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).

Name: ______

Section: ______

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, , KCl, and (mol/L)

Compound / 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
/ 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
/ 1.3 / 3.2 / 5.2 / 7.0 / 9.0 / 11.0
  1. Calculate the initial molarities of , KCl, NaCl, .

First Batch of Crystals

  1. The first batch of crystals is formed at 10C. Describe these crystals in terms of shape, color, consistency, etc.
  1. Use the solubility chart to determine the identity of the crystals. Explain your answer.

Second Batch of Crystals

  1. What was the temperature of the filtrate when the second batch of crystals formed?
  1. Describe these crystals in terms of shape, color, consistency, etc.
  1. 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

  1. 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?
  1. 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.)