An electrolyte is a substance that conducts electric current as a result of a dissociation into positively and negatively charged particles called ions, which migrate toward and ordinarily are discharged at the negative and positive terminals (cathode and anode) of an electric circuit, respectively. Electrolytes can be divided into acids, bases, and salts, because they all give ions when dissolved in water/Chemical_Reactions/Chemical_Reactions_Examples/Electrolytes). The most familiar electrolytes are acids, bases, and salts, which ionize when dissolved in such solvents as water or alcohol. Electrolytes are important body constituents because they conduct electricity, which is essential for muscle and nerve function. They also exert osmotic pressure, keeping body fluids in their own compartments, and act as buffers to resist pH changes in body fluids.

Some key points about electrolytes include:

• Cations: Positively charged ions are called cations.
• Anions: Negatively charged ions are called anions.
• Strong electrolytes: These completely ionize when dissolved, and no neutral molecules are formed in solution. Examples include NaCl, HNO3, HClO3, and CaCl2/Chemical_Reactions/Chemical_Reactions_Examples/Electrolytes).
• Weak electrolytes: These only partially ionize when dissolved, and some neutral molecules are present in their solutions. Examples include NH4OH (ammonia), H2CO3 (carbonic acid), CH3COOH (acetic acid), and most organic acids and bases/Chemical_Reactions/Chemical_Reactions_Examples/Electrolytes).
• Nonelectrolytes: These substances do not dissociate in water because they have no electric charge. Examples include glucose and urea.

Electrolytes are required in batteries, even in dry cells. The simplest battery consists of two electrodes. For example, a copper-zinc battery has a zinc electrode. The zinc atoms have a tendency to become ions, leaving the electrons behind/Chemical_Reactions/Chemical_Reactions_Examples/Electrolytes).