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1. Find the mass of five iron tablets. Crush the weighed tablets in a mortar and pestle to give a large surface area to volume ratio. This will mean that the rate of reaction will be increased because the more particles are exposed to the other reactant, which will be sulfuric acid.
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2. Transfer all the ground material to a beaker where it will be dissolved in approximately 100cm3 of the 1 mol dm-3 of aqueous sulfuric acid. Sulfuric acid is used instead of deionised water because the titration needs to be carried out under acidic conditions. Iron (II) is less likely to be oxidised to iron (III) by atmospheric oxygen in acidic solution than in neutral solution and for an accurate result the iron should not be converted to iron (III) before the titration is conducted.
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3. All of this solution (including washings) is transferred to a 250cm3 volumetric flask and the solution made up to the mark with deionised water. Deionised (distilled) water is used as it does not contain ions or impurities that may affect the results of the titration, usually by reacting with acid/alkali themselves or by changing the pH of the solution. As water is pH 7, it is neutral and will not change the pH. A pipette should be used when the solution is very close to the gradation line. The solution should be brought up to the graduation line so that the bottom of the meniscus lines up with the flask’s graduation mark. The pipette can be used to remove the excess solution. The volumetric flask should be stoppered and inverted several times. This is done to ensure that the solution is thoroughly mixed so that the reactants can react together. This is the standard solution containing iron (II) ions.
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4. Wash the pipette, burette and conical flask with deionised water. Rinse the burette with the potassium manganate (VII) solution and the pipette with the iron(II) solution. Using a pipette filler, fill the pipette with the iron(II) solution and transfer the contents of the pipette to the conical flask. Acidify this solution by adding 10cm3 of dilute sulfuric acid. If a brown precipitate appears during the titration this means that Mn(IV) is formed, because of incomplete reduction of the Mn(VII). This should only happen if there is insufficient sulfuric acid in the conical flask. The remedy is to add more dilute sulfuric acid to the flask, or, preferably, to repeat the experiment with sufficient acid present in the flask.
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5. Using a funnel, fill the burette with potassium manganate (VII) solution, making sure that the part below the tap is filled before adjusting to zero. Because of the intense colour of KMnO4 solution, readings are taken from the top of the meniscus.
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6. With the conical flask standing on a white tile, add the solution from the burette to the flask. Swirl the flask continuously and occasionally wash down the walls of the flask with deionised water using a wash bottle.
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7. The end point of the titration is detected by ‘the first persisting pink colour’. Note the burette reading.
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8. Repeat the procedure ten times, adding the potassium manganate (VII) dropwise approaching the end point. These accurate titres should agree to within 0.1cm3. Calculate the concentration of the iron (II) solution and from this calculate the mass of iron in an iron tablet.
1.
1. Find the mass of five iron tablets. Crush the weighed tablets in a mortar and pestle to give a large surface area to volume ratio. This will mean that the rate of reaction will be increased because the more particles are exposed to the other reactant, which will be sulfuric acid.
1.
2. Transfer all the ground material to a beaker where it will be dissolved in approximately 100cm3 of the 1 mol dm-3 of aqueous sulfuric acid. Sulfuric acid is used instead of deionised water because the titration needs to be carried out under acidic conditions. Iron (II) is less likely to be oxidised to iron (III) by atmospheric oxygen in acidic solution than in neutral solution and for an accurate result the iron should not be converted to iron (III) before the titration is conducted.
1.
3. All of this solution (including washings) is transferred to a 250cm3 volumetric flask and the solution made up to the mark with deionised water. Deionised (distilled) water is used as it does not contain ions or impurities that may affect the results of the titration, usually by reacting with acid/alkali themselves or by changing the pH of the solution. As water is pH 7, it is neutral and will not change the pH. A pipette should be used when the solution is very close to the gradation line. The solution should be brought up to the graduation line so that the bottom of the meniscus lines up with the flask’s graduation mark. The pipette can be used to remove the excess solution. The volumetric flask should be stoppered and inverted several times. This is done to ensure that the solution is thoroughly mixed so that the reactants can react together. This is the standard solution containing iron (II) ions.
1.
4. Wash the pipette, burette and conical flask with deionised water. Rinse the burette with the potassium manganate (VII) solution and the pipette with the iron(II) solution. Using a pipette filler, fill the pipette with the iron(II) solution and transfer the contents of the pipette to the conical flask. Acidify this solution by adding 10cm3 of dilute sulfuric acid. If a brown precipitate appears during the titration this means that Mn(IV) is formed, because of incomplete reduction of the Mn(VII). This should only happen if there is insufficient sulfuric acid in the conical flask. The remedy is to add more dilute sulfuric acid to the flask, or, preferably, to repeat the experiment with sufficient acid present in the flask.
1.
5. Using a funnel, fill the burette with potassium manganate (VII) solution, making sure that the part below the tap is filled before adjusting to zero. Because of the intense colour of KMnO4 solution, readings are taken from the top of the meniscus.
1.
6. With the conical flask standing on a white tile, add the solution from the burette to the flask. Swirl the flask continuously and occasionally wash down the walls of the flask with deionised water using a wash bottle.
1.
7. The end point of the titration is detected by ‘the first persisting pink colour’. Note the burette reading.
1.
8. Repeat the procedure ten times, adding the potassium manganate (VII) dropwise approaching the end point. These accurate titres should agree to within 0.1cm3. Calculate the concentration of the iron (II) solution and from this calculate the mass of iron in an iron tablet.
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Im confused about this chemistry question, why does it form these productsLast reply 1 week ago
Im confused about this chemistry question, why does it form these products