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

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

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

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

Aqueous (aq) Ionic compounds that break apart in water

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

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

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

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

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

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

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….

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)

Net ionic book clip

Example #2

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

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

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

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

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

Example 3

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

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)