How many grams of calcium phosphate can be produced when 78.5 grams of calcium hydroxide reacts with excess phosphoric acid? unbalanced equation: h3po4 + ca(oh)2 → h2o + ca3(po4)2 show, or explain, all of your work along with the final answer.

The balanced chemical equation is written as :
2H3PO4 + 3Ca(OH)2 → 6H2O + Ca3(PO4)2.

From the above equation we can see that 3 moles of Ca(OH)2 produces 1 mole Ca3(PO4)2 .
( Don't take tension about H3PO4 as it is present in excess )

Further ,
we are given 78.5 g Ca(OH)2 .
then no of moles Ca(OH)2 given = 78.5/74 = 1.06 moles.

3 moles Ca(OH)2 produces → 1 mole Ca3(PO4)2.
=> 1 mole Ca(OH)2 produces → 1/3 mole Ca3(PO4)2.
=> 1.06 mole Ca(OH)2 produces → (1/3)×1.06 mole Ca3(PO4)2.
Hence number of moles Ca3(PO4)2 produced = (1/3)×1.06 = 0.353 moles.

Now gram molecular mass of Ca3(PO4)2 is = 310 g /mole .
hence grams of Ca3(PO4)2 produced
= 0.353× 310 = 109.43 g

Hope it helps...