Timeline for Acidity of oxonium ion
Current License: CC BY-SA 3.0
19 events
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| Mar 6, 2015 at 20:59 | history | edited | DavePhD | CC BY-SA 3.0 |
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| Jan 29, 2015 at 11:02 | vote | accept | EJC | ||
| Jan 28, 2015 at 20:42 | comment | added | DavePhD | @Marko You have to study Debye-Huckel theory and further advances of that theory. Activity coefficients initially decrease with increasing ionic strength, go through a minimum and then increase sharply. | |
| Jan 28, 2015 at 19:30 | comment | added | EJC | Why does the activity coefficient increase, when the concentration increases? Is it because of triple ions formation? | |
| Jan 28, 2015 at 17:53 | history | edited | DavePhD | CC BY-SA 3.0 |
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| Jan 28, 2015 at 17:49 | comment | added | DavePhD | @Marko OK, see digitalcommons.unl.edu/cgi/… should be no paywall, has pH -4 and below, I'll add it to answer | |
| Jan 28, 2015 at 17:41 | comment | added | EJC | Negative sure, but I am interested in less than -1.7. | |
| Jan 28, 2015 at 16:53 | comment | added | DavePhD | @Babounet the Wikipedia table isn't correct, the pHs are really even more negative than that at high concentration | |
| Jan 28, 2015 at 16:38 | comment | added | Babounet | Another example, just check the wikipedia page for HCl en.wikipedia.org/wiki/Hydrochloric_acid and you can see that you can "easily" reach negative pH. | |
| Jan 28, 2015 at 16:35 | history | edited | DavePhD | CC BY-SA 3.0 |
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| Jan 28, 2015 at 16:34 | comment | added | DavePhD | @Marko As a substitute see community.asdlib.org/imageandvideoexchangeforum/2013/07/31/… which illustrates one of the paradoxes: that [H+] can be cut in half, yet hydrogen ion activity increases is a given example | |
| Jan 28, 2015 at 16:16 | comment | added | EJC | Sadly, can't access the: Paradoxes: Demonstrating That It Is Not True That pH ≡ -log[H+]. | |
| Jan 28, 2015 at 15:33 | history | edited | DavePhD | CC BY-SA 3.0 |
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| Jan 28, 2015 at 15:12 | history | edited | DavePhD | CC BY-SA 3.0 |
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| Jan 28, 2015 at 15:00 | comment | added | DavePhD | @Marko, OK, I added to the answer, basically because hydrogen ion activity greatly deviates from hydrogen ion concentration in concentrated acids and pH is defined as -log of hydrogen ion acitivity, not concentration. | |
| Jan 28, 2015 at 14:58 | history | edited | DavePhD | CC BY-SA 3.0 |
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| Jan 28, 2015 at 14:01 | comment | added | EJC | How is -3.6 possible? Please elaborate. | |
| Jan 27, 2015 at 22:05 | history | edited | DavePhD | CC BY-SA 3.0 |
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| Jan 27, 2015 at 21:55 | history | answered | DavePhD | CC BY-SA 3.0 |