Experiment 3_ Pre-Lab

Please answer the question at the bottom. Fractional distillation  Measure 55 mL of 40% ethanol  Place 50 mL of ethanol in your distilling flask taking care that no liquid enters the side arm.  Place the remaining 5 mL of ethanol in a test tube and set aside for procedure 2.  Add a few marble or porcelain chips to the distilling flask to prevent bumping. Bumping is a term given to irregular boiling  Assemble the rest of the apparatus for a simple distillation set-up. You may ask assistance from your instructor  Cover the top of the distilling flask with a cork fitted with a thermometer. Make sure that the tip of the thermometer bulb is just below the side arm of the distillation flask  Check all connections for tightness  Heat the contents of the flask to boiling. Adjust the flame when the sample is already boiling. Make sure that it does not boil to dryness.  Note the temperature of the first drop.  Collect 60 drops of distillate per test tube. You will need 5 test tubes, thus five…

1-propanol, 2-propanol, and 1-butanol all have boiling  too close together  to be separated  using the simple distillation  column. What equipment  be used to separate a mixture  of these three?

1. What boiling point of the following mixture of compounds. Then, which would boil first? And Finally, indicate what type of distillation will you use to separate them.

6. Suppose you have a mixture of water and your 2-bromo-2-methylbutane product in a separatory funnel. Use densities to predict which phase will be the top layer in the funnel. a. 2-bromo-2-methylbutane (organic phase) b. water (aqueous phase) c. there would only be one phase since the substances are miscible

Pure aspirin has a melting point of 135-136 °C. Before the melting point was determined - if the sample contains water by absorbing moisture in the air - what effect could this have on the observed melting point from the sample?

Suppose that you have a 1:1 mixture of compounds that is comprised of compound X and compound Y. You desire pure compound X and are planning a recrystallization to enhance the purity. Which solvent below is optimal for your recrystallization?      Ethanol (boiling point = 78 °C)   Solubility At   0  °C 100  °C Compound X 0.05 g/mL 0.20 g/mL Compound Y 0.02 g/mL 0.40 g/mL           Water (boiling point = 100 °C)   Solubility At   0  °C 100  °C Compound X 0.02 g/mL 0.05 g/mL Compound Y 0.01 g/mL 0.10 g/mL           Methanol (boiling point = 65 °C)   Solubility At   0  °C 65  °C Compound X 0.04 g/mL 0.10 g/mL Compound Y 0.02 g/mL 0.30 g/mL         Acetone (boiling point = 56 °C)   Solubility At   0  °C 56  °C Compound X 0.10 g/mL 0.50 g/mL Compound Y 0.20 g/mL 0.50 g/mL         Ethyl Acetate (boiling point = 77 °C)   Solubility At   0  °C 77  °C Compound X 0.10 g/mL 0.60 g/mL Compound Y 0.30 g/mL 0.60…

Could the following compound mixtures be separated by simple distillation? Explain why or why not? a. diethyl ether/ 1-butanol (b.p. 34.6 degrees celsius/ 117 degrees celsius) b. water/ethanol (b.p. 100 degrees celsius/ 78 degrees celsius)

Is this correct for the diaper dissection lab

Remaining Time: 28 minutes, 52 seconds. Question Completion Status: A Moving to another question will save this response. Question 1 Which alcohol will be more soluble in water? ОН O A. OH O B. ÓH OH OH O E. A Moving to another question will save this response.

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4. Why is fractional distillation more "efficient" than simple distillation? During boiling point determination the temperature of the vapors is be E

3. Standard white vinegar you can buy in the grocery store is 5% concentration. That means 5% of the liquid vinegar is acetic acid and 95% of the solution is water. In a hardware store, you can buy industrial strength vinegar, which is 30% concentration. This means that 30% of the vinegar is acetic acid, and the remaining 70% is water. Samuel does another experiment, this time with 5% vinegar and 30% vinegar. He sets up two science fair volcanoes (in no particular order), each with the same temperature, mass of baking soda and volume of vinegar. But one volcano uses 5% vinegar and the other volcano uses 30% vinegar. He measures the volume of gas production for the first minute of each reaction, and he records the data below. Volcano # 1 Volume of gas Volume of gas produced (mL) vs. Time (s) for Volcano #1 Time (s) produced (mL) 60 E 50 10 25 40 20 38 30 46 30 • Volume of gas produced (mL) 40 50 50 52 10 60 53 20 40 60 80 Time (s) Volcano # 2 Volume of gas produced (mL) vs. Time (s) for…

3. Standard white vinegar you can buy in the grocery store is 5% concentration. That means 5% of the liquid vinegar is acetic acid and 95% of the solution is water. In a hardware store, you can buy industrial strength vinegar, which is 30% concentration. This means that 30% of the vinegar is acetic acid, and the remaining 70% is water. Samuel does another experiment, this time with 5% vinegar and 30% vinegar. He sets up two science fair volcanoes (in no particular order), each with the same temperature, mass of baking soda and volume of vinegar. But one volcano uses 5% vinegar and the other volcano uses 30% vinegar. He measures the volume of gas production for the'first minute of each reaction, and he records the data below. Volcano # 1 Time Volume of gas Volume of gas produced (mL) vs. Time (s) for Volcano #1 (s) produced (mL) 60 50 10 20 30 25 38 40 46 30 • Volume of gas produced (ml) 40 50 20 50 52 e 10 60 53 20 40 60 80 Time (s) Volcano # 2 Volume of gas produced (mL) vs. Time (s)…

A mixture containing ethanol (bp: 78 °C), acetone (bp: 56 °C), and ether (bp: 36 °C) undergoes distillation. Which of the following is NOT TRUE?   a. Acetone is more volatile than ethanol but less volatile than ether. b. Ether will be the first to be collected in the receiving flask. c. Ethanol will remain in the distilling flask when the mixture is distilled at 56°C. d. Ether molecules have the strongest IMFA among the three.