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

A. Sulfur(S) has a larger atomic size than oxygen (O), so H2S is a more stable, stronger acid than H2O
B. Sulfur (S) has a larger atomic size than oxygen (O), so H2S is a more stable, weaker base than H20
C. Sulfur (S) has a larger atomic size than oxygen (O), so HS- is a more stable, weaker base than OH-
D. Sulfur (S) has a larger atomic size than oxygen (O), so HS- is more stable, stronger acid than OH-

1 answer

The correct statement that explains why H2S is a stronger acid than water (H2O) is:

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

Here's the reasoning: When H2S donates a proton (H+), it forms HS-. The larger size of sulfur compared to oxygen allows the negative charge on HS- to be more effectively stabilized. This makes HS- a weaker base than OH-, which means that H2S is a stronger acid compared to water. A weaker conjugate base (HS-) indicates that the acid (H2S) is stronger.

Remember, stronger acids have weaker conjugate bases. Since OH- is a stronger base compared to HS-, this supports the conclusion that H2S is a stronger acid than water.