# Mass of KxFe(C2O4)y · zH2O : 5.60 gMass of sample : 0.155 gMass of FeCl3 used in preparation : 1.60 gMolarity of standard NaOH used : 0.100V1, volume of standard NaOH required for first equivalence point : 9.000 mLV2, volume of standard NaOH required for second equivalence point : 15.90 mLCalculate the percent of iron in the sample :

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Mass of KxFe(C2O4)y · zH2O : 5.60 g

Mass of sample : 0.155 g

Mass of FeCl3 used in preparation : 1.60 g

Molarity of standard NaOH used : 0.100

V1, volume of standard NaOH required for first equivalence point : 9.000 mL

V2, volume of standard NaOH required for second equivalence point : 15.90 mL

Calculate the percent of iron in the sample :

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Step 1

The given data indicates that titration is being carried out. The aqueous solution of the given compound is first passed through a cation exchange resin which results in the exchange of K+ ions with H+ ions. The H+ ions reacts with NaOH. The first equivalence point indicates the point where all the H+ ions are neutralised. After all acid is removed, further addition of NaOH results in the reaction with the othe part of the given compound. Thus, the volume of NaOH used for this reaction is the volume of NaOH for second equivalent point - Volume of NaOH for first equivalence point.

Thus, the given compound first dissociates as:

Step 2

After passing through cation exchange resin, further addition of NaOH results in the reaction:

Step 3

Thus, according to the stoichiometry of the above reaction, moles of Fe in ...

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