Electrolytes are substances that dissociate into ions when dissolved in water, allowing them to conduct electricity. They can be classified into strong and weak electrolytes based on their degree of ionization in solution. Here are some common compounds that are classified as electrolytes:
Strong Electrolytes:
- Sodium chloride (NaCl) - Dissociates completely into sodium (Na⁺) and chloride (Cl⁻) ions.
- Potassium chloride (KCl) - Dissociates into potassium (K⁺) and chloride (Cl⁻) ions.
- Calcium chloride (CaCl₂) - Dissociates into calcium (Ca²⁺) and chloride (Cl⁻) ions.
- Magnesium sulfate (MgSO₄) - Dissociates into magnesium (Mg²⁺) and sulfate (SO₄²⁻) ions.
- Hydrochloric acid (HCl) - Strong acid that dissociates into hydrogen (H⁺) and chloride (Cl⁻) ions.
- Sodium hydroxide (NaOH) - Strong base that dissociates into sodium (Na⁺) and hydroxide (OH⁻) ions.
- Potassium nitrate (KNO₃) - Dissociates into potassium (K⁺) and nitrate (NO₃⁻) ions.
Weak Electrolytes:
- Acetic acid (CH₃COOH) - Partially dissociates into acetate (CH₃COO⁻) and hydrogen (H⁺) ions.
- Ammonium hydroxide (NH₄OH) - Partially dissociates into ammonium (NH₄⁺) and hydroxide (OH⁻) ions.
- Carbonic acid (H₂CO₃) - Partially dissociates into bicarbonate (HCO₃⁻) and hydrogen (H⁺) ions.
- Phosphoric acid (H₃PO₄) - Partially dissociates into dihydrogen phosphate (H₂PO₄⁻), hydrogen (H⁺), and phosphate (PO₄³⁻) ions in steps.
Both strong and weak electrolytes play vital roles in various biological, chemical, and industrial processes.