Acid-Base Chemistry: Bronsted-Lowry and Lewis Definitions with Examples

Acid-Base Definitions

Bronsted-Lowry Definition

• Acid: A proton (H^+) donor.
• Base: A proton (H^+) acceptor.

Lewis Definition

• Acid: An electron pair acceptor.
• Base: An electron pair donor.

Types of Acids

Inorganic (Mineral) Acids

• Hydrofluoric acid: HF
• Hydrochloric acid: HCl
• Hydrobromic acid: HBr
• Hydriodic acid: HI
• Sulfuric acid: H2SO4
• Carbonic acid: H2CO3
  • Formed from carbon dioxide and water: CO2 + H2O \rightarrow H2CO3

Organic Acids

• Acetic acid: CH3COOH or CH3CO_2H
  • Structure: H_3C-C(=O)-OH
• Benzoic acid: A benzene ring with a carboxylic acid functional group (-COOH) attached.

Types of Bases

Inorganic Bases

• Hydroxide ions: OH^-
• Ammonia: NH_3
• Bicarbonate ions: HCO_3^-

Organic Bases

• Ammonia: NH_3
• Amide: R-NH_2
  • Note: 'R' represents any carbon-containing group.
  • Organic bases containing an 'R' group (e.g., R-NH_2) can function as either an acid or a base depending on the specific group and reaction conditions, often due to the presence of a lone pair on nitrogen (acting as a Lewis base) or the ability to donate a proton (acting as a Bronsted-Lowry acid under certain conditions).