A 0.9132-gram sample of iron ore is dissolved in aqueous hydrochloric acid. It dissolves completely and in the process, all of the iron goes into solution as Fe2+ ion. The following chemical reaction is a redox reaction and it is the focus of the question:
The acid solution containing all of the Fe2+ is placed in a beaker. A solution of aqueous potassium dichromate is used to fill a burette. A redox titration is performed. A volume of exactly 28.72 mL of 0.05051M K2Cr2O7 (aq) is required to complete the redox titration. The unbalanced redox equation is:
Fe2+(aq) + K2Cr2O7(aq) (in acid) → Fe3+(aq) + Cr3+(aq)
Required:
What is the mass percent iron in the original sample of iron ore? Please show all your work.
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A 0.9132-gram sample of iron ore is dissolved in aqueous hydrochloric acid. It dissolves completely...
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