Twenty tablets of an iron food supplement whose total mass was 22.131 g were crushed and perfectly mixed. Then 2.998g of the powder was dissolved in HNO3 and the solution was heated to convert all the iron to Fe+3. By addition of NH3 it was quantitatively precipitated as Fe(OH)3 H2O which was calcined to form 0.264g of Fe203. Calculate the Fe content in each tablet.

Twenty tablets of an iron food supplement whose total mass was 22.131 g were crushed and perfectly mixed. Then 2.998g of the powder was dissolved in HNO3 and the solution was heated to convert all the iron to Fe+3. By addition of NH3 it was quantitatively precipitated as Fe(OH)3 H2O which was calcined to form 0.264g of Fe203. Calculate the Fe content in each tablet.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

Twenty tablets of an iron food
supplement whose total mass was
22.131 g were crushed and perfectly
mixed. Then 2.998g of the powder
was dissolved in HNO3 and the
solution was heated to convert all the
iron to Fe+3. By addition of NH3 it
was quantitatively precipitated as
Fe(OH)3•H20 which was calcined to
form 0.264g of Fe203. Calculate the
Fe content in each tablet.

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