Chemistry: Matter and Change

Chapter 18: Acids and Bases

Standardized Test Practice

1
Which of these is a product of the first step in the ionization of phosphoric acid, H3PO4?

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A)H3PO4
B)H2PO4
C)HPO4
D)PO4
2
Which one of the following could not be a BrÆnsted-Lowry acid?
A)H2O
B)H3O+
C)NH4+
D)BF3
3
Which of the following is a weak acid?
A)HCl
B)HNO3
C)HClO4
D)HF
4
Which of the following is the strongest base according to the Bronsted-Lowry theory?
A)Cl-
B)NO3-
C)F-
D)I-
5
The acid ionization constant, Ka, is __________ for __________ acids.

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A)largest, anhydride
B)largest, weak
C)smallest, strong
D)smallest, weak
6
If a 20-watt light bulb circuit passes through the following 0.10 M acid solutions, which 20-watt bulb will be brightest?

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A)hydrofluoric
B)carbonic
C)perchloric
D)hydrosulfuric
7
Acetic acid is a weak acid. Which of the following gives the correct acid ionization constant expression

CH3COOH yields H+ + CH3COO-
A)Ka = [H+]/[CH3COOH]
B)Ka = [CH3COO-]/[CH3COOH]
C)Ka = [CH3COOH]/[CH3COO-]
D)Ka = [CH3COO-][H+]/[CH3COOH]
8
A solution of pH = 2.1 would be described as __________.
A)distinctly basic
B)slightly basic
C)slightly acidic
D)distinctly acidic
9
Calculate the pH of 0.075M KOH.
A)10.4
B)11.12
C)11.46
D)12.88
10
About how much larger is [H+] for soft drinks than for coffee?

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A)100
B)10
C)1.7
D)0.6
11
Calculate Ka for a 0.05 M solution of the weak acid HF. The pH of the solution is 2.274.

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A)6.3 x 10-4
B)0.12
C)5.7 x 10-4
D)0.11
12
Neutralization is the chemical process in which ____________.
A)sodium ions react with chloride ions to form sodium chloride
B)hydrogen ions react with chloride ions to form hydrogen chloride
C)sodium ions react with hydroxide ions to form sodium hydroxide
D)hydrogen ions react with hydroxide ions to form water
13
Which of the following cannot be a buffer?
A)a mixture of a weak acid and a weak base
B)a mixture of a weak acid and a strong base
C)a mixture of a strong acid and a weak base
D)a mixture of a strong acid and a strong base
14
Calculate the H+ ion and OH- ion concentrations in a 0.50M solution of HBr.
A)[H+] = 0.50M and [OH-] = 0.50M
B)[H+] = 0.50M and [OH-] = 2.0M
C)[H+] = 0.50M and [OH-] = 2.0 x 10-14M
D)[H+] = 1.0 x 10-7M and [OH-] = 1.0 x 10-7M
15
Which of these salts will produce an acidic solution?
A)KF
B)NH4Cl
C)NaNO3
D)NaCl
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