2007-06-04 16:19:39 · 5 answers · asked by lostinlalaland 2 in Science & Mathematics ➔ Chemistry
Generally, chemists define a "strong" acid as one that is ionized completely in solution (generally assumed to be water unless otherwise specified). By the "chemist's definition, HF would clasify as a weak acid because it does not completely ionize in solution. It is true that it will eat glass and cause serious burns however.
2007-06-04 16:53:20 · answer #1 · answered by Flying Dragon 7 · 2⤊ 0⤋
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RE:
is HF a weak or strong acid?
2015-08-19 00:46:04 · answer #2 · answered by Mariellen 1 · 0⤊ 0⤋
Just because HCL, HBr and HI are strong acids dont think HF is a strong acid. HF is a very weak acid.
2007-06-04 16:59:11 · answer #3 · answered by Emad 2 · 1⤊ 0⤋
HF is an extremely STRONG acid, infact it is one of the most hazardous and potent. It has to do with the electronegativity of an element, which for Fluorine is the highest. Fluorine has the highest electronegitivity of ANY element, b/c it is very reactive and can give up electrons very easily. HCl also a strong acid for the same reason, Cl has strong electronegitivity too, but not as strong as HF. Hope this helps.
2007-06-04 16:24:16 · answer #4 · answered by brix510 4 · 1⤊ 1⤋
Acid strength depends on what solvent it is in but normally HF is considered a very strong acid. It is not stored in glass containers because it will eat up the glass. If you get it on your skin it will eat you to the bone.
2007-06-04 16:25:55 · answer #5 · answered by Anonymous · 1⤊ 1⤋
In Chem textbooks, HF is the weakest of the periodic acids. If you compare it to acetic acid (a weak acid), the pKa of HF is 3.7-5 (depending if in water or another solvent) and the pKa of acetic acid is 4.8. I would call it weak but I wouldn't handle it without precautions (same as acetic acid).
2007-06-04 16:43:03 · answer #6 · answered by Tiffany T 3 · 1⤊ 1⤋
"Because of its low tendency to dissociate into H+ and F- ions in water, it is properly considered a weak acid"---from Wikipedia
It is, however, highly corrosive ....this is all explained in the Wikipedia article. The "Safety" section is particularly informative.
2007-06-04 16:23:53 · answer #7 · answered by Sea Anemone 2 · 1⤊ 1⤋