There is the experiment of Enthalpy of neutralization of strong HCl and strong base NaOH The problem statement, all variables and given/known data Chemicals: 0.2 M HCl and 0.2 M NaOH Polythene bottle. Water equivalent of polythene bottle e=900 t1=29.7 c temp of mixture= 32 c Rise in temperature = 2.3 c The attempt at a solution enthalpy change during neutralization of 100 mL 0.2 M HCl=-(200+e)(rise in temp)1.184 J For 1 M HCl = -(200+e)(rise in temp)1.184/0.2×1000 =-52.92 KJ This was my answer. But on the internet, I found the answer of same around -57.1 KJ Some of my frnd's answer was near to it. I tried many times, but my answer was nearly -53 KJ.. Actually, I performed this experiment alone, as I was absent during this test. So, please tell me am I right or wrong? What is the absolute value of enthalpy of neutralization of strong acid HCl and strong base NaOH. Is it same for dilute solution and for strong or different? what are the exact values.. Please answer soon..