The manager of a small chemical plant receives an order for 2000 kg, of a 30% solution (by weight) of phosphoric acid in water (this is used as a food additive for cattle; it boosts milk production). The solution is prepared at the plant just prior to delivery by reacting solid calcium phosphate with concentrated sulfuric acid (which is 2% water by weight) to make the phosphoric acid, which is then added to water to make the final solution. The other product of the reaction, calcium sulfate, is dried and sold as a soil additive.
a. What are the molecular weights of H3PO4, H2SO4, Ca3(PO4)2 and CaSO4?
b. What is the balanced chemical equation for the reaction used to produce phosphoric acid?
c. What mass (or weight) of concentrated sulfuric acid will be required in the reaction to produce the amount of phosphoric acid solution that was ordered?