Temperature and Degrees Celsius
Enthalpy of Neutralization J. Smith M. Smith CHEM 1290-xx 10-31-06 TA
Purpose: The purpose of the experiment is to determine the calorimeter constant for the calorimeter holding a specific solution based on the data of heat lost and heat gained. The purpose is to also be able to determine the enthalpy of neutralization for the reaction of a strong acid (phosphoric acid) and a strong base (sodium hydroxide). Experimental: Materials: The materials needed for this lab included; 2 large beakers, a Calorimeter Styrofoam cup, computer, stirring rod, 2 thermometers, Logger Program, and Probes volumetric pipet. Sodium hydroxide (NaOH) (corrosive and toxic), and phosphoric acid (H3PO4) (corrosive and toxic) were used. Procedure:
The calorimeter was set up as shown in Figure 1 above. A Styrofoam cup was used to line the beaker. Cold distilled water (50 mL) was put into the cup along with a thermometer. Continue writing your procedure (what you actually did, not what you were supposed to do) in paragraph format. The list format below is to show an example of how to switch from directions in your lab manual to the formal lab report) 1. Set up the Calorimeter as in Figure 1. 2. Use Styrofoam cup as a liner in the beaker.
a. b.
measure 50.0 ml cold distilled H2O in cup place thermometer inside
3. Place 50.0 ml distilled warm water (15-20 degrees above room temp.) in beaker 4. Measure and record initial temperature for both hot and cold for 2-3 minutes a. b. quickly lift lid and add hot water to the cold recover, stir and note mixing time
5. Record temperature every 30 seconds for 20 minutes or until temperature reaches its max. 6. Empty and dry all equipment 7. Place 50.0 ml NaOH in Styrofoam cup 8. Place 50.0 ml assigned acid (phosphorc acid) in beaker 9. Repeat steps 4-6 10. 11. Prepare computer apparatus Set the vertical axis for temperature and the horizontal for time
12. Connect one probe to CH1 and the other to CH2 13. Set up 2 large beakers a.
Purpose: The purpose of the experiment is to determine the calorimeter constant for the calorimeter holding a specific solution based on the data of heat lost and heat gained. The purpose is to also be able to determine the enthalpy of neutralization for the reaction of a strong acid (phosphoric acid) and a strong base (sodium hydroxide). Experimental: Materials: The materials needed for this lab included; 2 large beakers, a Calorimeter Styrofoam cup, computer, stirring rod, 2 thermometers, Logger Program, and Probes volumetric pipet. Sodium hydroxide (NaOH) (corrosive and toxic), and phosphoric acid (H3PO4) (corrosive and toxic) were used. Procedure:
The calorimeter was set up as shown in Figure 1 above. A Styrofoam cup was used to line the beaker. Cold distilled water (50 mL) was put into the cup along with a thermometer. Continue writing your procedure (what you actually did, not what you were supposed to do) in paragraph format. The list format below is to show an example of how to switch from directions in your lab manual to the formal lab report) 1. Set up the Calorimeter as in Figure 1. 2. Use Styrofoam cup as a liner in the beaker.
a. b.
measure 50.0 ml cold distilled H2O in cup place thermometer inside
3. Place 50.0 ml distilled warm water (15-20 degrees above room temp.) in beaker 4. Measure and record initial temperature for both hot and cold for 2-3 minutes a. b. quickly lift lid and add hot water to the cold recover, stir and note mixing time
5. Record temperature every 30 seconds for 20 minutes or until temperature reaches its max. 6. Empty and dry all equipment 7. Place 50.0 ml NaOH in Styrofoam cup 8. Place 50.0 ml assigned acid (phosphorc acid) in beaker 9. Repeat steps 4-6 10. 11. Prepare computer apparatus Set the vertical axis for temperature and the horizontal for time
12. Connect one probe to CH1 and the other to CH2 13. Set up 2 large beakers a.
References: 1 Chem. 1290 Laboratory Manual: Enthalpy of Neutralization. 2006. Thomson Brooks/Cole. Belmont, CA.