chem

Arrhenius Model

Acids produce H⁺ ions and bases produce OH⁻ ions in aqueous solution.

Brønsted-Lowry Model

Acids are proton (H⁺) donors, and bases are proton acceptors.

Conjugate Acid

Formed when a base gains a proton (H⁺).

Conjugate Base

Formed when an acid loses a proton (H⁺).

Conjugate Acid/Base Pair

Two substances that differ by one proton (e.g., NH₃/NH₄⁺).

Monoprotic

An acid that donates one proton per molecule (e.g., HCl).

Diprotic

An acid that donates two protons per molecule (e.g., H₂SO₄).

Triprotic

An acid that donates three protons per molecule (e.g., H₃PO₄).

Weak Acid

An acid that only partially ionizes in solution.

Weak Base

A base that only partially accepts protons in solution.

Neutral Solution

A solution with equal concentrations of H₃O⁺ and OH⁻; pH = 7.

Hydronium Ion (H₃O⁺)

A water molecule with an extra proton (H⁺); the form of H⁺ in water.

Neutralization Reaction

Reaction of an acid and a base to form water and a salt.

Self-Ionization of Water

2 H₂O ⇌ H₃O⁺ + OH⁻

Ion Product Constant for Water (K₁)

K₁ = [H₃O⁺][OH⁻] = 1.0 × 10⁻¹⁴ at 25°C.

Titration

Lab method to find the unknown concentration of a solution using a solution of known concentration.

Equivalence Point

The point in a titration where moles of acid = moles of base.

Titration Curve

Graph of pH vs. volume of titrant; shows how pH changes during titration.