CHEMISTRY 11 ANSWERS TO REVIEW SHEET
1.
2.
An old barometer hanging on the wall of a mountain hut has a reading of 25.5 inches of mercury. If 1 inch of mercury equals 0.0334 atm (atmoshperes) and 1 atm = 101.3 kPa and 1 kPa = 7.50 torr. What is the pressure reading of the barometer in torr?
If sugar is $9.80 for 10 kg, what is the cost of: (a) 90.0 kg of sugar? (b) 6.00 tonnes of sugar (recall 1 tonne = 1000 kg)?
QUANTITY WRITTEN UNIT UNIT SYMBOL length mass time amount of substance volume
WRITTEN PREFIX AND UNIT PREFIX AND UNIT SYMBOLS EXPONENTIAL EQUIVALENTS
1.3 kilograms
38.3 dekametres
1.25 µmol
37.5 mmol
93.5 cL
7.25 x 10 6 t
REVIEW FOR FINAL EXAMINATION 1

CHEMISTRY 11 ANSWERS TO REVIEW SHEET
3. Convert the following:
4.
5.
6.
7.
8.
(a) 2.25 mL into L (c) 3125 ML into kL
If 1 L of granite has a mass of 5.50 kg,
(a) what is the mass of 7.00 L of granite?
(e) 25 cm/µs into km/s
(b) what is the volume occupied by 22 kg of granite?
A student measured the volume of an iron nail to be 0.880 mL and found that the mass was 6.92 g. What is the density of the iron?
A sample of vegetable oil had a density of 0.916 g/mL. Calculate the mass of 0.250 L of the oil.
What volume would 2.86 g of silver occupy? The density of silver is 10.5 g/mL.
Write the following numbers in scientific notation:
(a) 23 000 (c) 21 700 000 (e) 95 007 000
9. Write the following numbers in decimal notation:
(a) 2.25 x 10 3 (c) 3.125 x 10 -4 (e) 2.57 x 10 6
10. How many significant figures does each of the following measurements have?
(a) 3218.04 cm (c) 6.84 x 10 -4 mmol (e) 2500 s
(b) 250.000 mL (d) 9 000 000 µs (f) 5.2500 x 106 cg
REVIEW FOR FINAL EXAMINATION 2

CHEMISTRY 11
11. Determine the volumes of the following graduated cylinders:
ANSWERS TO REVIEW SHEET
12. Determine the reading on the following scales:
13 State the rule for rounding to the correct number of significant figures after multiplying or dividing numbers.
REVIEW FOR FINAL EXAMINATION 3

CHEMISTRY 11 ANSWERS TO REVIEW SHEET
14. Perform the indicated operations and the give the answer to the correct number of significant figures.
(a)
(b)
35.8 x 0.12
128.62 ÷ 9.25
(d) 1750 x (6.7254 x 10 2 )
(e) (6.1428 x 10 3 ) ÷ 0.004810
15. In the following mixed calculations perform multiplications and divisions before doing the additions and subtractions. Keep track of the number of significant figures at each stage of a calculation.
(a) 65.00 x 0.24000 – 15.78 x 0.148
(d)
16. Which of the following statements describe physical properties and which describe chemical properties?
(a) glass is transparent (d) copper conducts electricity
(b) salt melts at 801°C
(c) Adding lye to fat makes soap
(e) fumes from ammonia and hydrochloric acid mix to produce a white smoke
17. Which of the following are intensive properties and which are extensive?
(a) shape
(b) smell
(c)
(d) length colour
18. Briefly describe the characteristics of solids, liquids, and gases.
(e) time to dissolve
(f) density
19. Classify each of the following as one of element, compound, solution, or mechanical mixture.
(a) gravel
(b) coffee
(d)
(e) iron water
(g)
(h) orange juice ammonia
REVIEW FOR FINAL EXAMINATION 4

CHEMISTRY 11 ANSWERS TO REVIEW SHEET
20. Classify each of the following as one of an atom, molecule, or ion.
(a) NH
3
(b) Cr
2
O
7
2-
(c)
(d)
Pb
PCl
5
(e) SO
4
2-
(f) Co
21. How can you separate all the components in a mixture containing sand, iron filings, water, gasoline, red water-soluble dye, and blue water-soluble dye? In pure form the dyes are powders.
22. Which of the following represents the cooling curve for a pure substance. Explain how you know. (Bonus).
23. Classify each of the following as either a chemical (primarily) or physical change.
(a) formation of fog (d) rusting nail
(b)
(c) burning paper plant growing
24. List 4 characteristics of metals.
(e) dissolving salt into water
(f) filtering sand and water
25. List 4 characteristics of nonmetals.
REVIEW FOR FINAL EXAMINATION 5

CHEMISTRY 11 ANSWERS TO REVIEW SHEET
26. Indicate which terms apply to each species. There is more than one term which applies to each species.
N (neutral) C (cation) A (anion)
M (monatomic) D (diatomic) P (polyatomic)
(a) SO
4
2-
(b) NH
3
(c) Ba 2+
(d) ClO -
(e) N
2
H
5
+
(f) Fe
27. Write the formulae for the following ionic compounds.
(a) calcium dihydrogen phosphate (b) uranium (IV) sulphate
28. Name the following ionic compounds.
(a) Ag
3
PO
4
(b) Na
2
HPO
4
29. Write the formulae for the following covalent compounds.
(b) oxygen diiodide (a) diphosphorus trichloride
30. Name the following covalent compounds.
(a) S
4
N
2
(b) ClF
3
31. Write the formulae for the following hydrated compounds.
(a) zinc perchlorate hexahydrate (b) iron (III) sulphate nonhydrate
32. Name the following hydrated compounds.
(a) FeSO
4
•5H
2
O (c) Co
3
(PO
4
)
2
•8H
2
O
33. Write the formulae for the following acids.
(a) sulphuric acid
(b) nitric acid
(c) acetic acid
(d) hydrochloric acid
REVIEW FOR FINAL EXAMINATION 6

CHEMISTRY 11 ANSWERS TO REVIEW SHEET
34. Name the following acids.
(a) HF
(b) H
2
SO
3
(c) H
3
PO
4
(d) HNO
2
35. Review the following terms : Avogadro’s hypothesis, mole, atomic mass, molar mass, molar volume, STP, density, empirical formula, molecular formula, empirical mass, concentration, dilution, molarity.
36. Calculate the molar mass of each of the following.
(a)
NCl
3
(b) Al
37. Calculate the molar mass of each of the following.
2
(SO
4
)
3
(a) NiSO
4
•7H
2
O (b) Cr(NO
3
)
3
•9H
2
O
38. Calculate the mass of the following.
(a) 4.50 mol of PCl
3
(b) 5.64 x 10 -5 mol of AuCl
3
39. Calculate the number of moles in the following.
(a) 85.6 g of CaO (b) 6.48 kg of KMnO
4
40. Calculate the molar mass of 0.00496 mol sample of cholesterol has a mass of 1.894 g
41. What is STP and what are the experimental conditions of STP?
REVIEW FOR FINAL EXAMINATION 7

CHEMISTRY 11 ANSWERS TO REVIEW SHEET
42. Calculate the volume at STP occupied by the following.
(a)
24.8 mol of NH
3
(b) 0.0861 mol of HCl
43. Calculate the number of moles in the following gases at STP.
(a) 64.8 L of Xe
(g)
(b) 645 mL of SO
2(g)
44. How many atoms are contained in the following.
(a) 1 molecule of CH
3
CO
2
H (b) 2.56 mol of (NH
4
)
3
PO
4
45. Find the mass, in grams, of each of the following.
(a) 1 Pb atom (b) 5.62 x 10 18 Fe(OH)
3
molecules
46. How many atoms are contained in each of the following?
(a) 60.5 g of AlCl
3
(b) 84.6 mL of HCl
(g)
at STP
47. What volume at STP is occupied by each of the following?
(a) 8.27 x 10 20 molecules of O
2(g)
(b) 125.0 g of Cl
2(g)
48. Calculate the percentage composition of the following.
(a) NaHCO
3
(b) CuSO
4
•5H
2
O
49. Calculate the percentage composition of the bold species in each of the following.
(a) Cr( NO
3
)
6
Cl
3
•H
2
O (b) Al
2
( SO
4
)
3
•18H
2
O
REVIEW FOR FINAL EXAMINATION 8

CHEMISTRY 11 ANSWERS TO REVIEW SHEET
50. Find the empirical formula for the following compounds.
(a) 12.6% Li, 29.2% S, 58.2% O (b) 38.8% Fe, 16.7% C, 44.5% O
51. A gas has the empirical formula CH
2
. If 0.550 L of the gas at STP has a mass of 3.44 g, what is the molecular formula?
52. A sample of gas is analyzed and found to contain 33.0% Si and 67.0% F. If the gas has a density of 7.60 g/L at STP, what is the molecular formula?
53. Calculate the molar concentration of the following solutions.
(a) 0.578 mol of NaCl in 52.0 mL of solution
(b) 50.0 g of Fe(NO
3
)
3
in 150.0 mL of solution
54. Calculate the mass of solute needed to make the following solutions.
(a) 125.0 mL of 0.0750 M KOH, from solid KOH
(b) 500.0 mL of 0.120 M FeCl
3
, from solid FeCl
3
•6H
2
O
55. What is the concentration of the solution that results when 250.0 mL of water is added to
550.0 mL of 3.50 M NaOH?
56. If 500.0 mL of 0.100 M LiOH is boiled down to 200.0 mL, what is the concentration?
57. What is the resulting concentration when 500.0 mL of 0.250 M NaCl is mixed with
250.0 mL of 0.450 M NaCl and the mixture is boiled down to 400.0 mL?
58. If 250.0 mL of solution A containing 28.0 g of LiOH is mixed with 500.0 mL of solution B containing 56.0 g of LiOH and the resulting solution is boiled down to
600.0 mL, what is the concentration?
59. How can you tell that a chemical reaction has occurred?
REVIEW FOR FINAL EXAMINATION 9

CHEMISTRY 11 ANSWERS TO REVIEW SHEET
60. What is the Law of Conservation of Mass?
61. How can you tell that a chemical equation is balanced?
3. Balance the following chemical reactions:
A. ___ Si
4
H
10
+ ___ O
2
 ___ SiO
2
+ ___ H
2
O
B. ___ Ca
3
(PO
4
)
2
+ ___ SiO
2
+ ___ C  ___ CaSiO
3
+ ___ CO + ___ P
4
C. ___ C
3
H
7
N
2
O
7
+ ___ O
2
 ___ CO
2
+ ___ H
2
O + ___ N
2
62. Write and balance the following word equations:
A. Aluminum + Copper (II) sulphate  Aluminum sulphate + Copper
__________________________________________________________________
B. Magnesium nitride + Water  Magnesium hydroxide + Ammonia (NH
3
)
__________________________________________________________________
C. Calcium hydroxide + Ammonium chloride  Ammonia + Calcium chloride +
Water
__________________________________________________________________
63. Complete and balance the following reactions and classify each equation as one of: synthesis, decomposition, single replacement, double replacement, neutralization or combustion.
A. ___ HF + ___ Fe(OH)
3
 ____________________________________________
B. ___ FeCl
2
+ ___ K
2
S  ______________________________________________
C. ___ Al + ___ S
8
 __________________________________________________
D. ___ N
2
O  _______________________________________________________
E. ___ C
3
H
6
OS
2
+ ___ O
2
 ____________________________________________
F. ___ Mg + ___ HCl  _______________________________________________
REVIEW FOR FINAL EXAMINATION 10

CHEMISTRY 11 ANSWERS TO REVIEW SHEET
64. Define the terms:
A. Exothermic
B. Endothermic
65. Classify the following is exothermic or endothermic:
A. 2Na + 2H
2
O  2NaOH + H
2
+ 283 kJ
B. KClO
3
+ 41.4 kJ  K + + ClO
3
–
C. C
2
H
6
+ O
2
 CO
2
+ H
2
O ∆H = – 3718 kJ
D. 12CO
2
+ 11H
2
O  C
12
H
22
O
11
+ 12O
2
∆H = +5638 kJ
66. What are limiting and excess reactants?
67. Consider the reaction: 4C
4
H
9
SO
2
+ 25O
2
 16CO
2
+ 18H
2
O + 4SO
2
A. How many oxygen molecules react with 20 molecules of C
4
H
9
SO
2
?
B. How many moles of C
4
H
9
SO
2
are required to produce 100 moles of water?
C. What mass of SO
2
is formed when 50.0 g of C
4
H
9
SO
2
is reacted?
68. A 25.0 mL sample of Al(OH)
3
is titrated with 67.8 mL of 0.450 M HCl according to the reaction
Al(OH)
3
+ 3HCl  AlCl
3
+ 3H
2
O
What is the concentration of the original Al(OH)
3
solution?
REVIEW FOR FINAL EXAMINATION 11

CHEMISTRY 11 ANSWERS TO REVIEW SHEET
69. What mass of CS
2
is produced when 25.8 g of C are reacted with 54.2 g of SO
2
according to the equation
5C + 2SO
2
 CS
2
+ 4CO
A. What mass of CS
2
is produced?
B. What mass of the excess reactant will be left over?
70. Consider the reaction
K
2
Cr
2
O
7
+ 6NaI + 7H
2
SO
4
 Cr
2
(SO
4
)
3
+ 3I
2
+ 7H
2
O + 3Na
2
SO
4
+ K
2
SO
4
A 35.0 g sample of pure K
2
Cr
2
O
7
produces 9.67 g of H
2
O. What is the percentage yield
.
72. Fill in the following table:
SYMBOL
Rh
107 Pd 2+
123 Sb 3–
PROTONS
93
50
NEUTRON ELECTRONS
89
46
REVIEW FOR FINAL EXAMINATION 12

CHEMISTRY 11 ANSWERS TO REVIEW SHEET
1.
2.
An old barometer hanging on the wall of a mountain hut has a reading of 25.5 inches of mercury. If 1 inch of mercury equals 0.0334 atm (atmoshperes) and 1 atm = 101.3 kPa and 1 kPa = 7.50 torr. What is the pressure reading of the barometer in torr? 647 torr
If sugar is $9.80 for 10 kg, what is the cost of: (a) 90.0 kg of sugar? $88.20 (b) 6.00 tonnes of sugar (recall 1 tonne = 1000 kg)? $5.88E3
QUANTITY WRITTEN UNIT UNIT SYMBOL length mass time amount of substance volume
WRITTEN PREFIX AND UNIT
1.3 kilograms
1.25 micromoles
7.25 megatonnes
37.5 millimoles
38.3 dekametres
93.5 centilitres
3. Convert the following:
Metre g
Second
Mole
Litre
PREFIX AND UNIT SYMBOLS
1.3 kg
1.25 µmol
7.25 Mt
37.5 mmol
38.3dam
93.5 cL
M g
S
Mol
L
EXPONENTIAL EQUIVALENTS
10 3
1.25 E -6
7.25 x 10 6 t
37.5E-3 mol
38.3 E1 m
93.5 E-2 L
REVIEW FOR FINAL EXAMINATION 13

CHEMISTRY 11 ANSWERS TO REVIEW SHEET
4.
(a) 2.25 mL into L (c) 3125 ML into kL
2.25E-3L 3.125E6 kL
If 1 L of granite has a mass of 5.50 kg,
(a) what is the mass of 7.00 L of granite? 38.5 kg
(e) 25 cm/µs into km/s
2.5 E 2 km/s
5.
6.
7.
8.
9.
(b) what is the volume occupied by 22 kg of granite? 4L
A student measured the volume of an iron nail to be 0.880 mL and found that the mass was 6.92 g. What is the density of the iron? 7.86 g/mL
A sample of vegetable oil had a density of 0.916 g/mL. Calculate the mass of 0.250 L of the oil. 229g
What volume would 2.86 g of silver occupy? The density of silver is 10.5 g/mL..
0.272mL
Write the following numbers in scientific notation:
(a) 23 000, 2.3E4 (c) 21 700 000, 2.17E7 (e) 95 007 000,
9.5007E7
Write the following numbers in decimal notation:
(a) 2.25 x 10 3 , 2250 (c) 3.125 x 10 -4
, (e)
2.57 x 10 6
0.0003125
2 570 000
10. How many significant figures does each of the following measurements have?
(a) 3218.04 cm 6
(b) 250.000 mL 6
(c) 6.84 x 10 -4 mmol 3 (e) 2500 s 2
(d) 9 000 000 µs 1 (f) 5.2500 x 10 -6 cg 5
REVIEW FOR FINAL EXAMINATION 14

CHEMISTRY 11
11. Determine the volumes of the following graduated cylinders:
ANSWERS TO REVIEW SHEET
54.2+/-.1 82+/-1
12. Determine the reading on the following scales:
38.0+/-.5
15.17+-.01 15.69+-.01
10.0+-.02 16.4+-.02
6.40+-.05 7.60+-.05
13 State the rule for rounding to the correct number of significant figures after multiplying or dividing numbers. Lowest number for mult and div, only one uncertain column for add and sub
REVIEW FOR FINAL EXAMINATION 15

CHEMISTRY 11 ANSWERS TO REVIEW SHEET
14. Perform the indicated operations and the give the answer to the correct number of significant figures.
(a)
(b)
35.8 x 0.12 =4.3
128.62 ÷ 9.25=13.9
(d) 1750 x (6.7254 x 10 2 )=1.18E6
(e) (6.1428 x 10 3 ) ÷ 0.004810=
1.277E6
15. In the following mixed calculations perform multiplications and divisions before doing the additions and subtractions. Keep track of the number of significant figures at each stage of a calculation.
(a) 65.00 x 0.24000 – 15.78 x 0.148
=13.26
(d) =3E2
16. Which of the following statements describe physical properties and which describe chemical properties?
(a) glass is transparent P (d) copper conducts electricity P
(b) salt melts at 801°C P (e) fumes from ammonia and
(c) Adding lye to fat makes soap C hydrochloric acid mix to produce a white smoke C
17. Which of the following are intensive properties and which are extensive?
(a) shape e (c) length e (e)time to dissolve e
(b) smell i (d) colour i (f) density i
18. Briefly describe the characteristics of solids (fixed shape and volume, particles touching with only vibrations), liquids (fixed volume, particles can slide past one another, and gases (particles move quickly and are separated by lots of space).
REVIEW FOR FINAL EXAMINATION 16

CHEMISTRY 11 ANSWERS TO REVIEW SHEET
19. Classify each of the following as one of element, compound, solution, or mechanical mixture.
(a) gravel m
(b) coffee s
(d)
(e) iron e water c
(g)
(h) orange juice m ammonia c
20. Classify each of the following as one of an atom, molecule, or ion.
(a) NH
3 m (c) Pb a (e) SO
4
2 i
(b) Cr
2
O
7
2 i (d) PCl
5
m (f) Co a
21. How can you separate all the components in a mixture containing sand, iron filings, water, gasoline, red water-soluble dye, and blue water-soluble dye? In pure form the dyes are powders…magnet (iron), filter (sand), sep funnel (gas), evaporate (water), chromatography (dyes)
REVIEW FOR FINAL EXAMINATION 17

CHEMISTRY 11 ANSWERS TO REVIEW SHEET
22. Which of the following represents the cooling curve for a pure substance. Explain how you know.
23. Classify each of the following as either a chemical (primarily) or physical change.
(a) formation of fog p
(b) burning paper c
(d) rusting nail c
(e) dissolving salt into water p
(c) plant growing c (f) filtering sand and water p
24. List 4 characteristics of metals. Shiny, ductile, malleable, conductor
25. List 4 characteristics of nonmetals. Brittle, dull, poor conductor, usually gas
26. Indicate which terms apply to each species. There is more than one term which applies to each species.
N (neutral) C (cation) A (anion)
M (monatomic) D (diatomic) P (polyatomic)
(a) A, P, SO
4
2-
(b) N, P, NH
3
(c) C, M, Ba 2+
(d) A, D, ClO -
(e) C, P, N
2
H
5
+
(f) N, M, Fe
REVIEW FOR FINAL EXAMINATION 18

CHEMISTRY 11 ANSWERS TO REVIEW SHEET
27. Write the formulae for the following ionic compounds.
(a) calcium dihydrogen phosphate (b) uranium (IV) sulphate
Ca
2
(H
2
PO
4
)
2
U(SO
4
)
2
28. Name the following ionic compounds.
(a) Ag
3
PO
4 (b)
Na
2
HPO
4
Silver phosphate sodium monohydrogen phosphate
29. Write the formulae for the following covalent compounds.
(a) diphosphorus trichloride P
2
Cl
3
(b) oxygen diiodide OI
2
30. Name the following covalent compounds.
(a) S
4
N
2 tetrasulphur dinitride (b) ClF
3
Chlorine trifluoride
31. Write the formulae for the following hydrated compounds.
(a) zinc perchlorate hexahydrate (b) iron (III) sulphate nonhydrate
Zn(ClO
4
)
2
.6H
2
O Fe
2
(SO
4
)
3
.9H
2
O
32. Name the following hydrated compounds.
(a) FeSO
4
•5H
2
O (b) Co
3
(PO
4
)
2
•8H
2
O
Cobalt (II) phosphate octahydrate Iron (II) sulphate pentahydrate
33. Write the formulae for the following acids.
(a) sulphuric acid H
2
SO
4
(c) acetic acid CH
3
COOH
(d) hydrochloric acid HCl (b) nitric acid HNO
3
34. Name the following acids.
(a) HF hydrofluoric acid
(b) H
2
SO
3 sulphurous acid
(c)
(d)
H
3
PO
HNO
4
2
phosphoric acid nitrous acid
REVIEW FOR FINAL EXAMINATION 19

CHEMISTRY 11 ANSWERS TO REVIEW SHEET
36. Calculate the molar mass of each of the following.
(b)
NCl
3
120.5g/mol
(c)
Al
2
(SO
342.3g/mol
4
)
3
37. Calculate the molar mass of each of the following.
(a) NiSO
4
•7H
2
O (b) Cr(NO
3
)
3
•9H
2
O
280.8g/mol 400.0g/mol
38. Calculate the mass of the following.
(a) 4.50 mol of PCl
3
(b) 5.64 x 10 -5 mol of AuCl
3
619 g
39. Calculate the number of moles in the following.
0.0171 g
(a) 85.6 g of CaO (b) 6.48 kg of KMnO
4
1.53 mol 41.0 mol
40. Calculate the molar mass of 0.00496 mol sample of cholesterol has a mass of 1.894 g.
382 g/mol
41. What is STP and what are the experimental conditions of STP? Standard temp (0
o C) and pressure (101.3 kPa)
42. Calculate the volume at STP occupied by the following.
(c)
24.8 mol of NH
3
(c) 0.0861 mol of HCl
556 L 1.93L
43. Calculate the number of moles in the following gases at STP.
REVIEW FOR FINAL EXAMINATION 20

CHEMISTRY 11 ANSWERS TO REVIEW SHEET
(a) 64.8 L of Xe
(g)
= 2.89 mol (b) 645 mL of SO
2(g)
= 2.88E-2 mol
44. How many atoms are contained in the following.
(a) 1 molecule of CH
3
CO
2
H (b) 2.56 mol of (NH
4
)
3
PO
4
8 3.08E25
45. Find the mass, in grams, of each of the following.
(a) 1 Pb atom (b) 5.62 x 10 18 Fe(OH)
3
molecules
3.44E-22 g 9.97E-4 g
46. How many atoms are contained in each of the following?
(a) 60.5 g of AlCl
3
= 1.09E24 (b) 84.6 mL of HCl
(g)
at STP=
4.55E21
47. What volume at STP is occupied by each of the following?
(a) 8.27 x 10 20 molecules of O
2(g)
(b) 125.0 g of Cl
2(g)
30.1mL 39.4L
48. Calculate the percentage composition of the following.
(a) Na (27.4)H (1.2)C (14.3) O
3
(57.1) (c) CuSO
4
•5H
2
O
Cu-25.4, S-12.1, O-57.7, H-4.0
49. Calculate the percentage composition of the bold species in each of the following.
(a) Cr( NO
3
)
6
Cl
3
•H
2
O (b) Al
2
( SO
4
)
3
•18H
2
O
67.8% 43.3%
50. Find the empirical formula for the following compounds.
(a) 12.6% Li, 29.2% S, 58.2% O
Li
2
SO
4
(b) 38.8% Fe, 16.7% C, 44.5% O
FeC
2
O
4
REVIEW FOR FINAL EXAMINATION 21

CHEMISTRY 11 ANSWERS TO REVIEW SHEET
51. A gas has the empirical formula CH
2
. If 0.550 L of the gas at STP has a mass of 3.44 g, what is the molecular formula? C
10
H
20
52. A sample of gas is analyzed and found to contain 33.0% Si and 67.0% F. If the gas has a density of 7.60 g/L at STP, what is the molecular formula? Si
2
F
6
53. Calculate the molar concentration of the following solutions.
(a) 0.578 mol of NaCl in 52.0 mL of solution. 11.1M
(b) 50.0 g of Fe(NO
3
)
3
in 150.0 mL of solution 1.38M
54. Calculate the mass of solute needed to make the following solutions.
(a) 125.0 mL of 0.0750 M KOH, from solid KOH 0.526g
(b) 500.0 mL of 0.120 M FeCl
3
, from solid FeCl
3
•6H
2
O
55. What is the concentration of the solution that results when 250.0 mL of water is added to
550.0 mL of 3.50 M NaOH? 2.41M
56. If 500.0 mL of 0.100 M LiOH is boiled down to 200.0 mL, what is the concentration?
0.25M
57. What is the resulting concentration when 500.0 mL of 0.250 M NaCl is mixed with
250.0 mL of 0.450 M NaCl and the mixture is boiled down to 400.0 mL?0.594M
58. If 250.0 mL of solution A containing 28.0 g of LiOH is mixed with 500.0 mL of solution B containing 56.0 g of LiOH and the resulting solution is boiled down to
600.0 mL, what is the concentration? 5.86M
59. How can you tell that a chemical reaction has occurred?
New properties due to new substances.
(d) What is the Law of Conservation of Mass?
Mass of products = mass of reactants in a closed reaction
REVIEW FOR FINAL EXAMINATION 22

CHEMISTRY 11 ANSWERS TO REVIEW SHEET
60.
How can you tell that a chemical equation is balanced? a.
Equal #s of atoms on each side
61. Balance the following chemical reactions:
A. 2 Si
4
H
10
+ 13 O
2
 8 SiO
2
+ 10 H
2
O
B. 2 Ca
3
(PO
4
)
2
+ 6 SiO
2
+ 10 C  6 CaSiO
3
+ 10 CO + 1 P
4
C. 4C
3
H
7
N
2
O
7
+ 5 O
2
 12 CO
2
+ 14 H
2
O + 4 N
2
62. Write and balance the following word equations:
A. Aluminum + Copper (II) sulphate  Aluminum sulphate + Copper
2Al + 3CuSO
4
 1Al
2
(SO
4
)
3
+ 3Cu
B. Magnesium nitride + Water  Magnesium hydroxide + Ammonia (NH
3
)
1Mg
3
N
2
+ 6H
2
O  3Mg(OH)
2
+ 2NH
3
C. Calcium hydroxide + Ammonium chloride  Ammonia + Calcium chloride +
Water
1Ca(OH)
2
+ 2NH
4
Cl  2NH
3
+ 1CaCl
2
+ 2H
2
O
63. Complete and balance the following reactions and classify each equation as one of: synthesis, decomposition, single replacement, double replacement, neutralization or combustion.
A. 3 HF + 1 Fe(OH)
3
 neut 3H
2
O + 1FeF
3
B. 1 FeCl
2
+ 1K
2
S  dr 1FeS + 2KCl
C. 16 Al + 3 S
8
 syn 8Al
2
S
3
D. 2N
2
O  decom 2N
2
+ 1O
2
E. 1C
3
H
6
OS
2
+ ___ O
2
 combust 3CO
2
+ 3H
2
O + 2SO
2
F. 1 Mg + 2 HCl  s.r. 1MgCl
2
+ 2H
2
64. Define the terms:
A. Exothermic
Heat exits the system
REVIEW FOR FINAL EXAMINATION 23

CHEMISTRY 11 ANSWERS TO REVIEW SHEET
B. Endothermic
Heat enters the system
65. Classify the following is exothermic or endothermic:
A. 2Na + 2H
2
O  2NaOH + H
2
+ 283 kJ ex
B. KClO
3
+ 41.4 kJ  K + + ClO
3
– en
C. C
2
H
6
+ O
2
 CO
2
+ H
2
O ∆H = – 3718 kJ ex
D. 12CO
2
+ 11H
2
O  C
12
H
22
O
11
+ 12O
2
∆H = +5638 kJ en
65. What are limiting (runs out and determines the amount of product) and excess (there is more than is needed to fully react with the limiting reactant )reactants?
66. Consider the reaction: 4C
4
H
9
SO
2
+ 25O
2
 16CO
2
+ 18H
2
O + 4SO
2
A. How many oxygen molecules react with 20 molecules of C
4
H
9
SO
2
?
125
B. How many moles of C
4
H
9
SO
2
are required to produce 100 moles of water?
22.2
C. What mass of SO
2
is formed when 50.0 g of C
4
H
9
SO
2
is reacted? 26.5g
67. A 25.0 mL sample of Al(OH)
3
is titrated with 67.8 mL of 0.450 M HCl according to the reaction
Al(OH)
3
+ 3HCl  AlCl
3
+ 3H
2
O
What is the concentration of the original Al(OH)
3
solution? 0.407M
68. What mass of CS
2
is produced when 25.8 g of C are reacted with 54.2 g of SO
2
according to the equation
5C + 2SO
2
 CS
2
+ 4CO
REVIEW FOR FINAL EXAMINATION 24

CHEMISTRY 11 ANSWERS TO REVIEW SHEET
A. What mass of CS
2
is produced? 32.2g
B. What mass of the excess reactant will be left over? 0.4g C
69. Consider the reaction
K
2
Cr
2
O
7
+ 6NaI + 7H
2
SO
4
 Cr
2
(SO
4
)
3
+ 3I
2
+ 7H
2
O + 3Na
2
SO
4
+ K
2
SO
4
A 35.0 g sample of pure K
2
Cr
2
O
7
produces 9.67 g of H
2
O. What is the percentage yield?
64.5%
71. Fill in the following table:
SYMBOL
Rh
107 Pd 2+
123 Sb 3–
237 Np 4+
119 Sn 4+
PROTONS
45
46
51
93
50
NEUTRON
58
61
72
144
69
ELECTRONS
45
44
54
89
46
REVIEW FOR FINAL EXAMINATION 25