Calcium hydroxide and phosphoric acid react to form calcium phosphate and water. Ca(OH)2 + H3PO4 --> Ca3(PO4)2 + H2OHow many grams of Ca(OH)2 are needed to produce 1,076 grams of Ca3(PO4)2?Write your final answer in two decimal places.Use the following mass numbers:Ca - 40 g/molH - 1 g/molO - 16 g/molP - 31 g/mol
Question
Calcium hydroxide and phosphoric acid react to form calcium phosphate and water. Ca(OH)2 + H3PO4 --> Ca3(PO4)2 + H2OHow many grams of Ca(OH)2 are needed to produce 1,076 grams of Ca3(PO4)2?Write your final answer in two decimal places.Use the following mass numbers:Ca - 40 g/molH - 1 g/molO - 16 g/molP - 31 g/mol
Solution
First, we need to balance the chemical equation. The balanced equation is:
3Ca(OH)2 + 2H3PO4 --> Ca3(PO4)2 + 6H2O
Next, we calculate the molar mass of Ca3(PO4)2 and Ca(OH)2.
For Ca3(PO4)2: Ca: 40 g/mol x 3 = 120 g/mol P: 31 g/mol x 2 = 62 g/mol O: 16 g/mol x 8 = 128 g/mol Total = 310 g/mol
For Ca(OH)2: Ca: 40 g/mol O: 16 g/mol x 2 = 32 g/mol H: 1 g/mol x 2 = 2 g/mol Total = 74 g/mol
Now, we can set up a proportion to find out how many grams of Ca(OH)2 are needed to produce 1,076 grams of Ca3(PO4)2.
(3 mol Ca(OH)2 / 1 mol Ca3(PO4)2) = (x g Ca(OH)2 / 1,076 g Ca3(PO4)2)
We can cross multiply and solve for x:
x = (3 mol Ca(OH)2 / 1 mol Ca3(PO4)2) * 1,076 g Ca3(PO4)2 * (74 g Ca(OH)2 / 1 mol Ca(OH)2)
x = (3 * 1,076 * 74) / 310
x = 822.32 g
So, 822.32 grams of Ca(OH)2 are needed to produce 1,076 grams of Ca3(PO4)2.
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