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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:

1. bronsted acid
2. bronsted base
3. conjugate acid
4. conjugate base

Correct answer: conjugate base

Solution

H2PO4− transfers a proton to water, so it acts as an acid in the forward reaction. After losing H+, it becomes HPO4^2−, which is the conjugate base of H2PO4−.

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