Elektrolita

Elektrolita, commonly referred to as electrolyte, is a substance that dissociates into ions when dissolved in a solvent, usually water, and thereby conducts electricity. In an aqueous solution, elektrolita release charged particles (cations and anions) that move and carry electric current. By contrast, non-electrolytes do not produce significant numbers of ions and conduct electricity poorly. Elektrolita include soluble salts, acids, and bases. They can be classified as strong elektrolita, which dissociate essentially completely (for example NaCl, HCl, KOH), or weak elektrolita, which dissociate only partially (for example acetic acid, ammonia). In molten salts or melted ionic solids, ionic conduction can occur as well.

In biology and medicine, electrolytes refer to the ions present in body fluids that support nerve impulses, muscle contraction, fluid balance, and pH buffering. Major physiological electrolytes include sodium, potassium, calcium, magnesium, chloride, bicarbonate, phosphate, and sometimes sulfate. Concentrations are tightly regulated by diet, kidneys, hormones, and other systems; imbalances can cause dehydration, cramps, arrhythmias, confusion, or coma. Electrolyte solutions are administered for rehydration and electrolyte replenishment after losses from vomiting, diarrhea, or sweating.

In technology, elektrolita enable ionic conduction in batteries, electroplating, corrosion processes, and electrolysis. Liquid electrolytes in some batteries contain salts dissolved in organic solvents; aqueous or gel electrolytes are used in other chemistries. Key properties include ionic conductivity, electrochemical stability, and compatibility with electrodes. The study of elektrolita intersects chemistry, physics, and materials science and underpins a wide range of practical applications.