For the species HSO_4^{-} and NH_3,their conj | vedclass

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(C) According to the Bronsted-Lowry theory,a conjugate acid is formed when a base accepts a proton $(H^{+})$. To find the conjugate acid of a species,

Vedclass · Accepted Answer

$H_2SO_4$ and $NH_4^{+}$

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(C) According to the Bronsted-Lowry theory,a conjugate acid is formed when a base accepts a proton $(H^{+})$. To find the conjugate acid of a species,we add one $H^{+}$ ion to it. For $HSO_4^{-}$,adding $H^{+}$ gives $H_2SO_4$. For $NH_3$,adding $H^{+}$ gives $NH_4^{+}$. Therefore,the conjugate acids are $H_2SO_4$ and $NH_4^{+}$. Thus,the correct option is $C$.

For the species $HSO_4^{-}$ and $NH_3$,their conjugate acids respectively are

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