Geometric Isomers Post Lab Report

The dialysis bag experiment resulted with beaker one having relatively similar numbers, showing as an isotonic medium. Beaker two’s solution gradually increased within an hour which caused the product to

tube was placed inside, then another test tube with an equal amount of substance would be placed

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.

Maleic acid and fumaric acid have different molecular structure. Maleic acid has a lower melting point than Fumaric acid which has a higher melting point. The reason why is because maleic acid has intramolecular forces, being a cis isomer, which causes it to have weak bonds. This causes it to be easily broken when energy is put in. On the other hand, fumaric acid has intermolecular forces, being a trans isomer, which has stronger bonds. This is harder for bonds to break because of how far apart the carboxylic acid groups are. In addition, maleic acid is more soluble than fumaric acid. Maleic acid has hydrogen bonding due to its intermolecular forces. This causes it to be attracted to water and dissolve. While fumaric acid does not have any hydrogen bonding because of its intramolecular forces which makes it harder for fumaric acid to dissolve in water because it fumaric acid is not attracted to

We were also able to conclude that when you combine equal parts of an acid and base you can expect to see a higher temperature change than you would if you added more parts of a base than a acid. Our reasoning behind this conclusion is that when we added 10 mL of both solutions that temperature increased by 5ºc, but when we added 15 mL of NaOH and only 5 mL of CH3COOH there was only a temperature increase of 3ºc. In correlation, we calculated that when you have equal parts of acid and base, the ΔHrxn will be higher than when you use more parts base than

The next step in this lab is to rinse the Erlenmeyer flask with distilled water down the drain and then repeat the experiment, this time adding 10 ml of 0.10M KI and 10 ml of distilled water to the flask instead. The flask should again be swirling to allow the solution to succumb to the same temperature as the water bath and once it has reached the same temperature, 10 ml of 3% H2O2 must then be added and a stopper must be immediately placed on the flask and recording should then begin for experiment two. After recording the times, the Erlenmeyer flask must then be rinsed again with distilled water down the drain. After rinsing the flask, the last part of the lab can now be performed. Experiment three is performed the same way, but instead, 20 ml of 0.10 ml M KI and 5 ml of distilled water will be added and after the swirling of the flask, 5 ml of 3% H2O2 will be added. After the times have been recorded, data collection should now be complete.

Discussion: As seen in the melting point determination, the average melting point range of the product was 172.2-185.3ºC. The melting points of the possible products are listed as 101ºC for o-methoxybenzoic acid, 110ºC for m- methoxybenzoic acid, and 185ºC for p- methoxybenzoic acid. As the melting point of the sample

Starting with 8.03 grams of maleic anhydride crystals, the students successfully converted them into two isomers of butenedioic acid. From the experiment, the students learned that maleic acid converts to fumaric acid in the presence of a proton. Little occurred during the reaction between the maleic anhydride and water. The solution remained clear during the heating. Moreover, all the crystals produced during the experiment are white and brittle. Furthermore, the students obtained 6.09 grams of maleic acid, the crystals produced in the first part of the lab and 0.90 grams of fumaric acid, the crystals produced in the second part of the lab. During the melting point test, the crystals of maleic acid begin melting at 121oC and fully melted

Identifying this organic acid was an extensive task that involved several different experiments. Firstly, the melting point had to be determined. Since melting point can be determined to an almost exact degree, finding a close melting point of the specific unknown can accurately point to the identification of the acid. In this case the best melting point

The volume of a small test tube and a thin-stemmed pipet were determined in this section of the lab. Water was poured into a small test tube until the water reached the very top edge of the test tube. The test tube was then emptied into a plastic 25 mL graduated cylinder and volume was measured and recorded into data table 3. A think-stemmed pipet was completely filled with water. Drops were carefully counted and emptied into the empty plastic 25 mL graduated cylinder until the water level reached 1 mL. The number of drops in 1 mL was recorded into data table 3. The thin-stemmed pipet had a total volume of 4 mL and that was also recorded into data table 3.

Pre-test 1: The same amount of water is poured into two standard beakers and the child is asked to determine if the beakers have the same amount of water. If the child determines that the amount of water is the same, the study will continue. If not, the child cannot be used for this study.

In the experiment, the majority of the times tested, the concentration of KMnO4 in the water had increased from the previous time it had been tested. But, in a few circumstances

Overall the test was fair as many of the variables were kept the same and controlled. The independent variable was kept the same and the dependant variable was recorded every time.

Prepare 11 different solutions of water and isopropanol (IPA) each with a total mole content of 0.556 mol. The mass of each compound should be measured analytically. Use a high-precision adjustable volumetric pipette to accurately measure the volume of each solution. Determine the mole fraction of IPA for each solutions then plot the total volume against the calculated values. If the resulting plot is perfectly linear, then the solution behaves ideally; otherwise it behaves like a ‘real

The objectives of this lab are, as follows; to understand what occurs at the molecular level when a substance melts; to understand the primary purpose of melting point data; to demonstrate the technique for obtaining the melting point of an organic substance; and to explain the effect of impurities on the melting point of a substance. Through the experimentation of three substances, tetracosane, 1-tetradecanol and a mixture of the two, observations can be made in reference to melting point concerning polarity, molecular weight and purity of the substance. When comparing the two substances, it is evident that heavy molecule weight of tetracosane allowed