Sagot :
Answer: a) [tex]HF(aq)+NH_3(aq)\rightarrow NH_4^+(aq)+F^-(aq)[/tex]
b) [tex]NH_4^+[/tex]: conjugate acid of [tex]NH_3[/tex]
[tex]F^-[/tex] : conjugate base of [tex]HF[/tex]
Explanation:
According to the Bronsted-Lowry conjugate acid-base theory, an acid is defined as a substance which looses donates protons and thus forming conjugate base and a base is defined as a substance which accepts protons and thus forming conjugate acid.
For the given reaction:
[tex]HF(aq)+NH_3(aq)\rightarrow NH_4^+(aq)+F^-(aq)[/tex]
Here [tex]HF[/tex] is loosing a proton, thus it is considered as an acid and after losing a proton, it forms [tex]F^-[/tex] which is a conjugate base.
Similarly ,[tex]NH_3[/tex] is gaining a proton, thus it is considered as an base and after gaining a proton, it forms [tex]NH_4^+[/tex] which is a conjugate acid.