red solutions that will lead to a possible identity of each red solution. Starting with red solution #1‚ we are able to conclude that there are no nanoparticles in this solution and that is a molecular compound due to the fact that when potassium iodide was added‚ there was no color change and no precipitate formation to indicate that a chemical reaction had happened. Having no color change occur when an ionic compound is added to a solution means that the solution is
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ANALYSIS OF VITAMIN C IN COMMERCIAL FRUIT JUICES BY IODOMETRIC TITRATION. SHAMSUL AZRIN BIN MD. KANAFE Final Year Project Report Submitted in Partial Fulfilment of the Requirement for the Degree of Bachelor of Science (Hons.) Chemistry in the Faculty of Applied Sciences‚ Universiti Teknologi MARA. APRIL 2009 This Final Year Project Report entitled “ANALYSIS OF VITAMIN C IN COMMERCIAL FRUIT JUICES BY IODOMETRIC TITRATION” was submitted by Shamsul Azrin Bin Md. Kanafe‚ in partial
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Experiment 8 Unique # 51070 The main purpose of the experiment involves two oxidation-reduction reactions to calculate the oxidizing capacity of a sample of unknown bleach. In order to determine the volume of Na2S2O3 added‚ students will conduct a titration of bleach with thiosulfate with addition of a starch indicator to find the end point of the titration. Moreover‚ the oxidizing capacity of bleach is calculated with the percentage by mass of NaOCl in the unknown bleach sample. The overall
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VIHS/ Department of Chemistry Chemistry Revision Unit II (Edexcel) (01) a) When lithium nitrate and sodium nitrate are heated separately‚ both decompose giving oxygen gas as one of the products. (i) Which of these two nitrates would decompose at the lower temperature? .........................................................………………………………………….................... (ii) Give the name of any other product formed when sodium nitrate is heated. .....................................................
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unstable and inconvenient to work with‚ you will titrate vitamin C samples in this lab with potassium iodate‚ KIO3‚ in the presence of an acidic iodide solution. The iodate ion oxidizes iodide to iodine. IO3Ϫ ϩ 5IϪ ϩ 6Hϩ 1 3I2 ϩ 3H2O Notice that an equilibrium is established. To ensure that the reaction goes to completion‚ it is necessary to use excess iodide and to make the solution acidic. The iodine formed in this reaction immediately
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Department of Chemistry‚ Grinnell College‚ Grinnell‚ Iowa 50112‚ United States S Supporting Information * ABSTRACT: A simple organic chemistry experiment is described that investigates the kinetics of the reaction between 1-bromobutane (BuBr) and iodide (I−) as followed by observing the disappearance of BuBr and the appearance of 1-iodobutane (BuI) using 1H NMR spectroscopy. In small groups of three to four‚ students acquire data to examine the concentrationdependence of both the organic substrate
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11/10/2014 experiment 1 Analysis of Commercial Vitamin C Tablets Objective To employ titration technique to determine the content of vitamin C in commercial tablets using volumetric analysis and compare it with the manufacturers’ specifications. Introduction Deficiency of essential antioxidant Vitamin C in human will lead to scurvy. In this experiment‚ the vitamin C content of commercial tablets is determined and then compared with the manufacturers’ specifications. Vitamin C‚ ascorbic
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SYLLABUS Cambridge O Level Chemistry 5070 For examination in June and November 2014 University of Cambridge International Examinations retains the copyright on all its publications. Registered Centres are permitted to copy material from this booklet for their own internal use. However‚ we cannot give permission to Centres to photocopy any material that is acknowledged to a third party even for internal use within a Centre. © University of Cambridge International Examinations 2011 Contents
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Reagent - 1.5 mL in Vial 2 Pipet‚ Empty Short Stem 1 Silver Nitrate‚ 0.1 N - 6 mL in White Dropper Bottle 1 Sodium Bromide‚ 0.1 M - 2.5 mL in Pipet 1 Sodium Carbonate‚ 0.25 M - 2.5 mL in Pipet 1 Sodium Chloride‚ 0.1 M - 2.5 mL in Pipet 1 Sodium Iodide‚ 0.1 M - 2.5 mL in Pipet 1 Sodium Phosphate‚ 0.1 M - 2.5 mL in Pipet 1 Sodium Sulfate‚ 0.1 M - 2.5 mL in Pipet 1 Sodium Sulfide‚ 0.1 M - 2.5 mL in Pipet 1 Unknown - 5 mL in Pipet 1 Lead Acetate Strips - 2 in Bag 2"x 3" – Assembly Procedure 1. Before
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Laboratory Report Title: Observation of Chemical Change Course: General College Chemistry Purpose This experiment examines the reactions of common chemical s contained in consumer products. The purpose is to observe the macroscopic changes that these chemicals undergo. The goals of the experiment observe properties of chemical reactions and to associate chemical properties with household products. Procedure We do not have the ability to see with a naked eye individual atoms and molecules
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