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Oxyacids of Phosphorus

What is the c...

Question

What is the conjugate base in this reaction?

$H_{2} S_{(g)} + {H_{2} O}_{(l)} ⇌ {H_{3} O}_{(a q)}^{+} + {H S^{-}}_{(a q)}$

H_{2} S

; donating a proton

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H_{2} O

; donating a proton

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H_{3} O^{+}

; donating a proton

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H S^{-}

; accepting a proton

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Solution

The correct option is A $H_{2} S$ ; donating a proton
A conjugate base is formed when an acid loses a proton $(H^{+})$ .

In the given reaction,

$H_{2} S_{(g)} + H_{2} O_{(l)} ⇋ H_{3} O_{(a q)}^{+} + H S_{(a q)}^{-}$

The acid $H_{2} S$ loses a proton to give $H S^{-}$ .

Hence, $H S^{-}$ is the conjugate base of acid $H_{2} S$ .

Further, this base accepts a proton in backward reaction.

Hence, the correct option is $A$

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