Final answer:
HCl is a strong acid and a strong electrolyte because it dissociates almost completely into ions when dissolved in water. It is recognized as a strong acid in standard reference tables and by its chemical behavior.
Step-by-step explanation:
HCl, which stands for hydrochloric acid, dissociates essentially 100% into ions when it is dissolved in water. This high degree of ionization indicates that HCl is a strong acid and, consequently, a strong electrolyte. Because its reaction is almost completely to completion, it is classified as a strong acid. A weak acid or weak base, in contrast, only partially dissociates in solution, leading to a relatively low concentration of ions.
Using references such as Table 14.7.1 and other academic sources, HCl is consistently listed as a strong acid. In chemical equations, we represent the dissociation of HCl as: HCl → H+ + Cl. The fact that this reaction goes to completion, as opposed to establishing an equilibrium, further confirms the strong acidic nature of HCl.
Weak acids, such as acetic acid (HC2H3O2), do not dissociate completely and their reactions are better represented as reversible. Since HCl is not in this category, it does not display properties of a weak acid, strong base, weak base, or non-electrolyte.