Question

Which statement correctly explains why H2S is a stronger acid than H2O ?(1 point)ResponsesSulfur (S) has a larger atomic size than oxygen (O), and the HS− conjugate base is stronger than the OH− conjugate base.Sulfur ( S ) has a larger atomic size than oxygen ( O ), and the H S raised to the negative power conjugate base is stronger than the O H raised to the negative power conjugate base.Sulfur (S) has a smaller atomic size than oxygen (O), so H2S partly dissociates while H2O does not dissociate.Sulfur ( S ) has a smaller atomic size than oxygen ( O ), so H sub 2 S partly dissociates while H sub 2 O does not dissociate.Sulfur (S) has a smaller atomic size than oxygen (O), so H2S completely dissociates while H2O does not dissociate.Sulfur ( S ) has a smaller atomic size than oxygen ( O ), so H sub 2 S completely dissociates while H sub 2 O does not dissociate.Sulfur (S) has a larger atomic size than oxygen (O), and the HS− conjugate base is weaker than the OH− conjugate base.Sulfur ( S ) has a larger atomic size than oxygen ( O ), and the H S raised to the negative power conjugate base is weaker than the O H raised to the negative power conjugate base.

Answer 1

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

Sulfur (S) has a larger atomic size than oxygen (O), and the HS⁻ conjugate base is stronger than the OH⁻ conjugate base.

This is because the larger atomic size of sulfur results in a weaker bond between the hydrogen and sulfur in H₂S compared to the bond in H₂O. As a result, H₂S can donate its proton (H⁺) more easily, making it a stronger acid, while the HS⁻ conjugate base is relatively stable compared to the more basic OH⁻ conjugate base. Therefore, this difference in size and the stability of the conjugate bases accounts for H₂S's increased acidity.