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Chapter 16 and 17 Prep Test Per 2

Multiple Choice
Identify the choice that best completes the statement or answers the question.
 

 1. 
Acids taste
a.
sweet.
c.
bitter.
b.
sour.
d.
salty.
 

 2. 
Acids make blue litmus paper turn
a.
red.
c.
blue.
b.
yellow.
d.
black.
 

 3. 
Acids react with
a.
bases to produce salts and water.
c.
water to produce bases and salts.
b.
salts to produce bases and water.
d.
neither bases, salts, nor water.
 

 4. 
Bases feel
a.
rough.
c.
slippery.
b.
moist.
d.
dry.
 

 5. 
The traditional (1st) definition of acids is based on the observations of
a.
Brønsted and Lowry.
c.
Arrhenius.
b.
Lewis.
d.
Faraday.
 

 6. 
A substance that ionizes nearly completely in aqueous solutions and produces H+ is a
a.
weak base.
c.
weak acid.
b.
strong base.
d.
strong acid.
 

 7. 
Which of the following is NOT a strong acid?
a.
HNO3
c.
H2SO4
b.
CH3COOH
d.
HCl
 

 8. 
Which of the following is a diprotic acid?
a.
H2SO4
c.
HCl
b.
CH3COOH
d.
H3PO4
 

 9. 
A Brønsted-Lowry acid is
a.
an electron-pair acceptor.
c.
a proton acceptor.
b.
an electron-pair donor.
d.
a proton donor.
 

 10. 
In the equation HCl(g) + H2O(l) ® H3O+(aq) + Cl–(aq), which species is a Brønsted-Lowry acid?
a.
HCl
c.
Cl–
b.
Na2O
d.
none of the above
 

 11. 
A conjugate base is the species that
a.
remains after a base has given up a proton.
b.
is formed by the addition of a proton to a base.
c.
is formed by the addition of a proton to an acid.
d.
remains after an acid has given up a proton.
 

 12. 
A species that is formed when a base gains a proton is a
a.
conjugate base.
c.
strong base.
b.
conjugate acid.
d.
strong acid.
 

 13. 
In the reaction HF + H2O mc013-1.jpg H3O+ + F–, a conjugate acid-base pair is
a.
HF and H2O.
c.
H3O+ and H2O.
b.
F– and H3O+.
d.
HF and H3O+.
 

 14. 
In the reaction HClO3 + NH3 mc014-1.jpg NH4+ + ClO3–, the conjugate acid of NH3 is
a.
HClO3.
c.
NH4+.
b.
ClO3–.
d.
not shown.
 

 15. 
In the reaction HClO3 + NH3 mc015-1.jpg NH4+ + ClO3–, the conjugate base of HClO3 is
a.
ClO3–.
c.
NH4+.
b.
NH3.
d.
not shown.
 

 16. 
A species that can react as either an acid or a base is a(n)
a.
Lewis acid.
c.
oxyacid.
b.
amphoteric substance.
d.
organic substance.
 

 17. 
In the reaction HSO4– + H2O mc017-1.jpg H3O+ + SO42–, the ion HSO4– acts as a(n)
a.
acid.
c.
spectator species.
b.
base.
d.
salt.
 

 18. 
In the reaction H3PO4 + H2O mc018-1.jpg H3O+ + H2PO4–, the molecule H2O acts as a(n)
a.
acid.
c.
spectator species.
b.
base.
d.
salt.
 

 19. 
The substances produced when KOH(aq) neutralizes HCl(aq) are
a.
HClO(aq) and KH(aq).
c.
H2O(l) and KCl(aq).
b.
KH2O+(aq) and Cl–(aq).
d.
H3O+(aq) and KCl(aq).
 

 20. 
Pure water can partially break down into charged particles in a process called
a.
hydration.
c.
self-ionization.
b.
hydrolysis.
d.
dissociation.
 

 21. 
Which expression represents the pH of a solution?
a.
log[H+]
c.
log[OH–]
b.
– log[H+]
d.
– log[OH–]
 

 22. 
If [H+] of a solution is greater than [OH–], the solution
a.
is always acidic.
c.
is always neutral.
b.
is always basic.
d.
might be acidic, basic, or neutral.
 

 23. 
The pH scale in general use ranges from
a.
0 to 1.
c.
0 to 7.
b.
–1 to 1.
d.
0 to 14.
 

 24. 
The pH of a basic solution is
a.
less than 0.
c.
greater than 7.
b.
less than 7.
d.
greater than 14.
 

 25. 
What is the pH of a 1 x 10–5 M KOH solution?
a.
3
c.
9
b.
5
d.
11
 

 26. 
If [H+] = 1.00 x 10–5 M, what is the pH of the solution?
a.
2.00
c.
5.00
b.
3.00
d.
9.00
 

 27. 
What is the pH of a 0.001 M KOH solution?
a.
3.00
c.
12.0
b.
11.0
d.
14.0
 

 28. 
What is the hydrogen ion concentration of a solution whose pH is 4.00?
a.
1.0 x 10–10 M
c.
6.0 x 10–4 M
b.
5.0 x 10–6 M
d.
1.0 x 10–4 M
 

 29. 
A reaction in which products can react to re-form reactants is
a.
at equilibrium.
c.
buffered.
b.
reversible.
d.
impossible.
 

 30. 
At equilibrium,
a.
all reactions have ceased.
b.
only the forward reaction continues.
c.
only the reverse reaction continues.
d.
both the forward and reverse reactions continue.
 

 31. 
At equilibrium, the total amount of the product(s)
a.
is always equal to the total amount of the reactants.
b.
is always greater than the total amount of the reactants.
c.
is always less than the total amount of the reactants.
d.
may be equal to, greater than, or less than the total amount of the reactants.
 

 32. 
Which symbol represents the equilibrium constant?
a.
T
c.
c
b.
K
d.
R
 

 33. 
A very low value of K indicates that
a.
equilibrium is reached slowly.
c.
reactants are favored.
b.
products are favored.
d.
equilibrium has been reached.
 

 34. 
In the equation mc034-1.jpg, what represents the concentrations of the reactants?
a.
[Y] and [Z]
c.
mc034-2.jpg
b.
[W] and [X]
d.
mc034-3.jpg
 

 35. 
How do coefficients from a chemical equilibrium appear when the chemical equilibrium expression is written?
a.
as coefficients
c.
as subscripts
b.
as exponents
d.
They do not appear.
 

 36. 
What is the chemical equilibrium expression for the equation

2A2B + 3CD mc036-1.jpg A4D + C3B2?
a.
mc036-2.jpg
c.
mc036-4.jpg
b.
mc036-3.jpg
d.
mc036-5.jpg
 

 37. 
An equilibrium mixture of SO2, O2, and SO3 gases is determined to consist of 2 mol/L SO2,     1 mol/L O2, and 4 mol/L SO3. What is the equilibrium constant for the system at this temperature? The balanced equation for this reaction is

2SO2(g) + O2(g) mc037-1.jpg 2SO3(g).
a.
1
c.
16
b.
28
d.
4
 

 38. 
If the pressure on the equilibrium system 2CO(g) + O2(g) mc038-1.jpg 2CO2(g) is increased,
a.
the quantity of CO(g) increases.
b.
the quantity of CO2(g) decreases.
c.
the quantity of CO2(g) increases.
d.
the quantities in the system do not change.
 

 39. 
If the temperature of the equilibrium system CH3OH(g) + 101 kJ mc039-1.jpg CO(g) + 2H2(g) increases,
a.
[CH3OH] increases and [CO] decreases.
b.
[CH3OH] decreases and [CO] increases.
c.
[CH3OH] increases and [CO] increases.
d.
the concentrations in the system do not change.
 

 40. 
If the temperature of the equilibrium system CH3OH(g) + 101 kJ mc040-1.jpg CO(g) + 2H2(g) increases, K
a.
increases.
c.
increases or decreases.
b.
decreases.
d.
does not change.
 

 41. 
If a reaction system has come to equilibrium, it can be made to run to completion
a.
only if it is not reversible.
c.
by applying Le Châtelier's principle.
b.
only if the temperature is low enough.
d.
under no circumstances.
 

 42. 
What is the equilibrium constant, K, for the ionization of acetic acid, shown in the reaction
CH3COOH(aq) + H2O(l) mc042-1.jpg H3O+(aq) + CH3COO–(aq)?
a.
[H3O+] [CH3COOH–]
c.
mc042-3.jpg
b.
mc042-2.jpg
d.
mc042-4.jpg
 

 43. 
The pH of a solution is 12. What is its [OH-]?
a.
1 x 10–12 M
c.
0.01 M
b.
1 x 10–7 M
d.
12 M
 

Matching
 
 
grp001-1.jpg
a.
a
d.
d
b.
b
e.
e
c.
c
 

 44. 

 Represents the activation energy of the forward reaction.
 

 45. 

 Represents the potential energy of the activated complex.
 

 46. 

 Represents the potential energy of the reactants.
 

 47. 

 Represents the change in energy of the forward and reverse reaction.
 

 48. 

 Represents the activation energy of the reverse reaction.
 



 
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