Question Which statement correctly explains why H2S is a stronger acid than H2O?(1 point) Responses 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 H2S is a more stable, weaker base than H2O 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- Sulfer (S) has a larger atomic size than oxygen (O), so H2S is a more stable, stronger acid than H2O
1 answer
The correct statement is: "Sulfur (S) has a larger atomic size than oxygen (O), so HS- is a more stable, stronger acid than OH-."
This statement captures the relationship between atomic size, conjugate base stability, and acid strength. In general, larger atoms can better stabilize negative charges, which applies to the HS⁻ ion compared to OH⁻. Consequently, H₂S is a stronger acid than H₂O because its conjugate base (HS⁻) is more stable than the conjugate base of water (OH⁻).
