I'm confused about the dissolution of strong acids (like HCl) in water. We're told that they dissolve completely because They are strong electrolytes. The hydrogen atom that is lost during dissociation is *not* strongly bound to the rest of the acid molecule. Therefore, the solvent (usually water) pulls at the H+ atom more strongly than the rest of the acid molecule. As far as I can tell, this is completely contradictory. If it's a strong electrolyte, wouldn't the rest of the acid molecule (the Cl- part) have a *stronger* hold on the H+ ion than a weaker acid/weaker electrolyte? Wouldn't it be *harder* to separate the H+ ion from the molecule?