Question

Which statement correctly explains why H2S is a stronger acid than water?





(1 point)
Responses

Sulfur (S) has a larger atomic size than oxygen (O), so HS– is a more stable, stronger acid than OH–.
Sulfur (S) has a larger atomic size than oxygen (O), so HS – is a more stable, stronger acid than OH – .

Sulfur (S) has a larger atomic size than oxygen (O), so HS– is a more stable, weaker base than OH–.
Sulfur (S) has a larger atomic size than oxygen (O), so HS – is a more stable, weaker base than OH – .

Sulfur (S) has a larger atomic size than oxygen (O), so H2S is a more stable, weaker base than H2O.
Sulfur (S) has a larger atomic size than oxygen (O), so H 2 S is a more stable, weaker base than H 2 O.

Sulfur (S) has a larger atomic size than oxygen (O), so H2S is a more stable, stronger acid than H2O.
Sulfur (S) has a larger atomic size than oxygen (O), so H 2 S is a more stable, stronger acid than H 2 O.
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Answer 1

"Sulfur (S) has a larger atomic size than oxygen (O), so HS– is a more stable, weaker base than OH–."

Reason: The larger S atom spreads the negative charge in HS– over a bigger volume, stabilizing the conjugate base (making it a weaker base), so H2S donates H+ more readily than H2O.