Hi! I have a question on this. In this problem, When 20.0mL of 1.00M NaCl at 22.00°C is mixed with 20.0mL of 1.00M AgNO3 at 22.00°C in a calorimeter, a white precipitate forms and the temperature of the mixture reaches 29.60°C. Assume that the specific heat capacity of the mixture is 4.184 J/g*C, its density is 1.00g/mL, and the volumes are additive.

a) Write the net ionic equation for this reaction.

b) Calculate ΔH for the reaction.

Why when calculating the ΔH, is the Molarity of AgNO3 used as how many moles of Ag+ there is when calculating from 0.0200L x 1.0mol Ag+/1L=0.0200mol Ag+. This is what is shown on the lecture about this and I don't understand why the molarity is used to find the moles to then use those moles to find the ΔH. Could you please explain? Thanks!