Electrolytes are substances that, when dissolved in water or other solvents, dissociate into ions and become electrically conductive.
Properties:
- Electrical Conductivity: Electrolytes conduct electricity in solution due to the presence of free ions.
- Dissociation: Electrolytes dissociate into ions through a process called ionization.
- Ionic Strength: The concentration of ions in solution affects the electrolyte’s ability to conduct electricity.
Types of Electrolytes:
- Strong Electrolytes: Ionize completely in solution, producing a high concentration of ions. Examples: $ NaCl $ , $ HCl $ , $ NaOH $
- Weak Electrolytes: Ionize only partially, producing a lower concentration of ions. Examples: $ CH_3COOH $ (acetic acid), $ NH_3 $ (ammonia)
Examples:
Strong Electrolytes:
- Sodium chloride ( $ NaCl $ )
- Hydrochloric acid ( $ HCl $ )
- Sodium hydroxide ( $ NaOH $ )
- Potassium chloride ( $ KCl $ )
- Calcium chloride ( $ CaCl_2 $ )
Weak Electrolytes:
- Acetic acid ( $ CH_3CO(OH) $ )
- Ammonia ( $ NH_3 $ )
- Carbonic acid ( $ H_2CO_3 $ )
- Phosphoric acid ( $ H_3PO_4 $ )
- Hydrofluoric acid ( $ HF $ )
Applications:
- Batteries: Electrolytes facilitate the flow of ions between electrodes, generating an electrical current.
- Electrolysis: Electrolytes allow the separation of elements or compounds through an electrical current.
- Water Purification: Electrolytes can be used to remove impurities from water by a process called electrodialysis.