1. The problem statement, all variables and given/known data NaOH(aq) + HCl(aq) ------> NaCl(aq) + H2O(l) 50mL of 1.0M HCl and 50ml 1.0M NaOH was mixed. Total heat is 2826J. If the density of 0.5M NaCl produced in this reaction is 1.02g/mL: a) What is the mass of the solution? b) Moles of water formed c) Moles of NaCl formed d) Molar heat of reaction 2. Relevant equations 3. The attempt at a solution a) 1.02g/ml x 100ml = 102 g b) 50ml x 0.001 x 1M =0.05 moles of Water d) 2826/0.05 = 56.52kJ Iam very confused about c). Why is there "0.5M"in the question? Do I have to use that molarity during calculation?