How is an electrolyte defined?

An electrolyte is defined as a substance that dissociates into ions when dissolved in a solvent, typically water. This dissociation leads to the formation of charged particles that are capable of conducting electricity. The presence of these free ions allows the solution to enable electrical flow, which is a fundamental property of electrolytes.

The significance of the solvent, usually water, is that it is polar and can stabilize the charged ions through solvation, allowing the ions to move freely in the solution. In electrochemical cells, for example, electrolytes are crucial for the movement of ions between the anode and cathode, facilitating the flow of electric current.

In contrast to this definition, a substance that remains solid in any solvent would not dissociate into ions and, therefore, could not conduct electricity in solution. Similarly, a material that does not conduct electricity would not function as an electrolyte since conductivity is a key characteristic of these substances. Lastly, a compound used to increase the boiling point of water does not pertain to the definition of an electrolyte, which is specifically concerned with the dissociation into ions and conductive properties.