I know that acidity of an acid increases across a period(with electronegativity increase of the atom bonded to hydrogen) and hence HF is more acidic than H2O or 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 HF is shorter than that of H2O (92 pm vs 96pm) and bond enthalpy of HF is 565kJ/mol as opposed to 490kJ/mol of water. Isn't this contradictory? Why is HF still more acidic than H2O? Is it because the conjugate base of HF is highly solvated and more stable in an aqueous solution? Is there not a direct correlation between ease of bond dissociation and acidity?

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

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).

I know that acidity of an acid increases across a period(with electronegativity increase of the atom bonded to hydrogen) and hence HF is more acidic than H2O or 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 HF is shorter than that of H2O (92 pm vs 96pm) and bond enthalpy of HF is 565kJ/mol as opposed to 490kJ/mol of water. Isn't this contradictory? Why is HF still more acidic than H2O?

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

I know that acidity of an acid increases across a period(with electronegativity increase of the atom bonded to hydrogen) and hence HF is more acidic than H2O or 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 HF is shorter than that of H2O (92 pm vs 96pm) and bond enthalpy of HF is 565kJ/mol as opposed to 490kJ/mol of water. Isn't this contradictory? Why is HF still more acidic than H2O? Is it because the conjugate base of HF is highly solvated and more stable in an aqueous solution? Is there not a direct correlation between ease of bond dissociation and acidity?

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