Zeolites Lab

After this, the solution was poured into a volumetric flask just about to the 1dm3 line and then it was left there to cool to the same temperature as the room before filling precisely to the 1dm3 line with distilled water. The molar mass of CuSO4.5H20 was 249.5 so that means 249.5g of copper sulphate was needed to dissolve, in order to make a standard solution, into 1dm3of distilled water. Following this, a linear dilution of the CuSO4.5H2O was made in order to be used to make a calibration curve after using the colorimeter to write down the absorbance of each sample. A linear dilution is diluted with distilled water in order for it to make the concentration weaker and weaker. For this investigation, the dilutions made ranged from 0.01 to 0.1 M/l . It was essential to only make up 10cm3

The product was placed in a Craig tube and several drops of hot (100°C) solvent (50% water, 50% methanol, by volume) was added and heated until all of the crystals dissolved. The Craig tube was plugged and set in an Erlenmeyer flask to cool. Crystallization was induced once the mixture was at room temperature by scratching the inner wall of the tube. It was then placed into an ice bath for ten minutes until crystallization was complete. The tube was then

The same solution of 0.5 ml BSA was then added from test tube 1 to the test tube 2 after being properly mixed, and from test tube 2 the solution was being added to test tube 3, and so forth all the way up to test tube 5, with the same exact procedure. From the last tube, we then disposed the 0.5 ml solution. After above procedures, we now labeled another test tube “blank”; 0.5 ml blank distilled water was purred into the tube with the serial dilution of 1:10. We also had a tube C labeled “unknown” with the same 0.5 ml of solution. And after adding 5ml of Coomassie Blue to each tube (1-5) and to the blank, the result of absorbance was read at 595 nm.

Experimental Method: A filtration apparatus was set up. Solid iron(III) chloride hexahydrate was dissolved in water. In a separate container, sodium acetate trihydrate (NaC2H3O2 x 3 H2O) was also dissolved in water. Sodium acetate trihydrate was then added to iron(III) chloride. 2, 4-pentanedione (C5H8O2) was dissolved in methanol; it was then added to the iron(III) chloride/sodium acetate solution. The product of this mixture was filtered, and the precipitate

Make sure to use the same type of cuvette to keep the width consistent and to prevent any experimental error from arising. Obtain 5 of the same type of cuvettes and pre-rinse them thoroughly. Label them numbers one through five in increasing molarity. Then, fill each of the cuvettes with one of the five solutions you created back in Part A. We will first examine the solution that exhibits the highest concentration or molarity. Make sure to wipe the outside of the cuvette with a Kimwipe before placing into the SpectroVis Plus device. Observe the graph that is generated and make sure to take note where the maximum absorbance takes place.

The values of color absorbance are effective because color absorbance has a linear relationship with concentration values, which in turn, allows us to easily find concentration values for many solutions. Beer’s law describes this phenomenon since the absorbance is directly proportional to concentration. We observed that as the color absorbance increased, the concentration of the FeSCN2+ complex ion increased. This is because as the FeSCN2+ concentration increases, the blood-red color becomes darker due to more presence of the blood-red FeSCN2+ ion. Therefore, the color absorbance increases because there is more blue color absorbed by the darker red color. We then graphed the absorbance and concentration values and created a line of best fit. Using the line of best fit, we were able to predict the equilibrium concentrations of the FeSCN2+ solutions and find the change required to reach equilibrium. Since we already knew the initial concentration of FeSCN2+ and since we already found the equilibrium concentration of FeSCN2+, we can calculate the change in equilibrium. Using this data, we were able to calculate the equilibrium concentration of all of the species in this lab, since we already knew the change from the initial concentration to the equilibrium change. Q is less than K because there was no initial concentration of FeSCN2+, but after the system reached

Where A is the initial absorbance when the experiment first starts, l is the path length of the cuvette (2.54 cm), and [CV]t is the initial concentration of crystal violet.

From that point, the oxalate solution was added to the iron (III) chloride solution in the 150 mL beaker and stirred. To ensure the highest percent yield, any remaining K2C2O4 was rinsed with 3 mL of DI water and added to the 150 mL beaker. After all solutions were

Apparatus: Spectrophotometer (UV-1201), cuvettes, water bath (set at 37°C), 200µl and 1000µl micropipettes and test tube

In this experiment 10 cuvettes were filled with the appropriate dilution, an additional cuvette should be filled with distilled water which should be used to calibrate the colorimeter. Record the absorbance and transmittance for each dilution generated from the Webquest. Additionally, two samples of Gatorade contains Blue Dye #1 (Low Calorie and Glacial Frost) were tested and found that the Low Calorie Gatorade had an absorbance of .135 and the absorbance of the Glacial Frost Gatorade was .153. Using linear regression the concentration of the two samples can be found if the value of transmittance is substituted for the Y value. The concentration of sample 1 is 62.8 µM and the concentration of sample 2 is 69.68 µM respectively reporting in four significant

The solutions were then transferred to 5 cuvettes that had previously been labeled 1-5 and subsequently covered with a 1.2 X 7 cm strip of parafilm wax. This was used to prevent any possible spills from occurring. Once this was completed, the first cuvette was taken and the percent transmittance was measured using the spectrophotometer. This will acted as the initial percent for each cuvette as well as the control to compare the other cuvettes to once the experiment was

Incorporation of assay controls included setting up a spectrophotomer and running the chart recorder with a full-scale deflection before the start of the assay. The set recorder had a corresponding value of 1 for the change in the absorbance. Therefore, prior testing was done to observe whether a change occurred in the readings. This helped to indicate that the results were valid, as they could have been affected by a fault during the setting up of the spectrophotometer. On the other hand this was considered as one of the controls for the experiment. Nevertheless, a new cuvette had to be used for each assay.

We repeat this process with the next corresponding wavelength, which would be at 490,500,510,520,525,530,535,540,545,550,555,560,565,570,575,580,585,590,600,610,620 nm. After we finish recording all of our data points for absorbance level at these various wavelength for oxyhemoglobin. We prepare our third cuvette tube with the same oxyhemoglobin solution, while at the same time add the reducing agent NaSH, into that same cuvette and waited approximately 15 minutes for it to take affect.

The temperature of the bath was initially set at 30°C.Using acrylic sheet containing a hole at the center, the beaker was closed through which a spindle from an electric motor placed on the top of the sheet was introduced into the solution. For stirring the solution,at the end of the rod, a Teflon paddle was attached. The saturation of the solution was confirmed by adding the synthesized salt in small amounts and using a motorized stirrer the solution was stirred which was continued till the formation of precipitate. Throughout the entire volume of the solution the stirring confirmed to have a uniform temperature and concentration. Gravimetrically, the equilibrium concentration of the solution was analyzed after attainment of saturation.

Once cooled, the mixture was then transferred to a separatory funnel using the funnel while avoiding adding the boiling chip. 10 ml of water was then added to the mixture. The mixture was gently shaken and the phases were allowed to separate. The funnel was then unstopped and the lower aqueous phase was drained into a beaker. 5 ml of 5% aqueous NaHCO3 was added and then shaken gently. A great deal of caution was taken into consideration because of the production of carbon dioxide gas which caused pressure to develop inside the funnel. The pressure needed to be released so the funnel was vented frequently. The phases were allowed to separate and the lower aqueous phases was drained into the beaker. After draining, 5 ml of saturated NaCl was added to the funnel and then shaken gently. Once again, the phases were allowed to separate and the lower aqueous phase was drained into a beaker. An ester product was produced and was transferred into a 25 ml Erlenmeyer flask. This organic product was then dried over anhydrous Na2SO4 to trap small amounts of water in its crystal lattices thus removing it from the product. Finally the ester was decanted, so that the drying agent was excluded from the final product.