Year 10 Precipitation reaction.

1. Y E A R 1 0 – C O M P O U N D S A N D R E A C T I O N
G . A J E T R A O
PRECIPITATION

2. AIM
To investigate
precipitation reaction
Write a hypothesis for the
experiment.

3. BACKGROUND INFORMATION
Precipitation reaction occurs when two solutions are mixed
together to form an insoluble compound called precipitate that
settles out of solution.
AB + CD  AD + BC
double displacement reaction

4. SOLUBILITY RULE
Soluble Ionic Compounds
• 1. All common compounds of the Group 1A ions (Li+, Na+,
K+, etc.) and the ammonium ion (NH4
+) are soluble.
• 2. All common nitrates (NO3
-), acetates (C2H3O2
-), and most
perchlorates (ClO4
-) are soluble.
• 3. All common chlorides (Cl-), bromides (Br-), and iodides
(I-) are soluble, except those of Ag+, Pb2+, and Hg2
2+.
• 4. All common sulfates (SO4
2-) are soluble, except those of
Ca2+, Sr2+, Ba2+, Pb2+, and Ag+.

5. SOLUBILITY RULE CONTINUED
Insoluble Ionic Compounds
• 5. All metal hydroxides (OH-) are insoluble, except those of
Group 1A, NH4
+, which are soluble, and Ca2+, Sr2+, and Ba2+,
which are slightly soluble.
• 6. All sulfides (S2-) are insoluble, except those of Group 1A,
NH4
+, Ca2+, Sr2+, and Ba2+.
• 7. All carbonates (CO3
2-) and phosphates (PO4
3-) are
insoluble, except those of Group 1A and NH4
+.

6. EQUIPMENT
Metal ions – barium
nitrate, calcium nitrate,
lead nitrate, copper nitrate
in dropper bottle
Non-metal ions- sodium
carbonate, sodium
chloride, sodium
hydroxide, sodium
sulfate, sodium iodide in
dropper bottle.
• Spotting plate

7. RISK ASSESSMENT
Risk Injury Prevention
Stain Silver nitrate and lead
nitrate are poisonous
Avoid contact with skin.
Use small amounts of
solutions in dropper bottle

8. METHOD
1. Take a spotting plate.
2. Add one drop of solution to
each well of the spotting
plate.
3. Add a drop of other solution
as shown in the table on the
next slide.
4. Record the presence or
absence of precipitate.
5. If there is a precipitate
observe and record the
colour of the precipitate
and the colour of the
solution.

9. TABLE
CO3
2-
Sodium
carbonate
Cl-
Sodium chloride
OH-
Sodium
Hydroxide
I-
Sodium Iodide
SO4
2-
Sodium sulfate
Ba2+
Barium nitrate
Ca2+
Calcium nitrate
Pb2+
Lead nitrate
Cu2+
Copper nitrate

10. RESULT TABLE
• Construct a result table for data you are going to gather from
the investigation.

11. DISCUSSION
1. Which metals ions are soluble?
2. Which non- metals ions are insoluble?

12. CONCLUSION
• Write a appropriate conclusion (make sure it is related to your
results).