Report 4: Metathesis – To Exchange or Not
Hopefully here for the Report Form
Note: In preparing this report you are free to use references and consult with others.
However, you may not copy from other students’ work (including your laboratory
partner) or misrepresent your own data (see honor code).
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Part 1: Metathesis Reactions
1. Copper (II) sulfate + sodium carbonate
Observations
Molecular equation
Complete ionic equation
Net ionic equation
2. Copper(II) sulfate + barium chloride
Observations
Molecular equation
Complete ionic equation
Net ionic equation
3. Copper(II) sulfate + sodium phosphate
Observations
Molecular equation
Complete ionic equation
Net ionic equation
4. Sodium carbonate + sulfuric acid
Observations
Molecular equation
Complete ionic equation
Net ionic equation
5. Sodium carbonate + hydrochloric acid
Observations
Molecular equation
Complete ionic equation
Net ionic equation
6. Cadmium chloride + sodium sulfide
Observations
Molecular equation
Complete ionic equation
Net ionic equation
7. Cadmium chloride + sodium hydroxide
Observations
Molecular equation
Complete ionic equation
Net ionic equation
8. Nickel chloride + silver nitrate
Observations
Molecular equation
Complete ionic equation
Net ionic equation
9. Nickel chloride + sodium carbonate
Observations
Molecular equation
Complete ionic equation
Net ionic equation
10. Hydrochloric acid + sodium hydroxide
Observations
Molecular equation
Complete ionic equation
Net ionic equation
11. Ammonium chloride + sodium hydroxide
Observations
Molecular equation
Complete ionic equation
Net ionic equation
12. Sodium acetate + hydrochloric acid
Observations
Molecular equation
Complete ionic equation
Net ionic equation
13. Sodium sulfide + hydrochloric acid
Observations
Molecular equation
Complete ionic equation
Net ionic equation
14. Lead nitrate + sodium sulfide
Observations
Molecular equation
Complete ionic equation
Net ionic equation
15. Lead nitrate + sulfuric acid
Observations
Molecular equation
Complete ionic equation
Net ionic equation
16. Potassium chloride + sodium nitrate
Observations
Molecular equation
Complete ionic equation
Net ionic equation
Part 2: Solubility, Temperature and Crystallization
Table 3 Molar Solubilities of NaCl, NaNO3 , KCl, and KNO3 (mol/L)
0°C
20°C
40°C
60°C
80°C
100°C
NaCl
5.4
5.4
5.5
5.5
5.5
5.6
NaNO3
6.7
7.6
8.5
9.4
10.4
11.3
KCl
3.4
4.0
4.6
5.1
5.5
5.8
KNO3
1.3
3.2
5.2
7.0
9.0
11.0
Compound
1. Calculate the initial molarities of NaNO3 , KCl, NaCl, KNO3 .
First Batch of Crystals
2. The first batch of crystals is formed at 10C. Describe these crystals in terms of
shape, color, consistency, etc.
3. Use the solubility chart to determine the identity of the crystals. Explain your answer.
Second Batch of Crystals
4. What was the temperature of the filtrate when the second batch of crystals formed?
5. Describe these crystals in terms of shape, color, consistency, etc.
6. Assuming that the first batch of crystals crystallized completely, removing all of it’s
ions from solution, what is the identity of the second batch of crystals? (use your
solubility chart and explain your answer)
Third Batch of Crystals
7. The reason that we see a third batch of crystals is that we don’t get complete
crystallization of the salts in the 1st and 2nd batches of crystals. Assuming there is a
small concentration of each ion left in solution after the second batch of crystals is
formed, what is the identity of the third batch of crystals according to your solubility
chart?
8. Describe these crystals in terms of shape, color, consistency, etc.
BONUS QUESTION:
Describe two different tests that we could use to determine the identity of each set of
crystals. To receive full credit you must give the name of the test, a description of the
theory, and describe the results that you would for your proposed identity of each set of
crystals. (5 points max.)