Elektrolyte

An Elektrolyte is a substance that dissociates into ions when dissolved in water or melted, enabling the solution or melt to conduct electricity. The presence of mobile ions is the basis for electrical conduction in electrolytic systems.

In chemistry, electrolytes include acids, bases, and salts. They are classified as strong electrolytes, which dissociate completely in solution, and weak electrolytes, which only partially dissociate. Substances that do not form ions in solution are called non-electrolytes and conduct electricity poorly.

Common examples of electrolytes include sodium chloride (a salt), hydrochloric acid (a strong electrolyte), and potassium hydroxide (a strong electrolyte). Weak electrolytes include substances such as acetic acid. In the molten state, many salts also behave as electrolytes, enabling ionic conduction without water.

In biology, electrolytes are essential ions in body fluids. They regulate nerve impulses, muscle contraction, hydration, blood pH, and fluid balance. Major ions include sodium, potassium, chloride, bicarbonate, calcium, and magnesium. The body maintains electrolyte balance through intake, renal regulation, and hormonal control; imbalances can affect cardiovascular and neuromuscular function.

Industrial and technological uses of electrolytes include electrolysis, electroplating, and metal refining, where ions move between electrodes. In energy storage, electrolytes enable ion transport in batteries and capacitors; solid-state and polymer electrolytes are studied to improve safety and performance.

Measurement of electrolyte levels is common in medicine. Abnormal levels can result from dehydration, kidney disease, endocrine disorders, or gastrointestinal losses and are treated with dietary adjustments or intravenous fluids.