Determining the Enthalpy of a Neutralization Reaction
Materials
• One pair of goggles
• One apron
• 175 mL of 1.00 mol/L HCl(aq) at room temperature
• 175 mL of 1.00 mol/L NaOH(aq) at room temperature
• One calorimeter with a stirring rod
• One 100 mL graduated cylinder
• Two 250 mL beakers
• One thermometer
• One roll of paper towel
Procedure
1. Before starting the experiment, the procedure was written and approved by the teacher.
2. An observations table was made to record the initial volume and temperature of NaOH (aq) and HCl (aq); the table also included sections to record temperatures, at 5 second intervals with a final 30 second plateau, for each of the 3 trials.
3. The locations for the waste disposal bin, the eye wash station, and the fire extinguishers were identified.
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4. Shoe laces were tied. 5. Hair was tied back. 6.
Goggles were put on and adjusted to ensure comfort.
7. All glassware needed for the experiment was rinsed with water and dried with paper towel.
8. 175 mL of sodium hydroxide solution was retrieved and contained in a 250 mL beaker.
9. 175 mL of hydrochloric acid solution was retrieved and contained in the other 250 mL beaker.
10. 50 mL of the sodium hydroxide solution was poured into the graduated cylinder from the breaker.
11. The temperature of the sodium hydroxide solution was measured by placing a thermometer in the graduated cylinder and the measurement was recorded in the observations table.
12. The thermometer was rinsed with water and dried with paper towel.
13. The 50 mL sodium hydroxide solution was carefully poured from the graduated cylinder into the calorimeter.
14. The graduated cylinder was rinsed with water and dried with paper towel.
15. 50 mL of the hydrochloric acid solution was poured into the graduated cylinder from its beaker.
16. The temperature of the hydrochloric acid solution was measured by placing a thermometer in the graduated cylinder and the measurement was recorded on the observations table.
17. The thermometer was rinsed with water and dried with paper
towel. 18. The 50 mL solution of hydrochloric acid was carefully poured from the graduated cylinder into the calorimeter. 19. The lid of the calorimeter was quickly sealed. 20. The stirring rod and the thermometer were quickly placed in the calorimeter through the two openings at the top of the lid. 21. The temperature was measured and recorded on the observations table at 5 second intervals with a 30 second plateau. 22. The stirring rod and the thermometer were removed from the calorimeter, rinsed with water, and dried with paper towel. 23. The lid of the calorimeter was opened and the neutralized solution of hydrochloric acid and sodium hydroxide was disposed of in the waste disposal container. 24. The calorimeter was rinsed and dried. 25. Steps 8 – 22 were repeated for two more trials. 26. All materials used were put away in their original locations. 27. The observations table was checked to ensure that it was completely filled. 28. The data was compared with that of other groups.
The mixture was poured through a weight filter paper and Sucrose washed with a 5ml of dichloromethane. The resulting solid was left in a breaker to dry for one week, to be measured. Left it in the drawer to dry out for a week and weighted it to find the sucrose amount recovered amount.
Two equations were used in this experiment to determine the initial temperature of the hot water. The first equation
Start with the hot water and first measure the temperature. Record it. 8. Then pour 40 ml into the beaker. You can measure how much water was used by looking at the meniscus.
2. A test tube was then filled with 35ml of yeast and placed in the
We used the pipette filler and filled the glucose rinsed pipette to add 10ml of 10% of glucose in test tube 0.
Once the mixture had been completely dissolved, the solution was transferred to a separatory funnel. The solution was then extracted twice using 5.0 mL of 1 M
The purpose of this lab was to calculate the specific heat of a metal cylinder
We must first begin the today’s lab by connecting the thermometer that digitally detects surrounding temperature to the Lab Pro Interface located on the computer via...
the chances of collisions increase thus giving a faster rate of reaction. Then the s Apparatus:. Beaker Hydrochloric acid Distilled water Measuring cylinder Pipette Test tubes Test tube rack Diagram:.. [ IMAGE] Method: The.. Measure out 10cm3 of hydrochloric acid, as the concentration requires. for each concentration its composition is.
Distance between the wick and the base of the copper calorimeter: this distance will be 5cm measured using a ruler and adjusted if necessary. The fuel has been weighed correctly: The fuel will be weighed twice, to ensure accuracy. Make sure there is the right amount of water in the copper calorimeter: to make sure the correct amount of water is in the copper I will use a measuring cylinder, I will accurately fill it to 100cm. I will place the cylinder on a flat surface just to check that the measurement is correct. Make sure fresh water has been placed in the container, so that it isn’t still warm and that the copper calorimeter is also cooled down: by making sure that the water has been tipped away straight after the experiment, should hopefully be enough to make sure it will be replaced, also as we have to note the temperature of the water before we start, it should be noticeable.
Quickly and carefully transfer the heated metal from the test tube to the water in the calorimeter.
To determine sodium chlorides enthalpy of solution, samples of sodium chloride were dissolved in water as the temperature of the solution was monitored with a temperature probe. 1.0 grams of sodium chloride was weighed out on an analytical scale and set aside. Using a 100 mL beaker, 50 mL of deionized water was measured out. The 50 mL of deionized water was then transferred to a calorimeter. The calorimeter consisted of one Styrofoam cup in the other, capped with a thick piece of Styrofoam. A Vernier temperature probe was attached to the computer with GoLink! interface. The computer software used to interpret and monitor the temperature readings was LoggerPro. LoggerPro was set to collect a temperature reading from the calorimeter every 3 seconds. The initial temperature of the deionized water in the calorimeter and recorded. The 1.0 grams of sodium chloride was then added to the 50 mL of deionized water, the calorimeter cap was placed quickly, and the temperature probe inserted through a small hole in the cap. The temperature was monitored until steady as the solution was stirred with the temperature probe. This procedure was replicated twice more for a total of three trials. Following these experiments, the procedure was replicated again with the exception of using 2.0 and 3.0 grams of sodium chloride instead of 1.0 grams described
In a 100ml beaker 30mls of water was placed the temperature of the water was recorded. 1 teaspoon of Ammonium Nitrate was added to the water and stirred until dissolved. The temperature was then recorded again. This was to see the difference between the initial temperature and the final temperature.
Neutralization Experiment AIM:- To investigate how heat is given out in neutralizing sodium hydroxide (NaOH) using different concentrations of Hydrochloric Acid. Background Information:- Substances that neutralize acids are called alkalis. An acid is a substance that forms hydrogen ions (H+ ) when placed in water. It can also be described as a proton donor as it provides H+ ions. An example of an acid is hydrochloric acid (HCl), Sulphuric acid (H2SO4) etc.
The purpose of this experiment is to use our knowledge from previous experiments to determine the exact concentration of a 0.1M sodium hydroxide solution by titration (Lab Guide pg.141).