4.1 REACTIVE EXTRACTION
DESCRIPTION
A simple reaction, followed by isolation of the desired product from the solution, will give a example of a typical application of extraction.
Few organic acids are liquid and soluble in water. Sodium salts of carbon organic acids are ionic compounds that are also very soluble in water. If an aqueous solution of one such salt is acidified with a strong mineral acid, the much weaker organic acid is produced.
Weak organic acid is largely un-ionized in the aqueous solution.
No change is observed when the reaction is carried out because the solutions of the starting materials and the products are colorless. The organic acid is soluble in water and thus, does not separate. It is necessary to extract the propionic acid from the aqueous solution with solvent. The solvent solution must be dried to remove residual water, following which
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Dissolve the salt in 120 ml of tap water. Add 60 ml 6 M Hcl and stir the mixture with a glass rod.
Add 24 g solid Nacl to the solution and stir the mixture for about 2 minutes.
Support a 500 ml separatory funnel on a ring, close stopcock and then a clean beaker is placed beneath the exit tube. Transfer the aqueous solution from the beaker to the separatory funnel. Do not transfer any un-dissolved sodium chloride in the beaker to the funnel.
Extract the aqueous solution with selected solvent in the following manner:
a) Add 40 ml of solvent to the solution in the separatory funnel.
b) Place the plastic stopper in the neck of the funnel. Shake
c) Slowly remove the lower aqueous layer through the stopcock into the same 500 ml beaker in which the solution is there.
d) Pour the upper solvent layer through the neck of the funnel into a clean 125 ml Erlenmeyer flask.
Return the aqueous solution from the 500 ml beaker to the separatory funnel. Add another fresh 40 ml of solvent to the funnel and again extract the aqueous solution as you did in b)
Next, about 10 mL of both solutions, Red 40 and Blue 1, were added to a small beaker. The concentration of the stock solution were recorded, 52.1 ppm for Red 40 and 16.6 ppm for Blue 1. Then, using the volumetric pipette, 5 mL of each solution was transferred into a 10 mL volumetric flask, labelled either R1 or B1. Deionized water was added into the flask using a pipette until the solution level reached a line which indicated 10 mL. A cap for the flask was inserted and the flask was invented a few times to completely mix the solution. Then, the volumetric pipette was rinsed with fresh deionized water and
Put the filtered liquid back into the beaker, then, clean up the Buchner funnel and filter
CaCl2 and 5 mL water, 2 tsp. CaCl2 and 2 tsp. CaCl2.The question asked at the beginning of the lab was what chemical must be present for a color change to occur. My hypothesis was that if Phenol red was present then a color change would occur. This hypothesis was true because every reaction that had phenol red experienced a dramatic color change while the other reactions did not.
Then the flask was filled the rest of the way with distilled water to the mark. Similar steps were taken for the rock solution. The rock solution from the prior lab was filtered into a volumetric flask (100mL), then 15 M NH4¬OH (8mL) was added to the flask. After that, the flask was filled to the mark with distilled water. Both flasks were then swirled to combine the solution
The converse was true for the 5% NaCl solution without Elodea and the 5% solution with Elodea (table 1). A comparative observation revealed that the beaker with Elodea in salt solution required more NaOH than did the beaker with Elodea in tap water (figure 1). Table 1. The number of drops of NaOH in each beaker Beaker Name Number of Drops Tap Water
Background Research: Isopods are group of small, cold-blooded, crustaceans also known as pillbugs and sowbugs (pillbugs are commonly known as “roly polies”). Pillbugs are almost exactly like sowbugs, but differ because they can curl up into balls and are thicker than sowbugs (PNNL). Isopods are related to a few water crustaceans including crabs, crayfish, and shrimp, so water is necessary for them to survive. For that reason, they live in damp or wet areas such as forests and meadows. Isopods have seven armour plates, called “pereonites,” that serve as protection from predators and have seven pairs of legs.
Mixture Separation October 6, 2015 Sasha Crowley Harrison Rossi Purpose The purpose of the laboratory was to determine the physical properties of four substances, then to separate a mixture of the substances based on their physical properties with limited amounts of materials available. Hypothesis
When baking soda and acetic acid were mixed, the mixture bubbled up and the foam rose up from a quarter of to the midpoint of the test tube. The mixture bubbling up suggest that gas is being released. Therefore, this is a chemical reaction. Another example of a chemical reaction is when cornstarch was mixed with water and iodine solution, After cornstarch was mixed water, the mixture was mixed with iodine solution. When the iodine solution was added, the mixture went from cloudy white to dark purple.
Observations: 1. The first step had to be repeated due to not following proper instructions. I did not grease the screw, so as I was shaking the mixture, solids were forming around the screwpart of the separatory funnel. 2. When adding 5.0 mL of NaOH to the unknown mixture and shaking it for about 30 seconds, layers had formed.
= 10^-3 M = 1,000 mL Here C1,C2; are the first and second concentrations of solution V1 and V2 ; are the required and current volumes. The impeller turned on and DDA, and tap water left to be mixed properly with water for 2 minutes. Approximately 150 grams of quartz added into the solution.
Weighed 1 gram of NaC2H3O2 and mixed it with ionized water. Boiled 12 mL of 1.0M Acetic Acid added into a beaker containing the sodium carbonate on a hot plate until all the liquid is evaporated
Therefore, we added 1.11g of CaCl₂ and 1.06g of NaCO₃ to a beaker filled with 70mL of distilled water. To separate the precipitate from the aqueous solution, we vacuum filtrated the contents of the beaker. Once we determined that the
Acids are proton donors in chemical reactions which increase the number of hydrogen ions in a solution while bases are proton acceptors in reactions which reduce the number of hydrogen ions in a solution. Therefore, an acidic solution has more hydrogen ions than a basic solution; and basic solution has more hydroxide ions than an acidic solution. Acid substances taste sour. They have a pH lower than 7 and turns blue litmus paper into red. Meanwhile, bases are slippery and taste bitter.
The solvents that were used in this particular experiment included the likes of - n – hexane, Cyclohexane, cyclohexanol and Cyclohexyl acetate. Further they also reported the distribution coefficient and separation factors. When the two phase region was considered, n hexane and Cyclohexane proved to be suitable agents for establishment of equilibrium data of propionic acid-water-solvent mix. On the other hand, when distribution coefficient values were considered it was shown that Cyclohexyl acetate is most suitable. In conclusion, when all the properties were taken into consideration it could be concluded that cyclohexyl acetate is the most suitable extracting agent that was studied is this research.
Once dissolved, fill the rest of the volumetric flask up to the line on the neck of the flask. Again mix the solution. Use four, 10mL volumetric flask, and label them from 1-4. Add approximately 2mL of copper sulfate pentahydrate into flask 1, 4mL to flask 2,