Enthalpy of neutralization is defined as the enthalpy change when 1 mole of acid/base is completely neutralized by base/acid in dilute solution. For strong acid and strong base neutralization net chemical change is `H_((aq))^(+) + OH_((aq))^(-) rarr H_(2)O_((l)), Delta H_(r )^(0) -= - 55.84 kJ//mol`
What is `Delta H^(0)` for complete neutralisation of strong diacidic base `A(OH)_(2) " by " HNO_(3)`?

Options

A. `-55.84 kJ`
B. `-111.68kJ`
C. 55.84 kJ/mol
D. none of these

Answer

B

Explanation

For strong base with strong acid, `-55.84 rarr1` eq
diacidic `rArr` 2eq `=2 xx (-55.84) = - 111.68kJ`