Timeline for link between acidity and [H3O+]
Current License: CC BY-SA 3.0
8 events
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| Nov 18, 2015 at 15:14 | history | edited | aidaGoG | CC BY-SA 3.0 |
added 38 characters in body
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| Nov 18, 2015 at 14:48 | comment | added | aidaGoG | I was considering pH as a measure of acidity of a solution in my question. What puzzles me is that two solutions having the same concentration of $\ce{H3O+}$, but one having on top of that some $\ce{CH3COOH}$ in it are considered equally acid, as far as pH is concerned. | |
| Nov 18, 2015 at 14:42 | comment | added | Nicolau Saker Neto | $\mathrm{pH}$ is a measure of acidity of a solution, not of a substance. One of the measures for the latter would be the substance's $\mathrm{pK_a}$. If you look at the formula for the $\mathrm{pK_a}$, you can see that a type of normalization is going on; you divide the amount of protons and deprotonated acid in a solution of the acid by the amount of still protonated acid. If you really want to compare substance acidities using $\mathrm{pH}$, you also need to know the concentration of the acid, which ultimately allows one to calculate the $\mathrm{pK_a}$, even if only implicitly. | |
| Nov 18, 2015 at 14:34 | answer | added | Jan | timeline score: 2 | |
| Nov 18, 2015 at 14:18 | comment | added | Jan |
Please use the \ce{...} environment for chemical formulae. Type $\ce{SO4^2-}$ for $\ce{SO4^2-}$ or $\ce{CH3COO-}$ for $\ce{CH3COO-}$. It not only makes typing much easier but also uses an upright font. Check out the help center and this meta-post for more information.
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| Nov 18, 2015 at 14:17 | history | edited | Jan | CC BY-SA 3.0 |
added \e
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| Nov 18, 2015 at 14:02 | review | First posts | |||
| Nov 18, 2015 at 14:20 | |||||
| Nov 18, 2015 at 13:59 | history | asked | aidaGoG | CC BY-SA 3.0 |