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Experiment 9 – Online Version
A. Metathesis Reactions
Watch the videos that follow to see what each metathesis reaction looks like.
Next, use the information given in the Discussion portion of this experiment
as well as the following example to fill out Part A. on the report sheet.
example:
lead(II) nitrate + potassium iodide
Observations: (determined from watching a video of the reaction) two
colorless solutions mix to form a solid yellow precipitate
Molecular equation: Pb(NO3)2(aq) + 2 KI(aq)
→
PbI2(s) + 2 KNO3(aq)
Complete ionic equation: Pb2+(aq) + 2 NO3-(aq) + 2 K+(aq) + 2 I-(aq)
PbI2(s) + 2 K+(aq) + 2 NO3-(aq)
Net ionic equation: Pb2+(aq) + 2 I-(aq)
→
PbI2(s)
1. Copper(II) sulfate + sodium carbonate

2. Copper(II) sulfate + barium chloride

3. Copper(II) sulfate + sodium phosphate
→
(in this video, copper(II) chloride is used instead of copper(II) sulfate – but the
reaction would look similar to that with copper(II) sulfate)

4. Sodium carbonate + sulfuric acid
(in this video, solid sodium bicarbonate is used instead of a sodium carbonate
solution – but the reaction would look similar to that with a sodium carbonate
solution)

5. Sodium carbonate + hydrochloric acid
(visually, this reaction would look the same as the video above (with sodium
bicarbonate reacting with sulfuric acid))
6. Cadmium chloride + sodium sulfide

7. Cadmium chloride + sodium hydroxide

8. Nickel chloride + silver nitrate
(no video found, in this reaction – a white precipitate would form in a green
solution)
9. Nickel chloride + sodium carbonate
(in this video, nickel(II) nitrate is used instead of nickel chloride – but the
reaction would look similar to that with nickel chloride)
10. Hydrochloric acid + sodium hydroxide
(note that an indicator was used in the video – without the indicator (as would
have been in the lab) the reaction would remain colorless)

11. Ammonium chloride + sodium hydroxide
(solid ammonium chloride is used instead of an ammonium chloride solution but the reaction would appear the same)

12. Sodium acetate + hydrochloric acid
(no video found, in this reaction – the solution would remain clear and
colorless)
13. Sodium sulfide + hydrochloric acid
(solid sodium sulfide is used instead of a sodium sulfide solution – but the
reaction would appear the same)

B. Solubility, Temperature, and Crystallization
Watch the following video, which shows an example of crystallizing KNO3
from a solution. This is not the same as the experiment in this lab, but it will
give you an idea of what a crystallization looks like.

Fill in the graph on Part B. of your report sheet by using the information in
Table 9.3 on page 105 to complete the solubility versus temperature plot for
each NaCl, NaNO3, KCl, and KNO3
1. Molarities: (determine on your own – assume the exact amounts of 8.5 g of
NaNO3, and 7.5 g of KCl in 25 mL of water (as described in the procedure) to
calculate each of the molarities listed)
Remember that these are ionic compounds which will dissociate into their
respective ions in water; therefore if there was, for example 0.5 mol/L of Na+
and 0.5 mol/L of Cl-, this would mean there is 0.5 mol/L NaCl, or 0.5 M NaCl.
2. Crystal shape (first batch): would appear as rhombic-type needles
3. Identity of crystals (first batch): (determine on your own by using your graph
and the information about each crystal shape below)
4. Temperature of filtrate: assume around 20 °C
5. Crystal shape of second batch: cubes
6. Identity of second batch of crystals: (determine on your own by using your
graph and the information about each crystal shape below)
7. Crystal shape of third batch: cubes
8. Identity of third batch of crystals: (determine on your own by using your
graph and the information about each crystal shape below)
Crystal shape of NaCl: face-centered cubic (cube)
Crystal shape of NaNO3: trigonal and rhombohedral
Crystal shape of KCl: face-centered cubic (cube)
Crystal shape of KNO3: orthorhombic

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