1. Calculate molar mass with steps of calcium phosphate Ca3(PO4)

2. Calculate number of moles present in 268g of calcium phosphate

3. Calculate the number of calcium atoms present in 0.658 mol of calcium phosphate

4. Calculate mass of calcium chloride CaCl2 required to prepare 50.0ml of solution with concentration 0.425M.

5. Determine the final concentration if 125ML of 0.425m of calcium chloride solution is diluted to a final volume of 500.0ml

The solubility product for calcium phosphate is 2.0x10^-29.

A. Calculate the molar solubility of calcium phosphate, and theconcentrations of

the calcium and phosphate ions at equilibrium.

B. Using Excel, create a spreadsheet that calculates the calciumand phosphate ion

concentrations at equilibrium following the addition of1.0x10^-8

M to

1.0x10^-7

M calcium chloride, in increments of 1.0x10^-9

M. From this data, plot

the concentration of the phosphate ion versus the concentrationof the calcium

ion at equilibrium. (You may want to multiply the concentrationsby some

constant value to make it easier to read the axes labels.) Printout and turn in

your plot with sample calculations (handwritten) of the calciumand phosphate

ion concentrations calculated for any three points between1.0x10^-8

M to

1.0x10^-7

M calcium chloride. (Make sure you plot adheres to therequired

standards on page 33 of the lab manual.)

it has 2 partsh

2.(3) Translate the following statement into a balanced chemical equation.

Three moles of calcium chloride react with two moles of sodium phosphate to produce solid calcium phosphate and six moles of sodium chloride.

3.(3) 50.0 mL of 1.0 M Ag(NO3) is added to 5.55 g of CaCl2 (MM=111.0 g). What is the concentration of nitrate ion in the final solution in moles/liter?

3a.(3) How many grams of silver chloride can be produced in this reaction?