Chemistry
Raymond Chang
10th edition
Chapter 15
Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Question 1
Which is true regarding the equilibrium below?
HF(g) + H2O(l) ↔ F- + H3O+(aq)
A) HF is acting as a Bronsted base.
B) Water is acting as a Bronsted base.
C) The reaction goes to completion leaving
little HF.
D) The Fluoride ion is acting as Bronsted
acid.
Question 2
Which of the following is(are) true?
A) pH can never be greater than 14.
B) pH can never be less than 0.
C) At room temperature, pH + pOH = 14.
D) All of the above.
Question 3
Which of the following is a neutral salt (neither
acidic nor basic)?
A) KCl
B) NaCN
C) NH4NO3
D) NaF
Question 4
The hydroxide ion is the conjugate base of the
hydronium ion.
A) True
B) False
Question 5
Which of the following has an impact on the
percent ionization of a weak acid?
A) The acid ionization constant.
B) The concentration of the acid.
C) Both A and B.
D) None of the above.
Question 6
Which of the following best describes the acid
strengths of the hydrohalic acids?
A) HF>HCl>HBr>>HI
B) HF<<HCl<HBr<HI
C) HF=HCl=HBr=HI
D) HF=HCl<HBr=HI
Question 7
Which of the following will produce a basic
solution when dissolved in water?
A) Na2O
B) NaOH
C) Both A and B
D) None of the above
Question 8
The substance that is largely responsible for
acid rain is
A) calcium carbonate.
B) sodium chloride.
C) ozone.
D) sulfur dioxide.
Question 9
A Lewis base is a(an)
A) substance that contains the hydroxide ion.
B) proton acceptor.
C) electron pair donor.
D) none of the above
Question 10
In a 0.100 M solution of sodium hydroxide,
what are the equilibrium concentrations of
sodium hydroxide, sodium ions, hydroxide
ions, and hydronium ions, respectively?
A) 0.100; 0.100; 0.100; 0
B) 0.100; 0.100; 0.100; 1X10-13
C) 0; 0.100; 0.100; 0
D) 0; 0.100; 0.100; 1X10-13
Question 11
The chloride ion in aqueous solution is a
A) strong conjugated acid.
B) weak conjugated acid.
C) strong conjugated base.
D) weak conjugated base.
Question 12
Water can act as a
A) weak acid.
B) strong acid.
C) weak base.
D) strong base.
E) two of the above.
Question 13
Which pH region is most likely for a sample of
vinegar?
A) 0 to 1
B) 1 to 6
C) 8 to 13
D) 13 to 14
E) none of the above
Question 14
Calculate the pH of a 0.018M solution of
Ca(OH)2.
A) 12.56
B) 1.8
C) 1.44
D) 12.25
E) none of the above
Question 15
Identify the Bronsted acids and bases in the
following reaction:
A) option 1
B) option 2
C) option 3
D) option 4
E) option 5
Question 16
When KOH and HNO3 are mixed, a reaction
occurs. What are the spectator ions in the
reaction?
A) K+ and H+
B) H+ and OHC) K+ and NO3D) H+ and NO3E) there are no spectator ions in this reaction
Question 17
What is the difference between a strong acid
and a weak acid?
A) a strong acid contains strong covalent
bonds whereas a week acid does not
B) a strong acid has more hydrogen atoms
in its molecule than a weak acid
C) a weak acid is nonpolar, whereas a
strong acid is polar
D) strong acids react with both strong and
weak bases, whereas weak acids do not
E) none of the above
Question 18
What will be the pH of a 1.0 × 10-8 M solution of
HCl?
A) 8.0
B) 6.0
C) cannot be calculated
D) it will be slightly less than 7.0
E) it will be slightly more than 7.0
Question 19
Which of the following salts is expected to
produce a basic solution upon hydrolysis?
A) calcium chloride
B) ammonium sulfate
C) sodium acetate
D) ammonium acetate
E) ferrous bromide
Question 20
Calculate the mass in grams of 0.0504 moles
of an acid having the molar mass equal to
100.5.
A) 5.1
B) 19.84
C) 5.07
D) 5.065
E) none of the above
Answer Key – Chapter 15
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C