Name: _Joshua Bryant___________
Page: 1 of 8
Lab Number: ____4________________
Grade: _____________________________
Title: The Eight Solution Problem: Exploring Reactions of Aqueous Ionic
Compounds
Purpose: The purpose of this activity is to observe a variety of double replacement
reactions, identify their solubilities and write net ionic equations for all reactions
producing precipitates. I will also use my observations and data-taking skills to
identify 8 unknown solutions.
Procedure:
Part 1
1. I obtained my 96 well plate and oriented it on the table so that the long edge
was at the top.
2. I placed 2 drops of each horizontal and vertical reactant listed on data table 1
into each well. I began by placing 2 drops of iron (II) chloride in each of 11
wells across the first row. As I began to add the second solution, I made sure
not to touch the pipette to the well or its contents to prevent contamination
of the pipette.
3. To the first well, I added two drops of lead (III) nitrate. I used a toothpick to
swirl the solutions together until they were mixed. I then recorded my
observations.
4. I continued in the same fashion by observing all of the combinations listed on
my table.
5. After I finished all 66 reactions, I carefully rinsed the micro plates with water
and used cotton swabs to clean any of the wells that had remaining
precipitate.
Part 2
1. I then obtained the eight unknown solutions as directed by my instructor.
The eight unknown solutions came from the original 12 solutions that were
already tested. I then wrote the numbers of the eight solutions horizontally
on a new data table. I then reversed the order of the numbers as I wrote them
down the vertical column to mimic the set up of the chemical reactions in
part 1. I then mixed two drops of each solution in a well just as I had in part 1.
I then stirred them with a toothpick and recorded my observations in data
table 2.
2. I then analyzed the results of my unknown mixings by comparing them with
the results recorded in part 1.
Name: _Joshua Bryant___________
Page: 2 of 8
Lab Number: ____4________________
Grade: _____________________________
Data Analysis:
Table 1
Pb(NO3)2 HCl Na3PO4 KI CuSO4 H2SO4 NaOH AgNO3 CaCl2 HNO3 Na2CO3
FeCl3
1
12
22
31
39
46
52
57
61
64
66
Na2CO3
2
13
23
32
40
47
53
58
62
65
HNO3
3
14
24
33
41
48
54
59
63
CaCl2
4
15
25
34
42
49
55
60
AgNO3
5
16
26
35
43
50
56
NaOH
6
17
27
36
44
51
H2SO4
7
18
28
37
45
CuSO4
8
19
29
38
KI
9
20
30
Na3PO4
10
21
HCl
11
The numbers in each cell are labeling to identify the reactions in the next table.
Reaction #
1
2
3
4
5
6
7
8
Reactions/Observations
Pb(NO3)2(aq) + FeCl2(aq)  PbCl2(s) + Fe(NO3)2(aq)
Pb2+(aq) + 2Cl-(aq)  PbCl2(s)
Observations: Solid white precipitate formed along with a yellow liquid.
Pb(NO3)2(aq) + Na2CO3(aq)  PbCO3(s) + 2NaNO3(aq)
Pb2-(aq) + CO32-(aq)  PbCO3(s)
Observations: Formation of a milky white liquid
Pb(NO3)2(aq) + HNO3(aq)  No reaction
Observations: No change occurred in the well.
Pb(NO3)2(aq) + CaCl2(aq)  PbCl2(s) + Ca(NO3)2(aq)
Pb2-(aq) + 2Cl-(aq)  PbCl2(s)
Observations: No change in the well was observed.
Pb(NO3)2(aq) + AgNO3(aq)  No reaction
Observations: No change in the well was observed.
Pb(NO3)2(aq) + 2NaOH(aq)  Pb(OH)2(s) + 2NaNO3(aq)
Pb2-(aq) + 2OH-(aq)  Pb(OH)2(s)
Observations: A white precipitate formed as solid particles.
Pb(NO3)2(aq) + H2SO4(aq)  PbSO4(s) + 2HNO3(aq)
Pb2-(aq) + SO42-(aq)  PbSO4(s)
Observations: A white precipitate formed that seemed like a fine white
powder in suspension in the solution.
Pb(NO3)2(aq) + CuSO4(aq)  PbSO4(s) + Cu(NO3)2(aq)
Pb2-(aq) + SO42-(aq)  PbSO4(s)
Observations: A white precipitate formed at the bottom of the solution.
Name: _Joshua Bryant___________
Page: 3 of 8
Lab Number: ____4________________
Grade: _____________________________
9
10
11
12
13
14
15
16
17
18
19
20
21
22
23
Pb(NO3)2(aq) + 2KI(aq)  PbI2(s) + 2KNO3(aq)
Pb2-(aq) + 2I-(aq)  PbI2(s)
Observations: A bright yellow precipitate formed.
3Pb(NO3)2(aq) + 2Na3PO4(aq)  Pb3(PO4)2(s) + 6NaNO3(aq)
3Pb2-(aq) + 2PO43-(aq)  Pb3(PO4)2(s)
Observations: A white precipitate formed in what appeared to be cloudlike structures suspended in the solution.
Pb(NO3)2(aq) + 2HCl(aq)  PbCl2(s) + 2HNO3(aq)
Pb2-(aq) + 2Cl-(aq)  PbCl2(aq)
Observations: A white precipitate with the appearance of suspended
particles formed.
HCl(aq) + FeCl2(aq)  No reaction
Observations: No change was observed in the well.
2HCl(aq) + Na2CO3(aq)  2NaCl(aq) + H2O(l) + CO2(g)
2H+(aq) + CO32-(aq)  H2O(l) + CO2(g)
Observations: The solution created a small amount of bubbles.
HCl(aq) + HNO3(aq)  no reaction
Observations: No change was observed in the well.
HCl(aq) + CaCl2(aq)  no reaction
Observations: No change was observed in the well.
HCl(aq) + AgNO3(aq)  AgCl(s) + HNO3(aq)
Ag-(aq) + Cl+(aq)  AgCl(s)
Observations: A milky white precipitate was formed in the clear solution.
HCl(aq) + NaOH(aq)  NaCl(aq) + H2O(l)
H+(aq) + OH-(aq)  H2O(l)
Observations: No change was observed in the well.
HCl(aq) + H2SO4(aq)  No Reaction
Observations: No change was observed in the well.
HCl(aq) + CuSO4(aq)  CuCl2(aq) + H2SO4(aq)
No Net onic Equation.
Observations: No change was observed in the well.
HCl(aq) + KI(aq)  HI(aq) + KCl(aq)
No net ionic equation.
Observations: No change was observed in the well.
3HCl(aq) + Na3PO4(aq)  3NaCl(aq) + H3PO4(aq)
No net ionic equation.
Observations: No change was observed in the well.
2Na3PO4(aq) + 3FeCl2(aq)  6NaCl(aq) + Fe3(PO4)2(s)
3Fe2+(aq) + 2PO43-(aq)  Fe3(PO4)2(s)
Observations: An off-white/yellow precipitate was formed.
Na3PO4(aq) + Na2CO3(aq)  No reaction
Observations: No change was observed in the well.
Name: _Joshua Bryant___________
Page: 4 of 8
Lab Number: ____4________________
Grade: _____________________________
24
25
26
27
28
29
30
31
32
33
34
35
36
37
Na3PO4(aq) + 3HNO3(aq)  3NaNO3(aq) + H3PO4(aq)
No net ionic equation
Observations: No change was observed in the well.
2Na3PO4(aq) + 3CaCl2(aq)  6NaCl(aq) + Ca3(PO4)2(s)
3Ca2+(aq) + 2PO43-(aq)  Ca3(PO4)2(s)
Observations: A white precipitate formed.
Na3PO4(aq) + 3AgNO3(aq)  3NaNO3(aq) + Ag3PO4(s)
3Ag1+(aq) + PO43-(aq)  Ag3PO4(s)
Observations: A light yellow precipitate forms.
Na3PO4(aq) + NaOH(aq)  No Reaction
Observations: No change was observed in the well.
2Na3PO4(aq) + 3H2SO4(aq)  3Na2SO4(aq) + 2H3PO4(aq)
No net ionic equation
Observations: No change was observed in the well.
2Na3PO4(aq) + 3CuSO4(aq)  3Na2SO4(aq) + Cu3(PO4)2(s)
3Cu2+(aq) + 2PO43-(aq)  Cu3(PO4)2(s)
Observations: A light, baby blue precipitate was formed.
Na3PO4(aq) + 3KI(aq)  K3PO4(aq) + 3NaI(aq)
No net ionic equation
Observations: No change was observed in the well.
2KI(aq) + FeCl2(aq)  2KCl(aq) + FeI2(s)
Fe2+(aq) + 2I-(aq)  FeI2(s)
Observations: An orange precipitate was formed.
2KI(aq) + Na2CO3(aq)  K2CO3(aq) + 2NaI(aq)
No net ionic equation
Observations: No change was observed in the well.
KI(aq) + HNO3(aq)  KNO3(aq) + HI(aq)
No net ionic equation
Observations: A red/yellow liquid was.
2KI(aq) + CaCl2(aq)  2KCl(aq) + CaI2(aq)
No net ionic equation
Observations: No change was observed in the well.
KI(aq) + AgNO3(aq)  KNO3(aq) + AgI(s)
Ag+(aq) + I-(aq)  AgI(s)
Observations: A light yellow precipitate was formed.
KI(aq) + NaOH(aq)  KOH(aq) + NaI(aq)
No net ionic equation
Observations: No change was observed in the well.
2KI(aq) + H2SO4(aq)  2HI(aq) + K2SO4(aq)
No net ionic equation
Observations: No change was observed in the well.
Name: _Joshua Bryant___________
Page: 5 of 8
Lab Number: ____4________________
Grade: _____________________________
38
39
40
41
42
43
44
45
46
47
48
49
50
51
2KI(aq) + CuSO4(aq)  K2SO4(aq) + CuI2(s)
Cu2+(aq) + 2I-(aq)  CuI2(s)
Observations: An orange precipitate was formed.
CuSO4(aq) + FeCl2(aq)  FeSO4(aq) + CuCl2(aq)
No net ionic equation
Observations: Nothing was observed in the well.
CuSO4(aq) + Na2CO3(aq)  CuCO3(s) + Na2SO4(aq)
Cu2+(aq) + CO32-(aq)  CuCO3(s)
Observations: A blue precipitate was formed.
CuSO4(aq) + 2HNO3(aq)  Cu(NO3)2(aq) + H2SO4(aq)
No net ionic equation
Observations: No change was observed in the well.
CuSO4(aq) + CaCl2(aq)  CuCl2(aq) + CaSO4(aq)
No net ionic equation
Observations: No change was observed in the well.
CuSO4(aq) + 2AgNO3(aq)  Cu(NO3)2(aq) + Ag2SO4(aq)
No net ionic equation
Observations: No change was observed in the well.
CuSO4(aq) + 2NaOH(aq)  Na2SO4(aq) + Cu(OH)2(s)
Cu2+(aq) + 2OH-(aq)  Cu(OH)2(s)
Observations: A blue precipitate was formed.
CuSO4(aq) + H2SO4(aq)  No reaction
Observations: No change was observed.
H2SO4(aq) + FeCl2(aq)  2HCl(aq) + FeSO4(aq)
No net ionic equation
Observations: No change was observed.
H2SO4(aq) + Na2CO3(aq)  H2O(l) + CO2(g) + Na2SO4(aq)
2H+(aq) + CO32-(aq)  H2O(l) + CO2(g)
Observations: No change was observed in the well.
H2SO4(aq) + HNO3(aq)  No reaction
Observations: No change was observed in the well.
H2SO4(aq) + CaCl2(aq)  2HCl(aq) + CaSO4(s)
Ca2+(aq) + SO42-(aq)  CaSO4(s)
Observations: No change was observed in the well.
H2SO4(aq) + 2AgNO3(aq)  2HNO3(aq) + Ag2SO4(aq)
No net ionic equation
Observations: No change was observe in the well.
H2SO4(aq) + 2NaOH(aq)  Na2SO4(aq) + 2H2O(l)
2H-(aq) + 2OH-(aq)  2H2O(l)
Observations: No change was observed in the well.
Name: _Joshua Bryant___________
Page: 6 of 8
Lab Number: ____4________________
Grade: _____________________________
52
53
54
55
56
57
58
59
60
61
62
63
64
65
66
2NaOH(aq) + FeCl2(aq)  Fe(OH)2(s) + 2NaCl(aq)
Fe2+(aq) + 2OH-(aq)  Fe(OH)2(s)
Observations: A rust colored, solid precipitate was formed.
NaOH(aq) + Na2CO3(aq)  No reaction
Observations: No change was observed in the well.
NaOH(aq) + HNO3(aq)  NaNO3(aq) + H2O(l)
H-(aq) + OH-(aq)  H2O(l)
Observations: No change was observed in the well.
2NaOH(aq) + CaCl2(aq)  2NaCl(aq) + Ca(OH)2(s)
Ca2+(aq) + 2OH-(aq)  Ca(OH)2(s)
Observations: A white precipitate as fine, white particles was formed.
NaOH(aq) + AgNO3(aq)  AgOH(s) + NaNO3(aq)
Ag+(aq) + OH-(aq)  AgOH(s)
Observations: A green/brown precipitate was formed.
2AgNO3(aq) + FeCl2(aq)  2AgCL(s) + Fe(NO3)2(aq)
2Ag+(aq) + 2Cl-(aq)  2AgCl(s)
Observations: A white precipitate was formed in a yellow liquid.
2AgNO3(aq) + Na2CO3(aq)  Ag2CO3(s) + 2NaNO3(aq)
2Ag+(aq) + CO32-(aq)  Ag2CO3(s)
Observations: A solid white precipitate was formed.
AgNO3(aq) + HNO3(aq)  No reaction
Observations: No change was observed in the well.
2AgNO3(aq) + CaCl2(aq)  2AgCl(s) + Ca(NO3)2(aq)
2Ag-(aq) + 2Cl-(aq)  2AgCl(s)
Observations: A clumpy white precipitate was formed.
CaCl2(aq) + FeCl2(aq)  No Reaction
Observations: No change was observed in the well.
CaCl2(aq) + Na2CO3(aq)  2NaCl(aq) + CaCO3(s)
Ca2+(aq) + CO32-(aq)  CaCO3(s)
Observations: A white precipitate was formed.
CaCl2(aq) + 2HNO3(aq)  2HCl(aq) + Ca(NO3)2(aq)
No net ionic equation
Observations: No change was observed in the well.
2HNO3(aq) + FeCl2(aq)  2HCl(aq) + Fe(NO3)2(aq)
No net ionic equation
Observations: No change was observed in the well.
2HNO3(aq) + Na2CO3(aq)  H2O(l) + CO2(g) + 2NaNO3(aq)
2H+(aq) + CO32-(aq)  H2O(l) + CO2(g)
Observations: Heavy bubbling was observed in a clear liquid.
Na2CO3(aq) + FeCl2(aq)  2NaCl(aq) + FeCO3(s)
Fe2+(aq) + CO32-(aq)  FeCO3(s)
Observations: An orange precipitate was formed.
Name: _Joshua Bryant___________
Page: 7 of 8
Lab Number: ____4________________
Grade: _____________________________
Unknown #
1
2
3
4
5
6
7
8
1
8
14
19
23
26
28
7
2
9
15
20
24
27
6
3
10
16
21
25
5
4
11
17
22
4
5
12
18
3
6
13
2
7
The numbers along the first column and the first row are the identification numbers
of the unknown solution. The numbers in the grid are identification numbers of the
equations just as in the above table.
Table 2
Reaction #
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
19
20
21
22
23
24
25
Observations/Comparisons
Observations: A milky white precipitate was formed in the clear solution.
Observations: No change in the well was observed.
Observations: A white precipitate was formed in a yellow liquid.
Observations: No change was observed in the well.
Observations: A solid white precipitate was formed.
Observations: A light yellow precipitate was formed.
Observations: A clumpy white precipitate was formed.
Observations: No change was observed in the well.
Observations: No change in the well was observed.
Observations: No change was observed in the well.
Observations: No change was observed in the well.
Observations: A white precipitate was formed.
Observations: No change was observed in the well.
Observations: No change was observed in the well.
Observations: A bright yellow precipitate formed.
Observations: An orange precipitate was formed.
Observations: An orange precipitate was formed.
Observations: No change was observed in the well.
Observations: The solution created a small amount of bubbles.
Observations: Formation of a milky white liquid
Observations: An orange precipitate was formed.
Observations: A blue precipitate was formed.
Observations: No change was observed in the well.
Observations: A white precipitate formed at the bottom of the solution.
Observations: Nothing was observed in the well.
Name: _Joshua Bryant___________
Page: 8 of 8
Lab Number: ____4________________
Grade: _____________________________
26
27
28
Observations: No change was observed in the well.
Observations: Solid white precipitate formed along with a yellow liquid.
Observations: A white precipitate with the appearance of suspended
particles formed.
Solution Identification:
1. AgNO3
2. CaCl2
3. KI
4. Na2CO3
5. CuSO4
6. FeCl3
7. Pb(NO3)2
8. HCl
Conclusion:
The product of a double displacement reaction can vary widely, depending
on the reactants. Some double displacement reactions produce gas, such as the
reaction between hydrochloric acid and sodium carbonate to produce sodium
chloride and carbonic acid with the aqueous sodium chloride dissolving in the water
and forcing the carbon dioxide out of the solution causing the final products to be
aqueous sodium chloride, water, and carbon dioxide. There are also some double
displacement reactions that produce no precipitate but change color in the liquid.
The reaction still takes place; it is just that the products formed are all aqueous
solutions where each has different optical properties. Some double displacement
reactions are also neutralization reactions such as the reaction between
hydrochloric acid and sodium hydroxide. There are also some double displacement
reactions that have no net equation because both of the products are aqueous
solutions leaving the products to just form a solution of different ions that are
forming and disassociating simultaneously.