydrogen ion (H+) in aqueous solution, formed by H+(aq) + H2O(l).

Strong acids

Strong electrolytes that dissociate 100% to form ions in water.

Weak acids

Weak electrolytes that dissociate ~5% to form ions in water.

Monoprotic acid

An acid that produces 1 H+ (or H+(aq)) per acid molecule.

Diprotic acid

An acid that produces 2 H+ (or H+(aq)) per acid molecule.

Triprotic acid

An acid that produces 3 H+ (or H+(aq)) per acid molecule.

Strong bases

Strong electrolytes, typically metal hydroxides, that produce -OH(aq) in aqueous solutions.

Weak bases

Bases (often containing nitrogen) that react with water to accept H+ and form a cation and -OH, but do not dissociate 100%.

Acid-Base Reaction

A double-displacement reaction involving an acid and a base.