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.
(b) Calculate the volume of 0.2M UO3- needed to react with 20.00 cm3 of 0.1M Cr2O72-. 3. 24.40 g of hydrated iron(II) sulphate, FeSO4.xH2O was dissolved and made up to 1.0 dm3 of aqueous solution, acidified with sulphuric acid. 25.00 cm3 of the solution was titrated with 20.00 cm3 of 0.022M potassium manganate(VII) solution for complete oxidation. a) Write the equation for the reaction.
Allow the mixture to cool for a few minutes then filter it, using either gravity or vacuum filtration. (We shall be using vacuum filtration.) Wash the residue in the funnel once with a little water and collect all the filtrate. 4. Pour all the filtrate and washings into a 250cm3 volumetric flask.
Indirect Gravimetric Determination of a Hydrated Compound in a Mixture Morgan Dufer I. The purpose of this lab was to find the percent of BaCl2*2H2O in a sample of unknown composition by using gravimetric analysis. II. Pre-lab Questions 1. What mass of MgCO3 is contained in a 2.750g solid sample consisting of only MgCO3 and MgO if heating to decompose all the MgCO3 according to the following equation leaves a solid residue weighing 2.160g?
AP Chemistry P2 Experiment 2: Formula of a Hydrate 9/24/2013 Purpose: Calculate the percent composition of water in a hydrate and determine the empirical formula of the hydrate. Procedure: 1) Set up ring stand with ring clamp, clay triangle, crucible with lid, and burner. Adjust the height of the ring stand. 2) Dehydrating Procedures: 3. Measure approximately 1 g of Copper(II) Sulfate Hydrate into the crucible and crucible and lid.
For zinc ion to react, the NaEDTA must also be an ion in the solution which means that the large salt must be dissolved in water. Procedure 1) Weighed out 3.64 of NaEDTA on an electronic beam balance 2) Added this mass of NaEDTA using wide mouth funnel to a 250 mL volumetric flask. 3) Rinsed the funnel with a squirt bottle containing deionized water making sure none of the solid remained in the funnel. 4) Added about 100-200 mL of deionized water to the volumetric flask containing the solid NaEDTA. 5) Swirled the solution until the NaEDTA (s) dissolved entirely.
4. Any hanging drop was removed from the jet, and the sodium hydroxide was then drawn up using the pipette, to above the graduation mark and allowed to run into the sink. This process was the rinsing of the pipette. 5. Sodium hydroxide was again drawn up using the pipette, to above the graduation mark, where the meniscus was allowed to fall until the bottom of it was rested on the graduation mark when viewed at eye level.
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
10. Repeat the procedure for a second metal. Analysis: Our data | Trial #1 | Trial | Mass of zinc | 1.99g | 4.01g | Mass of water in Calorimeter | 45g | 45g | Temp. of water in Calorimeter | 20°C | 21°C | Temp. of boiling water | 100°C | 100°C | Peak temp.
Gravimetric Determination of Sulfate Purpose The purpose of this lab is to determine the percentage of sulfate in the hydrate by precipitating the sulfate as barium sulfate. Materials Filler paper Sodium sulfate Graduated cylinder Bunsen burner Watch glass Beakers (250 mL, 400 mL) Rubber bulb Graduated pipette Beaker tongs Funnel Filter Paper Sodium Sulfate Drying oven Wash bottle Stirring rod Silver nitrate Hydrochloric acid Distilled water Small test tube Procedures First, .4861 grams of sodium sulfate was placed into a clean 400mL beaker. Exactly 200mL of water and 1mL of HCl was added to the same beaker. A watch glass was placed on the beaker and the solution was heated using the Bunsen burner to a gentle boil. The watch glass was removed with the beaker tongs.