1.0 ABSTRACT The production of reducing sugars by acid of carbohydrate cereals powder‚ jams (total sugar content) and jams (reducing sugar content) were performed in order to study reducing sugar production. The study involved hydrolysis carbohydrate cereals powder and jams by immersing in boiling water at environmental temperature. Acid hydrolysis was carried out through reflux boiling for 20 minutes with 10ml 0f 1.5M concentrations of diluted sulphuric acid. Reducing sugars concentrations
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Cobalt(II) Oxygen adduct complex Inorganic 461 lab 2-29-2012 Abstract This experiment uses Co(salen) as a model compound illustrating the uptake of oxygen in hemoglobin. SalenH2 was prepared as the intermediate‚ and reacted with hydrated cobalt to prepare Co(salen). Using Co(salen) the oxygen up-take was tested. The synthesis of SalenH2 produced 0.65 g. The percent yield of salenH2 was 116% on the filter paper and 105% after transferring salenH2 to a vial. The melting point of salenH2‚ was
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whereby an ester is prepared‚ and involves heating a carboxylic acid with an alcohol in the presence of an acid catalyst‚ which is used to expedite the reaction. In this experiment the process was used to synthesis isopentyl alcohol‚ which was the limiting reagent‚ with sulfuric acid and excess of acetic acid. Had equal amounts of acetic acid and isopenthyl alcohol been used‚ approximately only two thirds of each would be converted to acetate. This mixture was heated under reflux for one hour to ensure
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Ramos and Kristina Todorovic Chemistry 203 DEN Dr. Mohamed El-Maazawi Part A. Acid-Base Indicators Purpose In this part of the experiment‚ we will find a reagent that will shift the acid-base equilibrium reaction described by Equation (2) in one direction and then a second reagent that will cause the equilibrium position to shift back in the opposite direction. Introduction An acid–base indicator is a substance that changes color as the pH of a solution changes
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Neutralization Titrations: The Determination of Sodium Carbonate from Unknown Soda Ash Unknown # I. Purpose: The goal of this experiment is to determine the weight % of Na2CO3 through the preparation of NaOH and HCl standards. The molarity of the standards will be found through titration of KHP for NaOH‚ HCl vs the known NaOH‚ and the unknown Soda Ash sample vs the known HCl. II. Equations and Sample Calculations: Titration of HCl with NaOH: Complete Equation: HCl (aq) + NaOH (aq)
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Synopsis The objective of this experiment is to determine the percentage by mass of calcium carbonate‚CaCO3 in toothpaste using back titration technique. A known weight portion of toothpaste is obtained to react with known volume and concentration of standard acid solution. After completing the reaction‚ the resulting solution containing excess acid is back titrated with known volume and concentration of standard base solution. Determination of excess acid after reaction allow us to calculate the
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potassium iodide. The reaction will release iodine:Example: (a) With KMnO4 2MnO4- + 16H+ + 10I(b) With KIO3 IO3- + 5I+ 6H+ 3I2 + 3H2O 2Mn2+ + 5I2 + 8H2O The iodine that is released is titrated against a standard thiosulphate solution. From the stoichiometry of the reaction‚ the amount of iodine can be determined and from this‚ the concentration of the oxidising agent which released the iodine‚ can be calculated. In an iodometric titration‚ a starch solution is used as an indicator as it can absorb
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Chemistry Stage 3 Standards Guide Exemplification of Standards through the 2010 WACE Examination Chemistry: Stage 3 Standards Guide 1 2010/33606 Copyright © Curriculum Council‚ 2011 This document—apart from any third party copyright material contained in it—may be freely copied‚ or communicated on an intranet‚ for noncommercial purposes by educational institutions‚ provided that it is not changed in any way and that the Curriculum Council is acknowledged as the copyright owner. Copying
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| Percent Yield Lab | | | | 4/20/2012 | Mrs.Sardella Per4 Matt ‚ Kait Mrs.Sardella Per4 Matt ‚ Kait | Introduction *Limiting Reactant: A reactant that is completely consumed during a chemical reaction‚ limiting the amount of product that is produced. *Excess Reactant: A reactant that remains after a reaction is over. *Theoretical Yield: The amount of product that is predicted by stoichiometric calculations *Actual Yield: The amount of product that is recovered
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Thermochemistry Saxon Evans & Zac Taylor Dr. Nachman 2/08/2011 Abstract: Using the chemical equation we can study the reaction taking place between magnesium metal and sulfuric acid in solution. The = for the reaction of sulfuric acid and magnesium metal. Introduction This report demonstrates calorimetry‚ or the technique of measuring heat effects in the surroundings. In order to make sure that there is no temperature change‚ or that it is an isothermal heat transfer‚ it is kept
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