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Consider the ionic reaction, ${HC}_{2} O_{4}^{-} + {PO}_{4}^{- 3} ⇌ {HPO}_{4}^{2 -} + C_{2} O_{4}^{2 -} .$ Identify the incorrect statement(s)

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The above equilibrium mixture can act as a buffer (both acids have nearly the same dissociation constant)

$H C_{2} O_{4}^{-}$ And $C_{2} O_{4}^{- 2}$ are conjugate acid-base pairs

The P – O bond order in $P O_{4}^{- 3}$ is 1.75

The C – O bond order in $C_{2} O_{4}^{2 -}$ is 1.50

answer is C.

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Detailed Solution

Solution of weak acid and it’s salt acts as buffer.

${_{a c i d}^{H C_{2} O_{4}^{-}} +}_{b a s e}^{P O_{4}^{- 3}} ⇌_{C . A}^{H P O_{4}^{- 2}} +_{C . B}^{C_{2} O_{4}^{- 2}}$
$B . O = \frac{n o . o f b o n d}{n o . o f R . S} P O 4^{3 -} B . O = 1.25$

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