Dichromate reacts with aqueous iron (II) ion in acidic solution according to the balanced equation:        Cr2O72-(aq)  +  6 Fe2+ (aq) + 14 H+ (aq)    2 Cr3+(aq)  +  6 Fe3+ (aq)   + 7 H2O (l) A volume of 18.72 mL of 15.00 M K2Cr2O7 solution was required to titrate a sample of FeSO4 to the endpoint.  What was the mass of iron in the sample? How can the balanced net ionic equation help in your determination? Why arent K+ ans SO2-4 found in the balanced equation?  Solve and list the steps to the problem.

Question
  1. Dichromate reacts with aqueous iron (II) ion in acidic solution according to the balanced equation:

       Cr2O72-(aq)  +  6 Fe2+ (aq) + 14 H+ (aq)    2 Cr3+(aq)  +  6 Fe3+ (aq)   + 7 H2O (l)

A volume of 18.72 mL of 15.00 M K2Cr2O7 solution was required to titrate a sample of FeSO4 to the endpoint.  What was the mass of iron in the sample?

How can the balanced net ionic equation help in your determination? Why arent K+ ans SO2-found in the balanced equation? 

Solve and list the steps to the problem. 

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