6.03 Calorimetry Lab

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For two of the sparklers, write a short paragraph presenting & discussing your data and observations. You should include identification and discussion of the cations determined to be present
We had a red sparkler and a green sparkler. We held the red sparkler up to the flame and the sparkler was ignited displaying a strong red color. We found there to be a high level of intensity in the peaks as well as several peaks present on the graph. The five largest peaks found were 588.1nm, 633.7nm, 658.5 nm, 671.9 nm, 766.9nm. From this data we were able to conclude that the lithium cation and strontium cation is present in the red sparkler. The peaks found in the green sparkler matched up with the peaks found in the lithium and strontium cations. Specifically the biggest peak on the red sparkler was 766.9 which matches the color that lithium burns (red), allowing us to confirm that the lithium cation was present. Our next sparkler was the green one. We held the sparkler up to the flame and the sparkler was ignited displaying a light green color. Found there to be a high level of intensity in the peaks as well as several …show more content…
This is because copper cations (Cu2+) in copper(II) gluconate produce a green flame. The cation is the part of the compound responsible for color. You know that the copper ions is responsible for color because for example in lab when we measured K+ which was actually KCl, it was found that KCl produces a purple flame. K+ was the part of the compound that is responsible for color thus it would also make sense that Potassium gluconate produces a light purple flame because it contains a potassium cation. Using this logic it can be concluded that cation part of copper gluconate (Cu2+) would be responsible for the color being green. The cations are within the visible spectrum thus we can see a certain color depending on the

6.03 Calorimetry Lab

Calculate the mass of potassium nitrate and the mass of water in each solution Calculate the ratio of the mass of potassium nitrate to the mass of water for each solution. Multiply the mass ratio by 100 to determine the concentration of each saturated solution in grams of potassium nitrate per 100 grams of water. Plot a graph of solubility of potassium nitrate (in g of solute/100 g of water) on the y-axis versus temperature on the x-axis. Scale each axis as necessary. Draw a smooth…

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6.03 Calorimetry Lab

In a chemical reaction, matter is neither created nor destroyed. This is the law of conservation of mass, which begs the question, does this linearity also apply to volume? One of the goals of this experiment was to see if two pure liquid substances are together, will the volume of the solution be the total sum of each individual substance? Three characteristics must be known about the solution: the mass, volume, and density. Mass can be accurately measured out by a digital scale, volume can be measured…

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6.03 Calorimetry Lab

The average enthalpy of neutralization for HNO3 and NaOH is -55.95 kJ/mol H2O. Post Lab Questions: 1. The temperature change of water will increase because the heat in hot water will transfer to cold water in the calorimeter. 2. Part A.5. His decision will decrease the specific heat of the unknown metal. The highest measured temperature…

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6.03 Calorimetry Lab

Get a piece of copper wire, proceed to clean it with steel wool and clean it until the surface is shiny. Using the electronic balance given, mass the copper wire and record it in the data table. Put the copper into a 150 mL beaker. When placed in the beaker, the Copper needs to be smashed down flat. Place the beaker with the Copper in it, in the fume hood. Proceed to carefully add 12 mL of concentrated Nitric acid ( HNO3 ) into the beaker. Let all the copper dissolve, slowly add 100 mL of distilled…

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6.03 Calorimetry Lab

For the first reaction, which is NaOH(s) → NaOH(aq), I would first need to measure out the required .041 moles of NaOH, which would weigh 1.65 grams. I would then measure out 41 milliliters, so that when I mixed the two, my concentration of NaOH in my aqueous solution will be 1M. In all, this should weigh about 41.8 grams when mixed together; however, prior to pouring the NaOH, I will first need to measure the temperature of the water itself with the calorimeter; I will do this at least five times…

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6.03 Calorimetry Lab

For Part A of the experiment, acetic acid was titrated with NaOH. First, the 0.05M acetic acid solution was prepared. A 50-milliliter graduated cylinder was obtained and used to add 45 milliliters of deionized water was added to a labeled 150-milliliter beaker. A ten-milliliter graduated cylinder was used to add five milliliters of acetic acid to the beaker and the solution was placed on the stir plate and stirred with a magnetic stir bar. Next, a 0.05M NaOH solution was prepared. A 50-milliliter…

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6.03 Calorimetry Lab

sulfate(II) sulfate and adding iron sulfate and copper will be used in a single replacement action. Also it should be able to find the ratio of moles of a reactant to moles of a product in the chemical reaction. Thus, it should answer another purpose for the lab which is to find is to be able to relate this ratio to the coefficients of these substances in the balanced equation for the reaction. Hypothesis: Both of coefficient off iron Variables: Procedure Find the mass of a clean, dry 100 ml beaker. Record…

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6.03 Calorimetry Lab

Before beginning this experiment make sure to write down observations of all the chemicals that are going to be used. To begin, 25 mL of .05 M lead nitrate into a clean 50 mL graduated cylinder and add to a clean Erlenmeyer flask. Measure out 1.4 mL of .025 M sodium carbonate and also add it to the Erlenmeyer flask. After adding mix both chemicals for 15 seconds or so. After mixing set up vacuum filtration flask using deionized water. In order for the apparatus to work it needs to be set up correctly…

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