Answer:-

1. The acetate ion, which is the conjugate base of acetic acid, becomes less stable due to the electron-donating (+ I) effect of the methyl (-CH3) group.

2. The weaker the stabilization of the conjugate base, the weaker the acid itself becomes.

3. In the case of the formate ion, there is no destabilization effect caused by the presence of a methyl group.

4. Therefore, formic acid is stronger in acidity compared to acetic acid because it does not experience the destabilizing influence of the methyl group on its conjugate base.