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Posted: Wed Dec 04, 2019 9:02 pm
Why is HF not a strong acid like HCl or HI?
Posted: Wed Dec 04, 2019 9:08 pm
If you recall, Dr. Lavelle stated that the strength of an acid is determined by two aspects the first being how easily it gives off its H+ and the second being the stability of the remaining anion. In the case of HF, the anion would not be as stable as HCl because Cl- is able to withdraw much more e- density.
Posted: Wed Dec 04, 2019 9:29 pm
My TA said it's because F has a smaller atomic radii
Posted: Wed Dec 04, 2019 9:30 pm
but its IMF's are greater in the HF than the others due to higher electronegativity right?
Posted: Wed Dec 04, 2019 11:19 pm
F- is not stable in solution and would react with the H+ ions in solution taking them out of solution.