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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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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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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| 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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Chemistry102 5/7/2013 Lecture Presentation Chapter 17 Additional Aspects of Aqueous Equilibria John D. Bookstaver St. Charles Community College Cottleville‚ MO © 2012 Pearson Education‚ Inc. Common Ion Effect HA(aq) + H2O(l) ⇔ A−(aq) + H3O+(aq) • Adding a salt containing the anion NaA‚ which • is the conjugate base of the acid (the common ion)‚ shifts the position of equilibrium to the left This causes the pH to be higher than the pH of the acid solution 9lowering the H3O+ ion concentration
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Introduction An electrophile is a reagent attracted to electrons and accepts an electron pair in order to bond to a nucleophile. Electrophiles will attack benzene and result in hydrogen substitution. However‚ this is not thermodynamically favoured because a sp3 hybridized carbon is generated‚ which disrupts the cyclic conjugation. In order to regenerate the aromatic ring‚ a proton is lost at the sp3 hybridized carbon. Thus‚ p-Nitroaniline can be prepared by means of electrophilic aromatic substitution
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solution was swirled‚ it became orange again. At the end point‚ the solution turned from orange to pink. Calculations 2HCl + Na2CO3 -> 2NaCl + CO2 + H2O Therefore‚ mole ratio of Hydrochloric Acid to Sodium Carbonate is 2:1 Percentage uncertainty of volume of HCl = 0.10/14.63 * 100 = 0.68% Percentage uncertainty of volume of Na2CO3 = 0.06/25 * 100 =0.24% Number of moles of sodium carbonate
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Water Technology Hardness of Water: Natural waters containing large quantities of dissolved salts of Calcium (Ca) & Magnesium (Mg) is called hard water. It is a characteristic of preventing lather formation of water with soap. Ca2+ & Mg2+ ions react with soaps which are salts of fatty acids (stearic or palmitic acid) to give insoluble scums or precipitates of calcium or magnesium stearate or palmitate. 2C17H35COO- + Ca2+ → (C17H35COO)2 Ca (scum) 2C17H35COO- + Mg2+ → (C17H35COO)2
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