General Chemistry 001C Lecture 13 Review

A set of vocabulary flashcards covering key concepts from General Chemistry Lecture on Acid-Base Equilibria.

Polyprotic Acids

Acids that can donate more than one proton (H+). Examples include H2CO3 and H2SO4.

Diprotic Acids

Acids that can donate two protons (H+), with Ka1 being greater than Ka2.

pH

A measure of the acidity or basicity of a solution; defined as the negative logarithm of the hydronium ion concentration.

Ka

The acid dissociation constant; a measure of the strength of an acid in solution.

Conjugate Base

The species that remains after an acid donates a proton.

Hydrolysis

The reaction of a substance with water to form ions.

Salts

Ionic compounds made up of cations and anions, formed from the neutralization of an acid and a base.

Equilibrium Expression

An equation that relates the concentrations of reactants and products at equilibrium.

Hydronium Ion (H3O+)

The ion formed when an acid donates a proton to water.

Weak Acid

An acid that partially ionizes in solution, resulting in a low concentration of H3O+.

Strong Acid

An acid that completely ionizes in solution, resulting in a high concentration of H3O+.

Bicarbonate Ion (HCO3−)

A polyatomic ion that acts as a weak base and can also donate protons.

Conjugate Acid

The species formed when a base accepts a proton.

Sulfate Ion (SO42−)

A polyatomic ion with the formula SO4, which can act as a conjugate base.

Ka1, Ka2

The dissociation constants of the first and second H+ ions removed in polyprotic acids.

Triprotic Acids

Acids that can donate three protons; they have three dissociation steps.

Neutralization Reaction

A reaction between an acid and a base that produces a salt and water.

Cation

A positively charged ion.

Anion

A negatively charged ion.

Dihydrogen Phosphate Ion (H2PO4−)

The conjugate base of phosphoric acid (H3PO4) that can donate a proton.

Hydrogensulfate Ion (HSO4−)

A polyatomic ion that can act as both an acid and a base.