Lab 13 (Reactions of Aqueous Ionic Compounds)
Name______________________
Group # ________
Introduction:
Science progresses through the process of experimentation: asking questions, finding ways to answer them and
generating more questions. As a student of chemistry you make many observations in the process of designing and
carrying out experiments. You organize your observations in tables so that they are clearly available for
answering questions and solving problems. Then you can compare your well-organized data in order to answer
questions and solve problems. You consider all the data so you can make correlations that would not be possible
if each observation were considered alone. Your correlations may raise more questions than they answer. But
these new questions promote further experimentation that raises more answers and more questions.
All of the steps in the process of experimentation depend on your carefully made observations. The
prerequisite to answering any chemical question or to solving any chemical problem is the accumulation of
sufficient, accurate, and well-organized observations.
Purpose:
Observe a large number of chemical reactions by mixing solutions of ionic compounds and recording the data
efficiently using a data matrix that ensures all possible binary (two at a time) combinations.
Identify reactions that form precipitates with lead (II) nitrate and write balanced chemical equations for those
reactions.
Identify reactions that formed a gas and write balanced chemical equations for those reactions.
Identify reactions that produced only color changes.
Materials:
Apron
Goggles
Reaction Surface (Saran Wrap)
Paper Towels (For clean-up)
Experimental Page with “X’s” for mixtures
(to help determine color)
Safety Note:





Conc.
Household
1.0 M
1.0 M
1.0 M
1.0 M
0.1 M
1.0 M
0.2 M
0.1 M
0.1 M
0.1 M
0.5 M
0.1 M
Chemical Names and Formulas
Ammonium Hydroxide, NH4OH (aq)
(Ammonia Water) NH3 + H2O
Sodium Hydroxide,
NaOH (aq)
Hydrochloric Acid,
HCl (aq)
Nitric Acid,
HNO3 (aq)
Sulfuric Acid,
H2SO4 (aq)
Sodium Phosphate,
Na3PO4 (aq)
Calcium Chloride,
CaCl2 (aq)
Copper (II) Sulfate,
CuSO4 (aq)
Iron (III) Chloride,
FeCl3 (aq)
Lead (II) Nitrate,
Pb(NO3)2 (aq)
Potassium Iodide,
KI (aq)
Sodium Carbonate,
Na2CO3 (aq)
Silver Nitrate,
AgNO3 (aq)
Many of the chemicals used are toxic or corrosive and should be handled with extreme care.
Follow all safety precautions wearing your safety goggles and lab apron at all times during the lab.
Notify your instructor of any chemical spills immediately.
Wash your hands whenever you come in contact with any of the chemicals.
Also, wash your hands completely after completing the lab.
Lab 13 (Reactions of Aqueous Ionic Compounds)
Name ______________________
Group # ________
Procedures:
1.
2.
Put on your apron and goggles.
Place the experimental page on a flat surface and cover with a piece of Plastic that can be taped to the table. This
will act as your reaction surface.
Adding chemicals to the rows
Note:
3.
4.
When adding the first drop you can touch the plastic surface but make sure that one row does not come in
contact with another row.
Obtain the chemical listed to the left of each row. Add one drop of the chemical to each “X” in the row. For
example: Place one drop of the chemical NH4OH, ammonium hydroxide (also called ammonia water), on each
“X” in the first row.
Repeat step #3 for each row until you get to the last chemical, hydrochloric acid, HCl.
Adding chemicals to the columns
Note:
When adding the second drop hold the dropper bottles vertical as you add drops and keep the tip away from
the drops you added in step #3 and #4 so it does not come in contact with the other chemicals and
contaminate the bottle.
5.
Obtain the chemical listed at the top of the column. Add one drop of the chemical to each “X” in the column. For
example: Place one drop of Pb(NO3)2, lead (II) nitrate to each “X” in the first column.
6.
Record any changes that take place when the two drops are combined.
Hints for recording data:
 Insoluble solids will show up as a cloudy precipitate. This can be recorded as “ppt.”
 Gas bubbles forming can be recorded as “bbls.”
 Color changes can be recorded according to the change in color observed.
Note: The color needs to be different than the original solution.
 If no reaction seems to take place, record this observation as “NVR” for No Visible Reaction.
 If no precipitate is seen record this observation as “NVP” for No Visible Precipitate.
Cleaning up:
7.
Avoid contamination by cleaning up in a way that protects you and your environment. Carefully clean the smallscale reaction surface (Plastic Sheet) by absorbing the contents onto a paper towel. Wrap the reaction surface in a
clean paper towel and dispose of in the red chemical waste bin. Wash your hands thoroughly with soap and
water.
Lab 13 (Reactions of Aqueous Ionic Compounds)
Name ______________________
Group # ________
Data and Observations:
LAB 13 DATA TABLE
Table 13.1
Pb(NO3)2
HCl
Na3PO4
KI
Reactions of Aqueous Ionic Compounds
CuSO4
H2SO4
NaOH
AgNO3
CaCl2
HNO3
Na2CO3
FeCl3
NH4OH
NH4OH
FeCl3
FeCl3
Na2CO3
Na2CO3
HNO3
HNO3
CaCl2
CaCl2
AgNO3
AgNO3
NaOH
NaOH
H2SO4
H2SO4
CuSO4
CuSO4
KI
KI
Na3PO4
KEY
NVR= No Visible Reaction
NVP= No Visible Precipitate
ppt. = Precipitate (Turned cloudy)
bbls. = Bubbles
Na3PO4
HCl
HCl
Pb(NO3)2
Calculations and Graphs:
No calculations or graphs are necessary for this report.
Lab 13 (Reactions of Aqueous Ionic Compounds)
Name ______________________
Group # ________
Analysis and Conclusion:
Use what you learned in this lab to answer the following questions.
Note: Equations will be completed in class after you have collected all the data in the experiment.
1.
Write and balance chemical equations for each precipitation reaction you observed for Lead (II) nitrate.
Equation
Ions
Involved
Equation
Ions
Involved
Equation
Ions
Involved
Equation
Ions
Involved
Equation
Ions
Involved
Equation
Ions
Involved
Equation
Ions
Involved
Equation
Ions
Involved
Equation
Ions
Involved
Equation
Ions
Involved
NH4OH (aq)
NH4+ (aq)
OH-(aq)
FeCl3 (aq)
Fe3+ (aq)
Cl -(aq)
Ca2+ (aq)
+
Cl -(aq)
Na+ (aq)
H+ (aq)
+
Cu2+ (aq)
+
K+ (aq)
Na+ (aq)

+
Pb(NO3)2 (aq)

+
Pb(NO3)2 (aq)

+
Pb(NO3)2 (aq)

+
Pb(NO3)2 (aq)

+
Pb(NO3)2 (aq)

+

+

+
Pb2+ (aq) NO3 -(aq)
+
PO4 3-(aq)
Pb(NO3)2 (aq)
Pb2+ (aq) NO3 -(aq)
+
Cl -(aq)
Pb(NO3)2 (aq)
Pb2+ (aq) NO3 -(aq)
I -(aq)
HCl (aq)
H+ (aq)
+
+
Na3PO4 (aq)
+
Pb2+ (aq) NO3 -(aq)
SO4 2-(aq)
KI (aq)

Pb2+ (aq) NO3 -(aq)
SO4 2-(aq)
CuSO4 (aq)
Pb(NO3)2 (aq)
Pb2+ (aq) NO3 -(aq)
OH-(aq)
H2SO4 (aq)
+
Pb2+ (aq) NO3-(aq)
+
NaOH (aq)

Pb2+ (aq) NO3-(aq)
CO3 2-(aq)
CaCl2 (aq)
Pb(NO3)2 (aq)
Pb2+ (aq) NO3 -(aq)
+
Na2CO3 (aq)
Na+ (aq)
+
Pb(NO3)2 (aq)
Pb2+ (aq) NO3 -(aq)
Lab 13 (Reactions of Aqueous Ionic Compounds)
2.
Name ______________________
Group # ________
You may have noticed that some chemicals formed precipitates when mixed with ammonia, NH 3. This is because ammonia
reacts with water to produce ammonium hydroxide, NH4OH (aq). and the hydroxide anion reacts with the cation in the other
solution.
Equation
NH3 (g)
+

H2O (l)
NH4OH (aq)
NH4+ (aq)
OH -(aq)
To write the chemical equation for the precipitates when mixed with ammonia, you need to replace NH 3 with ammonium
hydroxide, NH4OH (aq).
Equation
Ions
Involved
Equation
Ions
Involved
Equation
Ions
Involved
Equation
Ions
Involved
3.
NH4OH (aq)
NH4+ (aq)
+
OH -(aq)
+
OH -(aq)
CuSO4 (aq)
+
OH-(aq)
AgNO3 (aq)
Ag+ (aq)
NH4OH (aq)
NH4+ (aq)
+

+

+

+
Cu2+ (aq) SO42-(aq)
NH4OH (aq)
NH4+ (aq)

Pb2+ (aq) NO3 -(aq)
NH4OH (aq)
NH4+ (aq)
Pb(NO3)2 (aq)
+
OH - (aq)
NO3-(aq)
FeCl3 (aq)
Fe3+ (aq) Cl -(aq)
Write chemical equations to describe all the reactions that produced bubbles.
Equation
Ions
Involved
Equation
Ions
Involved
Equation
Ions
Involved
Na2CO3 (aq)
Na+ (aq)
CO3 2-(aq)
Na2CO3 (aq)
Na+ (aq)
CO3 2-(aq)
HCl (aq)
H+ (aq)
+
CO3 2-(aq)
Na2CO3 (aq)
Na+ (aq)
+
+
+

+
+

+
+
SO42-(aq)
HNO3 (aq)
H+ (aq)
+
Cl -(aq)
H2SO4 (aq)
H+ (aq)

NO3 -(aq)
4.
What chemicals do all the reactions that produced bubbles have in common?
5.
Which reactions gave color changes but no precipitate? Why do you think this happened?
6.
Which mixings could you have predicted in advance would not result in a reaction?
Lab 13 (Reactions of Aqueous Ionic Compounds)
EXPERIMENTAL PAGE
Pb(NO3)2
HCl
NH4OH
FeCl3
Na2CO3
HNO3
CaCl2
AgNO3
NaOH
H2SO4
CuSO4
KI
Na3PO4
HCl
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
HCl
Pb(NO3)2
Name ______________________
Group # ________
Reactions of Aqueous Ionic Compounds
Na3PO4
KI
CuSO4
H2SO4
NaOH
AgNO3
CaCl2
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
XXX X
XXX
XX
X
Na3PO4
HNO3
Na2CO3
FeCl3
FeCl3
Na2CO3
HNO3
CaCl2
AgNO3
NaOH
H2SO4
CuSO4
KI
KEY
NVR= No Visible Reaction
NVP= No Visible Precipitate
ppt. = Precipitate
bbls. = Bubbles
NH4OH