To solve this problem, we need to analyze both statements regarding acid strength.$\\$Statement I:$\\$The acid strength increases in the order $HF << HCl << HBr << HI. \\$Statement II:$\\$As the size of the elements F, Cl, Br, I increases down the group, the bond strength of$\\ HF, HCl, HBr,$ and $HI$ decreases and so the acid strength increases.$\\$Let's analyze these statements:$\\$• Acid strength is determined by the ability of the acid to donate a proton (H$^+$).$\\$• For hydrogen halides (HX), the bond strength between H and X is crucial.$\\$• As we move down the group from F to I, the size of the halogen atom increases.$\\$• Larger atoms form weaker H-X bonds because the bond length increases, making it easier$\\$ for the acid to donate a proton.$\\$Therefore, the bond strength decreases in the order:$\\ HF > HCl > HBr > HI \\$This means the acid strength increases in the order:$\\ HF << HCl << HBr << HI \\$• Statement I is correct as it reflects the correct order of acid strength.$\\$• Statement II is also correct because it explains the reason for the increase in acid strength$\\$ down the group due to decreasing bond strength.$\\$Thus, both Statement I and Statement II are true.$\\$The correct answer is Option 1: Both Statement I and Statement II are true.