- #1
pinkyjoshi65
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Could someone give and example of a substance that is a Bronsted-Lowry base, but not an Arrhenius base..
Example of a substance that is a Bronsted-Lowry, but not Arrhenius
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Discussion Overview
The discussion revolves around identifying a substance that qualifies as a Bronsted-Lowry base but does not meet the criteria for an Arrhenius base. The focus is on theoretical definitions and classifications within acid-base chemistry.
Discussion Character
- Exploratory, Technical explanation, Debate/contested
Main Points Raised
- One participant suggests ammonia (NH3) as an example of a Bronsted-Lowry base, noting that it accepts a proton but does not dissociate hydroxide ions in water, thus not qualifying as an Arrhenius base.
- Another participant introduces the concept of Lewis acids and bases, questioning the relevance of the Bronsted-Lowry and Arrhenius definitions.
- A further reply reiterates the Lewis definition, stating that ammonia can also be classified as a Lewis base due to its ability to donate a pair of electrons. This participant also mentions that NH3 is considered amphoteric and can autoionize.
Areas of Agreement / Disagreement
Participants do not reach a consensus, as there are competing views regarding the definitions and classifications of ammonia in the context of Bronsted-Lowry and Arrhenius theories.
Contextual Notes
The discussion includes varying interpretations of acid-base definitions and the implications of ammonia's behavior in different contexts, such as its amphoteric nature and autoionization.
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