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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)?
I think your last sentence answers your own question very well:
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.
