Assertion :HClO is stronger acid than HBrO. Reason: Greater is the electronegativity of the halogen, greater will be attraction of electron pair towards it and hence more easily the $H^{+}$ ion will be released.

Both Assertion and Reason are correct and Reason is the correct explanation for Assertion

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Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion

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Assertion is correct but Reason is incorrect

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Both Assertion and Reason are incorrect

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Solution

The correct option is A Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
HClO is stronger acid than HBrO.
Greater is the electronegativity and smaller is the size of the halogen, greater will be attraction of electron pair towards it and hence more easily the $H^{+}$ ion will be released.

Cl is more electronegative (and smaller in size) than Br. Hence, the tendency of Cl to withdraw electrons from Cl-O-H bond is higher than the tendency of Br to withdraw electrons from Br-O-H bond.
This is because, the inductive effect of Cl is higher than the inductive effect of Br. Thus, O-H bond in HClO breaks more easily than H-O bond in HBrO. Hence, HClO is more acidic than HBrO.

Hence, both Assertion and Reason are correct and Reason is the correct explanation for Assertion.

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Assertion :HClO is stronger acid than HBrO. Reason: Greater is the electronegativity of the halogen, greater will be attraction of electron pair towards it and hence more easily the H+ ion will be released.

Assertion :HClO is stronger acid than HBrO. Reason: Greater is the electronegativity of the halogen, greater will be attraction of electron pair towards it and hence more easily the $H^{+}$ ion will be released.