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Well, let’s put it this way:
The Brønsted-Lowry definition, being less specific, is more encompassing than the Arrhenius definition.
Here’s what I mean.
The Brønsted-Lowry definition says that:
The Arrhenius definition says that:
As a result of the more specific nature of the Arrhenius definition, it is confined to only aqueous . With Arrhenius bases, it is additionally specific in that a ##”OH”^(-)## must be donated to solution… while protons aren’t really considered.
One example of a Brønsted-Lowry base that is NOT an Arrhenius base is sodium ethoxide (##”NaOCH”_2″CH”_3##) dissolved in ethanol (##”CH”_3″CH”_2″OH”##).
We should notice that it can accept a proton (by donating electrons), just like the Brønsted-Lowry base definition requires, but it does not donate an ##”OH”^(-)## to water; it can’t, because we aren’t even using water as the !
Thus, sodium ethoxide in ethanol is not an Arrhenius base; though, it IS a Lewis base since its oxygen donates two to get its proton.
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