Solubility Workbook
Period
Worksheets
Quiz

1. Solubility and Saturated Solutions.
WS 1
1

2. Ion Concentration Calculations and Ionic Equations.
WS 2-3
2

3. Solubility to Ksp.
WS 4
3

4. Ksp to Solubilty and Size of Ksp.
WS 5
4

5. Trial Ksp.
WS 6
5

6. Separating Ions
WS 7
6

7. Common Ion Effect and
WS 8
7

8. Titrations and Max Ion Concentration
WS 9
8

9. Review
Web Review Practice Test 1

10. Review
Practice Test 2

11. Test
The following workbook is designed to ensure that you can demonstrate your
understanding of all aspects of the solubility unit. Ask yourself, “do I want to do well in
this class?” If you are determined to be successful the minimum expectation that you
should have for yourself is that you do all of these questions by the due dates given by
your teacher. There are other things that you should do to prepare for the test at the end of
the unit. Remember, what you put into this course is what you will get out. There is no
substitute for consistent effort and hard work. If you can’t do a question, get some help
before the end of the unit, you need to know, understand, and remember everything.
Good luck! I know you can do well in this unit. Keep up the great work!
Worksheet # 1
Solubility and Saturated Solutions
1.
Define and give units for solubility.
2.
Describe the relationship between the rate of dissolving and the rate of
crystallization when a small amount of solute is added to an unsaturated solution.
3.
Describe the relationship between the rate of dissolving and the rate of
crystallization when a small amount of solute is added to a saturated solution.
4.
Describe the relationship between the rate of dissolving and the rate of
crystallization when a small amount of solute is added to a supersaturated
solution.
5.
Which of the above solutions would need to be prepared in order to determine the
solubility of an ionic solution.
6.
2.65 g of Ba(OH)2 is dissolved in 70.0 mL of water to produce a saturated
solution at 20 oC. Calculate the solubility in units of g/100 mL; g/L ; and M.
7.
A beaker containing 100.0 mL of saturated BaCO3 solution weighs 159.60 g. The
beaker is evaporated to dryness and weighs 56.36 g. The empty beaker weighs
24.33 g. Calculate the solubility in units of g/100 mL; g/ L; and M.
8.
9.
Write dissociation equations to represent the equilibrium present for a saturated
solution of each ionic compound. Write the solubility product (Ksp expression)
for each of the equilibrium systems. The first one is done.
a)
Al2(SO4)3
b)
FeCO3
c)
Co2(SO4)3
d)
Na3PO4
2Al3+
⇄
SO42-
+
Ksp = [Al3+]2 [SO42-]3
Write formula, complete ionic, and net ionic equations for each.
a)
H2SO4(aq)
+ 2NaOH(aq) →
Na2SO4 + 2HOH(l)
2H+ + SO42- + 2Na+ + 2OH- → 2Na+ + SO42- + 2HOH(l)
H+ + OH- → HOH(l)
b)
Mg(NO3)2(aq) +
Na2CO3(aq)
→
c)
Al(NO3)3(aq) +
(NH4)3PO4(aq)
→
d)
H3PO4(aq) + Ca(OH)2(aq)
→
Worksheet # 2
Solubility
1.
What is the concentration of each ion in a 10.5 M sodium silicate solution?
2.
What is the concentration of each ion in the solution formed when 94.5 g of
nickel (III) sulphate is dissolved into 850.0 mL of water?
3.
If 3.78 L of 0.960 M sodium fluoride solution is added to 6.36 L of 0.550 M
calcium nitrate solution, what is the resulting concentration of [Ca+2] and [F-]?
4.
What is the concentration of each ion in the solution formed when 94.78 g of
iron (III) sulphate is dissolved into 550.0 mL of water?
5.
If the [F-] = 0.200 M, calculate the number of grams AlF3 that would be
dissolved in 2.00 L of water.
6.
If the [SO42-] = 0.200 M in 2.0 L of Al2(SO4)3, determine the [Al3+] and the
molarity of the solution.
Dissociation Equations Write dissociation equations for any chemicals, which
dissociate when dissolved in water:
1.
HCl (aq)
→
H+
2.
C6H12O6(S)
→
C6H12O6(aq)
3.
Na2S (s)
4.
Al(CH3COO)3 (s)
5.
MgBr2 (s)
6.
Na2CO3 (s)
7.
C12H22O11 (s)
8.
K3PO4 (s)
9.
CH3OH (l)
+
Cl-
ionic compounds dissociate
molecular compounds do not dissociate
Net Ionic Equations
Write chemical equations, total ionic equations and net ionic equations for each reaction.
The first one is done for you. (assume that all reactions occur):
1.
Magnesium metal is placed in hydrochloric acid
Mg (s)
+ 2 HCl (aq)
→
Mg (s) + 2 H+ (aq) + 2 Cl- (aq) →
Mg (s)
+ 2 H+ (aq)
→
MgCl2 (aq)
+
H2 (g)
Mg2+ (aq) + 2Cl- (aq) + H2 (g)
Mg2+ (aq) +
H2 (g)
2.
Zinc metal is placed in silver nitrate solution
3.
Barium chloride solution is added to lead (II) nitrate solution.
4.
Sulphuric acid is added to strontium hydroxide solution.
5.
Sodium carbonate solution is added to nickel (III) nitrate solution.
6.
Aqueous chlorine is added to sodium bromide solution.
7.
Nitric acid is added to strontium hydroxide solution.
Worksheet # 3
1.
Solubility
Classify each as an ionic or molecular (covalent) solution.
NaCl (aq) __________
CoCl2 (aq) _________
CH3OH (aq) ________
NH4OH (aq) ________
NH3 (aq) __________
AgCl (aq) _________
HCl (aq) __________
I2 (aq) ___________
2.
Define each:
a) unsaturated solution:
b) saturated solution:
c) solubility:
3.
Describe how you would prepare a saturated solution.
4.
Describe how you would determine the solubility of NaCl in water at 20oC.
5.
In terms of equilibrium describe the difference between a saturated and
unsaturated solution.
6.
What is the effect of temperature on solubility?
7.
200.0 g of CoCl2 is dissolved in 500.0 mL of water at 0oC to form a saturated
solution. What is the solubility of CoCl2 at 0oC in three different units?
8.
In a saturated solution of CaCl2, a small amount of solid is present. Write a net
ionic equation showing the equilibrium reaction. Write the solubility product (Ksp
expression)
9.
If you were given a saturated, unsaturated and supersaturated solution, how would
you distinguish one from another?
a) Unsaturated solution:
b) Saturated solution:
c) Supersaturated solution:
10.
Write the equilibrium equation and solubility product Ksp for each salt.
The first one is done.
a)
Ca(OH)2 (s) → Ca2+ + 2OHKsp = [Ca2+] [OH-]2
b)
AgCl (s)
c)
Na3PO4 (s)
d)
(NH4)3PO4 (s)
e)
Cu2SO4 (s)
f)
Al(CH3COO)3 (s)
g)
Ca3(PO4)2 (s)
Worksheet # 4
Solubility to Ksp
The Ksp is a measure of the solubility of an ionic salt. The larger the value of the Ksp, the
greater is the solubility of the salt. You can only calculate a Ksp if the solution is
saturated. Only saturated salt solutions are in equilibrium. You can calculate the Ksp from
the solubility of a salt, since the solubility represents the concentration required to
saturate a solution.
1.
Calculate the Ksp for CaCl2 if 200.0g of CaCl2 is required to saturate 100.0 mL of
solution.
2.
Calculate the Ksp for AlCl3 if 100.0g is required to saturate 150.0 mL of a
solution.
3.
The solubility of SrF2 is 2.83 x 10-5 M. Calculate the Ksp.
4.
The solubility of GaBr3 is 15.8 g per 100.0 mL. Calculate the Ksp.
5.
The solubility of Ag2SO4 is 1.33 x 10-7g per 100.0 mL. Calculate the Ksp.
6.
If 2.9 x 10-3 g of Ca(OH)2 is needed to saturate 250.0 mL of solution, what is the
Ksp?
7.
At a certain temperature, a 40.00 mL sample of a saturated solution of barium
hydroxide, is neutralized by 29.10 mL of 0.300 M HCl. Calculate the Ksp of
Ba(OH)2.
Calculate the concentrations of all ions in each solution.
8.
0.50 M Al2(SO4)3(aq)
9.
25.7 g (NH4)3PO4(aq) in 250.0mL H2O.
10.
210. g CoCl2 • 6H2O in 800.0 mL H2O.
Worksheet # 5
Ksp to Solubility
Calculate the solubility in M and g/L for each. Use the Ksp values found in your chart.
1.
BaCO3
2.
Fe(OH)2
3.
PbCl2
4.
How many grams of Mg(OH)2 are required to completely saturate 1.5 L of
solution?
Review
1.
If 200.0 g of MgCl2 is required to saturate 1.5 L of solution at 20 oC, calculate the
Ksp.
2.
If the Ksp for Al2O3 is 2.8 x 10-8, calculate [Al3+] and [O-2] in
Worksheet # 6
mol
/L.
Trial Ksp
1.
Will a precipitate form if 200.0 mL 0.00020M Ca(NO3)2 is mixed 300.0 mL of
0.00030M Na2C03?
2.
Will a precipitate form if 25.0 mL of .0020M Pb(NO3)2 is mixed with 25.0 mL
of 0.040M NaBr.
3.
Will a precipitate form if equal volumes of 0.00020M Ca(NO3)2 is mixed with
0.00030M Na2C03?
4.
Co(OH)2
5.
Ag2C2O4 Solubility = 8.3 x 10-4 M
Solubility = 3.0 x 10-3 g/L Calculate the Ksp at 250 C.
Ksp=?
6.
SrF2
Calculate the solubility in (M).
7.
Cu(IO3)2
Worksheet # 7
chart!!
1.
2.
3.
4.
5.
Solubility Calculate the solubility in (g/L).
Separation Positive Ions: Work from top to bottom of solubility
Ag+
Mg2+ Ba2+
i)
Add:
Filter Out:
Net Ionic equation:
ii)
Add:
Filter Out:
Net Ionic equation:
iii)
Add:
Filter Out:
Net Ionic equation:
Pb2+
Ba2+
i)
Add:
Filter Out:
Net Ionic equation:
ii)
Add:
Filter Out:
Net Ionic equation:
iii)
Add:
Filter Out:
Net Ionic equation:
Cu+
Ca2+
i)
Add:
Filter Out:
Net Ionic equation:
ii)
Add:
Filter Out:
Net Ionic equation:
iii)
Add:
Filter Out:
Net Ionic equation:
Be2+
Sr2+
i)
Add:
Filter Out:
Net Ionic equation:
ii)
Add:
Filter Out:
Net Ionic equation:
iii)
Add:
Filter Out:
Net Ionic equation:
Be2+
Ca2+
i)
Add:
Filter Out:
Net Ionic equation:
ii)
Add:
Filter Out:
Net Ionic equation:
iii)
Add:
Filter Out:
Net Ionic equation:
Sr2+
Sr2+
Ag+
Pb2+
6.
Calculate the Ksp for CaCl2, if 50.0 g is required to saturate 25.0 mL of water.
7.
Calculate the molar solubility of Mg(OH)2.
8.
Will a precipitate form if equal volumes of 0.00020 M Na2CO3 is mixed with
0.00020 M MgCl2.
9.
Write the formula, complete, and net ionic equation.
Formula Equation:
Complete Ionic:
CaCl2(aq) + AgNO3(aq) →
Net Ionic:
Separation of Negative Ions: Work from bottom to top of solubility chart!!
1.
2.
3.
4.
5.
6.
SO32- OH-
I-
i)
Add:
Filter Out:
Net Ionic equation:
ii)
Add:
Filter Out:
Net Ionic equation:
iii)
Add:
Filter Out:
Net Ionic equation:
CO32- OHi)
Add:
Filter Out:
Net Ionic equation:
ii)
Add:
Filter Out:
Net Ionic equation:
Br-
S2-
i)
Add:
Filter Out:
Net Ionic equation:
ii)
Add:
Filter Out:
Net Ionic equation:
iii)
Add:
Filter Out:
Net Ionic equation:
PO43- OH-
PO43-
S2-
i)
Add:
Filter Out:
Net Ionic equation:
ii)
Add:
Filter Out:
Net Ionic equation:
iii)
Add:
Filter Out:
Net Ionic equation:
OH-
S2-
i)
Add:
Filter Out:
Net Ionic equation:
ii)
Add:
Filter Out:
Net Ionic equation:
iii)
Add:
Filter Out:
Net Ionic equation:
S2-
SO42- Cl-
i)
Add:
Filter Out:
Net Ionic equation:
ii)
Add:
Filter Out:
Net Ionic equation:
iii)
Add:
Filter Out:
Net Ionic equation:
SO42-
Common Ion Effect Worksheet # 8
Consider the following equilibrium system.
PbCl2(s) ⇄ Pb2+(aq) + 2 Cl-(aq)
Describe what happens to the solubility of PbCl2 after each of the changes.
1.
2.
3.
4.
5.
PbCl2(s) is added
Pb(NO3)2 is added
NaCl is added
H2O is added
AgNO3 is added
6.
NaBr is added
Consider the following equilibrium system.
AgBr(s) ⇄ Ag+(aq) +
Br-(aq)
Describe what happens to the solubility of AgBr after each of the changes are made.
7.
AgBr(s) is added
8.
Pb(NO3)2 is added
9.
NaCl is added
10.
H2O is added
11.
AgNO3 is added
12.
NaBr is added
13.
Explain why more Zn(OH)2 dissolves when 3 M HCl is added to a saturated
solution of
Zn(OH)2. Start by writing the correct equilibrium equation.
14.
In an experiment, 0.1 M AgNO3 is added to 0.1 M NaCl, resulting in the
formation of a white precipitate. When 0.1 M NaI is added to this mixture, the white
precipitate
dissolves and a yellow precipitate forms.
The formula for the white precipitate is
The formula for the yellow precipitate is
The net ionic equation for the first equilibrium is
The net ionic equation for the formation of the yellow precipitate is
Explain why the white precipitate dissolves. Start by writing the equilibrium
equation for the white precipitate, then, explain how adding NaI affects this
equilibrium.
Titrations and Maximum Ion Concentration
1.
Worksheet # 9
In a titration 25.0 ml of a 0.250 M AgNO3 solution was used to precipitate out all
of the Br- in a 200.0 ml sample. Calculate [Br-].
In a titration 26.5ml of 0.100M Pb(NO3)2 was used to precipitate out all of the Clin a 30.0 ml sample of water. Calculate [Cl-].
Maximum Ion Concentration
2.
3.
Calculate the maximum concentration of OH- that can exist in a 0.200M
Mg(N03)2 solution.
4.
Calculate the maximum concentration of CO3-2 that can exist in a 0.500M AgNO3
solution.
5.
Calculate the maximum concentration of IO3- that can exist in a 0.200M Cu(N03)2
solution.
6.
Calculate the maximum concentration of Ca2+ that can exist in a 0.200 M Na2C03
solution.
7.
Calculate the minimum number of moles of Pb(NO3)2 required to start
precipitation in 50.0 mL of 0.15 M ZnCl2.
8.
In a titration 12.5 mL of 2.00 x 10-5 M HCl is required to neutralize 250.0 mL of
saturated AgOH solution. Calculate the [OH-] and then determine the Ksp for
AgOH.
9.
When excess Ag2CO3(s) is shaken with 1.00 L of 0.200 M K2CO3 it is determined
that 6.00 x 10-6 moles of Ag2CO3 dissolves. Calculate the solubility product of
Ag2CO3.
Quiz #1
1.
To determine the solubility of solute in water, a solution must be prepared that is:
A.
B.
C.
D.
2.
4.
zero
one
two
three
Which one of the following equilibrium systems is described by Ksp?
A.
CaCO3(s) ⇄ CaO(s) + CO2(g)
B.
CaCO3(s) ⇄ Ca2+(aq) + CO32- (aq)
C.
Ca 2+(aq) + CO2-3(aq) ⇄ CaCO3(s)
D.
Ca(OH)2(aq) + H2CO3(aq) ⇄ CaCO3(s) + 2H2O(l)
In a saturated solution, the rate of dissolving is
A.
B.
C.
D.
5.
saturated
unsaturated
concentrated
supersaturated
From the list of salts below, how many are considered soluble at 25oC?
CuCl2
CaSO4
PbS
Ag3PO4
A.
B.
C.
D.
3.
Solubility and Saturated Solutions
equal to zero
equal to the rate of crystallization
less than the rate of crystallization
greater than the rate of crystallization
A soluble magnesium salt is
A.
B.
C.
D.
6.
7.
The equation that represents the equilibrium in a saturated solution of Fe2(SO4)3
is
A.
Fe2(SO4)3(s) ⇄ 3Fe2+(aq) + 2SO43-(aq)
B.
Fe2(SO4)3(s) ⇄ 2Fe2+(aq) + 3SO43-(aq)
C.
Fe2(SO4)3(s) ⇄ 3Fe3+(aq) + 2SO42-(aq)
D.
Fe2(SO4)3(s) ⇄ 2Fe3+(aq) + 3SO42-(aq)
Which one of the following salts is soluble?
A.
B.
C.
D.
8.
9.
BaSO4
CaCO3
K3PO4
Fe(OH)2
The equation representing the equilibrium in a saturated solution of CaSO4 is
A.
CaSO4(s) ⇄ Ca2+(aq) + SO42-(aq)
B.
CaSO4(s) ⇄ Ca2+(aq) + S2-(aq) + 4O2-(aq)
C.
CaSO4(s) + H2O(l) ⇄ CaO(aq) + H2SO4(aq)
D.
CaSO4(s) + 2H2O(l) ⇄ Ca(OH)2(aq) + H2SO4(aq)
Which of the following units is commonly used to describe solubility?
A.
B.
C.
D.
10.
MgSO3
MgCO3
Mg(NO3)2
Mg3(PO4)2
mL/s
g/oC
mol/L
o
C/mol
Which of the following represents the equilibrium in a saturated solution of
Cr2(SO4)3
A.
Cr2(SO4)3(s) ⇄ Cr2+(aq) + SO43-(aq)
B.
Cr2(SO4)3(s) ⇄ Cr3+(aq) + SO42-(aq)
C.
Cr2(SO4)3(s) ⇄ 2Cr2+(aq) + 3SO43-(aq)
D.
Cr2(SO4)3(s) ⇄ 2Cr3+(aq) + 3SO42-(aq)
Quiz #2
1.
A 200.0 mL solution contains 0.050 mol of Ba(NO3)2. The [NO3-] is
A.
B.
C.
D.
2.
5.
Ksp = [Ca2+][PO43-]
Ksp = [Ca2+]3[PO43-]2
Ksp = [3Ca2+][2PO43-]
Ksp = [3Ca2+]3[2PO43-]2
In 1.5 M (NH4)2SO4 , the ion concentrations are
A.
B.
C.
D.
4.
0.050 M
0.10 M
0.25 M
0.50 M
The Ksp expression for a saturated solution of Ca3(PO4)2 is
A.
B.
C.
D.
3.
Ionic Concentrations Calculations & Ionic Equations
[NH4+] = 1.5 M and [SO42-] = 1.5 M
[NH4+] = 1.5 M and [SO42-] = 3.0 M
[NH4+] = 3.0 M and [SO42-] = 1.5 M
[NH4+] = 3.0 M and [SO42-] = 3.0 M
The Ksp expression for Ca3(PO4)2 is
A.
Ksp = [Ca2+]3[PO43-]2
[Ca3(PO4)2]
B.
Ksp = [2Ca2+][3PO43-]
[Ca3(PO4)2]
C.
Ksp = [Ca2+]3[PO43-]2
D.
Ksp = [2Ca2+][3PO43-]
The solubility product expression for a saturated solution of Fe2(SO4)3 is
A.
Ksp = [Fe3+]2[SO42-]3
B.
Ksp = [2Fe3+][3SO42-]
6.
C.
Ksp = [Fe3+]2[SO42-]3
[Fe2(SO4)3]
D.
Ksp = [2Fe3+][3SO42-]
[Fe2(SO4)3]
Molecular solutions do not conduct electricity because they contain
A.
B.
C.
D.
7.
If equal volumes of 0.2 M KBr and 0.2M FeSO4 are mixed, then
A.
B.
C.
D.
8.
A precipitate does not form
A precipitate of ZnS forms
A precipitate of MgSO4 forms
Precipitates of MgSO4 and ZnS form
In an experiment, 0.500 mol of Fe(NO3)3 is dissolved in water to produce a 2.00 L
solution. The [NO3-] in this solution is
A.
B.
C.
D.
10.
No precipitate will be observed
A precipitate of FeBr2 will be observed
A precipitate of K2SO4 will be observed
A precipitate of both K2SO4 and FeBr2 will be observed
Which of the following occurs when equal volumes of 0.20 M MgS and 0.20 M
ZnSO4 are mixed?
A.
B.
C.
D.
9.
Molecules only
Cations and anions
Molecules and anions
Molecules and cations
0.250 M
0.500 M
0.750 M
1.50 M
The complete ionic equation for the reaction between MgCl2(aq) and AgNO3(Aq) is
A.
B.
C.
D.
Ag+(aq) + Cl-(aq) → AgCl(s)
2AgNO3(aq) + MgCl2(aq) → 2AgCl(s) + Mg(NO3)2(aq)
2Ag+(aq) + Mg2+(aq) + 2NO3- (aq) + 2Cl-(aq) → MgCl2(s) + 2Ag+(aq) + 2NO3- (aq)
2Ag+(aq) + 2NO3- (aq) + Mg2+(aq) + 2Cl-(aq) → 2AgCl(s) + Mg2+(aq)+ 2NO3- (aq)
11.
Which one of the following would form an ionic solution when dissolved in
water?
A.
B.
C.
D.
12.
If the solubility of Pb (OH) 2 is 0.155g/L, then the concentration of each ion in a
saturated solution of a Pb (OH) 2 is
A.
B.
C.
D.
13.
14.
[Pb2+] = 0.155 g/L and [OH-] = 0.155g/L
[Pb2+] = 0.052 g/L and [OH-] = 0.103g/L
[Pb2+] = 6.43 x 10-4 M and [OH-] = 1.29 x 10-3 M
[Pb2+] = 6.43 x 10-4 M and [OH-] = 6.43 x 10-4 M
The Ksp expression for calcium hydroxide is
A.
Ksp = [Ca2+][OH-]2
B.
Ksp =
C.
Ksp = [Ca2+][2OH-]2
D.
Ksp =
1
[Ca2+][OH-]2
1
[Ca2+][2OH-]2
A precipitation reaction occurs when equal volumes of 0.2 M Pb(NO3)2 and 0.2 M
KI are mixed. The net ionic equation for this reaction is
A.
B.
C.
D.
15.
I2
CH3OH
Ca(NO3)2
Cl2H22O11
Pb2+(aq) + 2I-(aq) → PbI2(s)
PbI2(s) → Pb2+(aq) + 2I-(aq)
K+(aq) + NO3-(aq) → KNO3(s)
KNO3(s) → K+(aq) + NO3-(aq)
When dissolved in water, which of the following is an ionic solution?
A.
B.
C.
O2
CH4
CaCl2
D.
16.
In a 200.0 mL sample of 0.030 M Na3PO4, the [Na+] is
A.
B.
C.
D.
Quiz #3
1.
Solubility to Ksp
9.1 x 10-14
3.6 x 10-13
2.0 x 10-9
4.1 x 10-9
The solubility of manganese (II) sulphide is 1.7 x 10-7 M at 25oC. The solubility
product constant is
A.
B.
C.
D.
3.
0.006 M
0.010 M
0.018 M
0.090 M
In a saturated solution of manganese (II) hydroxide, Mn(OH)2, and [Mn2+] equals
4.5 x 10-5 M. therefore, the Ksp of Mn(OH)2 is
A.
B.
C.
D.
2.
C12H22O11
2.9 x 10-14
1.7 x 10-7
3.4 x 10-7
4.1 x 10-4
The compound Ag2S has a solubility of 1.3 x 10-4 moles per litre at 25oC. The Ksp
for this compound is
A.
B.
C.
D.
2.2 x 10-12
8.8 x 10-12
1.7 x 10-8
3.4 x 10-8
4.
The solubility of barium oxalate, BaC2O4, is 4.8 x 10-4 M. The value of Ksp is
5.
A.
2.3 x 10-7
B.
4.8 x 10-4
C.
2.4 x 10-4
D.
2.2 x 10-2
The solubility of MnS is 4.8 x 10-7 M, at 25oC. The Ksp value is
A.
B.
C.
2.3 x 10-13
4.8 x 10-7
9.6 x 10-7
D.
6.
At 25oC, the solubility of an unknown compound is 7.1 x 10-5 M. the compound is
A.
B.
C.
D.
7.
CuI
AgI
CaCO3
CaSO4
The solubility of barium fluoride is 3.6 x 10-3 M. the solubility product constant is
A.
B.
C.
D.
8.
6.9 x 10-4
4.7 x 10-8
1.9 x 10-7
1.3 x 10-5
2.6 x 10-5
At a certain temperature, the solubility of BaF2 is 7.4 x 10-3 moles per litre. The
Ksp of BaF2 is
A.
B.
C.
D.
1.6 x 10-6
5.5 x 10-5
1.1 x 10-4
7.4 x 10-3
Quiz #4
1.
Identify the most soluble sulphide
A.
B.
C.
D.
2.
HgS,
PbS,
FeS,
MnS,
Ksp = 1.6 x 10-54
Ksp = 7.0 x 10-29
Ksp = 3.7 x 10-19
Ksp = 2.3 x 10-13
Saturated solutions of Na2S, CuS, SnS2, and Al2S3 are prepared at 25oC. The [S2-]
will be greatest in the solution of
A.
B.
C.
D.
3.
Ksp to Solubility and Size of Ksp
Na2S
CuS
SnS2
Al2S3
A solution of AgNO3 is slowly added to a mixture containing 0.10 M I-, Cl-, Br-,
and IO3-. The precipitate, which forms first, is
A.
AgI
B.
C.
D.
4.
The [OH-] is measured to be 3.3 x 10-3 mol/L in a 100.0 mL sample of saturated
solution of Al(OH)3. The solubility of Al(OH)3 is
A.
B.
C.
D.
5.
2.8 x 10-9 M
5.3 x 10-5 M
1.1 x 10-4 M
7.3 x 10-3 M
At 25oC, the solubility of Mg (OH)2 is
A.
B.
C.
D.
9.
BaS
AlCl3
CaSO3
ZnSO4
The solubility of AgBrO3 is
A.
B.
C.
D.
8.
1.2 x 10-16 M
5.5 x 10-9 M
1.1 x 10-8 M
1.0 x 10-4 M
The least soluble in salt water is
A.
B.
C.
D.
7.
1.1 x 10-4 mol/L
3.3 x 10-4 mol/L
1.1 x 10-3 mol/L
3.3 x 10-3 mol/L
The [SO24-] in a saturated solution of PbSO4 is (Ksp = 1.1 x 10-8)
A.
B.
C.
D.
6.
AgCl
AgBr
AgIO3
1.1 x 10-32 M
5.6 x 10-12 M
2.4 x 10-6 M
1.1 x 10-4 M
A student evaporated 200.0 mL of a saturated solution of SrCrO4 to dryness. The
residue contained 1.2 x 10-3 mol SrCrO4. The solubility of SrCrO4 is
A.
B.
1.4 x 10-6 M
3.6 x 10-5 M
C.
D.
10.
The solubility of magnesium carbonate is
A.
B.
C.
D.
11.
CaCO3
BaSO4
CuSO4
MgSO4
Which of the following salts has the lowest solubility?
A.
B.
C.
D.
Quiz #5
1.
9.3 x 10-5 M
3.7 x 10-4 M
4.4 x 10-2 M
1.4 x 10-7 M
Which of the following is the least soluble in water at 25oC ?
A.
B.
C.
D.
13.
9.3 x 10-5 M
3.4 x 10-6 M
6.8 x 10-6 M
2.6 x 10-3 M
A saturated container of NiCO3 was evaporated to dryness. A 250.0 mL sample
was found to contain 1.1 x 10-2 g NiCO3. The molecular mass of NiCO3 is 118.7
g/mol. The molar solubility of NiCO3 is
A.
B.
C.
D.
12.
2.4 x 10-4 M
6.0 x 10-3 M
Copper (I) chloride
Ammonium sulphide
Potassium hydroxide
Mercury (II) sulphate
Trial Ksp
In an experiment, a student mixes equal volumes of 0.0020 M Pb2+ ions with
0.0040 M I- ions. The trial ion product is
A.
B.
C.
D.
2.
In an experiment, 20.0 ml of 0.0060 M CaCl2 and 20.0 mL of 0.0050 M NaSO4 are
mixed together. The trial ion product (trial Ksp) is
A.
B.
C.
D.
3.
No precipitate forms
A precipitate of only SrS forms
A precipitate of only NaOH forms
Precipitates of both NaOH and SrS form
When solutions of Pb(NO3)2 and NaCl are mixed, the trial ion product (Trial Ksp)
is 9.8 x 10-6. Which of the following statements is true?
A.
B.
C.
D.
7.
AlCl3 precipitates
CaSO4 precipitates
AlCl3 and CaSO4 precipitate
no precipitate forms
When a student mixes equal volumes of 0.20 M Na2S and 0.20 M Sr(OH)2.
A.
B.
C.
D.
6.
Less than 0.10 M
More than 10.0 M
More than 0.10 M but less than 1.0 M
More than 1.0M but less than 10.0 M
When 0.20 M Al2(SO4)3 is added to an equal volume of 0.20 M CaCl2,
A.
B.
C.
D.
5.
7.5 x 10-6 and a precipitate will form
7.5 x 10-6 and a precipitate will not form
3.0 x 10-5 and a precipitate will form
3.0 x 10-5 and a precipitate will not form
In a saturated solution of Zn(OH)2, the [Zn2+] is
A.
B.
C.
D.
4.
4.0 x 10-9
3.2 x 10-8
1.3 x 10-7
8.0 x 10-6
A precipitate forms because Ksp > 9.8 x 10-6
A precipitate forms because Ksp < 9.8 x 10-6
A precipitate does not form because Ksp < 9.8 x 10-6
A precipitate does not form because Ksp > 9.8 x 10-6
When equal volumes of 0.060 M AgNO3 and 0.00090 M NaBrO3 are mixed, the
trial ion product (TIP) is
A.
Less than Ksp and a precipitate forms
B.
C.
D.
8.
The mixture that could produce a precipitate of two compounds is
A.
B.
C.
D.
9.
SrS
SrCl2
SrSO4
Sr(OH)2
When equal volumes of 2.0 M Pb(NO3)2 and 2.0 M KCl are mixed
A.
B.
C.
D.
Quiz #6
1.
0.2 M HgSO4 and 0.2 M FeCl2
0.2 M AgNO3 and 0.2 MgCl2
0.2 M K2CO3 and 0.2 CuSO4
0.2 M ZnSO4 and 0.2 Ba(OH)2
Which of the following has a solubility of less than 0.10 M?
A.
B.
C.
D.
10.
Greater than Ksp and a precipitate forms
Less than Ksp and no precipitate forms
Greater than Ksp and no precipitate forms
A precipitate forms because trial ion product < Ksp
A precipitate forms because trial ion product > Ksp
A precipitate does not form because trial ion product < Ksp
A precipitate does not form because trial ion product > Ksp
Separating Ions
During a lab on qualitative analysis, an unknown solution containing one cation
was analyzed and the following data were collected:
0.2 M Anions Added to
the Unknown Solution
S2SO42OHCO32-
Observation
no precipitate
precipitate
precipitate
precipitate
Which one of the following cations is found in the unknown solution?
A.
B.
C.
D.
2.
Which of the following could be used to precipitate both Mg2+ and Ca2+ from hard
water?
A.
B.
C.
D.
3.
KNO3
AgNO3
Pb(NO3)2
Al(NO3)3
The precipitate formed when equal volumes of 0.2 M Sr(OH)2 and 0.2 M MgS are
mixed is
A.
B.
C.
D.
5.
Lithium sulphate
Sodium phosphate
Potassium sulphide
Ammonium chloride
A reagent that may be used to separate Cl- from S2- by precipitation is
A.
B.
C.
D.
4.
Mg2+
Be2+
Sr2+
Ba2+
SrS
Mg(OH)2
a mixture of Mg(OH)2 and SrS
a mixture of Sr(OH)2 and MgS
Which of the following ions could be used to separate Cl-(aq) from SO42-(aq) by
precipitation?
A.
B.
Ag+
Ca2+
C.
D.
6.
Which of the following ions could be added to an aqueous mixture containing
Pb2+ and Ba2+ to separate the ions by precipitating one of them?
A.
B.
C.
D.
7.
INO3PO43SO42-
Which of the following would precipitate the Ca2+ and Mg2+ found in hard water?
A.
B.
C.
D.
8.
NH4+
Pb2+
S2PO43SO42CH3COO-
A solution containing an unknown cation was added to three solutions and the f
following observations were recorded:
SOLUTION
NaI
Na2SO4
NaOH
OBSERVATION
no precipitate
precipitate
no precipitate
The unknown cation is
A.
B.
C.
D.
9.
To remove Mg2+ from a solution by precipitation, a student should add
A.
B.
C.
D.
10.
Pb2+
Sr2+
Ca2+
Ag+
NaI
KOH
Li2SO4
(NH4)2S
Which of the following could be used to separate Pb2+ from Ba2+ by precipitation?
A.
B.
C.
Na2S
NaOH
Na2CO3
D.
11.
A student wishes to identify an unknown cation in a solution. A precipitate does
not form with the addition of SO42-, but does form with the addition of S2-. Which
of the following is the unknown cation?
A.
B.
C.
D.
12.
Ag+
Mg2+
Ca2+
Cu2+
A solution contains CO32- and OH-. Separation of these two anions by selective
precipitation is accomplished by first adding Sr(NO3)2 solution, then filtering and
finally adding to the filtrate a solution of
A.
B.
C.
D.
13.
Na3PO4
HNO3
RbNO3
NH4NO3
Zn(NO3)2
A nitrate solution containing an unknown cation is added to each of the following
three test tubes.
1.0 M NaOH
1.0 M Na2S
1.0 M Na2SO4
A precipitate forms in one test tube only. The unknown cation is
A.
B.
C.
D.
Ag+
Ca2+
Sr2+
NH4+
14.
A solution containing a single unknown cation is added to three test tubes. the
following anions were added and observations were recorded.
TEST TUBE
1
2
3
ANION ADDED
SO42S2OH-
OBSERVATION
precipitate
precipitate
precipitate
The solution contains
A.
B.
C.
D.
Sr2+
Ag+ or Pb2+
Ca2+ or Ba2+
K+, NH4+ or H+
Quiz #7
1.
Common Ion Effect
Consider the following equilibrium: CaCO3(s) ⇄ Ca2+(aq) + CO32-(aq)
Which of the following reagents, when added to the equilibrium system, would
cause more CaCO3 to dissolve?
A.
B.
C.
D.
2.
A solution contains a mixture of SO42- and S2-. Which of the following cations
could be used to remove only the SO42- from the solution by precipitation?
A.
B.
C.
D.
3.
KNO3(s)
CaCO3(s)
H2C2O4(s)
Na2CO3(s)
K+
Sr2+
Pb2+
Cu2+
Consider the following solubility equilibrium: MgCO3(s)⇄ Mg2+(aq) + CO32-(aq)
The addition of which of the following substances would decrease the solubility
of MgCO3?
A.
B.
C.
H2O
NaCl
NaOH
4.
D.
Na2CO3
A student could precipitate silver chloride from a saturated solution of silver
chloride by adding
A.
B.
C.
D.
5.
The greatest mass of solid SnS will dissolve in 1.0 L of
A.
B.
C.
D.
6.
[I-] increases and [Pb2+] increases
[I-] decreases and [Pb2+] decreases
[I-] increases and [Pb2+] decreases
[I-] decreases and [Pb2+] increases
Consider the following equilibrium: Pbl2(s) + heat ⇄ Pb2+(aq) + 2I-(aq)
Which of the following changes would result in more Pbl2 dissolving?
A.
B.
C.
D.
9.
MgCl2
NaNO3
Na2CO3
Mg(NO3)2
Sodium iodide is added to a saturated solution of lead (II) iodide. The net change
is
A.
B.
C.
D.
8.
H2O
0.10 M MgS
0.10 M (NH4)2S
0.10 M Sn(NO3)2
Magnesium carbonate would be the most soluble in a solution of
A.
B.
C.
D.
7.
Water
Sodium iodide
Sodium nitrate
Sodium chloride
Adding more Pbl2
Increasing the pressure
Adding some Pb(NO3)2
Increasing the temperature
Consider the following equilibrium: AgCl(s) ⇄ Ag+(aq) + Cl-(aq)
Sodium chloride is added to a saturated solution of AgCl. The amount of solid
AgCl will
A.
B.
Increase as the equilibrium shifts to the left
Decrease as the equilibrium shifts to the left
C.
D.
10.
Consider the following equilibrium: NH4Cl(s) + energy ⇄ NH+4(aq) + Cl-(aq)
Which of the following will increase the solubility of ammonium chloride?
A.
B.
C.
D.
Quiz #8
1.
1.1 x 10-5 M
5.3 x 10-5 M
2.6 x 10-4 M
7.3 x 10-3 M
3.4 x 10-7M
3.4 x 10-6 M
1.7 x 10-6 M
5.8 x 10-4 M
A student titrates a 25.00 mL sample of well water with 18.2 mL 0.100 M AgNO3
to completely precipitate the chloride ion. The [Cl-] is
A.
B.
C.
D.
4.
Titrations and Max Ion Concentration
What is the maximum [Sr2+] that can exist in a solution of 0.10 M Na2SO4?
A.
B.
C.
D.
3.
Stirring the solution
Adding more water
Adding more NH4Cl(s)
Increasing the temperature
What is the maximum [Ag+] that can exist in 0.20 M NaBrO3?
A.
B.
C.
D.
2.
Increase as the equilibrium shifts to the right
Decrease as the equilibrium shifts to the right
1.82 x 10-3 M
7.28 x 10-2 M
1.37 x 10-1 M
1.50 x 10-1 M
What is the maximum concentration of sodium sulphate, Na2SO4, that will
dissolve in 1.0 L of 0.10 M Pb(NO3)2 without forming a precipitate?
A.
B.
C.
D.
1.8 x 10-8 M
1.8 x 10-7 M
1.3 x 10-4 M
1.0 x 10-1 M
5.
Consider the following equilibrium: AgCl(s) ⇄ Ag+(aq) + Cl-(aq)
When Br-(aq) is added to a saturated solution of AgCl,
A.
B.
C.
D.
6.
In a saturated solution of zinc hydroxide, at 40oC, the [Zn2+] = 1.8 x 10-5 M.
The Ksp of Zn(OH)2 is
A.
B.
C.
D.
7.
1 M HCl
1 M MgCl2
1 M AgNO3
1 M NH4NO3
At 25oC, the maximum [Zn2+] that can exist in a 0.250 M Na2S is
A.
B.
C.
D.
10.
[Co2+] = 3.5 M and [Cl-] = 3.5 M
[Co2+] = 3.5 M and [Cl-] = 7.0 M
[Co2+] = 0.35 M and [Cl-] = 0.35 M
[Co2+] = 0.35 M and [Cl-] = 0.70 M
In which of the following would solid AgCl be most soluble?
A.
B.
C.
D.
9.
5.8 x 10-15
2.3 x 10-14
1.8 x 10-14
6.5 x 10-10
What is the [Co2+] and [Cl-] when 0.35 mol of CoCl2 is dissolved in enough water
to make 100.0 mL of solution?
A.
B.
C.
D.
8.
More AgCl dissolves and its solubility product increases
More AgCl precipitates and its solubility product decreases
More AgCl dissolves and its solubility product remains constant
More AgCl precipitates and its solubility product remains constant
5.0 x 10-26
2.0 x 10-25
8.0 x 10-25
4.5 x 10-13
The molar solubility of iron (II) sulphide is
A.
B.
C.
D.
3.6 x 10-37
3.0 x 10-19
6.0 x 10-19
7.7 x 10-10
Solubility Web Review
1.
Describe the relationship between the rate of dissolving solid and rate of
crystallization:
a)
A saturated solution and some solid
b)
An unsaturated solution and some solid
c)
A supersaturated solution and some solid is added
2.
Write the equilibrium expression and Ksp equation for Fe2O3.
3.
Write the net ionic equation for the reaction between Al(NO3)3 and Na2CO3. Note
the difference between this equation and the last one.
4.
Mg+2, Sr+2, Ca+2 and Be+2 are possibly in a solution. The solution reacts with
Na2SO4 but not NaOH or Na2S. What cations are in the solution?
5.
A solution contains SO42- or OH- or both. It reacts with Zn(NO3)2and Sr(NO3)2,
What anions are in the solution?
6.
Ag2CO3(s) ⇄ 2Ag+ + CO32- Describe the effect on the solubility of Ag2CO3 for
each change below:
a)
Add Ag2CO3
b)
Add water
c)
Add NaCl
d)
Add Pb(NO3)2
e)
Add Na2CO3
f)
Add AgNO3.
7.
If the trial Ksp = 1.7x10-7 and the Ksp = 3.8x10-7 will a precipitate occur?
8.
For a saturated solution of Fe(OH)3 the [OH-] is found to be 1.3x10-4 M. Calculate
the [Fe+3] and the solubility of the salt in moles/L.
9.
Consider the equilibrium that exists in a saturated solution of PbCl2. Write the
equilibrium expression. If the equilibrium shifts to the right, what affect does this
have on the solubility? Describe how the addition of each of the following will
affect the solubility of PbCl2.
a)
AgNO3
b)
NaCl
c)
Na2S
d)
H2O
10.
e)
NaNO3
f)
Pb(NO3)2
If the reaction is endothermic, how do the Ksp and the solubility change if the
temperature is increased? What is the only way to change the Ksp?
Calculations
1.
In a titration 250 mL of a .200 M AgNO3 solution was used to precipitate out all
of the Cl- in a 500 mL sample. Calculate [Cl-].
2.
In a titration 26.5 mL of .100M Pb(NO3)2 was used to precipitate out all of the Iin a 3.00 mL sample of water. Calculate [I-].
3.
Co(OH)2 Solubility = 3.0x10-3 g/L
Ksp=?
4.
Ag2C2O4 Solubility = 8.3x10-4 M
Ksp=?
5.
SrF2 Ksp = 2.8 x 10-9
Solubility in (M) = ?
Ksp = 1.4 x 10-7
6.
Cu(IO3)2
Solubility (g/L) = ?
7.
Calculate the maximum concentration of OH- that can exist in a 0.200M Ca(N03)2
solution. Ksp (Ca(OH)2) = 2.8 x 10-8
8.
Calculate the maximum concentration of CO3-2 that can exist in a 0.500 M
Fe(NO3)3 solution. Ksp (Fe2(CO3)3) = 2.8 x 10-14
9.
Will a precipitate form if 200.0 mL .0020M Mg(NO3)2 is mixed 300.0 mL of
0.0030M NaOH?
10.
Will a precipitate form if 25.0mL of .0020M Pb(NO3)2 is mixed with 25.0mL of
0.040M NaBr.
11.
20.0 g of PbCl2 is placed in 2.0 L of water. Some but not all dissolves to form a
saturated solution. How many grams do not dissolve?
Solubility Practice Test # 1
1.
Which combination of factors will affect the rate of the following reaction?
Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)
A.
B.
C.
D.
2.
Temperature and surface area only
Temperature and concentration only
Concentration and surface area only
Temperature, concentration, and surface area
Consider the following reaction:
2MnO4-(aq) + 5C2O42- + 16H+(aq) → 2Mn2+(aq) + 10CO2(g) + 8H2O(l)
The rate of decomposition of the oxalate ion is increased by
A.
B.
C.
D.
Adding NaOH
Removing CO2
Adding a catalyst
Decreasing the pressure
3.
An equilibrium system shifts left when the temperature is increased. The forward
rate is
A.
Exothermic and ∆H is positive.
B.
Exothermic and ∆H is negative.
C.
Endothermic and ∆H is positive.
D.
Endothermic and ∆H is negative.
4.
The value of the Keq can be changed by
A.
B.
C.
D.
5.
adding a catalyst.
changing the temperature.
changing the reactant concentration.
changing the volume of the container
Consider the following equilibrium: 2NOCl(g) ⇄ 2NO(g) + Cl2(g)
In a 1.0 L container at equilibrium there are 1.0 mol NOCl, 0.70 mol NO and 0.40
mol Cl2. At constant temperature and volume, 0.10 mol NOCl is added. The
concentrations in the “new” equilibrium in comparison to the concentrations in
the “old” equilibrium are
[NOCl]
[NO]
[Cl2]
A
B
C
D
6.
7.
A.
Fe2(SO4)3(s) ⇄ 3Fe2+(aq) + 2SO43-(aq)
B.
Fe2(SO4)3(s) ⇄ 2Fe2+(aq) + 3SO43-(aq)
C.
Fe2(SO4)3(s) ⇄ 3Fe3+(aq) + 2SO42-(aq)
D.
Fe2(SO4)3(s) ⇄ 2Fe3+(aq) + 3SO42-(aq)
KOH
Fe(OH)3
Mg(OH)2
Zn(OH)2
When 250 mL of 0.36 M Sr(OH)2 are added to 750 mL of water, the resulting ion
concentrations are
[Sr2+]
[Sr2+]
[Sr2+]
[Sr2+]
= 0.12 M and [OH-]
= 0.12 M and [OH-]
= 0.090 M and [OH-]
= 0.090 M and [OH-]
=
=
=
=
0.12 M
0.24 M
0.090 M
0.180 M
When equal volumes of 2.0 M Pb(NO3)2 and 2.0 M KCl are mixed,
A.
B.
C.
D.
11.
K+(aq) + NO3-(aq) → KNO3(s)
2Ag+(aq) + CrO42-(aq) → Ag2CrO4(s)
K2CrO4(aq) + 2AgNO3(aq) → Ag2CrO4(s) + 2KNO3(aq)
2Ag+(aq) + CrO4-(aq) + 2K+(aq) + 2NO3-(aq) → Ag2CrO4(s) + 2KNO3(s)
Which of the following compounds could be used to prepare a 0.20 M solution of
hydroxide ion?
A.
B.
C.
D.
10.
new = old
new > old
new > old
new > old
When equal volumes of 0.20 M K2CrO4 and 0.20 M AgNO3 are mixed, a red
precipitate is formed. The net ionic equation for this reaction is
A.
B.
C.
D.
9.
new = old
new > old
new < old
new > old
The equation that represents the equilibrium in a saturated solution of Fe2(SO4)3 is
A.
B.
C.
D.
8.
new = old
new > old
new < old
new < old
a precipitate forms because the trial ion product < Ksp
a precipitate forms because the trial ion product > Ksp
a precipitate does not form because the trial ion product < Ksp
a precipitate does not form because the trial ion product > Ksp
Consider the following equilibrium: AgCl(s) ⇄ Ag+(aq) + Cl-(aq)
When Br-(aq) is added to a saturated solution of AgCl,
A.
B.
C.
D.
more AgCl dissolves and its solubility product increases.
more AgCl precipitates and its solubility product decreases.
more AgCl dissolves and its solubility product remains constant.
more AgCl precipitates and its solubility product remains constant.
12.
The molar solubility of iron II sulphide is
A.
B.
C.
D.
13.
3.6
3.0
6.0
7.7
x
x
x
x
10-37 M
10-19 M
10-19 M
10-10 M
A solution containing an unknown cation was added to three solutions and the
following observations were recorded:
Solution
NaI
Observation
no precipitate
The unknown cation is
A.
B.
C.
D.
14.
[Pb2+]
[Pb2+]
[Pb2+]
[Pb2+]
=
=
=
=
0.155 g/L and [OH-] = 0.155 g/L
0.155 g/L and [OH-] = 0.103 g/L
6.43 x 10-4 M and [OH-] = 1.29 x 10-3 M
6.43 x 10-4 M and [OH-] = 6.43 x 10-3 M
Na2S
NaOH
Na2CO3
Na2SO4
When dissolved in water, which of the following form a molecular solution?
A.
B.
C.
D.
17.
Pb2+
Sr2+
Ca2+
Ag+
Which of the following could be used to separate Pb2+ from Ba2+ by precipitation?
A.
B.
C.
D.
16.
NaOH
no precipitate
If the solubility of Pb(OH)2 is 0.155 g/L, then the concentration of each ion in a
saturated solution is
A.
B.
C.
D.
15.
Na2SO4
precipitate
HCl(g)
NaNO3(s)
CH3OH(l)
K2SO4(s)
Which of the following will be most soluble in water at 25 oC.
A.
AgI
B.
PbS
C.
MgSO4
D.
Ba(OH)2
18.
At 25 oC, the solubility of Mg(OH)2 is
A.
B.
C.
D.
19.
increasing
decreasing
increasing
no change
8.4 x 10-28
2.9 x 10-14
5.8 x 10-14
1.7 x 10-7
Which of the following causes a precipitate to form when Sr2+(aq) is added but not
when Zn2+(aq) is added?
A.
B.
C.
D.
23.
increasing
increasing
decreasing
increasing
The solubility of PbS is 2.9 x 10-14 M. What is the value of the Ksp.
A.
B.
C.
D.
22.
CuI
AgI
CaCO3
CaSO4
When solid AgBr is added to a saturated solution of AgBr, the reaction rates can
be described as:
Rate of Dissolving
Rate of Crystalizing
A.
B.
C.
D.
21.
x 10-32 M
x 10-12 M
x 10-6 M
x 10-4 M
At 25 oC, the solubility of an unknown compound is 7.1 x 10-5 M. The compound
is
A.
B.
C.
D.
20.
1.1
1.1
1.1
1.1
S2ClSO42CO32-
A 3.0 L solution of NiCl2 is found to have a chloride concentration of 0.60 M.
The concentration of nickel II ions is
A.
B.
C.
D.
0.30 M
0.60 M
0.90 M
1.2 M
24.
When equal volumes of 0.20 M K2CO3 and 0.2 M Na3PO4 are mixed,
A.
B.
C.
D.
25.
A solution of AgNO3 is slowly added to a mixture containing 0.10 M I-, Cl-, Br-,
and IO3-. The precipitate which forms first is
A.
B.
C.
D.
26.
no precipitate will form
a precipitate of K3PO4 will form
a precipitate of Na2CO3 will form
a precipitate of K3PO4 and Na2CO3 will form
AgI
AgCl
AgBr
AgIO3
Which of the following units can be used to represent solubility?
A.
B.
C.
D.
g
mol
mol/L
mL/s
27.
Consider the following equilibrium: CaCO3(s) ⇄ Ca2+(aq) + CO32-(aq)
Which of the following reagents when added to the equilibrium system, would
cause more CaCO3 to dissolve?
A.
KNO3(s)
B.
CaCO3(s)
C.
H2C2O4(s)
D.
Na2CO3(s)
28.
Which of the following could be used to precipitate both Mg2+ and Ca2+ from hard
water?
A.
B.
C.
D.
29.
lithium sulphate
sodium phosphate
potassium sulphide
ammonium chloride
What is the maximum [Ag+] that can exist in 0.20 M NaBrO3?
A.
B.
C.
D.
1.1 x 10-5 M
5.3 x 10-5 M
2.6 x 10-4 M
7.3 x 10-3 M
30.
Which of the following ions could be used to separate Cl-(aq) from SO42-(aq) by
precipitation?
A.
B.
C.
D.
31.
The Ksp expression for a saturated solution Ca3(PO4)2 is
A.
B.
C.
D.
32.
35.
=
=
=
=
[Ca2+][PO43-]
[Ca2+]3[PO43-]2
[3Ca2+][2PO43-]
[3Ca2+][2PO43-]
solution will be saturated
pH will be less than 7
trial Ksp is less than the Ksp
concentrations of the ions are equal
Which of the following describes the changes in ion concentrations when 1.0 g of
solid ZnS is added to a saturated solution of ZnS?
A.
B.
C.
D.
34.
Ksp
Ksp
Ksp
Ksp
When Ca(OH)2 attains solubility equilibrium, the
A.
B.
C.
D.
33.
Ag+
Ca2+
NH4+
Pb2+
[Zn2+]
[S2-]
increases
decreases
increases
remains constant
decreases
decreases
increases
remains constant
The net ionic equation for the reaction between Sr(OH)2 and H2SO4 is
A.
B.
C.
H+ + OH- → H2O
Sr2+ + SO42- → SrSO4
Sr(OH)2 + H2SO4 → SrSO4 + 2H2O
D.
Sr2+ + 2OH- + 2H+ + SO42- → SrSO4 + 2H2O
The relationship between the solubility and the size of the Ksp is
A.
B.
C.
there is no relationship
the smaller the Ksp the greater the solubility
the greater the Ksp the greater the solubility
36.
D.
the solubility is always the square root of the Ksp
Which of the following compounds will form a saturated solution with the
greatest concentration of Ag+?
A.
B.
C.
D.
37.
When equal volumes of 0.20 M CuSO4 and 0.20 M Li2S are combined, the
complete ionic equation is
A.
B.
C.
D.
38.
S2-(aq) → CuS(s)
+ Li2S(aq) → CuS(s) + Li2SO4(aq)
SO42-(aq) + 2Li+(aq) + S2-(aq) → CuS(s) + Li2SO4(aq)
SO42-(aq) + 2Li+(aq) + S2-(aq) → CuS(s) + 2Li+(aq) + SO42-(aq)
0.40 L of 0.050 M Fe(NO3)3
0.80 L of 0.020 M Fe2(SO4)3
0.50 L of 0.040 M FeC6H5O7
0.50 L of 0.010 M Fe2(C2O4)3
A solution contains both Ag+ and Mg2+ ions. During selective precipitation, these
ions are removed one at a time by adding
A.
B.
C.
D.
40.
Cu2+(aq) +
CuSO4(aq)
Cu2+(aq) +
Cu2+(aq) +
Which of the following would have the [Fe3+] = 0.020 M?
A.
B.
C.
D.
39.
AgI
AgBr
AgIO3
AgBrO3
I- followed by OHOH- followed by S2SO42- followed by ClNO3- followed by PO43-
The solubility of an AB2 type salt is 2.3 x 10-6 M. The salt is
A.
B.
C.
D.
PbBr2
Fe(OH)2
Cu(IO3)2
Mg(OH)2
1.
A saturated solution of BaSO4 is given to patients needing digestive tract x-rays.
a)
Write an equation that represents the solubility equilibrium
b)
Calculate the [Ba2+] present in the saturated solution.
2.
Will a precipitate form when 90.0 mL of 1.00 x 10-2 M Cu(NO3)2 and 10.0 mL of
1.00 x 10-2 M NaIO3 are mixed? Explain using appropriate calculations.
3.
What is the maximum [CO32-] that can exist in a 1.3 x 10-4 M AgNO3 solution?
4.
The following data was collected when a 25.00 mL sample of water containing
chloride ion was titrated using 0.100 M AgNO3 to completely precipitate the
chloride ion.
Initial volume of AgNO3
Final volume of AgNO3
18.30 mL
27.22 mL
a)
Write the net ionic reaction for the precipitation reaction.
c)
Calculate the [Cl-].
5.
In an experiment to determine the solubility of BaF2, 500.0 mL of the saturated
solution was heated in an evaporating dish to remove the water. The evaporating
dish and the residue were then heated two more times to ensure all the water was
removed.
Volume of the saturated solution of BaF2
Mass of the evaporating dish
Mass of the evaporating dish and BaF2 after the first heating
Mass of the evaporating dish and BaF2 after the second heating
Mass of the evaporating dish and BaF2 after the third heating
Using the above data, calculate the Ksp for BaF2
500.0 mL
72.540 g
73.500 g
72.855 g
72.855 g
Chemistry 12 Solubility Test # 2
1.
Consider the following experiment:
1.0 mL 0.20 M Ag+ +
an unknown solution →
1.0 mL 020 M Sr2+ +
an unknown solution →
The unknown solution could contain
A
B
C
D
2.
0.062 M
1.60 M
3.65 M
6.24 M
Calculate the [Li+] in 200.0 mL of 1.5 M Li2SO4.
A
B
C
D
5.
CuS
AgBr
CaCO3
CaSO4
A saturated solution of NaCl contains 36.5 g of solute in 0.100 L of solution. The
solubility of the compound is
A
B
C
D
4.
0.20 M OH0.20 M NO30.20 M PO430.20 M SO42-
A compound has a solubility of 7.1 x 10-5 M at 25 oC. The compound is
A
B
C
D
3.
precipitate
no precipitate
0.30 M
0.60 M
1.5 M
3.0 M
The Ksp expression for a saturated solution of Mg(OH)2 is
A
Ksp = [Mg2+][OH-]2
[Mg(OH)2]
B
Ksp = [Mg2+][OH-]2
C
Ksp = [Mg2+][OH-]
D
6.
Ksp = [Mg2+][2OH-]2
Consider the following saturated solution solutions
CuSO4
BaSO4
CaSO4
The order of cation concentration, from highest to lowest, is
A
B
C
D
7.
>
>
>
>
[Cu2+]
[Ba2+]
[Ba2+]
[Ca2+]
Trial Ksp > Ksp and a precipitate forms
Trial Ksp < Ksp and a precipitate forms
Trial Ksp > Ksp and no precipitate forms
Trial Ksp < Ksp and no precipitate forms
7.8
2.8
5.6
1.7
x
x
x
x
10-28
10-14
10-14
10-7
The ion concentrations in 0.25 M Al2(SO4)3 are
A
B
C
D
10.
[Ca2+]
[Cu2+]
[Ca2+]
[Ba2+]
The solubility of CdS = 2.8 x 10-14. The value of the Ksp is
A
B
C
D
9.
>
>
>
>
When 1.0 x 10-3 moles of CuCl2(s) are added to 1.0 L of 1.0 x 10-3 M IO3-, the
A
B
C
D
8.
[Ba2+]
[Ca2+]
[Cu2+]
[Cu2+]
[Al3+]
[SO42-]
0.25 M
0.50 M
0.75 M
0.10 M
0.25 M
0.75 M
0.50 M
0.15 M
Which of the following will not produce a precipitate when equal volumes of 0.20
M solutions are combined?
A
B
C
D
KOH and CaCl2
Zn(NO3)2 and K3PO4
Sr(OH)2 and (NH4)2S
Na2SO4 and Pb(NO3)2
11.
Consider the following equilibrium: Mg(OH)2(s) ⇄ Mg2+(aq) + 2OH-(aq)
A compound that can be added to cause a shift to the right is
A
B
C
D
12.
If the trial ion product for AgBrO3 is calculated to be 1.0 x 10-7, then
A
B
C
D
13.
a precipitate forms because the trial ion product > Ksp
a precipitate forms because the trial ion product < Ksp
no a precipitate forms because the trial ion product > Ksp
no a precipitate forms because the trial ion product < Ksp
Which of the following will dissolve in water to produce a molecular solution?
A
B
C
D
14.
NaOH
HCl
Sr(OH)2
Mg(OH)2
CaCl2
NaOH
CH3OH
Sr(OH)2
In a solubility equilibrium, the
A
B
C
D
rate of dissolving equals the rate of crystallization
neither dissolving or crystallization occurs
concentration of solute and solvent are equal
mass of dissolved solute is greater than the mass of the solution
15.
The maximum [SO42-] that can exist in 1.0 x 10-3 M Ca(NO3)2 without a
precipitate
forming is
A
B
C
D
16.
7.1
1.0
8.4
7.1
x 10-5 M
x 10-3 M
x 10-3 M
x 10-2 M
When equal volumes of 0.20 M CuSO4(aq) and 020 M Li2S(aq) are combined, the
complete ionic equation is
A
Cu2+(aq) +
S2-(aq)
→
CuS(s)
B
CuSO4(aq)
+
Li2S(aq) →
CuS(s)
+
Li2SO4(s)
C
Cu2+(aq) + SO42-(aq) + 2Li+(aq) + S2-(aq)
→ Li2SO4(aq)
CuS(s)
D
Cu2+(aq) + SO42-(aq) + 2Li(aq) + S2-(aq) → CuS(s) + 2Li+(aq)
+
+ SO42-
(aq)
17.
Consider the solubility equilibrium: CaCO3(aq) ⇄ Ca2+(aq) + CO32-(aq)
An additional piece of solid CaCO3 is added to the equilibrium above. The rate of
dissolving and the rate of crystallization have
A
B
C
D
18.
Rate of crystallization
increases
increases
not changed
not changed
increases
not changed
increased
not changed
At 25 oC, which of the following compounds would dissolve to form a saturated
solution with the greatest [Pb2+]?
A
B
C
D
19.
Rate of Dissolving
PbI2
PbCl2
PbBr2
Pb(IO3)2
Consider the following anions:
I
II
III
10.0 mL of 0.20 M Cl10.0 mL of 0.20 M OH10.0 mL of 0.20 M SO32-
When 10.0 mL of 0.20 M Pb(NO3)2 are added to each of the above, precipitates
form in
A
B
C
D
20.
I and II only
I and III only
II and III only
I, II, and III
Which of the following units could be used to describe solubility?
A
B
C
D
21.
The solubility of SnS is 3.2 x 10-3 M. The value of the Ksp is
A
B
C
D
22.
1.0 M HCl
1.0 M NaNO3
1.0 M ZnCl2
1.0 M AgNO3
4.3
6.6
1.0
1.6
x
x
x
x
10-9
10-5
10-3
10-
Ksp
Ksp
Ksp
Ksp
=
=
=
=
[Ag2+][CO32-]
[Ag+]2[CO32-]
[2Ag+][CO32-]
[2Ag+]2[CO32-]
How many moles of solute are dissolved in 200.0 mL of a saturated solution of
A
B
C
D
26.
10-5
10-3
10-3
10-2
The Ksp expression for a saturated solution of Ag2CO3 is
A
B
C
D
25.
FeS?
x
x
x
x
The solubility of SrF2 is
A
B
C
D
24.
1.0
3.2
6.4
5.7
Silver chloride, AgCl, would be least soluble in
A
B
C
D
23.
g/s
g/L
M/L
mol/s
1.2
6.0
1.5
7.7
x
x
x
x
10-19
10-19
10-10
10-10
A solution contains both Ag+ and Mg2+ ions. During selective precipitation, these
ions are removed one at a time by adding
A
B
C
D
27.
Which of the following does not define solubility?
A
B
C
solution
D
solution
28.
[Al3+]
[SO42-]
0.25 M
0.50 M
0.75 M
0.10 M
0.25 M
0.75 M
0.50 M
0.15 M
KOH and SrCl2
Zn(OH)2 and K3PO4
Zn(OH)2 and (NH4)2S
Na2SO4 and Pb(NO3)2
What is observed when H2SO4 is added to a saturated solution of CaSO4?
A
B
C
D
31.
the minimum amount of solute required to produce one litre of saturated
Which of the following will not produce a precipitate when equal volumes of 0.20
M solutions are combined?
A
B
C
D
30.
the concentration of solute in a saturated solution
the moles of solute dissolved in a given amount of solution
the maximum mass of solute that can dissolve in a given amount of
The ion concentrations in 0.25 M Al2(SO4)3 are
A
B
C
D
29.
I- followed by OHOH- followed by S2SO42- followed by ClNO3- followed by PO43-
CaSO4(s) dissolves
the [Ca2+] increases
bubbles of H2 are given off
additional CaSO4 precipitates
The solubility of CdS is 2.8 x 10-14 M. The value of the Ksp is
A
B
C
7.8 x 10-28
2.8 x 10-14
5.6 x 10-14
D
32.
1.7 x 10-7
Consider the following solutions:
0.10 M Cl0.10 M IO3-
0.10 M Br0.10 M BrO3-
Equal moles of AgNO3 are added to each solution. It is observed that a precipitate
forms in all but one solution. Which solution does not form a precipitate?
A
B
C
D
33.
ClBrIO3BrO3-
Consider the following equilibrium: 2O3(g) ⇄ 3O2(g) Keq = 65
Initially, 0.10 mole O3 and 0.10 mole of O2 are placed in a 1.0 L container. Which
of the following describes the changes in concentrations as the reaction proceeds
to equilibrium?
A
B
C
D
34.
[O3]
[O2]
decreases
decreases
increases
increases
decreases
increases
decreases
increases
Consider the following potential energy diagram for the reversible reaction.
PE
(KJ)
140
130
110
Progress of the reaction
A
B
C
D
35.
ΔH (kJ)
10
10
30
20
-20
-30
+10
+30
Increasing the temperature of a reaction increases the rate by
I
increasing frequency of collision
II
increasing the kinetic energy of collision
III
decreasing the potential energy of collision
A
B
C
D
36.
Ea reverse (kJ)
I only
I and II only
II and III only
I, II, and III
What is the Keq expression for the following equilibrium?
Fe (s) + 4H2O(g) ⇄ Fe3O4(s) + 4H2(g)
A
Keq = [H2]4
B
Keq = [H2]
[H2O]
C
Keq = [H2]4
[H2O]4
D
Keq = [Fe3O4][H2]4
[Fe]3[H2O]4
Subjective
1.
Write the net ionic equation representing the reaction that occurs when 50.0 mL
of
0.20 M ZnSO4 and 50.0 mL 0.20 M BaS are combined.
2.
A 100.0 mL sample of 0.600M Ca(NO3)2 is diluted by adding 400.0 mL of water.
Calculate the concentrations of all of the ions.
3.
When 1.00 L of CaF2 was evaporated to dryness, 2.66 x 10-2 g of residue was
formed. Calculate the Ksp.
4.
A maximum of 0.60 g Pb(NO3)2 can be added to 1.5 L of 0.100 M NaBr(aq)
without forming a precipitate. Calculate the ksp of PbBr2.
5.
Consider the following solutions at 25 oC
Saturated AgCl(aq)
Saturated Ag2CO3(aq)
Using calculations, identify the solution with the greater [Ag+].
Solubility Unit Plan
Notes- double click on the lesson number and download Power Point Viewer if you do
not have it.
Worksheets
Quiz

1. Solubility and Saturated Solutions.
WS 1
1

2. Ion Concentration Calculations and Ionic Equations. WS 2-3
2

3. Solubility to Ksp.
WS 4
3

4. Ksp to Solubilty and Size of Ksp.
WS 5
4

5. Trial Ksp.
WS 6
5

6. Separating Ions
WS 7
6

7. Common Ion Effect and
WS 8
7

8. Titrations and Max Ion Concentration
8
Quizmebc
WS 9 Web Review

9. Review
Practice Test1

10. Review
Practice Test 2

11. Test
Text book
Hebden
Read Unit III
The following workbook is designed to ensure that you can demonstrate your
understanding of all aspects of the solubility unit. Ask yourself, “do I want to do well in
this class?” If you are determined to be successful the minimum expectation that you
should have for yourself is that you do all of these questions by the due dates given by
your teacher. There are other things that you should do to prepare for the test at the end of
the unit. Remember, what you put into this course is what you will get out. There is no
substitute for consistent effort and hard work. If you can’t do a question, get some help
before the end of the unit, you need to know, understand, and remember everything.
Good luck! I know you can do well in this unit. Keep up the great work!
Web Site Address: http://www.wjmouat.com/
Chemistry 12
Solubility and Saturated Solutions
1. Define and give units for solubility.
M,
g/100mL,
WS #1
g/L
2. Describe the relationship between the rate of dissolving and the rate of crystallization
when a small amount of solute is added to an unsaturated solution.
Rate of dissolving is greater than the rate of crystallization
3. Describe the relationship between the rate of dissolving and the rate of crystallization
when a small amount of solute is added to a saturated solution.
Rate of dissolving equals the rate of crystallization
4. Describe the relationship between the rate of dissolving and the rate of crystallization
when a small amount of solute is added to a supersaturated solution.
Rate of dissolving is less than the rate of crystallization
5. Which of the above solutions would need to be prepared in order to determine the
solubility of an ionic solution.
Saturated
6. 2.65 g of Ba(OH)2 is dissolved in 70.0 mL of water to produce a saturated solution at
20 oC. Calculate the solubility in units of g/100 mL, g/L, and M.
0.221M
37.9g/L
3.79g/100mL
7. A beaker containing 100. mL of saturated BaCO3 solution weighs 159.60 g. The
beaker is evaporated to dryness and weighs 56.36 g. The empty beaker weighs 24.33 g.
Calculate the solubility in units of g/100 mL, g/ L, and M.
56.36 g
32.03g = 320g x 1 mole
Do not use the mass with water included!
- 24.33g
100 mL
L
197.3g
32.03 g
=
1.62 M
8. Write dissociation equations to represent the equilibrium present for a saturated
solution of each ionic compound. Write the solubility product (Ksp expression) for each
of the equilibrium systems. The first one is done.
a) Al2(SO4)3
⇄
2Al3+
+
3SO42-
Ksp = [Al3+]2
+
CO32-
Ksp = [Fe2+]
[SO42-]3
b) FeCO3
[CO32-]
⇄ Fe2+
c) Co2(SO4)3
⇄ 2Co3+
+
3SO42-
Ksp = [Co3+]2
⇄
+
PO43-
Ksp = [Na+]3
[SO42-]3
d) Na3PO4
3Na+
[PO43-]
10. Write formula, complete ionic, and net ionic equations for each.
a) H2SO4(aq)
NaOH(aq) →
+
H2SO4 (aq)
+ 2NaOH (aq) →
2H2O (l)
2H+(aq) + SO42-(aq) + 2Na+(aq) + 2OH-(aq)
→
+
Na2SO4 (aq)
2H2O (l) + 2Na+(aq)
+ SO42-(aq)
2H+(aq) + 2OH-(aq)
b) Mg(NO3)2(aq) +
→ 2H2O (l)
Na2CO3(aq) →
Mg(NO3)2 (aq)
+ Na2CO3 (aq) →
MgCO3 (s)
+
2NaNO3 (aq)
Mg2+(aq) + 2NO3-(aq)
+ 2Na+(aq) + CO32-(aq) → MgCO3 (s) + 2Na+(aq) +
2NO3 - (aq)
Mg2+(aq)
c) Al(NO3)3(aq) +
+ CO32-(aq) →
MgCO3 (s)
(NH4)3PO4(aq) →
Al(NO3)3 (aq)
+ (NH4)3PO4 (aq) →
AlPO4 (s)
+
3NH4NO3 (aq)
Al3+(aq) + 3NO3-(aq)
+ 3NH4+(aq) + PO43-(aq) → AlPO4 (s)+ 3NH4+(aq) +
3NO3 - (aq)
Al3+(aq)
+ PO43-(aq) →
AlPO4 (s)
d) H3PO4(aq) + Ca(OH)2(aq) →
2H3PO4(aq) + 3Ca(OH)2(aq) → Ca3(PO4)2(s) + 6HOH(l)
6H+ (aq) + 2PO43-(aq) + 3Ca2+(aq) + 6OH-(aq)
→ Ca3(PO4)2(s)
6H+ (aq) + 2PO43-(aq) + 3Ca2+(aq) + 6OH-(aq)
→ Ca3(PO4)2(s)
Chemistry 12
1.
Solubility
WS #2
+ 6HOH(l)
+ 6HOH(l)
Ion Concentration Calculations
What is the concentration of each ion in a 10.5 M sodium silicate solution?
Na2SiO3
⇄
2Na+
+
SiO32-
10.5 M
21.0 M 10.5 M
[Na+] = 21.0 M,
[SiO32-] = 10.5 M
2.
What is the concentration of each ion in the solution formed when 94.5 g of nickel
(III) sulphate is dissolved into 850.0 mL of water?
Molarity =
Ni2(SO4)3
94.5 g x
⇄
1 mole
405.7g
0.850L
2Ni3+
=
+
0.2740
0.548 M
[Ni3+] = 0.548 M,
[SO42-] = 0.822 M
0.2740
3SO420.822 M
3.
If 3.78 L of 0.960 M sodium fluoride solution is added to 6.36 L of 0.550 M
calcium nitrate solution, what is the resulting concentration of [Ca+2] and [F-]?
NaF
Ca(NO3)2
⇄
3.78 x 0.960 M =
6.36 x 0.550 M =
10.14
10.14
[Ca2+] = 0.345 M,
⇄
Na+
+
F-
Ca2+
+
2NO3-
0.358 M
0.345 M
0.358M
0.690M
[F-] = 0.358 M
4.
What is the concentration of each ion in the solution formed when 94.78 g of iron
(III) sulphate is dissolved into 550.0 mL of water?
[Fe3+] = 0.8619 M,
[SO42-] = 1.293 M
5. If the [F-] = 0.200 M, calculate the number of grams AlF3 that would be dissolved in
2.00 L of water.
AlF3
⇄
0.06667M
Al3+
3F-
+
0.06667M
2.00L x 0.06667 mole x
L
84.0 g
mole
=
0.200M
11.2g
6. If the [SO42-] = 0.200 M in 2.0 L of Al2(SO4)3, determine the [Al3+] and the molarity
of the solution.
Al2(SO4)3
⇄
0.067 M
2Al3+
+
3SO42-
0.13 M
0.20 M
Dissociation Equations Write a dissociation equation for any chemical which
dissociate when dissolved in water:
1.
HCl (aq)
⇄
H+
+
Cl-
2.
Na2S (s)
⇄
2 Na+ (aq)
+
S2- (aq)
3.
Al(CH3COO)3 (s)
⇄
Al3+ (aq)
+
3CH3COO- (aq)
4.
MgBr2 (s)
⇄
Mg2+ (aq)
+
2 Br- (aq)
5.
Na2CO3 (s)
⇄
2 Na+ (aq)
+
CO32- (aq)
6.
C12H22O11 (s)
compounds do not dissociate)
7.
K3PO4 (s)
8.
CH3OH (l)
compounds do not dissociate)
Net Ionic Equations
⇄
C12H22O11 (aq)
⇄
3 K+ (aq)
⇄
CH3OH (aq)
(molecular
+
PO43- (aq)
(molecular
Write chemical equations, total ionic equations and net ionic equations for each reaction.
The first one is done for you. (assume that all reactions occur):
1.
Magnesium metal is placed in hydrochloric acid
Mg (s)
+ 2 HCl (aq)
→
Mg (s) + 2 H+ (aq) + 2 Cl- (aq) →
Mg (s)
+ 2 H+ (aq)
→
MgCl2 (aq)
+
H2 (g)
Mg2+ (aq) + 2Cl- (aq) + H2 (g)
Mg2+ (aq) +
H2 (g)
2.
Zinc metal is placed in silver nitrate solution
Zn (s)
+ 2Ag NO3 (aq) →
Ag (s) +
+
Zn(s) + 2Ag (aq) + 2 NO3-(aq) →
2NO3-(aq)
Zn(s)
3.
Zn+2 (aq)
+
2Ag(s)
Barium chloride solution is added to lead (II) nitrate solution.
+ Pb(NO3)2 (aq) → PbCl2 (s)
BaCl2 (aq)
Ba2+(aq)
2NO3
→
2Ag+ (aq)
+
2 Zn(NO3)2 (aq)
2Ag(s) + Zn+2 (aq) + +
-
Ba2+ (aq)
(aq)
2Cl- (aq)
+
→
PbCl2 (s)
Sulphuric acid is added to Strontium hydroxide solution.
H2SO4 (aq)
+ Sr(OH)2 (aq) →
2H+(aq) + SO42-(aq) + Sr2+(aq) + 2OH-(aq)
2H2O (l)
→
2H+(aq) + SO42-(aq) + Sr2+(aq) + 2OH-(aq)
5.
Ba(NO3)2 (aq)
+ 2Cl-(aq) + Pb2+(aq) + 2NO3-(aq) → PbCl2 (s) +
Pb2+ (aq)
4.
+
+
SrSO4 (s)
2H2O (l) + SrSO4 (s)
→ 2H2O (l) + SrSO4 (s)
Sodium carbonate solution is added to nickel (III) nitrate solution.
3Na2CO3(aq)
+ 2Ni(NO3)3 (aq) → Ni2(CO3)3 (s)
+
6NaNO3 (aq)
6Na+(aq) +3CO32-(aq) +2Ni3+(aq) +6NO3-(aq) → Ni2(CO3)3 (s) + 6Na+(aq)
+6NO3-(aq)
3CO32-(aq)
6.
Cl2 (aq)
+
2Ni3+(aq) →
Ni2(CO3)3 (s)
Aqueous chlorine is added to sodium bromide solution.
+ 2NaBr (aq) → 2NaCl (aq)
+ Br2 (aq)
Cl2 (aq) + 2Na+ (aq) + 2Br- (aq) → 2Na+ (aq) + 2Cl- (aq) + Br2 (aq)
+
Cl2 (aq)
7.
+ 2Br- (aq)
→ 2Cl- (aq)
+
Br2 (aq)
Nitric acid is added to aluminum hydroxide solution.
2HNO3 (aq)
+ Sr(OH)2 (aq) → 2H2O (l)
2H+(aq) +
2NO3-(aq) +
Sr2+(aq) +
+
2OH-(aq)
Sr(NO3)2 (aq)
→
3H2O (l) + Sr2+(aq) + 2NO3-
(aq)
H+(aq) + OH-(aq)
→
H2O (l)
WS # 3
1. Classify each as an ionic or molecular (covalent) solution.
NaCl (aq) __________Ionic
NH3 (aq) __________ molecular
CoCl2 (aq) _________ Ionic
AgCl (aq) _________ Ionic
CH3OH (aq) ________ molecular
HCl (aq) __________ Ionic (although this is
a covalent compound when gaseous, it ionizes in solution)
NH4OH (aq) ________ Ionic
I2 (aq) ___________ molecular
2. Define each:
a) unsaturated solution: contains less than the maximum amount of dissolved
solute
b) saturated solution: contains the maximum amount of dissolved solute
c) solubility: the maximum amount of solute the can dissolve in a given amount
of solution (M, g/L, or g/100mL).
3. Describe how you would prepare a saturated solution.
Add measured increments of solute to a given volume of water until it no longer
dissolves. Add the mass of the solute added and divide by the volume of
solution.
4. Describe how you would determine the solubility of NaCl in water at 20oC.
Add measured increments of NaCl to 100 mL of water until it no longer dissolves.
Add the mass of the solute and divide by 0.100 L of solution.
5. In terms of equilibrium describe the difference between a saturated and unsaturated
solution.
A saturated solution is at equilibrium and an unsaturated solution is not.
6. What is the effect of temperature on solubility?
Increasing the temperature usually increases the solubility.
7. 200g of CoCl2 is dissolved in 500.0 mL of water at 0oC to form a saturated solution.
What is the solubility of CoCl2 at 0oC in three different units?
Molarity
129.9 g
=
=
200g
x 1 mole
129.9g
=
3.08 M
400 g/L = 40.0 g/100mL
0.500 L
3.0793 mole x
L
1 mole
8. In a saturated solution of CaCl2, a small amount of solid is present. Write a net ionic
equation showing the equilibrium reaction. Write the solubility product
(Ksp expression)
CaCl2 <------> Ca2+
2Cl-
+
Ksp = [Ca2+][Cl-]2
9. If you were given a saturated, unsaturated and supersaturated solution, how would you
distinguish one from another?
a) Unsaturated solution: add some solute and it will dissolve
b)
Saturated solution: add some solute and it will not dissolve
c) Supersaturated solution: add some solute and it will cause more crystallization
10.
Write the equilibrium equation and solubility product Ksp for each salt. The first
one is done.
a)
Ca(OH)2 (s) ⇄
b)
AgCl (s) ⇄ Ag+ +
c)
Na3PO4 (s) ⇄
d)
(NH4)3PO4 (s) ⇄
e)
Cu2SO4 (s) ⇄
f)
Al(CH3COO)3 (s) ⇄ Al+3
+
3CH3COO-
Ksp = [Al+3] [CH3COO-]3
g)
Ca3(PO4)2 (s) ⇄
+
2PO4-3
Ksp = [Ca+2]3 [PO4-3]2
Chem 12
WS #4
Ca2+
+
2OH-
Cl-
3Na+
Ksp = [Ag+] [Cl-]
+
3NH4+
2Cu+1
3Ca+2
Ksp = [Ca2+] [OH-]2
PO4-3
+
PO4-3
SO4-2
+
Solubility to Ksp
Ksp = [Na+]3 [PO4-3]
Ksp = [NH4+]3 [PO4-3]
Ksp = [Cu+1]2 [SO4-2]
The Ksp is a measure of the solubility of an ionic salt. The larger the value of the Ksp, the
greater is the solubility of the salt. You can only calculate a Ksp if the solution is
saturated. Only saturated salt solutions are in equilibrium. You can calculate the Ksp from
the solubility of a salt, since the solubility represents the concentration required to
saturate a solution.
1. Calculate the Ksp for CaCl2 if 200.0 g of CaCl2 are required to saturate 100.0 mL of
solution.
Molarity
=
200 g x 1 mole
111.1 g
0.100L
CaCl2
⇄
18.0 M
18.0 M 36.0M
Ca2+
+
=
18.001 M
2Cl-
Ksp = [Ca2+][Cl-]2
Ksp = [18.0][36.0]2
Ksp = 2.33 x 104
2. Calculate the Ksp for AlCl3 if 100.0 g is required to saturate 150.0 mL of a solution.
Ksp = 1.679 x 104
3. The solubility of SrF2 is 2.83 x 10-5 M. Calculate the Ksp.
Ksp = 9.07 x 10-14
4. The solubility of GaBr3 is 15.8 g per 100 mL. Calculate the Ksp.
Molarity
=
15.8 g x 1 mole
309.4 g
0.100 L
=
0.51066 M
⇄
GaBr3
0.51066 M
Ga3+
0.51066 M
+
3Br-
1.532 M
Ksp = [Ga3+][Br-]3
Ksp = [0.51066][1.532]3
Ksp = 1.83
5.
The solubility of Ag2SO4 is 1.33 x 10-7g per 100 mL. Calculate the Ksp.
Ksp = 3.10 x 10-25
6.
If 2.9 x 10-3 Ca(OH)2 g is needed to saturate 250 mL of solution, what is the Ksp.
Ksp =1.5 x 10-11
7.
At a certain temperature, a 40.00 mL sample of a saturated solution of barium
hydroxide, is neutralized by 29.10 mL of 0.300 M HCl. Calculate the Ksp of
Ba(OH)2.
2HCl
0.02910 L
0.300 M
+
Molarity Ba(OH)2
1 mole Ba(OH)2
Ba(OH)2
0.0400 L
?M
=
→
BaCl2 +
0.02910 L HCl
x
2HOH
0.300 moles
1L
2 moles HCl
0.0400 L
=
Ba(OH)2
0.1091 M
⇄
0.109 M
Ba2+
0.1091 M
+
2OH0.2183 m
x
Ksp
=
[Ba2+][OH-]2
Ksp
=
[0.1091][0.2183]2
=
5.20 x 10-3
Calculate the concentrations of all ions in each solution.
8.
0.50 M Al2(SO4)3(aq)
Al2(SO4)3 ⇄
2Al3+
0.50 M
1.0 M
[Al3+] = 1.0M
+
3SO421.5 M
[SO42-] = 1.5M
9. 25.7g (NH4)3PO4 (aq) in 250mL H2O.
[NH4+] = 2.07M
[PO43-] = 0.690M
10. 210g CoCl2 • 6H2O in 800mL H2O.
[Co2+] = 1.10M
[Cl-] = 2.20M
Chemistry 12
Ksp to Solubility
WS # 5
Calculate the solubility in M and g/L for each. Use the Ksp values found in your chart.
1) BaCO3
BaCO3(s)
⇄
x
x
ksp
=
[Ba2+][ CO32-]
ksp
=
x2
Ba2+
+
x
CO32-
2.6 x 10-9 =
x2
5.099 x 10-5 M
5.099 x 10-5 mole x 197.3 g
L
1 mole
=
1.0 x 10-2 g/L
2) Fe(OH)2
2.1 x 10-4 g/L
3) PbCl2
4.0 g/L
4) How many grams of Mg(OH)2 are required to completely saturate 1.5 L of solution?
Mg(OH)2
⇄
x
Mg2+ +
2OH-
x
2x
Ksp
=
[Mg2+][OH-]2
Ksp
=
[x][2x]2
Ksp
=
4x3
5.6 x 10-12
=
4x3
1.119 x 10-4 M
=
x
1.5 L x 1.119 x 10-4 mole x 58.3 g
=
9.8 x 10-3 g
1L
1 mole
Review
1. If 200 g of MgCl2 is required to saturate 1.5 L of solution at 20 oC, calculate the Ksp.
Ksp = 11
2. 2. If the Ksp for Al2O3 is 2.8 x 10-8, calculate [Al3+] and [O-2] in
[Al+3] = 2.4 x 10-2 M
Trial Ksp
mol
/L.
[O-2] = 3.6 x 10-2 M
Worksheet 6
1. Will a precipitate form if 200ml 0.00020M Ca(NO3)2 is mixed 300ml of 0.00030M
Na2C03?
CaCO3
⇄
Ca2+
+
CO32-
200 x 0.00020 M
500
300 x 0.00030 M
500
0.000080 M
0.00018 M
Trial Ksp
=
[0.000080][0.00018]
Trial Ksp
=
1.4 x 10-8
>
Ksp(5.0 x 10-9)
Therefore a precipitate forms!
2. Will a precipitate form if 25.0ml of .0020M Pb(NO3)2 is mixed with 25.0ml of
.040M NaBr.
Trial ksp = 4.0 x 10-7 no ppt
3. Will a precipitate form if equal volumes of 0.00020M Ca(NO3)2 is mixed with
0.00030M Na2C03?
Note: When equal volumes are mixed the dilution factor is ½ for each ion.
Trial ksp = 1.5 x 10-8 ppt > Ksp and there is a precipitate
Ksp
4. Co(OH)2
Solubility = 3.0x10-3 g/L Ksp=?
ksp = 1.3 x 10-13
5. Ag2C2O4 Solubility = 8.3x10-4 M
Ksp=?
ksp = 2.3 x 10-9
Solubility
6. SrF2 Solubility in (M) = ?
1.0 x 10-3 M
7. Cu(IO3)2
Solubility (g/L) = ?
1.1 g/L
Separation Positive Ions: Work from top to bottom of solubility chart!!
7
1.
Ag+ Mg2+ Ba2+
i) Add:
Ag+
NaCl(aq)
Filter Out:
AgCl(s)
Net Ionic equation:
Filter Out:
BaSO4(s)
Net Ionic equation:
Mg(OH)2(s)
Net Ionic equation:
+ Cl- ------> AgCl(s)
ii) Add:
Ba2+
Na2SO4(aq)
+ SO4-2 ------> BaSO4(s)
iii) Add:
NaOH(aq)
Filter Out:
Mg2++2OH-------> Mg(OH)2(s
2.
WS #
Pb2+
Ba2+
Sr2+
i) Add:
Pb+2
NaCl(aq)
Filter Out:
PbCl2(s)
Net Ionic equation:
Filter Out:
Ba(OH)2(s)
Net Ionic equation:
Filter Out:
Sr3(PO4)2(s)
Net Ionic equation:
Filter Out:
CuCl(s)
Net Ionic equation:
Filter Out:
Ca(OH)2(s)
Net Ionic equation:
Sr3(PO4)2(s)
Net Ionic equation:
Filter Out:
AgCl(s)
Net Ionic equation:
Filter Out:
SrSO4(s)
Net Ionic equation:
Filter Out:
Be(OH)2(s)
Net Ionic equation:
Filter Out:
PbCl2(s)
Net Ionic equation:
CaSO4(s)
Net Ionic equation:
+ 2Cl- ------> PbCl2(s)
ii) Add:
NaOH(aq)
Ba2++2OH-------> BaOH)2(s)
iii) Add:
Na3PO4(aq)
3Sr2++2PO4-3------> Sr3(PO4)2(s)
Cu+
3.
i) Add:
Cu+
Ca2+
Sr2+
NaCl(aq)
+ Cl- ------> CuCl(s)
ii) Add:
NaOH(aq)
Ca2++2OH-------> Ca(OH)2(s)
iii) Add:
Na3PO4(aq)
Filter Out:
3Sr2++2PO4-3------> Sr3(PO4)2(s)
Be2+
4.
i) Add:
Ag+
Sr2+
Ag+
NaCl(aq)
+ Cl- ------> AgCl(s)
ii) Add:
Sr2+
Na2SO4(aq)
+ SO4-2 ------> SrSO4(s)
iii) Add:
NaOH(aq)
Be2++2OH-------> Be(OH)2(s)
5.
Be2+
i) Add:
Pb+2
Pb2+
NaCl(aq)
+ 2Cl- ------> PbCl2(s)
ii) Add:
Ca2+
Ca2+
Na2SO4(aq)
Filter Out:
+ SO4-2 ------> CaSO4(s)
iii) Add:
NaOH(aq)
Filter Out:
2+
Be +2OH ------> Be(OH)2(s)
Be(OH)2(s)
Net Ionic equation:
]
6. Calculate the Ksp for CaCl2, if 50.0 g is required to saturate 25.0 mL of water.
50.0 g x 1 mole
111.1 g
2.33 x 104
0.0250 L
=
Ksp = 4x3
18.0 M
=
4(18.0)3
=
7. Calculate the molar solubility of Mg(OH)2.
Mg(OH)2
x
⇄
Mg2+ +
x
2OH2x
4x3 = 5.6 x 10-12
x = 1.1 x 10-4 M
8.
Will a precipitate form if equal volumes of 0.00020 M Na2CO3 is mixed with
0.00020 M MgCl2.
MgCO3(s)
⇄
Mg2+
+
½ (0.00020 M)
0.00010 M
Trial Ksp
=
[Mg2+][CO32-]
(0.00010)(.00010)
1 x 10-8
Trial Ksp < Ksp = 6.8 x 10-6
9.
CO32½ (0.00020 M)
0.00010 M
no ppt
Write the formula, complete, and net ionic equation.
Formula Equation: CaCl2(aq) + 2AgNO3(aq) → Ca(NO3)2(aq) +
Complete Ionic:
+ 2AgCl(s)
Ca2+ + 2Cl- + 2Ag+ + 2NO3- →
2AgCl(s)
Ca2+ + 2NO3-
Net Ionic:
1.
SO32- OH-
i) Add:
Ag+ + Cl-
→
Filter Out:
SrSO3(s)
Net Ionic equation:
Zn(OH)2(s)
Net Ionic equation:
Filter Out:
AgI(s)
Net Ionic equation:
Filter Out:
SrCO3(s)
Net Ionic equation:
Zn(OH)2(s)
Net Ionic equation:
Sr3(PO4)2(s)
Net Ionic equation:
ZnS(s)
Net Ionic equation:
AgCl(s)
I-
Sr(NO3)2(aq)
Sr2+ + SO32- ---->SrSO3(s)
ii) Add:
Zn(NO3)2(aq) Filter Out:
Zn2+ + 2OH- ----> Zn(OH)2(s)
iii) Add:
AgNO3(aq)
Ag+ + I- ---->AgI(s)
2.
CO32- OH-
i) Add:
Sr(NO3)2(aq)
Sr2+ + CO32- ---->SrCO3(s)
ii) Add:
Zn(NO3)2(aq) Filter Out:
Zn2+ + 2OH- ----> Zn(OH)2(s)
3.
Br-
i) Add:
S2-
PO43-
Sr(NO3)2(aq)
Filter Out:
3Sr2+ + 2PO43- ----> Sr3(PO4)2(s)
ii) Add:
Zn(NO3)2(aq) Filter Out:
Zn2+ + 2S-2 ----> ZnS(s)
iii) Add:
equation:
4.
AgNO3(aq)
Filter Out:
Ag+ + Br- ---->AgBr(s)
PO43- OH-
S2-
AgBr(s)
Net Ionic
i) Add:
Sr(NO3)2(aq)
Filter Out:
Sr3(PO4)2(s)
Net Ionic equation:
Mg(OH)2(s)
Net Ionic equation:
ZnS(s)
Net Ionic equation:
Mg(OH)2(s)
Net Ionic equation:
BaSO4(s)
Net Ionic equation:
ZnS(s)
Net Ionic equation:
BaSO4(s)
Net Ionic equation:
ZnS(s)
Net Ionic equation:
AgCl(s)
Net Ionic equation:
3Sr2+ + 2PO43- ----> Sr3(PO4)2(s)
ii) Add:
Mg(NO3)2(aq) Filter Out:
Mg2+ + 2OH- ----> Mg(OH)2(s)
iii) Add:
Zn(NO3)2(aq) Filter Out:
Zn2+ + 2S-2 ----> ZnS(s)
5.
OH-
i) Add:
S2-
SO42-
Mg(NO3)2(aq) Filter Out:
Mg2+ + 2OH- ----> Mg(OH)2(s)
ii) Add:
Ba(NO3)2(aq) Filter Out:
Ba2+ + SO42- ---->BaSO4(s)
iii) Add:
Zn(NO3)2(aq) Filter Out:
Zn2+ + 2S-2 ----> ZnS(s)
6.
S2-
i) Add:
SO42- ClBa(NO3)2(aq) Filter Out:
Ba2+ + SO42- ---->BaSO4(s)
ii) Add:
Zn(NO3)2(aq) Filter Out:
Zn2+ + 2S-2 ----> ZnS(s)
iii) Add:
AgNO3(aq)
Filter Out:
Ag+ + Cl- ---->AgCl(s)
Common Ion Effect Worksheet # 8
Consider the following equilibrium system.
PbCl2(s) ⇌
Pb2+(aq)
+ 2 Cl-(aq)
Describe what happens to the solubility of PbCl2 after each of the changes are made.
Solu
1. PbCl2(s) is added
no c
2. Pb(NO3)2 is added
decr
3. NaCl is added
decr
4. H2O is added
(remember that solubility is moles per litre)
no c
5. AgNO3 is added (Ag+ reacts with Cl- to form AgCl(s) which has low solubility)
increases
6. NaBr is added
(Br- reacts with Pb2+ to form PbBr2(s) which has low solubility)
increases
AgBr(s) ------> Ag+(aq)
Consider the following equilibrium system.
+
Br-(aq)
Describe what happens to the solubility of PbCl2 after each of the changes are made.
7. AgBr(s) is added
8. Pb(NO3)2 is added
Pb2+ reacts with Br- to form PbBr2(s) which has low solubility
9. NaCl is added
(Ag+ reacts with Cl- to form AgCl(s) which has low solubility)
10. H2O is added
(remember that solubility is moles per litre)
11. AgNO3 is added
decreases
12. NaBr is added
decreases
13.
Explain why more Zn(OH)2(s) dissolves when 3 M HCl is added to a saturated
solution of Zn(OH)2. Start by writing the correct equilibrium equation.
Zn(OH)2(S)
⇌
Zn2+
+
2OH-
The HCl increases the concentration of H+ which reacts with OH- lowering
the [OH-]. This causes the above equilibrium to shift to the right
and more
Zn(OH)2(S) dissolves.
14.
In an experiment, 0.1 M AgNO3 is added to 0.1 M NaCl, resulting in the
formation of a white precipitate. When 0.1 M NaI is added to this mixture, the
precipitate dissolves and a yellow precipitate forms.
white
The formula for the white precipitate is
AgCl
The formula for the yellow precipitate is
AgI
The net ionic equation for the first equilibrium is
⇌
AgCl(s)
Ag+
+
Cl-
The net ionic equation for the formation of the yellow precipitate is
+
I→
AgI(s)
Ag+
Explain why the white precipitate dissolves. Start by writing the equilibrium
equation for the white precipitate, then, explain how adding NaI affects this
equilibrium.
⇌
AgCl(s)
Ag+
+
Cl-
The NaI increases the concentration of I- which reacts with Ag+ lowering the
This causes the above equilibrium to shift to the right
and
AgCl(s)
dissolves.
[Ag+].
Titrations and Maximum Ion Concentration
Worksheet # 9
1.
In a titration 25.0ml of a 0.250M AgNO3 solution was used to precipitate out all
of the Br- in a 200 ml sample. Calculate [Br-].
Ag+
+
0.0250 L
0.250 M
Br-
→
AgBr(s)
0.200 L
?M
0.0250 L
1 mole Br[Br-] =
1 mole Ag+
x
0.250 mole
1L
0.200 L
[Br-] =
0.0313M
x
2.
In a titration 26.5ml of .100M Pb(NO3)2 was used to precipitate out all of the Clin a 30.0 ml sample of water. Calculate [Cl-].
[Cl-] = 0.177 M
Maximum Ion Concentration
3.
Calculate the maximum concentration of OH- that can exist in a 0.200 M
Mg(N03)2 solution.
Mg(OH)2(s)
⇄
Mg2+ +
2OH-
0.200 M
[OH-]
Ksp
=
[Mg2+][OH-]2
5.6 x 10-12
=
[0.200][OH-]2
[OH-]
=
5.3 x 10-6 M
4.
Calculate the maximum concentration of CO3-2 that can exist in a .500M AgNO3
solution.
[CO3-2] = 3.4 x 10-11 M
5.
Calculate the maximum concentration of IO3- that can exist in a .200M Cu(N03)2
solution.
[IO3-] = 5.9 x 10-4 M
6.
Calculate the maximum concentration of Ca+2 that can exist in a .200M Na2C03
solution.
[Ca2+] = 2.5 x 10-8 M
7.
Calculate the minimum number of moles of Pb(NO3)2 required to start
precipitation in 50.0 mL of 0.15 M ZnCl2.
PbCl2 ⇄
Pb2+
+
[Pb2+]
2Cl0.30 M
Ksp = [Pb2+][ Cl-]2
Don’t forget to multiple 0.15 M by 2 due to ZnCl2
1.2 x 10-5
= [Pb2+][ 0.30]2
[Pb2+] = 1.33 x 10-4 M
0.0500 L x .000133 moles = 6.7 x 10-6 moles
L
8.
In a titration 12.5 mL of 2.00 x 10-5 M HCl is required to neutralize 250 mL of
saturated AgOH solution. Calculate the [OH-] and then determine the Ksp for AgOH.
Ag+ +
.250 L
?M
Cl→
.0125 L
.00002 M
[Ag+] =
0.0125 L Cl- x
AgCl(s)
Cl0.250 L
0.00002 moles x
L
1 mole Ag+
1 mole
=
1.0 x 10-6 M
AgOH(s)
1.0 x 10-6 M
⇄
Ag+
+
1.0 x 10-6 M
Ksp
=
[Ag+][OH-]
Ksp
=
(1.0 x 10-6 )2
Ksp
=
1.0 x 10-12
OH1.0 x 10-6 M
9.
When excess Ag2CO3(s) is shaken with 1.00 L of 0.200 M K2CO3 it is determined
that 6.00 x 10-6 moles of Ag2CO3 dissolves. Calculate the solubility
product of
Ag2CO3.
Ag2CO3(s)
⇄
2Ag+
6.00 x 10-6 M
x2
1.20 x 10-5M
This molarity is determined by the soluble K2CO3
There is a 2 in the formula Ag2CO3
Ksp
=
[Ag+]2[CO32-]
=
[1.20 x 10-5]2[0.200]
=
2.88 x 10-11
+
CO320.200 M