Lecture 14: Aqueous Reactions - General Ideas and Definitions

These flashcards summarize the key concepts and vocabulary from Lecture 14 on aqueous reactions, including definitions related to solvation, electrolytes, types of chemical reactions, and solubility rules.

Solution

A homogeneous mixture, which need not be liquid.

Solvent

The dissolving medium; the component present in greatest amount.

Solute

The substance that is dissolved; component(s) present in smaller amounts.

Hydration

The process of a solute interacting with water molecules when a substance is soluble in water.

Strong Electrolyte

A solute that completely dissociates into ions in solution, allowing it to conduct electricity well.

Weak Electrolyte

A solute that only partially dissociates into ions in solution, resulting in limited conductivity.

Nonelectrolyte

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

Precipitation Reaction

A type of chemical reaction where two soluble salts combine to form an insoluble salt.

Acid-Base Reaction

A reaction involving the transfer of protons (H+) between reactants, forming water and a salt.

Covalent Compound

A compound formed by the sharing of electrons between atoms; generally, if soluble in water, acts as a nonelectrolyte.

Solubility Rule

Guidelines used to predict whether an ionic compound will dissolve in water.

Double Displacement Reaction

A reaction where the cations and anions of two different compounds exchange places, often resulting in precipitation.

Ionic Compound

A compound formed from the electrostatic attraction of oppositely charged ions.