Chem 1211 Chapter 4: Aqueous Reactions and Solution Stoichiometry

Vocabulary flashcards covering core concepts of aqueous solutions, electrolyte behavior, reaction stoichiometry, precipitation, acid-base theories, titrations, and redox chemistry from Chapter 4.

Solution

A homogeneous mixture composed of two or more substances.

Solvent

The component in a solution that is present in the greatest amount.

Solute

The component or components in a solution present in lesser amount(s).

Soluble

Describes a substance that dissolves to a significant amount in a solvent.

Insoluble

Describes a substance that does not dissolve to a significant amount in a solvent.

Hydrated

Solute particles surrounded by water molecules during the dissolution process.

Solvated

Solute particles surrounded by solvent molecules during the dissolution process.

Concentration

The quantity of solute dissolved in a standard quantity of solution.

Concentrated Solution

A solution containing a relatively high concentration of solute relative to solvent.

Dilute Solution

A solution containing a relatively low concentration of solute relative to solvent.

Molarity ($M$)

The moles of solute dissolved in $1\text{ liter}$ of solution ($M = \frac{\text{mol solute}}{\text{L solution}}$).

Percent Concentration by Mass

A concentration unit calculated as $\frac{\text{g solute}}{\text{g solution}} \times 100$.

Dilution

The process of preparing a less concentrated solution from a stock solution using the relationship $M_1 \times V_1 = M_2 \times V_2$.

Electrolyte

A substance that dissolves in water to form an electrically conducting solution.

Nonelectrolyte

A substance that dissolves in water to form a solution that does not conduct electricity due to a complete lack of ionization.

Strong Electrolyte

A substance that is essentially completely ionized in solution, forming a high concentration of ions and exhibiting high electrical conductivity.

Weak Electrolyte

A substance that is only partially ionized in solution, forming a low concentration of ions and exhibiting low electrical conductivity.

Formula Equation

A chemical equation that gives the overall reaction stoichiometry but not necessarily the actual forms of the reactants and products in solution.

Complete Ionic Equation

An equation in which strong electrolytes are written as separate ions, representing each substance by its predominant form in the reaction mixture.

Net Ionic Equation

An ionic equation that shows only the chemical species that actually take part in the reaction, omitting spectator ions.

Spectator Ions

Ions that do not take part in a chemical reaction and appear unchanged on both sides of the equation; they serve to maintain charge balance.

Precipitation Reaction

A reaction in aqueous solution that results in the formation of an insoluble product, or precipitate.

Solubility

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

Metathesis Reaction

An exchange reaction that appears to involve the swapping of parts (ions) between two reacting compounds.

Brønsted-Lowry Acid

A substance that acts as a proton donor in an acid-base reaction.

Brønsted-Lowry Base

A substance that acts as a proton acceptor in an acid-base reaction.

Strong Acid

An acid that ionizes completely in aqueous solution and acts as a strong electrolyte (e.g., $HClO_4$, $H_2SO_4$, $HI$, $HBr$, $HCl$, $HNO_3$).

Strong Base

A base that is present in aqueous solution entirely as ions, one of which is $OH^{1-}$, acting as a strong electrolyte (e.g., $LiOH$, $NaOH$, $KOH$, $Ca(OH)_2$, $Sr(OH)_2$, $Ba(OH)_2$).

Weak Acid

An acid that only partially ionizes in aqueous solution, behaving as a weak electrolyte.

Weak Base

A base that only partially ionizes in aqueous solution, behaving as a weak electrolyte.

Neutralization Reaction

A reaction of an acid with a base that typically yields a salt and water.

Salt

An ionic compound produced from a neutralization reaction containing the cation from a base and the anion from an acid.

Monoprotic Acid

An acid capable of donating only one proton per molecule (e.g., $HCl$, $HNO_3$, $HC_2H_3O_2$).

Polyprotic Acid

An acid capable of donating more than one proton per molecule (e.g., $H_2S$, $H_2SO_4$, $H_3PO_4$).

Quantitative Analysis

The determination of the amount or concentration of a substance present in a sample.

Volumetric Analysis (Titration)

A quantitative method involving volume measurement by carrying out a controlled addition of one solution to another.

Gravimetric Analysis

A quantitative method based on mass measurement where the analyte is converted into an insoluble product that can be isolated and weighed.

Equivalence Point

The point in a titration where the reaction is just complete because exactly enough titrant has been added to react with all analyte present.

End Point

The point in a titration experiment where the addition of titrant is halted based on an observable signal.

Oxidation-Reduction (Redox) Reaction

A chemical reaction that involves the transfer of electrons between reacting species.

Oxidation

A process characterized by the gain of oxygen, loss of hydrogen, loss of electrons, or an increase in oxidation number.

Reduction

A process characterized by the loss of oxygen, gain of hydrogen, gain of electrons, or a decrease in oxidation number.

Oxidizing Agent

The electron acceptor species that oxidizes another substance while itself being reduced.

Reducing Agent

The electron donor species that reduces another substance while itself being oxidized.