Reactions in Aqueous Solution - Vocabulary Flashcards

Vocabulary flashcards covering key terms, definitions, and concepts from Chapter 4 (Reactions in Aqueous Solution) including electrolytes, precipitation, acid-base neutralization, redox reactions, molarity, and titrations.

Solution

A homogeneous mixture of two or more pure substances.

Solvent

The component of a solution that is present in the greatest abundance.

Solute

Any substance dissolved in a solvent within a solution.

Aqueous Solution

A solution in which water serves as the solvent.

Solvation

The process by which solute particles are surrounded by solvent molecules as a substance dissolves.

Dissociation

The separation of an ionic compound into individual ions surrounded by water molecules upon dissolving.

Electrolyte

A substance that dissociates into ions when dissolved in water, producing a solution that conducts electricity.

Strong Electrolyte

A solute that dissociates completely into ions when dissolved in water, resulting in a strong conductor of electricity.

Weak Electrolyte

A solute that only partially dissociates into ions in aqueous solution.

Nonelectrolyte

A substance that dissolves in water without forming ions, resulting in a solution that does not conduct electricity.

Chemical Equilibrium

A state in a chemical reaction where the forward and backward reactions occur simultaneously, indicated in chemical equations by a double arrow $\rightleftharpoons$.

Precipitation Reaction

A reaction occurring when solutions of soluble salts are mixed to produce an insoluble salt.

Precipitate

An insoluble solid produced during a precipitation reaction in aqueous solution.

Metathesis Reaction

A reaction, also known as an exchange reaction, in which the cations and anions in the reactant compounds transpose or swap partners ($AX + BY \rightarrow AY + BX$).

Molecular Equation

A chemical equation that lists reactants and products using complete chemical formulas without indicating their ionic state in solution.

Complete Ionic Equation

An equation showing all soluble strong electrolytes dissociated into their individual ions as they exist in solution.

Net Ionic Equation

A chemical equation formed by removing spectator ions from a complete ionic equation, leaving only the species directly involved in the reaction.

Spectator Ions

Ions present in a reaction mixture that do not participate in the chemical reaction and remain unchanged on both sides of the equation.

Acid

A substance that ionizes in aqueous solution to form hydrogen ions ($H^+$), acting as a proton donor.

Base

A substance that reacts with or accepts $H^+$ ions and increases the concentration of hydroxide ions ($OH^-$) when dissolved in water.

Strong Acid

An acid that completely dissociates into ions in aqueous solution.

Strong Base

A base that completely dissociates into metal cations and hydroxide anions ($OH^-$) in water.

Strong Acids and Bases Reference Table

A summary listing common strong acids ($HCl$, $HBr$, $HI$, $HClO_3$, $HClO_4$, $HNO_3$, $H_2SO_4$) and strong bases (Group 1A hydroxides and heavy Group 2A hydroxides).

Neutralization Reaction

A reaction between an acid and a base, typically producing water and a salt.

Salt

An ionic compound formed from the cation of a base and the anion of an acid during a neutralization reaction.

Common Antacids Table

A table detailing commercial antacids and their acid-neutralizing active ingredients, such as $NaHCO_3$, $Al(OH)_3$, $Mg(OH)_2$, and $CaCO_3$.

Oxidation

The loss of electrons by a substance during a chemical reaction.

Reduction

The gain of electrons by a substance during a chemical reaction.

Oxidation-Reduction Reaction (Redox Reaction)

A reaction involving the transfer of electrons between reacting species, where one species is oxidized and another is reduced.

Oxidation Number

An assigned positive or negative charge value given to an atom to track electron distribution in a neutral compound or polyatomic entity.

Displacement Reaction

A redox reaction in which an ion in solution oxidizes an element, leading to the displacement of an element from solution.

Activity Series

A list of metals organized by ease of oxidation, used to predict whether a displacement reaction will occur in aqueous solution.

Concentration

The quantity of solute present in a specified amount of solvent or total solution.

Molarity ($M$)

A measure of concentration defined as the number of moles of solute divided by the volume of solution in liters ($M = \frac{\text{moles of solute}}{\text{volume of solution in liters}}$).

Dilution

The process of reducing solution concentration by adding solvent, described by the formula $M_c V_c = M_d V_d$.

Titration

An analytical technique used to calculate the unknown concentration of a solute in a solution by reacting it with a solution of known concentration.

Standard Solution

A reagent solution of accurately known concentration used in a titration.

Equivalence Point

The point in a titration where the added amount of standard reagent is stoichiometrically equal to the amount of analyte.

End Point

The observed point in a titration, usually marked by an indicator color change, signaling that the reaction is complete.