A) \[HBr{{O}_{4}}\]
B) \[HOCl\]
C) \[HN{{O}_{2}}\]
D) \[{{H}_{3}}P{{O}_{3}}\]
Correct Answer: A
Solution :
Key Idea: The strength ofoxy acid depends on the oxidation state of central atom. Greater the oxidation state of central atom more will be its strength. So calculate the oxidation state of central atom in each of the oxy acids to find which one of them is strongest. [a] \[HBr{{O}_{4}}\] Let oxidation state of \[Br=x\] \[\therefore \] \[1+x+(-2+4)=0\] or \[x=+7\] [b] \[HOCl\] Let oxidation state of \[Cl=x\] \[\therefore \] \[+1+(-2)+x=0\] or \[x=+1\] [c] \[HN{{O}_{2}}\] Let oxidation state of \[O=x\] \[\therefore \] \[+1+x+(-2\times 2)=0\] or \[x=+3\] [d] \[{{H}_{3}}P{{O}_{3}}\] Let oxidation state of \[P=x\] \[\therefore \] \[+1\times 3+x+(-2\times 3)=0\] or \[3+x-6=0\] \[\therefore \] \[x=3\] \[\because \] The oxidation state of Br is highest among the given oxyacids. \[\therefore \] \[HBr{{O}_{4}}\] is the strongest acid.
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