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Chemistry 30
Review of Chemistry 20 Workbook
Review of Nomenclature
Formula
1.
NaHCO3(s)
sodium silicate
2.
3.
HgS(s)
4.
Na2SO4  4H2O(s)
5.
H2SO4(aq)
sucrose
6.
7.
Fe2O3(s)
magnesium hydroxide
8.
9.
NaHSO4(s)
oxygen
10.
11.
NaHSO3(s)
iron (II) carbonate
12.
13.
IUPAC Name
H2S(aq)
dinitrogen tetraoxide
14.
15.
CaSO4 2H2O(s)
16.
CH3OH(l)
17.
chlorine
18.
ammonium dihydrogen phosphate
19.
CH3COOH(aq)
20.
carbon tetrachloride
21.
magnesium sulphate heptahydrate
22.
Na2S2O3 5H2O(s)
23.
C2H6(g)
24.
SO2(g)
25.
calcium phosphate
26.
phosphoric acid
Chem 30 Review of Chem 20 Workbook
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Review of Chemical Reactions
For each of the following questions, identify the reaction type and write out a balanced chemical reaction
including the states of matter.
1. Propane gas is burned in a camp stove.
C3H8(g) + 5O2(g)  4H2O(g) + 3CO2)g
2. Phosphoric acid is used to remove rust, Fe(OH)3(s).
H3PO4(aq) + Fe(OH)3(s) 3HOH(l) + FePO4(s)
3. The cap is removed from a carbonated beverage. The carbonic acid in the beverage decomposes to
produce carbon dioxide and water.
H2CO3(aq) H2O(l) + CO2(g)
4. A nickel strip placed in a copper (II) sulphate solution becomes plated with copper.
Ni(s) + CuSO4(aq)  NiSO4(aq) + Cu(s)
5. Baking soda (sodium hydrogen carbonate) is used to neutralize a spill of car battery acid (sulphuric
acid). The products are sodium hydrogen sulphate, carbon dioxide and water.
NaHCO3(aq) + H2SO4(aq) 
NaHSO4(aq) + CO2(g) + HOH(l)
6. Mercury (II) oxide is decomposed into its elements.
2HgO(s)  2Hg(l) + O2(g)
7. Iron rusts, producing iron (III) oxide trihydrate, in moist air (water and oxygen) causing millions of
dollars of damage each year.
8. Sulphur dioxide emissions from industries combines with water vapour in the atmosphere to produce
acid rain, sulphurous acid.
Chem 30 Review of Chem 20 Workbook
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Review of Dissociation Equations
Write the dissociation equation, including states, for each of the following soluble substances:
1. lithium chloride
2. hydrobromic acid
3. sodium hydroxide
4. potassium acetate
5. sodium fluoride
6. sodium dichromate
7. copper (II) sulphate pentahydrate
8. lithium hydroxide
9. ammonium phosphate
10. potassium carbonate
Chem 30 Review of Chem 20 Workbook
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Review of Net Ionic Equations
For each of the following, write the non ionic, total ionic and net ionic equations.
1. A solution of iron (III) chloride is tested for the presence of iron (III) ions by the addition of dilute
sodium hydroxide. A red precipitate indicates a positive result.
Fe3+(aq) + 3OH-(aq)  Fe(OH)3(s)
2. Aqueous solutions of potassium sulphate and barium bromide are mixed.
Ba2+(aq) + SO42-(aq) BaSO4(s)
3. Hydrochloric acid reacts with calcium metal.
Ca(s) + 2H+(aq)  Ca2+(aq) + H2(g)
4. An aqueous solution of washing soda (Na2CO3) is added to hard water containing magnesium
sulphate. The magnesium ions are precipitated from the water.
Mg2+(aq) + CO32-(aq)  MgCO3(s)
5. Calcium metal is added to water.
Ca(s) + 2HOH(l)  Ca(OH)2(s) + H2(g)
Review of Concentration and Solution Preparation
1. Calculate the concentration of Cu(NO3)2(s) if 230 g are dissolved in 4.00 L of water.
0.307 mol/L
2. What mass of sulfuric acid is needed to prepare 3.50 L of a 0.400 mol/L solution.
137 g
3. What volume of 0.500 mol/L NaHSO4(aq) is made when 6.60 g of the solid solute is dissolved in
water?
.110 L or 110 mL
0
4. Describe how to prepare 100 mL of a 0.150 mol/L solution of sodium hydroxide.
0.600 g
Dissolve
of NaOH in 50 mL of water in a 100 mL beaker. Stir until completely
dissolved. Transfer to a 100 mL volumetric flask using a funnel, making sure to rinse the beaker and
stirring rod, and funnel. Add enough water to reach the 100 mL mark in the volumetric flask.
5. Describe how to prepare 250 mL of a 0.100 mol/L solution of copper (II) sulphate pentahydrate.
Dissolve 6.24 g of CuSO *5H O in 50 mL of water in a 100 mL beaker. Stir until
4
2
completely dissolved. Transfer to a 250 mL volumetric flask using a funnel, making sure to rinse
the beaker and stirring rod, and funnel. Add enough water to reach the 250 mL mark in the
volumetric flask.
Chem 30 Review of Chem 20 Workbook
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Review of Concentration of Ions in Solution
For each of the following, show the dissociation equation and calculate the concentration of each ion:
1. 0.120 mol/L Na2CO3(aq)
Na2CO3(aq) 2Na+(aq)
0.240 mol/L
+ CO32-(aq)
0.120 mol/L
2. 0.0910 mol/L Cr(NO3)3(aq)
Cr(NO3)3(aq) Cr3+(aq)
+ 3NO3-(aq)
0.0910 mol/L 0.273 mol/L
3. 8.00 g of zinc chloride is dissolved in 250 mL of water
ZnCl2(s) 
Zn2+(aq) +
2Cl-(aq)
0.235 mol/L
0.470 mol/L
C = m/(MV)
= 8/((65.41+(35.45*2)(.25)
=0.235 mol/L
For each of the following, show the dissociation equation and calculate the concentration of the solution:
4. 0.500 mol/L Na+(aq) in a sodium sulphate solution.
Na2SO4(s)  2Na+(aq) + SO4-(aq)
0.250 mol/L
5. 0.20 mol/L Cr2O72(aq) in a potassium dichromate solution.
K2Cr2O7(s)  2K+(aq) + Cr2O72(aq)
0.200 mol/L
6. 0.575 mol/L Cl(aq) in an iron (III) chloride solution.
Review of Stoichiometry
1. What mass of oxygen is required to completely oxidize 3.60 g of steel wool (pure iron) to produce
iron (III) oxide?
1.55g
2. When gasoline, C8H18(l), burns in an engine, water vapour is produced. What volume of water
vapour would be produced from the complete combustion of 15.0 g of octane at SATP?
28.9 L
3. In the laboratory preparation of oxygen, potassium chlorate is heated. The products are potassium
chloride and oxygen. What mass of potassium chlorate must be decomposed to produce 6.40 g of
oxygen gas?
16.3 g
Chem 30 Review of Chem 20 Workbook
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4. An excess of barium chloride solution was added to 400 mL of silver nitrate solution and 5.10 g of
precipitate was produced. What was the concentration of the silver nitrate solution?
0.0889 mol/L
5. If 25.0 mL of a sulphuric acid solution reacts completely with 15.0 mL of a 0.200 mol/L solution of
sodium hydroxide, what is the concentration of the sulphuric acid solution?
0.0600 mol/L
6. What mass of zinc would be needed to completely react with 50.0 mL of 6.00 mol/L hydrochloric
acid?
9.81 g
Review of Limiting and Excess Reagents
1. If 10.0 g of Pb(NO3)2(aq) and 10.0 g of K3PO4(aq) react, what is the mass of the solid precipitate
produced?
8.17 g
2. If 20.0 g of silver nitrate reacts with 10.0 g of magnesium chloride, what is the mass of the solid
produced?
16.9 g
Chem 30 Review of Chem 20 Workbook
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