General Chemistry: Reactions in Aqueous Solutions

These flashcards cover key vocabulary terms related to the topic of reactions in aqueous solutions in general chemistry.

Solution

A homogenous mixture of two or more substances.

Solute

Substance present in the smaller amount in a solution.

Solvent

Substance present in the larger amount in a solution.

Electrolyte

A substance that, when dissolved in water, results in a solution that can conduct electricity.

Nonelectrolyte

A substance that, when dissolved, results in a solution that does not conduct electricity.

Strong Electrolyte

Substances that completely dissociate into ions in solution.

Weak Electrolyte

Substances that only partially dissociate into ions in solution.

Hydration

The process in which an ion is surrounded by water molecules arranged in a specific manner.

Precipitate

An insoluble solid that separates from solution.

Net Ionic Equation

An equation that shows only the species that actually change during the reaction, excluding spectator ions.

Acid

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

Base

A substance that produces hydroxide ions (OH-) in solution.

Arrhenius Acid

A substance that produces H+ ions in water.

Arrhenius Base

A substance that produces OH- ions in water.

Brønsted Acid

A proton donor.

Brønsted Base

A proton acceptor.

Titration

A technique where a solution of known concentration is gradually added to a solution of unknown concentration to determine the latter's concentration.

Equivalence Point

The point in a titration at which the reaction is complete.

Oxidation State

The charge an atom would have in a molecule or ion if electrons were completely transferred.

Combination Reaction

A reaction where two or more substances combine to form a single product.

Displacement Reaction

A reaction where one element replaces another in a compound.

Activity Series

A list of metals arranged in order of decreasing activity.

Dissociation

The process in which ionic compounds separate into ions when dissolved in water.

Molarity

A way to express concentration; the number of moles of solute per liter of solution.

Dilution

The process of reducing the concentration of a solute in solution by mixing with a solvent.

Concentration

The amount of solute present in a given volume of solution.

Saturation Point

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

Soluble

A substance that can dissolve in a solvent.

Insoluble

A substance that cannot dissolve in a solvent.

Colloid

A mixture where tiny particles of one substance are evenly distributed throughout another substance.

Suspension

A mixture in which particles are dispersed throughout a liquid or gas but are large enough that they settle out over time.

pH Scale

A scale used to specify the acidity or basicity of an aqueous solution, ranging from 0 (acidic) to 14 (basic).

Buffer

A solution that resists changes in pH when small amounts of acid or base are added.

Salinity

The concentration of salt in water, usually expressed in parts per thousand (ppt).

Le Châtelier's Principle

If a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change

Dissociation

The process in which ionic compounds separate into ions when dissolved in water.

Molarity

A way to express concentration; the number of moles of solute per liter of solution.

Dilution

The process of reducing the concentration of a solute in solution by mixing with a solvent.

Activity Series

A list of metals arranged in order of decreasing activity.

Oxidation State

The charge an atom would have in a molecule or ion if electrons were completely transferred.

Combination Reaction

A reaction where two or more substances combine to form a single product.

Displacement Reaction

A reaction where one element replaces another in a compound.

Equivalence Point

The point in a titration at which the reaction is complete.

Titration

A technique where a solution of known concentration is gradually added to a solution of unknown concentration to determine the latter's concentration.

Brønsted Acid

A proton donor.

Brønsted Base

A proton acceptor.

Strong Electrolyte

Substances that completely dissociate into ions in solution.

Weak Electrolyte

Substances that only partially dissociate into ions in solution.

Acid

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

Base

A substance that produces hydroxide ions (OH-) in solution.

Arrhenius Acid

A substance that produces H+ ions in water.

Arrhenius Base

A substance that produces OH- ions in water.

Hydration

The process in which an ion is surrounded by water molecules arranged in a specific manner.

Precipitate

An insoluble solid that separates from solution.

Net Ionic Equation

An equation that shows only the species that actually change during the reaction, excluding spectator ions.