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A mass of 6.08 grams of iron(II) sulfate crystals (FeSO4.xH2O) was dissolved in deionised water which had been acidified with dilute sulfuric acid. The resulting solution was made up to 250cm3 in a volumetric flask. 25cm3 of this solution required 21.8cm3 of 0.02 M KMnO4 solution for complete reaction. (a) Outline the procedure for transferring the crystals to the volumetric flask. (b) Why was it necessary to acidify the deionised water used to dissolve the crystals? (c) In carrying out the titration, it was also necessary to add sulfuric acid to the conical flask. What is the reason for this? What would be observed if sulfuric acid were not added to the conical flask? (d) Calculate the value of x in the above formul
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