Find the delta H for the neutralization reaction and find the delta H per mole of H+ and OH- ions reacting

Using 25mL of 1.00 M HCl solution and 25mL of 1.00 M NaOH
Original temp of HCl 21.1°C
Original temp of NaOH 20.7°C
Final temp of neutralized mixture 28.5°C
Change in temp, Delta T 7.6°C
qH2O (assume 50g H2O are present) 1588.4J
ΔH for the neutralization reaction ?
ΔH per mole of H+ and OH- ions reacting ?

I have been trying to figure this out for the past 4 hrs, can someone please help me and also explain to me how you got the answer show your work. Please Help!!!!

find moles
(0.025L) (1.00 mol HCl / Litre) = 0.025 moles of H+
(0.025L) (1.00 mol NaOH / Litre) = 0.025 moles of OH-

(1588.4J) / 0.025 mol )= 63,597 jouoles per mole of H+ and OH- ions reacting

that's
dH = - 63.6 kJ / mole of H+ and OH- ions reacting
("minus", because this reaction is exothermic)