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Warm UP 5.7

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.

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Warm UP 5.7

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  1. Warm UP 5.7 Determine if the following are soluble or insoluble using the solubility table: • CaSO4 • Ni3(PO4)2 • KOH • HgCl • MgCrO4 insoluble • 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. • . Except for rule 1: carbonates, chromates, sulfides, hydroxides, oxides, phosphates, & silicates insoluble insoluble soluble insoluble insoluble

  2. 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

  3. Aqueous ( aq) Ionic compounds BREAK APART in water Draw this image

  4. Spectator Ions Ions that: • are not directly involved in rxn • end up getting canceled out

  5. Precipitate (s) • Insoluble portion of a rxn • Tiny little solids Precipitate Book Clip

  6. 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

  7. Example #1 Determine what goes in the parenthesis AgNO3(?) + NaCl (?) AgCl (?) + NaNO3 (?)

  8. AgNO3( ) + NaCl( ) AgCl(?) + NaNO3( ) aq aq aq 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. • . 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 ***** this is the same for NaCl & NaNO3

  9. AgNO3(aq) + NaCl (aq) AgCl( ) + NaNO3 (aq) S 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. • . 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

  10. AgNO3(aq) + NaCl (aq)  AgCl (s) + NaNO3 (aq) Every time you see (aq)- break ionic compound apart Ag1+( )+NO31-( )+Na1+( )+Cl1-( )AgCl( )+Na1+( ) +NO31-( ) Every time you see (s)- leave it alone aq aq aq aq aq S aq

  11. AgNO3(aq) + NaCl (aq)  AgCl (s) + NaNO3 (aq) Now becomes: Ag1+(aq) +NO31-(aq)+Na1+(aq)+Cl1-(aq)AgCl(s)+Na1+(aq)+NO31-(aq) See how NaCl broke apart? See how NaNO3 broke apart? See how AgNO3 broke apart? See how AgCl stayed together?

  12. Remember… Every time you see (aq)- break ionic compound apart Every time you see (s)- leave it alone

  13. 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) + NO31-(aq)

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

  15. Net ionic book clip

  16. Example #2

  17. 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

  18. Now, Balance the reaction _K2CO3(aq) +_Sr(NO3)2(aq)_KNO3(aq)+ _SrCO3(s)

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

  20. Next, cancel out ions that match Before: K2CO3(aq) + Sr(NO3)2(aq) 2KNO3(aq)+ SrCO3(s) Notice subscripts became coefficients (so you can cancel them out) 2K1+(aq) +CO32-(aq)+Sr2+(aq)+2NO31-(aq) 2K1+(aq)+2NO31-(aq)+SrCO3(s)

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

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

  23. Example 3

  24. 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

  25. ZnSO4( )+Ba(C2H3O2)2 ( )  BaSO4( )+ Zn(C2H3O2)2 ( ) 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+(aq)+SO42-(aq)+Ba2+(aq)+2C2H3O21-(aq)BaSO4(s)+ Zn2+(aq)+ 2C2H3O21-(aq) Step 4: cancel out spectator ions Zn2+(aq)+SO42-(aq)+Ba2+(aq)+2C2H3O21-(aq)BaSO4(s)+ Zn2+(aq)+ 2C2H3O21-(aq) Lastly, Net Ionic: Ba2+(aq) + SO42-(aq)  BaSO4(s)

  26. Types of reaction review (3:39)

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