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Which of the following gives the correct order of acidic strength?

1. HOF > HOCl > HOBr > HOI
2. HClO4 > HBrO4 > HIO4
3. LiOH < Be(OH)2 < B(OH)3 < H2CO3
4. All of the above

Correct answer: All of the above

Solution

Option A: For hypohalous acids HOX, as electronegativity of X decreases (F > Cl > Br > I), the O-H bond becomes weaker (less electron withdrawal from X), so acidity decreases. HOF > HOCl > HOBr > HOI. Correct. Option B: HClO4, HBrO4, HIO4 - all are the strongest oxoacids of respective halogens. Going down group 17, central atom size increases, the O-H bond strength increases relative to element-oxygen bond; acidity of highest oxoacids decreases down the group. HClO4 > HBrO4 > HIO4. Correct. Option C: LiOH is a strong base, Be(OH)2 is amphoteric (weakly basic), B(OH)3 is a weak acid, H2CO3 is a stronger acid. So acidity order: LiOH < Be(OH)2 < B(OH)3 < H2CO3. Correct. All three are correct, so answer is All of the above.

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