Timeline for Why is HCl a stronger acid than Acetic Acid?
Current License: CC BY-SA 3.0
10 events
| when toggle format | what | by | license | comment | |
|---|---|---|---|---|---|
| Feb 3, 2020 at 12:23 | answer | added | RandomName | timeline score: 0 | |
| Oct 31, 2018 at 4:57 | answer | added | Dr. J. Pelezo | timeline score: 1 | |
| Mar 15, 2016 at 6:28 | review | First posts | |||
| Mar 15, 2016 at 6:52 | |||||
| Mar 15, 2016 at 6:20 | vote | accept | user307178 | ||
| Mar 14, 2016 at 22:59 | comment | added | MaxW | The chloride anion and the acetate anion are such different species that the "why" in the question is hard to explain without blowing smoke. The place to start is to recognize that the Pauling electronegativity scale is for free atoms in space, not ions in aqueous solution. // Obviously in aqueous solutions you can lookup pKa's to order acid strengths. | |
| Mar 14, 2016 at 21:46 | answer | added | Lighthart | timeline score: 11 | |
| Mar 14, 2016 at 20:13 | history | tweeted | twitter.com/StackChemistry/status/709472449621069824 | ||
| Mar 14, 2016 at 17:03 | comment | added | user10153 | Also acetic acid tends to dimerise, thus reducing the effective number of acetate ions | |
| Mar 14, 2016 at 15:48 | comment | added | etherealflux | I can't dig into my textbook right now, but I believe the reasoning is that water solvates chloride ions extremely well - so a massive amount can dissolve very easily. Acetate ions are stable, but don't interact as well with water. I'll try and get a proper answer written later this evening, if I haven't forgotten (: | |
| Mar 14, 2016 at 15:30 | history | asked | user307178 | CC BY-SA 3.0 |