Warm UP 5.7

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)