The synthesis of NaCl further identified the ionic compound by reacting sodium hydroxide and hydrochloric acid and obtaining solid sodium chloride. The synthesized compound formed was used to perform another flame test and the chloride anion test, which further solidified the identification of NaCl as the ionic compound. Introduction The purpose of the experiment was to identify unknown ionic compound
To observe the change in properties of various synthesized copper compounds in order to identify the reactions and products being formed. Secondly, to become familiar with methods of separating compounds through decanting, heating with Bunsen burner and suction filtration system. In doing so, be able to recover copper metal and interpret the resulting percentage yield by applying the law of conservation of matter. Upon combining 20.0mL of NaOH to 10.0mL of Cu(NO3)2 and stirring the solution, there was a darkening of the initial blue color. Adding distilled water to the solution lowers the initial intensity of the blue color, bringing back to a lighter blue.
Observing Changes – Materials & Procedures Materials Water Copper (II) sulphate (Powder) Copper (II) sulphate solution Iron nail Sodium carbonate Hydrochloric acid Magnesium ribbon Flame (candle) Sugar Aluminum foil Test tubes Test tube rack Tongs Medicine dropper Spoons Beakers Safety goggles Scoopulas Procedures Water and Copper (II) Sulphate Procedure 1. Add a small amount of solid copper (II) sulphate to a test tube with a scoopula. Record the physical properties. 2. Write a hypothesis on what you think will happen when water is added.
What color do you observe? NH3 (ammonia, a base) and 1 drop of BTB (bromothymol blue). What color do you observe? Record the colors you expect when BTB reacts with an acid and with a base. HCI and blue dye.
Fill the burette with 0.005mol dm-3 potassium manganate(VII) solution. 6. Pour some of the thyme extract solution into a 250cm3 plastic beaker. 7. Using a measuring cylinder, add 50cm3 of 1.0mol dm-3 sulphuric(VI) acid to the thyme extract in the conical flask.
The purpose of this lab is to focus on how to make zinc iodide in a different way using compounds instead of elements, which are barium iodide and zinc sulfate. We will see if the reaction between these two compounds will occur and make a prediction by writing a chemical equation. The procedures for this lab are to place a small test tube inside a 50mL beaker and weigh it. Then, using a spatula, add 0.45±0.03 g of zinc sulfate heptahydrate into the small test tube and record the mass. After that, dissolve the sample in 2 mL of deionized water and shake the test tube for 1 to 1 ½ minutes to dissolve the solid.
Once a light blue solution remained, 5mL of distilled water was added. This solution was then placed onto the magnetic stir plate and magnetic stir bar was placed in liquid solution. Then to the solution .75g of zinc was added to solution. Then once the solution was colorless, the solution was removed from magnetic stir plate and the liquid was decanted away from the copper. Then 5mL of HCl was added to copper to completely remove all traces of zinc.
Next I added two drops of HCl into well D1, and then added two drops of blue dye, and recorded what I saw. After that I put two drops of blue dye in well E1 and added two drops of NaOCl, then observed, after this I added one drop of HCl into well E1 and observed the changes. Next I put two drops of KI into well F1 and then added two drops of Pb(NO3)2 and then described the precipitate that formed. Then I put two drops of NaOH into well G1 and added two drops of phenolphthalein, and observed the color. After this I put two drops of HCl into well H1 and added two drops of phenolphthalein, and observed.
We added anhydrous Sodium Sulfate as a drying agent. To complete, we distilled the cyclohexene and collected the product. Knowing this data, we determined the yield % which is 58.5%. This experiment features the dehydration of cyclohexanol and produce cyclohexene. The acid catalyzed dehydration of cyclohexanol with distillative removal of the resulting cyclohexene from the reaction mixture
Using a Buchner funnel, a hose, and a suction flask we created a vacuum filtrator which we used to help remove the remaining liquid on the copper so that we may make a more precise measurement of the mass of the remaining copper. Our final mass of copper was .7951 grams. Results and Discussion: Initial Mass of Cu: .25 grams When we mixed the 5 ml of 6 molar HNO3 the copper had disappeared, indicating it had been used in the reaction. The copper had undergone a single replacement reaction and a decomposition reaction. Initial equation: Cu(s) + HNO3(aq) -> Cu(NO3)2(aq) + NO2(g) +H2O(l) Balanced: Cu(s) + 4HNO3(aq) -> Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l) The copper had replaced the Hydrogen in the HNO3 and the NO3 had also broken down into NO2 and O2- allowing the H+ to bond with it and create