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)rarrH_(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 neutralized, the 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_("neutralization")^(@)=DeltaH_("ionization")^(@)+Delta_(r )H^(@)(H^(+)+OH^(-)rarrH_(2)O)`
If enthalpy of neutralization of `CH_(3)COOH` by HCl is -49.86 kJ/mol then enthalpy of ionization of `CH_(3)COOH` is :

Options

A. If both the statements are TRUE and STATEMENT-2 is the correct explanation of STATEMENT-1
B. If both the statements are TRUE but STATEMENT-2 is NOT the correct explanation of STATEMENT-15
C. If STATEMENT-1 is TRUE and STATEMENT-2 is FALSE
D. If STATEMENT-1 is FALSE and STATEMENT-2 is TRUE

Answer

A