PRECIPITATION REACTIONS
Name:__________________________
Materials:
Set 1: 0. 1 M of each:
barium nitrate
magnesium sulfate
aluminum chloride
sodium sulfate
magnesium nitrate
aluminum sulfate
magnesium chloride
Set 2: 0.1 M of each:
potassium chloride
Barium chloride
magnesium chloride sodium sulfate
magnesium sulfate sodium hydroxide (.2M)
Set 3: 0.1 M of each:
0.2 M of each:
barium chloride
sodium chromate
silver nitrate
magnesium nitrate
aluminum sulfate
potassium chromate
Reaction wells, stirring rod per group. Wash bottle.
PROCEDURES:
1. Obtain reaction well and stirring rod; clean them. Get wash bottle and fill with
Deionized water.
2. Using Data Table 1 as a guide, mix every possible combination of chemical per set.
Rinse rod with deionized water after each stir.
3. Observe each well for signs of a precipitate. Look carefully, using dark and light
backgrounds.
4. Dispose of as directed.
CONCLUSIONS
1. Why do precipitates form?
2. What are spectator ions?
3. What is the difference between a net ionic equation and a complete ionic equation?
4. Fill out Conclusion table 2.
DATA TABLE 1
Solution A
SET 1
1 Barium Nitrate
1 Barium Nitrate
1 Barium Nitrate
1 Barium Nitrate
1 Barium Nitrate
2 Sodium sulfate
2 Sodium sulfate
2 Sodium sulfate
2 Sodium sulfate
3 Aluminum sulfate
3 Aluminum sulfate
3 Aluminum sulfate
4 Magnesium nitrate
4 Magnesium nitrate
5 Magnesium chloride
SET 2
7 Potassium chloride
7 Potassium chloride
7 Potassium chloride
7 Potassium chloride
7 Potassium chloride
8 Magnesium chloride
8 Magnesium chloride
8 Magnesium chloride
8 Magnesium chloride
9 Sodium sulfate
9 Sodium sulfate
9 Sodium sulfate
10 Sodium hydroxide
10 Sodium hydroxide
11 Barium chloride
SET 3
13 Barium chloride
13 Barium chloride
13 Barium chloride
13 Barium chloride
13 Barium chloride
14 Magnesium nitrate
14 Magnesium nitrate
14 Magnesium nitrate
14 Magnesium nitrate
15 Sodium chromate
15 Sodium chromate
15 Sodium chromate
16 Aluminum sulfate
16 Aluminum sulfate
17 Potassium chromate
Solution B
2
3
4
5
6
3
4
5
6
4
5
6
5
6
6
Sodium Sulfate
Aluminum sulfate
Magnesium nitrate
Magnesium chloride
Aluminum chloride
Aluminum sulfate
Magnesium nitrate
Magnesium chloride
Aluminum chloride
Magnesium nitrate
Magnesium chloride
Aluminum chloride
Magnesium chloride
Aluminum chloride
Aluminum chloride
8 Magnesium chloride
9 Sodium sulfate
10 Sodium hydroxide
11 Barium chloride
12 Magnesium sulfate
9 Sodium sulfate
10 Sodium hydroxide
11 Barium chloride
12 Magnesium sulfate
10 Sodium hydroxide
11 Barium chloride
12 Magnesium sulfate
11 Barium chloride
12 Magnesium sulfate
12 Magnesium sulfate
14
15
16
17
18
15
16
17
18
16
17
18
17
18
18
Magnesium nitrate
Sodium chromate
Aluminum sulfate
Potassium chromate
Silver nitrate
Sodium chromate
Aluminum sulfate
Potassium chromate
Silver nitrate
Aluminum sulfate
Potassium chromate
Silver nitrate
Potassium chromate
Silver nitrate
Silver nitrate
Results of mixing A and B
Conclusion Table 2
SET 1
Solution Pairs Yielding
Precipitates
Ba(NO3)2
SET 2
SET 3
Na2SO4
Formulas of Possible Precipitates
CIRCLE CHOICE
BaSO4
NaNO3
Reason for choice
No ppt in combination 2 and 4
Prep Room
25 ml of 0.1 M of:
Aluminum chloride
Barium nitrate
Barium chloride
Magnesium chloride
Magnesium nitrate
Magnesium sulfate
Potassium chloride
Sodium sulfate
Sample data
Solution A
SET 1
1 Barium Nitrate
1 Barium Nitrate
1 Barium Nitrate
1 Barium Nitrate
1 Barium Nitrate
2 Sodium sulfate
2 Sodium sulfate
2 Sodium sulfate
2 Sodium sulfate
3 Aluminum sulfate
3 Aluminum sulfate
3 Aluminum sulfate
4 Magnesium nitrate
4 Magnesium nitrate
5 Magnesium chloride
SET 2
7 Potassium chloride
7 Potassium chloride
7 Potassium chloride
7 Potassium chloride
7 Potassium chloride
8 Magnesium chloride
8 Magnesium chloride
8 Magnesium chloride
8 Magnesium chloride
9 Sodium sulfate
9 Sodium sulfate
9 Sodium sulfate
10 Sodium hydroxide
10 Sodium hydroxide
11 Barium chloride
SET 3
13 Barium chloride
13 Barium chloride
13 Barium chloride
13 Barium chloride
13 Barium chloride
14 Magnesium nitrate
14 Magnesium nitrate
14 Magnesium nitrate
14 Magnesium nitrate
15 Sodium chromate
15 Sodium chromate
15 Sodium chromate
16 Aluminum sulfate
16 Aluminum sulfate
17 Potassium chromate
0.48 g of the hexahydrate
0.52 g
0.48 g of the dihydrate
0.50 g of the hexahydrate
0.30 g
0.50 g of the hyptahydrate
0.15 g
0.28 g
25 ml of 0.2 M of:
Aluminum sulfate
Potassium chromate
Silver nitrate
Sodium chromate
Sodium hydroxide
Solution B
Results of mixing A and B
2
3
4
5
6
3
4
5
6
4
5
6
5
6
6
White ppt BaSO4
White ppt BaSO4
No ppt
No ppt
No ppt
No ppt
No ppt
No ppt
No ppt
No ppt
No ppt
No ppt
No ppt
No ppt
No ppt
Sodium Sulfate
Aluminum sulfate
Magnesium nitrate
Magnesium chloride
Aluminum chloride
Aluminum sulfate
Magnesium nitrate
Magnesium chloride
Aluminum chloride
Magnesium nitrate
Magnesium chloride
Aluminum chloride
Magnesium chloride
Aluminum chloride
Aluminum chloride
1.36 g
0.78 g
Standard solution
0.60 g
0.16 g
8 Magnesium chloride
9 Sodium sulfate
10 Sodium hydroxide
11 Barium chloride
12 Magnesium sulfate
9 Sodium sulfate
10 Sodium hydroxide
11 Barium chloride
12 Magnesium sulfate
10 Sodium hydroxide
11 Barium chloride
12 Magnesium sulfate
11 Barium chloride
12 Magnesium sulfate
12 Magnesium sulfate
No ppt
No ppt
No ppt
No ppt
No ppt
No ppt
White flocculent ppt Mg(OH)2
No ppt
No ppt
No ppt
White ppt BaSO4
No ppt
No ppt
White flocculent ppt Mg(OH)2
White ppt Mg(OH)2
14
15
16
17
18
15
16
17
18
16
17
18
17
18
18
No ppt
Yellow ppt BaCrO4
White ppt BaSO4
Yellow ppt BaCrO4
White ppt AgCl
No ppt
No ppt
No ppt
No ppt
No ppt
(Al2(CrO4)3 can form if cold enough; temp dependant)
No ppt
Red ppt Ag2CrO4
No ppt
(Al2(CrO4)3 can form if cold enough; temp dependant)
No ppt (transitory ppt could arise here)
Red ppt Ag2CrO4
Magnesium nitrate
Sodium chromate
Aluminum sulfate
Potassium chromate
Silver nitrate
Sodium chromate
Aluminum sulfate
Potassium chromate
Silver nitrate
Aluminum sulfate
Potassium chromate
Silver nitrate
Potassium chromate
Silver nitrate
Silver nitrate