HCOOH, also known as formic acid, is an organic acid with the chemical formula CH2O2. To predict its acidity or basicity, we can examine its molecular structure and use relevant chemical principles, such as the Bronsted-Lowry theory and resonance stabilization.According to the Bronsted-Lowry theory, an acid is a substance that donates a proton H+ , while a base is a substance that accepts a proton. In the case of HCOOH, the molecule has a hydrogen atom bonded to an oxygen atom, which is part of a hydroxyl group -OH . This hydrogen atom can be easily donated as a proton, making HCOOH an acidic molecule.The acidity of HCOOH can also be explained by the resonance stabilization of its conjugate base. When HCOOH donates a proton, it forms the formate ion HCOO- as its conjugate base. The negative charge on the oxygen atom in the formate ion can be delocalized through resonance, which stabilizes the ion. This stabilization of the conjugate base contributes to the acidity of HCOOH.Furthermore, the electronegativity of the oxygen atom in the hydroxyl group also plays a role in the acidity of HCOOH. Oxygen is highly electronegative, meaning it attracts electrons towards itself. This electron-withdrawing effect weakens the O-H bond in the hydroxyl group, making it easier for the hydrogen atom to be donated as a proton.In summary, HCOOH is predicted to be acidic due to its ability to donate a proton, the resonance stabilization of its conjugate base, and the electronegativity of the oxygen atom in the hydroxyl group. These factors contribute to the molecule's acidic properties and justify the prediction based on relevant chemical principles.