16 Chemistry 30 Redox Stoichiometry 1.In a redox titration, 12.50 mL of 0.0800 mol/L K2Cr2O7(aq) was used in an acidic solution to oxidize Sn2+(aq)ions to Sn4+(aq)ions. The volume of K2Cr2O7(aq)used was just sufficient to oxidize all the Sn2+(aq)in 10 mL of the solution. Calculate the concentration of Sn2+(aq)ions in the solution. What color change indicated the endpoint of this titration? (0.30 mol/L) 2.What volume of 0.0500 mol/L KMnO4(aq)is needed to oxidize all the Br-(aq)ions in 25.0 mL of an acidic 0.200 mol/L NaBr(aq)solution. What colour change indicates the endpoint of this reaction?
3.In an experiment, 0.0200 mol/L K2Cr2O7(aq) was used in an acidic solution to oxidize Fe2+(aq)ions to Fe3+(aq)ions. The following data were obtained. Volume of Fe2+(aq)solution (mL)……………..25.0 Final buret reading (K2Cr2O7(aq)) (mL)…….…48.7 Initial buret reading (mL)…….…………………3.7 Calculate the concentration of Fe2+(aq)ions in the solution.
4.The copper (II) ions in a solution can be converted to copper metal by trickling the solution over scrap iron. The reaction produces iron (II) ions from the scrap iron. If the process produces 25.0 L of solution containing 0.00200 mol/L Fe2+(aq)ions, what mass of copper is produced? (3.18 g)