1. Solubility Chart (don’t copy on ¼ salmon sheet)
1. All compounds of Group 1 and ammonium soluble.
. All nitrates, acetates & chlorates soluble
. All halides soluble: except those of silver, mercury (I) & lead.
. All sulfates soluble: except calcium, barium, strontium, lead, & mercury.
. Carbonates, chromates, sulfides, hydroxides, oxides, phosphates, & silicates insoluble Except if in Rule #1

2. Solubility Guidelines
Solubility Practice:
Using the solubility guidelines determine whether each compound is soluble or insoluble
CaSO4
Ni3(PO4)2
KOH
HgCl
AgNO3
Solubility Guidelines
1. All compounds of Group 1 and ammonium soluble.
. All nitrates, acetates & chlorates soluble
. All halides soluble: except those of silver, mercury (I) & lead.
. All sulfates soluble: except calcium, barium, strontium, lead, & mercury.
. Carbonates, chromates, sulfides, hydroxides, oxides, phosphates, & silicates insoluble Except if in Rule #1

3. Warm UP 4.4- answers
Determine if the following are soluble or insoluble using the solubility table on your salmon flowchart note sheet:
CaSO4 insoluble
Ni3(PO4)2 insoluble
KOH soluble
HgCl insoluble
AgNO3 soluble

4. What does this mean… If SOLUBLE then ….. Dissolves in H2O
Ionic compound breaks apart = aqueous (aq) solution
If INSOLUBLE then ...
Does not dissolve in H2O
In reaction it forms solids (s) = it’s the precipitate -ppt

5. Aqueous (aq)
Ionic compounds that break apart in water

6. Spectator Ions Ions not directly involved in the reaction
They end up getting canceled out

7. Precipitate Insoluble portion of a reaction. Tiny little solids.
Precipitate Book Clip

8. Net ionic reactions
Only particles that actually take part in reaction - spectator ions are “thrown out” - aqueous (aq) break apart - solids (s) stay together

9. AgNO3( ) + NaCl ( )  AgCl ( ) + NaNO3 ( )
Fill in the ( ) using the solubility table
Solubility Table: ( don’t copy…already on your salmon sheet)
1. All compounds of Group 1 and ammonium soluble.
. All nitrates, acetates & chlorates soluble
. All halides soluble: except those of silver, mercury (I) & lead.
. All sulfates soluble: except calcium, barium, strontium, lead, & mercury.
. Expect for rule 1: carbonates, chromates, sulfides, hydroxides, oxides, phosphates, & silicates insoluble
*** AgNO3, NaCl & NaNO3 are all soluble; therefore we put an (aq) after them
*** AgCl is Insoluble so it remains a solid in solution

10. AgNO3(aq) + NaCl (aq)  AgCl (s) + NaNO3 (aq)
Every time you see (aq)- break ionic compound apart and include their charges
Every time you see (s)- leave it alone

11. AgNO3(aq) + NaCl (aq)  AgCl (s) + NaNO3 (aq)

12. Ag1+(aq) +NO31- (aq) +Na1+(aq)+ Cl1-(aq)AgCl(s)+Na1+(aq)+NO31-(aq)
Now.. If the same element appears on both sides of the reaction in the same form you can cancel it….

13. What is left is the NET IONIC REACTION: Ag + Cl  AgCl (s)
Ag1+(aq)+NO31- (aq) + Na1+(aq)+ Cl1-(aq)  AgCl (s) + Na1+(aq) + NO31-(aq)
What is left is the NET IONIC REACTION:
Ag + Cl  AgCl (s)

14. Net ionic book clip

15. Example #2

16. Determine what goes in the parenthesis
__K2CO3( ) + __Sr(NO3)2 ( )  __KNO3( ) + ___SrCO3( )
Solubility Table: ( don’t copy…already on your salmon sheet)
1. All compounds of Group 1 and ammonium soluble.
. All nitrates, acetates & chlorates soluble
. All halides soluble: except those of silver, mercury (I) & lead.
. All sulfates soluble: except calcium, barium, strontium, lead, & mercury.
. Expect for rule 1: carbonates, chromates, sulfides, hydroxides, oxides, phosphates, & silicates insoluble

17. Next, Break ions apart
K2CO3(aq) + Sr(NO3)2 (aq) 2KNO3(aq)+ SrCO3(s)

18. Next, cancel out ions that match
2K1+(aq) +CO32-(aq) +Sr2+(aq) + 2NO31-(aq) 2K1+(aq)+2NO31-(aq)+ SrCO3(s)

19. Finally, write the Net Ionic Reaction
2K1+(aq) +CO32-(aq) +Sr2+(aq) + 2NO31-(aq) 2K1+(aq)+2NO31-(aq)+ SrCO3(s)

20. CO32-(aq) + Sr2+(aq)  SrCO3(s)
The Net Ionic Reaction
CO32-(aq) + Sr2+(aq)  SrCO3(s)

21. Example 3

22. Determine the net ionic reaction
ZnSO4( )+Ba(C2H3O2)2 ( )  BaSO4( )+ Zn(C2H3O2)2 ( )
Solubility Table: ( don’t copy…already on your salmon sheet)
1. All compounds of Group 1 and ammonium soluble.
. All nitrates, acetates & chlorates soluble
. All halides soluble: except those of silver, mercury (I) & lead.
. All sulfates soluble: except calcium, barium, strontium, lead, & mercury.
. Expect for rule 1: carbonates, chromates, sulfides, hydroxides, oxides, phosphates, & silicates insoluble

23. Answer: Lastly, Net Ionic: Ba (aq) + SO4 (aq)  BaSO4(s)
Step 1 & 2: determine parenthesis and balance
ZnSO4(aq)+Ba(C2H3O2)2 (aq)  BaSO4(s)+ Zn(C2H3O2)2 (aq)
Step 3: break apart ions
Zn2++ SO42-+Ba2++2C2H3O21- BaSO4(s)+ Zn2++ 2C2H3O21-
Step 4: cancel out spectator ions
Lastly, Net Ionic:
Ba (aq) + SO4 (aq)  BaSO4(s)