Chemistry 30 Review Test 2
Acids, Bases, Neutralization, Equilibrium
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Part I Multiple choice / Numerical Response
Answer the following multiple choice questions on the scantron sheet. Answer the numerical response on
your short answer sheet. DO NOT WRITE ON THE TEST PAPER!
(25 marks)
1. The property that acids and bases have in common is that they
a) conduct electricity
b) turn red litmus blue
c) turn blue litmus red
d) taste sour
2. A base added to a neutral aqueous solution will:
a) decrease [OH-]
b) decrease [H3O+]
c) decrease the pH of the solution
d) donate protons to another substance in the solution
3. Choose the equation in which HSO3-(aq) exhibits the behaviour of a Bronsted-Lowry base:
a) HSO3-(aq) + HClO4(aq)  HSO4-(aq) + HClO3(aq)
b) HSO3-(aq) + H2PO4-(aq)  H2SO3(aq) + HPO42-(aq)
c) HSO3-(aq) + H2O(l)  H3O+(aq) + SO32-(aq)
d) HSO3-(aq) + HCO3-(aq)  SO32-(aq) + H2CO3(aq)
4. Which of the following is the weakest base?
a) F-(aq)
b) Ph-(aq)
c) SO42-(aq)
d) HSO4-(aq)
5. Which solution can neutralize or partially neutralize both acidic and basic solutions?
a) HCOO-(aq)
b) CH3COO-(aq)
c) HCO3-(aq)
d) S2-(aq)
Numerical response #1
An apple was analyzed and found to have a pH of 3.30. The [OH-] for this sample is:_________ x10x mol/L
6. Which of these 0.10 mol/L solutions has a pH of 7.00?
a) Na2CO3(aq)
b) KCl(aq)
c) KCN(aq)
d) HF(aq)
7. HA is a weak acid. In a 0.10 mol/L solution of HA(aq), the species present in the highest concentration is:
a) HA(aq)
b) A-(aq)
c) H3O+(aq)
d) OH-(aq)
8. 1.80 g of CH3COOH(l) are dissolved in enough water to make 300 mL of solution. If the indicator dropped into
the solution is:
a) orange IV, the colour of the solution will be orange
b) bromothymol blue, the colour of the solution will be blue
c) methyl violet, the colour of the solution will be yellow
d) thymol blue, the colour of the solution will be yellow
9. If equal quantities of HOCl(aq) and KCH3COO(aq) are mixed together, the following equilibrium is established:
HOCl(aq) + CH3COO-(aq)  OCl-(aq) + CH3COOH(aq)
Chemistry 30 - Acids, Bases and Equilibrium Review Test
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This equilibrium:
a) favours the reactants
b) favours the products
c) favours neither side because all concentrations are equal
d) is impossible to predict, given the information available
Use the following information to answer question 10
A solution is tested with a number of indicators in order to determine its pH. The results of the tests are
summarized in the table.
Indicator
methyl violet
phenol red
indigo carmine
phenolpthalein
Colour
blue
red
blue
colourless
10. The pH of the solution is approximately:
a) 5.2
b) 6.0
c) 8.1
d) 11.4
11. At which point on the graph does the [OH-] equal the [H3O+]?
d
pH
c
a
b
volume of HCl(aq) (mL)
12. Which of the following equations is an acid-base neutralization reaction?
a) 2HCl(aq) + Mg(s)  MgCl2(aq) + H2(g)
b) LiOH(s) + HBr(aq)  LiBr(aq) + H2O(l)
c) 2HNO3(aq) + 3H2SO3(aq)  2NO(g) + H2O(l) + 3H2SO4(aq)
d) Pb(NO3)2(aq) + 2KI(aq)  PbI2(s) + 2KNO3(aq)
13. The strongest acid listed is:
a) H3X(aq)
b) H2X-(aq)
c) HX2-(aq)
d) X3-(aq)
14. Solution I is red in phenol red and colourless in phenolpthalein. Solution II is pink in phenolpthalein and yellow
in alizarin yellow. The [H3O+] is about:
a) two times higher in solution I than in solution II
b) two times higher in solution II than in solution I
c) 100 times higher in solution I than in solution II
d) 100 times higher in solution II than in solution I
Numerical response #2
The pOH of a solution made by mixing 50.0 mL of 0.200 mol/L HCl(aq) with 200 mL of 0.300 mol/L NaOH(aq)
is___________ (to 2 digits)
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15. Which of the following 50.0 mL solution requires the greatest volume of 0.100 mol/L HCl(aq) to completely
neutralize?
a) 0.100 mol/L NaOH(aq)
b) 0.100 mol/L NH3(aq)
c) 0.100 mol/L Ba(OH)2(aq)
d) 0.100 mol/L HOOCCOOH(aq)
Numerical response #3
The [H3O+] in 0.020 mol/L Ba(OH)2(aq) is: ____________x 10x mol/L
16. The equivalence point in an acid-base titration will have a pH of 7 for the titration of:
a) OH- with vinegar
b) ammonia with H3O+
c) acetic acid with potassium hydroxide
d) hydrochloric acid with sodium hydroxide
Use the following information to answer the next two questions
pH
volume of NaOH(aq) (mL)
16. The acid in the titration is:
a) HOOCCOOH(aq)
b) CH3COOH(aq)
c) HNO3(aq)
d) HCl(aq)
Numerical response #4
If a 50.0 mL sample of the acid required 35.0 mL of 0.100 mol/L NaOH to reach the endpoint, the concentration
of the acid is _________________ x10x mol/L
18. In the reaction HCl(g) + H2O(l)  H3O+(aq) + Cl-(aq), water is:
a) an acid
b) a proton donor
c) an electron acceptor
d) a proton acceptor
19. The equilibrium H2O(l) + HBb(aq)  H3O+(aq) + Bb-(aq) exists when bromothymol blue indicator is added to water.
Which of the following statements is correct?
a) When KOH(aq) is added, the [HBb] increases and the solution turns yellow
b) When HCl(aq) is added, the [H3O+] increases and the solution turns yellow
c) When HCl(aq) is added, the equilibrium is shifted toward the reactants and the solution turns blue.
d) When KOH(aq) is added, the equilibrium is shifted toward the reactants and the solution turns yellow.
20. A correct description of the action of a base is that a base:
a) decreases the pH of an aqueous solution
b) decreases [OH-] of an aqueous solution
c) donates protons in chemical reactions
d) accepts protons in chemical reactions
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21. Arrhenius defined an acid as a substance that:
a) tastes sour
b) turns litmus blue
c) increases the concentration of H+(aq) in a solution
d) increases the concentration of OH-(aq) in a solution
22. If 20.0 mL of 0.100 mol/L NaOH(aq) are added to 40.0 mL of 0.100 mol/L HCl(aq) containing phenolpthalein and
bromothymol blue, the resulting solution will be:
a) blue
b) pink
c) yellow
d) colourless
Numerical response #5
What concentration of HCl(aq) would yield the same pH as 0.10 mol/L CH3COOH(aq)? ________x10x mol/L
23. Solutions of methanoic acid and sodium ethanoate are mixed. The net ionic equation that best describes the
resulting reaction is:
a) H3O+(aq) + OH-(aq)  H2O(l) + H2O(l)
b) H3O+(aq) + CH3COO-(aq)  CH3COOH(aq) + H2O(l)
c) HCOOH(aq) + CH3COO-(aq)  CH3COOH(aq) + HCOO-(aq)
d) HCOOH(aq) + NaCH3COO(aq)  CH3COOH(aq) + NaHCOO(aq)
Use the following information to answer question 24
A chemist performed a titration experiment and found that the volume of acid used from the burette was lower
than the calculated theoretical volume needed to neutralize the base. Some of the suggested experimental
error were:
I Too much base was pipetted into the flask
II The endpoint was passed
III The wrong indicators were chosen
IV There was water in the burette when the acid was added
V There was water in the flask when the base was pipetted into it
24. Which of the suggested experimental errors would account for the low volume of acid used?
a) III only
b) II, III, and IV only
c) I, III, IV, and V only
d) I, II, III, IV, and V
25. When used to describe an acid, the word “weak” means that the acid
a) has a low pH
b) has a low concentration
c) shows incomplete dissociation
d) is monoprotic
26. A student suspects that an unknown acid of known concentration is diprotic. In order to test this hypothesis, the
most useful procedure for the student to follow would be to:
a) determine the molar mass
b) find the pH by using an indicator
c) titrate with a known concentration of NaOH(aq)
d) establish the degree of electrical conductivity
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27. A 0.10 mol/L solution containing a single dissolved substance is a very good conductor of electricity and turns
blue litmus paper red. The pH of this solution could be approximately:
a) 1.4
b) 5.6
c) 7.0
d) 12.3
28. A catalyst speeds up a reaction because
a) there are more collisions per second
b) collisions occur with greater energy
c) because there are more collisions and they occur with greater energy
d) the activation energy is lowered
29. What is the equilibrium expression for the reaction: C(s) + O2(g)  CO2(g)
a) Keq = [C][O2]
[CO2]
c) Keq = [CO2]
[O2]
b) Keq = [CO2]
[C][O2]
d) Keq = [O2]
[CO2]
30. What is the Keq for the following gaseous reaction?
2NO2(g)  2NO(g) + O2(g)
a) [NO2]2
[NO]2[O2]
c) [NO][O2]
[NO2]
b) [NO]2[O2]
[NO2]2
d) [NO2]
[NO][O2]
31. Analysis of the equilibrium 2NOCl(g)  2NO(g) + Cl2(g) gave the following information:
[NOCl] = 0.50 mol/L
[NO] = 2.0x10-2 mol/L
[Cl2] = 1.0x10-2 mol/L
What is the value for Keq for this system?
a) 4.0x10-4
b) 1.6x10-5
c) 1.3x10-5
d) 1.3x105
32. Which change listed below would shift the following reaction to the right?
4HCl(g) + O2(g)  2Cl2(g) + 2H2O(g)
a)
b)
c)
d)
addition of Cl2
removal of O2
volume decrease
addition of inert He gas
Use the following information to answer the next three questions
2HI(g)  H2(g) + I2(g)
H = -53.0 kJ
Keq = 1.84x10-2 at 730C
33. The H for the reverse reaction is :
a) -53.0 kJ
b) +53.0 kJ
c) -106 kJ
d) +106 kJ
34. A temperature of 500C:
a) would favour the forward reaction
b) would favour the reverse reaction
Chemistry 30 - Acids, Bases and Equilibrium Review Test
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c) neither reaction would be favoured
d) Keq is not affected by temperature
35. The H for the reaction HI(g)  ½ H2(g) + ½ I2(g) is:
a) -53.0 kJ
b) -26.5 kJ
c) +26.5 kJ
d) -7.28 kJ
Part II - Short Answer Questions
Answer the following questions on a separate piece of paper. Show all of your work for part marks.
(20 marks)
1. A student recorded data during the titration of a 25.0 mL sample of an unidentified base with 0.100 mol/L
HCl(aq):
Volume of Acid (mL)
0.00
10.00
20.00
30.00
35.00
pH
10.1
9.1
8.9
8.3
7.9
Volume of Acid (mL)
40.00
45.00
50.00
60.00
70.00
pH
5.0
2.2
1.9
1.6
1.5
a) On a piece of graph paper (provided in the diploma), carefully plot the data from the table. Mark the
equivalence point on the graph with a neat “x” and label it. Then calculate the initial concentration of the
unidentified base.
b) What indicator would be suitable for use in this titration?
c) What conclusion can you draw about the strength of the base? Justify your answer. (8 marks total)
2. Examine the results of tests performed on the following 0.10 mol/L solutions:
Solution Reacts with zinc
Conducts Electricity
Colour in thymol blue
I
no
no
yellow
II
yes
yes
orange
III
yes
yes
red
IV
no
yes
blue
Classify each solution as acidic, basic, neutral, ionic, or neutral molecular. Indicate which test results are
essential to classifying the solution and explain why. (8 marks total)
3. For an acid-base titration, describe an experimental procedure that can be used to obtain the:
a) endpoint of the titration
b) equivalence point of the titration
Distinguish between the terms endpoint and equivalence point (4 marks)
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