formation of a white ring around the glass closer to the side of the heavier substance (HCl‚ M = 36.4611 g/mole; dAve = 10.8 cm). The agar-water gel set up was composed of a petri dish of agar-water gel containing three wells. Drops of potassium permanganate (KMnO4)‚ potassium dichromate (K2Cr2O7) and methylene blue were simultaneously introduced to each well. Methylene blue‚ having the largest molecular weight‚ displayed the smallest diameter (18 mm) and diffused at the slowest rate (0.3668 mm/min.). Thus
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which diffused at a faster rate of 24.8 cm and formed a white smoke near the HCl end that had the molecular weight of 36 g/mole. The water agar-gel setup was made up of a petri dish containing the gel with three wells. Drops of potassium permanganate (KMnO4)‚ potassium dichromate(K2Cr2O7) and methylene Blue were concurrently placed in the wells. Methylene Blue had the smallest diameter which diffused at the slowest Rate of 0.13 mm/min since it has the largest molecular Weight. Thus‚ the larger
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Lab 4: Titration of a Redox Reaction The purpose of this experiment is to standardize a solution of Mohr’s salt‚ and to use titration to determine the volume ration of ferrous solution to the permanganate standard and calculate the concentration of the ferrous solution. First‚ Mohr’s salt was mixed with H2SO4. Then‚ the solution was titrated until the end point was reached. The volumes were recorded‚ and used to calculate the molarity of the ferrous solution. The major
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sulfuric acid was added after the allotted time and acted as an inhibitor. The inhibitor left a mixture of the products and original hydrogen peroxide. Our titrant of potassium permanganate (KMNO4) shows through its purple color the remnants of the hydrogen peroxide‚ which we were able to record. Hypothesis: If we add potassium permanganate to our mixtures then those beakers that were given a longer duration to react will require less titrant because of the little amount of unreacted hydrogen peroxide
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of EXPERIMENTAL METHODS Preparation of the 0.15M Potassium Permanganate (KMnO4) solution {text:list-item} B. Prepare precipitation mixtures 1. Obtain three labeled 20-mL vials from the cart. 2. Burets are set up in the lab with 0.250 M MgSO4 and 0.250 M Na2C2O4. Refer to Table 1‚ and add the appropriate volume of each solution to the numbered vials. Table 1. Precipitation reactant volumes Standardize the Permanganate Solution {text:list-item} {text:list-item} {text:list-item}
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Aim To prepare a standard iron (II) solution To determine the concentration of potassium permanganate solution Instructions Preparation of Standard Iron (II) Solution 8g of hydrated iron (II) ammonium sulfate is weighed accurately using a 50mL beaker. The salt is transferred to a 250mL volumetric flask using a filter funnel‚ washed down with distilled water. The container is rinsed carefully and the rinsing is added to the volumetric flask. 100mL of water is added slowly to the volumetric
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components. * To standardize potassium permanganate solution KMNO4‚ which then be used for titration of iron unknown solution. * To write the net ionic equations of redox reaction carried out in this experiment. * Concept of experiments: * A standard KMNO4 solution‚ used in this experiment as titrant‚ cannot be prepared directly by dissolving of a known amount of solid KMNO4 because this reagent is a very strong oxidizing agent. Solutions of potassium permanganate are unstable and their concentration
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Hydrocarbons Equipment Required: -4 Test tubes -Dropper - Cyclohexane (C6H12) (3ml) - Cyclohexene (C6H10) (3ml) - Toluene (CH3C6H5) (3ml) - Potassium Permanganate solution (KMnO4) .01 mol L-1 (4ml) - Sulfuric Acid (H2SO4) 2mol L-1 (2ml) - Bromine Water (Br2) (5ml) Procedure: Reaction of hydrocarbons with acidified permanganate: 1) Into three separate‚ labeled test tubes place 1 ml of cyclohexane‚ cyclohexene and toluene respectively. 2) In a separate test tube add 4 ml of 0
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to standardize a solution of potassium permanganate by redox titration with a standard solution of iron (II) ions. A solution of oxalic acid is then titrated with the permanganate solution to determine the exact concentration of oxalic acid. Purpose: The purpose of the experiment was to use the permanganate ion‚ a strong oxidizing agent‚ in a titration in order to determine the concentration of a FeSO4 solution. Purple MnO4- ion from a standardized potassium permanganate solution was titrated thrice
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hydrogen peroxide in a consumer product? Design: An acidic solution of primary standard‚ iron (II) ammonium sulfate-water (1/6)‚ is prepared and the potassium permanganate standard. A 25.0 mL sample of a consumer solution of hydrogen peroxide is diluted to 1.00 L with water (that is‚ it is diluted by a factor of 40). The standardized potassium permanganate solution is used to titrate the diluted and acidified hydrogen peroxide. The amount concentration of the original hydrogen peroxide is obtained by
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