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.
Introduction: In this experiment, we are required to discover the 2 unknown chemicals provided by the teacher through the usage of different lab equipment and scientific procedures to conclude what the unknown substances are. The findings/results will be presented in a qualitative table and further discussed. There are 6 possible substances that the 2 unknowns could be. If the substance is benzoic acid then it would have to pass the organic solvent test because it dissolves in only organic solvents, while if it were silicon dioxide it would fail both solubility tests for organic and aqueous solvents.
Additionally, during testing, it was discovered using the pH section of the testing
Experimental Procedure Identifying the Unknown We performed three tests on our compound to definitively identify it. First we combined 5 g of our unknown compound with 10 mL of distilled water and measured the pH change in the water to test its solubility. Then, to try to identify the cation present in our compound and narrow down the possibilities, we held a sample over a flame and watched for color change. We performed an acid test where we applied a few drops of HCl and watched for a bubbling reaction, to test for the presence of carbonate.
For steps #2, 3 and 4, identify the type of chemical property that was observed. For steps #2, 3 and 4, the chemical property which was observed through the experiment is reactivity with a mixture. It was a mixture being featured because while copper sulphate is a pure substance, when it was added to the water, the copper sulphate became a mixture. I can justify which the property observed was reactivity with a mixture because all the steps consisted of reacting materials residing from different states of matter into the solution. The various reactions ranged from higher temperatures, to gas bubbles, to even colour
In this experiment zinc was added to the solution Cu(H2O)6. Bubbles started to form around the zinc. As the reaction continued,The solution changed from a light blue color to a clear solution and the zinc changed from silver to a red color. The decanting process was done again to remove any acid. It was expected for the Zinc to undergo a change but it was unexpected for the solution to change, from light blue to clear.
In this experiment, four white powders were tested. After visually inspecting the powders, Powder A appeared to be white, lumpy, and possessed no lust, Powder B appeared to be white, soft, and lumpy, Powder C appeared to look smooth, white, and soft, and Powder D appeared to be lumpy, solid, and whitish-yellow. The materials that were utilized in this lab were cornstarch, baking powder, baking soda, powdered sugar, spot plate, scoopula, dropper, water, vinegar, iodine, toothpicks, and paper towels. The physical property that was observed was solubility, the ability of something to be dissolved, and the chemical property that was observed, reactivity, is the tendency of a substance to undergo chemical change. Knowing both chemical and physical properties of the substances is important because they give more information about the identities of the substances and back up observations
Dyala Moshtaha Biology SL Ms. Cardinal January 18th, 2015 Biology Lab Report Vision Lab Title: To test the efficiency of ones direct vision vs. peripheral vision Introduction: Studies prove that ones peripheral vision is the most effective way in terms of sight in the dark. The retina includes two forms of photoreceptor cells, the rod and cone. The cones are segments that are further sensitive to color, and the rods are better at motion detection, and are able to function well in low light environments.
The third test was in a 125ml Erlenmeyer flask and we mixed 30ml of M Hydrocloric Acid and 7g/4g of
The hypothesis for the different experiments is that with each of the different substances and mixtures will be different depending on what they are. II Equipment The late nite lab was used to conduct this experiment. The product used were a balance, a graduated cylinder, water, Ethanol, and unknown liquid, Iron and an unknown metal. III Procedure
The experiment began by gathering the materials. The materials consisted of a ring stand, test tube clamp, 600 mL beaker, 10 cm watch glass, Vernier temperature probe, alcohol thermometer, 11 dram vial, cork with a slit cut in side, spatula, powder funnel, rubber band, 20 cm wire, top-loading balance, analytical
Experiment 1 In the first experiment, half a gram of magnesium was combined with 3 milliliters of hydrochloric acid in a glass beaker. The magnesium looked like a gray powder. The hydrochloric acid appeared to be clear liquid and looked very similar to rubbing alcohol. Before, the reaction took place the magnesium and hydrochloric acid weighed 4.44 grams when weighed together.
The maximally effective pH was determined to be approximately 5. The maximally effective temperature was determined to be 37°C. The Q10
The technique utilized in this experiment was titration and is used to determine the concentration of an unknown solution by reaction with a known concentration of solution. In a titration, the titrant is placed into the burette and the analyte poured into the conical flask using a pipette. Titration involves adding a small amount of titrant slowly to the analyte to achieve the equivalence point. The equivalence point is when the moles of standard soluton are same as the solution of unknown concentration and is produced at a pH of 7. The indicator used in this experiment was Phenolphthalein which determined the end point, which was shown as a form of colour change.
The solution of DCM and cyclohexane was clear and colourless. The following graph shows the recorded
