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)?




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.


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