Answer:
So the chemist can produce 418.7 grams of calcium phosphate.
Step-by-step explanation:
We can start the problem by using the balanced chemical equation for the reaction and the stoichiometry to determine the amount of calcium phosphate that can be produced.
2K3PO4 (aq) + 3CaCl2 (aq) → Ca3(PO4)2 (s) + 6KCl (aq)
From the balanced equation, we can see that for every 2 moles of potassium phosphate (K3PO4) reacted, 1 mole of calcium phosphate (Ca3(PO4)2) is produced.
We are given that the chemist has 750.0 mL of a 1.8 M solution of potassium phosphate. We can convert this information into moles by using the formula:
moles = concentration x volume
moles = 1.8 M x (750.0 mL) / 1000 mL/L = 1.35 moles
To find the number of grams of calcium phosphate that can be produced we can use the molar mass of calcium phosphate which is 310.18 g/mol
grams = moles x molar mass
grams = 1.35 x 310.18 = 418.7 grams
So the chemist can produce 418.7 grams of calcium phosphate.