If HCl is a strong acid, and it is, and strong acids completely dissociate, is t
ID: 706103 • Letter: I
Question
If HCl is a strong acid, and it is, and strong acids completely dissociate, is there any difference in the concentration (molarity) of H30+ ion and the concentration of HCl? For example, we call a solution 2.0 M HCl. Since HCl dissociates into separate ions, H+ or (H30+) and cl-, wouldn’t it be just as accurate to describe the solution as 2.0 M H30+? If HCl is a strong acid, and it is, and strong acids completely dissociate, is there any difference in the concentration (molarity) of H30+ ion and the concentration of HCl? For example, we call a solution 2.0 M HCl. Since HCl dissociates into separate ions, H+ or (H30+) and cl-, wouldn’t it be just as accurate to describe the solution as 2.0 M H30+?Explanation / Answer
We cannot describe HCl acid solution as H3O+ solution beacuse a chemical compound has to be represented as a whole, meaning it should tell all the species present in the compound as they do participate in the reaction.
Describing HCl solution as H3O+ solution will be like describing all acids as H3O+ solution because all acids (weak or strong) release H3O+ ions. This is highly incorrect as it does not tell us about the resulting anionic (negatively charged) species which result in solution after dissociation of acidic compound. This anoinic species also take part in reaction and can gravely affect the results if wrong acidic compound is used which also gives H3O+ ions