Chemistry

posted by .

How many grams of calcium phosphate (precipitate) could be produced by combining 12.096g of calcium nitrate dissolved in water with 16.498g of rubidium phosphate dissolved in water? Report your answer to 3 decimal places.

  • Chemistry -

    This is a limiting reagent problem. I know that because amounts for BOTH reactants are given.

    Write and balance the equation.

    Convert Ca(NO3)2 to mols. mols = grams/m
    molar mass.
    Do the same for Rb3PO4.

    Using the coefficients in the balanced equation,convert mols of each of the reactants to mols of Ca3(PO4)2. It is likely you will get two values; one of them must be wrong. The correct answer in limiting reagent problems is ALWAYS the smaller one and the reagent responsible for that smaller number is the limiting reagent.

    Now convert the smaller number to grams. g = mols x molar mass.

  • Chemistry -

    Can you explain how to convert mols of each of the reactants to mols of Ca3(PO4)2 more please?

  • Chemistry -

    3Ca(NO3)2 + 2Rb3PO4 ==> Ca3(PO4)2 + 6RbNO3
    mols Ca(NO3) = about 12.096/164.09 = about 0.0737.

    It's a factor. Notice how the units you don't want cancel and the unit you want to convert to remains.
    0.0737 mols Ca(NO3)2 x [1 mol Ca3(PO4)3/3 mols Ca(NO3)2] = 0.0737 x (1/3) = ? mols Ca3(PO4)2
    Using factor like this you can convert anything to anything. The factors are
    [what you have x (mols what you want/mols what you have)] where mols of each are the coefficients in the balanced equation.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemistry

    How many grams of calcium phosphate (precipitate) could be produced by combining 12.443g of calcium nitrate dissolved in water with 16.083g of rubidium phosphate dissolved in water?
  2. Chemistry

    The acid-base reaction between phosphoric acid, H3PO4, and calcium hydroxide, Ca(OH)2, yields water and calcium phosphate. For each mole of calcium phosphate produced by this reaction, how many moles of water are also produced?
  3. chemistry

    A precipitate of calcium phosphate is formed when aqueous solutions of sodium phosphate and excess calcium chloride are mixed. If 100.0 mL of 1.5 M sodium phosphate solution is the limiting reactant, how many grams of calcium phosphate …
  4. Chemistry

    Calculate the mass of calcium phosphate that forms when 5.50 x 10 -2 mol of solid calcium chlorate is dissolved in 600.0 mL of 1.00 x 10 -2 M lithium phosphate solution.
  5. chemistry

    50 mL of a 2.50 M solution of ammonium phosphate is added to 100mL of a 1.50 M solution of calcium nitrate. At the end of the reaction 11.2 grams of precipitate produced. What is the percent yield
  6. Chemistry

    Calcium can also be precipitated out of the solution by adding sodium phosphate (Na3PO4) to form solid calcium phosphate. A.) write a net ionic equation for this process B.)calculate the mass of this precipitate you would generate …
  7. chemistry

    When calcium chloride and ammonium phosphate are mixed, an insoluble precipitate of calcium phosphate forms and falls out of solution. After careful analysis of the purified precipitate, 8.16 * 10^25 atoms of calcium are found in the …
  8. chemistry

    a 36 grams sample of calcium hydroxide is allowed to react with 40.5 grams of phosphoric acid according to the following reaction. how many grams of calcium phosphate are produced?
  9. chemistry

    Stoichiometrics: a 36 grams sample of calcium hydroxide is allowed to react with 40.5 grams of phosphoric acid according to the following reaction. 3Ca(OH)2 + 2H3PO4 = Ca3(PO4)2 + 6H2O how many grams of calcium phosphate are produced?
  10. Analytical chemistry

    0.6140 grams of sodium phosphate (Na3PO4) was dissolved in 2 L of water to make a stock solution. 34 mL of this solution is then diluted to 100mL volumetrically to prepare the final solution. Calculate the molarity of phosphate ions …

More Similar Questions