Respuesta :
Answer : The option (c) is not a conjugate acid-base pair.
Explanation :
According to the Bronsted Lowry concept, Bronsted Lowry-acid is a substance that donates one or more hydrogen ion in a reaction and Bronsted Lowry-base is a substance that accepts one or more hydrogen ion in a reaction.
Or we can say that, conjugate acid is proton donor and conjugate base is proton acceptor.
(a) The equilibrium reaction will be,
[tex]HOCl+H_2O\rightleftharpoons OCl^-+H_3O^+[/tex]
In this reaction, [tex]HOCl/OCl^-[/tex] are act as a conjugate acid-base pair.
(b) The equilibrium reaction will be,
[tex]HNO_2+H_2O\rightleftharpoons NO_2^-+H_3O^+[/tex]
In this reaction, [tex]HNO_2/NO_2^-[/tex] are act as a conjugate acid-base pair.
(c) The equilibrium reaction will be,
[tex]O^{2-}+H_2O\rightleftharpoons OH^-+OH^-[/tex]
In this reaction, [tex]O^{2-}/OH^-[/tex] are not act as a conjugate acid-base pair.
(d) The equilibrium reaction will be,
[tex]HSO_4^-+H_2O\rightleftharpoons SO_4^{2-}+H_3O^+[/tex]
In this reaction, [tex]HSO_4^-/SO_4^{2-}[/tex] are act as a conjugate acid-base pair.
(e) The equilibrium reaction will be,
[tex]H_2CO_3+H_2O\rightleftharpoons HCO_3^{-}+H_3O^+[/tex]
In this reaction, [tex]H_2CO_3/HCO_3^{-}[/tex] are act as a conjugate acid-base pair.
Hence, from this we conclude that, the option (c) is not a conjugate acid-base pair but it is a act as conjugate base-acid pair.
