CHAPTER 4 STUDY GUIDE - 2
General Properties of Aqueous Solutions
1. Which of the following schematic drawings best describes a solution of
Li2SO4?
2. Aqueous solutions of three different substances, AX, AY, and AZ, are
represented by the three accompanying diagrams. Identify each substance as
a strong electrolyte, a weak electrolyte, or a nonelectrolyte.
a. A = weak electrolyte, B = strong electrolyte, C = weak electrolyte
b. A = weak electrolyte, B = nonelectrolyte, C = strong electrolyte
c. A = strong electrolyte, B = weak electrolyte, C = nonelectrolyte
d. A = strong electrolyte, B = nonelectrolyte, C = weak electrolyte
3. You are presented with a white solid. Because the container was labeled
incorrectly, you aren’t sure whether it is barium chloride, lead chloride, or
zinc chloride. When you transfer the solid to a beaker and add water, the
solid dissolves to give a clear solution. Next, you add a Na2SO4 (aq) solution
and a white precipitate forms. What is the identity of the unknown solid?
a. barium chloride
b. lead chloride
c. zinc chloride
d. None of these
Precipitation Reactions
4. Which combination will produce a precipitate?
a. NaF (aq) and HCl (aq) b. KOH (aq) and Mg(NO3)2 (aq)
c. AgNO3(aq) and Ca(C2H3O2)2 (aq)
d. NaC2H3O2 (aq) and HCl (aq) e. NaOH (aq) and HCl (aq)
5. Aqueous potassium chloride will react with which one of the following in
an exchange (metathesis) reaction? a. sodium chloride b. sodium bromide
c. barium nitrate d. lead nitrate
e. calcium nitrate
6. Aqueous solutions of a compound did not form precipitates with Cl-, Br-,
I-, SO42-, CO32-, 4) PO43-, OH-, or S2-. This highly water-soluble
compound produced the foul-smelling gas H2S when the solution was
acidified. This compound is ________. a. Li2CO3
b. Pb(NO3)2 c. (NH4)2S
d. AgNO3 e. KBr
7. A compound was found to be soluble in water. It was also found that
addition of acid to an aqueous solution of this compound resulted in the
formation of carbon dioxide. Which one of
the following cations would
form a precipitate when added to an aqueous solution of this
compound? a. Cr3+
b. Rb+
c. NH4+
d. K+
e. Na+
8. Separate samples of a solution of an unknown salt are treated with dilute
solutions of HBr, H3SO4, and NaOH. A precipitate forms in all three
cases. Which of the following cations could be present in the unknown
salt solution?
a. K+
b. Pb2+
c. Ba2+
d. Cr4+
9. You know that an unlabeled bottle contains an aqueous solution of one of
the following: AgNO3 , CaCl2 , Al2(SO4)3. A friend suggests that you test
a portion of the solution with Ba(NO3)2 , record the results, and then test
a new portion of the unknown solution with NaCl solutions. According
to your friend’s logic, which of these chemical reactions could occur, thus
helping you identify the solution in the bottle? Barium sulfate could
precipitate
a. Silver chloride could precipitate
b. Silver sulfate could precipitate
c. More than one, but not all of the above reactions.
d. All of the reactions in a-c
10. The labels have fallen off three bottles containing powdered samples of
metals; one contains zinc, one lead, and the other platinum. You have
three solutions at your disposal: 1 M sodium nitrate, 1 M nitric acid, and 1
M nickel nitrate. How could you use these solutions to determine the
identities of each metal powder?
a. Test all solutions on all the powdered metals. Zinc will react with
nitric acid and nickel nitrate, lead will react only with nitric acid,
and platinum will not react with any solution
b. Test all solutions on all the powdered metals. Zinc will react with
sodium nitrate and nickel nitrate, lead will react only with nitric
acid, and platinum will not react with only sodium nitrate
c. Only two tests are needed. Test all metals with nitric acid and
nickel nitrate. Zinc will react with both of these, lead will react
with just nitric acid, and platinum won’t react with either of the
solutions.
d. Only one test is needed. Test all metals with nickel nitrate, and the
only one that reacts should be lead. The other two can be
distinguished by their color – platinum is much more shiny
Acids and Bases and Neutralization Reactions
11. Which of the following solutions is the most acidic?
a. 0.2 M LiOH
b. 0.2 M HI
c. 1.0 M methyl alcohol (CH3OH)
d. 0.2 M CH3COOH
12. Which of the following solutions is the most basic?
a. 0.6 M NH3
b. 0.150 M KOH
c. 0.100 M Ba(OH)2
d. 1.0 M H2O
13. Which of the following statements is false?
a. NH3 contains no OH- ions and yet its aqueous solutions are basic
b. HF is a strong acid
c. Although sulfuric acid is a strong electrolyte, an aqueous solution of
H2SO4 contains more HSO4- ions than SO42- ions.
d. All of these are true
14. Which of the following is a weak base?
a. Ca(OH)2
b. RbOH
c. KOH
d. Al(OH)3
15. Which of the following is a weak acid?
a. H30+
b. HCl
c. HBr
d. HClO4
16. The net ionic equation for formation of an aqueous solution of Al(NO3)3
via mixing solid Al(OH)3 and aqueous nitric acid is
a. Al(OH)3 (s) + 3NO3- (aq) → 3OH- (aq) + Al(NO3)3 (s)
b. Al(OH)3 (s) + 3NO3- (aq) → 3OH- (aq) + Al(NO3)3 (aq) c. Al(OH)3 (s) + 3H+ (aq) → 3H2O (l) + Al3+ (aq)
d. Al(OH)3 (s) + 3HNO3 (aq) → 3H2O (l) + Al(NO3)3 (aq) e. Al(OH)3 (s) + 3HNO3 (aq) → 3H2O (l) + Al3+ (aq) + NO3- (aq)
17. The net ionic equation for the reaction between aqueous sulfuric acid and
aqueous sodium 12) hydroxide is
a. H+ (aq) + HSO4- (aq) + 2Na+ (aq) + 2OH- (aq) → 2H2O (l) + 2Na+
(aq) + SO42-(aq)
b. 2H+ (aq) + SO42- (aq) + 2Na+ (aq) + 2OH- (aq) → 2H2O (l) + 2Na+
(aq) + SO42- (aq)
c. H+(aq) + HSO4- (aq) + 2OH- (aq) → 2H2O (l) + SO42- (aq)
d. H+(aq) + OH-(aq) → H2O (l)
18. The reaction between strontium hydroxide and chloric acid produces
a. two weak electrolytes
b. two molecular compounds c. a molecular compound and a weak electrolyte
d. two strong electrolytes e. a molecular compound and a strong electrolyte
Redox Reactions
19. Which region of the periodic table shown here contains elements that are
easiest to oxidize?
a. A
b. B
c. C
A
D
d. D
C
B
20. In which reaction does the oxidation number of oxygen increase?
a. MgO (s) + H2O (l) → Mg(OH)2 (s) b. HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)
c. 2SO2(g) + O2(g) → 2SO3(g)
d. Ba(NO3)2 (aq) + K2SO4 (aq) → BaSO4 (s) + 2KNO3 (aq)
e. 2H2O(l) → 2H2(g) + O2(g)
21. Based on the activity series, which one of the reactions below will occur?
a. 3FeBr2 (aq) + 2Au (s) → 3Fe (s) + 2AuBr3 (aq)
b. SnCl2 (aq) + Cu (s) → Sn (s) + CuCl2 (aq) c. Zn (s) + MnI2(aq) → ZnI2(aq) + Mn (s) d. 2AgNO3 (aq) + Pb (s) → 2Ag (s) + Pb(NO3)2 (aq)
e. 3Hg (l) + 2Cr(NO3)3 (aq) → 3Hg(NO3)2 + 2Cr (s)
22. The metal cadmium tends to form Cd2+ ions. The following observations
were made in the laboratory: 1) When a strip of zinc metal is placed in CdCl2
(aq), cadmium metal is deposited on the strip, 2) When a strip of cadmium metal
is placed in Ni(NO3)2 (aq), nickel metal is deposited on the strip. What are the
correct net ionic equations for these two reactions?
a. Zn2+ + Cd (s)  Zn (s) + Cd2+ (aq)
Cd(s) + Ni2+ (aq)  Cd2+ (aq) + Ni (s)
b. Zn (s) + Cd2+ (aq)  Cd (s) + Zn2+ (aq)
Cd (s) + Ni2+ (aq)  Cd2+ (aq) + Ni (s)
c. Zn (s) + Cd2+ (aq)  Cd (s) + Zn2+ (aq)
Cd2+ (aq) + Ni (s)  Cd (s) + Ni2+ (aq)
d. Zn (s) + Cd2+ (aq)  Cd (s) + Ni2+ (aq)
Cd2+ (aq) + Ni (s)  Cd (s) + Zn2+ (aq)
23. Based on #22, which elements most closely match the position of cadmium on the
activity series?
a. chromium, iron, and cobalt
b. zinc, nickel, and iron
c. magnesium, aluminum, and sodium
d. gold, platinum, and mercury
24. Based on #22, which experiments could you perform to locate more precisely the
position of cadmium on the activity series?
a. Place an iron strip in CdCl2 (aq). If Cd (s) is deposited, Cd is less active
than Fe; if there is no reaction Cd is more active than Fe.
b. Place a cobalt strip in CdCl2 (aq). If Cd (s) is deposited, Cd is less active
than Co; if there is no reaction Cd is more active than Co
c. Place a strip of Cr in CdCl2 (aq). If Cd (s) is deposited, Cd is less active
than Cr; if there is no reaction Cd is more active than Cr
d. All of the above
e. A and B only
Concentrations
25. A 0.100 M solution of ________ will contain the highest concentration of
potassium ions.
a. potassium hydrogen carbonate b. potassium iodide c. potassium phosphate
d. potassium oxide
e. potassium hypochlorite
26. Which solution has the same number of moles of KCl as 75.00 mL of 0.250
M solution of KCl?
a. 50.0 mL of 0.125 M solution of KCl b. 100 mL of 0.0500 Msolution of KCl
c. 20.0 mL of 0.200 M solution of KCl
d. 129 mL of 0.145 M solution of KCl
e. 25.0 mL of 0.175 M solution of KCl
27. Starting with solid sucrose C12H22O11, how would you prepare 250 mL of a
0.250 M solution of sucrose?
a. 21.4 grams of sucrose and dissolve in 250 mL of distilled water
b. 342.2965 grams of sucrose and dissolve in 1.00 L of distilled water,
then take one half of that solution and add another 1.00 L of distilled
water
c. 85.6 grams of sucrose and dissolve in 250 mL of distilled water
d. 85.6 grams of sucrose and dissolve in 500 mL of distilled water, then
take half of that solution and add 250 mL of distilled water.
28. A 0.200 M K2SO4 solution is produced by ________. 27)
a. dissolving 43.6 g of K2SO4 in water and diluting to a total volume
of 250.0 mL
b. dilution of 1.00 mL of 250 M K2SO3 to 1.00 L
c. dissolving 20.2 g of K2SO4 in water and diluting to 250.0 mL, then
diluting 25.0 mL of this solution to a total volume of 500.0 mL
d. dilution of 250.0 mL of 1.00 M K2SO4 to 1.00 L
e. diluting 20.0 mL of 5.00 M K2SO4 solution to 500.0 mL
29. One cup of fresh orange juice contains 124 mg of ascorbic acid (vitamin C,
C6H8O6). Given that one cup = 236.6 mL, what is the molarity of vitamin C in
orange juice?
a. 2.98 x 10-3 M
b. 2.98 M
c. 0.524 M
d. 6.98 x 10-2 M
30. The concentration of alcohol (CH3CH2OH) in blood, called blood alcohol
concentration, or BAC, is given in units of grams of alcohol per 100 mL of
blood. The legal definition of intoxication, in many states of the US, is that the
BAC is 0.08 or higher. What is the concentration of alcohol, in terms of
molarity, in blood that has a BAC of 0.08?
a. 1.4 M
b. 0.012 M
c. 0.02 M
d. 0.8 M
31. Vodka is an aqueous solution of approximately 6.86 M ethanol. If you wanted
to make your own vodka, how many grams of ethanol, CH3CH2OH, should
you dissolve in water to make 1.00 L of vodka?
a. 316 g
b. 401 g
c. 256 g
d. 180 g
Solution Stoichiometry and Chemical Analysis
32. An aliquot (28.7 mL) of a KOH solution required 31.3 mL of 0.118 M HCl
for neutralization. What mass (g) of KOH was in the original sample?
a. 0.173
b. 0.207
c. 0.414
d. 1.64
e. 7.28
33. You are titrating an acidic solution with a basic one, and just realized you
forgot to add the indicator that tells you when the equivalence point is
reached. In this titration, the indicator turns blue at the equivalence point
from an initially colorless solution. You quickly grab a bottle of indicator
solution and throw some into your titration beaker, and the whole
solution turns dark blue! What should you do now that would be the
most efficient use of time and materials?
a. Burn it. Burn it all!
b. Add a known amount of base to the beaker to get it to turn
colorless again, then titrate the acid into the beaker to identify the
equivalence point.
c. Add a known amount of the unknown acid to the beaker to turn it
back to colorless, then carefully titrate the base into the solution to
identify the equivalence point when it turns back to blue.
d. Start over.
34. What volume (L) of 0.250 M HNO3 is required to neutralize a solution
prepared by dissolving 17.5 g of NaOH in 350 mL of water? a. 0.44
b. 1.75 ×10-3
c. 50.0
d. 1.75
e. 0.070
35. You are given two clear solutions of the same unknown monoprotic acid,
but with different concentrations. Which statement is true?
a. There is no chemical method designed to tell the two solutions
apart.
b. If the same volume of each sample was taken, then more base
solution would be required to neutralize the one with lower
concentration.
c. The product of concentration and volume of the less concentrated
solution equals the product of concentration and volume of the
more concentrated solution.
d. A smaller volume of the less concentrated solution contains the
same number of moles of the acid compared to the more
concentrated solution.
e. It would take more base solution (per milliliter of the unknown
solution) to neutralize the more concentrated solution.
36. Which of the following would require the largest volume of 0.100 M
sodium hydroxide solution for neutralization? a. 20.0 mL of 0.0500 M nitric acid
b. 15.0 mL of 0.0500 M hydrobromic acid c. 10.0 mL of 0.0500 M phosphoric acid
d. 5.0 mL of 0.0100 M sulfuric acid e. 10.0 mL of 0.0500 M perchloric acid
37. A mysterious white powder is found at a crime scene. A simple chemical
analysis concludes that the powder is a mixture of sugar and morphine
(C17H19NO3), a weak base similar to ammonia. The crime lab takes 10.00 mg
of the mysterious powder, dissolves it in 100.00 mL water, and titrates it to
the equivalence point with 2.84 mL of a standard 0.0100 M HCl solution.
What is the percentage of morphine in the white powder?
a. 8.10%
b. 17.3%
c. 49.7%
d. 81.0%
e. 32.6%
38. You want to analyze a silver nitrate solution. You could add HCl to the
solution to precipitate out AgCl (s). What is the volume of a 0.15O M HCl (aq)
solution is needed to precipitate the silver ions from 15.0 mL of a 0.200 M
AgNO3 solution?
a. 20.0 mL
b. 38.1 mL
c. 15.8 mL
d. 23.6 mL