Electrolyte
Definition and meaning of Electrolyte in chemistry.
Electrolyte is a substance that, when dissolved in a polar solvent (usually water) or melted, dissociates into free-moving ions and forms a liquid capable of conducting electric current.
In more detail
Conductivity arises because the liberated cations and anions migrate toward oppositely charged electrodes when an electric field is applied, carrying charge through the liquid. Electrolytes are classified by the extent of ionization: strong electrolytes (most ionic salts and strong acids/bases) dissociate essentially completely, giving high conductivity, while weak electrolytes (like weak acids) ionize only partially, giving lower conductivity. Substances that dissolve without forming ions, such as sugar, are non-electrolytes and do not conduct electricity.
Key facts
| Field | General Chemistry |
|---|---|
| Common example | NaCl (sodium chloride) |
| Charge carriers | Mobile cations and anions |
| Classification | Strong, weak, or non-electrolyte |
Dissolving sodium chloride (NaCl) in water releases Na+ and Cl- ions, and the resulting solution readily conducts electricity, whereas an equally concentrated sugar solution does not.
Frequently asked questions
What is the difference between a strong and a weak electrolyte?
A strong electrolyte, such as NaCl or HCl, dissociates almost completely into ions in solution and conducts electricity well. A weak electrolyte, such as acetic acid (CH3COOH), ionizes only partially, so its solution conducts much more weakly.
Is pure water an electrolyte?
Pure water is an extremely weak electrolyte because it self-ionizes only slightly (2H2O ⇌ H3O+ + OH-), so it conducts electricity poorly unless additional ions are dissolved in it.