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Coordination Compound Synthesis Lab

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The main purpose of the following experiment is to produce a coordination compound that contains the oxalate ligand, and to determine the number of each ion in the KaFeb(ox)c·dH2O formula. In this case, the oxalate is a bidentate ligand which essentially chelates to the iron atom through two points (1). First discovered in the early 18th century by the Alfred Werner, the concept of coordination compounds was not grasped until after 200 years passed (3). Coordination compounds are composed of a central metal, ligands that bind with the metal, and oftentimes counterions. The combination of the complex ion and the counterions form a coordination compound. Subsequently, Coordination compounds are prominent and vital to biological life because of their various applications. They can …show more content…

This was possible because the mixture of potassium oxalate and iron (III) chloride is not soluble in water. This product created a precipitate, which resulted in a green crystallized product. The crystal precipitate was then isolated from the rest of the liquid substance and dried to determine the percent composition to determine the formula. The second day of the coordination compound synthesis lab consisted of performing titrations and then determining the mass of oxalate (ox) (2). An ion-exchange technique was then used to find the amount of potassium and iron (III) in the compound. Ion-exchange columns are prominent in research labs to target and remove certain ions from a solution or mixture (2). Essentially, an ion exchange column will exchange the K+ with the H+ ions and will result in a solution of hydrogen ions and the iron-oxalate anion. After this, an acid-base titration will be conducted. The hypothesis of this lab is that the creation of a coordination compound can help determine an unknown formula by determining the percent composition and conducting titration of the ions present in the

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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.

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554 Words | 3 Pages

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

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1049 Words | 5 Pages

The pseudo-first order rate constants increase with increases in [PDTS]. Plots of 1 / kobs versus 1 / [PPDTS]2 are linear with positive slopes and positive intercepts (Figure 2) confirming the formation of 1:2 complex between Fe(III) and PPDTS. Effect of hydrogen ion It has been observed that these reactions are decelerated by hydrogen ion. Kinetic runs were performed at different [H+], keeping the concentrations of Fe(III), PPDTS and PABAH / PCBAH constant and the pseudo-first order rate constants were evaluated (Figure 3).

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177 Words | 1 Pages

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

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383 Words | 2 Pages

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.

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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.

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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.

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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.

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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).

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806 Words | 4 Pages

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.

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I taught, as the sole instructor, a variety of undergraduate courses including analytical chemistry, an analytical chemistry laboratory, fundamental chemistry and advanced inorganic chemistry at the China Agricultural University. At Dalhousie University, I served as a teaching associate for

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1582 Words | 7 Pages

It is important to recognize the nature of the ligand – the availability for coordination sites or ligating and the conditions under which these are available for coordination. Complexes can be positively charged, neutral or negatively charged. The overall charge on the complex is depends on the oxidation state of the metal

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1931 Words | 8 Pages

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.

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1116 Words | 5 Pages

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.

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1346 Words | 6 Pages

Practical I: Acid-base equilibrium & pH of solutions Aims/Objectives: 1. To determine the pH range where the indicator changes colour. 2. To identify the suitable indicators for different titrations. 3.

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