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Warm UP 5.7. Determine if the following are soluble or insoluble using the solubility table: CaSO 4 Ni 3 (PO 4 ) 2 KOH HgCl MgCrO 4 . insoluble. Solubility Table: ( don’t copy…already on your salmon sheet) 1 . All compounds of Group 1 and ammonium soluble. - PowerPoint PPT Presentation
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Warm UP 5.7
Determine if the following are soluble or insoluble using the solubility table:
1. CaSO4
2. Ni3(PO4)2
3. KOH4. HgCl 5. MgCrO4
Solubility Table: ( don’t copy…already on your salmon sheet)1. All compounds of Group 1 and ammonium soluble. 2. All nitrates, acetates & chlorates soluble3. All halides soluble: except those of silver, mercury (I) & lead.4. All sulfates soluble: except calcium, barium, strontium, lead, & mercury.5. Except for rule 1: carbonates, chromates, sulfides, hydroxides, oxides, phosphates, & silicates insoluble
insoluble
insolublesoluble
insoluble
insoluble
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 BREAK APART in water
Draw this image
Spectator Ions
Ions that: – are not directly involved in rxn –end up getting canceled out
Precipitate (s)
• Insoluble portion of a rxn• Tiny little solids
Precipitate Book Clip
Net ionic reactions
Only particles that actually take part in rxn• aqueous (aq)= break apart ions• solids (s) stay together• spectator ions are crossed out
not part of the rxn
Example #1
AgNO3(?) + NaCl (?) AgCl (?) + NaNO3 (?)
Determine what goes in the parenthesis
AgNO3( ) + NaCl( ) AgCl (?) + NaNO3( )
AgNO3is soluble in the solubility table
its aqueous
Solubility Table: ( don’t copy…already on your salmon sheet)
1. All compounds of Group 1 and ammonium soluble. 2. All nitrates, acetates & chlorates soluble3. All halides soluble: except those of silver, mercury (I) & lead.4. All sulfates soluble: except calcium, barium, strontium, lead, & mercury.5. Expect for rule 1: carbonates, chromates, sulfides, hydroxides, oxides, phosphates, & silicates insoluble
***** this is the same for NaCl & NaNO3
aq aq aq
AgNO3(aq) + NaCl (aq) AgCl ( ) + NaNO3 (aq)
AgCl is INsoluble in the solubility table
is precipitate (s)
Solubility Table: ( don’t copy…already on your salmon sheet)
1. All compounds of Group 1 and ammonium soluble. 2. All nitrates, acetates & chlorates soluble3. All halides soluble: except those of silver, mercury (I) & lead.4. All sulfates soluble: except calcium, barium, strontium, lead, & mercury.5. Expect for rule 1: carbonates, chromates, sulfides, hydroxides, oxides, phosphates, & silicates insoluble
S
Every time you see (aq)- break ionic compound apart
Ag1+( )+NO31-( )+Na1+( )+Cl1-( )AgCl( )+Na1+( ) +NO3
1-( )
Every time you see (s)- leave it alone
AgNO3(aq) + NaCl (aq) AgCl (s) + NaNO3 (aq)
S aqaq aq aq aq aq
Now becomes:
Ag1+(aq) +NO31-(aq) +Na1+(aq)+Cl1-(aq)AgCl(s)+Na1+(aq)+NO3
1-
(aq)
AgNO3(aq) + NaCl (aq) AgCl (s) + NaNO3 (aq)
See how AgNO3 broke apart?See how NaCl broke apart?
See how NaNO3 broke apart?
See how AgCl stayed together?
Every time you see (aq)- break ionic compound apart
Every time you see (s)- leave it alone
Remember…
Now.. If the same element appears on both sides of the reaction in the same form you can cancel it….
Ag1+(aq) +NO31- (aq) +Na1+(aq)+ Cl1-(aq) AgCl(s)+Na1+(aq) + NO3
1-(aq)
Ag1+(aq)+NO31- (aq) + Na1+(aq)+ Cl1-(aq) AgCl (s) + Na1+(aq) + NO3
1-(aq)
What is left is the NET IONIC REACTION: Ag1+(aq)+ Cl1-(aq) 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. 2. All nitrates, acetates & chlorates soluble3. All halides soluble: except those of silver, mercury (I) & lead.4. All sulfates soluble: except calcium, barium, strontium, lead, & mercury.5. Expect for rule 1: carbonates, chromates, sulfides, hydroxides, oxides, phosphates, & silicates insoluble
Now, Balance the reaction
_K2CO3(aq) +_Sr(NO3)2 (aq)_KNO3(aq)+ _SrCO3(s)
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)+2NO3
1-(aq) 2K1+(aq)+2NO31-(aq)+SrCO3(s)
Notice subscripts became coefficients (so you can cancel them out)
Before:K2CO3(aq) + Sr(NO3)2 (aq) 2KNO3(aq)+ SrCO3(s)
Finally, write the Net Ionic Reaction
2K1+(aq) +CO32-(aq) +Sr2+(aq) + 2NO3
1-(aq) 2K1+(aq)+2NO31-(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. 2. All nitrates, acetates & chlorates soluble3. All halides soluble: except those of silver, mercury (I) & lead.4. All sulfates soluble: except calcium, barium, strontium, lead, & mercury.5. Expect for rule 1: carbonates, chromates, sulfides, hydroxides, oxides, phosphates, & silicates insoluble
Step 1 & 2: determine parenthesis and balanceZnSO4(aq)+Ba(C2H3O2)2 (aq) BaSO4(s)+ Zn(C2H3O2)2 (aq)Step 3: break apart ionsZn2+(aq)+SO4
2-(aq)+Ba2+(aq)+2C2H3O21-
(aq) BaSO4(s)+ Zn2+(aq)+ 2C2H3O2
1-(aq)
Step 4: cancel out spectator ionsZn2+(aq)+SO4
2-(aq)+Ba2+(aq)+2C2H3O21-
(aq) BaSO4(s)+ Zn2+(aq)+ 2C2H3O2
1-(aq)
Lastly, Net Ionic: Ba2+(aq) + SO4
2-(aq) BaSO4(s)
ZnSO4( )+Ba(C2H3O2)2 ( ) BaSO4( )+ Zn(C2H3O2)2 ( )
Types of reaction review (3:39)