Chemistry: Acids and Bases Overview

Study Notes

Acids and bases exhibit various physical and chemical properties.
The hydronium ion (H₃O⁺) forms when water reacts with an acid.
Acids and bases are classified using the Arrhenius, Brønsted-Lowry, and Lewis models.

Acid strength differs from concentration.
Strong acids completely ionize in solution, while weak acids only partially ionize.
Concentrated acids contain a high amount of solute per unit volume, diluted acids contain a low amount.
Monoprotic acids donate one proton, diprotic donate two, and polyprotic acids donate more than two protons

Titration is a technique for determining the concentration of an unknown solution.
A known concentration (titrant) is used to react with a known volume of unknown solution.
The equivalence point in a titration is the point where the moles of H⁺ from the acid equals the moles of OH⁻ from the base.
An abrupt change in pH occurs at the equivalence point.
The formula cbMaVa = caMbVb is important in titration calculations. Where cb = concentration of base, ca = concentration of acid, Ma = molarity of acid, Mb = molarity of base, Va = volume of acid, Vb = volume of base.

Indicators are used to mark the end point of a titration.
Different indicators change color at different pH values.
Water is a universal solvent for acids and bases and undergoes self-ionization. The reaction is H₂O(l) + H₂O(l) ⇌ H₃O⁺(aq) + OH⁻(aq).