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Statement-I : The enthalpy of neutraliza...

Statement-I : The enthalpy of neutralization of the reaction between `HCl` and `NaOH` is `-13.7` kCal/mol. If the enthalpy of neutralization of oxalic acid `(H_(2)C_(2)O_(4))` by a strong base is `-25.4` kCal/mol, then the enthalpy change `(|Delta_(r)H|)` of the process `H_(2)C_(2)O_(4) rarr 2H^(+)+C_(2)O_(4)^(2-)` is `11.7` kCal/mol.
Statement-II : `H_(2)C_(2)O_(4)` is a weak acid.

A

If both Statement-I & Statement-II are True & the Statement-II is a correct explanation of the Statement-I

B

If both Statement-I & Statement-II are True but Statement-II is not a correct explanation of the Statement-I

C

If statement-I is True but the Statement-II is False.

D

If Statement-I is False but the Satement-II is True

Text Solution

Verified by Experts

The correct Answer is:
D
`H^(+)+OH^(-) =13.7`
`2H^(+)+2OH^(-) rarr H_(2)O=27.4`
But energy released `=25.4`
`:. H_(1)C_(2)O_(4) rarr 2H^(+) +C_(2)O_(4)^(-2)" "DeltaH=2" kCal/mol."`
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