Which of the following can best describe the nature of an electrolyte?

An electrolyte is best described as a solution that dissolves ionic compounds. This is because electrolytes are substances that, when dissolved in water (or another solvent), dissociate into ions. These dissolved ions are free to move and carry an electric charge, which allows the solution to conduct electricity.

For example, when table salt (sodium chloride) is added to water, it breaks apart into sodium ions (Na⁺) and chloride ions (Cl⁻). This process of dissociation is crucial for the formation of an electrolyte, as these ions are responsible for the conductivity of the solution.

In contrast, non-conductive liquids do not have the ions necessary to facilitate the flow of electricity. Gases that conduct electricity typically require very specific conditions, such as being ionized, which is not the typical behavior of a gas under standard conditions. Solid conductors, while they do conduct electricity, do not qualify as electrolytes since they do not involve a liquid solution containing free-moving ions. Hence, the defining characteristic of an electrolyte is its ability to exist as a solution containing dissolved ionic compounds, enabling electrical conductivity through those ions.