Final answer:
To calculate the mass of Ba3(PO4)2, the stoichiometry of the reaction between Na3PO4.12H2O and excess BaCl2.2H2O is used.
Step-by-step explanation:
Heating the mixture in step 3 for 20 minutes promotes the reaction between BaCl₂ and Na₃PO₄.12H₂O to produce Ba₃(PO₄)₂. It provides the necessary energy to overcome the activation energy barrier and increase the reaction rate.
To calculate the mass of Ba3(PO4)2 produced, we need to first establish the stoichiometry of the reaction between Na3PO4.12H2O and excess BaCl2.2H2O. The balanced chemical equation for this reaction is: 3 BaCl2.2H2O (aq) + 2 Na3PO4.12H2O (aq) → Ba3(PO4)2 (s) + 6 NaCl(aq) + 36 H2O (l)
Heating the mixture in step 3 for 20 minutes helps to drive the reaction to completion by removing water, which shifts the equilibrium towards the product side by Le Chatelier's principle, thereby maximizing the yield of Ba3(PO4)2.