Timeline for Why do carbon dioxide and sodium hydroxide not form sodium oxide and carbonic acid?
Current License: CC BY-SA 3.0
8 events
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| Oct 26, 2015 at 18:23 | comment | added | Curt F. |
Good point Jan. I was going off of Wikipedia which says A base anhydride is neither an Arrhenius base, nor a Brønsted–Lowry base, since it does not accept protons and do not increase the hydroxide ion concentration of water. However, a base anhydride is a Lewis base, since it will share an electron pair with some Lewis acids, most notably acidic oxides. It sounds like that is not completely correct. If someone edits Wikipedia I'll edit my answer.
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| Oct 26, 2015 at 14:49 | comment | added | Jan | $\ce{O^2-}$ is a base according to Brønsted and Lowry’s definition as it takes up $\ce{H+}$ ions to form $\ce{OH-}$. $-1$ | |
| Mar 12, 2015 at 19:20 | history | edited | bon | CC BY-SA 3.0 |
edited body
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| Mar 12, 2015 at 16:38 | comment | added | Curt F. | It would be very positive, a hint that the reaction is likely to be thermodynamically unfavorable. (I say "hint" because favorability is determined by $\Delta G=\Delta H - T \Delta S$, so in theory it would be possible for an extremely large positive entropy change to counteract the very large enthalpy change, thus making $\Delta G$ negative and the reaction thermodynamically feasible, but since the reaction consumes a gas, it's entropy change is probably negative, which would only make even more disfavored.) | |
| Mar 12, 2015 at 16:34 | comment | added | Vatsal Manot | On a related note, on of the commenters asked me to look up the standard enthalpy of my proposed reaction. Any ideas why? | |
| Mar 12, 2015 at 16:28 | history | edited | Curt F. | CC BY-SA 3.0 |
reworded "formation" to "hydration"
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| Mar 12, 2015 at 16:26 | vote | accept | Vatsal Manot | ||
| Mar 12, 2015 at 16:21 | history | answered | Curt F. | CC BY-SA 3.0 |