PURPOSE The purpose of this experiment is to become familiar with the separation of mixtures of solid and learn separation techniques based on the chemical properties of a substance.
PROCEDURES
1. Separating out the Iron
a. Use your digital scale to determine the mass of your weighing dish.
b. Empty the entire mixture of solids from the plastic bag into the weighing dish and determine the gross mass of the total mixture and weighing dish. Compute the net mass of the mixture: this is equal to the gross mass of the weighing dish with the mixture less the mass of just the weighing dish determined in 1-A.
c. Spread the mixture into a very thin layer over a full sized piece of paper.
d. Cut a second piece of paper into a 10-cm square.
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5. Cleanup: Thoroughly clean, rinse, and dry all equipment and return it to the LabPaq. Throw all used paper cups and paper towels in the trash.
OBSERVATIONS, DATA, AND CALCULATIONS
Part 1
Mass of weighing dish = 0.5g
Total mixture = 7.5g
Net mass of mixture = 6.8g
Piece of paper = 0.8g
Iron fillings + paper = 2.7g
Net mass of Iron fillings = 1.9g
Part 2
Net mass of sand = 2.0g
Part 3
Paper cup mass = 6.2g
Filter paper = 1.0g
Filter paper + benzoic acid = 2.7g
Net mass of benzoic acid = 1.7g
Part 4
Paper cup + salt = 7.1g
Net mass of salt = 0.9g
Data Table 1: Experiment Data Grams Percent of mixture
Iron filings 1.9 27.94 %
Sand 2.0 29.41 %
Table salt 0.9 11.76 %
Benzoic acid 1.7 25.00 %
Total 6.5 95.59 %
QUESTIONS
A. How did your proposed procedures or flow charts at the beginning of this experiment compare to the actual procedures of this lab exercise?
It was similar to the procedure described. The only difference was the last step when separating out the Table Salt. I had proposed that we would have to heat the mixture instead of letting it evaporate.
B. Discuss potential advantages or disadvantages of your proposed procedure compared to the one actually used.
If heated, the salt and water mixture would not have formed any crystals and there would be a chance
1. Capillary action will draw the salt solution up the paper. As it passes through the dots, it will begin to separate the dyes. When the salt water is 1/4 inch (0.5 cm) from the top edge of the paper, remove it from the glass and place it on a clean, flat surface to dry.
Experiment 55 consists of devising a separation and purification scheme for a three component mixture. The overall objective is to isolate in pure form two of the three compounds. This was done using extraction, solubility, crystallization and vacuum filtration. The experiment was carried out two times, both of which were successful.
If I were given the opportunity to repeat the experiment these are the parts of it that I would change:
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There are millions of different organic compounds. Most of them are found in mixtures and in order to achieve a pure form they need to be separated, isolated, and purified. However, there are endless numbers of possible mixtures, which make it impossible to have a pre-designed procedure for every mixture. So chemists often have to make their own procedures. The purpose of this experiment was to prepare the student to the real world by them designing their own procedure which will help them understand the techniques of separation and purification better. The goal was to extract two of the components of the
The objective of this extraction experiment was to achieve a comprehensive understanding, as well as master the practice, of the technique of separating various individual components of a compound.
Evaluate how implementing best practices would have reduced the chances for failure. Provide support for your rationale.
To understand the different separation methods and techniques that depend on the chemical properties of a specific substance. Also to become more comfortable with performing those actions of separation so I have them in the future. For this experiment, I will separate a mixture of four distinct substances: sodium chloride, benzoic acid, silicon dioxide, and iron fillings into pure beings.
To tube 2 and tube 3 a boiling chip is added. The two tubes are boiled to remove any residual ether. Next, the tubes are cooled to room temperature and placed into an ice bath to allow for crystallization. The solution is then removed from the solid in each tube and discarded. To tube 2 and 3 ~0.5 ml of H2O is added for recrystallization, the tubes
The purpose of this experiment is to familiarize oneself with the general procedures determining a partition coefficient at the microscale level and learn in weighing milligram quantities of materials on an electronic balance, the use of automatic pipets, the use of transfer pipet, and the use of a vortex mixer. Also, to familiarize oneself with extraction
After cooled down a little, mix with a glass stirring rod until sample is uniform in texture and appearance, then re-weigh the sample.
The purpose of this experiment was to use solvent extraction techniques in order to separate a mixture consisting of a carboxylic acid (p-toulic acid), a phenol (p-tert-butylphenol), and a neutral compound (acetanilide). Extraction is the process of selectively dissolving one or more of the compounds of a mixture into an appropriate solvent, the solution that contains these dissolved compounds is called an extract (Manion, 2004).
precipitate; then pour over the solid in the funnel. Finally, pour two 10-mL portions of
eliminate water within the mixture and to form the desired paper thickness. The material then proceeds to a drying
1. Obtain a sample of the mixture. The mixture you will separate contains three components: NaCl, NH4Cl, and SiO2. Their separation will be accomplished by heating the mixture to sub-lime the NH4Cl, extracting the NaCl with water, and drying the remaining SiO2.