and Technology CHE: 205L: CHEMICAL ANALYSIS LABORATORY Experiment IV Redox Titration Name: Helena Al Jawhary / Partner’s Name: Eyad Aridi Instructor’s Name: Dr Juliana El Khoury Date of experiment: 10/3/2013 Redox Titration Objective: • To learn some technique in volumetric analysis: Redox titration. • To review the stoichiometry of an oxidation-reduction reaction. • To practice the titration technique. • To determine the concentration of an unknown sodium oxalate (Na2C2O4)
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of H2O2 and transfer that into the Baseline cup. Fourth‚ we gently swirled the contents of the Baseline cup to mix the solution. Then‚ we used the syringe labeled Transfer and removed 5 mL of the solution in the Baseline cup into the cup labeled Titration. Lastly‚ we titrated the 5 mL sample of the Baseline solution.
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Determination of the relative atomic mass of lithium Introduction: For this investigation I will determine the Relative atomic mass (Ar) by using two different methods. In the first method I will dissolve a piece of lithium of a known mass in water‚ I will then collect the hydrogen gas produced‚ which can be used to calculate the relative atomic mass of Lithium. In the second method I will titrate the resulting solution of lithium hydroxide with a known concentration of hydrochloric acid‚ this
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between KMnO4 and oxalic acid is a redox reaction and the titration is therefore called a redox titration. 2. Oxalic acid is the reducing agent and KMnO4 is the oxidizing agent. 3. KMnO4 acts as an oxidizing agent in all the mediums; i.e. acidic‚ basic and neutral medium. 4. KMnO4 acts as the strongest oxidizing agent in the acidic medium and therefore dil. H2SO4 is added to the conical flask before starting the titration. 5. The titration
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ABSTRACT In the majority field of chemical processes‚ the reactor vessel in which the reaction process take place is the key component of the equipment.The design of the reactors is very important to the success of the production. In this experiment‚ sodium hydroxide and ethyl acetate react in tubular flow reactor.Both of the reactants fed to the reactor at equimolar flowrate for a certain time.The reaction is carried out at different volumetric flowrate.The conductivity value of outlet stream
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Acid Base Titration Purpose: The purpose is to calculate the molarity of a NaOH solution by titrating the base with 5mL of standard HCl solution in each trial. By adding the base with unknown molarity to the acid with 0.10M the molarity of NaOH can be calculated. The base‚ NaOH‚ helps bring the pH of the acid‚ HCl‚ closer to seven‚ which neutralizes it. When using the buret the amount of NaOH used is able to be determined. Then by writing a balanced chemical equation and using the titration
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BACKGROUND: Esterification is a reaction that combines an alcohol with an organic acid‚ with a water molecule is being taken out‚ and an ester is formed. A concentrated acid catalyst speeds up the esterification. In this experiment set up‚ sulphamic acid was used‚ as it is a solid acid and be added dry‚ without any water‚ which is a reactant in this experiment equilibrium. Esterification is a slow and reversible reaction. The equation for the reaction between an acid RCOOH and an alcohol RẬᶦ
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the prepared KHP from the previous part into a 250ml Erlenmeyer flask and added 2 drops of the indicator‚ phenolphthalein. Next we filled the burette with the approximately 0.1 M NaOH so that our initial volume will be 0.0mls. We then started our titration by carefully pouring a little amount of the base into the prepared 25ml of KHP with phenolphthalein until we reached the end point. Since the molarity of the NaOH was designed to be more or less the same with the acid‚ we knew that it would take
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Objective: This lab focuses on the detection of ions using titration as an analysis tool. You will standardize NaOH and HCl solutions so that you know the exact concentration and then prepare samples of common household items in order to determine the amount of calcium in Tang®‚ Mg(OH)2 in Milk of Magnesia‚ etc. You will learn to prepare samples of a specified concentration‚ learn about acids and bases through the use of titrations and learn how to detect endpoints using different indicators
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reacts with carbon dioxide from the air. In that case‚ it cannot be accurately weighed in air. In an experiment like this‚ a solution of the approximate required concentration was prepared. Afterwards‚ the exact concentration was determined by titration against a solution whose concentration can be calculated accurately from careful weighing. This experiment included a standard solution‚ which according to Lewis‚ R. and Evans‚ W. 2011‚ “is a solution of known concentrations”. They also stated that
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