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 1,788 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

To solve this problem, we first need to determine the molar mass of each compound involved in the reaction.

1. Calculate the molar mass of Ca3(PO4)2 (calcium phosphate):

   • 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 The molar mass of Ca3(PO4)2 is 120 + 62 + 128 = 310 g/mol.

2. Calculate the molar mass of Ca(OH)2 (calcium hydroxide):

   • Ca: 40 g/mol
   • O: 16 g/mol x 2 = 32 g/mol
   • H: 1 g/mol x 2 = 2 g/mol The molar mass of Ca(OH)2 is 40 + 32 + 2 = 74 g/mol.

3. Determine the number of moles of Ca3(PO4)2 produced:

   • We know that 1,788 g of Ca3(PO4)2 were produced. To find the number of moles, we divide the mass by the molar mass: 1,788 g ÷ 310 g/mol = 5.77 moles of Ca3(PO4)2.

4. Determine the number of moles of Ca(OH)2 needed:

   • From the balanced chemical equation, we know that 1 mole of Ca(OH)2 produces 1 mole of Ca3(PO4)2. Therefore, to produce 5.77 moles of Ca3(PO4)2, we need 5.77 moles of Ca(OH)2.

5. Determine the mass of Ca(OH)2 needed:

   • We multiply the number of moles by the molar mass: 5.77 moles x 74 g/mol = 427.18 g of Ca(OH)2.

So, to produce 1,788 grams of Ca3(PO4)2, we need approximately 427.18 grams of Ca(OH)2.