Coordination Compound Synthesis Lab

An error that could have been present during the lab includes not letting the zinc react completely with the chloride ions by removing the penny too early from the solution. For instance, the percent error of this lab was 45.6%, which was determined by the subtraction of the theoretical percent of Cu 2.5% and the experimental percent of Cu 3.64% and dividing by the theoretical percent of Cu 2.5%. This experiment showed how reactants react with one another in a solution to drive a chemical reaction and the products that result from the

While the solution dissolved, 50 mL of distilled water was added to a 150 mL beaker and heated on the hot plate. When the solution started to boil 2.65 grams of Na2SiO3*5H2O was added to the beaker with a stir bar and heated to a gentle boil. When both solutions began to boil, the sodium silicate solution was slowly added to the sodium aluminate. The solution was kept at 900C for 60 minutes and stirred with stir bar. After 60 minutes, the zeolite solution was cooled for 5 minutes and for the magnetized zeolite , 0.78 grams of FeCl3 and 0.39 grams of FeSO4*7H2O was added to the flask and stirred until the iron parts dissolved.

Malachite was synthesized using the following reaction (1): 2CuSO4*5H2O(aq) + 2Na2CO3(aq) CuCO3Cu(OH)2(s) + 2Na2SO4(aq) + CO2(g) + 9H2O(l) Based on this chemical equation, two moles of aqueous hydrated copper (II) sulfate reacted with aqueous sodium carbonate, a precipitate of copper (II) carbonate hydroxide was formed along with aqueous sodium sulfate, gaseous carbon dioxide, and liquid water. The copper (II) carbonate hydroxide precipitate is also the malachite that was obtained from the solution. It was known that a chemical reaction was occurring when the copper (II) sulfate solution was mixed in with the sodium carbonate based on the fact that the color of the solution changed from blue to light blue and the solution frothed. The malachite

After that, put an aluminum wire into the beaker, and after a certain period of time the solution gains color. To finish the reaction, 5 drops of 6M of Hydrochloric acid is added into the beaker to clean the solution, which means that acid dissolves all salts of aluminum that is on the solution. After finishing the chemical process, collect and use the Butcher funnel to wash the cooper because it is going to be used to a vacuum filtration. After finishing the filtration, measure the weight of the sample and dry it. Finally, Do again these two steps until notice that the subtractions of these masses are about 0.005 g, and then arrange all the chemical

Qualitative question: Was there any CuCl2 left? There was no CuCl2 left, so the reaction went to completion. When the NH4OH was added to the solution, it did not turn blue. When NH4OH is added to a solution with copper in it, the solution should turn a cobalt blue color. However, the solution created a gel that indicates that AlCl3 was in solution, and there was minimal color change (caused by the change in the way light passes through gel).

Abstract: The purpose of this experiment was to identify given Unknown White Compound by conducting various test and learning how to use lab techniques. Tests that are used during this experiment were a flame test, ion test, pH test, and conductivity test. The results drawn from these tests confirmed the identity of the Unknown White Compound to be sodium acetate (NaC2H3O2) because there were no presence of ions and sodium has a strong persistent orange color. The compound then will be synthesized with the compounds Na2CO3 and HC2H3O2 to find percent yield.

In this lab, the hypothesis, if a chemical reaction occurs, there will be signs of a chemical change such as a change in temperature, color, and/or smell, was accepted. In each experiment, clear signs of a chemical reaction were observed. In chemical reaction #1, we put drops of vinegar onto a small pile of baking soda. The baking soda and vinegar produced bubbles of gas right as the first drop hit the baking soda, which is a clear sign that there was a chemical change occurring. This can be classified as a double replacement chemical reaction.

Then 2.0-g solid KI was added and allowed to completely dissolve. Then 50.00-mL of KIO3 was added to the flask. This brown solution was titrated with thiosulfate until the solution was a pale yellow. At this point, 2.0-mL of the starch indicator was added, creating a dark blue solution, and titrating was continued until the solution was colorless. This process was repeated for an additional two trials.

Long duration of heating will loosen the bond between central atom and ligands. Characteristic of acetone is to increase the formation of complex. There is error in the acetone provided thus causing the adding steps of acetone to dissolve all the complex formed in the experiment. Sodium acetate trihydrate, as a base in this experiment, causing acetylacetone to lose a proton to form acetylacetone anion, acac-. Manganese has wide range of oxidation state from +7 to -1, however, in aqueous solution, manganese with +2 oxidation state is most stable and common.

Chapter five taught about the separation of mixtures through a number of different processes. These processes use differences in characteristic properties in the elements of the mixture. For example, fractional distillation uses boiling point to separate liquid mixtures. As the liquid boils, the vapor is redirected through a tube into a different test tube and then condenses. The tube is moved into a different test tube after the first fraction concludes boiling, and then the next fraction can be extracted, etc.

Carbon dioxide and water in the solution were also clear. Once the solution was completely titrated, Mn7+ ions remained unreduced and changed the color of the solution to pink. The KMnO4 was added to each solution until the oxalate solution reached the end point and changed to an extremely light pink color. The change in volume in the burette of the potassium permanganate recorded in all three trials was used to calculate the moles of oxalate in the 0.100-gram compound, giving the percent composition of the compound. The three trials reacted 27.95 mL, 26.61 mL, and 25.74 mL of potassium permanganate to determine 55.7%, 53.0%, and 51.3% respectively of oxalate in the compound with a 53.3% average.

First, 50 mL of the sample was placed into a 250 mL Erlenmeyer flask, and onto a stirring plate. Then, the pH of the solution was measured and adjusted to be within the range of 4 and 6, using nitric acid and sodium hydroxide. After the pH was optimal for the experiment, a single mL of indicator- acidifier reagent was added to the sample. Then, 50 mL of mercuric nitrate was place into a burette and titrated with the sample until the color of the solution turned from blue to purple. The volume of titrant used for the reaction to reach endpoint was recorded.

Norah Albaiz CHMY143-016 Katie Link Lab Partner: Lydia Aman Standardization of Acids and Bases Purpose: The purpose of this experiment was to determine the unknown concentrations of NaOH, HCl, H2SO4, Ba(OH)2 by using a technique called titration. Titration is where the titrant is added from a buret to a known quantity of an analyte until the reaction is complete. Acid-base titration techniques can help determine the unknown concentrations of the analytes.

She looked at different diamine ligands and trying to make them with butane diones and different anilines. She reacted her ligands with iron (II) chloride and found that her ligands immediately turned brown when exposed to the air because they were air sensitive.

Chemical Engineering School of Engineering and Physical Sciences FIRST YEAR LABORATORY REPORT COVER SHEET Name: Farid Mustafayev Experiment Title: Acids and Basis: Determination of Concentration Using Titration Date of Experiment: Demonstrator: Sevda Zargarova Supervisor: Ziyafaddin Asadov   Contents