question_answer 14)

The species: \[{{H}_{2}}O,HCO_{3}^{-},HSO_{4}^{-},N{{H}_{3}}\]can act both as Bronsted acids and bases. For each case give the corresponding conjugate acid and conjugate base.

Answer:

\[\mathbf{Acid-}{{\mathbf{H}}^{\mathbf{-}}}\to \mathbf{Conjugatebase}\] \[{{H}_{2}}O-{{H}^{+}}\to O{{H}^{-}}\] \[HCO_{3}^{-}-{{H}^{+}}\to CO_{3}^{2-}\] \[HSO_{4}^{-}-{{H}^{+}}\to SO_{4}^{2-}\] \[N{{H}_{3}}-{{H}^{+}}\to NH_{2}^{-}\] \[\mathbf{Base+}{{\mathbf{H}}^{\mathbf{+}}}\to \mathbf{Conjugateacid}\] \[{{H}_{2}}O-{{H}^{+}}\to O{{H}^{-}}\] \[HCO_{3}^{-}-{{H}^{+}}\to {{H}_{2}}C{{O}_{3}}\] \[HSO_{4}^{-}+{{H}^{+}}\to {{H}_{2}}S{{O}_{4}}\] \[N{{H}_{3}}+{{H}^{+}}\to NH_{4}^{+}\]