# Solubility vs Dissociation of HF

Ok, so I understand that solubility is a measure of how well a compound is solvated by the solvent. And dissociation is a measure of how much of a compound splits into its ionized forms. Does HF have high solubility, but low dissociation (weak acid)? How can that be?

Is it because it forms strong hydrogen bonds in solution and thus forms stable solvation spheres (solubility), but its high electronegativity prevents H+ atoms from leaving its vicinity (dissociation)?

• Solubility and dissociation are totally unrelated things, like bulimia and amnesia. Sugar (or better yet, ethanol) dissolves extremely well, but does not dissociate at all. $\ce{AgCl}$ is an example of the opposite kind. – Ivan Neretin Oct 5 '16 at 13:24
• @IvanNeretin - For chemicals which are considered to be ionic compounds solubility and dissociation are somewhat linked. – MaxW Oct 5 '16 at 13:55
• Yeah, maybe, somewhat. BTW, would you consider $\ce{HF}$ ionic? To me, it isn't (that is, unless dissolved in water, but even then, not quite). – Ivan Neretin Oct 5 '16 at 14:09
• – Mithoron Oct 5 '16 at 20:09

It is because it forms strong hydrogen bonds in solution and thus forms stable solvation spheres (solubility), but its high electronegativity prevents $\ce{H+}$ atoms from leaving its vicinity (dissociation).
Dissociation is one mechanism of dissolution, but not the only one. Also, however, the $\ce{H-F}$ bond strength is not solely determined by electronegativity.