Lab Report Of The Copper Acetate Monohydrate

This experiment is based on determining the chemical formula for a hydrated compound containing copper, chloride, and water molecules in the crystal structure of the solid compound, using law of definite proportion. The general formula of the compound is CuxCly•zH2O, and aim is to determine chemical formula of this compound.

The purpose of this lab was to determine the empirical formula of copper oxide compound. In the lab, hydrochloric acid and copper oxide compound was mixed until it formed a blue solution. An oxidation-reduction reaction, a reaction in which there is an exchange of electrons between elements, was performed by adding zinc to the solution to displace the copper in copper chloride. Zinc, in this case, was oxidized by losing two electrons (0 → 2+) while copper was reduced by gaining two electrons (2+ → 0). Also, when the copper was displaced, it became a precipitate, which is a substance that comes out of a solution as a solid due to insolubility.

In this task the concentration of an unknown sample of copper sulphate using colorimetry was used to find the concentration. In this investigation copper sulphate was used which is CuSO4.5H20 as a formula. To make a standard solution which was 1M, the same clean equipment was used to make up the standard solution as used to make sodium carbonate. However there was one difference and that was that the hot distilled water was used to dissolve the copper sulphate crystals. There had to be enough hot water in order to dissolve the crystals into the beaker and then add cold distilled water to cool the solution.

The purpose of performing the variety of tests that we did was to give more accurate results of what the unknown mineral was. By roasting the copper mineral, we obtained copper(II) oxide. This new sample came out of the crucible grayish-black. It was very brittle and full of cracks. This provided the percent composition that was necessary in finding the unknown mineral. When performing

For our science assessment we had the task to research about a metal of our choice. Since I am really into computers, I chose copper. A metal used in all kinds of wires, cpu’s and other stuff without a computer wouldn’t work. This fits really well into what we have to do for the second part, describe how this metal has helped human society.

The purpose of the lab copper- silver nitrate reaction is to find the mole relationships between reactants and products. My hypothesis was that the mole relationship between silver and copper will be 2 mol Cu: 1 mol Ag ratio. My hypothesis is supported by the data I found during the lab. First evidence, in the beginning of my calculation I have to determine the mass of copper that reacted during the experiment and converted to moles of copper and got .0033 moles of Cu. Next, I determined the mass of silver produced during the experiment and converted into moles of silver and got .0063 moles of Ag. After I found the moles of copper and silver, I determined the value of the ratio of .0063 moles Ag /.0033 moles Cu and got 1.90 moles. 1.90 mol

13) When the tray is thoroughly dry, determine its mass. Record the mass in the data table. You have to wait until day three to weigh the copper.

It’s important for reactions in aqueous solutions to reach equilibrium, meaning that both products and reactants need to be present before continuing to the next reaction or next step. In this experiment, copper was changed through eight different reactions. Throughout the process, qualitative observations were recorded to see what effect each type of acid and decanting has on copper. All of these steps were successfully completed by using different acidic solutions and zinc to take copper through the cycle from copper solid to copper nitrate to copper hydroxide, to copper oxide, to copper II sulfate, and back to copper solid.

In this experiment, the experimenter will determine the chemical formula for the copper chloride hydrates using the law of definite proportions. The hydrated compound has a general formula of CuxCly•zH2O, with the variables x, y, and z. The variables represent the whole number ratio of moles that will be the “true” chemical formula of the hydrate. The chemical formula shows the number of atoms of each element in a compound.

Before the synthesis of the Copper Iodine Compound, the identities provided (CuNO3)2 and Nal weighed 1.65 g and 4.7 g, respectively. After being weighed, the (CuNO3)2 exhibited a blue color, while the Nal, through observation, was a white color. However, when both identities were combined, the product turned into a brown and red rocky material. Once 20 mL of deionized water was added, the product quickly turned pale pink paste. After the solution was repeatedly washed with a total of an additional 100 mL of deionized water, the product was powdery and pink with small grains, and was left to air-dry. Once the product was air dried, it was observed to be a pale pink color, while the filter paper was stiff as the product was hard and dry. Therefore, the solid was scraped off onto a recrystallizing dish. However, the mass of an empty recrystallizing dish needed to be recorded in order to compare how much of the synthesized copper iodide was obtained. Within this case, the empty recrystallizing dish used weighed 32.01 g, the product on the empty dish weighed 1.03 g, having a total weight of 33.04 g.

XIII. Carefully remove the copper metal from the filter paper onto the watch glass. (with a spatula) Place a 400 ml beaker on a hot plate contained with water. Carefully place the watch glass before the water boils to dry the copper metal. (Use the tongs to handle the hot watch glass)

Mol of Cu = 0.043866 mol CuSO4 * 1 mol Cu1 mol CuSO4 = 0.043866 mol [IV]

The reaction characteristics of basic copper carbonate 〖mCuCO〗_3⋅n〖Cu(OH)〗_2 were observed by changing the reaction mole ratio. The reaction mole ratio of sodium carbonate to copper chloride (II) was controlled from 1.08 to 1.68. Fig. 1 shows the XRD patterns of copper carbonate powder. At a reaction ratio of 1.08, paratacamite (Cu_2 Cl(OH)_3 ), beside alkali copper carbonate, was formed because of incomplete reaction at a copper content of 53.9 wt%. Lack of sodium carbonate may cause incomplete reaction with copper chloride (II) because of low pH (6.0) of the solution [12]. The copper content according to the reaction mole ratio were 57.7, 50.5, 58.8, 59.3, and 59.8 wt% at the reaction mole ratios of 1.20, 1.32, 1.44, 1.56, and 1.68, respectively.

Solutions of CuSO45H2O (0.506 g in 10mL water, 3.17E-3 mol) and ammonium peroxodisulfate (1.030 g in 10mL water, 4.51E-3 mol) were prepared and mixed

When the sulfuric acid was added to copper (II) oxide, the solution turned blue. This was due to the formation of aqueous copper (II) sulfate, which produced the copper ions to change the color of the solution.