Which of the following is not a conjugate acid- base pair?

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$[HP {O_{3}}^{2-}, P {O_{3}}^{3 -}]$

$[H_{2} P {O_{4}}^{-}, P {O_{4}}^{3 -}]$

$[H_{2} P {O_{4}}^{-}, HP {O_{4}}^{2 -}]$

$[H_{2} P {O_{4}}^{-}, H_{3} {PO}_{4}]$

answer is D.

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Detailed Solution

A conjugate acid-base pair, according to the Bronsted-Lowry definition of acids and bases, consists of two substances that are unique only in that they contain a proton (H⁺). When a proton is supplied to a base, a conjugate acid is formed, and vice versa when a proton is taken away from an acid, a conjugate base is formed.

Due to its two-proton difference, the acid-base pair $[H_{2} P {O_{4}}^{-}, P {O_{4}}^{3 -}]$ is not conjugate.

Only one proton separates a conjugate acid-base pair from another. For example, the only proton that separates HCl and Cl- ion. They are the conjugate acid-base pair.

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