Aluminum Synthesis Lab Report

For example, silver nitrate formed a white precipitate when it was tested with ammonium chloride. In contrast, unknown 3 did not formed any precipitate with ammonium chloride. Ammonium chloride change the color of unknown 3 to a light green while the solution of silver nitrate and ammonium chloride was cloudy white solution. Likewise, the metal in unknown 3 could have been Calcium neither. Data and observation shows that calcium nitrate whether formed a white precipitate or did not react at all while unknown 3 formed an orange precipitate. Therefore, silver and calcium are not the two metal present in unknown

Many signs show that a chemical reaction has occurred. Some ways we know there is a chemical reaction are the formation of gas, formation of precipitate, change in temperature, and,or change in color. In part one of the experiment, we know there was a chemical change because of the formation of the white precipitate. We poured the ammonia and water in the flask with alum and water, forming a white, cloudy substance in between the two liquids. The white, cloudy substance between the two is liquids is also known as aluminum hydroxide. The second part of the experiment was very similar to the first, but in the second part we mixed epon salt, water, and ammonia. The precipitate formed from mixing the epson salt, water, and ammonia was called magnesium hydroxide.

When the red Co(NO3)2*6H2O crystal was added to the white NH4 crystal, and water was added to dissolve, the solution turned blue in color. As the solution was nixed, the color changed to that of a blue-purple and a blue precipitate formed. When the 6 M NH3 began to be added, the color shifted to dark purple color after 15 mL of ammonia and the amount of the precipitate was less. After 20 mL of ammonia, the solution became a red brown with very little of the blue precipitate. After 30 mL of ammonia, the solution was similar in color to an iodine solution, a dark brown-red, almost black in color. At this point there was no visible precipitate on the surface of the solution. After 40 mL of the ammonia had been added, the solution was the same iodine like color as before. When closely examined, there was a black precipitate that had settled on the bottom of the beaker. At this point, hydrogen peroxide, 3% H2O2, was added to solution. After 4 mL of the H2O2 was added, the solution was the same color and the precipitate had not changes. After 8 mL of the H2O2, there was not noticeable change. After 12 mL of the H2O2, the solution was slightly redder in color but the precipitate had not changed. After 15 mL of H2O2, the solution was the same color and no changes had occurred to the precipitate. At 17 mL, the solution began to effervesce slightly, though there

The objective of this lab was to use prior knowledge about the Law of Conservation of Matter and of different types of chemical reactions in order to evaluate if aluminum disappears during the reaction and copper appears. The reaction that occurred between Copper (II) Chloride and aluminum was a single replacement reaction. Clear signs that a chemical reaction took place include heat release/temperature change, color change, and formation of a precipitate. When a single element, in this instance aluminum, replaces another element in a compound, copper, a single replacement reaction occurs. A basic formula for these reactions is AB + C → AC + B.

3CuCl2 reacts with 2AlCl3 to create 2AlCl3 and 3Cu. CuCl was the limiting reactant in this lab. The CuCl can only make a specific amount of copper therefore, limits the amount produced and means Al is the excess reactant.

From the start I had determined which one was NH3 just but the strong smell. I then put drops of NH3 into the rest of the solutions on the spot plates and determined the following reactions with Mn, Co, Cu, Zn, and Mg which occurred in the following reactions. Mn: Mn2+(aq) + 2NH3(aq) + 2H2O(l) < ==> Mn(OH)2(s) + 2NH4+(aq), which looks like a white gelatinous precipitate that oxidizes to brown.

Before placing the Aluminum foil into the Copper Chloride Water (CuCl2 + H2O), I had examined the characteristics of the aluminum foil. It came to view that the Aluminum foil was a silver-coloured, shiny metal. When the aluminum foil was placed into the CuCl2 Water solution, several observations were made.

Feasibility Study of Producing Potassium Alum via Aluminum Foil Lujia Cheng and Shalin Presgraves CHEM 1065, Experiment No.5, October 11, 2016 Abstract. Alum is one of the oldest and the most explored substance in human history. Dozens of ways were discovered to produce it. One way of synthesizing potassium alum was covered in this report.

This lab mainly focused on presenting 10 elements (2 unknown) that could be analyzed and then grouped together predominantly by metallic character. Each element was observed thoroughly and the findings can be seen in the above data table. By viewing the periodic table and observations, each element was labeled as either a metal, nonmetal, or metalloid, providing insight towards each element's physical properties and behavior with the two solutions, hydrochloric acid and copper chloride. The nonmetals, sulfur and carbon, did not undergo a chemical reaction with either solution.

One change that demonstrates a positive test in this lab is precipitate forming. If silver nitrate solution is mixed with a substance and a precipitate forms, chloride ions must be present in that substance. Another change the demonstrates a positive test in this lab is a colour change to a dark red colour. If potassium thiocyanate is mixed with a substance and the colour of the substance changes to dark red, Iron (III) ions must be present in the substance. Why do you think chemical tests, similar to tests used in this investigation are called

Aluminum isopropoxide (Al(-O-i-Pr)3) and aluminum nitrate nonahydrate (ANN) were used as alumina sources and tetra ethyl orthosilicate (TEOS) as a silica source. Mullite precursor gel solution was prepared by dissolving stoichiometric amounts of aluminium isopropoxide and TEOS in the aqueous solution of aluminium nitrate nonahydrate and stirring it vigorously for 2 hours. The molar ratio of Al(-O-i-Pr)3/Al(NO3)3.9H2O was kept at 7:2 in order to form spinnable sols and the mole ratio of Al/Si was 3:1. Moreover, pH of the solution was also maintained at 5. By adding aqueous solution of five concentrations of thecopper salts- 0.4 M, 0.6 M, 0.8 M, 1.0 M, and 1.2 M to the original solution and stirring it for 90 minutes, doped solutions were prepared.

To begin the experiment and start the process of narrowing down the list of twenty-five compounds, a Tollens’ test was performed on the chosen unknown (Unknown #6). In a test tube, 1 mL of 0.3 M AgNO3 was added along with 0.5 mL of 3 M NaOH. To that, 2 M NH4OH was added dropwise until the brown silver oxide precipitate dissolved. After, one drop of the unknown was introduced to the mixture, the tube was shaken and left to sit at room temperature for ten minutes. The predicted silver mirror coloration did not appear indicating a negative test result.

In this experiment, alum was synthesized from aluminum. The goal was to calculate the number if water moles that are part of alum’s crystalized structure. This research into the number of moles of water in alum’s structure is important because the number of moles of water within the alum contribute to it’s structure. Alum is a hydrated crystal, or a number of hydrates bonded to an ion that can also be referred to as potassium aluminum sulfate dodecahydrate. There are 12 hydrates bonded to the potassium aluminum sulfate ion.

Add 5-10 drops of 0.1 M AgNo3 to each test tube. Add 10 drops of 6 m HNO3 to each test tube. Stir with a glass stirring rod. Any white solid that remains in AgCl(s). The color for unknown B was clean while the color of NaCl was a milky color, which mean Cl- was present.

The cations in both the known and unknown samples were identified by using qualitative analysis, of which were determined to be acidic, basic, or neutral by using litmus paper. Acid-base reactions, oxidation-reduction reactions, and the formation of complex ions are often used in a systematic way for either separating ions or for determining the presence of specific ions. When white precipitate formed after adding hydroxide, aluminum ion was determined to be present in the solution. However, nickel was determined to test positive when the solution changed to a hot pink color after adding a few drops of dimethylglyoxime reagent and iron was present when the solution was a reddish brown color when sodium hydroxide was added to the mixture at the very beginning of the experiment. Qualitative analysis determines that ions will undergo specific chemical reactions with certain reagents to yield observable products to detect the presence of specific ions in an aqueous solution where precipitation reactions play a major role. The qualitative analysis of ions in a mixture must add reagents that exploit the more general properties of ions to separate major groups of ions, separate major groups into subgroups with reactions that will distinguish less general properties, and add reagents that will specifically confirm the presence of individual