This question is worth three points. The following acid and base solutions are placed in a calorimeter at constant pressure: 25.0 mL of 0.10 M HCl solution and 50.0 mL of 0.20 M NaOH. The total vol-ume of the solution is 75.0 mL.

The water in the mixture has a specific heat of 4.184 J/g◦C. The solution is in-itially at 19.5◦C and at the end of the reaction is at 24.7◦C.

a. Write the balanced chemical equation for the reaction. Include states of matter and subscripts.
b. Calculate the heat q for this reaction using the calorimetry equation (mc△T). Assume the density of the solution is 1.0 g/mL (d=m/V).
c. Calculate the number of moles of HCl added to the reaction.
d. Calculate the moles of NaOH added to the reaction.
e. Determine which reactant is the limiting reactant.
f. Use the relation q +△H = 0 to find the enthalpy change for the reaction.
g. Find the molar heat of reaction by using △H/n where n is the number of moles of the limiting reactant. Recall that the limiting reactant is the reac-tant that produces the smaller amount of products in a reaction.