Introduction to Acids

Acids are fascinating chemical compounds defined by their ability to donate protons (H⁺ ions) or accept electron pairs. When dissolved in water, they increase the concentration of H⁺ ions (or hydronium ions, H₃O⁺).

• Key Behavior: Release H⁺ ions in aqueous solution. For example, HCl → H⁺ + Cl⁻.
• Classification:
  • Inorganic (Mineral) Acids: Derived from inorganic sources, e.g., H₂SO₄ (sulfuric acid), HNO₃ (nitric acid).
  • Organic Acids: Contain carbon, typically with a carboxyl group (-COOH), e.g., CH₃COOH (acetic acid in vinegar), citric acid in lemons.
• Strength:
  • Strong Acids: Dissociate almost completely in water (e.g., HCl, H₂SO₄ for the first H⁺).
  • Weak Acids: Dissociate only partially in water (e.g., CH₃COOH, H₂CO₃).

The visualizer demonstrates H⁺ ion dissociation and typical acid structures.