A Reaction Between Sodium Phosphate and Calcium Chloride



I.� Purpose:


The purpose of this lab is to determine the theoretical yield and the percent yield of a reaction between

aqueous sodium phosphate and aqueous calcium chloride.


II.� Procedure:


  1. You will need 3 beakers and a stirring rod.� Make sure they are all clean and have been rinsed with distilled water before using them.
  2. Measure out 0.9-1.1 g of anhydrous CaCl2 and place it in your smallest beaker (50 ml or 100 ml).� Add 20.0 ml of distilled water and dissolve using a clean glass stirring rod.
  3. Measure out 1.9-2.1 g of Na3PO4.12 H2O (hydrated sodium phosphate) and place it in a clean 100 ml or 150 ml beaker.� Add 40.0 ml of distilled water and dissolve using a clean glass stirring rod.� Note:� The sodium phosphate solid you are using is not anhydrous.� It is a hydrate1, meaning that it has water molecules trapped inside of its crystal lattice structure.� In fact, every gram of the solid that you measure out only contains 0.43 g of Na3PO4.
  4. Add the aqueous calcium chloride to the beaker containing aqueous sodium phosphate.
  5. Write your initials on a piece of filter paper and determine its mass.� Fold the filter paper to make it fluted and use it to filter out all of the solid precipitate that you obtained in step 4.� Use your wash bottle (distilled water) to rinse out the beaker to capture as much of the product as possible.
  6. When you have collected as much of the filtrate2 as possible, place the filter paper in a drying oven overnight and determine the mass of your precipitate the next day or thereafter.


III. �Data
























1           Many ionic solids absorb moisture from the air forming hydrates.

2           The filtrate is the liquid that passes through the filter paper.