H2SO4, also known as sulfuric acid, is a strong acid. Its acidity can be predicted based on its chemical structure and bonding.Sulfuric acid consists of a central sulfur atom S bonded to four oxygen atoms O and two hydrogen atoms H . The sulfur atom is double-bonded to two oxygen atoms and single-bonded to the other two oxygen atoms. The two single-bonded oxygen atoms are each bonded to one hydrogen atom, forming two OH groups.The acidity of H2SO4 is due to the presence of these two OH groups. In an aqueous solution, sulfuric acid can donate protons H+ to water molecules, forming hydronium ions H3O+ and sulfate ions SO4^2- . The ability to donate protons is a characteristic of acidic substances. The chemical equation for this reaction is:H2SO4 + 2H2O 2H3O+ + SO4^2-The first proton dissociation is almost complete, making H2SO4 a strong acid. The second proton dissociation is also significant, but not as complete as the first one. This means that sulfuric acid is a strong diprotic acid, meaning it can donate two protons per molecule.The chemical bonding in H2SO4 that leads to its acidic behavior can be explained by the presence of polar O-H bonds in the molecule. The oxygen atom is more electronegative than the hydrogen atom, resulting in a polar bond with a partial negative charge on the oxygen atom and a partial positive charge on the hydrogen atom. This polarity allows the hydrogen atom to be easily donated as a proton H+ to a water molecule or another base.In summary, H2SO4 is a strong acid due to its ability to donate two protons per molecule. The chemical bonding present in the molecule, specifically the polar O-H bonds, allows for the easy donation of protons, leading to its acidic behavior.