are extracted from the fruit by boiling pulp with dil. H2SO4. Then oxalate ions are estimated volumetrically by titrating the dilution with standard KMnO4 solution. fig:- Oxalate Ion Requirements: - 100 ml. Measuring flask‚ pestle & mortar‚ beaker‚ titration flask‚ funnel‚ burette‚ weight-box‚ pipette‚ filter paper‚ dilute H2SO4‚ N/20 KMnO4 solution‚ guava fruits at different stages of ripening. PROCEDURE 1.) Weigh 50.0 g of fresh guava & crush it to a fine pulp using pestle-mortar.
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Experiment: Comparing reactivities of alkanes and alkenes Aim: To compare the reactivities of an alkane and an alkene with bromine water and a solution of potassium permanganate (KMnO4). Equipment: • 4 test tubes • Test-tube rack • 4 pipettes Safety: safety glasses must be worn to prevent injury to the eyes. Ensure room is well ventilated whilst using the hydro carbons. Method: 1. Place 1 ml of sample A (cyclohexane) into a test tube containing 4 mls of the bromine water solution. Record
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(W/W) of NiCl2 was recorded to calculate the apparatus constant as 5.7538. cv and cm for each solution was determined in order to calculate the number of unpaired electrons for each paramagnetic complex. Fe(NH4)2(SO4)26(H20) had 4 unpaired electrons‚ KMnO4 had zero unpaired electrons‚ and K3[Fe(CN)6] had 1 unpaired electron. The apparent 1 unpaired electron in K3[Fe(CN)6] when there should be five according to atomic orbital calculations arises from a strong ligand field produced by CN-. Introduction:
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In this experiment it is used to visually identify the production in the previous reaction‚ since it changes color from purple to yellow-brown if reacted with alkene under aqueous conditions. Balanced equation: C10H14O2 + KMnO4 + 2H2O --> C10H16O4 Mechanism: 2 - Table of reagents . |Compound |Mol Mass (g/mol) | |Dissolution of MCPBA in CH2Cl2
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Investigation:1.5.1) Observations: Experiment 1: Using HCl(aq) Alcohol Observed Properties Structural Diagram 1-butanol -No reaction 2-butanol -Slightly cloudy 2-methyl-2-propanol -White and cloudy -Steam Experiment 2: Using KMnO4 (aq) Alcohol Observed Properties Structural Diagram 1-butanol -Very thick
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Ketones lack the easily removed hydrogen that is adjacent to the carbonyl. The goal of this experiment is to carry an oxidization of diphenylmethanol with a solid oxidant of KMnO4 and CuSO4. Scheme 5.5: KMnO4 is the oxidant in this reaction that oxidizes the alcohol to the ketone. The CuSO 4 is there to support the KMnO4. The oxidant reacts with the secondary alcohol which forms benzophenone and MnO2. Then the melting point of the hexanes will be identified. The reactant is a secondary alcohol
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rinsed with 3 mL of KMnO4. Once rinsed‚ the burette was filled with KMnO4 to an initial volume of 2.5 mL. The solution was placed under the burette and a stir bar was put in the 125 mL Erlenmeyer flask. The solution was then titrated with the KMnO4 in 1 mL intervals until a light pink color was achieved and held for 30 seconds. 31.10 mL of KMnO4 were added in order to achieve the desired color of light pink. The second solution was then also heated to 80 ºC and titrated with KMnO4 in the same way. 30
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LAB REPORT Group: 6 Section: Group member: Phạm Thanh Thủy ID: BTARIU12005 Course name : GENERAL CHEMISTRY LABORATORY Period : 2012-2013 Date performed : 11-03-2013 Date submitted : 02-05-2013 INSTRUCTOR’S NAME : Hoàng Lê Sơn EXPERIMENT 1: CHEMICAL REACTIONS I. INTRODUCTION – OBJECTIVES In this first experiment‚ we will perform 8 chemical reactions and 1 flame test in order to determine 2 things : a) firstly‚ we can know
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of the tests with Br2 and KMnO4‚ as well as the IR absorbtion spectrum of the final product. Purpose: The purpose of this experiment is to obtain pure 4-methylcyclohexene by reacting 4-methylcyclohexanol and phosphoric acid. Through distillation‚ extraction‚ and drying‚ the crude product is isolated. The crude product is then distilled and collected to produce a product which was determined to be pure after testing it with Br2 and KMnO4 as well as completing an IR
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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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