Colligative Chemistry1412 P

Colligative
Chemistry1412 P.01
South Texas College
Fall 2018
For: Dr. J. Studer
By: Aileen M Lizcano
Objective: Colligative properties of solutions depend of the amount of quantity of the solute to be dissolved to the solvent than the true identity of the solute. The phenomenon of the freezing point lowering will be viewed as an example of a colligative property in choice I . And for choice II it will be viewed in the process of osmosis and dialysis.

Material:
Cooper wire
Test tubes
T-butyl alcohol
Rubber stopper holes
600 ML Beaker
Tap water
Distilled water
Unknown Identification “F”
25 ML Graduated Cylinder
Ice chips
Weight boat
Balance bean
Thermometers
Stop watches

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Safety Material:
Googles
Gloves
Lab Coat
Hair tie
Closed shoes
Long pants

Summary procedure:
Wear gloves, goggles, and apron to begin the lab procedure. Set material on the table.
Part 1. Grab 25 ml graduated cylinder and weight it in the balance. Record it. Then measuredly add 25ml of the T-Butanol on the graduated cylinder. Measure the graduated cylinder again with the chemical and record . Grab the 600ml beaker and fill it with 400 ml with tap water. On the side grab ice cubes on a weight boat. Add ice to the beaker and record temperature when you place it. Again record temperature when ice is melted. Meanwhile when is melting grab the 25ml graduated cylinder with the (t butanol) and fill the 25ml in a test tube put a thermometer and a cooper wire in a rubber stopper holes to begin the experiment. To begin this experiment put the test tube in the graduated beaker when the ice is melted. Have another thermometer in the graduated beaker to know the cold temperature is constant or not. Start recording every 15 seconds when the test tube is inside the beaker and while someone is moving the copper up and down. Record every 15 second for 480 seconds. End the determination after the 480 seconds are over by having an slushy alcohol in the tube. Take off the test tube and add heat energy of your hands to melt it.

Part 2. Add more ice chips to the beaker that was used for part 1 for the freezing water bath. Using an pipet add 0.20ml of distilled water to the sample of the t-butyl alcohol used in part 1. Stir the mixture together until the water has dissolved well enough for the solution to look homogeneous. Then add the thermometer and cooper wire in the rubber stopper holes to be placed in the tube to begin the experiment again. Have another thermometer in the graduated beaker to know the cold temperature is constant or not. Record every 15 seconds as well for up to 480 seconds but the cooper wire has to be constantly moving. End the determination after the 480 seconds are over by having an slushy alcohol in the tube. Take off the test tube and add heat energy of your hands to melt it. And discard the test tube on a container that is made for hazard waste under the hood.

Part 3. Add more ice chips to the beaker to be the ice water bath. Grab the unknown that the instructor has. Measure 25ml of the T-Butanol on the graduated cylinder and transfer it into a test tube. Measure the mass of the alcohol and test tube. Carefully transfer the solid to the test tube that has the alcohol in it. Then add the thermometer and cooper wire in the rubber stopper holes to be placed in the tube to begin the experiment again. Have another thermometer in the graduated beaker to know the cold temperature is constant or not. Carefully move the stir to the alcohol and the unknown until it completely dissolved well. Keep checking the temperature of the ice water bath so it won’t go higher than 16*C and no lower than 14*C. Position test tube just like part 2. Constantly stir the cooper wire into the unknown solution . Record every 15 second for 480 seconds. End the determination after the 480 seconds are over by having an slushy alcohol in the tube. Take off the test tube and add heat energy of your hands to melt it.

Part 4. Repeat the past procedure with the Unknown solution exactly how it was done to have another determination. Then discard the unknown solution in the discard container under the hood where the instructor told to do so.

Data Charts:
61.89grams 25 ML graduated Cylinder
80.92grams25ML Grad. Cyl. + (T-Butanol)
19.3 Celsius Initial Temperature water with ice
16.0 Celsius Final Temperature of ice melted
Time Temp. Time Temp.

15 23.6 270 22.3
30 22.7 285 22.1
45 22.3 300 22.1
60 22.8 315 22.0
75 22.8 330 22.0
90 22.8 345 21.9
105 22.8 360 21.8
120 22.8 375 21.8
135 22.7 390 21.7
150 22.7 405 21.7
165 22.6 420 21.6
180 22.5 435 21.6
195 22.5 450 21.6
210 22.4 465 21.5
225 22.3 480 21.5
240 22.3 255 22.3 Part 1Part 2
Time Temp. Time Temp.

15 25.7 270 17.1
30 24.2 285 17.1
45 23.5 300 17
60 22.1 315 17
75 21.0 330 16.9
90 20.8 345 16.8
105 20.1 360 16.6
120 19.3 375 16.4
135 18.8 390 16.2
150 18.8 405 16.1
165 18.5 420 15.9
180 18.2 435 15.8
195 17.5 450 15.7
210 17.1 465 15.5
225 16.9 480 15.4
240 17.0 255 17.2 Time Temp. Time Temp.

15 23.3 270 11.4
30 21.5 285 11.2
45 19.6 300 11
60 18.3 315 10.9
75 17.4 330 10.6
90 16.6 345 10.5
105 16.1 360 10.1
120 15.6 375 9.4
135 15.5 390 9
150 14.8 405 8.7
165 14.7 420 8.2
180 13.5 435 8.1
195 12.5 450 8
210 12.3 465 8
225 11.7 480 8.1
240 11.5 255 11.2 Time Temp. Time Temp.

15 25.0 270 14.8
30 22.8 285 14.7
45 20.9 300 14.6
60 19.2 315 14.5
75 17.9 330 14.4
90 17.8 345 14.3
105 17.4 360 14.2
120 16.8 375 14.2
135 16.3 390 14.1
150 15.7 405 14.1
165 15.3 420 14
180 15.2 435 14
195 15.1 450 13.9
210 15 465 13.8
225 15 480 13.8
240 14.9 255 14.8 Part 3Part 4

Calculations:
Determining the Freeze Temp. of t-Butyl alcohol.

For each set of time / temperature record the data during the freezing point measurement.
This graph has the data information inputted but it doesn’t have 15, 30,45… seconds underneath but it’s dot represent its time and the 15 seconds that it has passed. (Graph represent 0 to 480 seconds horizontally and temperature of Celsius on the left side vertically)
Conclusions: Each of the four experiments that was done had different results to each other from starting point to end. The first part did not have a degree change as the others. It was more constant of than the others. Second part did made a huge change compared to the first. It wasn’t constant at all from starting to a 25.7 Celsius to 15.4 at ending freeze point. As from the other last two containing the unknown solution it had a more freezing point compared with the first two that didn’t have the unknown solution.

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