Lichen Lab

8. Draw conclusions – Assuming that your experiment produced results identical to those seen in Table 4, would you reject or accept the hypothesis that you produced in question 3? Explain how you determined this.

The Vitamin C turned to a red/orange color with no physical/chemical reaction. For the salt the solution turned to an orange color with no physical/chemical reaction. With the Alka-Seltzer, the solution turned to a brown color with no reaction as well. Last but not least, the Baking soda turned to an orange/brown color with no reaction.

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.

Lab procedures must be communicated in a lab to ensure that the lab is a safe place to perform experiments. Using good judgment, observe safety rules and follow directions can prevent accidents form happening. Experiments should include comments to alert people

Yes, because the solution seen was still blue meaning that not all the copper chloride was extracted from the beaker.

•Be sure to write a detailed procedure for each lab design so that the same procedure can be followed accurately by anyone who reads it. Include details on the setup, the control of variables, and how the rate of each trial will be compared.

Based on the results of your experiment, would you reject or accept the hypothesis that you produced in question 1? Explain how you determined this.

1. Make sure that you understand the objective of the lab(s) and the requirements for successfully performing them.

2. Based on the results of your experiment, would you reject or accept each hypothesis that you produced in question 1? Explain how you determined this.

Heavy precipitate emerged immediately and solution turned white in color; solution then became opaque and turned light, bright blue in color.

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.

Dissolve 2.34 g of cobalt chloride hexahydrate (CoCl2.6H2O) in 100 ml of water in an Erlenmeyer flask. While stirring the oxalic acid solution constantly, add the cobalt chloride solution drop by drop. Let the mixture cool in an ice bath. A precipitate will form slowly.

Were your hypotheses right or wrong? Tell how those hypotheses would have to be modified in another experiment.

When the solution was cooled after 25 minutes of heating, the top layer was pale violet red and the bottom layer was maroon. Furthermore the top layer took the larger volume of the flask, about tenfold the volume of the bottom layer.

The zinc powder was black in colour while copper (II) sulphate solution was blue in colour because of the presence of copper (II) ions. When the zinc powder was added to the copper (II) sulphate solution and stirred, it was hard to observe the pattern of the colour change because the polystyrene cup as covered with a lid.