Chemistry college
posted by Willy on .
The standard enthalpies of formation of ions in aqueous solutions are obtained by arbitrarily assigning a value of zero to H ions;that is, delta H(f) [H+(aq)]=0
A.for this reaction: calculate delta H(f) for the Cl ions.
HCl(g) ==H2O==>H+(aq)+Cl(aq)
delta H= 74.9 kJ/mol
(answer has to be in kJ/mol)
B.given that delta H(f) for OH ions is 229.6 kJ/mol, calculate the enthalpy of neutralization when 1 mole of a strong monoprotic acid (such as HCl) is titrated by 1 mole of a strong base (such as KOH) at 25^C.
(answer has to be in kJ/mol)

A: you can either look at the properties table or use 74.9kJ/mol= x +
92.3 kJ/mol and solve for x which is 167.16...... juse the equation deltaH= Sum deltaH of products  sum deltaH of reactants
idk how to do B yet 
For part B:
Heat of neutralization is 56.2