Give the conjugate acid of the following species: $HS^{-}, NH_{3}, C_{6}H_{5}COO^{-}, OH^{-}$
The conjugate acid is formed by adding a proton $(H^{+})$ to the given base.
$1$. For $HS^{-}$,the conjugate acid is $HS^{-} + H^{+} \rightarrow H_{2}S$.
$2$. For $NH_{3}$,the conjugate acid is $NH_{3} + H^{+} \rightarrow NH_{4}^{+}$.
$3$. For $C_{6}H_{5}COO^{-}$,the conjugate acid is $C_{6}H_{5}COO^{-} + H^{+} \rightarrow C_{6}H_{5}COOH$.
$4$. For $OH^{-}$,the conjugate acid is $OH^{-} + H^{+} \rightarrow H_{2}O$.
Therefore,the conjugate acids are $H_{2}S, NH_{4}^{+}, C_{6}H_{5}COOH, H_{2}O$.
$1$. For $HS^{-}$,the conjugate acid is $HS^{-} + H^{+} \rightarrow H_{2}S$.
$2$. For $NH_{3}$,the conjugate acid is $NH_{3} + H^{+} \rightarrow NH_{4}^{+}$.
$3$. For $C_{6}H_{5}COO^{-}$,the conjugate acid is $C_{6}H_{5}COO^{-} + H^{+} \rightarrow C_{6}H_{5}COOH$.
$4$. For $OH^{-}$,the conjugate acid is $OH^{-} + H^{+} \rightarrow H_{2}O$.
Therefore,the conjugate acids are $H_{2}S, NH_{4}^{+}, C_{6}H_{5}COOH, H_{2}O$.
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