Ion Exchange Chromatography Lab Report

Different procedures were used to isolate benzil from the ether layer and benzoic acid from the aqueous layers. To isolate benzil, anhydrous MgSO4 was added to the flask containing the ether layer solution. MgSO4 removes the remaining water in the ether layer solution. After making sure that enough amount of MgSO4 present in the solution, the ether solution was filtered by using gravity filtration. During filtration, MgSO4 was removed from the solution and the ether solution was collected in 25 ml flask. To separate benzil from the filtered ether solution, the beaker containing the ether solution was heated until the ether evaporated. After letting the beaker to cool to room temperature, the mass of the beaker with the benzil crystals was measured. From the combined mass of the beaker and the benzil crystals and from the predetermined mass of the beaker, the mass of the collected crystals was calculated to be 0.266 gram.

The purpose of this experiment is to practice common organic laboratory techniques inside the lab to get one oriented to the basic methods of procedure that can be used for later experiments. This experiment involves the separation of benzoic acid from a more crude form, consisting of benzoic acid, methyl orange, a common acid/base indicator, and cellulose, a natural polymer of glucose (Huston, and Liu 17-24). The technique that is used to perform this separation is called extraction. Extraction is a systematic process of separating mixtures of compounds, taking advantage of the affinity differences of compounds to separate them (Padias 128-37). This technique recognizes the principle that “like dissolves in like,” that is,

After about 1 minute of shaking, the two layers separated. The organic layer on the top layer (consisted of ethyl acetate and naphthalene) collected for further experiment; by adding Sodium Sulfate into organic phase and filtering the Na2So4 from the solution using the wool. The dried organic layer was weighed to get its mass and the residue of Na2SO4 were rinsed with ethyl acetate under vacuum (rotary evaporator). The acid extract on the bottom layer which is a combination of benzoic acid and NaOH were collected in the 50 mL Erlenmeyer beaker for the recovery of acid.

The solvent that was chosen for the experiment is a polar aprotic solvent that can be used to stabilize charge. This stabilization can also be used to stabilize an ionic transition state. This stabilization of the transition state along with the nature of the products based on the chemical properties would encourage the reaction to proceed toward the N-ethylsaccharin product. This product is more stable

Again, label 7 1.5ml tubes 0 thru 6. Place 15μl of each serially diluted extract into its corresponding labeled tube. Next add 465μl of media into each tube. Then 60μl of Alamar blue in each tube. Finally add an additional 60μl of cells (adjusted to 10,000 cells/20 μl). Vortex each tube for 5 seconds. Now, take 3 different samples 190μl samples of concentration 0 and put it in Wells A2, B2, and C2. Repeat this step again by taking 3 more different 190μl samples of concentration 1 and putting it in wells A3, B3, C3. It should be noted that it is important to vortex each 1.5μl tube again be-fore putting it into the 96 well plate. Contin-ue this same procedure consecutively for the re-maining concentrations.

Table 2: Consists of color extract taken from a red cabbage for a natural indicator. The pH reading that was measured by using the pH meter and the result of the pH reading to determine whether the solution was acidic or basic.

Repeat steps 3-4: Fill 1 tube with 50% NaCl. Weigh each of the tubes/cells. Record on the chart. 3. Label a 500mL beaker with 50% NaCl and fill it with 400mL of the 50% NaCl solution.

Repeat steps 4–11 two more times. Be sure to record your observations in the data tables in your lab notebooks, in the rows for trials 2 and 3. (Can you separate the dyes of grape soda using space sand?). The entirety of the Procedures.

This experiment examined the use of a liquid-liquid extraction – a method based on the solubility differences between organic compounds in two immiscible liquids. The compound of interest will be found in the liquid phase that it has a higher affinity for. This experiment relied on the fact that once an organic compound is converted into its ionic form it became soluble in polar solvents – water, in this case. It should also be noted that non-polar organic compounds would not be soluble in the aqueous (water) phase but would be soluble in the organic phase (ethyl acetate). The following are examples of the relevant acid-base reactions for the two unknown organic substances identified in this experiment based on the fact that unknown #2 was

Before being able to find the unknown ions inside the solution provided by the teacher, the ions needed to be examined for any physical or chemical changes to ensure the confirmation of each one. There were three separate sections to this lab, each one containing the same fifteen steps that needed to be followed to identify every ion. In the first part, the ions were given labeled in their original containers and divided into separate test tubes. Each ion was tested with the steps leading to their confirmation. Things such as color change or the formation of a precipitate signified a chemical reaction that confirmed the presence of an ion. This was used to give a better perspective on what would happen during the "real" lab procedure

Purpose: To accomplish this experiment, firstly will be analyzed a solution that contains six known cations and then, will be analyzed an unknown solution with the purpose of discovering the cations present on it. For this experiment will be conducted a qualitative analysis on the solution to identify the substances presents on the solution. In addition, this experiment will endow ones with a different perception about the nature of ions. Chemicals and Materials Required: Materials: 8 test tubes (12 × 75 mm), stirring rods, test tube holder, centrifuge, test tube rack, spatula, hot Plate, red Litmus paper, 400 mL beaker, blue Litmus paper, 100 mL beaker, Capillary pipet, and 250 mL beaker.

Pour 10 ml of the affinity gel into the column. Allow a few minutes for the solution to harden and transform into a gel-like consistency.

The main goals of the experiment are to be aware of the ionic compound by comprehending of the principle of solubility. Then to be acquainted of the solubility rules because it’s important to design combination of a various compounds . After that, detach the solid product to see the final solution. However, in this experiment we have been used several material, such as, BaSO4, Zn(OH)2, Al(OH)3, and NaCl to discuss what will be the final compound. On the other hand, now we can define the Ionic compound, as a common, yet distinctive type of a chemical compound, and it’s a compound, which created by ions bonding with each other through electrostatic forces. However, the acid base reaction includes the transfer of hydrogen ions; in general, we

Ion-exchange chromatography is a separation technique that separates molecules and ions based on their overall net charge (1,6). It can be used to separate amino acids, proteins, and

Gel-Filtration Chromatography is a commonly used method used in order purify a protein from a mixture, by means of separations. Different biomolecules differ in size, or their molecular weight. In the gel matrix inside the chromatography column, there are gel beads which are porous to allow certain sized molecules to enter. The molecules that are able to enter the pores of the gel, are held in stationary phase and will elute from the column later on, these are usually smaller, to medium sized molecules. Larger molecules that are not able to fit in the pores will elute out of the column first, they are involved in mobile phase where they just go straight through the column without interacting with the gel beads. Smaller molecules will have a higher elution volume, while the larger molecules will have a lower elution volume. The volume to elute the protein is inversely proportional to the molecules size.