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Chemistry · Various concepts of acids and bases (Arrhenius, Bronsted Lowry and Lewis) and their ionization, acid-base equilibria (including multistage ionization) and ionization constants

In the reaction, = \) +\boldsymbol{H} \boldsymbol{P} \boldsymbol{O}_{4}^{2-}(l)

In the reaction, \( \boldsymbol{H}_{2} \boldsymbol{P} \boldsymbol{O}_{4}^{-}+\boldsymbol{H}_{2} \boldsymbol{O}(l)= \) \( \boldsymbol{H}_{3} \boldsymbol{O}^{+}(\boldsymbol{l})+\boldsymbol{H} \boldsymbol{P} \boldsymbol{O}_{4}^{2-}(l) \) the hydrogen phosphate ion is the:

  • A. bronsted acid
  • B. bronsted base
  • C. conjugate acid
  • D. conjugate base

Step-by-step solution

In the reaction H2PO4- + H2O → H3O+ + HPO4^2-, H2PO4- donates a proton to H2O, making it the acid. After losing a proton, H2PO4- becomes HPO4^2-, which is the conjugate base of H2PO4-.
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