elektrolit

An elektrolit is a substance that dissociates into ions when dissolved in water or melted, allowing the solution or melt to conduct electricity. In chemistry, electrolytes include salts, acids, and bases that release ions such as Na+, Cl−, H+, and OH−. By contrast, non-electrolytes dissolve without producing ions and therefore conduct poorly.

Electrolytes are often described by their extent of dissociation. Strong electrolytes dissociate completely in solution (for example, many salts like NaCl and bases like KOH). Weak electrolytes dissociate only partially (such as acetic acid), producing a limited concentration of ions. Non-electrolytes do not ionize to a significant extent.

In biology, electrolytes are ions present in body fluids that are essential for membrane potentials, nerve impulses, muscle contraction, fluid balance, and pH regulation. Major ions include sodium, potassium, calcium, chloride, bicarbonate, and magnesium. Their concentrations are tightly regulated by the kidneys and hormonal systems; imbalances can affect heart rhythm, hydration, and metabolism.

In technology and industry, electrolytes enable electrochemical reactions used in electrolysis, electroplating, and refining. They are also a key component of energy storage devices. Batteries and supercapacitors use electrolyte solutions or solids to conduct ions between electrodes. These electrolytes can be aqueous or non-aqueous, and solid or gel-like in newer designs. Lithium-ion systems, for example, rely on lithium salts in organic solvents, while solid-state and polymer electrolytes are areas of active development.

Commonly encountered electrolytes include salts such as sodium chloride, potassium chloride, and calcium salts, as well as acids and bases that dissociate in water. In medicine and nutrition, electrolyte balance is important for hydration and physiological function. See also conductivity, electrochemistry, and battery technology.