When acids an bases react they liberate some amount of energy which is represented as `DeltaH` neutralization if one equivalent of acid and base reacts. The energy liberated depends on the concentration of acid and base and also on whether the acid is strong or weak. For strong acids and bases, the value is constant and for weaker acids as bases the magnitude is generally lesser.
Using this info and the date below answer the question that follow :
[Given data :
`Delta_("neutralization")HCl//NaOH = - 14 Kcal//eq` (at infinite dil.)
`DeltaH_("ionisation")CH_(3)COOH = 2kcal//mol`
`DeltaH_("ionisation")NH_(4)OH = 3kcal//eq]`
Which of the following option(s) is//are correct assuming weak acids/bases to be completely unionized ?

Options

A. `DeltaH_("neutralization")H_(2)SO_(4)//NaOH = -28 kcal//"mole"` of `H_(2)SO_(4)`
B. `DeltaH_("neutralization")HCl//NH_(4)OH = -11kcal//"mole"` of `HCl`
C. `DeltaH_("neutralization")CH_(3)COOH//NH_(4)OH = - 9kcal//"mole"` of `CH_(3)COOH`
D. `DeltaH_("neutralization")KOH//CH_(3)COOH = - 11 kcal//"mole"` of `KOH`

Answer

a,b,c