Redox Titrations Bleach! help!! 1. The problem statement, all variables and given/known data An unknown metal hypochlorite salt, M(ClO)2, is subjected to analysis by iodometric titration: the salt is dissolved in dilute sulfuric acid, treated with excess aqueous KI, and then titrated with Na2S2O3 in the same manner as your experiment. The unknown metal ion (M2+) is completely unreactive in the titration. However, all of hypochlorite ion bondd to the metal reacts completely with Na2S2O3. Iodemetric titration of an acidified 0.0499 g sample of M(ClO)2 required 28.42 ml of 0.05521 mol/L Na2S2O3 to reach the equivalence point. What is the identity of metal M? 2. Relevant equations IO3^- + 5I^- + 6H^+ → 3I2 + 3H20 I2 + 2S2O3^2- → 2I^- + S4O6^2- ClO^- + 2I^- + 2H^+ → I2 + Cl^- + H20 3. The attempt at a solution So far all I have is the number of moles for Na2S2O3 = 0.001569 mol I have no idea where to go from there! please help ALSO one more question 1. The problem statement, all variables and given/known data A sample of Au(ClO)3 is contaminated with LiClO. An acidified 0.2000 g sample of this mixture is treated with excess sodium iodide and subjected to iodometric titration. The sample requires 48.24 mL of 0.08893 mol/L Na2S2O3 to reach the equivalence point. Assuming that the Au^3+ and Li^+ ions are unreactive during the titration, determine the mass percent of LiClO in the sample. 2. Relevant equations All the equations used in the first question! 3. The attempt at a solution Only moles so far. =0.004289 mol Pleae help. Thanks!