Questions. The first two questions will demonstrate Hess's Law. 1. a. Algebraically combine reactions a and c to obtain reaction d of Part B, which is. HCl(aq, 1.00 M) + NaOH(s) → NaCl(aq, 0.50 M) + H2O(l) Write out the equations to show their addition: Reaction a) HCl(aq, 1.00 M) + NaOH(aq, 1.00 M) → NaCl(0.500 M) + H2O(l) Reaction c) NaOH(s) → NaOH(aq, 1.00 M) b. Combine the molar enthalpy change values of reactions a and c in the manner indicated in your answer to part (a) to obtain the value of the enthalpy change of reaction d. c. Compare this value with your measured value in Part B. 2. We did not measure experimentally the reaction between acetic acid and solid NaOH: HC2H3O2(aq, 1.00 M) + NaOH(s) → NaC2H3O2(aq, 0.50 M) + H2O(l) Using the same method as in Question 1, combine reactions b and c in Part B in a way that allows the ΔH of this reaction to be calculated. Show your work in detail, with a numerical result. Reaction b) HC2H3O2(aq, 1.00 M) + NaOH(aq, 1.00 M) → NaC2H3O2(aq, 0.500 M) + H2O(l) Reaction c) NaOH(s) → NaOH(aq, 1.00 M) 3. In scientific work we are sometimes in the position of making simplifying approximations. This can be acceptable if we understand the effect they will have on results and verify that it will be small. Use your measured value of C to compare the value of CΔT to msΔT for Part B(a). Does approximating C as 0 in equation 7 appear to be justified for this experiment?