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Reactivity Trends (Group 2)

Which is stro...

Question

Which is stronger base in the given pair?
$H {S O}_{4}^{-}, H {S O}_{3}^{-}$

H {S O}_{3}^{-}

H {S O}_{4}^{-}

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H {S O}_{3}^{-}

H {S O}_{4}^{-}

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H {S O}_{3}^{-}

H {S O}_{4}^{-}

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None of these

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Solution

The correct option is A $H {S O}_{3}^{-}$ > $H {S O}_{4}^{-}$
$H_{2} {S O}_{4}$ contains more number of electronegative oxygen atoms than $H_{2} {S O}_{3}$ .
Due to this, the negative charge (obtained due to dissociation of proton) is more stabilized in $H {S O}_{4}^{-}$ than in $H {S O}_{3}^{-}$ .
Hence, the correct order of the acid strength is $H_{2} {S O}_{3} < H_{2} {S O}_{4}$ .
Now, the conjugate base of strong acid is weaker base.
The correct order of basicity is $H {S O}_{3}^{-} > H {S O}_{4}^{-}$ .

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