For the reaction NH_4^+ + S^{2-} rightlefthar | vedclass

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(C) According to the Brønsted-Lowry theory,an acid is a proton $(H^+)$ donor and a base is a proton acceptor.In the reaction $NH_4^+ + S^{2-} \rightle

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Conjugate acid-base pair

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(C) According to the Brønsted-Lowry theory,an acid is a proton $(H^+)$ donor and a base is a proton acceptor.In the reaction $NH_4^+ + S^{2-} \rightleftharpoons NH_3 + HS^-$,$NH_4^+$ acts as an acid by donating a proton to $S^{2-}$.$NH_3$ is the conjugate base of the acid $NH_4^+$.$HS^-$ is the conjugate acid of the base $S^{2-}$.Therefore,$NH_3$ and $HS^-$ represent a conjugate acid-base pair.

For the reaction $NH_4^+ + S^{2-} \rightleftharpoons NH_3 + HS^-$,identify the nature of $NH_3$ and $HS^-$ in the context of the Brønsted-Lowry theory.

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