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An iodine / thiosulfate titration - Yola

An iodine / thiosulfate titration Specimen Results (standardising a thiosulfate solution). 3. Rough titre = cm Theory 3. Second titre = cm Aqueous iodine solutions normally contain potassium iodide (KI), 3. Third titre = cm which acts to keep the iodine in solution. This is due to the fact that an 3. Average of accurate titres = cm equilibrium is set up as follows: 3. Volume of iodine solution used in each titration = cm - - I2 + I I3 Concentration of iodine solution = M. - - I3 is much more soluble than I2 and it is as I3 the iodine is kept in solution. Specimen Calculations In this experiment, a standard ( M) solution of iodine is generated VA x MA x nB = VB x MB x nA. in the conical flask by reacting a standard ( M) solution of potassium iodate, for each titration , with excess potassium iodide. x MA x 1 = x x 2. iodine is liberated from iodate and iodide according to the equation: - - +.

An iodine / thiosulfate titration Theory Aqueous iodine solutions normally contain potassium iodide (KI), which acts to keep the iodine in solution.

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Transcription of An iodine / thiosulfate titration - Yola

1 An iodine / thiosulfate titration Specimen Results (standardising a thiosulfate solution). 3. Rough titre = cm Theory 3. Second titre = cm Aqueous iodine solutions normally contain potassium iodide (KI), 3. Third titre = cm which acts to keep the iodine in solution. This is due to the fact that an 3. Average of accurate titres = cm equilibrium is set up as follows: 3. Volume of iodine solution used in each titration = cm - - I2 + I I3 Concentration of iodine solution = M. - - I3 is much more soluble than I2 and it is as I3 the iodine is kept in solution. Specimen Calculations In this experiment, a standard ( M) solution of iodine is generated VA x MA x nB = VB x MB x nA. in the conical flask by reacting a standard ( M) solution of potassium iodate, for each titration , with excess potassium iodide. x MA x 1 = x x 2. iodine is liberated from iodate and iodide according to the equation: - - +.

2 IO3 + 5I + 6H 3I2 + 3H2O. MA = x x 2 / ( x 1). The iodine solution, which is a golden-brown colour, can be titrated against sodium thiosulfate solution. The sodium thiosulfate solution is Concentration of sodium thiosulfate solution = M. placed in the burette and, as it is added to the conical flask, it reacts with the iodine and the colour of the solution fades. When it reaches a Specimen Results (standardising an iodine solution). pale yellow colour, a few drops of a freshly prepared starch solution 3. are added. The solution becomes blue-black, and the titration is Rough titre = cm 3. continued until it goes colourless. Second titre = cm 3. Third titre = cm 3. The titration reaction may be represented by the equation: Average of accurate titres = cm 2- - 2- 3. I2 + 2S2O3 2I + S4O6 Volume of iodine solution used in each titration = cm Concentration of sodium thiosulfate solution = M.

3 (Note that in this experiment a standard solution of iodine is used to standardise a sodium thiosulfate solution. But you also need to know Specimen Calculations that a standard solution of sodium thiosulfate can be used to VA x MA x nB = VB x MB x nA. standardise an iodine solution.). 25 x MA x 2 = x x 1. Procedure NB: Wear your safety glasses. MA = x / 50 = M. Wash the pipette, burette and conical flask with deionised water. Rinse the student questions pipette with potassium iodate solution Why is hydrated sodium thiosulfate not suitable as a primary and the burette with the sodium standard? thiosulfate a pipette It loses water of crystallisation readily, and it is not stable. filler, fill the pipette with the potassium iodate solution, and transfer the Why are iodine solutions made up using potassium contents of the pipette to the conical iodide solution?

4 Flask. iodine is sparingly soluble in water. However it reacts with iodide - 3 forming I3 ions, which are very soluble. In this way the iodine is kept Using graduated cylinders, add 20 cm in solution. of dilute sulfuric acid, followed by 10. 3. cm of M potassium iodide solution. Why does starch solution have to be freshly prepared? Using a funnel, fill the burette with It deteriorates quickly on standing. sodium thiosulfate solution, making sure that the part below the tap is filled before adjusting to zero. Which of the three pieces of titration apparatus, the pipette, the burette or the conical flask, should not be rinsed with the With the conical flask standing on a white tile, add the solution from solution it is to contain? Give a reason for your answer. the burette to the flask. Swirl the flask continuously and occasionally The conical flask should not be rinsed with the solution it is to contain.

5 Wash down the walls of the flask with deionised water using a wash If it were washed out with the solution it was to contain, then traces of bottle. the solution would remain, and there would not be a precisely known amount of the solution in the flask. Add a few drops of the starch indicator solution just prior to the end- point, when the colour of the solution fades to pale yellow. Upon addition of the indicator a blue-black colour should appear. The Why is starch indicator added close to the end-point? thiosulfate solution should now be added dropwise, with thorough To give a sharp end-point, while avoiding the formation of excess swirling. starch- iodine complex, which would be difficult to decompose. The end-point of the titration is detected by a colour change from What happens at the end-point? blue-black to colourless. Note the burette reading.

6 The colour changes from blue-black to colourless. Repeat the procedure, adding the sodium thiosulfate solution dropwise approaching the end-point until two titres agree to within 3. cm . Calculate the concentration of the sodium thiosulfate solution.


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