A) \[HSO_{4}^{-}\]
B) \[N{{a}_{2}}C{{O}_{3}}\]
C) \[N{{H}_{3}}\]
D) \[O{{H}^{-}}\]
Correct Answer: A
Solution :
Bronsted acids have a tendency to donate proton while Bronsted base have a tendency of accepting protons. \[\because \] \[HSO_{4}^{-}\] can accept proton to form \[{{H}_{2}}S{{O}_{4}}\]and also give a proton to form \[SO_{4}^{2-},\] therefore it behaves like both Bronsted acid and Bronsted base.
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