For each solution, determine the
soluble ions.
A.
B.
C.
D.
Potassium Iodide (aq)
Barium Nitrate (aq)
Lead Nitrate (aq)
Sodium Sulfate (aq)
Mix the following solutions in pairs
A.
B.
C.
D.
Potassium Iodide
Barium Nitrate
Lead Nitrate
Sodium Sulfate
• When finished, try Silver Nitrate with
Potassium Iodide.
Determine the precipitates.
Solubility of Ions
Always
Sometimes
K+
IPb2+
NO3Ag+
Ba2+
SO42Na+
Precipitate Reactions
• Precipitates
• Solubility rules
• Using the rules of
solubility
Reaction of Pb(NO3)2 and KI
• Lead II Nitrate and
Potassium Iodide
• Both are strong
electrolytes
• That means they
completely dissociate
into ions
• Adding the
solutions together
will create
something new…
• A chemical change
the evidence is the
precipitate.
Look closer at
Lead (II) Nitrate
Strong Electrolyte
Ions completely
dissociate into:
Lead Pb2+ ions
Nitrate NO3 - Ions
Pb (NO3)2
The KI does the same thing
• Posassium K+
ions
and Iodide I- ions
form.
They are floating
around in the
water.
(an aqueous
solution)
When the lead and
the iodide ions come
into contact, they
form a precipitate
• The precipitate falls
to the bottom,
spectator ions are
left in solution
Solubility Rules
• All sodium, potassium,
ammonium, and nitrate
• Rationale:
salts are soluble in water.
Memorization of
solubility rules does
• ✘✘Memorization of other
“solubility rules” is beyond
not deepen
the scope of this course and understanding
the of the AP Exam
Stoichiometry in Aqueous Reactions
What volume of 0.200 M copper (II) sulfate is required to
react with 50.0mL if 0.100 M NaOH?
1) Write the net ionic equation
What volume of 0.200 M copper (II) sulfate is required to react
with 50.0mL if 0.100 M NaOH?
find the moles of each reactant needed:
nOH- =
nCu2+ =