Lesson 2 Notes: Acids, Bases, Electrolytes, and Net Ionic Equations

Vocabulary flashcards covering acids, bases, electrolytes, and net ionic equations from Lesson 2 notes.

Ammonia (NH3)

A weak base that partially ionizes in water to form NH4+ and OH−; not a strong electrolyte.

Strong acid

An acid that dissociates completely in water (e.g., HCl, HBr, HI, H2SO4, HNO3, HClO4).

Strong base

A base that dissociates completely in water to give OH−; examples include Group 1 hydroxides and Group 2 hydroxides: NaOH, KOH, Ca(OH)2, Sr(OH)2, Ba(OH)2.

Weak electrolyte

A substance that partially ionizes in water and conducts electricity weakly.

Nonelectrolyte

A substance that does not ionize in water and does not conduct electricity.

Oxyacid

An acid containing hydrogen, oxygen, and another element; often named with -ic or -ous endings depending on the oxidation state.

Spectator ion

An ion that appears on both sides of a reaction and does not participate in the chemical change; removed in the net ionic equation.

Precipitation reaction

A double displacement reaction that forms an insoluble solid (precipitate).

Precipitate

The insoluble solid formed in a precipitation reaction.

Net ionic equation

An ionic equation that shows only the species that undergo a chemical change; spectator ions are omitted.

Hydro- prefix

Prefix used for naming binary acids; often yields the acid name like hydrochloric acid (HCl) from HCl.

ate to ic rule

In oxyacids, the -ate anion becomes -ic in the acid name (e.g., sulfate → sulfuric acid).

ite to ous rule

In oxyacids, the -ite anion becomes -ous in the acid name (e.g., sulfite → sulfurous acid).

Nitrous acid

HNO2; a weak acid derived from nitrite (NO2−).

Precipitation example

Ba(NO3)2 + KF → BaF2(s) + 2KNO3 demonstrates formation of an insoluble precipitate (BaF2).