What distinguishes strong electrolytes from weak electrolytes?

Strong electrolytes are characterized by their ability to completely dissociate into their constituent ions when dissolved in water. This complete dissociation results in a solution that can conduct electricity very effectively due to the high concentration of free-moving ions. Examples of strong electrolytes include salts like sodium chloride (NaCl) and potassium nitrate (KNO3), which fully break apart into positive and negative ions.

In contrast, weak electrolytes do not completely dissociate in solution; they only partially ionize, resulting in a lower concentration of ions compared to strong electrolytes. This partial ionization limits their ability to conduct electricity. Common weak electrolytes include weak acids like acetic acid (CH3COOH) and weak bases like ammonia (NH3).

Thus, the distinction lies in the degree of dissociation in solution: strong electrolytes fully dissociate while weak electrolytes do so only partially. The choice stating that strong electrolytes completely dissociate captures the essence of what sets them apart from weak electrolytes.