1. Reactions of Aqueous Ionic Compounds
Lab 13 Results
Reactions of Aqueous
Ionic Compounds

2. White ppt. NVR NVR NVR Faint White ppt. Orange ppt. Amber NVP NVR
Pb(NO3)2
HCl
Na3PO4 KI
White
ppt.
NH4OH
NVR
NVR
NVR
Faint
White
ppt.
Orange
ppt.
Amber
NVP
NVR
FeCl3
White
ppt.
Na2CO3
bbls.
NVR
NVR

3. Analysis and Conclusions
Question 1:
Identify all reactions that produced a precipitate with:
Lead (II) nitrate
Pb(NO3)2 (aq)

4. Pb(NO3)2
HCl
Na3PO4 KI
White
ppt.
NH4OH
FeCl3
Na2CO3

5. + What Reacts? NH4OH(aq) Pb(NO3)2(aq) Pb2+ NO3-1 NH4+1 OH-1 -2 NO3-1

6. No! Both have (+) charges Will the two cations react?
NH4OH(aq)
Pb(NO3)2(aq)
NO3-1
Pb2+
NH4+1
OH-1
No!
Both
have
(+)
charges
Will
the two
cations
react?
repel
NH4+1
Pb2+
OH-1
NO3-1

7. No! Both have (-) charges Will the two anions react?+
NH4OH(aq)
Pb(NO3)2(aq)
NO3-1
Pb2+
NH4+1
OH-1
No!
Both
have
(-)
charges
Will
the two
anions
react?
NH4+1
Pb2+
OH-1
NO3-1
repel

8. Opposites Attract (+) (-) + NH4OH(aq) Pb(NO3)2(aq) NO3-1 Pb2+ NH4+1
Cations
Anions
Soluble
(stays dissolved
in H2O)
NH4+1
NH4NO3(aq)
NO3-1
NH4+1
NO3-1
Insoluble
(Falls out of
solution)
Pb2+
Pb(OH)2(s)
OH-1
Turns cloudy white
OH-1
Pb2+
OH-1
(White ppt.)

9. 2 2 NH4OH(aq) + Pb(NO3)2(aq)  NH4NO3(aq) + Pb(OH)2(s)
Chemical Equation is now balanced.
Chemical Equation needs to be balanced. 2
NH4OH(aq) Pb(NO3)2(aq)  NH4NO3(aq) Pb(OH)2(s) 2

10. + (+) (-) FeCl3(aq) FeCl3(aq) Pb(NO3)2(aq) Pb(NO3)2(aq) 2 NO3-1 Pb2+
Cations
Anions
Soluble
(stays dissolved
in H2O)
NO3-1
is always
soluble
Fe3+
Fe(NO3)3(aq)
NO3-1
Fe3+
NO3-1
NO3-1
NO3-1
Insoluble
(Falls out of
solution)
Pb2+
PbCl2(s)
Cl-1
Faint White
ppt.
Cl-1
Pb2+
Cl-1

11. 2 3 2 3 FeCl3 (aq) + Pb(NO3)2(aq)  Fe(NO3)3 (aq) + PbCl2(s)
Chemical Equation needs to be balanced.
Chemical Equation is now balanced. 2
FeCl3 (aq) Pb(NO3)2(aq)  Fe(NO3)3 (aq) PbCl2(s) 3 2 3

12. + (+) (-) Na2CO3(aq) Na2CO3(aq) Pb(NO3)2(aq) Pb(NO3)2(aq) 2 NO3-1 2
Cations
Anions
Soluble
(stays dissolved
in H2O)
Na+ & NO3-1
are always
soluble
Na+
NaNO3(aq)
NO3-1
Na+
NO3-1
Insoluble
(Falls out of
solution)
Pb2+
PbCO3(s)
CO32-
White
ppt.
CO32-
Pb2+

13. 2 Na2CO3 (aq) + Pb(NO3)2(aq)  NaNO3 (aq) + PbCO3(s)
Chemical Equation is now balanced.
Chemical Equation needs to be balanced.
Na2CO3 (aq) Pb(NO3)2(aq)  NaNO3 (aq) PbCO3(s) 2

14. + (+) (-) CaCl2(aq) CaCl2(aq) Pb(NO3)2(aq) Pb(NO3)2(aq) 2 NO3-1 Pb2+
Cations
Anions
Soluble
(stays dissolved
in H2O)
NO3-1
is always
soluble
Ca2+
Ca(NO3)2(aq)
NO3-1
Ca2+
NO3-1
NO3-1
Insoluble
(Falls out of
solution)
Pb2+
PbCl2(s)
Cl-1
Faint White
ppt.
Cl-1
Pb2+
Cl-1

15. CaCl2 (aq) + Pb(NO3)2(aq)  Ca(NO3)2 (aq) + PbCl2(s)
Chemical Equation is balanced as written.
CaCl2 (aq) Pb(NO3)2(aq)  Ca(NO3)2 (aq) PbCl2(s)

16. + (+) (-) NaOH(aq) Pb(NO3)2(aq) Pb(NO3)2(aq) 2 NO3-1 Pb2+ Na+ OH- Na+
Cations
Anions
Soluble
(stays dissolved
in H2O)
Na+ & NO3-1
are always
soluble
Na+
NaNO3(aq)
NO3-1
Na+
NO3-1
Insoluble
(Falls out of
solution)
Pb2+
Pb(OH)2(s)
OH-
White
ppt.
OH-
Pb2+
OH-

17. 2 2 NaOH(aq) + Pb(NO3)2(aq)  NaNO3(aq) + Pb(OH)2(s)
Chemical Equation is now balanced.
Chemical Equation needs to be balanced. 2
NaOH(aq) Pb(NO3)2(aq)  NaNO3(aq) Pb(OH)2(s) 2

18. + (+) (-) H2SO4(aq) H2SO4(aq) Pb(NO3)2(aq) Pb(NO3)2(aq) 2 NO3-1 2 H+
Cations
Anions
Soluble
(stays dissolved
in H2O)
NO3-1
is always
soluble H+
HNO3(aq)
NO3-1 H+
NO3-1
Insoluble
(Falls out of
solution)
Pb2+
PbSO4(s)
SO42-
White
ppt.
SO42-
Pb2+

19. 2 H2SO4 (aq) + Pb(NO3)2(aq)  HNO3 (aq) + PbSO4(s)
Chemical Equation is now balanced.
Chemical Equation needs to be balanced.
H2SO4 (aq) Pb(NO3)2(aq)  HNO3 (aq) PbSO4(s) 2

20. + (+) (-) CuSO4(aq) Pb(NO3)2(aq) Pb(NO3)2(aq) Cu2+ SO42- Pb2+ 2 NO3-1
Cations
Anions
Soluble
(stays dissolved
in H2O)
NO3-1
is always
soluble
Cu2+
Cu(NO3)2 (aq)
NO3-1
Cu2+
NO3-1
NO3-1
Insoluble
(Falls out of
solution)
Pb2+
PbSO4(s)
SO42-
White
ppt.
SO42-
Pb2+

21. CuSO4(aq) + Pb(NO3)2(aq)  Cu(NO3)2(aq) + PbSO4(s)
Chemical Equation balanced as written
Chemical Equation needs to be balanced.
CuSO4(aq) Pb(NO3)2(aq)  Cu(NO3)2(aq) PbSO4(s)

22. + (+) (-) KI(aq) Pb(NO3)2(aq) Pb(NO3)2(aq) 2 NO3-1 Pb2+ K+ I- K+
Cations
Anions
Soluble
(stays dissolved
in H2O)
K+ & NO3-1
are always
soluble K+
KNO3(aq)
NO3-1 K+
NO3-1
Insoluble
(Falls out of
solution)
Pb2+
PbI2(s) I-
Bright
Yellow
ppt. I-
Pb2+ I-

23. 2 2 KI(aq) + Pb(NO3)2(aq)  KNO3(aq) + PbI2(s)
Chemical Equation is now balanced.
Chemical Equation needs to be balanced. 2
KI(aq) Pb(NO3)2(aq)  KNO3(aq) PbI2(s) 2

24. + (+) (-) Na3PO4(aq) Na3PO4(aq) Pb(NO3)2(aq) Pb(NO3)2(aq) 3 Na+ PO43-
Cations
Anions
Soluble
(stays dissolved
in H2O)
Na+ & NO3-1
are always
soluble
Na+
NaNO3(aq)
NO3-1
Na+
NO3-1
Insoluble
(Falls out of
solution)
Pb2+
Pb3(PO4)2 (s)
PO43-
White
ppt.
PO43-
Pb2+
Pb2+
PO43-
Pb2+

25. 2 3 6 Na3PO4(aq) + Pb(NO3)2(aq)  NaNO3(aq) + Pb3(PO4)2(s)
Chemical Equation is now balanced.
Chemical Equation needs to be balanced. 2
Na3PO4(aq) Pb(NO3)2(aq)  NaNO3(aq) Pb3(PO4)2(s) 3 6

26. + (+) (-) HCl(aq) Pb(NO3)2(aq) Pb(NO3)2(aq) 2 NO3-1 Pb2+ H+ Cl- H+
Cations
Anions
Soluble
(stays dissolved
in H2O)
NO3-1
is always
soluble H+
HNO3(aq)
NO3-1 H+
NO3-1
Insoluble
(Falls out of
solution)
Pb2+
PbCl2(s)
Cl-
Faint
white
ppt.
Cl-
Pb2+
Cl-

27. 2 2 HCl(aq) + Pb(NO3)2(aq)  HNO3(aq) + PbCl2(s)
Chemical Equation is now balanced.
Chemical Equation needs to be balanced. 2
HCl(aq) Pb(NO3)2(aq)  HNO3(aq) PbCl2(s) 2

28. Analysis and Conclusions
Question 2:
Identify all reactions that produced a precipitate with the ammonia solution:
Ammonium hydroxide
NH4OH (aq)

29. + (+) (-) NH4OH(aq) Pb(NO3)2(aq) Pb(NO3)2(aq) Pb2+ 2 NO3-1 NH4+1 OH-1
Cations
Anions
Soluble
(stays dissolved
in H2O)
NH4+1 & NO3-1
are always
soluble
NH4+1
NH4NO3(aq)
NO3-1
NH4+1
NO3-1
Insoluble
(Falls out of
solution)
Pb2+
Pb(OH)2(s)
OH-1
OH-1
White
ppt.
Pb2+
OH-1

30. 2 2 NH4OH(aq) + Pb(NO3)2(aq)  NH4NO3(aq) + Pb(OH)2(s)
Chemical Equation is now balanced.
Chemical Equation needs to be balanced. 2
NH4OH(aq) Pb(NO3)2(aq)  NH4NO3(aq) Pb(OH)2(s) 2

31. + (+) (-) NH4OH(aq) CuSO4(aq) Cu2+ SO42- NH4+1 OH-1 (NH4)2SO4(aq)
Cations
Anions
Soluble
(stays dissolved
in H2O)
NH4+1
is always
soluble
(NH4)2SO4(aq)
NH4+1
SO42-
NH4+1
SO42-
NH4+1
Insoluble
(Falls out of
solution)
Cu2+
Cu(OH)2(s)
OH-1
Light
Blue
ppt.
OH-1
Cu2+
OH-1

32. 2 NH4OH(aq) + CuSO4(aq)  (NH4)2SO4(aq) + Cu(OH)2(s)
Chemical Equation is now balanced.
Chemical Equation needs to be balanced. 2
NH4OH(aq) CuSO4(aq)  (NH4)2SO4(aq) Cu(OH)2(s)

33. + (+) (-) NH4OH(aq) AgNO3(aq) Ag+ NO3-1 NH4+1 OH-1 NH4+1 NH4NO3(aq)
Cations
Anions
Soluble
(stays dissolved
in H2O)
NH4+1 & NO3-1
are always
soluble
NH4+1
NH4NO3(aq)
NO3-1
NH4+1
NO3-1
Insoluble
(Falls out of
solution)
AgOH(s)
Ag+
OH-1
Tan
ppt.
OH-1
Ag+

34. NH4OH(aq) + AgNO3(aq)  NH4NO3(aq) + AgOH(s)
Chemical Equation is now balanced.
Chemical Equation needs to be balanced.
NH4OH(aq) AgNO3(aq)  NH4NO3(aq) AgOH(s)

35. + (+) (-) NH4OH(aq) FeCl3(aq) FeCl3(aq) Fe3+ 3 Cl- NH4+1 OH-1 NH4+1
Cations
Anions
Soluble
(stays dissolved
in H2O)
NH4+1
is always
soluble
NH4+1
NH4Cl(aq)
Cl-
NH4+1
Cl-
Insoluble
(Falls out of
solution)
Fe3+
Fe(OH)3(s)
OH-
OH-1
Faint
Orange
ppt.
Fe3+
OH-
OH-

36. 3 3 NH4OH(aq) + FeCl3(aq)  NH4Cl(aq) + Fe(OH)3(s)
Chemical Equation is now balanced.
Chemical Equation needs to be balanced. 3
NH4OH(aq) FeCl3(aq)  NH4Cl(aq) Fe(OH)3(s) 3

37. Analysis and Conclusions
Question 3:
Identify all chemical reactions that produced bubbles:
Pb(NO3)2
HCl
Na3PO4 KI
CuSO4
H2SO4
NaOH
AgNO3
CaCl2
HNO3

38. + (+) (-) Na2CO3(aq) Na2CO3(aq) HCl(aq) Cl- 2 Na+ CO32- H+ Na+
Cations
Anions
Soluble
(stays dissolved
in H2O)
Na+
is always
soluble
Na+
NaCl(aq)
Cl-
Na+
Cl- H+
CO32-
CO32- H+ H+
H2O(l)
O2-
CO2
CO2
Bubbles
Bubbles

39. Chemical Equation is now balanced.
Chemical Equation needs to be balanced.
Na2CO3(aq) HCl(aq)  CO2(g) H2O(l) NaCl (aq) 2 2
Na+
CO2
CO2
O2- H+
Cl-
H2O(l)
NaCl

40. + (+) (-) Na2CO3(aq) Na2CO3(aq) H2SO4(aq) H2SO4(aq) SO42- 2 Na+ CO32-
Cations
Anions
Soluble
(stays dissolved
in H2O)
Na+
is always
soluble
Na2SO4 (aq)
Na+
SO42-
Na+
SO42-
Na+ H+
CO32-
CO32- H+ H+
H2O(l)
O2-
CO2
CO2
Bubbles
Bubbles

41. Chemical Equation is balanced as written.
Na2CO3(aq) H2SO4(aq)  CO2(g) H2O(l) + Na2SO4(aq)
Na+
CO2
CO2
O2- H+
SO42-
H2O(l)
Na2SO4

42. + (+) (-) Na2CO3(aq) Na2CO3(aq) HNO3 (aq) NO3- 2 Na+ CO32- H+ Na+
Cations
Anions
Soluble
(stays dissolved
in H2O)
Na+
is always
soluble
Na+
NaNO3 (aq)
NO3-
Na+
NO3- H+
CO32-
CO32- H+ H+
H2O(l)
O2-
CO2
CO2
Bubbles
Bubbles

43. Chemical Equation is now balanced.
Chemical Equation needs to be balanced.
Na2CO3(aq) HNO3(aq)  CO2(g) H2O(l) NaNO3(aq) 2 2
Na+
CO2
CO2
O2- H+
NO31-
H2O(l)
NaNO3

44. Analysis and Conclusions
Question 4:
What do all the chemical reactions that produced bubbles have in common?
Bubbles happened whenever an ACID was reacted with sodium carbonate, Na2CO3

45. Analysis and Conclusions
Question 5:
What reactions gave a color change but no precipitate?

46. PbNO3
HCl
Na3PO4 KI
NH4OH
Amber
NVP
FeCl3
Na2CO3

47. Fe3+ + I-  FeI2+(aq) Amber NVP
The reaction between KI and FeCl3 probably made a complex ion. KI
Fe3+ + I- 
FeI2+(aq)
(Still dissolved)
Amber
NVP
FeCl3

48. Analysis and Conclusions
Question 6:
Which mixings could you have predicted in advance would not result in a reaction?
Any reaction that had common ions.

49. Both have Cl- Both have Na+
PbNO3
HCl
Na3PO4 KI
NH4OH
Both
have
Cl-
FeCl3
Both
have
Na+
Na2CO3