Enthalpy of neutralization is always a constant when a strong acid is neutralized by a strong base: account for the statement.

Explanation

Strong acids and strong bases exist in the fully ionised form in aqueous solution as below:
`H_(3)O^(+)+Cl^(-)+Na^(+)+OH^(-)rarrNa^(+)+Cl+2H_(2)O`
(or)
`H_(3)O_((aq))^(+)+OH_((aq))^(-)rarr2H_(2)O(1)^(@)`
`DeltaH^(@)=-57.32KJ.`
The `H^(+)` ions produced in water by the acid molecules exist as `H_(3)O^(+)` Thus enthalpy change change of neutralization is essentially due to enthalpy change per mole of water formed from `H_(3)O^(+) and OH-`. Therefore, irrespective of the chemical natural. the enthalpy of neutralization of the strong acid by Strong base is a constant value which is equal to -57 . 32 kJ.