Salts

Definition and Properties

Salts are ionic compounds that contain cations other than H+ and anions other than OH-. They play important roles in physiological processes due to their ability to dissociate in water and conduct electrical currents.

• Examples: NaCl (sodium chloride), CaCO3 (calcium carbonate), KCl (potassium chloride)

• Dissociation: Salts easily dissociate into ions in the presence of water, forming electrolytes that conduct electrical currents.

• Functions of Salts/Electrolytes:

  • Nerve cell communication

  • Muscle contraction

  • Maintenance of fluid balance in the body

  • Physiological activities such as those listed above depend on proper electrolyte balance.

  • If electrolyte balance is disrupted, virtually nothing in the body will work and death will quickly ensue.

• Example of Salt Dissociation: The antidepressant lithium chloride dissociates as follows:

Acids and Bases

General Properties

Like salts, acids and bases are electrolytes. They ionize and dissociate in water and can conduct an electrical current.

Acids

Acids are substances that donate protons (H+ ions) in solution.

• Proton Donors: Acids release hydrogen ions when dissolved in water.

• Electrolyte Strength:

  • Acids are called acidic if they yield H+ in water.

  • Partial Dissociation (Weak Acid): For example, carbonic acid (H2CO3) dissociates partially:

  • Complete Dissociation (Strong Acid): For example, hydrochloric acid (HCl) dissociates completely:

Bases

Bases are substances that accept protons or release hydroxide ions (OH-) in solution.

• Proton Acceptors: Bases attract and combine with H+ ions in water.

Summary Table: Comparison of Salts, Acids, and Bases

Additional info:

• Electrolytes are crucial for maintaining homeostasis in the body. Imbalances can lead to serious health issues such as arrhythmias, muscle weakness, or neurological disturbances.

• Strong acids and bases dissociate completely in water, while weak acids and bases only partially dissociate.