Acids And Bases Chapter.3 Exam Questions

Organic Chemistry, 4e (Klein)

Chapter 3 Acids and Bases

1) A Brønsted-Lowry acid is defined as a ________.

A) proton acceptor

B) proton donor

C) species remaining after acid is deprotonated

D) species remaining after base is protonated

E) species that can react with water

Diff: 1

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

2) A Brønsted-Lowry base is defined as a ________.

A) proton acceptor

B) proton donor

C) species remaining after acid is deprotonated

D) species remaining after base is protonated

E) species that can react with water

Diff: 1

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

3) A conjugate acid is defined as a ________.

A) proton acceptor

B) proton donor

C) species remaining after acid is deprotonated

D) species remaining after base is protonated

E) species that can react with water

Diff: 1

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

4) A conjugate base is defined as a ________.

A) proton acceptor

B) proton donor

C) species remaining after acid is deprotonated

D) species remaining after base is protonated

E) species that can react with water

Diff: 1

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

5) For the following reaction, identify the Brønsted-Lowry base and the conjugate acid.

A) I and II

B) I and III

C) I and IV

D) II and IIII

E) II and IV

Diff: 1

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

6) For the following reaction, identify the Brønsted-Lowry acid and the conjugate acid.

A) I and II

B) I and III

C) I and IV

D) II and IIII

E) II and IV

Diff: 1

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

7) For the following reaction, identify the Brønsted-Lowry base and the corresponding conjugate base.

A) I and II

B) I and III

C) I and IV

D) II and IIII

E) II and IV

Diff: 1

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

8) For the following reaction, identify the Brønsted-Lowry acid and the conjugate base.

A) I and II

B) I and III

C) I and IV

D) II and IIII

E) II and IV

Diff: 1

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

9) For the following reaction, identify the Brønsted-Lowry base and the conjugate base.

A) I and II

B) I and III

C) I and IV

D) II and IIII

E) II and IV

Diff: 1

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

10) Which of the following is not a Brønsted-Lowry acid?

A) CH3OH

B) CBr4

C) HCl

D) CH3SH

E) H2O

Diff: 2

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

11) Which of the following is not a Brønsted-Lowry base?

A) CH3OH

B) CH3OCH3

C) CH3NH2

D) CH3CH3

E) CH3SH

Diff: 2

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

12) In a Brønsted-Lowry acid-base reaction, the acid is defined as ________.

A) a proton acceptor

B) a proton donor

C) the product resulting from loss of a proton

D) the product resulting from gaining a proton

E) the most reactive species

Diff: 1

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

13) In a Brønsted-Lowry acid-base reaction, the base is defined as ________.

A) a proton acceptor

B) a proton donor

C) the product resulting from loss of a proton

D) the product resulting from gaining a proton

E) the most reactive species

Diff: 1

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

14) Which of the following is always formed from the loss of proton from a Brønsted-Lowry acid?

A) a Lewis acid

B) a conjugate acid

C) a conjugate base

D) a species with a negative charge

E) a neutral solution

Diff: 1

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

15) Which of the following is always formed from the gain of proton by a Brønsted-Lowry base?

A) a Lewis base

B) a conjugate acid

C) a conjugate base

D) a species with a positive charge

E) a neutral solution

Diff: 1

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

16) Identify the conjugate base of nitric acid, HNO3.

A) NO3—

B) NO2—

C) HNO3

D) HNO2

E) H2NO3+

Diff: 2

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

17) Identify the conjugate base of phosphoric acid, H3PO4.

A) HPO42—

B) H2PO4—

C) HPO32—

D) PO43—

E) H2PO3—

Diff: 2

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

18) Identify the conjugate base of CH3CH2SH.

A) CH3CH2S—

B) CH3CH2—

C) CH3CH2SH2+

D) CH3CH2S2—

E) CH3CH2+

Diff: 1

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

19) Identify the conjugate acid of CH3CH2OH.

A) I

B) II

C) III

D) IV

E) V

Diff: 1

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

20) Identify the conjugate acid of CH3-O-CH3.

A) I

B) II

C) III

D) IV

E) V

Diff: 1

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

21) Identify the conjugate acid of the compound shown in the box below.

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

22) Identify the conjugate base of CH3C≡CH.

A) I

B) II

C) III

D) IV

E) V

Diff: 1

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

23) Identify the conjugate base of CH3CH2NH2.

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

24) Identify the conjugate base of the compound shown in the box below.

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

25) Identify the conjugate base of the compound shown in the box below.

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

26) For the following reaction, respectively identify the Brønsted-Lowry base and the conjugate base.

A) I and II

B) I and III

C) I and IV

D) II and IIII

E) II and IV

Diff: 2

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

27) For the following reaction, respectively identify the Brønsted-Lowry base and the conjugate acid.

A) I and II

B) I and III

C) I and IV

D) II and IIII

E) II and IV

Diff: 2

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

28) For the following reaction, respectively identify the Brønsted-Lowry acid and the conjugate base.

A) I and II

B) I and III

C) I and IV

D) II and IIII

E) II and IV

Diff: 2

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

29) For the following reaction, respectively identify the Brønsted-Lowry acid and the conjugate acid.

A) I and II

B) I and III

C) I and IV

D) II and IIII

E) II and IV

Diff: 2

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

30) For the following reaction identify the acid, base, conjugate acid and conjugate base.

A) I = base; II = acid; III = conjugate base; IV = conjugate acid

B) I = acid; II = base; III = conjugate base; IV = conjugate acid

C) I = base; II = acid; III = conjugate acid; IV = conjugate base

D) I = acid; II = base; III = conjugate acid; IV = conjugate base

E) I = base; II = base; III = conjugate acid; IV = conjugate acid

Diff: 2

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

31) For the following reaction identify the acid, base, conjugate acid and conjugate base.

A) I = base; II = acid; III = conjugate base; IV = conjugate acid

B) I = acid; II = base; III = conjugate base; IV = conjugate acid

C) I = base; II = acid; III = conjugate acid; IV = conjugate base

D) I = acid; II = base; III = conjugate acid; IV = conjugate base

E) I = base; II = base; III = conjugate acid; IV = conjugate acid

Diff: 2

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

32) For the following reaction identify the acid, base, conjugate acid and conjugate base.

A) I = base; II = acid; III = conjugate base; IV = conjugate acid

B) I = acid; II = base; III = conjugate base; IV = conjugate acid

C) I = base; II = acid; III = conjugate acid; IV = conjugate base

D) I = acid; II = base; III = conjugate acid; IV = conjugate base

E) I = base; II = base; III = conjugate acid; IV = conjugate acid

Diff: 2

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

33) The tail of the curved arrow must start at ________ electron density and the head must end at ________ electron density.

A) low, high

B) high, high

C) low, low

D) high, low

E) none of the above

Diff: 1

Learning Objective: 3.2 Use curved arrow representation to show flow of electrons in acid-base reactions

34) For the following acid-base reaction, identify the correct curved arrow mechanism.

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 3.2 Use curved arrow representation to show flow of electrons in acid-base reactions

35) For the following acid-base reaction, identify the correct curved arrow mechanism.

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 3.2 Use curved arrow representation to show flow of electrons in acid-base reactions

36) For the following acid-base reaction, identify the correct curved arrow mechanism.

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 3.2 Use curved arrow representation to show flow of electrons in acid-base reactions

37) For the following acid-base reaction, identify the correct curved arrow mechanism.

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 3.2 Use curved arrow representation to show flow of electrons in acid-base reactions

38) For the following acid-base reaction, identify the correct curved arrow mechanism.

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 3.2 Use curved arrow representation to show flow of electrons in acid-base reactions

39) For the following acid-base reaction, identify the correct curved arrow mechanism.

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 3.2 Use curved arrow representation to show flow of electrons in acid-base reactions

40) The following reaction mechanism contains mistakes. Which of the following statements correctly describes how the curved arrows should be drawn?

A) The curved arrow should start at the oxygen atom labeled (I).

B) The curved arrow should start at the hydride (IV), go to hydrogen atom (II) with a second arrow starting from the O–H bond and going to the oxygen atom (I).

C) The curved arrow should start at the O–H bond and go to hydride (IV).

D) There should be and additional arrow from the oxygen atom (I) to the sodium ion (III).

E) There should be an arrow from the oxygen atom (I) to the hydrogen atom (II).

Diff: 2

Learning Objective: 3.2 Use curved arrow representation to show flow of electrons in acid-base reactions

41) The following reaction mechanism contains mistakes. Which of the following statements correctly describes how the first curved arrows should be drawn?

A) The curved arrow should start at sodium ion labeled (III)

B) The curved arrow should start at the hydrogen atom labeled (II)

C) The curved arrow should end at the bond between the oxygen atom (I) and the hydrogen atom (II)

D) The curved arrow should start at the nitrogen atom labeled (IV)

E) There should be an arrow from the oxygen atom (I) to the hydrogen atom (II)

Diff: 2

Learning Objective: 3.2 Use curved arrow representation to show flow of electrons in acid-base reactions

42) The following reaction mechanism contains mistakes. Which of the following statements correctly describes how the first curved arrows should be drawn?

A) The first arrow (I) should start at the sodium ion.

B) The second arrow (II) should go in the opposite direction.

C) The second arrow (II) should start at the bond between the H and Br.

D) The arrow labeled II should go in the opposite direction.

E) The arrow labeled II is unnecessary.

Diff: 2

Learning Objective: 3.2 Use curved arrow representation to show flow of electrons in acid-base reactions

43) Identify the structure produced by the following acid-base reaction mechanism.

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 3.2 Use curved arrow representation to show flow of electrons in acid-base reactions

44) Identify the structure produced by the following acid-base reaction mechanism.

A) I

B) II

C) III

D) IV

E) V

Diff: 3

Learning Objective: 3.2 Use curved arrow representation to show flow of electrons in acid-base reactions

45) What is the Keq for the following reaction?

A) I

B) II

C) III

D) IV

E) V

Diff: 1

Learning Objective: 3.3 Use pKa values to compare acidity and basicity and to predict the position of equilibrium

46) Which of the following compounds is most acidic?

A) I

B) II

C) III

D) IV

E) V

Diff: 1

Learning Objective: 3.3 Use pKa values to compare acidity and basicity and to predict the position of equilibrium

47) Which of the following compounds is most basic?

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 3.3 Use pKa values to compare acidity and basicity and to predict the position of equilibrium

48) Which of the following compounds is most acidic?

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 3.3 Use pKa values to compare acidity and basicity and to predict the position of equilibrium

49) Which of the following compounds is most basic?

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 3.3 Use pKa values to compare acidity and basicity and to predict the position of equilibrium

50) Which of the following compounds is most basic?

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 3.3 Use pKa values to compare acidity and basicity and to predict the position of equilibrium

51) For the compound shown below, rank the indicated protons in order of increasing acidity.

A) Least acidic: I < II < III Most acidic

B) Least acidic: II < III < I Most acidic

C) Least acidic: III < I < II Most acidic

D) Least acidic: I < III < II Most acidic

E) Least acidic: II < I < III Most acidic

Diff: 3

Learning Objective: 3.3 Use pKa values to compare acidity and basicity and to predict the position of equilibrium

52) Histidine, an amino acid, is shown below. Rank the indicated protons in order of increasing acidity.

A) Least acidic: I < II < III Most acidic

B) Least acidic: II < III < I Most acidic

C) Least acidic: III < I < II Most acidic

D) Least acidic: I < III < II Most acidic

E) Least acidic: II < I < III Most acidic

Diff: 3

Learning Objective: 3.3 Use pKa values to compare acidity and basicity and to predict the position of equilibrium

53) For the following acid-base reaction, predict the position of the equilibrium and identify the most stable base.

A) favor the right side with compound I being the most stable base

B) favor the right side with compound II being the most stable base

C) favor the right side with compound III being the most stable base

D) favor the left side with compound I being the most stable base

E) favor the left side with compound II being the most stable base

Diff: 2

Learning Objective: 3.3 Use pKa values to compare acidity and basicity and to predict the position of equilibrium

54) For the following acid-base reaction, predict the position of the equilibrium and identify the most acidic compound.

A) favor the right side with compound I being the most acidic compound

B) favor the right side with compound II being the most acidic compound

C) favor the left side with compound I being the most acidic compound

D) favor the left side with compound II being the most acidic compound

E) favor the left side with compound III being the most acidic compound

Diff: 2

Learning Objective: 3.3 Use pKa values to compare acidity and basicity and to predict the position of equilibrium

55) For the following acid-base reaction, predict the position of the equilibrium and identify the most acidic compound.

A) favor the right side with compound I being the most acidic compound

B) favor the right side with compound II being the most acidic compound

C) favor the left side with compound I being the most acidic compound

D) favor the left side with compound II being the most acidic compound

E) favor the left side with compound III being the most acidic compound

Diff: 3

Learning Objective: 3.3 Use pKa values to compare acidity and basicity and to predict the position of equilibrium

56) For the following acid-base reaction, predict the position of the equilibrium and identify the most stable base.

A) favor the right side with compound I being the most stable base

B) favor the right side with compound II being the most stable base

C) favor the right side with compound III being the most stable base

D) favor the left side with compound I being the most stable base

E) favor the left side with compound II being the most stable base

Diff: 3

Learning Objective: 3.3 Use pKa values to compare acidity and basicity and to predict the position of equilibrium

57) Which of the following compounds is most acidic?

A) HF

B) HCl

C) HBr

D) HI

E) H2O

Diff: 1

Learning Objective: 3.4 Compare acidity and basicity of compounds based on structural (qualitative) analysis, including conjugate base stability and a comparison of the stability of negative charges (ARIO)

58) Which of the following compounds is most acidic?

A) CH3OH

B) HCl

C) HF

D) CH3SH

E) CH3NH2

Diff: 1

Learning Objective: 3.4 Compare acidity and basicity of compounds based on structural (qualitative) analysis, including conjugate base stability and a comparison of the stability of negative charges (ARIO)

59) Which of the following best explains which compound is more acidic?

HF or HBr

A) HF is more acidic due to the F atom being more electronegative than Br

B) HBr is more acidic due to the Br atom being less electronegative than F

C) HF is more acidic due to the F— anion being smaller than Br—

D) HBr is more acidic due to the Br— anion being larger than F—

E) HF is capable of participating in hydrogen bonding and therefore is a strong acid

Diff: 2

Learning Objective: 3.4 Compare acidity and basicity of compounds based on structural (qualitative) analysis, including conjugate base stability and a comparison of the stability of negative charges (ARIO)

60) Which of the following best explains which compound is more acidic?

CH3OH and CH3NH2

A) CH3OH is more acidic due to oxygen being more electronegative than nitrogen

B) CH3NH2 is more acidic due to nitrogen being less electronegative than oxygen

C) CH3OH is more acidic as it results in a stronger conjugate base

D) CH3NH2 is more acidic as it results in a stronger conjugate base

E) Both compounds are capable of hydrogen bonding and are of equal acidity

Diff: 2

Learning Objective: 3.4 Compare acidity and basicity of compounds based on structural (qualitative) analysis, including conjugate base stability and a comparison of the stability of negative charges (ARIO)

61) Which of the following best explains which proton is more acidic?

A) The H (I) attached to S is more acidic due to oxygen being more electronegative.

B) The H (II) attached to O is more acidic due to sulfur being more electronegative.

C) The H (I) attached to S is more acidic due to sulfur being more electronegative.

D) The H (II) attached to O is more acidic due to oxygen being more electronegative.

E) The H (I) attached to S is more acidic due to the sulfur being larger than oxygen.

Diff: 2

Learning Objective: 3.4 Compare acidity and basicity of compounds based on structural (qualitative) analysis, including conjugate base stability and a comparison of the stability of negative charges (ARIO)

62) Rank the indicated protons in order of increasing acidity.

A) Least acidic: I < II < III Most acidic

B) Least acidic: II < III < I Most acidic

C) Least acidic: III < I < II Most acidic

D) Least acidic: I < III < II Most acidic

E) Least acidic: II < I < III Most acidic

Diff: 2

Learning Objective: 3.4 Compare acidity and basicity of compounds based on structural (qualitative) analysis, including conjugate base stability and a comparison of the stability of negative charges (ARIO)

63) Which of the following compounds is most acidic?

A) I

B) II

C) III

D) IV

E) V

Diff: 1

Learning Objective: 3.4 Compare acidity and basicity of compounds based on structural (qualitative) analysis, including conjugate base stability and a comparison of the stability of negative charges (ARIO)

64) Consider the shown proton on each compound and identify which is most acidic.

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 3.4 Compare acidity and basicity of compounds based on structural (qualitative) analysis, including conjugate base stability and a comparison of the stability of negative charges (ARIO)

65) Rank the indicated protons in decreasing order of acidity.

A) Most acidic: II > I > III Least acidic

B) Most acidic: II > III > I Least acidic

C) Most acidic: I > III > II Least acidic

D) Most acidic: I > II > III Least acidic

E) Most acidic: III > II > I Least acidic

Diff: 2

Learning Objective: 3.4 Compare acidity and basicity of compounds based on structural (qualitative) analysis, including conjugate base stability and a comparison of the stability of negative charges (ARIO)

66) Which compound has the most acidic proton?

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 3.4 Compare acidity and basicity of compounds based on structural (qualitative) analysis, including conjugate base stability and a comparison of the stability of negative charges (ARIO)

67) Which of the following compounds is most acidic?

A) I

B) II

C) III

D) IV

E) V

Diff: 1

Learning Objective: 3.4 Compare acidity and basicity of compounds based on structural (qualitative) analysis, including conjugate base stability and a comparison of the stability of negative charges (ARIO)

68) Which of the following compounds is most acidic?

A) I

B) II

C) III

D) IV

E) V

Diff: 1

Learning Objective: 3.4 Compare acidity and basicity of compounds based on structural (qualitative) analysis, including conjugate base stability and a comparison of the stability of negative charges (ARIO)

69) Which of the following compounds is most acidic?

A) I

B) II

C) III

D) IV

E) V

Diff: 1

Learning Objective: 3.4 Compare acidity and basicity of compounds based on structural (qualitative) analysis, including conjugate base stability and a comparison of the stability of negative charges (ARIO)

70) Which of the following compounds is most acidic?

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 3.4 Compare acidity and basicity of compounds based on structural (qualitative) analysis, including conjugate base stability and a comparison of the stability of negative charges (ARIO)

71) Rank the following compounds in decreasing order of acidity.

A) III > II > IV > I

B) II > IV > III > II

C) IV > III > II > I

D) IV > II > III > I

E) III > IV > II > I

Diff: 3

Learning Objective: 3.4 Compare acidity and basicity of compounds based on structural (qualitative) analysis, including conjugate base stability and a comparison of the stability of negative charges (ARIO)

72) Which of the indicated protons is most acidic?

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 3.4 Compare acidity and basicity of compounds based on structural (qualitative) analysis, including conjugate base stability and a comparison of the stability of negative charges (ARIO)

73) Which of the following best explains which proton is more acidic?

A) The H (I) is more acidic due to having less carbons attached to the nitrogen

B) The H (II) is more acidic due to having less carbons attached to the nitrogen

C) The H (I) is more acidic due to be closer to the inductive effects of the fluorine atoms

D) The H (II) is more acidic due to be closer to the inductive effects of the fluorine atoms

E) The H (II) is more acidic due to the fluorine atoms being further away

Diff: 2

Learning Objective: 3.4 Compare acidity and basicity of compounds based on structural (qualitative) analysis, including conjugate base stability and a comparison of the stability of negative charges (ARIO)

74) Which of the following best explains why phenol is more acidic than ethanol.

A) The conjugate base of phenol is resonance stabilized, resulting in a weaker conjugate base.

B) The conjugate base of phenol is resonance stabilized, resulting in a stronger conjugate base.

C) The conjugate base of phenol has a localized charge, resulting in a stronger conjugate base.

D) The conjugate base of ethanol has a localized charge.

E) The conjugate base of ethanol has a delocalized charge.

Diff: 2

Learning Objective: 3.4 Compare acidity and basicity of compounds based on structural (qualitative) analysis, including conjugate base stability and a comparison of the stability of negative charges (ARIO)

75) Consider the shown proton on each molecule below, and select the statement that best explains which compound is more acidic.

A) Compound II is more acidic; the conjugate base of compound I has the negative charge on the more electronegative oxygen atom.

B) Compound I is more acidic; the conjugate base of compound I has the negative charge on the more electronegative oxygen atom.

C) Compound II is more acidic; the conjugate base of compound II has the negative charge on the more electronegative oxygen atom.

D) Compound I is more acidic; the conjugate base of compound II has the negative charge on the more electronegative oxygen atom.

E) Both compounds are equally stable as both protons are adjacent to a double bond.

Diff: 2

Learning Objective: 3.4 Compare acidity and basicity of compounds based on structural (qualitative) analysis, including conjugate base stability and a comparison of the stability of negative charges (ARIO)

76) Aspartic acid, an amino acid, has the structure shown below. Which of the following best explains which proton is most acidic?

A) Proton I is most acidic due to conjugate base stabilization by resonance and being further from the inductive effect of the positive nitrogen atom.

B) Proton II is most acidic due being attached to the carbon closest to the positive nitrogen atom.

C) Proton III is most acidic due to being attached to a positive nitrogen atom.

D) Proton IV is most acidic due to conjugate base stabilization by resonance and being closer to the inductive effect of the positive nitrogen atom.

E) Proton V is most acidic due to the possibility of conjugate base stabilization by resonance with the adjacent C=O bond.

Diff: 3

Learning Objective: 3.4 Compare acidity and basicity of compounds based on structural (qualitative) analysis, including conjugate base stability and a comparison of the stability of negative charges (ARIO)

77) For the following acid-base reaction, predict the position of the equilibrium and identify the most acidic compound.

A) favor the right side with compound I being the most acidic compound

B) favor the right side with compound III being the most acidic compound

C) favor the left side with compound I being the most acidic compound

D) favor the left side with compound III being the most acidic compound

E) The reaction is at equilibrium so all the compounds are in equal concentration

Diff: 1

Learning Objective: 3.6 Predict the equilibrium position of a reaction based on a comparison of the conjugate bases

78) For the following acid-base reaction, predict the position of the equilibrium and identify the most acidic compound.

A) favor the right side with compound I being the most acidic compound

B) favor the right side with compound III being the most acidic compound

C) favor the left side with compound I being the most acidic compound

D) favor the left side with compound III being the most acidic compound

E) The reaction is at equilibrium so all the compounds are in equal concentration

Diff: 1

Learning Objective: 3.6 Predict the equilibrium position of a reaction based on a comparison of the conjugate bases

79) For the following acid-base reaction, predict the position of the equilibrium and identify the most acidic compound.

A) favor the right side with compound I being the most acidic compound

B) favor the right side with compound II being the most acidic compound

C) favor the right side with compound III being the most acidic compound

D) favor the left side with compound III being the most acidic compound

E) favor the left side with compound II being the most acidic compound

Diff: 1

Learning Objective: 3.6 Predict the equilibrium position of a reaction based on a comparison of the conjugate bases

80) For the following acid-base reaction, predict the position of the equilibrium and identify the most acidic compound.

A) favor the right side with compound I being the most acidic compound

B) favor the right side with compound III being the most acidic compound

C) favor the left side with compound I being the most acidic compound

D) favor the left side with compound III being the most acidic compound

E) the reaction is at equilibrium so all the compounds are in equal concentration

Diff: 1

Learning Objective: 3.6 Predict the equilibrium position of a reaction based on a comparison of the conjugate bases

81) For the following acid-base reaction, predict the position of the equilibrium and identify the most stable base.

A) favor the right side with compound I being the most stable base

B) favor the right side with compound IV being the most stable base

C) favor the left side with compound I being the most stable base

D) favor the left side with compound II being the most stable base

E) the reaction is at equilibrium so all the compounds are in equal concentration

Diff: 2

Learning Objective: 3.6 Predict the equilibrium position of a reaction based on a comparison of the conjugate bases

82) For the following acid-base reaction, predict the position of the equilibrium and identify the most stable base.

A) favor the right side with compound I being the most stable base

B) favor the right side with compound II being the most stable base

C) favor the left side with compound I being the most stable base

D) favor the left side with compound II being the most stable base

E) favor the left side with compound III being the most stable base

Diff: 2

Learning Objective: 3.6 Predict the equilibrium position of a reaction based on a comparison of the conjugate bases

83) Determine if H2O is a suitable reagent to protonate each of the two compounds shown below.

A) I = yes; II = no

B) I = no; II = no

C) I = no; II = yes

D) I = yes; II = yes

E) Not possible to determine with the information provided

Diff: 2

Learning Objective: 3.6 Predict the equilibrium position of a reaction based on a comparison of the conjugate bases

84) Determine if H2O is a suitable reagent to protonate each of the two compounds shown below.

A) I = yes; II = no

B) I = no; II = no

C) I = no; II = yes

D) I = yes; II = yes

E) Not possible to determine with the information provided

Diff: 2

Learning Objective: 3.6 Predict the equilibrium position of a reaction based on a comparison of the conjugate bases

85) Which of the following best explains if H2O is a suitable reagent to protonate the compound shown below.

A) no, water would not protonate the compound as the resulting conjugate base would not be stabilized by resonance

B) no, water would not protonate the compound as the negative charge is more stable on the nitrogen atom

C) no, water would not protonate the compound as both water and the nitrogen in the compound have two bonds

D) yes, water would protonate the compound as the resulting conjugate base would be stabilized by resonance

E) yes, water would protonate the compound as the resulting conjugate base would have a negative on the more electronegative oxygen atom

Diff: 2

Learning Objective: 3.6 Predict the equilibrium position of a reaction based on a comparison of the conjugate bases

86) Determine if NaOH is a suitable reagent to deprotonate each of the two compounds shown below.

A) I = yes; II = no

B) I = no; II = no

C) I = yes; II = yes

D) I = no; II = yes

E) Not possible to determine with the information provided

Diff: 2

Learning Objective: 3.6 Predict the equilibrium position of a reaction based on a comparison of the conjugate bases

87) Determine if NaNH2 is a suitable reagent to deprotonate each of the two compounds shown below.

A) I = yes; II = yes

B) I = no; II = no

C) I = no; II = yes

D) I = yes; II = no

E) Not possible to determine with the information provided

Diff: 2

Learning Objective: 3.6 Predict the equilibrium position of a reaction based on a comparison of the conjugate bases

88) Which of the following best explains if NaOH is a suitable reagent to deprotonate the compound shown below?

A) no, there are no protons attached to the sp2 carbons

B) no, the compound would not be soluble in NaOH

C) no, NaOH has a negative charge on an oxygen atom, whereas the compound's conjugate base would have a negative charge on the carbon atom

D) yes, NaOH is considered a strong base

E) yes, protons attached to sp2 carbons are more acidic than those attached to sp3 carbons

Diff: 3

Learning Objective: 3.6 Predict the equilibrium position of a reaction based on a comparison of the conjugate bases

89) Which of the following best explains if NaNH2 is a suitable reagent to deprotonate the compound shown below?

A) no, the resulting conjugate base would have a localized negative on a carbon atom where NaNH2 has a negative on the more electronegative nitrogen atom

B) no, there are no acidic protons attached to the oxygen atoms

C) no, NaNH2 produces NH3 when protonated which then will leave the reaction mixture

D) yes, the resulting conjugate base would have delocalization of charge over two oxygen atoms, whereas NaNH2 has a localized negative charge.

E) yes, as NaNH2 has only two hydrogen atoms attached to the nitrogen atom, and the compound has eight total hydrogen atoms

Diff: 3

Learning Objective: 3.6 Predict the equilibrium position of a reaction based on a comparison of the conjugate bases

90) Which of the following best explains if CH3CH2ONa is a suitable reagent to deprotonate the compound shown below?

A) no, CH3CH2ONa would not deprotonate the compound since nitrogen has a lone pair and will not act as an acid

B) no, CH3CH2ONa has a negative charge on an oxygen atom, whereas the compound's conjugate base would have a negative charge on a nitrogen atom

C) yes, if deprotonated the negative charge would be more stable on the nitrogen atom

D) yes, CH3CH2ONa is considered a strong base

E) yes, the nitrogen atom has a proton that can be donated to an appropriate base

Diff: 3

Learning Objective: 3.6 Predict the equilibrium position of a reaction based on a comparison of the conjugate bases

91) Which of the following best explains if H2O is a suitable reagent to protonate the compound shown below?

A) no, water would not protonate the compound as the negative charge is more stable on the larger sulfur atom

B) no, water would not protonate the compound as the resulting conjugate base would not be stabilized by resonance

C) yes, water would protonate the compound the sodium ion rather be a counter ion to oxygen than sulfur

D) yes, water would protonate the compound as the resulting conjugate base would be stabilized by resonance

E) yes, water would protonate the compound as the resulting conjugate base would have a negative on the more electronegative oxygen atom

Diff: 3

Learning Objective: 3.6 Predict the equilibrium position of a reaction based on a comparison of the conjugate bases

92) Which of the following best describes the leveling effect?

A) the ability of a compound to dissolve in a given amount of solvent

B) the limiting of a compound's acidity or basicity by respective deprotonation or protonation by the solvent

C) the cause of weak acids or weak bases to incompletely dissociate in water

D) the reason that explains why moving down the periodic table results in compounds that are more acidic

E) the reduction of inductive effects as electronegative atoms are moved further from the acidic proton

Diff: 2

Learning Objective: 3.7 Describe the significance in understanding leveling effects

93) Which of the following solvents can be used with NaNH2?

A) CH3CH2OH

B) CH3OH

C) H2O

D) Liquid NH3

E) CH3CO2H

Diff: 2

Learning Objective: 3.7 Describe the significance in understanding leveling effects

94) Which of the following solvents cannot be used with (CH3)3COK?

A) (CH3CH2)2O

B) (CH3)3COH

C) H2O

D) Liquid NH3

E) Tetrahydrofuran (THF)

Diff: 2

Learning Objective: 3.7 Describe the significance in understanding leveling effects

95) Which of the following solvents can be used with (CH3)3CLi?

A) CH3CH2OH

B) CH3OH

C) H2O

D) Liquid NH3

E) CH3(CH2)4CH3

Diff: 2

Learning Objective: 3.7 Describe the significance in understanding leveling effects

96) As a result of the "leveling effect," the strongest acid that can exist in appreciable concentration in aqueous solution is ________.

A) H2SO4

B) HCl

C) H3O+

D) HNO3

E) H2O

Diff: 1

Learning Objective: 3.7 Describe the significance in understanding leveling effects

97) As a result of the "leveling effect," the strongest base that can exist in appreciable concentration in aqueous solution is ________.

A) (CH3)3CLi

B) NaNH2

C) H3O+

D) HO—

E) H2O

Diff: 1

Learning Objective: 3.7 Describe the significance in understanding leveling effects

98) Why is ethanol a better solvating solvent than tert-butyl alcohol?

A) ethanol is less sterically hindered and more capable of interacting with the solute

B) tert-butyl alcohol is less sterically hindered and more capable of interacting with the solute

C) ethanol is less sterically hindered and less capable of interacting with the solute

D) tert-butyl alcohol is less sterically hindered and less capable of interacting with the solute

E) tert-butyl alcohol has more carbons than ethanol making it more soluble in aqueous solutions

Diff: 1

Learning Objective: 3.8 Describe the significance in understanding solvating and steric effects

99) Identify the most sterically hindered alcohol.

A) CH3OH

B) CH3CH2OH

C) (CH3)2CHOH

D) (CH3)3COH

E) CH3CH2CH2CH2OH

Diff: 1

Learning Objective: 3.8 Describe the significance in understanding solvating and steric effects

100) What is a cation?

A) a negatively charged ion

B) a positively charged ion

C) a sodium atom

D) a hydrogen molecule

E) an atom that has gained electrons

Diff: 1

Learning Objective: 3.9 Explain what is meant by a counterion

101) What is the counterion in NaOCH2CH3?

A) Na+

B) NaO—

C) CH3CH2—

D) CH3CH2O—

E) Na—

Diff: 1

Learning Objective: 3.9 Explain what is meant by a counterion

102) What is the counterion in (CH3)3CLi?

A) CH3+

B) CH3—

C) (CH3)3C—

D) Li+

E) (CH3)3C+

Diff: 1

Learning Objective: 3.9 Explain what is meant by a counterion

103) What is a counterion in (CH3)3COK?

A) K—

B) (CH3)3CO+

C) KO—

D) (CH3)3CO—

E) K+

Diff: 1

Learning Objective: 3.9 Explain what is meant by a counterion

104) A Lewis acid is defined as ________.

A) a proton donor

B) an electron pair donor

C) a proton acceptor

D) an electron pair acceptor

E) a species that generates OH— in water

Diff: 1

Learning Objective: 3.10 Describe how Lewis acids and bases differ from Brønsted-Lowry acids and bases

105) A Lewis base is defined as ________.

A) a proton donor

B) an electron pair donor

C) a proton acceptor

D) an electron pair acceptor

E) a species that generates H+ in water

Diff: 1

Learning Objective: 3.10 Describe how Lewis acids and bases differ from Brønsted-Lowry acids and bases

106) CH3CH2OCH2CH3, is best classified as a ________.

A) Brønsted-Lowry acid

B) Lewis acid

C) Brønsted-Lowry base

D) Lewis base

E) Both C and D

Diff: 2

Learning Objective: 3.10 Describe how Lewis acids and bases differ from Brønsted-Lowry acids and bases

107) BF3, is best classified as a ________.

A) Brønsted-Lowry acid

B) Lewis acid

C) Brønsted-Lowry base

D) Lewis base

E) Both A and D

Diff: 1

Learning Objective: 3.10 Describe how Lewis acids and bases differ from Brønsted-Lowry acids and bases

108) The following compound is best classified as a ________.

A) Brønsted-Lowry acid

B) Lewis acid

C) Brønsted-Lowry base

D) Lewis base

E) Both C and D

Diff: 1

Learning Objective: 3.10 Describe how Lewis acids and bases differ from Brønsted-Lowry acids and bases

109) The following compound is best classified as a ________.

A) Brønsted-Lowry acid

B) Lewis acid

C) Brønsted-Lowry base

D) Lewis base

E) Both C and D

Diff: 1

Learning Objective: 3.10 Describe how Lewis acids and bases differ from Brønsted-Lowry acids and bases

110) Which of the following compounds is not a Lewis acid?

A) BH3

B) AlCl3

C) CBr4

D) CH3CH2+

E) FeBr3

Diff: 2

Learning Objective: 3.10 Describe how Lewis acids and bases differ from Brønsted-Lowry acids and bases

111) Which of the following compounds is not a Lewis acid?

A) BF3

B) FeCl3

C) CH3CH2+

D) Ph3P

E) AlBr3

Diff: 2

Learning Objective: 3.10 Describe how Lewis acids and bases differ from Brønsted-Lowry acids and bases

112) For the following reaction, identify the Lewis acid.

A) I

B) II

C) III

D) Both I and III

E) Both II and III

Diff: 1

Learning Objective: 3.10 Describe how Lewis acids and bases differ from Brønsted-Lowry acids and bases

113) For the following reaction, identify the Lewis acid.

A) I

B) II

C) III

D) Both I and III

E) Both II and III

Diff: 1

Learning Objective: 3.10 Describe how Lewis acids and bases differ from Brønsted-Lowry acids and bases

114) For the following reaction, identify the Lewis acid.

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 3.10 Describe how Lewis acids and bases differ from Brønsted-Lowry acids and bases

115) For the following reaction, identify the Lewis acid.

A) I

B) II

C) III

D) Both I and III

E) Both II and III

Diff: 2

Learning Objective: 3.10 Describe how Lewis acids and bases differ from Brønsted-Lowry acids and bases

116) For the following reaction, identify the Lewis base.

A) I

B) II

C) III

D) Both I and III

E) Both II and III

Diff: 1

Learning Objective: 3.10 Describe how Lewis acids and bases differ from Brønsted-Lowry acids and bases

117) For the following reaction, identify the Lewis base.

A) I

B) II

C) III

D) Both I and III

E) Both II and III

Diff: 1

Learning Objective: 3.10 Describe how Lewis acids and bases differ from Brønsted-Lowry acids and bases

118) For the following reaction, identify the Lewis acid and the Lewis base.

A) I = Lewis base; III = Lewis acid

B) I = Lewis acid; II = Lewis base

C) I = Lewis base; II = Lewis acid

D) I = Lewis acid; III = Lewis base

E) II = Lewis base; III = Lewis acid

Diff: 2

Learning Objective: 3.10 Describe how Lewis acids and bases differ from Brønsted-Lowry acids and bases

119) In a Brønsted-Lowry acid-base reaction, the conjugate acid is defined as ________.

A) a proton acceptor

B) a proton donor

C) the product resulting from loss of a proton

D) the product resulting from gaining a proton

E) the most reactive species

Diff: 1

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

120) For the following reaction, identify the Lewis acid and the Lewis base.

A) I = Lewis base; III = Lewis acid

B) I = Lewis acid; II = Lewis base

C) I = Lewis base; II = Lewis acid

D) I = Lewis acid; III = Lewis base

E) II = Lewis base; III = Lewis acid

Diff: 2

Learning Objective: 3.10 Describe how Lewis acids and bases differ from Brønsted-Lowry acids and bases

121) Identify the expected product for the following reaction.

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 3.10 Describe how Lewis acids and bases differ from Brønsted-Lowry acids and bases

122) Identify the expected product for the following reaction.

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 3.10 Describe how Lewis acids and bases differ from Brønsted-Lowry acids and bases

123) For the following reaction identify the acid and the base and predict the products.

A) I = acid; II = base; products = III, V, and VI

B) I = base; II = acid; products = III and IV

C) I = acid; II = base; products = IV and VII

D) I = base; II = acid; products = III, V, and VI

E) I = acid; II = base; products = IV, V, and VI

Diff: 3

Learning Objective: 3.10 Describe how Lewis acids and bases differ from Brønsted-Lowry acids and bases

124) For the following reaction identify the acid and the base and predict the position of the equilibrium.

A) I = acid; II = base; favor the right side

B) I = base; II = acid; favor the right side

C) I = acid; II = base; favor the left side

D) I = base; II = acid; favor the left side

E) I = acid; II = base; at equilibrium so equally favors both sides

Diff: 3

Learning Objective: 3.10 Describe how Lewis acids and bases differ from Brønsted-Lowry acids and bases

125) In a Brønsted-Lowry acid-base reaction, the conjugate base is defined as ________.

A) a proton acceptor

B) a proton donor

C) the product resulting from loss of a proton

D) the product resulting from gaining a proton

E) the most reactive species

Diff: 1

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

126) Identify the conjugate base of CH3CH2OH.

A) I

B) II

C) III

D) IV

E) V

Diff: 1

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

127) Identify the conjugate acid of CH3CH2NH2.

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 3.1 Define Brønsted-Lowry acid, Brønsted-Lowry base, conjugate acid, and conjugate base

128) Which of the following compounds is most acidic?

A) CH3OH

B) CH3Br

C) CH3Cl

D) CH3SH

E) CH3NH2

Diff: 2

Learning Objective: 3.4 Compare acidity and basicity of compounds based on structural (qualitative) analysis, including conjugate base stability and a comparison of the stability of negative charges (ARIO)

129) Which of the following compounds is least acidic?

A) I

B) II

C) III

D) IV

E) V

Diff: 1

Learning Objective: 3.4 Compare acidity and basicity of compounds based on structural (qualitative) analysis, including conjugate base stability and a comparison of the stability of negative charges (ARIO)

130) Which of the following compounds is most acidic?

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 3.4 Compare acidity and basicity of compounds based on structural (qualitative) analysis, including conjugate base stability and a comparison of the stability of negative charges (ARIO)

131) Which of the indicated protons is least acidic?

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 3.4 Compare acidity and basicity of compounds based on structural (qualitative) analysis, including conjugate base stability and a comparison of the stability of negative charges (ARIO)

132) What is an anion?

A) a negatively charged ion

B) a positively charged ion

C) a sodium atom

D) a hydrogen molecule

E) an atom that has lost electrons

Diff: 1

Learning Objective: 3.9 Explain what is meant by a counterion

133) Which of the following compounds is not a Lewis base?

A) H2O

B) NH3

C) NH2—

D) CH3CH3

E) CH3OCH3

Diff: 2

Learning Objective: 3.10 Describe how Lewis acids and bases differ from Brønsted-Lowry acids and bases

134) Which of the following compounds is not a Lewis Base?

A) NaOH

B) (CH3)3COK

C) CH3CH2CH2CH2Li

D) Ph3P

E) (CH3)3C+

Diff: 2

Learning Objective: 3.10 Describe how Lewis acids and bases differ from Brønsted-Lowry acids and bases

135) Identify the conjugate acid of CH3-NH-CH3.

A) I

B) II

C) III

D) IV

E) V

Diff: 1

Learning Objective: 3.5 Compare acidity and basicity of compounds based on structural (qualitative) analysis, focusing on the stability of positive charges (ARIO)

136) Which of the following best explains which compound is more basic?

CH3OH and CH3NH2

A) CH3OH is more basic due to oxygen being more electronegative than nitrogen

B) CH3NH2 is more basic due to nitrogen being less electronegative than oxygen

C) CH3OH is more basic as it results in a weaker conjugate acid

D) CH3NH2 is more basic as it results in a stronger conjugate acid

E) Both compounds are capable of hydrogen bonding and are of equal basicity

Diff: 1

Learning Objective: 3.5 Compare acidity and basicity of compounds based on structural (qualitative) analysis, focusing on the stability of positive charges (ARIO)

137) From the two compounds below identify which is more basic along with the best explanation.

A) I is more basic since it is only bound to one hydrogen atom

B) II is more basic due to the delocalized electrons on the nitrogen atom

C) I is more basic due to the localized electrons on the nitrogen atom

D) II is more basic due to inductive effects from the aromatic ring

E) Both compounds are capable of hydrogen bonding and are of equal basicity

Diff: 1

Learning Objective: 3.5 Compare acidity and basicity of compounds based on structural (qualitative) analysis, focusing on the stability of positive charges (ARIO)

138) From the two compounds below identify which would produce the more acidic conjugate acid along with the best explanation.

A) The conjugate acid of II is more acidic as it would have three hydrogen atoms attached.

B) The conjugate acid of I is more acidic due to protonation of the localized electrons on the nitrogen atom.

C) The conjugate acid of II is more acidic as the compound would no longer have delocalized electrons.

D) The conjugate acid of I is more acidic as compound II has resonance in the aromatic ring.

E) Once both compounds are protonated they can no longer hydrogen bond and thus are of equal acidity.

Diff: 1

Learning Objective: 3.5 Compare acidity and basicity of compounds based on structural (qualitative) analysis, focusing on the stability of positive charges (ARIO)

139) Which of the indicated protons is most acidic?

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 3.5 Compare acidity and basicity of compounds based on structural (qualitative) analysis, focusing on the stability of positive charges (ARIO)

140) Which of the indicated atoms would be most basic?

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 3.5 Compare acidity and basicity of compounds based on structural (qualitative) analysis, focusing on the stability of positive charges (ARIO)

141) Which of the indicated protons would be most acidic?

A) I

B) II

C) III

D) IV

E) V

Diff: 3

Learning Objective: 3.5 Compare acidity and basicity of compounds based on structural (qualitative) analysis, focusing on the stability of positive charges (ARIO)

142) For the following reaction identify the acid and the base and predict the position of the equilibrium.

I II

A) I = acid; II = base; favor the right side

B) I = base; II = acid; favor the right side

C) I = acid; II = base; favor the left side

D) I = base; II = acid; favor the left side

E) I = acid; II = base; at equilibrium so equally favors both sides

Diff: 3

Learning Objective: 3.5 Compare acidity and basicity of compounds based on structural (qualitative) analysis, focusing on the stability of positive charges (ARIO)

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