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Osmotic pressure lab

08/01/2021 Client: saad24vbs Deadline: 3 days

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Student Name


Mohammed Alnaimi


Student ID 48408 Lesson Colligative Properties and Osmotic Pressure Institution Ocean County College Session 2019L3 CHEM 182 DL1 Course CHEM 182 DL1 Instructor Nancy Marashi


Final Report


Exercise 1


Data Table 1: Dialysis Tubing Results


CHEM 182 DL1 Colligative Propert ies and Osmotic Pressure


The light corn syrup in the dialysis tubing is hypotonic to the water because it increased in mass over the amount of time.


1. In your experiment, is the light corn syrup in the dialysis tubing hypertonic or hypotonic to the water?


The molar mass of the antibiotic is 7.47 x 102 g/mol. This is because: 23.6 C = 296.75 K. 8.34 mm Hg x 1/760 mm Hg = .0197 atm. .0197 atm = M x (.0821 (L)(atm) / (mol)(K)) x 296.75 K. .0197 atm / 24.36 (L)(atm) / (mol). M = .0197 atm / 24.36 x (mol-1)(atm). M + 8.09 x 10-4mol/L. .604 g / 8.09 x 10-4mol = g / 1 mol = 7.46 x 102g/mol.


2. 0.302 grams of an antibiotic was dissolved in enough water at 23.6°C to make 500.0 mL of solution. T he solution has an osmotic pressure of 8.34 mm Hg. What is the molar mass of the antibiotic? Show your work.


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Exercise 2


Data Table 2: Temperature Readings for Freezing Point


Time Mass of Dialysis Tubing and Contents


0 minutes


30 minutes


60 minutes


17.2g


20.9g


25.2g


The three freezing points all differ. The first was 2, the second 0, and the third -2. I think there is relationship between the amount of solute in the solution and the freezing temperatures because each started at a lower temperature than the one before and they dropped and ended at a lower freezing point than the one before.


1. Describe the three f reezing points. Is there a relationship between the amount of solute in the solution and the f reezing temperature?


Some practical applications of freezing point depression are antifreeze for example, used in car radiators. Also, salt, when it is used on ice in winter.


2. What are some practical applications of f reezing point depression?


Time (seconds) Temp (°C) of Control (tap water)


30


60


90


4


3


3


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120


150


180


210


240


270


300


330


360


390


420


450


480


510


540


570


600


Time (seconds) Temp (°C) of Solution +0.5 tsp (~2.5 mL) salt


30


60


3


2


2


1


1


1


1


1


1


1


1


1


1


1


0


0


0


2


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90


120


150


180


210


240


270


300


330


360


390


420


450


480


510


540


570


600


Time (seconds) Temp (°C) of Solution +1.0


1


1


1


1


1


1


1


1


1


1


1


1


1


1


1


1


1


0


0


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tsp (~5 mL) salt


30


60


90


120


150


180


210


240


270


300


330


360


390


420


450


480


510


540


570


0


0


-1


-1


-1


-2


-2


-2


-2


-2


-2


-2


-2


-2


-2


-2


-2


-2


-2


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Graph 1: Freezing Point Depression of Salt Solutions


Exercise 3


600 -2


The three boiling points were quite close. I think there is a relationship between the amount of solute in the solution and the boiling temperature because the more solute, the higher the boiling points were.


1. Compare the three boiling points. Is there a relationship between the amount of solute in the solution and the boiling temperature?


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Data Table 3: Temperature Readings for Boiling Point


Some practical applications of the boiling point elevation are when ethylene glycol is added to increase the boiling point of a solution or when we use salt in the water when we cook in order to make the food boil quicker.


2. What are some practical applications of boiling point elevation?


Temp (°C) of Control (tap water)


Temperature at Rolling Boil


Temp (°C) of Solution +0.5 tsp (~2.5 mL) salt


Temperature at Rolling Boil


Temp (°C) of Solution +1.0 tsp (~5 mL) salt


Temperature at Rolling Boil


101 ºC


104 ºC


106 ºC

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