ColligativeChemistry1412 P.01South Texas CollegeFall 2018For: Dr. J.
StuderBy: Aileen M LizcanoObjective: 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 wireTest tubes T-butyl alcoholRubber stopper holes600 ML BeakerTap waterDistilled waterUnknown Identification “F”25 ML Graduated CylinderIce chipsWeight boatBalance beanThermometersStop watches Safety Material: Googles GlovesLab CoatHair tieClosed shoesLong pantsSummary 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 Cylinder80.92grams25ML Grad. Cyl.
+ (T-Butanol)19.3 Celsius Initial Temperature water with ice 16.0 Celsius Final Temperature of ice meltedTime Temp. Time Temp.
15 23.6 270 22.330 22.7 285 22.
1 45 22.3 300 22.160 22.
8 315 22.075 22.8 330 22.090 22.8 345 21.9105 22.8 360 21.8120 22.
8 375 21.8135 22.7 390 21.
7150 22.7 405 21.7165 22.6 420 21.6180 22.5 435 21.
6195 22.5 450 21.6210 22.4 465 21.5225 22.3 480 21.5240 22.3 255 22.
3 Part 1Part 2Time Temp. Time Temp. 15 25.7 270 17.
130 24.2 285 17.145 23.5 300 1760 22.
1 315 1775 21.0 330 16.990 20.8 345 16.8105 20.
1 360 16.6120 19.3 375 16.4135 18.8 390 16.2150 18.8 405 16.1165 18.
5 420 15.9180 18.2 435 15.8195 17.5 450 15.7210 17.1 465 15.
5225 16.9 480 15.4240 17.
0 255 17.2 Time Temp. Time Temp. 15 23.3 270 11.430 21.
5 285 11.2 45 19.6 300 1160 18.3 315 10.975 17.
4 330 10.690 16.6 345 10.5105 16.1 360 10.1120 15.
6 375 9.4135 15.5 390 9150 14.8 405 8.7165 14.7 420 8.
2180 13.5 435 8.1195 12.5 450 8210 12.3 465 8225 11.7 480 8.
1240 11.5 255 11.2 Time Temp. Time Temp. 15 25.
0 270 14.830 22.8 285 14.745 20.9 300 14.
660 19.2 315 14.575 17.9 330 14.490 17.8 345 14.
3105 17.4 360 14.2120 16.8 375 14.2135 16.3 390 14.1150 15.7 405 14.
1165 15.3 420 14180 15.2 435 14195 15.1 450 13.9210 15 465 13.8225 15 480 13.
8240 14.9 255 14.8 Part 3Part 4Calculations: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.
