Respuesta :
Answer: a) [tex]HSO_3^-[/tex]: Bronsted base
[tex]H_2O[/tex] : Bronsted acid
b) None
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 chemical equations:
a) [tex]HSO_3^-(aq.)+H_2O(l)\rightarrow H_2SO_3(aq.)+OH^-(aq.)[/tex]
Here, [tex]HSO_3^-[/tex] is accepting a proton, thus it is considered as a base and after gaining a proton, it forms [tex]H_2SO_3[/tex] which is an conjugate acid.
And, [tex]H_2O[/tex] is losing a proton, thus it is considered as a acid and after losing a proton, it forms [tex]OH^-[/tex] which is a conjugate base.
b) [tex[(CH_3)_3N(g)+BCl_3(g)\rightarrow (CH_3)_3NBCl_3(s)[/tex]
As there is no donation or acceptance of [tex]H^+[/tex], they cannot be considered as Bronsted acid or base. [tex](CH_3)_3N[/tex] gives its electrons to [tex]BCl_3[/tex], thus [tex](CH_3)_3N[/tex] act as lewis base and [tex]BCl_3[/tex] act as lewis acid.
