How are strong and weak electrolytes classified?

Strong electrolytes are substances that completely dissociate into ions when dissolved in water. This means that in a solution, all of the solute exists in the form of ions, which allows for the conduction of electricity. Common examples include strong acids like hydrochloric acid and strong bases like sodium hydroxide, which fully ionize to yield hydronium ions (H₃O⁺) and hydroxide ions (OH⁻), respectively.

In contrast, weak electrolytes only partially dissociate into ions, meaning that in a solution, both the undissociated molecules and the ions are present. This results in a lower conductivity compared to strong electrolytes. For example, acetic acid only partially ionizes in solution, producing both ionized and unionized forms.

Understanding this distinction is essential for recognizing how electrolytes behave in aqueous solutions and how they contribute to the overall conductivity of the solution. Choices that suggest weak electrolytes do not dissociate at all or that they completely dissociate misrepresent their behavior, as weak electrolytes do indeed form ions, just not to the extent observed in strong electrolytes.