Solutions and Chemical Reactions Bold Face Terms

Polar molecule

A molecule with an uneven distribution of electrical charge, creating positive and negative ends (poles).

Hydration

The process in which water molecules surround and interact with dissolved ions or molecules.

Solubility

The maximum amount of a substance that can dissolve in a given amount of solvent at a specified temperature.

Solute

The substance that is dissolved in a solution.

Solvent

The substance that dissolves the solute and is usually present in the larger amount.

Electrical conductivity

The ability of a substance or solution to conduct electric current.

Strong electrolytes

Substances that completely dissociate into ions in water and conduct electricity well.

Weak electrolytes

Substances that partially dissociate into ions in water and conduct electricity poorly.

Nonelectrolytes

Substances that do not produce ions in water and therefore do not conduct electricity.

Strong acids

Acids that ionize completely in water, producing a high concentration of H⁺ ions.

Strong bases

Bases that dissociate completely in water, producing a high concentration of OH⁻ ions.

Weak acid

An acid that only partially ionizes in water.

Weak base

A base that only partially ionizes in water.

Molarity (M)

The concentration of a solution expressed as moles of solute per liter of solution.

Molarity formula

M = moles of solute / liters of solution

Dilution

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

Precipitation reactions

Reactions in which two aqueous solutions react to form an insoluble solid called a precipitate.

Acid-base reactions

Reactions in which an acid reacts with a base, usually producing water and a salt.

Oxidation-reduction (redox) reactions

Reactions involving the transfer of electrons between substances, causing changes in oxidation states.

Precipitation reaction

A chemical reaction that produces an insoluble solid from two aqueous solutions.

Precipitate

The insoluble solid that forms and separates from a solution during a precipitation reaction.

Formula equation (molecular equation)

A chemical equation showing compounds as complete formulas without separating them into ions.

Complete ionic equation

A chemical equation showing all strong electrolytes as separate ions in solution.

Net ionic equation

A chemical equation showing only the ions and molecules directly involved in the reaction, excluding spectator ions.

Acid

A substance that donates H⁺ ions (protons) in solution.

Base

A substance that accepts H⁺ ions or produces OH⁻ ions in solution.

Volumetric analysis

A laboratory method used to determine the concentration of a solution by measuring the volume required to react with a known solution.

Titration

A technique in which a solution of known concentration is added to a solution of unknown concentration until the reaction is complete.

Equivalence (stoichiometric) point

The point in a titration where the acid and base have reacted in exactly the stoichiometric ratio required by the balanced equation.

Indicator

A substance that changes color near the equivalence point to signal the progress of a titration.

Endpoint

The point during a titration at which the indicator changes color, signaling that the titration should stop.