Bond strength and length of HF and H2O

I know that acidity of an acid increases across a period (with electronegativity increase of the atom bonded to hydrogen) and hence $$\ce{HF}$$ is more acidic than $$\ce{H2O}$$ or $$\ce{NH3}$$. But the reason I learnt it is this way, is that difference in electronegativities of the atoms increases and hence bond becomes more polar and weaker (hence easier to donate a proton).

But shouldn't bond strength increase with difference in electronegativities? Also bond length of $$\ce{HF}$$ is shorter than that of $$\ce{H2O}$$ ($$\pu{92 pm}$$ vs $$\pu{96 pm}$$) and bond enthalpy of $$\ce{HF}$$ is $$\pu{565kJ/mol}$$ as opposed to $$\pu{490kJ/mol}$$ of water. Isn't this contradictory? Why is $$\ce{HF}$$ still more acidic than $$\ce{H2O}$$? Is it because the conjugate base of $$\ce{HF}$$ is highly solvated and more stable in an aqueous solution? Is there not a direct correlation between ease of bond dissociation and acidity?

P.S.: I understand the acidic trend down the group (stability of conjugate base increases and since the halogen atom becomes bigger, resulting in weaker bonds).