Ashley Wilson 5 March 2018 General Chemistry Lab – Section 202 Experiment 7- Copper cycle Purpose: A series of reactions that convert a piece of copper metal, via several different copper- containing compounds, back into its original elemental form will be observed. Copper wire was dissolved in nitric acid. NaOH was then added to the dissolved copper solution, precipitating into Cu(OH)2. The precipitate was then placed on a hot plate and stirred until it became CuO. After sitting , the CuO was decanted twice, and H2SO4 was added.
Ensure that solid is completely dissolved using a stirring rod. 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.
2) Usage of water in step (5):So that after Estrification is completed , any excess unreacted acetic anhydride is hydrolyzed. 3) The addition of half-saturated NaCl (in step 6): to help in separating the two layers. 4) The usage of a Base (step 7): to neutralize remaning acid . 5) Usage of concentrated sodium chloride in step (9):To dry the ester from any dissolved
After filtration the rich "W" containing liquid is pumped to a crystallizer. The heat from the steam evaporates the water and a white chemical called Ammonium Paratungstate or APT - (NH 4 ) 2 . (H 2 O) x .WO 4 is precipitated. Application of high heat in a calciner causes the compound to reduce to a blue oxide which is approximately WO 3 O 11 . Pure tungsten oxide is WO 3 and yellow.
Copper/ Red Stuff/ Chemical Reaction The purpose of this experiment was to determine what the red stuff that was produced was. We put aluminum foil in a test tube filled with 100 milliliters of copper chloride. During the experiment, I observed that the aluminum foil was breaking away, the aluminum foil that was breaking away was turning into red stuff. After a while, the once light blue copper chloride was turning into a dull gray, almost clear. As the experiment went on, and as the blue copper chloride was turning clear, the reaction of the aluminum foil was slowing.
To do this you first have to place the weighing boat on the scale and hit tare, so it reads zero and then place copper(II) sulfate pentahydrate on the weighing boat. Transfer the copper(II) sulfate into a 250-mL beaker. Rinse the weighing boat with 5 mL of purified water in small quantities to rinse off leftover chemical into the beaker. Spin the beaker gently to dissolve the solid. Rinse the sides of the beaker with small amounts of the 5 mL of purified water.
If the wells are placed closest to the positive terminal it will result in the DNA running off the gel and a failed procedure. 1 X TAE buffer (quantity unknown) was added to the buffer chamber until the gel was completely submerged. The buffer solution was added to create the optimum pH and facilitate electrical conductivity within the chamber. Loading dye (5 µl) was then added to the first well using a carefully pipetting action. PCR product (5 µl) was added to each well and loading dye (5 µl) was added to the final well.
Dissolve the salt in 60 ml of tap water. Add 30 ml 6 M Hcl and stir the mixture with a glass rod. Add 12 g solid Nacl to the solution and stir the mixture for about 2 minutes. Support a 250 ml separatory funnel on a ring, making sure that the stopcock is closed and that a clean beaker is placed beneath the exit tube. Transfer the aqueous solution from the beaker to the separatory funnel.
Lecturer Date Introduction Theoretical Background Procedure The procedure was segmented into two categories, the reaction set up and the crude product isolation. Reaction set up The magnetic stirrer was prepared through placing it in the fume cupboard. 1 mmol of L-Phenylalanine was placed and weighed in a 5 mL conical vial. After that, a spin vane was inserted into the vial while adding 0.75 mL of 1M H2SO4 solution. During the addition of the sulphuric acid, the solution was stirred at room temperature until the amino acid (L-Phe) completely dissolved.
Reactivity of Metals in Single-Replacement Reactions A lab was conducted to test the reactivity of metals in single-replacement reactions. This lab was done to solve the problem of which metals will replace each other in single-replacement reactions. A single replacement reaction is a type of oxidation-reduction chemical reaction when an element or ion moves out of one compound and into another. It was presumed before the experiment that the location of the metal on the Activity Series chart would thus determine the reactivity of the metal. Copper, magnesium, iron, and zinc were all tested in the same five solution compounds; which included hydrochloric acid, sulfate, magnesium chloride, iron chloride, and zinc chloride.