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Experiment #12. Enthalpy of Neutralization
In the course of most physical processes and chemical reactions there is a change in energy. In chemistry what
is normally measured is H (enthalpy change), the change in heat at constant pressure and ignoring any work done by
the reacting system. If the reaction is exothermic, heat is given off and H has a negative value. When heat is absorbed
from the surroundings during the reaction, the reaction is endothermic and H has a positive value. The change in
enthalpy is a measure of the difference in energy between the bonds in the products and the bonds in the reactants.
The absolute energy of a compound cannot be measured directly, but the change in enthalpy that occurs during a
chemical reaction can be measured.
The reaction in today’s experiment is acid / base neutralization which is an exothermic process.
HCl (aq) +
NaOH (aq) 
H2O (l) + NaCl (aq)
The heat released by the reaction will be absorbed by the surroundings (aqueous solution). Coffee Cup
Calorimetry will be employed to determine the amount of heat lost by the reaction and gained by the salt water
solution. A calorimeter is simply a container used to measure the heat change. Coffee Cup Calorimetry just means that
we will be measuring heat at constant pressure, H. The heat lost by the reaction will actually be transferred to both
the salt water and its surroundings (the calorimeter.) The heat capacity of the calorimeter (in this case, two Styrofoam
cups) usually would be calculated first; however, we have found that the heat capacity of the cups is so small that it can
be neglected.
As the First Law of Thermodynamics applies,
Heat (q) lost by the reaction + heat (q) gained by the solution = 0
or qrxn = – qsoln
To find the heat lost by the reaction we use:
q = m x Cs x ΔT
where: m = mass of the solution (The density of the solution is 1.04 g/mL)
Cs = specific heat capacity of the solution (3.87 J/gC)
ΔT= change in temperature of the solution (Tfinal – Tinitial)
2 Styrofoam cups
50 or 100 mL graduated cylinder
2.00 M HCl
(2) Thermometers
Stirring rod
150 mL beaker
2.00 M NaOH
1. Rinse and dry the Styrofoam cups (calorimeter). Place one cup inside the other. Measure out 25.0 mL of 2.00 M
NaOH and pour it into the calorimeter. In a clean dry 150 mL beaker, take 25.0 mL of 2.00 M HCl.
2. Determine the temperature of both the acid and the base to the nearest 0.1C. Average the temperatures. Record
this average as the initial temperature Tinitial.
3. Pour the acid into the base quickly and carefully with gentle stirring. Start monitoring the temperature as soon as
the two are mixed. Continue to stir and monitor the temperature. Record the maximum temperature that the
solution reaches. This is Tfinal
4. Repeat Steps 1 - 3 (above) for a second trial.
All reactants and products may be disposed of into the sink.
CHM112 Lab – Heat of Neutralization – Grading Rubric
Points possible
Lab Performance
Printed lab handout and rubric was brought to lab
Safety and proper waste disposal procedures observed
Followed procedure correctly without depending too much
on instructor or lab partner
Work space and glassware was cleaned up
Lab Report
Calculations Q1-Q11 (1 point each)
Subject to additional penalties at the discretion of the instructor.
Points earned
Heat of Neutralization: Data Sheet
Name ________________________
Trial 1
Trial 2
3.87 J/g °C
3.87 J/g °C
Volume of 2.00 M HCl
Volume of 2.00 M NaOH
Volume of solution
T initial
T final
T (T final — T initial)
Specific heat capacity of NaCl solution
Calculations (Show all your work completely and clearly. Include proper units)
1. Calculate the mass of the solution for each trial (given the density of the solution is 1.04 g/ml)
2. Calculate the heat absorbed by the solution in each trial.(qsoln)
qsoln (Trial 1) ____________
qsoln (Trial 2) _____________
Average qsoln _________
3. Calculate q rxn = ____________________________
4. Calculate the number of moles of water formed (This is the same as moles of HCl):
moles of water = moles of HCl = __________________
5. Calculate Hneutralization (H°) per mole of water (kJ/mole) formed. Make sure the sign is correct.
H° = _________________
Heat of Neutralization: Calculations
Name ________________________
6. Write the chemical reaction for the autoionization of water (equilibrium constant Kw).
7. Look up the numerical value for Kw at Tinitial (Take the average of Tinitial from both trials)
8. How is the reaction in question 1 related to the net ionic reaction for the neutralization shown below?
H3O+(aq) + OH—(aq)  H2O(l) + H2O(l)
9. Use the value of Kw and the relationship between the reactions in questions 1 and 3 to find the numerical value for
the K for the neutralization reaction in question 3.
10. Given the K calculated for the neutralization reaction, calculate ΔGo for the neutralization reaction. (Use average
initial T from the two trials for the reaction Temperature.)
11. From ΔGo above, and the ΔH° that you have calculated, calculate the ΔS° for the reaction. (Use average initial T
from the two trials for the reaction Temperature.)