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: $H<em>2SO</em>4$
• Carbonic acid: $H<em>2CO</em>3$
  • Formed from carbon dioxide and water: $CO<em>2 + H</em>2O \rightarrow H<em>2CO</em>3$

Organic Acids

• Acetic acid: $CH<em>3COOH$ or $CH</em>3CO_2H$
  • Structure: H$_3$C-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).