| [Solubility Product Constant] | Experiment 11 | | Molly McCabe | 4/18/2013 | | Data Tables: Part 1 and Part 2 Experimental Data: Standard | Calculated volume of copper sulfate in standards | Absorbance values | Blank | 0.0 mL | 0.0 | 1 | 1.25 mL | 0.094 | 2 | 3.75 mL | 0.065 | 3 | 2.50 mL | 0.099 | 4 | 3.50 mL | 0.129 | 5 | 5.00 mL | 0.187 | Collected Data | Test tube 1 | Test tube 2 | Test tube 3 | Test tube 4 | Test Tube 5 |…
II. Purpose: The purpose of this lab is to see how iron reacts with a copper (II) chloride solution.…
9) Put 4mL of stock solution and 1mL of water in a test tube to make the second solution.…
Know the reaction equations, which reactions occur (ex. by heating, etc.) and physical descriptions/color of tings…
2. To determine the densities of water, an unknown liquid, a rubber stopper, and an unknown rectangular solid.…
The copper in the compound needed to be dissolved by using hydrochloric acid and then react with magnesium in order to only get copper left in the solution at the bottom of the beaker. The copper should be weighed and then compared with the other compounds (Table 2) in order to find the unknown. This was all performed in the…
When holding test tube inverted over heptane flame, condensation formed against top walls of the test tube. When the burning splint was added the walls of the test tube became less foggy from the condensation formed from the heptane flame.…
2. Next, we measured our 80 ml of copper II sulfate and 20 ml of distilled water and combined them in a graduated cylinder.…
.2400 grams of the unknown compound. This is done in duplicate and purple-tinted precipitates are placed in Gooch crucibles. The precipitates are suction dried using ethyl alcohol then acetone to…
Second, you will conduct a chemical reaction with the dried sample, which will produce elemental copper. By measuring the mass of copper that forms, you will have the necessary information to determine the moles of copper and chlorine in your sample, and you will be able to establish the proper chemical formula.…
The procedure for this experiment was followed using the guidelines found in CHL111 General Chemistry I Laboratory Manual Fall 2013, Chemical Reactions of Copper.…
Fill a small test tube halfway with copper (II) sulfate solution. Add a 2.0 gram iron rod to the solution and observe the reaction.…
In this experiment, we used an electronic balance to weight a clean, dry crucible before obtaining a sample of copper (II) sulfate (CuSO4), bright blue crystals, from the instructor. We then weighted two samples for the first and second trial with the crucible and found the samples’ weight to be 1.19 g and 1.55 g, respectively. A Bunsen burner was then set up for the heating of the crucible, with a wire triangle on the iron ring ensuring that the wire triangle will hold the crucible in an upright position. After setting up the Bunsen burner we heated the crucible with copper (II) sulfate for around eight minutes. During the heating process we haven’t noticed any splattering or popping of the material. After the 8-minute…
Compare different methods for finding the concentration of copper(II) ions in solution. Could include redox titration, colorimetry, ion exchange followed by acid/base titration, gravimetric, use of an electrochemical cell.…
This experiment was performed to demonstrate a cycle of chemical reactions involving copper. This lab will start with copper as a reactant in the first reaction through a series of five chemical forms of aqueous phase reactions and ending to calculate the percentage of recovered solid copper as a product in the last reaction of the experiment. The experiment resulted in a percent recovery from the cycle of copper reactions of an increase to 139%.…