The correct explanation for 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 weaker than the OH− conjugate base.
This is because the larger atomic size of sulfur allows the H-S bond to be weaker than the H-O bond in water, making it easier for H2S to donate a proton (H+) and therefore behave as a stronger acid. Additionally, the conjugate base HS− is weaker compared to OH−, which is consistent with the trend that weaker conjugate bases correspond to stronger acids.