Solutions, Solubility, and Polarity

These flashcards cover key vocabulary related to solutions, solubility, and polarity, specifically designed to aid in understanding and recalling important concepts for the exam.

Mixture

A combination of two or more substances where each retains its own properties.

Solvent

The component of a solution that is present in the greatest amount, typically a liquid that dissolves a solute.

Solute

The substance that is dissolved in a solution.

Electrolyte

A substance that dissociates into ions in solution and can conduct electricity.

Solubility

The maximum quantity of a solute that can dissolve in a given amount of solvent at a specific temperature.

Saturated Solution

A solution that contains the maximum amount of solute that can dissolve under specified conditions.

Unsaturated Solution

A solution that can still dissolve more solute at a given temperature and pressure.

Supersaturated Solution

A solution that contains more solute than is normally possible at a given temperature.

Miscible

Describes two liquids that are soluble in each other.

Immiscible

Describes two liquids that do not mix or form a homogeneous mixture.

Molarity (M)

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

Molality (m)

A measure of concentration, defined as moles of solute per kilogram of solvent.

Precipitate

An insoluble solid that forms when two aqueous solutions react.

Metathesis Reactions

Chemical reactions involving the exchange of partners between compounds, also known as double replacement reactions.

Net Ionic Equation

An equation that shows only the particles that participate in the reaction and omits spectator ions.

Titration

A laboratory method used to determine the concentration of a solution by reacting it with a solution of known concentration.

Oxidation Reduction Reactions (Redox)

Reactions where electrons are transferred between substances, changing their oxidation states.

Polar Molecule

A molecule that has a partial positive charge on one end and a partial negative charge on the other due to differences in electronegativity.