Solution Chemistry and Chemical Reactions in Water

30 vocabulary flashcards on key concepts in solution chemistry and chemical reactions in water.

Molarity

The amount of solute in moles divided by the volume of solution in liters.

Dilution

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

Hydronium Ion (H3O+)

The ion formed when a proton is donated to a water molecule.

Brønsted–Lowry Acid

Substances that donate protons (H+) in reactions.

Brønsted–Lowry Base

Substances that accept protons (H+) in reactions.

Neutralization Reaction

A reaction between an acid and a base to produce a salt and water.

Ionic Equation

An equation that shows all the ions in the reaction, distinguished by their state.

Net Ionic Equation

An equation that shows only the species that change during the reaction.

Strong Acid

An acid that completely dissociates in aqueous solution.

Weak Acid

An acid that only partially dissociates in aqueous solution.

Strong Base

A base that completely dissociates when dissolved in water.

Weak Base

A base that only partially ionizes in aqueous solution.

Amphiprotic

Substances that can act as either an acid or a base.

Titration

A technique to determine the concentration of a solute by reacting it with a standard solution.

End Point of a Titration

The point at which the indicator changes color, indicating the completion of the reaction.

Precipitation Reaction

A reaction in which soluble reactants form an insoluble product called a precipitate.

Oxidation Reaction

A reaction that increases the oxygen content of a substance or results in the loss of electrons.

Reduction Reaction

A reaction that decreases the oxygen content of a substance or results in the gain of electrons.

Oxidation Number

A measure of the number of electrons an atom has compared to when it is a free atom.

Redox Reaction

A reaction involving the transfer of electrons between species.

Half-Reaction Method

A technique for balancing redox reactions by separating oxidation and reduction processes.

Saturated Solution

A solution that contains the maximum concentration of solute at a given temperature.

Supersaturated Solution

A solution that contains more solute than the equilibrium solubility allows.

Electrolytes

Substances that dissociate into ions in solution and conduct electricity.

Reactants

Substances that undergo a chemical change in a reaction.

Products

Substances that are formed as a result of a chemical reaction.

Spectator Ions

Ions that do not participate in the actual reaction and are present in the solution.

Precipitate

An insoluble solid formed from a solution during a chemical reaction.

Molecular Equation

An equation that shows the complete chemical formulas of reactants and products.

Solubility Guidelines

Rules that determine whether a substance will dissolve in a particular solvent.

Electron Transfer

The movement of electrons from one atom or molecule to another during a chemical reaction.

Standard Solution

A solution with a known concentration used in titrations.

Analyte

The substance being analyzed or measured in a titration.

Equivalence Point

The point in a titration at which the amount of titrant added is stoichiometrically equivalent to the amount of substance being titrated.