Concept explainers
Interpretation:
The conjugate acid-base pairs for the given reaction has to be identified.
Concept Introduction:
Bronsted's definition is based on the
According to Bronsted's theory acid donates proton, whereas base accepts proton from acid resulting in the formation of water.
Example: Consider the following reaction.
Hydrogen chloride donates a proton, and hence it is a Bronsted acid. Ammonia accepts a proton, and hence it is a Bronsted base.
Conjugate acid: When Bronsted base accepts a proton the protonated species is known as conjugate acid.
Conjugate base: When Bronsted acid loses a proton deprotonated species is known as conjugate base.
The conjugated acid-base pair is present in opposite side of the reaction. In this the base has one proton less than the acid.
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