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_(r)H^(@) = -55.84 KJ//mol` `DeltaH_("ionization")^(@)` of aqueous solution of strong acid and strong base is zero. When a dilute solution of a weak acid or base is neutalized, teh enthalpy of neutralization is some what less because of the absorption of heat in the ionization of the weak acid or base, for weak acid/base `DeltaH_("neutrilization")^(2) = DeltaH_("ionization")^(@) + Delta_(r)H^(@) " " (H^(+) + OH^(-) rarr H_(2)O)` Under the same condition how many mL of `0.1` M NaOH and `0.05` M `H_(2)`A (strong diprotic acid) solution should be mixed for a total volume of `100` mL produce the highest rise in temperature:A. `25:75`B. `50:50`C. `75:25`D. `66.66:33.33`