Electrolyte

An electrolyte is a substance that dissociates into ions when dissolved in water or melted, enabling the solution or melt to conduct electricity. In aqueous solutions, salts, acids, and bases commonly act as electrolytes. The extent of dissociation determines electrolyte strength: strong electrolytes dissociate completely, while weak electrolytes dissociate only partially. Electrolyte solutions conduct electricity due to the mobility of the resulting ions. In solid-state chemistry, some materials function as electrolytes when molten or in solid form and are used in batteries and fuel cells.

In biology, the term electrolyte often refers to the ions present in body fluids, such as sodium, potassium, calcium, chloride, bicarbonate, magnesium, phosphate, and sulfate. These ions regulate osmotic balance, acid-base status, nerve impulse transmission, muscle contraction, and enzyme activity. The kidneys and hormones maintain electrolyte balance, and disturbances can arise from dehydration, illness, medications, or dietary changes. Abnormal levels of sodium, potassium, or calcium can have serious physiological consequences.

Clinical assessment uses a serum electrolyte panel to measure concentrations of these ions, guiding treatment. Management depends on the underlying cause and may involve intravenous or oral rehydration, electrolyte supplements, or dietary adjustments. Careful monitoring is essential, as rapid shifts in levels—particularly of sodium and potassium—can be dangerous.

Industrial and practical applications extend to electrolysis, electroplating, and energy storage technologies such as batteries and supercapacitors. In soils and environmental contexts, electrolyte concentrations influence conductivity and fertility. The term thus encompasses both chemical substances that provide ions and the physiologically critical ions that sustain life.