This experiment was composed of five reactions: The formation of Cu(NO3)2, the formation of Cu(OH)2, the formation of CuO, the formation of CuSO4, and the formation of Cu(S). For Reaction 1 which was the formation of Cu(NO3)2, the mass of the copper wire was taken in an analytical balance so that it can be compared to the final mass of copper at the end of the experiment. The copper wire was bent slightly and was laid flat in a 250 mL beaker so that the 16 M HNO3 solution could cover the whole wire. In the fume hood, a disposable pipette was used to distribute about 4 mL of 16 M HNO3 into the beaker with the copper wire. The solution was stirred by rotating the beaker until the copper wire had completely dissolved and the toxic, brown NO2 gas …show more content…
The 250 mL beaker from Reaction 2 was heated on a hot plate, and stirred continuously for approximately 20 minutes until the reaction was complete, which is visible by the solution becoming clear the precipitate formed being all one dark brown/black color. The beaker was removed from the hot plate and the solid settled to the bottom. Once the solid had settled the solution was poured out into a waste beaker to leave just the solid in the beaker. To the solid, 200 mL of deionized water was added to a clean 400 mL beaker that was heated until just below boiling point. Once the water was sufficiently close to boiling, the beaker was taken off the hot plate and the water was poured into the 250 mL beaker with the solid. The solution was stirred and once the solid settled the liquid was poured into a waste beaker to leave just the solid in the beaker. When reaction 3 was completed the observations from the reaction were recorded in Table …show more content…
In beaker with the formed CuSO4 from Reaction 4, a piece of aluminum wire, which was bent into a circular shape, was placed in the beaker, and completely submerged in the solution. To this beaker a small stir bar was added along with 5 drops of 6 M HCl to start the reaction. This beaker was place onto the hot plate, covered with a watch glass, and the stir setting on the hot plate was turned on so that the stir bar moved the piece of aluminum wire around and hit it repeatedly. The wire began to have copper form on it and the stir bar hitting the wire would knock off the formed copper. Before the beginning of the next step the reaction had to be completed. If the reaction was happening at too slow of a rate or formation of copper was not happening the solution could be gently heated to help facilitate the reaction. After the reaction was done, the beaker was removed from the hot plate and the stirring rod was used to scrape off the copper that remained on the aluminum wire. The aluminum wire was removed from the solution and the liquid was poured carefully into the waste beaker, making sure not lose any of the copper. To dry out Copper, a steam bath was created using a 100 mL beaker filled with 50 mL of water and it was left to boil on the hot plate while copper was being washed with deionized water and ethanol. A wash bottle filled with deionized water was used to rinse the copper from the beaker into a small evaporating dish. No
The purpose of the lab is to acquire the percent composition of zinc and copper. The procedure included obtaining a post 1983 penny and washing it with soap and water. Using a triangular file, we made an X on the penny. Then, we cleaned the top and bottom of the penny with steel wool until it was shiny. We rinsed the penny in acetone and dried it with paper towel.
For this lab, zeolite and magnetized zeolite were synthesized and compared with charcoal to find out with would be the most effective in the sequestering of Procion Red dye. Finding the concentration and absorbance of each zeolite, magnetized zeolite, and charcoal, along with a calibration curve, the best adsorbent is determined. Charcoal was the overall best sequestration of the Procion Red dye, since the adsorbent was highest compared to the others. Introduction Pollution has increased in the environment over the years, so the purpose of this experiment is to find the best adsorbent of chemicals to reduce the pollution.
Cadet Eric Wiggins Date: 18 September 2014 Course Name: Chem 100 Instructor: Captain Zuniga Section: M3A Identification of a Copper Mineral Intro Minerals are elements or compounds that are created in the Earth by geological processes. The method of isolating metals in a compound mineral is normally conducted through two processes.
Next, about 10 mL of both solutions, Red 40 and Blue 1, were added to a small beaker. The concentration of the stock solution were recorded, 52.1 ppm for Red 40 and 16.6 ppm for Blue 1. Then, using the volumetric pipette, 5 mL of each solution was transferred into a 10 mL volumetric flask, labelled either R1 or B1. Deionized water was added into the flask using a pipette until the solution level reached a line which indicated 10 mL. A cap for the flask was inserted and the flask was invented a few times to completely mix the solution. Then, the volumetric pipette was rinsed with fresh deionized water and
After placing the aluminum in said beaker, one should gather a stir stick and stir the solution in order to speed up the reaction. One should stir the solution until there are no visible silver pieces of aluminum left in the beaker of what was the copper (II) chloride solution. When there are no visible silver pieces of aluminum left in the beaker, this means that the reaction has occurred. After the reaction has occurred, one needs to separate the products, which are copper and aluminum chloride, from each other in order to see how much copper was able to be produced. Seeing as the products are a solid in the form of copper and a liquid in the form of aluminum chloride, the process of filtration can be used to separate them.
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
Then an estimated (by trial and error) 1-3 grams of hydrated copper sulfate was added to a crucible with the lid on top. The total mass of the hydrated copper sulfate was recorded by subtracting the total mass of the crucible, lid, and sample from the mass of the crucible and lid (described in table 1.3). By attaching the wire triangle to the ring, the crucible was able to sit securely while having the bunsen burner underneath. Lighting the burner once again, each substance was heated for several minutes until estimated that the compound had changed color. Once a prevalent color change had been observed at approximately 4 minutes (blue green color) the crucible was set on the counter using the tongs to cool for approximately 5 minutes.
This lab’s end result was to correctly identify each unknown solution using prior knowledge of chemical properties and the results of the first experiment conducted. Unknown solution D was the only colored solution, being blue while the others were clear. This made it easy to then match D up to Copper Sulfate because of its color. As unknown A and B were added together, lots of gaseous bubbles formed and revealed the fact that that reaction was the reaction between Hydrochloric Acid and Sodium Carbonate because it was the only reaction that produced a gas release. Unknown A and C produced the only yellow, brown precipitate just as the reaction between Sodium Carbonate and Silver Nitrate had previously.
grams of the compound into 50 mL of distilled water and then “swirling” the mixture to dissolve the compound. Once all of the solutions were created, the nichrome wire must be cleaned. This was done by rinsing it with distilled water and then burning it in the flame. Next, each aqueous solution was burned and the results were recorded. In between each test, however, the nichrome wire was cleaned again.
The heating of the solution caused the reaction to start which decomposed Cu(OH)2 and made the solution colorless and darkened the precipitate. The fourth step was the formation of CuSO4. After the solution was decanted from the precipitate and washed with near boiling water, 6 M H2SO4 was added to the beaker containing Copper (II) Oxide and this caused the precipitate to dissolve and the liquid become clear blue. The last step was the formation of Cu(s). This step recovered Solid elemental copper.
Later on all the observations were compared in order to found out which cation/cations made up the unknown solution. To ensure a safe classroom environment, all four laboratory bottles were cleaned and put away, the paper clip was thrown
With the two reactants being aqueous solutions, there is a possibility it the reaction could form a precipitate as one of
Next, a 10 mL beaker is filled with 3 mL of HCl and measure 10 mL of ionized water into a 140 mL beaker. Carefully turn on laboratory burner and start cleaning the Nichrome wire by dipping it into concentrated HCl acid. Hold the Nichrome wire on top of the flame and repeat the step until the wire doesn 't show any color. When the wire is clean, dip the wire again with some of the acid and dip it into the solution with the unknown compound in it. Place the wire back into the flame again and observe the color of the flame.
Introduction: The purpose of this experiment is to demonstrate the different types of chemical reactions, those including Copper. There are different types of chemical reactions. A double displacement reaction is a chemical process involving the exchange of bonds between two reacting chemical species. A a decomposition reaction is the separation of a chemical compound into elements or simpler compounds and the single-displacement reaction is a type of
Throughout the experiment, copper was altered a total of 5 times, but after the final chemical reaction, solid, elemental copper returned. Each time the solution changed color, a precipitate formed, or when gas appeared, indicated that a chemical reaction was occurring. For the first reaction, copper was added to nitric acid, forming the aqueous copper (II) nitrate (where the copper went), along with liquid water, and