Transcript 16_Clickers.pptx

Clicker Questions
Chapter 16
Barbara Mowery
York College
© 2015 Pearson Education, Inc.
A Brønsted–Lowry acid is
a.
b.
c.
d.
a proton donor.
a proton acceptor.
an electron-pair donor.
an electron-pair acceptor.
© 2015 Pearson Education, Inc.
A Brønsted–Lowry acid is
a.
b.
c.
d.
a proton donor.
a proton acceptor.
an electron-pair donor.
an electron-pair acceptor.
© 2015 Pearson Education, Inc.
A Brønsted–Lowry base is
a.
b.
c.
d.
a proton donor.
a proton acceptor.
an electron-pair donor.
an electron-pair acceptor.
© 2015 Pearson Education, Inc.
A Brønsted–Lowry base is
a.
b.
c.
d.
a proton donor.
a proton acceptor.
an electron-pair donor.
an electron-pair acceptor.
© 2015 Pearson Education, Inc.
A Lewis acid is
a.
b.
c.
d.
a proton donor.
a proton acceptor.
an electron-pair donor.
an electron-pair acceptor.
© 2015 Pearson Education, Inc.
A Lewis acid is
a.
b.
c.
d.
a proton donor.
a proton acceptor.
an electron-pair donor.
an electron-pair acceptor.
© 2015 Pearson Education, Inc.
A Lewis base is
a.
b.
c.
d.
a proton donor.
a proton acceptor.
an electron-pair donor.
an electron-pair acceptor.
© 2015 Pearson Education, Inc.
A Lewis base is
a.
b.
c.
d.
a proton donor.
a proton acceptor.
an electron-pair donor.
an electron-pair acceptor.
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Which of the following is the
conjugate base of HPO42−?
a.
b.
c.
d.
H3PO4
H2PO41−
PO43−
HPO32−
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Which of the following is the
conjugate base of HPO42−?
a.
b.
c.
d.
H3PO4
H2PO41−
PO43−
HPO32−
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Which species is amphiprotic?
a.
b.
c.
d.
H3PO4
H2PO41−
PO43−
None of these
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Which species is amphiprotic?
a.
b.
c.
d.
H3PO4
H2PO41−
PO43−
None of these
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Which of the following is the
conjugate acid of SO42−?
a.
b.
c.
d.
H2SO4
HSO41−
SO32−
H3SO4+
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Which of the following is the
conjugate acid of SO42−?
a.
b.
c.
d.
H2SO4
HSO41−
SO32−
H3SO4+
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The stronger the acid, the (X)
its conjugate base. Acids and
bases react to form their (Y)
conjugates.
a.
b.
c.
d.
X = stronger,
X = stronger,
X = weaker,
X = weaker,
© 2015 Pearson Education, Inc.
Y = stronger
Y = weaker
Y = stronger
Y = weaker
The stronger the acid, the (X)
its conjugate base. Acids and
bases react to form their (Y)
conjugates.
a.
b.
c.
d.
X = stronger,
X = stronger,
X = weaker,
X = weaker,
© 2015 Pearson Education, Inc.
Y = stronger
Y = weaker
Y = stronger
Y = weaker
For a conjugate acid–base
pair, Kw = Ka ___ Kb.
a.
b.
c.
d.
+
−

/
© 2015 Pearson Education, Inc.
For a conjugate acid–base
pair, Kw = Ka ___ Kb.
a.
b.
c.
d.
+
−

/
© 2015 Pearson Education, Inc.
The value of the ion-product
constant for water is
a.
b.
c.
d.
10−7.
10−14.
10+7.
impossible to determine without
additional information.
© 2015 Pearson Education, Inc.
The value of the ion-product
constant for water is
a.
b.
c.
d.
10−7.
10−14.
10+7.
impossible to determine without
additional information.
© 2015 Pearson Education, Inc.
What is the pH of a 0.0200 M
aqueous solution of HBr?
a.
b.
c.
d.
1.00
1.70
2.30
12.30
© 2015 Pearson Education, Inc.
What is the pH of a 0.0200 M
aqueous solution of HBr?
a.
b.
c.
d.
1.00
1.70
2.30
12.30
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What is the pH of a 0.0400 M
aqueous solution of KOH?
a.
b.
c.
d.
12.60
10.30
4.00
1.40
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What is the pH of a 0.0400 M
aqueous solution of KOH?
a.
b.
c.
d.
12.60
10.30
4.00
1.40
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What is the pH of a 0.0200 M
aqueous solution of HF? The
Ka of HF is 6.8  10−4.
a.
b.
c.
d.
1.70
2.43
3.17
12.30
© 2015 Pearson Education, Inc.
What is the pH of a 0.0200 M
aqueous solution of HF? The
Ka of HF is 6.8  10−4.
a.
b.
c.
d.
1.70
2.43
3.17
12.30
© 2015 Pearson Education, Inc.
A 0.30 M acid solution has a
pH of 1.85. What is the %
ionization?
a.
b.
c.
d.
21 %
16 %
6.2 %
4.7 %
© 2015 Pearson Education, Inc.
A 0.30 M acid solution has a
pH of 1.85. What is the %
ionization?
a.
b.
c.
d.
21 %
16 %
6.2 %
4.7 %
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What is the pH of a 0.100 M
aqueous solution of NH3?
The Kb of NH3 is 1.8  10−5.
a.
b.
c.
d.
2.87
4.74
9.26
11.13
© 2015 Pearson Education, Inc.
What is the pH of a 0.100 M
aqueous solution of NH3?
The Kb of NH3 is 1.8  10−5.
a.
b.
c.
d.
2.87
4.74
9.26
11.13
© 2015 Pearson Education, Inc.
What is the pH of a 0.0400 M
aqueous solution of KF? The
Ka of HF is 6.8  10−4.
a.
b.
c.
d.
2.28
2.43
6.12
7.88
© 2015 Pearson Education, Inc.
What is the pH of a 0.0400 M
aqueous solution of KF? The
Ka of HF is 6.8  10−4.
a.
b.
c.
d.
2.28
2.43
6.12
7.88
© 2015 Pearson Education, Inc.
What is the pH of a 1.0 
−8
10 M aqueous solution of
HBr?
a.
b.
c.
d.
6.00
6.96
7.04
8.00
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What is the pH of a 1.0 
−8
10 M aqueous solution of
HBr?
a.
b.
c.
d.
6.00
6.96
7.04
8.00
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Which of the following is not a
weak base?
a.
b.
c.
d.
NH3
NH2OH
F−
OH−
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Which of the following is not a
weak base?
a.
b.
c.
d.
NH3
NH2OH
F−
OH−
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Which of the following
correctly lists the acids in
order of decreasing strength?
a.
b.
c.
d.
HClO2 > HClO > HBrO > HIO
HClO > HBrO > HIO > HClO2
HIO > HBrO > HClO > HClO2
HClO2 > HIO > HBrO > HClO
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Which of the following
correctly lists the acids in
order of decreasing strength?
a.
b.
c.
d.
HClO2 > HClO > HBrO > HIO
HClO > HBrO > HIO > HClO2
HIO > HBrO > HClO > HClO2
HClO2 > HIO > HBrO > HClO
© 2015 Pearson Education, Inc.
Aqueous metal ions behave
as Lewis acids because they
a. can readily accept electrons in their
vacant d orbitals.
b. can readily donate electron pairs from
their outermost p orbitals.
c. attract electrons from the water
molecules they are dissolved in.
d. are attracted to the electronegative
oxygen atoms in the solvent.
© 2015 Pearson Education, Inc.
Aqueous metal ions behave
as Lewis acids because they
a. can readily accept electrons in their
vacant d orbitals.
b. can readily donate electron pairs from
their outermost p orbitals.
c. attract electrons from the water
molecules they are dissolved in.
d. are attracted to the electronegative
oxygen atoms in the solvent.
© 2015 Pearson Education, Inc.