R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 1 / 47
Chemistry 12
Provincial Exam Workbook
Unit 03: Solubility Equilibrium
Multiple Choice Questions
1.
Which of the following would be true when equal volumes of 0.2 M NaBr and 0.2 M
AgNO3 are combined?
A. No precipitate forms
B. A precipitate of AgBr forms
C. A precipitate of NaNO3 forms
D. Precipitates of both NaNO3 and AgBr form
2.
A.
B.
C.
D.
3.
Using the solubility table, determine which of the following ions could not be used to
separate S2 from SO42 by precipitation?
Be2
Ca2
Ba2
Sr 2
Which of the following is true when solid Na2 S is added to a saturated solution of
CuS and equilibrium is re-established?
A. S2  increases
B. Cu2  increases
C. S2  does not change
D. Cu2  does not change
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 2 / 47
4.
Which of the following describes the relationship between the solubility product
constant K sp  and the solubility  s  of PbI2 ?
A. K sp =s2
B. K sp =4s3
3
C. s=
K sp
4
D. s= K sp
Which of the following saturated solutions will have the lowest S2  ?
5.
A.
B.
C.
D.
6.
BaS
CaS
CuS
ZnS
What is the solubility of SrF2 ?
A. 3.2x1025M
B. 1.8x1017M
C. 4.3x109M
D. 1.0x103M
7.
Which of the following is a suitable term for representing solubility?
A. grams
B. moles
C. molarity
D. millilitres per second
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 3 / 47
8.
9.
A saturated solution is prepared by dissolving a salt in water. Which of the following
graphs could represent the ion concentrations as the temperature is changed?
What is the concentration of OH ions in 250 mL of 0.20 M Sr  OH2 ?
A. 0.050 M
B. 0.10 M
C. 0.20 M
D. 0.40 M
10.
What happens when 10.0 mL of 0.2 M KOH is added to 10.0 mL of 0.2 M CuSO4 ?
A. No precipitate forms
B. A precipitate of K 2 SO4 forms
C. A precipitate of Cu  OH2 forms
D. Precipitates of K 2 SO4 and Cu  OH2 form
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 4 / 47
11.
Consider the following equilibrium…
CaSO4 (s)  Ca2 (aq)  SO42 (aq)
Which of the following would shift the above equilibrium to the left?
A. adding CaSO4 (s)
B. adding MgSO4 (s)
C. removing some Ca2 (aq)
D. removing some SO42 (aq)
12.
Calculate the solubility of CaC2 O4 .
A. 2.3x109M
B. 1.2x105M
C. 4.8x105M
D. 8.3x104M
13.
A.
B.
C.
D.
How many moles of dissolved solute are present in 100.0 mL of a saturated SrCO3
solution?
5.6x1011mol
2.4x106mol
2.4x105 mol
2.4x104mol
14.
What happens when equal volumes of 0.2 M AgNO3 and 0.2 M NaCl are combined?
A. A precipitate forms because the trial ion product > K sp
B. A precipitate forms because the trial ion product < K sp
C. No precipitate forms because the trial ion product > K sp
D. No precipitate forms because the trial ion product < K sp
15.
Determine the maximum Na2 CO3  that can exist in 1.0 L of 0.0010M Ba NO3 2
without forming a precipitate.
A.
B.
C.
D.
2.6x1012M
2.6x109M
2.6x106M
2.6x105M
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 5 / 47
16.
Solid Ba  OH2 is added to water to prepare a saturated solution. Which of the
following is true for this equilibrium system?
A. anion  cation
B. trial K sp is less than K sp
C. blue litmus paper would turn red
D. the rate of dissolving = the rate of crystallization
17.
A saturated solution of PbI2 was subjected to a stress and the following graph was
obtained.
Which stress was applied at time t1 ?
A. the addition of PbI2
B. a temperature change
C. an increase in volume
D. the evaporation of water
18.
A solution is prepared containing both 0.2 M OH and 0.2 M PO43 ions. An equal
volume of a second solution is added in order to precipitate only one of these two
anions. The second solution must contain which of the following?
A. 0.2 M
B. 0.2 M
C. 0.2 M
D. 0.2 M
Cs
Zn2 
Pb2
Sr 2
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 6 / 47
19.
Consider the following equilibrium…
CaS(s)  Ca2 (aq)  S2 (aq)
When Ca NO3 2 (aq) is added to this solution, the equilibrium shifts to the…
A. left and S2  increases
B. left and S2  decreases
C. right and S2  increases
D. right and S2  decreases
20.
A.
B.
C.
D.
3.2x1016
9.0x109
6.7x105
1.3x104
21.
A.
B.
C.
D.
How many moles of Pb2 are there in 500.0 mL of a saturated solution of PbSO4 ?
Which of the following compounds is least soluble in water?
CuI
BeS
CsOH
AgBrO3
22.
Which of the following will dissolve to form a molecular solution?
A. H2 SO4
B. AgNO3
C. Ca  OH2
D. C6H12 O6
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 7 / 47
23.
Consider the following equilibrium…
energy  AgCl(s)  Ag (aq)  Cl (aq)
Addition of which of the following will increase the solubility of AgCl ?
A. heat
B. HCl
C. AgNO3
D. a catalyst
24.
What is the Cl  when 15.0 g of NaCl is dissolved in enough water to make 100.0
mL of solution?
A. 0.150 M
B. 0.390 M
C. 2.56 M
D. 3.90 M
25.
An equal number of moles of Na2 CO3 is added to four different 10.0 mL samples.
A precipitate forms in only one of the samples. Identify the cation which is present in the
precipitate.
A.
B.
C.
D.
Ba2
Ca2
Mg2
Sr 2
26.
What is the net ionic equation for the reaction between BaS(aq) and Sr  OH2 (aq) ?
A. Sr 2 (aq)  S2 (aq)  SrS(s)
B. Ba2 (aq)  2OH (aq)  Ba  OH2 (s)
C. Ba2 (aq)  S2 (aq)  Sr 2 (aq)  2OH (aq)  Ba  OH2 (s)  SrS(s)
D. Ba2 (aq)  S2 (aq)  Sr 2 (aq)  2OH (aq)  Ba  OH2 (s)  Sr 2 (aq)  S2- (aq)
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 8 / 47
27.
In which of the following would PbCl2 (s) be least soluble?
A. 1 M HCl
B. 1 M BaCl2
C. 1 M K 2 SO4
D. 1 M Pb NO3 2
28.
A.
B.
C.
D.
The solubility of ZnCO3 is 6.4x109M . What is the value of K sp for ZnCO3 ?
4.1x1017
6.4x109
1.3x108
8.0x105
29.
What is the K sp for the salt Pb IO3 2 if its solubility is 5.0x10-5M ?
A. 5.0x10-13
B. 1.3x10-13
C. 2.5x10-9
D. 5.0x10-5
30.
What is the maximum IO3-  that can exist in a 6.9x10-2M Cu2+ solution?
A. 2.0x10-6M
B. 1.0x10-6M
C. 1.0x10-3M
D. 6.9x10-2M
31.
Which of the following will form a saturated solution?
A. 0.10 mol CaSO4 added to 1.0 L of water
B. 0.10 mol Cs2 SO4 added to 1.0 L of water
C. 0.20 mol MgSO4 added to 2.0 L of water
D. 0.50 mol Pb NO3 2 added to 2.0 L of water
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 9 / 47
32.
Which of the following would be an appropriate measure of solubility?
A. moles of solute per volume of solute
B. mass of solute per volume of solution
C. volume of solvent per mass of solvent
D. moles of solute at a specific temperature
33.
What is the complete ionic equation for the precipitation reaction between MgS(aq)
and Sr  OH2 (aq) ?
A. Mg2+ (aq)+2OH(aq)  Mg  OH2 (s)
B. MgS(aq)+Sr  OH2 (aq)  SrS(aq)+Mg  OH2 (s)
C. Mg2+ (aq)+S2- (aq)+Sr 2+ (aq)+2OH (aq)  SrS(s)+Mg2+ (aq)+2OH- (aq)
D. Mg2+ (aq)+S2- (aq)+Sr 2+ (aq)+2OH (aq)  Sr 2+ (aq)+S2- (aq)+Mg  OH2 (s)
34.
What is the K sp expression for the low solubility salt formed when K 2 SO3 (aq) and
AlCl3 (aq) are mixed?
A. K sp = SO32- 
B. K sp = K +  Cl- 
2
3
3
2
C. K sp =  Al3+  SO32- 
D. K sp =  Al3+  SO32- 
35.
A.
B.
C.
D.
Which compound has the lowest solubility?
ZnS
CuS
AgCl
SrSO4
36.
What is the solubility of the salt PbCl2 ?
A. 1.4x10-2M
B. 2.4x10-3M
C. 3.5x10-3M
D. 1.2x10-5M
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 10 / 47
37.
A solution is found to contain a Pb2+  of 0.10 M. What is the maximum SO42-  that
can exist in this solution before a precipitate forms?
A. SO42-  =1.8x10-9M
B. SO42-  =1.8x10-8M
C. SO42-  =1.8x10-7M
D. SO42-  =1.3x10-4M
38.
Which solute will result in a molecular solution?
A. HCN
B. Ba  OH2
C. CH3 COOH
D. CH3 CH2OH
39.
Which best describes the equilibrium in a saturated solution?
A. The rate of crystallization determines the solubility.
B. The rate of crystallization equals the rate of dissolving.
C. There is no solid solute on the bottom of the container.
D. The solute is completely dissolved and the equilibrium favours the products.
40.
A.
B.
C.
D.
Which compound will have a solubility greater than 0.1 M at 25°C?
SrS
CoS
BaSO4
41.
Ag2 SO4
What is the net ionic equation for the reaction between 0.10 M Na2 S and 0.10 M
Zn NO3 2 ?
A. Zn2= (aq)+S2- (aq)  ZnS(s)
B. Na+ (aq)+NO3- (aq)  NaNO3 (s)
C. Na2S(aq)+Zn NO3 2 (aq)  ZnS(s)+2NaNO3 (aq)
D. 2Na+ (aq)+S2- (aq)+Zn2+ (aq)+2NO3- (aq)  ZnS(s)+2Na+ (aq)+2NO3- (aq)
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 11 / 47
42.
When equal volumes of 0.20 M NaOH and 0.20 M CaS are mixed together…
A. a precipitate forms and the trial K sp would be less than K sp
B. no precipitate forms and the trial K sp would be less than K sp
C. a precipitate forms and the trial K sp would be greater than K sp
D. no precipitate forms and the trial K sp would be greater than K sp
43.
A.
B.
C.
D.
Which of the following solutes will produce a molecular solution?
HCl
Fe3 S3
HNO3
CH3 OH
44.
Which of the following would best describe the solubility of a solute?
A. litres per gram
B. moles per litre
C. grams per mole
D. moles per second
45.
Which compound will have the lowest solubility?
A. FeS
B. CaSO4
C. AgBrO3
D. Fe NO3 3
46.
A.
B.
C.
D.
Which of the following precipitates may form when equal volumes of 0.3 M AgNO3 ,
0.3 M SrCl2 and 0.3 M Na2 CO3 are mixed together?
SrCO3 and AgCl
Ag2 CO3 and AgCl
SrCO3 and Ag2 CO3
SrCO3 , Ag2 CO3 and AgCl
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 12 / 47
47.
An experiment is conducted to identify an unknown cation that is present in each of
four beakers.
Which of the following could be the unknown cation?
A.
B.
C.
D.
Ag
Fe3
Ba2
Be2
48.
Given the equilibrium reaction…
2NaNO3 (aq)  Ag2S(s)  2AgNO3 (aq)  Na2S(aq)
Which K sp expression best describes the net ionic reaction?
2
A. K sp   Ag  S2 
1
B. K sp 
2
 Ag  S2 
2
C. K sp
 Ag  S2 

 Ag2S
 AgNO3  Na2S
D. K sp 
2
NaNO3 
2
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 13 / 47
49.
Two salt solutions were mixed and a trial K sp was calculated to be 2.0x109 . The K sp
value is 1.0x1010 . From this information, which of the following is a true statement?
50.
A.
B.
C.
D.
3.4x103M
5.8x104M
1.0x104M
3.4x107M
51.
A.
B.
C.
D.
A saturated solution of SrSO4 has an SO42  of 1.0x104M . What is the Sr 2  ?
Which of the following would form a saturated solution when 0.010 mol of the solid
solute is added to 100 mL of water?
BaCO3
FeSO4
NaCN
Pb NO3 2
52.
Which net ionic equation best describes the reaction that exists in a solution prepared
by mixing equal volumes of 0.20 M Ca NO3 2 and 0.20 M Na2 CO3 ?
A. Ca2 (aq)  CO32 (aq)  CaCO3 (s)
B. Na (aq)  NO3  (aq)  NaNO3 (s)
C. Ca NO3 2 (aq)  Na2CO3 (aq)  2NaNO3 (s)  CaCO3 (s)
D. Ca NO3 2 (aq)  Na2CO3 (aq)  2NaNO3 (aq)  CaCO3 (s)
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 14 / 47
53.
Which compound will have the greatest solubility in water?
A. CuCl
B. FeCO3
C. MgSO4
D. Cu3 PO4 2
54.
A.
B.
C.
D.
Which cation below can be used to separate SO42 from S2 ions by precipitation?
Sr 2
Pb2
Cs
Be2
55.
What will be the effect of adding some solid AgNO3 to a saturated solution of AgCl ?
A. The AgNO3 will not dissolve
B. More solid AgCl will dissolve
C. More solid AgCl will be produced
D. The AgNO3 will not affect the AgCl equilibrium
56.
For a saturated solution, the K sp expression does not contain any solid solute term.
What is the reason for this?
A. The solid solute is a product
B. The solid solute is a reactant
C. The solid solute continues to change in amount
D. The solid solute does not change in concentration
57.
Which of the statements below describes the K sp expression for the salt barium
phosphate?
A. K sp  Ba2  PO43 
3
2
B. K sp  Ba2  PO43 
C. K sp  3Ba2  2PO43 
2
D. K sp  3Ba2  2PO43 
2
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 15 / 47
What is the solubility of Fe  OH2 ?
58.
A. 4.9x1017M
B. 1.2x1017M
C. 3.7x106M
D. 2.3x106M
Which of the following ions would have the highest concentration in 0.1 M CO32 ?
59.
A.
B.
C.
D.
Ba2
Ca2
Sr 2
Mg2
60.
A.
B.
C.
D.
Which of the solutes below can form an ionic solution with the highest conductivity?
PbS
CH3 Cl
NaNO3
CH3 COOH
61.
The following data was collected to determine the solubility of a substance…
Mass of solute dissolved 5.00 g
Volume of solvent 250.0 mL
Molar mass of solute 100.0 g/mol
Molar mass of solvent 20.0 g/mol
Which of the following best describes its solubility?
A.
B.
C.
D.
2.00x102 g/mL
5.00x102mol
0.250 mol
1.00 mol/L
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 16 / 47
62.
Which value best represents the total ion concentration when 0.10 moles of K 3PO4 is
present in 0.5 L of solution?
A. 0.1 M
B. 0.2 M
C. 0.4 M
D. 0.8 M
63.
What will happen when equal volumes of 0.20 M NH4 2 S and 0.20 M Sr  OH2 are
mixed?
A. SrS precipitates
B. NH4 OH precipitates
C. Both NH4 OH and SrS precipitate
D. No precipitate forms
64.
Which anion would be most effective in removing the cations responsible for hard
water?
A. S2
B. Cl
C. PO43
D. SO42
65.
Which of the following is the K sp expression for barium phosphate?
A. K sp  Ba2  PO43 
3
2
B. K sp  Ba2  PO43 
C. K sp  3Ba2  2PO43 
3
D. K sp  3Ba2  2PO43 
66.
2
The solubility of Mg  OH2 is found to be 1.2x104M . What is its K sp ?
A. 6.9x1012
B. 1.7x1012
C. 1.4x108
D. 1.2x104
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 17 / 47
67.
Which of the following is true for the salt SrF2 at 25 C?
A. It has a high solubility
B. It will not dissolve at all
C. Its solubility is 1.6x103M
D. Its solubility is 1.0x103M
68.
Which of the following ions could be used in the lowest concentration to remove Ag
ions from a polluted water sample?
A. I
B. Br 
C. BrO3 
D. CO32
69.
Which of the solutes below is both ionic and most soluble?
A. RbOH
B. CH3OH
C. Ca  OH2
D. Fe  OH3
70.
Which of the following is commonly used to describe the solubility of a solute?
A. mass of solute moles of solute
B. moles of solution mass of solute
C. mass of solute volume of solution
D. mass of solution volume of solute
71.
Given a saturated solution of Ca  OH2 which of the following statements is always
true?
A. The Ca2  is twice that of OH 
B. The OH precipitates half as fast as the Ca2
C. The rate of crystallization equals the rate of dissolving
D. The rate of dissolving is greater than the rate of crystallization
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 18 / 47
Solid NaCl is added to a saturated AgCl solution. How have the  Ag  and Cl 
changed when equilibrium has been re-established?
72.
Which of the following expressions represents Fe3  in a saturated Fe  OH3
solution?
73.
K sp
A.
3 OH 
K sp
B.
OH 
3
K sp
C.
3
OH 
D. K sp  OH 
74.
3
What is the value of K sp for Zn  OH2 if the solubility of Zn  OH2 is equal to
4.2x106M ?
A. 1.0x102
B. 4.0x103
C. 1.8x1011
D. 3.0x1016
75.
A.
B.
C.
D.
What is the maximum number of moles of Cl that can exist in 500.0 mL of 2.0 M
AgNO3 ?
4.5x1011
9.0x1011
1.8x1010
1.8x109
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 19 / 47
76.
What is the concentration of the ions in 3.0 L of 0.50 M Al2  SO4 3 ?
77.
Consider the following equilibrium…
MgCO3 (s)  Mg2 (aq)  CO32 (aq)
Adding which of the following would cause the solid to dissolve?
A. HCl
B. K 2 CO3
C. MgCO3
D. Mg NO3 2
78.
A.
B.
C.
D.
Which of the following compounds could be used to prepare a solution with a S2 
greater than 0.1 M?
ZnS
PbS
Ag2 S
Rb2 S
79.
Which of the following will not form a precipitate when mixed with an equal volume of
0.2 M AgNO3 ?
A. 0.2 M
B. 0.2 M
C. 0.2 M
D. 0.2 M
NaBr
NaIO3
NaNO3
NaBrO3
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 20 / 47
80.
How many moles of solute are dissolved in 200.0 mL of a saturated solution of FeS ?
A. 1.2x1019
B. 6.0x1019
C. 1.5x1010
D. 7.7x1010
81.
Consider the following 10.0 mL solutions…
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. Cl
B. Br 
C. IO3 
D. BrO3 
82.
Which of the following could dissolve a precipitate of CaC2 O4 in a saturated solution
of CaC2 O4 ?
A. NaOH
B. CaC2 O4
C. H2 C2 O4
D. Ca NO3 2
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 21 / 47
83.
Which of the following will dissolve in water to produce a molecular solution?
A. CaCl2
B. NaOH
C. CH3 OH
D. Sr  OH2
84.
In a solubility equilibrium, the…
A. rate of dissolving equals the rate of crystallization
B. neither dissolving nor crystallization are occurring
C. concentration of solute and solvent are always equal
D. mass of dissolved solute is greater than the mass of the solution
85.
Which of the following solutions would have Fe3   0.020M ?
A. 0.40 L of 0.050 M Fe NO3 3
B. 0.80 L of 0.020 M Fe2  SO4 3
C. 0.50 L of 0.040 M FeC6H5 O7
D. 0.50 L of 0.010 M Fe2  C2 O4 3
86.
A.
B.
C.
D.
Which of the following substances has the lowest solubility?
BaS
CuS
FeS
ZnS
87.
The complete ionic equation for the reaction between MgS and Sr  OH2 is…
A. MgS(aq)  Sr(OH)2 (aq)  Mg(OH)2 (s)  SrS(s)
B. MgS(aq)  Sr(OH)2 (aq)  Mg(OH)2 (s)  SrS(aq)
C. Mg2 (aq)  S2 (aq)  Sr 2 (aq)  2OH  Mg2 (aq)  2OH (aq)  SrS(s)
D. Mg2 (aq)  S2 (aq)  Sr 2 (aq)  2OH  Mg  OH2 (s)  Sr 2 (aq)  S2- (aq)
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 22 / 47
88.
Consider the following equilibrium…
Fe  OH2 (s)  Fe2 (aq)  2OH (aq)
Which of the following will cause the equilibrium to shift to the right?
A. adding KOH
B. adding Na2 S
C. adding Fe  OH2
D. adding Fe NO3 2
89.
Consider the following experiment…
The unknown solution could contain…
A. 0.20 M OH
B. 0.20 M NO3 
C. 0.20 M PO43
D. 0.20 M SO42
90.
A.
B.
C.
D.
A compound has a solubility of 7.1x105M at 25o C . The compound is…
CuS
AgBr
CaCO3
CaSO4
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 23 / 47
91.
A saturated solution of NaCl contains 36.5 g of solute in 0.100 L of solution. The
solubility of the compound is…
A. 0.062 M
B. 1.60 M
C. 3.65 M
D. 6.24 M
92.
Calculate the Li  in 200.0 mL of 1.5 M Li2 SO4 …
A. 0.30 M
B. 0.60 M
C. 1.5 M
D. 3.0 M
93.
When equal volumes of 0.20 M RbCl and 0.20 M SrS are combined…
A. no precipitate forms
B. a precipitate of Rb2 S only forms
C. a precipitate of SrCl2 only forms
D. precipitates of both Rb2 S and SrCl2 form
94.
A solution contains both Ag and Mg2 ions. During selective precipitation, these ions
are removed one at a time by adding…
A. I followed by OH
B. OH followed by S2
C. SO42 followed by Cl
D. NO3  followed by PO43
95.
A. K sp
The K sp expression for a saturated solution of Mg  OH2 is…
Mg2  OH 

Mg  OH2 
2
2
B. K sp  Mg2  OH 
C. K sp  Mg2  OH 
D. K sp  Mg2  2OH 
2
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 24 / 47
96.
Consider the following saturated solutions: CuSO4 , BaSO4 , CaSO4 . The order of
cation concentration, from highest to lowest, is…
A. Ba2   Ca2   Cu2 
B. Ca2   Cu2   Ba2 
C. Cu2   Ca2   Ba2 
D. Cu2   Ba2   Ca2 
97.
When 1.0x103moles of CuCl2 (s) are added to 1.0 L of 1.0x103M IO3  , the…
A. Trial K sp  K sp and a precipitate forms
B. Trial K sp  K sp and a precipitate forms
C. Trial K sp  K sp and no precipitate forms
D. Trial K sp  K sp and no precipitate forms
98.
Which of the following forms a molecular solution in water?
A. SrSO4
B. Na3PO4
C. C6H12 O6
D. NH4 CH3 COO
99.
Which of the following is necessary to form a saturated solution at equilibrium?
A. excess solute
B. an ionic solute
C. solute of low solubility
D. trial ion product is less than K sp
100.
Which of the following will produce a solution with the highest OH  ?
A. AgOH
B. Sr  OH2
C. Fe  OH3
D. Mg  OH2
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 25 / 47
Written Questions
1.
A 30.00 mL sample of a saturated solution of Ag2 SO4 was heated in an evaporating
dish until all the water was evaporated. The following data were recorded...
Calculate the K sp value for Ag2 SO4 . (5 marks)
2.
Consider the following equilibrium and accompanying graph...
Zn IO3 2 (s)  Zn2+ (aq)+2IO3- (aq)
A. Identify the stress applied at t1 . (1 mark)
Complete the above graph from t1 to t 3 for the IO3-  . (2 marks)
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 26 / 47
3.
Calculate the solubility of SrSO4 in grams per litre. (3 marks)
4.
A 100.0 mL saturated solution of FeF2 contains 0.0787 g of solute. Determine the
Fe2+  and the F-  in the solution. (3 marks)
5.
Consider the following information and the accompanying diagram. In a titration
experiment, AgNO3 (aq) was used to determine the Cl-  in a water sample and the
following data were recorded...
Ag+ (aq)+Cl- (aq)  AgCl(s)
 AgNO3 
0.125 M
Volume of water sample containing Cl-
20.00 mL
Initial buret reading of AgNO3
5.15 mL
Final buret reading of AgNO3
37.15 mL
Using the above data, determine the Cl-  in the water sample. (3 marks)
6.
Calculate the mass of NaI necessary to begin precipitation of Cu+ from a 250.0 mL
sample of 0.010 M CuNO3 . (4 marks)
7.
A. Write the net ionic equation for the reaction between Pb NO3 2 and NaCl . (2 marks)
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 27 / 47
B. Determine, with calculations, whether a precipitate will form when 15.0 mL of 0.050 M
Pb NO3 2 is added to 35.0 mL of 0.085 M NaCl . (4 marks)
8.
After a 50.0 mL sample of a saturated solution of Ag2 SO4 was heated to dryness,
7.2x10-4 g of solid Ag2 SO4 remained. What is the value of K sp for Ag2 SO4 ? (5
marks)
9.
Calculate the maximum mass of BaCl2 (s) that can be added to 250 mL of 0.50 M
Pb NO3 2 (aq) without forming a precipitate of PbCl2 (s) . (6 marks)
10.
Sufficient Na2 SO4 is added to 0.10 M Ba NO3 2 to cause a precipitate to form.
A. Write the net ionic equation for the precipitate formation. (1 mark)
B. Calculate the SO42-  at the moment the precipitate starts to form. (2 marks)
11.
Calculate the mass of solid AgNO3 that can be added to 2.0 L of a 0.10 M K 2 CrO4
solution in order to just start precipitation. (4 marks)
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 28 / 47
12.
A. How would a saturated solution be prepared at room temperature? (1 mark)
B. Write a chemical equation to illustrate the equilibrium that exists in a saturated solution of
Be3 PO4 2 . (2 marks)
13.
14.
Calculate the iodate ion concentration in a saturated copper (II) iodate solution at
25C. (3 marks)
A solution is prepared by mixing equal moles of Ba NO3 2 , K 2 SO4 , and BaS and
precipitation occurs. Identify the precipitate(s) and write the net ionic equation
Precipitate
(1 mark)
Net Ionic Equation
(2 marks)
15.
What is the maximum Pb2+  that can exist in a saturated solution of BaSO4 without
causing precipitate formation? (4 marks)
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 29 / 47
16.
Consider the equilibrium for a saturated solution of CaCO3 ...
CaCO3 (s)  Ca2+ +CO32What is the maximum Mg2+  that can exist in a saturated solution of CaCO3 without causing
a precipitate to form? (4 marks)
17.
Consider the equilibrium for a saturated solution of PbI2 (s) ...
PbI2 (s)  Pb2+ (aq)+2I- (aq)
What is the maximum  Ag+  that can exist in a saturated solution of PbI2 (s) without causing
a precipitate to form? (4 marks)
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 30 / 47
18.
Consider the following equilibrium...
Mg  OH2 (s)  Mg2+ (aq)+2OH- (aq)
A. What happens to the amount of solid Mg  OH2 (s) when some HCl(aq) is added? (1 mark)
B. On the graph below, sketch the effect of adding HCl(aq) at time t1 . (3 marks)
19.
Will a precipitate form when 10.0 mL of 1.0 M Pb NO3 2 is mixed with 40.0 mL of
2.0x10-2M NaCl ? Justify your answer. (4 marks)
20.
At 25°C, will a precipitate form when 25.0 mL of 0.010 M Pb NO3 2 is combined with
75.0 mL of 0.010 M NaI ? Support your answer with calculations. (3 marks)
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 31 / 47
21.
Write the complete ionic equation for the reaction between NaBrO3 and AgNO3 . (1
mark)
A. Complete Ionic Equation
B. What is the maximum NaBrO3  that can exist in equilibrium with 2.0 M AgNO3 ? (2 marks)
22.
Write the balanced complete ionic equation for the reaction that occurs when 0.20 M
of Ba NO3 2 is added to an equal volume of 0.20 M Na2 CO3 . (2 marks)
Complete Ionic Equation
23.
Calculate the minimum number of moles of Pb NO3 2 required to start precipitation in
50.0 mL of 0.15 M ZnI2 . (5 marks)
24.
In a titration, 25.00 mL of NaCl(aq) reacts completely with 42.20 mL of 0.100 M
AgNO3 .
What is the Cl  in the original solution? (3 marks)
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 32 / 47
25.
The following data was obtained when 20.0 mL of a saturated solution of PbI2 was
evaporated to dryness.
Use this information to determine the K sp of PbI2 . (4 marks)
26.
Calculate the molar solubility of SrF2 . (4 marks)
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 33 / 47
Multiple Choice Questions Answer Key
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
19
20
B
A
A
B
C
D
C
D
D
C
B
C
B
A
C
D
B
D
B
C
21
22
23
24
25
26
27
28
29
30
31
32
33
34
35
36
37
38
39
40
A
D
A
C
D
B
B
A
A
C
A
B
D
C
B
A
C
D
B
A
41
42
43
44
45
46
47
48
49
50
51
52
53
54
55
56
57
58
59
60
A
C
D
B
A
D
B
A
B
A
A
A
C
A
C
D
B
D
D
C
61
62
63
64
65
66
67
68
69
70
71
72
73
74
75
76
77
78
79
80
A
D
D
C
B
A
D
A
A
C
C
B
B
D
A
B
A
D
C
C
81
82
83
84
85
86
87
88
89
90
91
92
93
94
95
96
97
98
99
100
D
A
C
A
D
B
D
B
A
C
D
D
A
A
B
C
D
C
A
B
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 34 / 47
Written Questions Answer Key
1.
2.
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 35 / 47
3.
4.
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 36 / 47
5.
6.
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7.
8.
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 38 / 47
9.
10.
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 39 / 47
11.
12.
(03062004)
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 40 / 47
13.
14.
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 41 / 47
15.
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 42 / 47
16.
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 43 / 47
17.
18.
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 44 / 47
19.
20.
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 45 / 47
21.
22.
R. Janssen, MSEC Chemistry 12 Provincial Workbook (Unit 03), P 46 / 47
23.
24.
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25.
26.