Chapter 3

MULTIPLE CHOICE QUESTIONS Part 3: Syror och baser
(Answers on page 18)
Topic: Acid-Base Definitions
1. According to the Lewis definition, a base is a(n):
A) Proton donor.
B) Electron pair donor.
C) Hydroxide ion donor.
D) Hydrogen ion donor.
E) Electron pair acceptor.
2. Which of the following is not both a Bronsted-Lowry acid and a Bronsted-Lowry base?
A) HSO4!
B) H2PO4!
C) HCO3!
D) OH!
E) SH!
3. Which of the following is not a conjugate acid - conjugate base pair (in that order)?
A) H3PO4, H2PO4!
B) HBF4, BF4!
C) CH3CH2OH, CH3CH2O!
D) H3O+, H2O
E) HPO4!, H2PO4!
4. The conjugate base of sulfuric acid is:
A) H3SO4+
B) SO3
C) HSO4!
D) H2SO3
E) HSO3!

A)
B)
C)
D)
E)

Topic: Acid-Base Definitions
6. Which of these is not a true statement?
A) All Lewis bases are also Bronsted-Lowry bases.
B) All Lewis acids contain hydrogen.
C) All Bronsted-Lowry acids contain hydrogen.
D) All Lewis acids are electron deficient.
E) According to the Bronsted-Lowry theory, water is both an acid and a base.
7. For the equilibrium
CH3NH3+ + H2O
CH3NH3+ + H3O+ the two substances which both are acids are:
A) H2O and H3O+
B) CH3NH3+ and H2O
C) CH3NH3+ and CH3NH2
D) CH3NH3+ and H3O+
E) CH3NH2 and H2O
8. Which of the following is not a Lewis base?
A) NH3
B) H!
C) BF3
D) H2O
E) H3C!
9. Which of the following is not a Bronsted-Lowry acid?
A) H2O
B) (CH3)3N
C) NH4+
D) CH3CO2H
E) HC"CH

5. Consider the equilibrium. Which are the Bronsted-Lowry bases?
PO43- + H2O

Chapter 3

HPO42- + HO-

PO43! and HPO42!
PO43! and OH!
PO43! and H2O
H2O and OH!
H2O and HPO42!
1

10. The reaction between which combination of substances below cannot be classified as a
Bronsted-Lowry acid-base reaction?
A) CH3Li + C2H5OH
B) H2SO4 + CH3CO2Na
C) BF3 + NH3
D) H3O+ + CH3NHE) two of the above
2

Chapter 3

Topic: Acid-Base Definitions
11.
A)
B)
C)
D)
E)

Chapter 3

Topic: Acid-Base Reactions

Which of these is not a Lewis acid?
AlCl3
H3O+
FeCl3
SO3
C4H10

16. Adding sodium hydride to ethanol would produce:
A) CH3CH2OCH2CH3 + H2
D) CH3CH2Na + NaOH
B) CH3CH2OCH2CH3 + NaOH
E) CH3CH3 + NaOH
C) CH3CH2ONa + H2
D)CH3CH2Na + NaOH
E) CH3CH3 + NaOH

12. This species is a carbon-based Lewis acid:
A) CH4
B) HCCl3
C) CH3+
D) :CH3!
E) ·CH3

17. Adding sodium amide (NaNH2) to 1-butyne (CH3CH2C CH) would produce:
A) CH3CH2C CNa + NH3
B) CH3CH2C C-C CH2CH3 + NaH + NH3
C) CH3CH2C CNH2 + NaH
D) NaCH2CH2C CH + NH3
E) CH3CH(Na)C CH + NH3

13. What is the conjugate base of ethanol?
A) CH3CH2O!
B) CH3CH2!
C) CH3CH2OH2+
D) CH3CH3
E) CH3OCH3

18. Which acid-base reaction would not take place as written?
A) CH3Li + CH3CH2OH ####$ CH4 + CH3CH2OLi
B) HC"CH + NaOH ####$ HC"CNa + H2O
C) HC"CNa + H2O ####$ HC"CH + NaOH
D) CH3OH + NaH ####$ CH3ONa + H2
E) CH3CO2H + CH3ONa ####$ CH3CO2Na + CH3OH

14. Which of the acids below would have the strongest conjugate base?
A) CH3CH2OH pKa = 18
B) CH3CO2H pKa = 4.75
C) ClCH2CO2H pKa = 2.81
D) Cl2CHCO2H pKa = 1.29
E) Cl3CCO2H pKa = 0.66
15. Which of the following is a Lewis acid?
A) H3O+
B) BF3
C) NF3
D) OH!
E) N"N

19. Which acid-base reaction would not take place as written?
A) CH3Li + CH3CH2CH2CH2NH2 ####$ CH4 + CH3CH2CH2CH2NHLi
B) CH3C"CH + NaOCH3 ####$ HC"CNa + CH3OH
C) HC"CNa + H2O ####$ HC"CH + NaOH
D) CH3OH + NaNH2 ####$ CH3ONa + NH3
E) CH3CO2H + CH3ONa ####$ CH3CO2Na + CH3OH
20. Which acid-base reaction would not take place as written?
A) CH3Li + CH3CH2OH ####$ CH4 + CH3CH2OLi
B) H2C=CH2 + NaOH ####$ H2C=CHNa + H2O
C) CH3C CNa + H2O ####$ CH3C CH + NaOH
D) (CH3)2CHOH + NaH ####$ (CH3)2CHONa + H2
E) CH3CO2H + CH3ONa ####$ CH3CO2Na + CH3OH

3

4

Chapter 3

Topic: Acid-Base Reactions

Chapter 3

Topic: Acid-Base Reactions

21. The amide ion, NH2 , is a base which can be used only in which of the solvents shown below: A) CH3OH
B) CH3CH2OH
C) H2O
D) D2O
E) Liquid NH3

26. Which reaction of these potential acids and bases does not occur to any appreciable degree due to an unfavorable equilibrium?
A) NaNH2 + CH3CH2CH2CH2CH2CH3
B) CH3CH2CO2Na + HI
C) CH3Li in hexane + ethyne
D) NaH + methanol
E) Two of the above will not occur

22. Acetic acid dissociates most completely in:
A) CCl4
B) Cl2C=CCl2
C) H2O
D) (CH3CH2)2O
E) the gas phase.

27. Which reaction of these potential acids and bases does not occur to any appreciable degree due to an unfavorable equilibrium?
A) NaNH2 + CH3CH2CH2CH2CH2OH
B) CH3CH2CO2H + NaCl
C) NaHCO3 + CH3CH2CO2H
D) NaH + CH3CH2CH2CH2CH2NH2
E) all of the above will occur due to a favorable equilibrium

!

23. Which pair of species are both bases in the following reaction?
HCN and H2O
H3O+ and CN!
A)
B)
C)
D)
E)

H2O and CN!
H3O+ and H2O
HCN and H3O+
HCN and CN!
H3O+ and CN!

28. Which combination of reagents is the least effective in generating sodium ethoxide,
CH3CH2ONa?
A) CH3CH2OH + NaH
B) CH3CH2OH + NaNH2
C) CH3CH2OH + NaOH
D) CH3CH2OH + CH3Li
E) CH3CH2OH + HC"CNa

24. What compounds are produced when sodium nitrate is added to a mixture of water and ethanol? A) HNO3 + NaOH
B) HNO3 + CH3CH2ONa
C) NaOH + CH3CH2ONa
D) CH3CH2OCH2CH3 + NaOH
E) No reaction occurs.

29. Which combination of reagents is effective in generating sodium ethoxide,
CH3CH2ONa?
A) CH3CH2OH + KH
B) CH3CH2OH + NaNH2
C) CH3CH2OH + Na
D) Two of the above
E) All of the above

25. Which reaction of these potential acids and bases does not occur to any appreciable degree due to an unfavorable equilibrium?
A) NaOH (aq) + CH3CH2CH2CO2H
B) CH3CH2ONa in ethanol + ethene
C) CH3Li in hexane + ethyne
D) NaNH2 in liq. NH3 + ethanol
E) NaC2H3O2 (aq) + HI

30. Which combination of reagents is effective in generating sodium propynide,
CH3C CNa?
A) CH3C CH + KH
B) CH3C CH + (CH3)2CHONa
C) CH3C CH + C2H5Li
D) Two of the above
E) All of the above

5

6

Chapter 3

Chapter 3

Topic: Acid-Base Reactions
+

Topic: Acid-Base Reactions, isotope labeling, Relative acid/base strength
+

31. In the reaction, Na NH2 + CH3OH ##$ CH3O Na + NH3, the stronger base is:
A) NaNH2
B) CH3OH
C) CH3ONa
D) NH3
E) This is not an acid-base reaction.

36. A product of the reaction, CH3CH2Li + D2O ####$ is
A) CH3CH2OD
B) CH3CH2CH2CH3
C) CH2=CH2
D) CH3CH2D
E) CH3CH2OCH2CH3

32. Which sequence is the best one to use to prepare CH3C"CD?
D2O
A) CH C CH NaH

37. The compounds ethane, ethene, and ethyne exhibit this order of increasing acidity:
A) Ethyne < ethene < ethane
B) Ethene < ethyne < ethane
C) Ethane < ethyne < ethene
D) Ethane < ethene < ethyne
E) Ethene < ethane < ethyne

!

!

3

B) CH C CH
3
C)

CH3C

CH

NaOH

D2O

CH3ONa

D2O

D) CH C CH DOH
3
E) None of these will be successful.
33. Adding sodium hydride, NaH, to water produces:
A) H2 and NaOH(aq)
B) H-(aq) + Na+(aq)
C) H3O+(aq) + Na+(aq)
D) H3O!(aq) + Na+(aq)
E) Na2O + H2
34. Adding methyllithium , CH3Li, to ethanol produces:
A) CH3CH2Li + CH3OH
B) CH3CH2OLi + CH4
C) CH3CH2OCH3 + LiH
D) All of the above
E) No reaction takes place
35. Which reaction will yield CH3CH2-D?
A) CH3CH3 + D2O
B) CH3CH2Li + D2O
C) CH3CH2OLi + D2O
D) CH3CH2OH + D2O
E) More than one of these

7

38. Which is an incorrect statement?
A) RSH compounds are stronger acids than ROH compounds.
B) PH3 is a weaker base than NH3.
C) NH2! is a stronger base than OH!.
D) OH! is a stronger base than OR!.
E) H! is a stronger base than OR!.
39. The correct sequence of the ions shown, in order of increasing basicity, is:
A) CH3CH2:! < CH2=CH:! < HC"C:!
B) CH3CH2:! < HC"C:! < CH2=CH:!
C) HC"C:! < CH3CH2:! < CH2=CH:!
D) CH2=CH:! < HC"C:! < CH3CH2:!
E) HC"C:! < CH2=CH:! < CH3CH2:!
Topic: Solvent effects
40. Which is a protic solvent?
A) CCl4
B) HCCl3
C) CH3OH
D) CH3(CH2)4CH3
E) CH3CH2OCH2CH3

8

Chapter 3

Chapter 3

Topic: Solvent effects
41
.

Topic: Relative acid/base strengths

Which might be used as protic solvent?
A)

O

D)
O

O

B)
C)

E)

O

H2N
O

45. The basic species are arranged in decreasing order of basicity in the sequence:
A) F! > OCH3! > NH2! > CH3CH2!
B) OCH3! > CH3CH2! > NH2! > F!
C) CH3CH2! > NH2! > OCH3! > F!
D) NH2! > CH3CH2! > F! > OCH3!
E) NH2! > OCH3! > CH3CH2! > F!
Topic: pKa calculations

N

42. Which of the following classes of substances cannot be used as protic solvents?
A) esters
B) aldehydes
C) ketones
D) carboxylic acids
E) two of the above
Topic: Acid constants
43. If a 0.01 M solution of a weak acid has a pH of 4.0, the pKa of the acid is:
A) 10.0
B) 8.0
C) 6.0
D) 4.0
E) 2.0
Topic: General
44. Which one of the following is a true statement?
A) The stronger the acid, the larger is its pKa.
B) The conjugate base of a strong acid is a strong base.
C) Acid-base reactions always favor the formation of the stronger acid and the stronger base. D) Strong acids can have negative pKa values.
E) Hydrogen need not be present in the molecular formula of a Bronsted-Lowry acid.

9

46. A particular acid has Ka = 2.0 x 10-5 (in aqueous solution). The evaluation of which of these expressions gives the value for pKa?
A) 10-14/2.0 x 10-5
B) 10-14(2.0 x 10-5)
C) 5 – log 2.0
D) -5 + log 2.0
E) 2.0 x 10-5/10-14
Topic: Solvent effects
47. As a consequence of the "leveling effect," the strongest acid which can exist in appreciable concentration in aqueous solution is:
A) H3O+
B) H2SO4
C) HClO4
D) HCl
E) HNO3
Topic: Relative acid/base strengths
48. Based on the position of the central atom in the periodic chart, we predict that the strongest acid of the following is:
A) H2O
B) H2S
C) H2Se
D) H2Te
Topic: Acid dissociation, thermodynamic calculations
49. An acid, HA, has the following thermodynamic values for its dissociation in water at
27º C: %H = -8.0 kJ mol-1; %S = -70 kJ K-1mol-1. The %G for the process is:
A) +29 kJ mol-1
B) +13 kJ mol-1
C) -6.1 kJ mol-1
D) -13 kJ mol-1
E) -29 kJ mol-1

10

Chapter 3

Topic: Relative acid/base strengths, solvent effects
50. Which of these bases is the strongest one which can be used (and retains its basic character) in aqueous solution?
A) OCH3!
B) F!
C) OH!
D) C2H3O2!
E) HSO4!

Topic: Acidity constant- thermodynamic principles
51. The acidity constant, Ka, differs from the equilibrium constant, Keq, for the dissociation of the same acid in water at the same temperature and concentration in what way?
A) Ka can be determined experimentally with less accuracy than Keq.
B) The two terms are identical numerically.
C) Ka is used for strong acids only; Keq for weak acids.
D) Ka is the reciprocal of Keq.
E) Keq = Ka/[H2O].
Topic: Acids/bases-general principles
52. Which of the following is an untrue statement?
A) The % dissociation of a weak acid increases with increasing dilution of the acid solution. B) The stronger an acid, the weaker its conjugate base.
C) The larger the value of Ka for an acid, the smaller the value of its pKa.
D) Comparison of the acidity of strong acids in solution requires the use of a solvent less basic than water.
E) The stronger the acid, the more positive the value of %Gº for the dissociation.
Topic: Acid-base reactions
53. When proton transfer reactions reach equilibrium, there have been formed:
A) the weaker acid and the weaker base.
B) the weaker acid and the stronger base.
C) the stronger acid and the weaker base.
D) the stronger acid and the stronger base.
E) All proton transfers go to completion; they are not equilibrium processes.
Topic: Relative acid-base strengths
54. For the simple hydrides, MHn, pKa values decrease in the order:
A) CH4 > NH3 > H2O > H2S > HBr
B) HBr > H2S > H2O > NH3 > CH4
C) HBr > H2O > NH3 > H2S > CH4
D) NH3 > H2S > CH4 > H2O > HBr
E) H2S > H2O > HBr > NH3 > CH4

11

Chapter 3

Topic: Relative acid-base strengths, solvent effects
55. The compound aniline, C6H5NH2, has weakly basic properties in aqueous solution. In this other solvent, aniline would behave as a strong base.
A) CH3OH
B) CH3CH2OH
C) CF3CO2H
D) Liquid NH3
E) CH3(CH2)4CH3
56. Which of the following organic compounds is the strongest acid?
A) C6H12 pKa = 52
B) CH3CH3 pKa = 50
C) CH3CH2OH pKa = 18
D) CH3CO2H pKa = 5
E) CF3CO2H pKa = 0
57. Which is the strongest acid?
A) CH3CH2OH
B) CH3CO2H
C) HC"CH
D) CH2=CH2
E) CH3CH3
58.
A)
B)
C)
D)
E)

Which is the strongest acid?
CH2ClCH2CH2CH2CH2CO2H
CH3CHBrCH2CH2CH2CO2H
CH3CH2CH2CBr2CH2CO2H
CH3CH2CH2CHFCH2CO2H
CH3CH2CH2CF2CH2CO2H

59.
A)
B)
C)
D)
E)

Which is the strongest acid?
CH3CH2CH2CH2CHFCO2H
CH3CHBrCH2CH2CH2CO2H
CH3CH2CH2CHClCH2CO2H
CH3CH2CH2CHFCH2CO2H
CH3CH2CH2CHICH2CO2H

12

Chapter 3

Topic: Relative acid-base strengths

Chapter 3

Topic: Relative acid-base strengths

60.
A)
B)
C)
D)
E)

Which is the weakest acid?
CH3CH2CH2CH2CHFCO2H
CH3CHCH2CH2CH2CH2OH
CH3CH2CH2CH2CH2SO3H
CH3CH2CH2CH2CH=CH2
CH3CH2CH2CH2NH2

64. Select the strongest base.
A) OH!
B) RC"C!
C) NH2!
D) CH2=CH!
E) CH3CH2!

61.
A)
B)
C)
D)
E)

Which of the following substances has a hydrogen atom with pKa !25?
CH3CH2CH2CH2CO2H
CH3CHCH2C CCH3
CH3CH2CH2C CH
CH3CH2CH2CH2CH=CH2
CH3CH2CH2CH2NH2

65. A group of acids arranged in order of decreasing acidity is:
HNO3 > CH3COOH > C6H5OH > H2O > HC"CH
What is the arrangement of the conjugate bases of these compounds in decreasing order of basicity?
A) NO3! > CH3COO! > C6H5O! > OH! > HC"C!
B) CH3COO! > C6H5O! > NO3! > OH! > HC"C!
C) C6H5O! > NO3! > HC"C! > OH! > CH3COO!
D) HC"C! > OH! > C6H5O! > CH3COO! > NO3!
E) No prediction of relative base strength is possible.

62. Hydrogen atom(s) from which position(s) is (are) most likely to be abstracted when the following substance is treated with NaH?
10

8

9
1

6
7

A)
B)
C)
D)
E)

4
5

2
3

1
1, 5, 6
1, 2
3, 4, 7, 8, 9, 10
Hydrogens from all of the positions are equally likely to be abstracted by NaH.

63. Which of the following correctly lists the compounds in order of decreasing acidity?
A) H2O > HC"CH > NH3 > CH3CH3
B) HC"CH > H2O > NH3 > CH3CH3
C) CH3CH3 > HC"CH > NH3 > H2O
D) CH3CH3 > HC"CH > H2O > NH3
E) H2O > NH3 > HC"CH > CH3CH3

13

66. What prediction can be made of the relative strengths of the conjugate bases of: H2S,
HCl, SiH4, PH3?
A) PH2! > SiH3! > HS! > Cl!
B) SiH3! > PH2! > HS! > Cl!
C) Cl! > HS! > PH2! > SiH3!
D) HS! > Cl! > SiH3! > PH2!
E) Cl! > PH2! > SiH3! > HS!
Topic: Acids/bases- general
67. Which of these species is not amphoteric?
A) HC"C!
B) HS!
C) NH3
D) CH3!
E) HPO4!

14

Chapter 3

Topic: Acids/bases- general

SHORT-ANSWER QUESTIONS WITH ANSWERS ON PAGES 19-20:

68. Which of these phosphorus-based acids is dibasic?
O
A)
HO

P

HO

P

73. The four basic types of reactions are: ________________.
OH

74. The process of bond-breaking where each fragment takes away one of the electrons from the bond is called ____________.

H

O

C)
H

P

H

75. Heterolytic bond-breaking produces __________.

OH
O

D)
HO

P

O
O

OH
O O

E)
HO

72. Addition reactions are characteristic of compounds with ______________.

OH

OH
O

B)

Chapter 3

P

P

P

OH

76. According to Bronsted-Lowry theory, an acid is a substance that can ____________.

OH

77. According to Lewis theory, a base is a substance that can _________.

OH

OH OH

78. The molecule or ion that is formed when an acid loses its proton is called the
______________.

69. Why cannot one determine the relative acid strengths of HClO4 and HNO3 using aqueous solutions of these acids?
A) The acids are insufficiently soluble for the measurements.
B) A more basic solvent than H2O must be used.
C) H2O is too basic a solvent for the distinction to be made.
D) These oxidizing acids cause redox reactions to occur.
E) Actually, the acid strengths can be determined using aqueous solutions.

79. Reagents that seek to react with a proton or some other electron-deficient center are called ____________.
80. A substance that can donate a lone pair of electrons is a ____________ according to
____________ theory.
81. When drawing mechanisms, chemists generally use curved arrows. The curved arrow begins with ______________ and points toward ______________.

70. Which of these is not a diprotic acid?
A) H2S
B) H2SO4
C) H2O
D) (COOH)2
E) H2PO4-

82. Why do water-insoluble carboxylic acids dissolve in aqueous sodium hydroxide?
83. Bond polarization that takes place through space and through the bonds of the molecule is called the _____________.
84. What are the two fundamental types of energy?

15

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Chapter 3

Chapter 3

ANSWERS MULTOPLE CHOICE QUESTIONS Chapt.3
85. Define a protic solvent.

Svar - Part 3: Syror och baser
86. Briefly, but clearly, explain why the –OH hydrogen in acetic acid (CH3CO2H) is more acidic than in ethanol (C2H5OH).

87. Isotope labeling is an important tool in the study of reaction mechanisms. How will you selectively deuterate the specified hydrogen atom, indicated by an arrow, in the following compound? Use equations to clarify your answer and briefly explain your rationale. H

Topic: Acid-base reactions
88. Write an equation to show the reaction between ethanol, C2H5OH and methyllithium,
CH3Li. Draw all non-bonding electrons and show electron flow with curved arrows.

Topic: Acid-base reactions, solvent selection
89. You are planning to carry out a reaction between propyne, CH3C CH and sodium amide, NaNH2. You also need to choose an appropriate solvent for carrying out the reaction. Would ethanol be suitable for this purpose? Explain your rationale clearly.

90. You are planning to purify an impure sample of benzoic acid, known to be contaminated with naphthalene. Propose a strategy for purifying this sample, making use of acid-base principles, using equations to further clarify your answer.

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Rätt/Fel

Chapter 3

Chapter 3

SHORT-ANSWER QUESTIONS ANSWERS:
87.

72.

Ans: multiple bonds

73.

Ans: substitution, addition, elimination, rearrangement

74.

Ans: The specified hydrogen is attached to an sp-hybridized carbon and is thus more acidic than all the other hydrogens in the molecule. By using an appropriate strong base, such as NaH or NaNH2, the acetylenic hydrogen is selectively removed; adding D2O then replaces the lost hydrogen atom with a deuterium atom.

Ans: homolysis

75.

H

Ans: charged fragments/ions

ii) D2O

76.

Ans: donate a proton

77.

Ans: donate a lone pair of electrons

78.

Ans: conjugate base

79.

Ans: nucleophiles

80.

Ans: base; Lewis

81.

Ans: a lone pair or covalent bond; a site of electron deficiency

82

Ans: Because they are converted to water-soluble salts.

83

Ans: inductive effect

84.

Ans: potential energy and kinetic energy

85.

Ans: one that has a hydrogen atom attached to a strongly electronegative element such as oxygen 86.

Ans: The greater acidity of the –OH hydrogen in acetic acid is due primarily to two factors: resonance and inductive effects. In acetic acid, the presence of the neighboring carbonyl group has an electron-withdrawing inductive effect on the –OH hydrogen, increasing its acidity relative to ethanol, in which there is no carbonyl group. Also, comparison of the respective conjugate bases shows that, unlike the ethoxide ion, the acetate ion is stabilized by resonance. This too, is reflected in the greater acid strength of the corresponding acid species.
O
O

H

88.

H

Ans:
.. H
+
O
..

..
+
O : Li
..

: CH3 Li+

+

CH4

89.

(- H+)

O

(- H+)

Ans: No, ethanol would be unsuitable for carrying out the reaction between propyne and methyllithium. The pKa of ethanol is ~16, and sodium amide is strong enough a base to readily abstract a proton from the solvent ( pKa of NH3 is ~38); in doing so, it becomes deactivated and is no longer available to react with propyne (pKa ~25). Typically, the selected solvent should be chemically inert toward all substances used in the reaction, so that it does not interfere with the desired reaction.

90.

Ans: Benzoic acid reacts with aqueous NaOH to form a water soluble salt, while naphthalene, which is not soluble in water to any appreciable extent, does not react with
NaOH. So, upon shaking the impure sample with NaOH (aq), the naphthalene remains as a solid, while the benzoic acid dissolves in the aqueous medium as sodium benzoate.
After filtration, HCl is added to the filtrate to regenerate benzoic acid, which precipitates as almost pure crystals. Cooling maximizes the yield of the purified product, after which pure crystals can be obtained by filtration.
Alternatively, before beginning the reaction with aqueous NaOH, the impure sample is first dissolved in diethyl ether (benzoic acid and naphthalene are both soluble in ether) and placed in a separatory funnel. After shaking thoroughly with aqueous NaOH, the aqueous layer (which now contains sodium benzoate) is collected. The rest of the procedure is as described earlier.
O

O
OH

NaOH

O
ONa

HCl

OH

O
O

Inductive effect: electron withdrawing

O

D

i) NaH or NaNH2

O

water insoluble
O

resonance stabilized anion

OH

water soluble
NaOH
X

No reaction

water insoluble
O

19

20

water insoluble
PURE