Mass of filter paper: 0.15 g

Mass of filter paper and precipitate: 4.63 g

Analysis:

1. What would be the flame color for the sodium solution and what would be the flame color for the magnesium solution?

2. Write the balanced chemical equation for this reaction.

3. Write the net ionic equation for this reaction.

4. Identify the limiting reactant. How did you determine that it was the limiting reactant?

5. Calculate the concentration of the unknown solution using the lab data.

Conclusion:

1. Calculate the percent deviation of your molar concentration of magnesium nitrate using the theoretical concentration of 0.15 mol/L.

2. Calculate the predicted mass of precipitate using the theoretical concentration of 0.15 mol/L for magnesium nitrate.

3. Calculate the percent yield of the experiment and explain why this yield is not 100%.

Chemicals: 50 mL sodium phosphate solution with a concentration of 0.200 mol/L 50 mL magnesium nitrate solution with an unknown concentration. Procedure: filter paper retort stand ring clamp funnel rlenme er flas 1. Using a volumetric pipette, measure 50.0 mL of the Mg(NO3)2(aq) solution into a 100 ml. beaker. 2. Slowly add the Na3PO4(aq) to the solution in small amounts while swirling the beaker. Continue until no more precipitate is formed upon adding small amounts of Na3PO,(aq). 3. Set up your filtration apparatus, as shown below. Record the mass of your filter paper. Be sure to record the mass of the filter paper before folding and wetting it. 4. Filter the mixture through the filter paper and record the color of the precipitate. Wash the precipitate with small amounts of deionized water. 5. Remove the filter paper with the precipitate and place it on a watch glass. 6. Leave the sample to dry (one hour in an oven at 70C or overnight on the counter)