Elektrolite

Elektrolite is a term used in some languages to refer to an electrolyte, a substance that dissociates into ions in solution and conducts electricity. In aqueous solutions, electrolytes break into positively and negatively charged ions; in molten salts, ions move freely and enable electrical conduction.

Electrolytes are commonly classified as strong electrolytes, which dissociate completely in solution, or weak electrolytes, which dissociate only partially. Non-electrolytes, by contrast, do not ionize and therefore conduct electricity poorly or not at all. The ability to conduct electricity depends on the concentration of mobile ions and the temperature of the solution.

Typical examples include sodium chloride (NaCl), potassium chloride (KCl), sulfuric acid (H2SO4), and sodium hydroxide (NaOH). These substances release ions such as Na+, K+, Cl-, H+, OH-, and SO4^2-. Substances like glucose or pure alcohols are non-electrolytes because they largely remain molecular in solution and do not yield significant ions.

Biological systems rely on electrolytes for essential functions, including maintaining osmotic balance, nerve transmission, and muscle contraction. In medicine, electrolyte solutions are used for hydration and treatment of imbalances. In industry, electrolytes enable processes in batteries, electroplating, electrorefining, and various electrochemical syntheses. The electrical conductivity of an electrolyte solution is a key property measured to assess concentration, purity, and suitability for a given application, often expressed in terms of molar conductivity and conductivity in siemens per meter.

See also electrolyte, electrochemistry, conductivity, and ion transport.