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8.1Acids and Bases

Introduction to Acids and Bases — AP CHEMISTRY Revision Notes & Topical Questions

5 min read 8 parts Lesson 6 of 16 2 quizzes

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Lesson summary

8.1 Introduction to Acids and Bases — AP CHEMISTRY notes: Define acids and bases, identify conjugate pairs and water's role, and relate pH to concentration.Acid — a proton (H+) donorBase — a proton acceptorReaction — an acid-base reaction is a proton transfer from acid to baseAmp…

  • Amphiprotic
  • Autoionisation
  • Neutral solution
  • Definitions
  • Strength relation
  • Brønsted-Lowry acid

Section 1 of 8Brønsted-Lowry definitions

Acid
  • Acid a proton (H+) donor
Base
  • Base a proton acceptor
Reaction
  • Reaction an acid-base reaction is a proton transfer from acid to base

Section 2 of 8Water

Amphiprotic
  • Amphiprotic water can act as an acid or a base
Autoionisation
  • 2H2O ⇌ H3O+ + OH−
Kw
  • [H3O+][OH−] = 1.00 × 10-14 at 25 °C
Neutral solution
  • [H3O+] = [OH−]

Section 3 of 8pH and pOH

Definitions
  • Definitions pH = −log[H3O+] and pOH = −log[OH−]
Relation
  • Relation pH + pOH = 14 at 25 °C
Acidic
  • Acidic pH < 7; basic — pH > 7; neutral — pH = 7

Section 4 of 8Conjugate acid-base pairs

Pair
  • Pair two species differing by one proton
Strength relation
  • Strength relation a strong acid has a weak conjugate base; a weak acid has a stronger conjugate base
Example
  • HBr/Br− and H3O+/H2O in HBr + H2O → Br− + H3O+

Section 5 of 8Strong and weak

TypeIonisationExample
Strong acidCompleteHCl, HNO3
Weak acidPartialCH3COOH
Strong baseComplete dissociationNaOH, Ba(OH)2
Weak basePartialNH3

Section 6 of 8More from the specification

More from the specification
Relative strength order of Brønsted acids
  • Relative strength order of Brønsted acids measuring dissociation constants establishes an empirical acidity order ranging from strong mineral acids to weak organics.
Charge
  • Q = It, measured in coulombs.
    What the symbols mean: Q = charge (C) · I = current (A) · t = time (s)
Reactants
  • The substances that react together at the start of a reaction.
Theory
  • A tested hypothesis that is widely accepted.
Aqueous
  • Dissolved in water.

Section 7 of 8Key terms

TermMeaning
Brønsted-Lowry acidProton donor.
Brønsted-Lowry baseProton acceptor.
AmphiproticAble to donate or accept a proton.
KwIonic product of water.
Conjugate pairTwo species related by one proton.

Section 8 of 8Exam technique

Avoid these mistakes
Saying a pH of 0 is not possible — very concentrated acids can have pH ≤ 0.
Calling any species with H a Brønsted-Lowry acid — it must be able to donate a proton.
Saying water is only a base.

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