How do strong electrolytes differ from weak electrolytes?

Strong electrolytes are substances that completely dissociate into ions when dissolved in a solvent, typically water. This complete dissociation is what allows them to effectively conduct electricity. When a strong electrolyte like sodium chloride (NaCl) is dissolved in water, it separates into its constituent ions (Na⁺ and Cl⁻), and these free-moving ions are essential for carrying an electric current.

In contrast, weak electrolytes only partially dissociate into ions, meaning that in solution, there will be a mixture of the undissociated compound and the ions. This results in a much lower conductivity compared to strong electrolytes. Examples of weak electrolytes include acetic acid (CH₃COOH) and ammonium hydroxide (NH₄OH), which do not provide as many ions to the solution as strong electrolytes.

Given this understanding, the assertion that strong electrolytes completely dissociate into ions accurately captures their defining characteristic. This differentiates them from weak electrolytes, which do not have the same level of ionization and, consequently, conductivity.