To determine the acidity order of diprotic acids $(H_2S, H_2Se, H_2Te)$ in aqueous solutions,$\\$we need to consider the trend in acidity down the group in the periodic table.$\\$• These acids belong to Group 16 (chalcogens) and their acidity is influenced by the$\\$bond strength between hydrogen and the chalcogen.$\\$• As we move down the group from sulfur (S) to tellurium (Te), the size of the chalcogen$\\$atom increases, leading to weaker H-X bonds.$\\$• Weaker H-X bonds result in easier release of $H^+$ ions, thus increasing acidity.$\\$Therefore, the acidity order is determined by the ease of dissociation of the H-X bond:$\\$H$_2$S$<$H$_2$Se$<$H$_2$Te$\\$This corresponds to Option 1.$\\$In summary, the correct order of acidity is:$\\$H$_2$S$<$H$_2$Se$<$H$_2$Te$\\$This is because the bond strength decreases as the size of the chalcogen increases,$\\$making it easier for the acid to donate $H^+$ ions.