Timeline for Why is fluoroantimonic acid so strong?
Current License: CC BY-SA 3.0
14 events
| when toggle format | what | by | license | comment | |
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| S Apr 29, 2014 at 17:04 | history | suggested | L.B. | CC BY-SA 3.0 |
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| Apr 29, 2014 at 16:48 | review | Suggested edits | |||
| S Apr 29, 2014 at 17:04 | |||||
| Apr 29, 2014 at 16:24 | comment | added | Martin - マーチン♦ | Dissociation as in $\ce{HB + H2O<=>H3+O + B-}$ is not ionisation. | |
| Apr 29, 2014 at 14:49 | answer | added | Uncle Al | timeline score: 6 | |
| Apr 29, 2014 at 9:32 | history | edited | please delete me | CC BY-SA 3.0 |
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| Apr 9, 2014 at 12:15 | vote | accept | please delete me | ||
| Oct 9, 2013 at 19:12 | comment | added | Ben Norris | The acid strength dichotomy of strong/weak is relative to $\ce{H3O+}$, the conjugate acid of water (see Brian's answer). We can make the divide relative to other conjugate acids, and then some of our "strong" acids may become weak acids. | |
| Oct 9, 2013 at 15:08 | history | edited | please delete me | CC BY-SA 3.0 |
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| Oct 9, 2013 at 15:04 | comment | added | please delete me | I think the way I phrased that is confusing. I meant that there are degrees of weakness but no degrees of strength because all strong acids 100% ionise. That it just what I learnt in high school so it must be wrong :) | |
| Oct 9, 2013 at 0:21 | history | tweeted | twitter.com/#!/StackChemistry/status/387734429789335552 | ||
| Oct 8, 2013 at 22:33 | answer | added | user1160 | timeline score: 12 | |
| Oct 8, 2013 at 22:06 | comment | added | Ben Norris | There are degrees of strength in acids, else there would not be strong acids and weak acids. There would just be acids. | |
| Oct 8, 2013 at 15:06 | review | First posts | |||
| Oct 8, 2013 at 16:23 | |||||
| Oct 8, 2013 at 14:51 | history | asked | please delete me | CC BY-SA 3.0 |