In part one of the lab we used a micro scale technique to derive an activity series for metals. With the use of this technique we measured the same amount of different metal nitrate solutions into each well. Then we placed a piece of metal in the other metal nitrate solutions. With the data we recorded we resulted our activity series for the metals. We resulted that lead, silver, and copper are the strongest oxidizing agents, and that magnesium and zinc are the weak oxidizing agents.
12. Place a paper towel over the drain, pour the content of the well plate, throw the paper towel and rinse the well plate. DATA, OBSERVATIONS, AND CALCULATIONS: Data Table: Oxidation - Reduction | | Reactions | Mg in Na2SO4 | Bubbles | Zn in MgSO4 | Small bubbles | Pb in Zn(NO3)2 | Dark lead changed into lighter color | Pb in FeCl3 | Changed the lead into slight green yellow | Fe in CuSO4 | Changed the iron into orange color | Note: I added more than 10 drops to make sure that the pieces are well covered. QUESTIONS: A. Based on your observations make an activity series of the metals used.
Abstract The purpose of the experiment was to identify unknown ionic compound #. After many tests, the unknown was identified as sodium chloride. The cation (Na+) was determined by having a yellow/orange color flame test. The anion (Cl-) was determined by the chloride anion test when the unknown test solution showed a positive test for chloride. The synthesis of NaCl further identified the ionic compound by reacting sodium hydroxide and hydrochloric acid and obtaining solid sodium chloride.
Through these processes and skills, the chemical composition of the unknown sample can be determined. If the unknown sample contains magnesium, iron, and chromium then the sample is chromite. If the sample does not contain all of these metals, then it is not chromite. Experimental: 1) Each person should be wearing safety glasses, pants, shoes, and a shirt. 2) Mineral chromite contains magnesium, iron, and chromium.
Hydrometallurgy to Analyze a Chromite Sample : Chromium can be used in the production of stainless steel and other nonferrous alloys in order to enhance their harden ability and to make the alloys more resistant to corrosion and oxidation. It can also be used to plate metals, make pigments, process leather, catalyze, and treat surfaces. Chromite is the only ore of chromium. Chromite is iron magnesium chromium oxide. Metallurgy can be used in order to recover the chromium from the chromite ore.
Aim: Magnesium with Hydrochloric Acid In this piece of coursework I will investigate to see if concentration affects the rate of reaction between Magnesium (Mg) and Hydrochloric acid (HCl). The rate of reactions using different concentrations of acid will allow me to do this. The rate of reaction involves how long it takes for the reactants to turn into products and so in this investigation we are looking at the amount of Hydrogen gas produced at different concentrations to see if concentration does affect the rate of reaction between Hydrochloric acid and Magnesium. In groups we had to carry out the reaction between the two elements to see how much Hydrogen gas was collected. Purpose of investigation: Picture 3 The purpose of this investigation was to see if concentration affects the rate of reaction between Magnesium and Hydrochloric acid.
Experimental Procedure: 250 mL of the copper solution was made by creating 100 mL of the solution, reacting CuO with HNO3, and then diluting to the mark of 250 mL. Using this stock solution, different concentrations were made and placed in the sprectrometer for observation. The absorbances and transmittances were recorded for use when identifying the amount of the color-absorbing copper ions later. A graph was plotted of Absorbance v. Molar Concentration easily see the results of the experiment. Pre-Lab Questions: 1.
Part 1 of The Redox Arena Objective: In this experiment, we had to conduct research on zinc, iodide, and acidified water. What my partner and I did was we mixed the aforementioned elements with acidified water to see what would happen. We took notes on the physical traits of each, and then we compared out qualitative results with the three samples we had. Materials & Observations: * electronic balance * Bunsen burner * Parafilm * Spatula * Boiling tube * Corks * large beaker * Stirring rod * large test tube * test tube rack * small graduated cylinder * pipets * grease pencil * Ziploc bag * Boiling chips- off white, small pebble like pieces * Desiccant- white small rocks, chalky * Acidified water- clear liquid * Sodium thiosulfate- clear liquid * Granular zinc- gray, small, mineral like * Iodine crystals- dark grey, shiny solid * Zinc ion- grey, irregular shaped * Solid zinc iodide- white solid * Mineral oil- colorless solution The Mass table was as followed: Chemicals | Amount | Granular Zinc | 2.01 grams | Iodine Crystals | 2.01 grams | Acidified Water | 5.0 mL | Procedure: 1. Obtain a boiling tube, a large test tube and a small test tube.
Si, P, S and Cl are increasingly electronegative. They cannot form oxide ions from oxygen at all, so they behave as acids. The trend is from strongly basic oxides on the left-hand side to strongly acidic ones on the right, via an amphoteric oxide (aluminium oxide) in the middle. In addition, when going across the period 3 the acid-base nature of the oxides change from base to amphoteric and finally to become acid. This is because the less electronegative sodium has a weak Na-O bond and the oxygen is more easily given up to reacts with H+.
When working dimethylglyoxamine, carefull attention has to be taken when adding the chemical because both an excess amount and insufficient amount of the organic compound will have an adverse effect. An excess amount of dimethylglyoxamine will ultimately dissolve nickel dimethylglyoxamine which would result in low percent recovery for nickel. An insufficient amount of dimethylglyoxamine, however, will cause some of the reagent to precipitate giving as a result a positive error in the percentage of nickel recovered. Materials and Methods To begin the experiment, three medium-porosity sintered-glass crucibles were brought to a constant mass by heating them for an hour at a constant 110 degrees Celcius. The initial