CHAPTER 4 REVIEW: TYPES OF CHEMICAL REACTIONS AND SOLUTION STOICHIOMETRY
QUICK REVIEW
Distinguish between strong, weak, and nonelectrolytes
1. State whether each of the following is a strong, weak, or nonelectrolyte:
(a) HClO4
(d) NH3
(b) C6H12
(e) CaCl2
(c) LiOH
(f) HC2H3O2
Determine the molarity of a solution. Calculate the molarity of each ion in a solution. Determine the
mass and/or volume of reagents necessary to prepare a solution of given molarity. Solve problems related
to dilution.
Predict formation of precipitates. Know solubility rules!!!
Write molecular, complete ionic, and net ionic equations.
2. Identify the precipitate formed in each of the following reactions:
(a) potassium chloride (aq) + lead (II) nitrate (aq)
(b) silver nitrate (aq) + magnesium bromide (aq)
(c) calcium hydroxide (aq) + ferric chloride (aq)
Solve a variety of problems involving the formation of precipitates.
3. Calculate the amount (g) of precipitate produced when 125 mL of 0.200 M silver nitrate is added to excess
sodium sulfide solution.
4. (Lab - Gravimetric analysis problem) An ore sample is to be analyzed for sulfur. As part of the procedure,
the ore is dissolved and the sulfur is converted to the sulfate ion. Barium nitrate is added which causes the
sulfate to precipitate out as BaSO4. The original sample has a mass of 3.187 g. The dried BaSO4 has a mass
of 2.005 g. What is the percent of sulfur in the original ore?
Solve a variety of problems related to acid-base neutralizations.
5. How many milliliters of a 0.800 M Sr(OH)2 solution is needed to neutralize 40.0 mL of a 0.600 M HCl
solution?
Assign oxidation numbers to atoms in a compound/polyatomic ion.
Balance redox reactions (acidic and basic solutions) Solve a variety of problems related to redox titrations
– Lab question.
6. A student titrated a 0.500 M acidified solution of ferrous nitrate with a 0.100 M potassium dichromate
solution. If the student used 25.0 mL of the ferrous nitrate solution, how many milliliters of the
potassium dichromate solution are required?
What is the color of the dichromate ion?
HW: CHAPTER 4 REVIEW
1. Classify the following as strong, weak, or nonelectrolyte
(a) C2H5OH
(c) HF
(b) C12H22O11
(d) MgCl2
2. Determine the molarity of the chloride ion in a solution prepared by dissolving 9.82 g of copper (II) chloride
in enough water the make 600. mL of solution.
3. A solution contains Ag+, Pb2+, and Fe3+. If you want to precipitate the Pb2+ selectively, what anion would you use?
4. You want to determine the molar mass of an unknown weak monoprotic acid. You mass out a 2.879 g sample
of the pure acid and dissolve it in distilled water. After adding 3 drops of phenolphthalein indicator, you
titrate the sample with 0.1704 M NaOH. The pink endpoint is reached after the addition of 42.55 mL of
the base. Calculate the molar mass of the acid.
5. A 2.000 g sample of silver alloy was dissolved in nitric acid and then precipitated as AgBr. After drying the
sample of silver bromide weighed 2.000 g. Calculate the percentage of silver in the alloy.
The following are MC meant to be answered without a calculator
6. How many milliliters of 0.40M FeBr3 solution would be necessary to precipitate all of the Ag + from 30.0 mL
of 0.40 M AgNO3 solution?
(a) 10 mL
(b) 20 mL
(c) 30 mL
(d) 60 mL
(e) 90 mL
7. If 87 g of K2SO4 (molar mass 174 g) is dissolved in enough water to make 250 milliliters of solution,
what are concentrations of the potassium and sulfate ions?
(a)
(b)
(c)
(d)
(e)
[K+]
0.020 M
1.0 M
2.0 M
2.0 M
4.0 M
[SO42-]
0.020 M
2.0 M
1.0 M
2.0 M
2.0 M
8. 2 H2O + 4 MnO4- + 3 ClO2-  4 MnO2 + 3 ClO4- + 4OHWhich species acts as an oxidizing agent in the reaction represented above?
(a) H2O
(b) ClO4(c) ClO2(d) MnO2
(e) MnO49. The volume of distilled water that should be added to 10.0 mL of 6.00 M HCl (aq) in order to prepare a 0.500 M
HCl (aq)solution is approximately
(a) 50.0 mL (b) 60.0 mL
(c) 100. mL
(d) 110 mL
(e) 120 mL
10. What is the oxidation number of oxygen in Na2O2?
(a) -1
(b) -2
(c) +1
(d) +2
(e) – ½