Introductory Chemistry II - Acids and Bases Lecture 1

Vocabulary flashcards reviewing fundamental acid-base concepts, Arrhenius theory, strong and weak electrolytes, and hydronium ion formation from Lecture 1.

Acid

A chemical substance whose aqueous solution is characterized by a sour taste, the ability to turn blue litmus red, the ability to react with bases and certain metals to form salts, and a pH smaller than 7.

Base

A chemical substance whose aqueous solution is characterized by a bitter taste, a slippery feel, the ability to turn red litmus paper blue, the ability to react with acids to form salts, and a pH greater than 7.

Arrhenius Acid

A substance that ionizes in water to give $H^+$ ions (increasing the concentration of hydronium ion, $H_3O^+$) and anions.

Arrhenius Base

A substance that ionizes in water to give hydroxide ions ($OH^-$) and cations.

Hydronium Ion

The species $H_3O^+$ formed in aqueous solution when a hydrogen ion ($H^+$) chemically bonds to a water molecule.

Strong Acid (Arrhenius)

An acid that ionizes completely (100%) in aqueous solution to yield $H_3O^+_{(aq)}$ and an anion, with six common examples including $HCl$, $HBr$, $HI$, $HNO_3$, $HClO_4$, and $H_2SO_4$.

Strong Base (Arrhenius)

A base that dissociates completely (100%) in aqueous solution to yield $OH^-_{(aq)}$ and a cation, with six common examples including $NaOH$, $LiOH$, $KOH$, $Ca(OH)_2$, $Sr(OH)_2$, and $Ba(OH)_2$.

Weak Acid and Base

Acids and bases that do not completely ionize in water and exist in a reversible equilibrium with their corresponding ions.

Arrhenius Acid-Base Reaction

A neutralization reaction involving the reaction of an Arrhenius acid and an Arrhenius base that produces water ($H_2O_{(l)}$) and a salt.

Limitations of the Arrhenius Concept

The restrictions that the model applies only to aqueous solutions involving $H^+$ and $OH^-$ ions, and cannot account for basic behavior in substances lacking $OH$ groups (such as $NH_3$) or reactions in non-aqueous solvents.