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Clicker Questions Chapter 16

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Presentation on theme: "Clicker Questions Chapter 16"— Presentation transcript:

1 Clicker Questions Chapter 16
Barbara Mowery York College

2 A Brønsted–Lowry acid is
a proton donor. a proton acceptor. an electron-pair donor. d. an electron-pair acceptor. Answer: a

3 A Brønsted–Lowry acid is
a proton donor. a proton acceptor. an electron-pair donor. d. an electron-pair acceptor. Answer: a

4 A Brønsted–Lowry base is
a proton donor. a proton acceptor. an electron-pair donor. d. an electron-pair acceptor. Answer: b

5 A Brønsted–Lowry base is
a proton donor. a proton acceptor. an electron-pair donor. d. an electron-pair acceptor. Answer: b

6 A Lewis acid is a proton donor. a proton acceptor.
an electron-pair donor. d. an electron-pair acceptor. Answer: d

7 A Lewis acid is a proton donor. a proton acceptor.
an electron-pair donor. d. an electron-pair acceptor. Answer: d

8 A Lewis base is a proton donor. a proton acceptor.
an electron-pair donor. d. an electron-pair acceptor. Answer: c

9 A Lewis base is a proton donor. a proton acceptor.
an electron-pair donor. d. an electron-pair acceptor. Answer: c

10 Which of the following is the conjugate base of HPO42−?
d. HPO32− Answer: c

11 Which of the following is the conjugate base of HPO42−?
d. HPO32− Answer: c

12 Which species is amphiprotic?
H3PO4 H2PO41− PO43− d. None of these Answer: b

13 Which species is amphiprotic?
H3PO4 H2PO41− PO43− d. None of these Answer: b

14 Which of the following is the conjugate acid of SO42−?
H2SO4 HSO41− SO32− d. H3SO4+ Answer: b

15 Which of the following is the conjugate acid of SO42−?
H2SO4 HSO41− SO32− d. H3SO4+ Answer: b

16 The stronger the acid, the (X) its conjugate base
The stronger the acid, the (X) its conjugate base. Acids and bases react to form their (Y) conjugates. X = stronger, Y = stronger X = stronger, Y = weaker X = weaker, Y = stronger d. X = weaker, Y = weaker Answer: d

17 The stronger the acid, the (X) its conjugate base
The stronger the acid, the (X) its conjugate base. Acids and bases react to form their (Y) conjugates. X = stronger, Y = stronger X = stronger, Y = weaker X = weaker, Y = stronger d. X = weaker, Y = weaker Answer: d

18 For a conjugate acid–base pair, Kw = Ka ___ Kb.
+ d. / Answer: c

19 For a conjugate acid–base pair, Kw = Ka ___ Kb.
+ d. / Answer: c

20 The value of the ion-product constant for water is
10−7. 10−14. 10+7. d. impossible to determine without additional information. Answer: c

21 The value of the ion-product constant for water is
10−7. 10−14. 10+7. d. impossible to determine without additional information. Answer: c

22 What is the pH of a 0.0200 M aqueous solution of HBr?
1.00 1.70 2.30 d Answer: b

23 What is the pH of a 0.0200 M aqueous solution of HBr?
1.00 1.70 2.30 d Answer: b

24 What is the pH of a 0.0400 M aqueous solution of KOH?
12.60 10.30 4.00 d. 1.40 Answer: a

25 What is the pH of a 0.0400 M aqueous solution of KOH?
12.60 10.30 4.00 d. 1.40 Answer: a

26 What is the pH of a 0.0200 M aqueous solution of HF? The Ka of HF is 6.8  10−4.
1.70 2.43 3.17 d Answer: b

27 What is the pH of a 0.0200 M aqueous solution of HF? The Ka of HF is 6.8  10−4.
1.70 2.43 3.17 d Answer: b

28 A 0.30 M acid solution has a pH of 1.85. What is the % ionization?
21 % 16 % 6.2 % 4.7 % Answer: d

29 A 0.30 M acid solution has a pH of 1.85. What is the % ionization?
21 % 16 % 6.2 % 4.7 % Answer: d

30 What is the pH of a 0. 100 M aqueous solution of NH3
What is the pH of a M aqueous solution of NH3? The Kb of NH3 is 1.8  10−5. 2.87 4.74 9.26 d Answer: d

31 What is the pH of a 0. 100 M aqueous solution of NH3
What is the pH of a M aqueous solution of NH3? The Kb of NH3 is 1.8  10−5. 2.87 4.74 9.26 d Answer: d

32 What is the pH of a 0.0400 M aqueous solution of KF? The Ka of HF is 6.8  10−4.
2.28 2.43 6.12 d. 7.88 Answer: d

33 What is the pH of a 0.0400 M aqueous solution of KF? The Ka of HF is 6.8  10−4.
2.28 2.43 6.12 d. 7.88 Answer: d

34 What is the pH of a 1.0  10−8 M aqueous solution of HBr?
6.00 6.96 7.04 d. 8.00 Answer: b

35 What is the pH of a 1.0  10−8 M aqueous solution of HBr?
6.00 6.96 7.04 d. 8.00 Answer: b

36 Which of the following is not a weak base?
NH3 NH2OH F− OH− Answer: d

37 Which of the following is not a weak base?
NH3 NH2OH F− OH− Answer: d

38 Which of the following correctly lists the acids in order of decreasing strength?
HClO2 > HClO > HBrO > HIO HClO > HBrO > HIO > HClO2 HIO > HBrO > HClO > HClO2 d. HClO2 > HIO > HBrO > HClO Answer: a

39 Which of the following correctly lists the acids in order of decreasing strength?
HClO2 > HClO > HBrO > HIO HClO > HBrO > HIO > HClO2 HIO > HBrO > HClO > HClO2 d. HClO2 > HIO > HBrO > HClO Answer: a

40 Aqueous metal ions behave as Lewis acids because they
can readily accept electrons in their vacant d orbitals. can readily donate electron pairs from their outermost p orbitals. attract electrons from the water molecules they are dissolved in. d. are attracted to the electronegative oxygen atoms in the solvent. Answer: a

41 Aqueous metal ions behave as Lewis acids because they
can readily accept electrons in their vacant d orbitals. can readily donate electron pairs from their outermost p orbitals. attract electrons from the water molecules they are dissolved in. d. are attracted to the electronegative oxygen atoms in the solvent. Answer: a


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