General Chemistry 003 - Chapter 4: Reactions in Aqueous Solution

Vocabulary flashcards covering fundamental aqueous solution chemistry concepts including concentration units, electrolyte classification, acid-base theories, precipitation, and redox reaction fundamentals.

Solvent

The substance present in the greatest amount in a solution.

Solute

The substance or substances present in a lesser amount in a solution.

Tincture

A solution that uses alcohol as its solvent.

Amalgam

An alloy in which one of the constituent metals is mercury ($Hg$).

Dissociation

The dissolving and separation of ionic compounds into ions, where any polyatomic group remains together.

Ionization

The dissolving process of a compound that generates new charged species, most commonly occurring with acids.

Strong Electrolyte

A material that completely dissociates into ions in aqueous solution and conducts electricity well.

Weak Electrolyte

A material that partially dissociates into ions in aqueous solution and conducts electricity moderately.

Non-Electrolyte

A material that dissolves into solution as molecules but does not dissociate into ions at all.

Precipitate

An insoluble solid compound formed when two soluble aqueous solutions react.

Spectator Ions

Ions present in an ionic reaction mixture that do not participate directly in the reaction and remain unchanged in solution.

Molarity ($M$)

A measure of concentration defined as $\text{Molarity } (M) = \frac{\text{Solute (mols)}}{\text{Total Volume (L)}}$. Its value changes with temperature.

Molality ($m$)

A measure of concentration defined as $\text{Molality } (m) = \frac{\text{Solute (mols)}}{\text{Mass Solvent (kg)}}$. Its value does not change with temperature.

Saturation

The point at which no more solute will dissolve in a solvent at a given condition, defining the solubility limit.

Arrhenius Acid

A substance that increases the concentration of hydrogen ions ($H^+$) in aqueous solution.

Arrhenius Base

A substance that increases the concentration of hydroxide ions ($OH^-$) in aqueous solution.

Brønsted-Lowry Acid

A substance that acts as an $H^+$ ion (proton) donor.

Brønsted-Lowry Base

A substance that acts as an $H^+$ ion (proton) acceptor.

Lewis Acid

A substance that acts as an electron pair acceptor.

Lewis Base

A substance that acts as an electron pair donor.

pH Scale

A logarithmic measurement of hydronium ion concentration, expressed as $pH = -\text{log}([H_3O^+])$, typically spanning from $0$ to $14$.

Superacids

Acids that are stronger than $100\,\%\,H_2SO_4$, characterized by a Hammett acidity ($H_0$) less than $-12.7$.

Equivalence Point

The point in a titration reaction where the concentration or amount of added titrant equals the amount of solute being analyzed ($[\text{Solute A}] = [\text{Solute B}]$).

Oxidation

A reaction process involving the loss of electrons by a chemical species.

Reduction

A reaction process involving the gain of electrons by a chemical species.

Activity Series

A series ranking metals according to their ease of oxidation, used to predict whether a redox displacement reaction will occur.