A) \[HCl{{O}_{4}}\]
B) \[HI{{O}_{3}}\]
C) \[HN{{O}_{3}}\]
D) \[HBr{{O}_{4}}\]
Correct Answer: A
Solution :
Key Idea Higher the oxidation number of a non-metal more will be its acidic nature, moreover, acidic character of oxy adds decrease along a group and increase along a period. In \[HCl{{O}_{4}}\] the O.N. of Cl is +7. In \[HI{{O}_{3}}\] the O.N. of iodine is +5. In \[HN{{O}_{3}}\] the O.N. of nitrogen is +5. In \[HBr{{O}_{4}}\] the O.N. of bromine is +7. The oxidation number of chlorine and bromine in \[HCl{{O}_{4}}\] and \[HBr{{O}_{4}}\] is same but acidic character of oxyacids decrease along a group. So, \[HCl{{O}_{4}}\] is stronger than \[HBr{{O}_{4}}\]. Further, the oxidation number of iodine and nitrogen is less than chlorine therefore, \[HCl{{O}_{4}}\] is the strongest acid.
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