PROCEDURES

This experiment will be conducted on a small scale. That is, only one drop of each solution will be necessary to observe the reactions. This experiment will be a collaborative effort between pairs of students. The partners should determine the division of labor. It is recommended that each student work on a set of solutions and then share the observations from all four sets of solutions tabulated below. Each solution set consists of six solutions (labeled by name and by number).

	Set I	Set II	Set III	Set IV
Solution #1	Ba(NO3)2	Na2SO4	FeCl3	BaCl2
Solution #2	BaCl2	Al2(SO4)3	Co(NO3)2	HNO3
Solution #3	NaI	Sr(NO3)2	CoCl2	Na2CO3
Solution #4	AgNO3	CaCl2	NaOH	Al2(SO4)3
Solution #5	NaNO3	Ba(NO3)2	KOH	HCl
Solution #6	KCl	AlCl3	NaNO3	AgNO3

1. Before lab prepare the large grid sheets for Set I, II, III and IV by labeling them appropriately as shown below.

	K+ / Cl-	Na+ / NO3-	Ag+ / NO3-	Na+ / I-	Ba2+ / Cl-
Ba2+ / NO3-
Ba2+ / Cl-
Na+ / I-
Ag+ / NO3-
Na+ / NO3-

2. Notice that the headings in the above sheet identify both ions in solution. Prepare two sets of sheets for each set. Both sets of sheets may be found on pgs 4-19 to 4-23 of your lab manual.

3. Place the plastic sheet over the labeled grid sheet and carefully add one drop of each solution to the appropriate squares. When you are finished, all possible combinations of solutions in the set will have been mixed.

4. On the observation grid sheet, record your observations in the corresponding squares, carefully noting any precipitates that form and their color. You may need to use colored paper to contrast a white precipitate.

5. When your observations are complete, use a small amount of water from your wash bottle to rinse the chemicals carefully off the plastic sheet into a waste beaker.

6. Dry the plastic sheet with a paper towel and repeat the procedure for the remaining solution sets.