prepare a standard solution of ammonium iron sulphate and use this solution to standardise a solution of potassium permanganate. Potassium permanganate (KMnO 4 ) is a powerful oxidizing agent and is a deep purple colour. It cannot be obtained in sufficiently pure form to weigh it out accurately and make up a standard solution directly. We must titrate an approximate solution of potassium permanganate (0.02 M) against a primary standard solution‚ ammonium iron sulphate (0.1 M). Prepare the ammonium iron
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solution being colorless indicated a positive sign of a double bond being present in 4-methylcyclohexene. The second test used potassium permanganate solution to test for the presence of alcohol. When 4-methylcyclohexanol was mixed with the potassium permanganate solution‚ the color changed from a clear solution to deep dark purple color. When the potassium permanganate solution was combined with 4-methylcyclohexene the color changed to brown‚ indicating the presence of the desired product. When
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various aspects of kinetics of three reactions. A. Reaction between lead nitrate (PbNO3) and potassium chromate (K2CrO4) solutions B. Reaction between potassium permanganate (KMnO4) and oxalate ion (C2O42-) C. Iodine clock reaction A. REACTION BETWEEN LEAD NITRATE AND POTASSIUM CHROMATE SOLUTIONS Lead nitrate reacts with potassium chromate to form yellow lead chromate precipitate and aqueous potassium nitrate. The formation of a yellow precipitate indicates the completion of the reaction. The
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OBJECTIVES: To determine the maximum wavelength of potassium permanganate. To plot the calibration curve of potassium permanganate. To determine the concentration of an unknown solution of potassium permanganate. INTRODUCTION: UV Spectrophotometer has 4 main components which is the UV light source‚ the sample‚ detector and the processor/recorder. Spectrophotometry is a technique that uses the absorbance of light by an analyte (the substance to be analyzed) at a certain wavelength to determine
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copper nitrate solution. 3. Observe what happens when copper metal is placed in zinc nitrate solution. 4. Observe whether 0.1 M iron (III) chloride solution or iron (II) sulfate decolorize when added to 0.1 M potassium permanganate. 5. Add drops of potassium permanganate to the solution that changed color in the previous step. Record how many drops were added until the purple color of the ion no longer changed. 6. Observe color changes when sodium iodide solution is reacted with
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between potassium permanganate with oxalic acid. We used 2cm3 of 0.02M potassium permanganate and 4cm3 of 1M sulphuric acid into a test tube. In another test tube‚ we placed 2cm3 of oxalic acid. We placed the test tubes in a water bath at 40‚ 45‚ 50‚ 55 and 60oC respectively. When the solutions have attained these temperatures pour the oxalic acid into the acidified permanganate solution and recorded the time taken for the permanganate to decolorize. At 400C ‚ the time taken for the permanganate to decolorize
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Permanganate Process (McBride Method) Optical Method of Analysis: Use of Beer’s Law on KMnO_4 Solution Abstract Potassium permanganate (KMnO_4) is commonly used as an oxidizing agent and in this experiment‚ it is used as both the titrant and indicator. A standard of potassium permanganate solution was prepared and computed to be 0.02235 M and was used to titrate a sulfuric acid solution wherein the sample salt was dissolved. The solution was heated to 90°C then titrated until a light pink colored
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Title : Properties of hydrocarbon Objective : 1) To study the properties of hydrocarbons. 2) To determine the unknown samples. Results : Part A : Combustion Compounds Observations Hexane There was orange flame and burned mildly during the burning process. No soots and smoke were produced. C6H14 + 19/2 O2 6CO2 + 7H2O Cyclohexene Orange flame burned vigorously. A small amount of black soot and smoke were produced during the burning process.
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Preparation of the Complex A sample of copper sulfate pentahydrate (6.285g) was weighed out. The copper sulfate pentahydrate was dissolved in water (11.99mL) in a 250mL beaker. The solution was heated on a hot plate to 90 degrees Celsius. A sample of potassium oxalate monohydrate (10.006g) was dissolved in water (50.0mL).
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A theoretical mass of 1140 mg and an experimental mass of 263 mg resulted in a 23.1% yield. This low percent yield is most likely due to error in the experiment. The potassium permanganate test was positive for the presence of a double bond in the product as brown precipitate formed along with the discoloration of the solution. An IR spectroscopy of the product was also performed. Results of the IR absorptions of this experiment
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