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    OXIDATION-REDUCTION TITRATIONS REDOX TITRATION •  involves oxidizing agents and reducing agents titrants and analytes •  oxidizing agents used as standard solutions:   potassium permanganate‚ KMnO4   potassium dichromate‚ K2Cr2O7   iodine‚ I2   ceric sulfate‚ Ce(SO4) 2   potassium iodate‚ KIO3 REDOX TITRATION •  reducing agents used as standard solutions:   ferrous sulfate‚ FeSO4   oxalic acid‚ H2C2O4   sodium oxalate‚ Na2C2O4   sodium thiosulfate‚ Na2S2O3   titanous chloride

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    Fe(NH4)2(SO4¬)2.6H2O = 392.13gmol-1 Volume of Fe(II) solution prepared = 0.250L Standardizing Potassium Permanganate Solution Stated concentration of KMnO4 (aq) on container = 0.02mol Volume of Fe(II) solution pipetted for titration = 25.0mL Burette Reading (mL) Titration Numbers 1 2 3 4 5 Final 24.40 25.00 49.30 23.80 47.50 Initial 0.00 0.00 25.00 0.00 23.80 Titre 24.40 23.80

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    | A little book of tips for titrations. • Recording results • Calculating the average titre • Evaluation of results • Evaluation of procedures Recording results and calculating the average/mean titre: |Titration |Rough |1 |2 |3 |4 |5 | |Initial burette

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    INTRODUCTION Differences between acids and bases An acid-base reaction is based on the reaction involving the ionization of water H2O -> H+ + OH- This means that water can break apart into a hydrogen ion and a hydroxide ion. These two ions can also join together to form a water molecule. When a strong acid is placed in water‚ it will ionize completely‚ and break down into its constituent ions in which one of it a hydrogen ion. When a strong base is placed in water‚ it will ionize

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    Name: Susan Sooklal Partner’s Name: Adana Taylor & malia Taylor Date: 26.02.2013 Title: titration method AIM 1. To titrate sodium hydroxide with hydrochloric acid Apparatus: * Burette (50cm3) * Pipette (10cm3) * Three (3) Conical Flasks (250cm3) * Two (2) Beakers (250cm3) * Funnel * Wash Bottle * Retort Stand * Boss and Clamp * Pipette filler Material: * 0.08 mol dm-3 hydrochloric acid * 0.1 mol dm-3 sodium

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    ------------------------------------------------- Titration From Wikipedia‚ the free encyclopedia   (Redirected from Back titration) Not to be confused with the mathematical notion of tetration. This article is about volumetric titration. For other uses‚ see Titration (disambiguation). A Winkler titration to determine the concentration of dissolved oxygen in a water sample Titration‚ also known as titrimetry‚[1] is a common laboratory method of quantitative chemical analysis that is used

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    Titration is a common laboratory method of quantitative chemical analysis that is used to determine the unknown concentration of a known reactant. Because volume measurements play a key role in titration‚ it is also known as volumetric analysis. A reagent‚ called the titrant or titrator‚[1] of a known concentration (a standard solution) and volume is used to react with a solution of the analyte or titrand‚[2] whose concentration is not known. Using a calibrated burette or chemistry pipetting syringe

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    Experiment #10 Volumetric Analysis The Titration of Acids and Bases Purpose This experiment will allow you to gain practical experience in the preparing standard solutions‚ using a pipette and a buret‚ and performing standard titrations. You will use this experience to experimentally determine the concentration of acetic acid in an unknown solution. There are three parts to this experiment‚ they are 1. Preparation a standard solution of oxalic acid (~0.07 M) 2. Preparation a sodium

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    hydroxide solution to 50ml. 2. Pipette the KH(C8H4O4) solution into a conical flask. Use three drops of phenolphthalein as the indicator. 3. Titrate carefully until a colour change from colourless to pink is observed. 4. Perform a rough titration first‚ then repeat until 3 concordant

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    Redox Titration Analysis of a Commercial Bleach A. Purpose ! ! ! To review oxidation-reduction reactions and their stoichiometry. To learn the concept and technique of redox titration. To determine the percent (m/v) of an active ingredient‚ sodium hypochlorite (NaOCl)‚ in a commercial bleaching agent. B. Theoretical Background Whereas acid-base reactions involve the transfer of a proton‚ oxidation-reduction or redox reactions involve the transfer of electrons from one substance to

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