Which statement correctly explains why H2S is a stronger acid than water?(1 point)

Question

Responses

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.
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 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–.

Answer 1

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

Answer 2

You know that water can act as an acid to form OH−. H2S is also an acid that can lose an H+ to form the conjugate base HS−. To determine which is the stronger acid, you need to look at the strength of the conjugate bases. Sulfur (S) and oxygen (O) are in the same group, but sulfur has a larger atomic size. Therefore, HS− is a more stable, weaker base than OH−. Since strong acids form weaker conjugate bases, H2S is a stronger acid than water.

Answer 3

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