Claim #1: "What is the reaction between Co(NO3)2 and Na3PO4?" Co(NO3)2 (aq) reacts with Na3PO4 (aq) to form Co3(PO4)2 (sol) and NaNO3 (aq). To express the reaction as a balanced equation, it may be written as 3Co(NO3)2 (aq) + 2Na3PO4 (aq) --> Co3(PO4)2 (sol) + 6NaNO3 (aq). Data referenced in this explanation is included in appendices labeled A1-A3 at the rear of the report. In determining the identity of the products in the observed reaction, a simple qualitative test may be carried out to confirm the identity of the precipitate. Samples of CoCl2 and K3PO3 were mixed. The result was a cloudy purple, indicating that the target precipitate was formed in this reaction (A1). NaCl mixed with KNO3 did not yield the purple precipitate, indicating that the observed solid is indeed Co3(PO4)2. It follows then that the second product must be NaNO3. The entire reaction can then be finalized by simply balancing and reducing the proportional molecular values.
Claim #2: "Are all of the reactants consumed in a reaction?" Unless a reaction progresses with proportionally exact reactant values, one reactant will be expended more quickly than the other. This claim can be verified both experimentally and conceptually. Experimentally, this result can be observed in experiment 2 (A2 and A3). Using a constant amount of Co(NO3)2 (approximately 20.0 mL) and a varying quantity of Na3PO4, four mixtures were prepared, each distinguished by the varying quantity of Na3PO4-- approximately 5.0 mL, 7.5 mL, 15.0 mL, and 20.0 mL (A2). After harvesting the supernatant of these mixtures, preparations of Na3PO4 and Co(NO3)2 were added to each. Qualitatively, supernatants from reactions with proportionally low amounts of initial Na3PO4 reacted to the addition of further Na3PO4 by producing further precipitate. These same supernatants did not react to the addition of further Co(NO3)2. The results