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Calorimetry Of Reaction Lab Report

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The copper(II) metal complex was prepared by reacting copper(II) chloride and sodium saccharinate together by applying heat. The copper(II) chloride was originally a white solid and the sodium saccharinate was a blue solid. A centigram balance was used to weigh out a 1.01g sample of the sodium saccharinate and a 0.75g sample of the metal salt, copper(II) chloride. Each reactant was placed in separate 50-mL beakers and then dissolved using 10 to 20-mL of deionized water. Once dissolved the reactants were combined into a 250-mL beaker along with a clean stir bar. The solution exhibited a blue color. The original beakers were rinsed with 2 to 3 mL of deionized water. These rinses were then added to the reactant solution; the solution evolved into a light blue color. …show more content…

A light blue precipitate formed along the walls and the bottom of the beaker after being exposed to heat for 15 minutes. After the precipitate was formed the hot plate was turned off and the solution was allowed to cool down until it became warm. Once it was warm the beaker was placed in an ice bath. While waiting for the solution to cool, a vacuum filtration was set up. The solution took around 25 to 30 minutes to cool. Once the solution was cool, we began to isolate the saccharinate salt by pouring the solution into the Büchner funnel. To help further isolate the product we rinsed the precipitate with ice-cold deionized water. Once isolated we dried the product and observed that it was a small-medium sized blue solid. This isolated solid was then weighed and found to have a mass of

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In cycle one, the double displacement reaction, Cu(s) + 4HNO3(aq) → Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l) occurred, the result of the reaction was that the reaction mixture began to bubble with the copper filling dissolving and a vapor like substance leaving the reaction. Furthermore, when water was added, the color change, from brown to a blue color pigment. Then in Cycle two, another double displacement reaction occurred, Cu(NO3)2(aq) + 2NaOH(aq) → Cu(OH)2(s) + 2NaNO3(aq), which resulted in the reaction becoming cloudy and a darker shade of blue. Following cycle two, a decomposition reaction occurred as the result of heat being administered to the mixture, thus the following reaction occurred in cycle three, Cu(OH)2(s) → CuO(s) + H2O(l). As a

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Next we moved the beaker into the fume hood where we added the nitric acid, HNO3(aq), where the solution started to fizzle and there was a brown gas produced called nitrogen dioxide, NO2(g), which then made the solution blue called copper nitrate, Cu(NO3)2(aq), which smelled like bleach. When we put the 25 mL of water nothing happened to the solution and looked the solution looked the same. After, we had to measure 2 mL of the concentrated sodium hydroxide, NaOH(aq), in the graduated cylinder and then poured into the beaker slowly which made the solution a darker blue and made it a solid copper hydroxide, Cu(OH)2(s). When the beaker was placed onto the hot plate the solution was turning black and into a solid that smelled bad called copper oxide, CuO(s). When it cooled down nothing happened but when the mixture was being filtered the solids stayed in the filter paper and a clear liquid came out which was sodium nitrate, NaNO3(aq).

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The solubility rate of copper (II) chloride in methanol is 53g/100ml whilst the solubility rate for sodium chloride is 65g/ml. Although there solubility rate is fairly close the difference is enough that when little amounts of methanol is added only the copper (II) chloride dissolves. A factor that affects the solubilty of metals is their molecular mass. Copper (II) has a molecular mass of 63.546 whilst sodium has a molecular mass of 22.989769 meaning copper has higher solubility rate than sodium, this is because as the molecular mass of a metal increases it becomes difficult for molecules to hold onto their solute particles and when those particles break away they can easily dissolve into the solvent. Therefore because coppers molecular mass is greater than sodiums it’s solute particles breakaway with less resistant meaning copper dissolves better.

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