A) \[PO_{4}^{3-}\]
B) PRs
C) \[{{H}_{3}}P{{O}_{4}}\]
D) \[HPO_{4}^{2-}\]
Correct Answer: D
Solution :
\[{{H}_{3}}P{{O}_{4}}\]is a tribasic acid, thus ionising in three steps: I. \[{{H}_{3}}P{{O}_{4}}{{H}^{+}}+{{H}_{2}}PO_{4}^{-}\] II. \[{{H}_{2}}PO_{4}^{-}{{H}^{+}}+HPO_{4}^{2-}\] III. \[HPO_{4}^{2-}{{H}^{+}}+PO_{4}^{3-}\] Conjugate base is formed when an acid loses its proton. Thus\[HPO_{4}^{2-}\]is the conjugate base of \[{{H}_{2}}PO_{4}^{2-}\](which is an acid in step II, but is the conjugate base of\[{{H}_{3}}P{{O}_{4}}\]in step I).
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