|MadSci Network: Chemistry|
The other halogen acids are strong acids. I realize the bond strenth is weaker in these acids, however, if the electronegativity of fluorine is so high, why doesn't it simply take the electron from the hydrogen and ionize? I also recognize the high degree of hydrogen bonding in HF may be a factor. Also, if strong acids are already ionized, why would they cause burns on the skin (ie the energy has already been released and the acid is fully ionized before it hits the skin)? Hope you can help! Thanks
Re: Why is hydrofluoric acid a weak acid?
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