Lecture 17: Net Ionic Equations, Acid-Base Reactions, Titrations, Gaseous Reactions

These flashcards cover important vocabulary related to net ionic equations, acid-base reactions, titrations, and gas-evolution reactions.

Net Ionic Equation

An equation that shows only the particles that participate in the reaction, excluding spectator ions.

Spectator Ions

Ions that do not participate in a chemical reaction and are not included in the net ionic equation.

Acid (Arrhenius Definition)

A substance that produces protons (H+) in water.

Base (Arrhenius Definition)

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

Neutralization Reaction

An exchange reaction between an acid and a base, producing water and a salt.

Titration

A procedure used to determine the molarity of a solution, typically involving the addition of a standard solution to an analyte until the equivalence point is reached.

Standard Solution

A solution with an accurately known concentration used in titrations.

Analyte

The solution whose concentration is unknown in a titration.

Equivalence Point

The point in a titration at which the amount of added standard solution is equivalent to the amount of analyte present.

Strong Acid

An acid that is fully ionized or dissociated in aqueous solution, behaving as a strong electrolyte.

Weak Acid

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

Gas-Evolution Reaction

A chemical reaction that produces a gas as one of its products.

Molarity (M)

The concentration of a solution expressed as moles of solute per liter of solution.

Complete Ionic Equation

An equation that shows all the soluble ionic substances as ions in an aqueous solution.

Hydronium Ion (H3O+)

The ion formed when a proton (H+) is added to a water molecule.