1. Solubility Guidelines and Predicting precipitates
Chem 12
Mrs. Kay

2. Solubility Guidelines
Summary of ionic-compounds interactions with water
The table breaks down the ionic compound into cation and anions and describes its level of solubility.
If it is soluble it will completely break up into its ions.
If it is insoluble it will not break up into ions, but remain the same compound.

3. NO– SO4 2– OH– Cl– Br– I– S 2– C2H3O 2– CO3 2– PO4 3– Na+ K+ NH4+ Ag+ss - I
Al3+ d
Ba2+
Ca2+
Co2+
Cu2+
Hg2+
Mg2+
Pb2+
Sr2+
Zn2+
S= soluble ss = slightly soluble I = insoluble d = decomposes in water

4. Practice:
Using your solubility tables from your data booklets, tell me if the following compounds will break up in water, or remain the same.
PbCl2
ZnO
AgCH3COO
KNO3
CaCO3
AlPO4
AgCl
ZnCO3
FeSO4
MgCl2
CaS

5. Mix two aqueous ionic compounds…
Two possibilities:
Compounds will remain in solution without reacting
Compounds will react with one another, producing new products.
HOW CAN YOU TELL WHAT WILL HAPPEN?

6. Double Displacement Reactions
WX + YZ  WZ + YX
You know its happened if:
Forms a precipitate (ions makes an insoluble solid)
Forms a gas (ions make a gas product)
Forms water (H+ and OH- combine)

7. In other words…
If all the reactants are soluble, even after a replacement has occurred and you have not formed a precipitate, a gas, or water, then no reaction has occurred.
It would look like:
NH4Cl + ZnSO4  NR
NH4+ + Cl- + Zn+2 + SO4-2  when combined it only makes soluble compounds, so no reaction

8. Ag+(aq) + Cl-(aq)  AgCl(s)
Balanced Equation:
AgNO3(aq) + NaCl(aq)  AgCl(s)+ NaNO3(aq)
Ionic Equation: (soluble compounds break up into ions, otherwise stay the same)
Ag+(aq) + NO3-(aq) + Na+(aq) + Cl-(aq)  AgCl(s) + Na+(aq) + NO3-(aq)
Net Ionic Equation: cancel out spectator ions (ones that are the same on both sides)
Ag+(aq) + Cl-(aq)  AgCl(s)