Objectives
An example of a solubility rule involves the sodium ion (Na+). Many people have observed over the years that compounds with sodium ions are very soluble in water, so there is a solubility rule that says "all sodium salts are soluble." If we combine a sodium compound with another compound and a solid is produced, we can be pretty sure that the positive ion in the product is not sodium.
Vocabulary
The reaction of barium hydroxide with sodium sulfate can be written
three different ways. First, there is the "plain reaction" which
just shows reactants and products:
Ba(OH)2 + Na2SO4
® BaSO4
+ 2NaOH
This only tells that a reaction takes place. In reality, these
will be combined as aqueous solutions in test tubes. We can
write these in terms of the ions that are involved ("aq" stands for aqueous
and "s" stands for solid):
Ba2+(aq) + 2OH–(aq)
+ 2Na+(aq) + SO42–(aq)
® BaSO4(s)
+ 2Na+(aq) + 2OH–(aq)
This overall ionic reaction tells us more than we need to know! Notice that the sodium ions and the hydroxide ions do not participate in the reaction at all. Since they are just hanging around watching, they are called spectator ions. Barium and sulfate combine to form a solid precipitate. A more useful way to show this reaction is to ignore the stuff we don't need to deal with: Ba2+(aq) + SO42–(aq) ® BaSO4(s)
This form is the net ionic equation. It includes only the positive and negative ions (cations and anions) that are relevant. For each reaction that takes place in this experiment, you will write the net ionic equation.
Procedure
Place a copy of the data table on your lab bench, under a piece of
clear plastic. Combine the ions in their correct columns and rows
by adding them two drops of each onto the sheet. Record the appearance
of any products on a second copy of this sheet. If no reaction takes
place, write "NR" in the space, and if you decide you don't need to combine
a pair, put an "X" in the space.
Anions®
|
CO32–
(Na2CO3) |
Cl–
(NaCl) |
OH–
(NaOH) |
NO3–
(NaNO3) |
PO43–
(Na3PO4) |
SO42–
(Na2SO4) |
Al3+
(AlCl3) |
. | .. | .. | .. | .. | .. |
NH4+
(NH4Cl) |
. | .. | .. | .. | .. | .. |
Ca2+
(CaCl2) |
. | . | . | . | . | . |
Cu2+
(CuSO4) |
. | . | . | . | . | . |
Na+
(NaCl) |
. | . | . | . | . | . |
Fe3+
(FeCl3) |
. | . | . | . | . | . |
Pb2+
(Pb(NO3)2) |
. | . | . | . | . | . |
Mg2+
(MgSO4) |
. | . | . | . | . | . |
K+
(KI) |
. | . | . | . | . | . |
Ag+
(AgNO3) |
. | . | . | . | . | . |
Zn2+
(ZnCl2) |
. | . | . | . | . | . |
Before you clean up, make sure you have accurately recorded all of your observations. Clean up according to your teacher's instructions.
Analysis