Chapter 4, Problem 4.71PAE

4.79 Phosphoric add (H₃PO₄) is important in the production of both fertilizers and detergents. It is distributed commercially as a solution with a concentration of about 14.8 M. Approximately 2.1 X l0⁹ gallons of this concentrated phosphoric acid solution is produced annually in the United States. Assuming that all of this H₃PO₄ is produced by the reaction below, what mass of the mineral fluoruapatite (Ca₅(PO₄)₃F) would be required each year?

   ${\text{Ca}}_{\text{5}}{\left({\text{PO}}_{\text{4}}\right)}_{\text{3}}\text{F }+{\text{ 5 H}}_{\text{2}}{\text{SO}}_{\text{4}}\to {\text{ 3 H}}_{\text{3}}{\text{PO}}_{\text{4}}+{\text{ 5 CaSO}}_{\text{4}}+\text{ HF}$