Which is the set of amphiprotic species?

H_{3} O^{+}, H P O_{4}^{2 -}, H C O_{3}^{-}

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H_{2} O, H P O_{3}^{2 -}, H_{2} P O_{2}^{-}

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H_{2} P O_{4}^{-}, H_{2} P O_{3}^{-}, H_{2} O

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All of these

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Solution

The correct option is C $H_{2} P O_{4}^{-}, H_{2} P O_{3}^{-}, H_{2} O$
A species that has the potential to act both as an acid by donating $H^{+}$ and as a base by accepting $H^{+}$ according to bronsted - lowry theory is said to be amphiprotic.
$H_{3} O^{+}$ can't accept $H^{+}$ more. So it can't act as base. Consequently aren't considered as amphiprotic species.
$H P O_{3}^{- 2}$ and $H_{2} P O_{2}^{-}$ can't donate $H^{+}$ any more. So, they can't act as acid and consequently aren't considered as amphiprotic species.

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Similar questions

H_{2} P O_{4}^{-}

H_{2} P O_{3}^{-}

H P O_{4}^{2 -}

H P O_{3}^{2 -}

C l O^{-}

C l O_{2}^{-}

N H_{3}

N H_{2}^{-}

H_{2} P O_{2}^{-}, H P O_{3}^{2 -}, H_{2} P_{2} O_{7}^{2 -}

Identify Bronsted acids in the reaction : $H_{2} C O_{3} + H P O_{4}^{2 -} ⇌ H_{2} P O_{4}^{-} + H C O_{3}^{-}$

N a H C O_{3}

H^{+}

O H^{-} i o n

H C O_{3}^{-} + H_{2} O i o n i z a t i o n ⇋ C O_{3}^{2 -} + H_{2} O

H C O_{3}^{-} + H_{2} O i o n i z a t i o n ⇋ H_{2} C O_{3} + O H^{-}

H C l O_{4}

H C O_{3}^{-}

H P O_{4}^{2 -}

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