Phosphoric acid (H3PO4) is important in the production of both fertilizers and detergents. It is produced in the following process. Cas (PO4)3 F +5 H₂SO4→ 3 H₂PO4 +5 CaSO4 + HF It is distributed commercially as a solution with a concentration of about 14.8 M. Approximately 1.81 x 10 gallons of this concentrated phosphoric acid solution are produced annually in this country alone. Assuming that all of this H3PO4 is produced in the reaction above, what mass (in g) of the mineral fluoroapatite. Cas (PO4)3F, would be required each year? g

Phosphoric acid (H3PO4) is important in the production of both fertilizers and detergents. It is produced in the following process. Cas (PO4)3 F +5 H₂SO4→ 3 H₂PO4 +5 CaSO4 + HF It is distributed commercially as a solution with a concentration of about 14.8 M. Approximately 1.81 x 10 gallons of this concentrated phosphoric acid solution are produced annually in this country alone. Assuming that all of this H3PO4 is produced in the reaction above, what mass (in g) of the mineral fluoroapatite. Cas (PO4)3F, would be required each year? g

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter4: Stoichiometry

Section: Chapter Questions

Problem 4.102PAE

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