LP6

• Acids and bases play a central role in chemistry
• Every chemical reaction can be classified as an acid-base reaction, except for redox reactions
• Acid-base chemistry is important outside of laboratory reactions, influencing bodily functions and maintaining homeostasis
• Arrhenius: Increases H+ in water
• Lewis: Electron-pair acceptor
• Three definitions of base Arrhenius, Increases OH-, 1880’s -Brønsted- Lowry, Proton acceptor, 1923 - Lewis (not part of Chem 1), Electron-pair donor, 1923
• Lewis base: Electron-pair donor
• Include soluble hydroxides like NaOH, KOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2
• Conjugate acids and bases
• Reactions between acids and bases yield conjugate bases and acids
• Strong acids have weak conjugate bases, weak acids have strong conjugate bases
• Concentrations of H+ and OH-
• Maintains pH levels and resists changes
• Buffer range is the pH range where a buffer effectively neutralizes added acids and bases
• Buffer systems are typically made of a weak acid and its conjugate base or a weak base and its conjugate acid
• Buffer pH depends on the weak acid or base involved, the ionization constant (Ka), and the relative concentrations of the weak acid or base and its conjugate base or acid