H2SO4, also known as sulfuric acid, is a strong acid. To predict its acidity, we can look at its molecular structure and its ability to donate protons H+ ions in an aqueous solution.Molecular structure:H2SO4 has the following structure:O||S - OH|O - HThe sulfur atom is bonded to four oxygen atoms, two of which are hydroxyl groups OH . The sulfur atom is in the +6 oxidation state, which creates a highly polarized bond between the sulfur and the oxygen atoms. This polarization makes it easier for the hydroxyl groups to donate protons H+ ions to the solution.Acidity:In an aqueous solution, H2SO4 can donate two protons H+ ions in a stepwise manner, making it a strong diprotic acid. The dissociation reactions are as follows:1 H2SO4 aq H+ aq + HSO4- aq 2 HSO4- aq H+ aq + SO42- aq The first dissociation is a strong reaction, meaning it occurs readily and almost completely. The second dissociation is weaker, but still significant. The dissociation constants Ka for these reactions are:Ka1 for the first dissociation 10^3Ka2 for the second dissociation 10^-2Since the Ka values are greater than 1, this indicates that H2SO4 is a strong acid.In conclusion, H2SO4 is a strong diprotic acid due to its molecular structure and its ability to donate two protons H+ ions in an aqueous solution. Its acidity is supported by the high Ka values for its dissociation reactions.