PURPOSE: To observe oxidation – reduction reactions. PROCEDURE: 1. Gather the following equipments: paper towel, well plate 24, plastic tweezers, copper (II) sulfate, iron (III) chloride, iron metal, magnesium metal ribbon, magnesium sulfate, 2 pieces lead metal, sodium sulfate, zinc metal, zinc nitrate. 2. Place 10 drops of sodium sulfate into A1 of the 24 well plate.
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.
This was done by taking small amounts of the unknown acid. It was then placed into capillary tubes and inserted into the Bibby Sterilin Device. Starting with a high plateau to find a quick melting point and then proceeding to find an actual melting point. The next experiment that aided in finding more characterizations of unknown #2651145-PLF13 was equivalent weight. In order to find the equivalent weight a titration of the unknown acid had to be conducted.
Gravimetric Analysis of a Metal Carbonate Post Lab TABLE Mass of Crucible + M2CO3 14.8145g Mass of Crucible + M2CO3 (1st weighing) 14.7915g Mass of Crucible 12.9405g Mass of M2CO3 1.851g Mass of filter paper + CaCO3 3.8025g Mass of filter paper 1.8120g Mass of CaCO3 1.9905g Moles of CaCO3 0.019887 mol Molar mass of M2CO3 93.08 g/mol Identity of M2CO3 Na2CO3 Percent Error 12.18% error ANALYSIS QUESTIONS 1. Calculate the moles of precipitated calcium carbonate, CaCO3. Enter this value in the Data Table. 1.9905g CaCO3 x 1 mol CaCO3 = 0.019887 mol CaCO3 1 100.09g 2. Calculate the molar mass of the unknown carbonate.
In the chart provided record if each compound is solubility in water. Part D - Conductivity 1. Obtain six 100ml beakers and add 50ml of water to each. 2. Place a 10g sample of each of the above compounds in a separate beaker.
Aim To compare the reactivity of various metals by observing their reaction with hydrochloric acid Hypothesis That the all the metals will produce foam and a pop. Variables Independent – Magnesium, Aluminium, Zinc, Copper Dependent – Detergent, Hydrochloric Acid Controlled – Size of the metals, amount of detergent and hydrochloric acid Materials 2 M hydrochloric acid Detergent 10 x test tubes and test tube rack and 5 rubber stoppers 0.5 cm pieces of magnesium, aluminium, zinc and copper 2 cm pieces of magnesium, aluminium, zinc and copper Steel wool Ruler Timer Bench mat Matches and birthday candle Marking pen Safety Remember to wear safety glasses and protective gloves when you do this experiment. 2 M HCl is corrosive. Wash with plenty of water should you get any on your skin or in your eyes. Method Part 1 1 Clean the surface of the 0.5cm piece of magnesium with a piece of steel wool 2 Place the magnesium into a test tube 3 Add three drops of detergent to the test tube 4 Add 2 cm of hydrochloric acid to the test tube.
The reduction of permanganate requires strong acidic conditions. Introduction: In this experiment a purple colored solution of potassium permanganate, with an approximate concentration of 0.025M, will be added to a solution containing Fe2+ ions. The manganese is reduced from a 7+ oxidation state in the permanganate ion to form colorless Mn2+ ions. The equivalence point is indicated at the point when all of the Fe2+ ions in the solution are oxidized and the colorless mixture retains a purple tint. Procedure: Fill a buret and tip with KMnO4.
The resulting material is heated with silica (SiO2) in flash smelting to remove the iron as slag. 2 CuFeS2 + 3 O2 → 2 CuS + 2 FeO + 2 SO2 FeO + SiO2 → FeSiO3 (slag) The copper matte (CuS) produced contains high concentration of copper, the sulfur is removed by blowing air through the molten matte. CuS + O2 → Cu + SO2 2 CuS + 3 O2 → 2 CuO + 2 SO2 This product is 98% pure copper but due to the broken surface created by the escaping sulfur dioxide gas, it is known as blister copper. To remove the oxygen, natural gas is blown through the molten copper oxide, and oxygen is burned off. The copper is then fed to electrolysis for refining.
Calculate the exact normality of Na2S2O3 knowing that in this chemical reaction 1 gram-equivalent of K2Cr2O7 react with 1 gram-equivalent of Na2S2O3 (1 mole K2Cr2O7 react with 6 moles Na2S2O3). Determination of peroxide value. Weigh 3.00 g oil (with precision of 0.001 g) into a 250 ml Erlenmeyer flask. Add 10 ml chloroform and swirl to dissolve oil. Add 15 ml acetic acid,
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+.