What Is the Identity of Metal M in M(ClO)2 Based on Iodometric Titration Data?

[jesse1256]

Redox Titrations Bleach! help!

Homework Statement

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?

Homework Equations

IO3^- + 5I^- + 6H^+ → 3I2 + 3H20
I2 + 2S2O3^2- → 2I^- + S4O6^2-
ClO^- + 2I^- + 2H^+ → I2 + Cl^- + H20

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

Homework Statement

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.

Homework Equations

All the equations used in the first question!

The Attempt at a Solution

Only moles so far. =0.004289 molPleae help. Thanks!

 

[Borek]

So far all I have is the number of moles for Na2S2O3 = 0.001569 mol

User stoichiometry to find out how many moles of ClO^- were present in the sample of the given mass, then use this information to find out molar mass of the metal.

 

[jesse1256]

okay that sounds easy enough, I think the main problem I have is not knowing what equation to use. Or do I set up my own stoichiometric equation adding M(ClO)2. and if I do, how do I go about doing that? Thanks!

 

[Borek]

Forget about using "equations", think about it as just another stoichiometry problem.

All titrations are nothing more but a simple stoichiometry. You know moles of this, you have to calculate corresponding moles of the other.