Solubility Exploration
1. Use the following reactants to discover what combination of ions are soluble and which are not.
2. First, make a prediction if the product with be soluble or not. Write a “Y” for soluble and an “N”
for not soluble. (The letters and numbers correspond to the rows and columns on the tray.)
Reactants:
1. HCl
2. NH4NO3
3. AgNO3
4. NaI
5. Pb(NO3)2
6. K2CrO4
HCl
A
NH4NO3
B
AgNO3
C
NaI
D
Pb(NO3)2
E
K2CrO4
F
3. Then, place 2 drops of each reactant into a well on the tray and observe.
4. Fill in the table with your observations writing a “Y” for soluble or an “N” for not soluble.
Reactants:
HCl
A
NH4NO3
B
AgNO3
C
NaI
D
Pb(NO3)2
E
K2CrO4
F
1. HCl
2. NH4NO3
3. AgNO3
4. NaI
5. Pb(NO3)2
6. K2CrO4
5. Compare your predictions with your actual observations. How many precipitates did you
correctly predict?
6. What compound(s) never participate in the formation of a precipitate?
7. What common ions are in these compounds that never form a precipitate? What does that
reveal about the solubility of these ions?
8. Did any compounds always form a precipitate? Which ones formed the most precipitates?