Lab6 Report

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School

Georgia Institute Of Technology *

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1310

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Chemistry

Date

Oct 30, 2023

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pdf

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Uploaded by ProfessorOwlMaster973

Preparation of a Chemical Rainbow in a Test Tube February 2 nd , 2023 CHEM 1310 Laboratory Methods In this lab, we wore PPE such as lab coats, gloves, and goggles, as hazardous reagents were in use. To begin the lab, a standard 30 mL beaker was placed on an electronic balance, and the mass was recorded to be used later. Next, approximately 4 mL of the first solution was measured out and placed inside of the beaker. The exact volume was recorded in the data table, and then the beaker plus solution was weighed using the electronic balance. The mass of the liquid was determined by subtracting the mass of the beaker from the liquid plus beaker (𝐵?𝑎𝑘?? + 𝐿𝑖?𝑢𝑖? 𝑚𝑎??) − (𝐵?𝑎𝑘?? 𝑚𝑎??) = 𝐿𝑖?𝑢𝑖? 𝑚𝑎?? , and the mass was recorded in the data table. Now, the density can be determined using the equation 𝑃 = ?𝑎𝑠𝑠 ?𝑜???𝑒 . Repeat these steps for each of the 6 liquids and record all the data. Data and Results Table 1: Volume, Mass, and Calculated Density of Various Liquids Liquid Volume (mL) Mass (g) Density (g/mL) DCD 4.0 5.064 1.266 EAC 4.0 3.400 0.850 FIF 4.0 4.256 1.064 LIG 4.0 4.912 1.228 HEA 4.0 5.400 1.350 DIW 4.0 3.838 0.960 The densities in descending order are: EAC<DIW<FIF<LIG<DCD<HEA

Figure 1: Relative Densities of Each Liquid Figure 2. Photograph of completed chemical rainbow. 0.000 0.200 0.400 0.600 0.800 1.000 1.200 1.400 1.600 DCD EAC FIF LIG HEA DIW Density (g/mL)

Conclusion To answer the question, what are the relative densities of various liquids, we followed the protocol outlined above. The relative densities of each liquid are listed in the previous data table and are in descending order here: EAC<DIW<FIF<LIG<DCD<HEA. This conclusion is supported by the data presented. For instance, the calculated relative density of EAC was 0.850 g/mL, while the relative density of DIW was calculated to be 0.960 g/mL. In terms of the broader experiment, this meant that EAC would naturally settle above DIW if other things such a miscibility didn’t interfere. This data was determined through the utilization of a common fact that density is equivalent to mass divided by volume. In the experiment, the mass and volume of each liquid were measured, and the equation was applied in order to find values of density. For instance, DCD with a volume of 4.0 mL and a mass of 5.064 grams was found to have a density of 1.266 g/mL. The relative densities equated allow us to start determining what liquids should be placed on top of one another, as higher density liquids will settle towards the bottom as is observed in everyday phenomena and generally explored in middle school or high school chemistry labs. This data was then used to determine the order of the various liquids, according to the following guidelines: the most dense solutions should be near the bottom if possible, miscible solutions shouldn ’ t be next to each other, and polarity should be different next to each solution. Our data combined with the data of other groups then led to the conclusion that the liquids should be layered as follows (from bottom to top): HEA, FIF, LIG, DCB, DIW, EAC. This order was determined by first placing all liquids that had similar densities next to each other such that the denser solution was on bottom, and then rearranging these solutions as best as possible such that no two liquids that were miscible were directly touching, as we didn ’ t want them to combine. This resulted in a decent rainbow, although the line between yellow and green was a bit difficult to see, and the liquids did seem to slightly mix. This may be due to inaccuracy in our data, or the data of other groups within the lab. It could also be due to cross contamination of tools across lab periods.

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