Given that the data for neutralization of weak acid (HA) and strong acid is :
`HA+OH^(-)toA^(-)+H_(2)O`, `DeltaH=-41.80 kJ`
`H^(+)+OH^(-)toH_(2)O`, `DeltaH=+ -55.90 kJ`
The enthalpy of dissociation of weak acid would be

Given that the data for neutralization of a weak acid (HA) and strong acid with a strong base is: HA +OH^(-) rArr A^(-) + H_(2)O: DeltaH = -41.80kJ , H^(+) + OH^(-) rArr H_(2)O, Delta H= -55.90kJ The enthalpy of dissociation of weak acid would be

Given that the data for neutralization of a weak acid (HA) and strong acid with a strong base is: HA +OH^(-) rArr A^(-) + H_(2)O: DeltaH = -41.80kJ , H^(+) + OH^(-) rArr H_(2)O, Delta H= -55.90kJ The enthalpy of dissociation of weak acid would be

HA+OH^(-) to H_(2)O+A^(-)+q_(1) kJ H^(+)+OH^(-) to H_(2)O+ q_(2) kJ The enthalpy of dissociation of HA is

H_(2)O(l)toH_(2)O(g) , DeltaH=+43.7 kJ H_(2)O(s)toH_(2)O(l) , DeltaH=+6.05kJ The value of DeltaH_((sublimation)) of ice is

HA + OH rightarrow H_(2)O + A^(-+) q_(1) kJ H^(+) + OH ^(-) rightarrow H_(2)O + q_(2)kJ the enthalpy of ionisation of HA is

HA + OH rightarrow H_(2)O + A^(-+) q_(1) kJ H^(+) + OH ^(-) rightarrow H_(2)O + q_(2)kJ the enthalpy of ionisation of HA is