Why is heat of neutralisation for a strong acid and strong base constant ?

The heat of neutralization for a strong acid by a strong base is a constant

What is Arrhenius concept of acids and bases ? On the basis of this concept explain why heat of neutralisation for a strong acid and a strong base is always constant.

Why is the heat of neutralization of a strong acid by a strong base is constant as 57.0 kJ/mole?

The heat of neutralization of a strong acid by a strong base is a constant because :

The heat of neutralisation for strong acid and strong base forming 2 moles of water is

Heat of neutralization of strong acid against strong base is constant and is equal to

The heat of neutralization of any strong acid and a strong base is nearly equal to :

Statement-1 : Chemical equation H^(+)(aq) + OH^(-)(aq) rarr H_(2)O(I), Delta H = -X kJ represents the enthalpy of formation of water And Statement-2 : Delta H_("neutralisation") of strong acid and strong base is constant.

Statement-1 : Neutralisation reaction is an Endothermic Process. Statement-2 : Standard Enthalpy of Neutralisation for different pairs of strong acid and strong base are different. Statement-3 : Standard Enthalpy of Neutralisation for a pair of strong acid and strong base is higher than that of weak acid and weak base.

Enthalpy of neutralisation of acetic acid by NaOH is -50.6 kJ mol^(-1) . Calculate DeltaH for ionisation of CH_(3)COOH . Given. The heat of neutralisation of a strong acid with a strong base is -55.9 kJ mol^(-1) .