You are going to do a precipitate reaction to determine the % purity of the CaBr2 in a very old and crusty bottle labeled “Calcium Bromide.” You carefully measure out 20.000 grams of solid CaBr2 and add water until the total volume of the solution is 750.00 mL. You recently bought a guaranteed 1.0000 M solution of high quality Na3PO4. You measure out 200.00 mL of the 1.0000 M Na3PO4 and add 100.00mL of water to make a dilution. You are going to mix 50.00 mL of your CaBr2 solution with some of your diluted Na3PO4 and filter out the precipitate. Write the molecular equation (it is always implied that you must balance equations and include s, l, g, or aq)

Write the net ionic equation (it is always implied that you must balance equations and include s, l, g, or aq)

Calculate the molarity of the CaBr2 solution you made if the CaBr2 was 100% pure. (The molar mass of CaBr2 is 199.88 g/mol)

Calculate the molarity of the diluted Na3PO4 solution you made

In order to ensure that the reaction is limited by the 50.00 mL of the impure CaBr2 solution, calculate the minimum volume, in mL, of the diluted Na3PO4 solution must you use. To be extra, super sure, that the Na3PO4 is the excess reactant, you add double the minimum volume. What volume do you add?

What is the theoretical yield of the precipitate in grams? (The molar mass of Ca3(PO4)2 is 310.18 g/mol)

Pretend the only source of error is the impurity of the CaBr2. If 0.5320 grams of precipitate are obtained, what is the percent purity of the CaBr2?