Answer Happy

Calorimetry: Heats of Neutralization Post-Laboratory Questions What would be the effect on the enthalpy change if the temperature probe read 1.0°C lower than the true temperature? Explain. (2 pts) 1. 2. How should the two heats of reaction for the neutralization of NaOH with a strong and weak acid compare? Why? (2 pts) 3. The experimental procedure requires that you wash your thermometer and dry it after you measure the temperature of the NaOH solution and before you measure the temperature of the HCl solution. Why? (2 pts) 4. a. After having that completed your experiment and calculated your enthalpy of neutralization, you are told concentration of the NaOH solution you used was 5% less than indicated on its label. When you recalculate the enthalpy of neutralization, will the recalculated value be larger, smaller, or the same as you originally calculated? POST-LAD b. Now consider the HCl you used in your experiment. If the concentration was 5% higher than that stated on its label, what will be the effect on the enthalpy of neutralization originally calculated? 5. A 50.0 mL sample of a 1.00 M solution of MgSO, is mixed with 50.0 mL of 2.00 M NaOH in a calorimeter. The temperature of both solutions was 23.2 °C before mixing and 29.3 °C after mixing. The heat capacity of the calorimeter is 15 J/°C. From these data, calculate AH for the process: MgSO4cm) +2 NaOH(aq) → Mg(OH)20) + Na SO.cap) Assume that the specific heat and density of the solution after mixing are the same as those of pure water and that the volumes are additive. (4 pts)