Reactivity 3 / IB Chemistry / Reactivity 3.1 (Including HL)

Reactivity 3. What are the mechanisms of chemical change?

Reactivity 3.1—Proton transfer reactions
Reactivity 3.1.1—Brønsted–Lowry acid is a proton donor and a Brønsted–Lowry base is a proton acceptor.
Reactivity 3.1.2—A pair of species differing by a single proton is called a conjugate acid–base pair.
Reactivity 3.1.3—Some species can act as both Brønsted–Lowry acids and bases.
Reactivity 3.1.4—The pH scale can be used to describe the [H+] of a solution
Reactivity 3.1.5—The ion product constant of water, Kw, shows an inverse relationship between [H+] and [OH–]. Kw = [H+] [OH–]
Reactivity 3.1.6—Strong and weak acids and bases differ in the extent of ionization.
Reactivity 3.1.7—Acids react with bases in neutralization reactions.
Reactivity 3.1.8—pH curves for neutralization reactions involving strong acids and bases have characteristic shapes and features.

Reactivity 3.1.9—The pOH scale describes the [OH–] of a solution
Reactivity 3.1.10—The strengths of weak acids and bases are described by their Ka, Kb, pKa or pKb values.
Reactivity 3.1.11—For a conjugate acid–base pair, the relationship Ka × Kb = Kw can be derived from the expressions for Ka and Kb.
Reactivity 3.1.12—The pH of a salt solution depends on the relative strengths of the parent acid and base.
Reactivity 3.1.13—pH curves of different combinations of strong and weak monoprotic acids and bases have characteristic shapes and features.
Reactivity 3.1.14—Acid–base indicators are weak acids, where the components of the conjugate acid–base pair have different colours. The pH of the end point of an indicator, where it changes colour, approximately corresponds to its pKa value.
Reactivity 3.1.15—An appropriate indicator for a titration has an end point range that coincides with the pH at the equivalence point.
Reactivity 3.1.16—A buffer solution is one that resists change in pH on the addition of small amounts of acid or alkali.
Reactivity 3.1.17—The pH of a buffer solution