Dear Students,
Please find below the solution to your problem.
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 equation:
a) H2O --> OH- + H+
Here, H2O is loosing a proton, thus it is considered as an acid and after losing a proton, it forms OH- which is a conjugate base.
H2O + H+ --> H3O+
And, H2O is gaining a proton, thus it is considered as a base and after gaining a proton, it forms H3O+ which is a conjugate acid.
b) HCO3- --> CO3{2-} + H+
Here, HCO3- is loosing a proton, thus it is considered as an acid and after losing a proton, it forms CO3{2-} which is a conjugate base.
HCO3- + H+ → H2CO3
And, HCO3- is gaining a proton, thus it is considered as a base and after gaining a proton, it forms H2CO3 which is a conjugate acid.
c) HSO4- --> SO4{2-} + H+
Here, HSO4- is loosing a proton, thus it is considered as an acid and after losing a proton, it forms SO4{2-} which is a conjugate base.
HSO4- + H+ --> H2SO4
And, HSO4- is gaining a proton, thus it is considered as a base and after gaining a proton, it forms H2SO4 which is a conjugate acid.
d) NH3 → NH2- + H+
Here, NH3 is loosing a proton, thus it is considered as an acid and after losing a proton, it forms NH2- which is a conjugate base.
NH3 + H+ --> NH4+
And, NH3 is gaining a proton, thus it is considered as a base and after gaining a proton, it forms NH4+ which is a conjugate acid.
Thanks and Regards
