Solutions and Solubility
7.3 Reactions in Solution
Predicting Ionic Solubility
most Ionic compounds (salts) are soluble in water,
but the degree of solubility is different for different
salts. Salts can be described in one of the following
categories:
soluble
partly (or sparingly) soluble
insoluble
REVIEW: Predicting IONIC SOLUBILITY
In a chemical reaction between two Ionic solutions,
a precipitate may form.
If a precipitate forms, one of the products of the
reaction is the precipitate, in other words, it is
insoluble and it is a solid.
We can predict which product forms the
precipitate if we have a solubility chart handy.
Solubility Table (pg. 324)
Predicting Ionic Solubility – warm-up

Use a solubility chart to predict the solubility of the following
compounds in water. State whether they are soluble or insoluble
in water.
Ca(NO3)2
CuCl2
KBr
(NH4)2CO3
Fe(NO3)3
Ca(OH)2
NH4CH3COO
Pb(NO3)4
Ca3(PO4)2
CuCl
KCH3COO
PbCO3
BaSO4
AgOH
Ag2SO4
Cr(OH)3
Predicting Ionic Solubility

Use a solubility chart to predict the solubility of the following
compounds in water. State whether they are soluble or insoluble
in water.
Ca(NO3)2
soluble
CuCl2
KBr
(NH4)2CO3
Fe(NO3)3
Ca(OH)2
NH4CH3COO
Pb(NO3)4
Ca3(PO4)2
CuCl
KCH3COO
PbCO3
BaSO4
AgOH
Ag2SO4
Cr(OH)3
Predicting Ionic Solubility

Use a solubility chart to predict the solubility of the following
compounds in water. State whether they are soluble or insoluble
in water.
Ca(NO3)2
soluble
CuCl2
KBr
soluble
(NH4)2CO3
Fe(NO3)3
Ca(OH)2
NH4CH3COO
Pb(NO3)4
Ca3(PO4)2
CuCl
KCH3COO
PbCO3
BaSO4
AgOH
Ag2SO4
Cr(OH)3
Predicting Ionic Solubility

Use a solubility chart to predict the solubility of the following
compounds in water. State whether they are soluble or insoluble
in water.
Ca(NO3)2
soluble
CuCl2
KBr
soluble
(NH4)2CO3
Fe(NO3)3
soluble
Ca(OH)2
NH4CH3COO
Pb(NO3)4
Ca3(PO4)2
CuCl
KCH3COO
PbCO3
BaSO4
AgOH
Ag2SO4
Cr(OH)3
Predicting Ionic Solubility

Use a solubility chart to predict the solubility of the following
compounds in water. State whether they are soluble or insoluble
in water.
Ca(NO3)2
soluble
CuCl2
KBr
soluble
(NH4)2CO3
Fe(NO3)3
soluble
Ca(OH)2
NH4CH3COO
soluble
Pb(NO3)4
Ca3(PO4)2
CuCl
KCH3COO
PbCO3
BaSO4
AgOH
Ag2SO4
Cr(OH)3
Predicting Ionic Solubility

Use a solubility chart to predict the solubility of the following
compounds in water. State whether they are soluble or insoluble
in water.
Ca(NO3)2
soluble
CuCl2
KBr
soluble
(NH4)2CO3
Fe(NO3)3
soluble
Ca(OH)2
NH4CH3COO
soluble
Pb(NO3)4
Ca3(PO4)2
insoluble
CuCl
KCH3COO
PbCO3
BaSO4
AgOH
Ag2SO4
Cr(OH)3
Predicting Ionic Solubility

Use a solubility chart to predict the solubility of the following
compounds in water. State whether they are soluble or insoluble
in water.
Ca(NO3)2
soluble
CuCl2
KBr
soluble
(NH4)2CO3
Fe(NO3)3
soluble
Ca(OH)2
NH4CH3COO
soluble
Pb(NO3)4
Ca3(PO4)2
insoluble
CuCl
KCH3COO
soluble
PbCO3
BaSO4
AgOH
Ag2SO4
Cr(OH)3
Predicting Ionic Solubility

Use a solubility chart to predict the solubility of the following
compounds in water. State whether they are soluble or insoluble
in water.
Ca(NO3)2
soluble
CuCl2
KBr
soluble
(NH4)2CO3
Fe(NO3)3
soluble
Ca(OH)2
NH4CH3COO
soluble
Pb(NO3)4
Ca3(PO4)2
insoluble
CuCl
KCH3COO
soluble
PbCO3
BaSO4
insoluble
AgOH
Ag2SO4
Cr(OH)3
Predicting Ionic Solubility

Use a solubility chart to predict the solubility of the following
compounds in water. State whether they are soluble or insoluble
in water.
Ca(NO3)2
soluble
CuCl2
KBr
soluble
(NH4)2CO3
Fe(NO3)3
soluble
Ca(OH)2
NH4CH3COO
soluble
Pb(NO3)4
Ca3(PO4)2
insoluble
CuCl
KCH3COO
soluble
PbCO3
BaSO4
insoluble
AgOH
Ag2SO4
insoluble
Cr(OH)3
Predicting Ionic Solubility

Use a solubility chart to predict the solubility of the following
compounds in water. State whether they are soluble or insoluble
in water.
Ca(NO3)2
soluble
CuCl2
KBr
soluble
(NH4)2CO3
Fe(NO3)3
soluble
Ca(OH)2
NH4CH3COO
soluble
Pb(NO3)4
Ca3(PO4)2
insoluble
CuCl
KCH3COO
soluble
PbCO3
BaSO4
insoluble
AgOH
Ag2SO4
insoluble
Cr(OH)3
soluble
Predicting Ionic Solubility

Use a solubility chart to predict the solubility of the following
compounds in water. State whether they are soluble or insoluble
in water.
Ca(NO3)2
soluble
CuCl2
soluble
KBr
soluble
(NH4)2CO3
soluble
Fe(NO3)3
soluble
Ca(OH)2
NH4CH3COO
soluble
Pb(NO3)4
Ca3(PO4)2
insoluble
CuCl
KCH3COO
soluble
PbCO3
BaSO4
insoluble
AgOH
Ag2SO4
insoluble
Cr(OH)3
Predicting Ionic Solubility

Use a solubility chart to predict the solubility of the following
compounds in water. State whether they are soluble or insoluble
in water.
Ca(NO3)2
soluble
CuCl2
soluble
KBr
soluble
(NH4)2CO3
soluble
Fe(NO3)3
soluble
Ca(OH)2
insoluble
NH4CH3COO
soluble
Pb(NO3)4
Ca3(PO4)2
insoluble
CuCl
KCH3COO
soluble
PbCO3
BaSO4
insoluble
AgOH
Ag2SO4
insoluble
Cr(OH)3
Predicting Ionic Solubility

Use a solubility chart to predict the solubility of the following
compounds in water. State whether they are soluble or insoluble
in water.
Ca(NO3)2
soluble
CuCl2
soluble
KBr
soluble
(NH4)2CO3
soluble
Fe(NO3)3
soluble
Ca(OH)2
insoluble
NH4CH3COO
soluble
Pb(NO3)4
soluble
Ca3(PO4)2
insoluble
CuCl
KCH3COO
soluble
PbCO3
BaSO4
insoluble
AgOH
Ag2SO4
insoluble
Cr(OH)3
Predicting Ionic Solubility

Use a solubility chart to predict the solubility of the following
compounds in water. State whether they are soluble or insoluble
in water.
Ca(NO3)2
soluble
CuCl2
soluble
KBr
soluble
(NH4)2CO3
soluble
Fe(NO3)3
soluble
Ca(OH)2
insoluble
NH4CH3COO
soluble
Pb(NO3)4
soluble
Ca3(PO4)2
insoluble
CuCl
insoluble
KCH3COO
soluble
PbCO3
BaSO4
insoluble
AgOH
Ag2SO4
insoluble
Cr(OH)3
Predicting Ionic Solubility

Use a solubility chart to predict the solubility of the following
compounds in water. State whether they are soluble or insoluble
in water.
Ca(NO3)2
soluble
CuCl2
soluble
KBr
soluble
(NH4)2CO3
soluble
Fe(NO3)3
soluble
Ca(OH)2
insoluble
NH4CH3COO
soluble
Pb(NO3)4
soluble
Ca3(PO4)2
insoluble
CuCl
insoluble
KCH3COO
soluble
PbCO3
insoluble
BaSO4
insoluble
AgOH
Ag2SO4
insoluble
Cr(OH)3
Predicting Ionic Solubility

Use a solubility chart to predict the solubility of the following
compounds in water. State whether they are soluble or insoluble
in water.
Ca(NO3)2
soluble
CuCl2
soluble
KBr
soluble
(NH4)2CO3
soluble
Fe(NO3)3
soluble
Ca(OH)2
insoluble
NH4CH3COO
soluble
Pb(NO3)4
soluble
Ca3(PO4)2
insoluble
CuCl
insoluble
KCH3COO
soluble
PbCO3
insoluble
BaSO4
insoluble
AgOH
insoluble
Ag2SO4
insoluble
Cr(OH)3
Predicting Ionic Solubility

Use a solubility chart to predict the solubility of the following
compounds in water. State whether they are soluble or insoluble
in water.
Ca(NO3)2
soluble
CuCl2
soluble
KBr
soluble
(NH4)2CO3
soluble
Fe(NO3)3
soluble
Ca(OH)2
insoluble
NH4CH3COO
soluble
Pb(NO3)4
soluble
Ca3(PO4)2
insoluble
CuCl
insoluble
KCH3COO
soluble
PbCO3
insoluble
BaSO4
insoluble
AgOH
insoluble
Ag2SO4
insoluble
Cr(OH)3
insoluble
General Solubility Rules (Time savers)
 Nitrates (NO31-)
soluble with all cations.
 Ammonium (NH41+)
soluble with all anions.
 Alkali Metals (Li1+, Na1+, K1+,…)
soluble with all anions.
Predicting the Precipitate that Forms in a
Chemical Reaction
 For example,
 When a solution of Potassium iodide [KI (aq)] reacts with a
solution of Lead (II) nitrate [Pb(NO3)2 (aq)], a yellow
precipitate forms.
 This reaction can be described in words:
 Potassium iodide solution reacts with Lead (II) nitrate
solution to form Potassium nitrate with Lead (II) iodide.
 One of the products is insoluble (the yellow precipitate)
Predicting the Precipitate that Forms in a
Chemical Reaction
 First Step: Write out the Balanced Chemical Equation:
2KI (aq) + 1Pb(NO3)2(aq)  2KNO3(?) + 1PbI2(?)
 Second step: Determine which product is insoluble:
Name of product
Potassium nitrate
Lead (II) iodide
Formula
Solubility
Predicting the Precipitate that Forms in a
Chemical Reaction
 First Step: Write out the Balanced Reaction Equation:
2KI (aq) + 1Pb(NO3)2(aq)  2KNO3(?) + 1PbI2(?)
 Second step: Determine which product is insoluble:
Name of product
Potassium nitrate
Lead (II) iodide
Formula
KNO3
PbI2
Solubility
Predicting the Precipitate that Forms in a
Chemical Reaction
 First Step: Write out the Balanced Reaction Equation:
2KI (aq) + 1Pb(NO3)2(aq)  2KNO3(?) + 1PbI2(?)
 Second step: Determine which product is insoluble:
Name of product
Potassium nitrate
Lead (II) iodide
Formula
KNO3
PbI2
Solubility
Soluble - ie (aq)
Predicting the Precipitate that Forms in a
Chemical Reaction
 First Step: Write out the Balanced Reaction Equation:
2KI (aq) + 1Pb(NO3)2(aq)  2KNO3(?) + 1PbI2(?)
 Second step: Determine which product is insoluble:
Name of product
Potassium nitrate
Lead (II) iodide
Formula
KNO3
Solubility
Soluble - ie (aq)
PbI2
Insoluble - ie (s)
WRITING TOTAL IONIC EQUATIONS
 The Total Ionic Equation shows all of the ions present in
the two solutions, and which ones form the precipitate.
When writing this equation, you must balance the atoms
and the charges, you must also indicate which species are
(aq) and which, if any forms the precipitate (s).
2K1+(aq) + 2I1-(aq)
WRITING TOTAL IONIC EQUATIONS
 The Total Ionic Equation shows all of the ions present in
the two solutions, and which ones form the precipitate.
When writing this equation, you must balance the atoms
and the charges, you must also indicate which species are
(aq) and which, if any forms the precipitate (s).
2K1+(aq) + 2I1-(aq) + 1Pb2+(aq) + 2NO31- (aq) 
WRITING TOTAL IONIC EQUATIONS
 The Total Ionic Equation shows all of the ions present in
the two solutions, and which ones form the precipitate.
When writing this equation, you must balance the atoms
and the charges, you must also indicate which species are
(aq) and which, if any forms the precipitate (s).
2K1+(aq) + 2I1-(aq) + 1Pb2+(aq) + 2NO31- (aq) 
2K1+(aq) + 2NO31-(aq)
WRITING TOTAL IONIC EQUATIONS
 The Total Ionic Equation shows all of the ions present in the two
solutions, and which ones form the precipitate. When writing this
equation, you must balance the atoms and the charges, you must
also indicate which species are (aq) and which, if any forms the
precipitate (s).
2K1+(aq) + 2I1-(aq) + 1Pb2+(aq) + 2NO31- (aq) 
2K1+(aq) + 2NO31-(aq) + 1PbI2(s)
WRITING NET IONIC EQUATIONS
 The Net Ionic Equation demonstrates only the ions that form the
precipitate. To show the Net Ionic Equation, you get rid of
Spectator Ions – ions that do not take part in the reaction (ie., they
appear the same on the reactant side as they do on the product
side.)
2K1+(aq) + 2I1-(aq) + 1Pb2+(aq) + 2NO31- (aq) 
2K1+(aq) + 2NO31-(aq) + 1PbI2(s)
WRITING NET IONIC EQUATIONS
 The Net Ionic Equation demonstrates only the ions that form the
precipitate. To show the Net Ionic Equation, you get rid of
Spectator Ions – ions that do not take part in the reaction (ie., they
appear the same on the reactant side as they do on the product
side.)
2K1+(aq) + 2I1-(aq) + 1Pb2+(aq) + 2NO31- (aq) 
2K1+(aq) + 2NO31-(aq) + 1PbI2(s)
WRITING NET IONIC EQUATIONS
 The Net Ionic Equation demonstrates only the ions that form the
precipitate. To show the Net Ionic Equation, you get rid of
Spectator Ions – ions that do not take part in the reaction (ie., they
appear the same on the reactant side as they do on the product
side.)
2K1+(aq) + 2I1-(aq) + 1Pb2+(aq) + 2NO31- (aq) 
2K1+(aq) + 2NO31-(aq) + 1PbI2(s)
WRITING NET IONIC EQUATIONS
 The Net Ionic Equation demonstrates only the ions that form the
precipitate. To show the Net Ionic Equation, you get rid of
Spectator Ions – ions that do not take part in the reaction (ie., they
appear the same on the reactant side as they do on the product
side.)
Simplified and rearranged:
1Pb2+(aq) + 2I1-(aq)  1PbI2(s)
SUMMARY – BIG IDEAS
 Some double displacement reactions form precipitates.
 Precipitates form in double displacement reactions between
two ionic solutions.
 Precipitates are insoluble ionic compounds, and do not
dissolve.
 A net ionic equation demonstrates only the ions that react.
Homework
1. Read pg. 331 – 336
2. Do #1 – 3 (Section Questions) on pg. 336 – 337
3. Worksheet: Net Ionic Equations