CHEM 219
Lab Report & Lab Notes
Experiments #: 1 - 8
Portage Learning
Inside you will get:
- All Experiments1 through 8
Clear, Concise Scientific Language.
- All Tables and Figures Labelled Clearly.
- Included Units for All Measurements.
- Proofread Report.
, TABLE OF CONTENTS
• Experiment 1: Distillation
• Experiment 2: Crystallization and Purification
• Experiment 3: Extraction
• Experiment 4: Fermentation
• Experiment 5: Column Chromatography
• Experiment 6: Synthesis
• Experiment 7: Nitration of Methyl Benzoate
• Experiment 8: Synthesis of Azo dye
,LAB REPORT
Experiment #: 1
Title: Distillation
Purpose: The purpose of the experiment is to compare and contrast the two
main types of distillation that are used in organic chemistry which are simple
and fractional distillation. Distillation is used to identify and purify organic
compounds by separating them from less-volatile materials. The lab will be
used to determine which type of distillation is more efficient at separating the
mixture using the difference in boiling points.
Procedure:
Simple distillation
1. Start with the distillation pot (100mL round bottomed flask) and add a
mixture of 30mL of water and 30mL of methanol.
2. Add a few pieces of marble (boiling chips) to the mixture.
3. Clamp the distillation pot to the ring stand securely and mate the heat
source to the still pot.
4. Turn on the cold-water supply to the condenser and also turn on the
heat source to bring it to a boil.
5. For every 2 mL of distillate record the temperature.
Fractional distillation
1. Start with the distillation pot (100mL round bottomed flask) and add a
mixture of 30mL of water and 30mL of methanol.
2. Add a few pieces of marble (boiling chips) to the mixture.
3. Clamp the distillation pot to the ring stand with the fractionating column
securely. Mate the heat source to the still pot.
4. Turn on the cold-water supply to the condenser and also turn on the
heat source to bring it to a boil.
5. For every 2 mL of distillate record the temperature.
, Data/Results/Calculations:
Vol (mL) Simple Temp (C) Fractional Temp (C)
2 73.8 64.8
4 74.9 65.6
6 75.9 66.8
8 77 67
10 77.9 67
12 79.1 67.1
14 79.3 67.1
16 79.9 67
18 80.9 67
20 82.9 67
22 83.8 67.6
24 84.9 69
26 87.8 70.1
28 90.1 72
30 94.1 89
32 95.1 94.5
34 98.8 101.9
36 101.1 102.9
38 102.5 103
40 103 103.5
42 104.2 103.9
44 104.5 103.9
46 104.9 103.9
48 105.1 103.9
50 105.1 103.9
Boiling point of CH3OH= 64.7 C
Boiling point of H2O= 100 C
Lab Report & Lab Notes
Experiments #: 1 - 8
Portage Learning
Inside you will get:
- All Experiments1 through 8
Clear, Concise Scientific Language.
- All Tables and Figures Labelled Clearly.
- Included Units for All Measurements.
- Proofread Report.
, TABLE OF CONTENTS
• Experiment 1: Distillation
• Experiment 2: Crystallization and Purification
• Experiment 3: Extraction
• Experiment 4: Fermentation
• Experiment 5: Column Chromatography
• Experiment 6: Synthesis
• Experiment 7: Nitration of Methyl Benzoate
• Experiment 8: Synthesis of Azo dye
,LAB REPORT
Experiment #: 1
Title: Distillation
Purpose: The purpose of the experiment is to compare and contrast the two
main types of distillation that are used in organic chemistry which are simple
and fractional distillation. Distillation is used to identify and purify organic
compounds by separating them from less-volatile materials. The lab will be
used to determine which type of distillation is more efficient at separating the
mixture using the difference in boiling points.
Procedure:
Simple distillation
1. Start with the distillation pot (100mL round bottomed flask) and add a
mixture of 30mL of water and 30mL of methanol.
2. Add a few pieces of marble (boiling chips) to the mixture.
3. Clamp the distillation pot to the ring stand securely and mate the heat
source to the still pot.
4. Turn on the cold-water supply to the condenser and also turn on the
heat source to bring it to a boil.
5. For every 2 mL of distillate record the temperature.
Fractional distillation
1. Start with the distillation pot (100mL round bottomed flask) and add a
mixture of 30mL of water and 30mL of methanol.
2. Add a few pieces of marble (boiling chips) to the mixture.
3. Clamp the distillation pot to the ring stand with the fractionating column
securely. Mate the heat source to the still pot.
4. Turn on the cold-water supply to the condenser and also turn on the
heat source to bring it to a boil.
5. For every 2 mL of distillate record the temperature.
, Data/Results/Calculations:
Vol (mL) Simple Temp (C) Fractional Temp (C)
2 73.8 64.8
4 74.9 65.6
6 75.9 66.8
8 77 67
10 77.9 67
12 79.1 67.1
14 79.3 67.1
16 79.9 67
18 80.9 67
20 82.9 67
22 83.8 67.6
24 84.9 69
26 87.8 70.1
28 90.1 72
30 94.1 89
32 95.1 94.5
34 98.8 101.9
36 101.1 102.9
38 102.5 103
40 103 103.5
42 104.2 103.9
44 104.5 103.9
46 104.9 103.9
48 105.1 103.9
50 105.1 103.9
Boiling point of CH3OH= 64.7 C
Boiling point of H2O= 100 C
