Paper Chromatography Lab Report

7. Tape the strip to a pencil and rest the pencil on top of the jar so that the strip hangs into the jar. The goal is to have the end of the chromatography strip just touching the surface of the solvent solution, with the colored dots above the surface of the liquid. Make sure that the colored spots do not come in direct contact with the liquid in the bottom of the glass.

This Lab Report is an analysis of the results of a two-part experiment. In the first part, we used a gel filtration column to separate the components of a mixture composed of protein and non-protein molecules. By doing so we hoped to obtain fractions that contained single components of the mixture, while also gaining insight into the relative molecular weight of each component compared to each other. We would then plot these fractions onto nitrocellulose paper in order to determine which fractions had protein. In the second part, we would use the fractions which we had determined had protein to conduct an SDS-PAGE. By doing so we hoped to determine an estimate on the molecular weight of the proteins present in each fraction by comparing it to a tracker dye composed of a variety of molecules of differing molecular weight.

If a sample’s Rf is lower, that means that it remained closer to the stationary phase. In both variations of the experiment, red dye #40 remained the closest to the stationary phase (on average). Therefore, the red dye #40 had the lowest rate of flow value. The intermolecular forces of the red dye are responsible for its low distance traveled. The molecules of the chromatography paper have strong intermolecular bonds that are highly polar. The red dye is attracted to the paper because of their similar characteristics. The negative and positive ends of both the paper molecules and the red dye #40 molecules attract to each other. It is extremely difficult for the isopropyl alcohol and the sodium chloride solutions to interfere with the bonds of paper and ready dye #40, as a result, both solutions are unable to fully dissolve red dye #40. . NaCl and isopropyl alcohol have very strong intermolecular forces, but the forces of the paper’s molecule were able to attract red dye #40 because they were even

For part one of this experiment, I only experienced separation of colors with the green and brown M&M’s, along with the yellow food coloring. The green M&M separated into yellow and blue, with blue travelling farther up the paper. It is not surprising that green separated into blue and yellow because those are the primary colors that make up green. The brown M&M separated into red and orange, with the orange travelling farther up the paper. Finally, the yellow food coloring separated into yellow and red, with yellow travelling farther up the paper. This could be because it was such a concentrated, small amount of food coloring. The colors that didn’t travel very far up the paper, such as orange and brown, are probably less soluble than the others, like blue and green.

Answer: Once the chromatogram has been completed and is ready to be measured and calculated, on the plate that was used to perform the chromatogram you should see where the red and blue have completely separated. The red food coloring dye should be lower on the plate than the blue food coloring dye.

The dyes in the laboratory experiment are made of numerous colors, mainly red and blue, the spectra from each of the dyes corresponded to the wavelengths obtained from each of dye i.e. 620 nm for red and 450 nm for blue.

The solutions are mixed in small amounts in cuvettes and inserted into the colorimeter, which reads the percentage transmittance during the time period. The colorimeter has an enclosed space for the cuvette to be inserted making sure light from other sources does not interfere with the reaction, hence providing accurate results. The rate of the reaction is determined by using the equation: Rate= k [CV+] [OH-], where k is the rate constant for the reaction.

Oparina/Miller hypothesis theorized was because of absence of free oxygen, chemicals, and so on could shape inorganic mixes for emerged on this planet.

Furthermore, this experiment demonstrated why and how Dichloromethane, a commonly used solvent, is used in many Organic Chemistry

As for experiment 2, the only unexpected result was that the Methylene Blue Dye only moved 4 millimeters. In theory the MB dye should have has a diameter between 13 mm and 5 mm. This fault is most likely due to an error in either measuring the diameter or in putting the drops of the dye into the agar wells.

Chromatography is a separation technique in which the mixture to be separated is dissolved in a solvent and the resulting solution, often called the mobile phase, is then passed through or over another material, the stationary phase. The separation of the original mixture depends on how strongly each component is attracted to the stationary phase. Substances that are attracted strongly to the stationary phase will be retarded and not move alone with the mobile phase. Weakly attracted substances will move more rapidly with the mobile phase.

Litmus paper will be used to test the eluent repeatedly until it is neutral to blue litmus paper. By elution with acidified methanol, the pure dye solution will be desorbed from the column. A rotary evaporator will then be used again to expel any excess solvent. 3.3 Characterization of dye extracts in terms of chemical structure,

After wearing the gloves we obtained a chromatography vial from professor and label it with my and my peer initials. We dried up the chromatography vial in fume hood and added 1 ml of chromatography solvent to the vial. Then we took a chromatography strip and measure it 1.5 cm with ruler from one end of the strip and drew a line with pencil we cut two small pieces below the pencil line to form a pointed end. We applied spinach on the strip using quarter to rub the spinach leaf on the line that we drew on the strip and put it into the chromatography vial and placed that in fume hood. We observed as the solvent was moving up the chromatography strip by capillary action. When the solvent was reached approximately 1 cm from the top of the strip then we removed the cap from the vial. We took out the strip from the vial using forceps and marked up the location of the solvent front because it evaporates quickly. We measure out the distance as well as the pigment in order to find out the rf value. Moreover we compared rf values to the one in reference list in order to identify the

The following procedure dealt with a chromatogram. The materials needed are: a pencil, safety goggles, scissors, chromatography paper strip, capillary tube, spinach plant pigment extract, test tube, cork stopper, graduated cylinder, chromatography solvent (alternative isopropyl alcohol), metric ruler, stopwatch or clock with a secondhand, hook/fashioned paperclip, paper towels, test tube rack, and mortar and pestle. First we obtained a strip of chromatography paper and cut it so it would fit inside a test tube (with it barely touching the bottom of the tube). Also, when touching the strip, touch the sides only. Then we attached (firmly) the top of the strip to a hook (or fashioned paperclip at bottom of the cork stopper). Make sure it fits in the test tube. Next we used the pencil to draw a faint line across the strip two centimeters from the bottom tip of the strip. We placed the cork and strip in place, and we put a mark on the test tube one centimeter below the top of the stopper.

As the solvent moves past the spotted mixture, two opposing forces created by the solvent and the adsorbent influence the mixture. Each component can either dissolve in the mobile solvent or remain adsorbed to the stationary adsorbent. This process generates an equilibrium, as some components are adsorbed and others are dissolved and transported with the solvent until they are readsorbed further along the plate. The different tendencies of each component to comply with the subjected forces may result in a successfully separated mixture on the plate.