Chapter 7: Reactions in Aqueous Solution

A collection of flashcards covering key terms and definitions related to reactions in aqueous solutions, including concepts of solutions, electrolytes, precipitation reactions, acid-base reactions, and redox reactions.

Solution

Any homogeneous mixture that is physically and chemically the same throughout the entire system.

Solvent

The component of a solution present in the largest amount, usually water in aqueous solutions.

Solute

The substance that is dissolved in the solvent, usually present in smaller amounts.

Electrolyte

Any aqueous solution that can conduct electricity.

Strong Electrolyte

A substance that completely dissociates into its constituent ions when dissolved in water.

Weak Electrolyte

Substances that dissolve in water producing fewer ions, resulting in lower conductivity.

Non-electrolyte

Substances that dissolve in water to form neutral molecules and have no effect on electrical conductivity.

Precipitation Reaction

Occurs when two soluble aqueous ionic solutions react to form an insoluble ionic solid.

Double Replacement Reaction

A type of chemical reaction where the positive ions switch places between two compounds to form two new compounds.

Arrhenius Acid

A substance that dissolves in water to produce hydrogen ions (H+).

Arrhenius Base

A substance that dissolves in water to produce hydroxide ions (OH−).

Molarity (M)

A measure of concentration, defined as moles of solute per liter of solution.

Dilution

The process of reducing the concentration of a solution by adding more solvent.

Redox Reaction

A reaction involving the transfer of electrons between two reactants, where one is oxidized and the other reduced.

Oxidation State

A number assigned to an atom in a compound that reflects its loss or gain of electrons in relation to other atoms.

Titration

A laboratory technique where a solution of known concentration is added to a solution of unknown concentration until the reaction reaches completion.