Calcium hydroxide and phosphoric acid react to form calcium phosphate and water. Ca(OH)2 + H3PO4 --> Ca3(PO4)2 + H2OHow many grams of H3PO4 are needed to produce 1,993 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 H3PO4 are needed to produce 1,993 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 calculate the molar mass of each compound involved in the reaction.
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Molar mass of Ca3(PO4)2: = 3*(40 g/mol for Ca) + 2*(31 g/mol for P) + 8*(16 g/mol for O) = 120 g/mol + 62 g/mol + 128 g/mol = 310 g/mol
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Molar mass of H3PO4: = 3*(1 g/mol for H) + 31 g/mol for P + 4*(16 g/mol for O) = 3 g/mol + 31 g/mol + 64 g/mol = 98 g/mol
Next, we need to balance the chemical equation. The balanced equation is:
3Ca(OH)2 + 2H3PO4 --> Ca3(PO4)2 + 6H2O
From the balanced equation, we can see that 2 moles of H3PO4 produce 1 mole of Ca3(PO4)2.
Now, we can calculate the amount of H3PO4 needed to produce 1,993 g of Ca3(PO4)2.
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Convert the mass of Ca3(PO4)2 to moles: = 1,993 g / 310 g/mol = 6.43 moles
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Calculate the moles of H3PO4 needed: = 6.43 moles * 2 (from the balanced equation) = 12.86 moles
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Convert the moles of H3PO4 to grams: = 12.86 moles * 98 g/mol = 1,260.28 g
So, 1,260.28 grams of H3PO4 are needed to produce 1,993 grams of Ca3(PO4)2.
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