Solution Manual For Essential Biochemistry, 4th Edition

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1
Solutions
Chapter 1
1. a. carboxylic acid; b. amine; c. ester; d. alcohol.
2. a. ether; b. phosphoric acid ester; c. thiol; d. ketone.
3. Hydroxyl group
Imino group
Ether linkage
CH3
O
N
OH
[From Li, S.-Y., Wang, X.-B., and Kong, L.-Y. Eur. J. Med. Chem.
71, 36–45 (2014).]
4.
Hydroxyl
Coenzyme Q
Ether
Nicotinic acid (niacin)
N
O
C
OH
H 3 C
O
O
CH3
H 3 C
O
O
C
H2
Vitamin C
Carboxyl
C
OH
CH
CH
HO
OHHO
Carbonyl
Carbonyl
Ester
O
C
O
C
H(CH2 CH C CH 2)10
CH 3
5. Amino acids, monosaccharides, nucleotides, and lipids are the
four types of biological small molecules. Amino acids, monosacchar-
ides, and nucleotides can form polymers of proteins, polysaccharides,
and nucleic acids, respectively.
6. a. N-acetylglucosamine is a monosaccharide. b. CMP is a nucle-
otide. c. Homocysteine is an amino acid. d. Cholesteryl ester is a lipid.
7. a. C and H plus some O; b. C, H, and O; c. C, H, O, and N plus
small amounts of S.
8. It is a lipid (it is actually lecithin). It is mostly C and H, with
relatively little O and only one N and one P. It has too little O to be
a carbohydrate, too little N to be a protein, and too little P to be a
nucleic acid.
9. You should measure the nitrogen content, since this would indi-
cate the presence of protein (neither lipids nor carbohydrates contain
appreciable amounts of nitrogen).
10. You could add the compound that contains the most nitrogen,
compound B, which is melamine. [Melamine is a substance that in
the past was added to some pet foods and milk products from China
so that they would appear to contain more protein. Melamine is toxic
to pets and children.] Compound C is an amino acid, so it would
already be present in protein-containing food.
11. A diet high in protein results in a high urea concentration, since
urea is the body’s method of ridding itself of extra nitrogen. Nitrogen
is found in proteins but is not found in significant amounts in lipids
or carbohydrates. A low-protein diet provides the patient with just
enough protein for tissue repair and growth. In the absence of excess
protein consumption, urea production decreases, and this puts less
strain on the patient’s weakened kidneys.
12. Asn has an amido group and Cys has a sulfhydryl group.
13.
H
H OH
H OH
H
OHCH 2
OH
HO
HC
O
Hydroxyl
Carbonyl
14. a. Fructose has the same molecular formula, C6H12O6, as glucose.
b. Fructose is a ketone, whereas glucose is an aldehyde.
15. Uracil has a carbonyl functional group, whereas cytosine has an
amino functional group.
16. Nucleotides consist of a five-carbon sugar, a nitrogenous ring,
and one or more phosphoryl groups linked covalently together.
17. As described in the text, palmitate and cholesterol are highly
nonpolar and are therefore insoluble in water. Both are highly aliphatic.
Alanine is water soluble because its amino group and carboxylate
group are ionized, which render the molecule “saltlike.” Glucose is
also water soluble because its aldehyde group and many hydroxyl
groups are able to form hydrogen bonds with water.
18. Glucose has several hydroxyl groups and is a polar molecule.
As such, it will have difficulty crossing the nonpolar membrane.
The 2,4-dinitrophenol molecule consists of a substituted benzene
ring and has greater nonpolar character. Of the two molecules, the
2,4-dinitrophenol will traverse the membrane more easily.
19. DNA forms a more regular structure because DNA consists of only
four different nucleotides, whereas proteins are made up of as many as
20 different amino acids. In addition, the 20 amino acids have much
more individual variation in their structures than do the four nucleotides.
Both of these factors result in a more regular structure for DNA. The cel-
lular role of DNA relies on the sequence of the nucleotides that make up
the DNA, not on the overall shape of the DNA molecule itself. On the
other hand, proteins fold into unique shapes, as illustrated by endothelin
in Figure 1.4. The ability of proteins to fold into a wide variety of shapes
means that proteins can also serve a wide variety of biochemical roles
in the cell. According to Table 1.2, the major roles of proteins in the cell
are to carry out metabolic reactions and to support cellular structures.
20. Polysaccharides serve as fuel-storage molecules and can also
serve as structural support for the cell.
21. Pancreatic amylase is unable to digest the glycosidic bonds that
link the glucose residues in cellulose. Figure 1.6 shows the structural
differences between starch and cellulose. Pancreatic amylase binds to
starch prior to catalyzing the hydrolysis of the glycosidic bond; thus
the enzyme and the starch must have shapes that are complementary.
The enzyme would be unable to bind to the cellulose, whose structure
is much different from that of starch.
22. Cellulose cannot be digested by mammals and therefore the energy
yield is 0 kilocalories per gram. Although both starch and glycogen

2 Solutions
are polymers of glucose, the glucose residues are linked differently in
the two molecules, and pancreatic amylase is unable to hydrolyze the
glycosidic bonds in cellulose (see Solution 21). Cellulose provides no
energy to the diet but is an important component of the diet as fiber.
23. A positive entropy change indicates that the system has become
more disordered; a negative entropy change indicates that the system has
become more ordered. a. negative; b. positive; c. positive; d. positive;
e. negative.
24. a. decrease; b. increase.
25. The polymeric molecule is more ordered and thus has less entropy.
A mixture of constituent monomers has a large number of different
arrangements (like the balls scattered on a pool table) and thus has
greater entropy.
26. Entropy increases as the reactants (7 molecules) are converted to
products (12 molecules).
27. The dissolution of ammonium nitrate in water is a highly endo-
thermic process, as indicated by the positive value of ΔH. This means
that when ammonium nitrate dissolves in water, the system absorbs
heat from the surroundings and the surroundings become cold. The
plastic bag containing the ammonium nitrate becomes cold and can
be used as a cold pack to treat an injury.
28. The dissolution of calcium chloride in water is a highly exo-
thermic process, as indicated by the negative value of ΔH. This
means that when calcium chloride dissolves in water, the system loses
heat to the surroundings and the surroundings become warm. The
plastic bag holding the calcium chloride solution becomes warm and
can be used as a hot pack by the camper at cold temperatures.
29. The dissolution of urea in water is an endothermic process and
has a positive ΔH value. In order for the process to be spontaneous,
the process must also have a positive ΔS value in order for the free
energy change of the process to be negative. Solutions have a higher
degree of entropy than the solvent and solute alone.
30. First, calculate ΔH and ΔS, as described in Sample Calculation 1.1:
ΔH = HB – HA
ΔH = 60 kJ · mol –1 – 54 kJ · mol–1
ΔH = 6 kJ · mol –1
ΔS = SB – SA
ΔS = 43 J · K–1 · mol–1 – 22 J · K–1 · mol–1
ΔS = 21 J · K–1 · mol–1
a. ΔG = (6000 J · mol–1
) – (4 + 273 K)(21 J · K–1 · mol–1
)
ΔG = 180 J · mol–1
The reaction is not favorable at 4°C.
b. ΔG = (6000 J · mol–1
) – (37 + 273 K)(21 J · K–1 · mol–1
)
ΔG = –510 J · mol–1
The reaction is favorable at 37°C.
31. 0 > 15,000 J · mol –1 – (T )(51 J · K–1 · mol –1 )
–15,000 > –(T )(51 K–1
)
15,000 < (T )(51 K–1
)
294 K < T
The reaction is favorable at temperatures of 21°C and higher.
32. Process a is always spontaneous; processes b and c are likely to
be spontaneous, depending on the temperature, and process d is never
spontaneous.
33. 0 > –14.3 kJ · mol–1 – (273 + 25 K)(ΔS)
14.3 kJ · mol–1 > – (273 + 25 K)(ΔS)
–48 J · K–1 · mol –1 > ΔS
ΔS could be any positive value, or it could have a negative value
smaller than – 48 J · K–1 · mol–1
.
34. –63 kJ · mol–1 = ΔH – (273 + 25 K)(190 J · K–1 · mol –1
)
ΔH = –63 kJ · mol–1 + 56.6 kJ · mol–1
ΔH = –6.4 kJ · mol–1
The reaction releases heat to the surroundings.
35. a. Entropy decreases when the antibody–protein complex binds
because the value of ΔS is negative.
b. ΔG = ΔH – TΔS
ΔG = –87,900 J · mol–1 – (298 K)(–118 J · K–1 · mol–1
)
ΔG = –52.7 kJ · mol–1
The negative value of ΔG indicates that the complex forms spon-
taneously.
c. The second antibody binds to cytochrome c more readily than
the first because the change in free energy of binding is a more
negative value. [From Raman, C. S., Allen, M. J., and Nall, B. T.
Biochemistry 34, 5831–5838 (1995).]
36. a. The reaction releases heat to the surroundings because the
value of ΔH is negative.
b. ΔG = ΔH – TΔS
–17,200 J · mol–1 = –9500 J · mol–1 – (310 K)(ΔS)
ΔS = 25 J · K–1 · mol–1
The positive value of ΔS indicates that the reaction proceeds with
an increase in entropy.
c. The ΔH term makes a greater contribution to the ΔG value.
This indicates that the reaction is spontaneous largely because the
reaction is exothermic.
37. a. The conversion of glucose to glucose-6-phosphate is not
favorable because the ΔG value for the reaction is positive, indi-
cating an endergonic process.
b. If the two reactions are coupled, the overall reaction is the sum
of the two individual reactions. The ΔG value is the sum of the
ΔG values for the two individual reactions.
ATP + glucose → ADP + glucose-6-phosphate
ΔG = –16.7 kJ · mol–1
Coupling the conversion of glucose to glucose-6-phosphate with
the hydrolysis of ATP converts an unfavorable reaction to a favor-
able reaction. The ΔG value of the coupled reaction is negative,
which indicates that the reaction as written is favorable.
38. a. The reaction is not favorable because the ΔG value for the
reaction is positive, indicating an endergonic process.
b.
GAP + Pi + NAD+ → 1,3BPG + NADH ΔG = +6.7 kJ · mol–1
1,3BPG + ADP → 3PG + ATP ΔG = –18.8 kJ · mol–1
GAP + Pi + NAD+ + ADP → 3PG + NADH + ATP ΔG = –12.1 kJ · mol–1
The coupled reaction is spontaneous because the ΔG value is
negative.
39. C (most oxidized), A, B (most reduced)
40. a. reduction; b. oxidation.
41. a. oxidized; b. oxidized; c. oxidized; d. reduced.
42. a. oxidizing agent; b. oxidizing agent; c. oxidizing agent;
d. reducing agent.
43. a. Palmitate’s carbon atoms, which have the formula —CH2—,
are more reduced than CO2 , so their reoxidation to CO2 releases
free energy.

Solutions 3
b. Because the —CH2— groups of palmitate are more reduced
than those of glucose (—HCOH—), their conversion to the fully
oxidized CO2 would be even more thermodynamically favorable
(have a larger negative value of ΔG) than the conversion of glu-
cose carbons to CO2. Therefore, palmitate carbons provide more
free energy than glucose carbons.
44. The complete oxidation of stearate to CO2 yields more energy
because 17 of the 18 carbons of stearate are fully reduced. The con-
version of these carbons to CO 2 provides more free energy than some
of the carbons of α-linolenate, which participate in double bonds and
are therefore already partially oxidized.
45. Morphological differences, which are useful for classifying large
organisms, are not useful for bacteria, which often look alike. Further-
more, microscopic organisms do not leave an easily interpreted imprint
in the fossil record, as vertebrates do. Thus, molecular information is
often the only means for tracing the evolutionary history of bacteria.
46. It is difficult to envision how a single engulfment event could have
given rise to a stable and heritable association of the eukaryotic host
and the bacterial dependent within a single generation. It is much more
likely that natural selection gradually promoted the interdependence
of the cells. Over many generations, genetic information supporting
the association would have become widespread.
47. A B C
48. a. H15 and H7 are closely related, as are H4 and H14.
b. H4 and H14 are most closely related to H3.
Chapter 2
1. The water molecule is not perfectly tetrahedral because the elec-
trons in the nonbonding orbitals repel the electrons in the bonding
orbitals more than the bonding electrons repel each other. The angle
between the bonding orbitals is therefore slightly less than 109°.
2. Because the partial negative charges are arranged symmetrically
(and the shape of the molecule is linear), the molecule as a whole is
not polar.
O C O

3. Water has the higher boiling point because, although each mol-
ecule has the same geometry and can form hydrogen bonds with its
neighbors, the hydrogen bonds formed between water molecules are
stronger than those formed between H 2 S molecules. The electroneg-
ativity difference between H and O is greater than that between H and
S and results in greater differences in the partial charges on the atoms
in the water molecule.
4. Water has the highest melting point because each water molecule
forms hydrogen bonds with four neighboring water molecules, and hy-
drogen bonds are among the strongest intermolecular forces. Ammonia
is also capable of forming hydrogen bonds, but they are not as strong
(due to the smaller electronegativity difference between hydrogen
and nitrogen). Methane cannot form hydrogen bonds; the molecules
are attracted to their neighbors only via weak London dispersion forces.
5. The arrows point toward hydrogen acceptors and away from
hydrogen donors:
O
C N
N
N N
N
H
H
H
H
H
O
O
S
O
O
O
O
O
CH3 N
H2 N
CH CH
COO
CH 2
NH 2
CH 2
CH 3
Aspartame
Uric acid
Sulfanilamide
6. Arrows point toward hydrogen acceptors and away from hydrogen
donors. [From Kubiny, H., in 3D QSAR in Drug Design: Volume 1:
Theory Methods and Application, Springer Science & Business
Media (1993).]
MTX DHF
N
N N
N
N
H
H
N RH
O
H
H
N
H
H
H
N
H H N
N
N
N
N
RH 3C
7. Identical hydrogen bonding patterns in the two molecules are
shown as open arrows in Solution 6.
8. [From Puschner, P., Poppenga, R. H., Lowenstine, L. J., Filigenzi,
M. S., and Pesavento, P. A. J. Vet. Diagn. Invest. 19, 616–624 (2007).]
N N
N N
N
N
H
O
H
HH
H H
Melamine cyanurate
H
ON
HN NH
O
9. a. H < C < S < N < O < F
b. The greater an atom’s electronegativity, the more polar its bond
with H and the greater its ability to act as a hydrogen bond acceptor.
Thus, N, O, and F, which have relatively high electronegativities, can
act as hydrogen bond acceptors, whereas C and S, whose electroneg-
ativities are only slightly greater than hydrogen’s, cannot.
10. Compound A does not form hydrogen bonds (the molecule has a
hydrogen bond acceptor but no hydrogen bond donor). Compounds
B and C form hydrogen bonds as shown because each molecule con-
tains at least one hydrogen bond donor and a hydrogen bond acceptor.
The molecules in D do not form hydrogen bonds with each other be-
cause ethyl chloride lacks both a hydrogen bond donor and a hydro-
gen bond acceptor. The molecules in E do because ammonia has a
hydrogen bond donor and diethyl ether has a hydrogen bond acceptor:

4 Solutions
18. Methanol, which has the highest dielectric constant, would be
the best solvent for the cationic NH 4
+
. The polarity of the alcohols,
which all contain a primary OH group, varies with the size of the
hydrocarbon portion. 1-Butanol, with the largest hydrophobic group,
is the least polar and therefore has the lowest dielectric constant.
19. Structure A depicts a polar compound, while structure B depicts
an ionic compound similar to a salt like sodium chloride. This is more
consistent with glycine’s physical properties as a white crystalline
solid with a high melting point. While structure A could be water sol-
uble because of its ability to form hydrogen bonds, the high solubility
of glycine in water is more consistent with an ionic compound whose
positively and negatively charged groups are hydrated in aqueous
solution by water molecules.
20. a. Surface tension is defined as the force that must be applied
to surface molecules in a liquid so that they may experience the
same forces as the molecules in the interior of the liquid. Water’s
surface tension is greater than ethanol’s because the strength and
number of water’s intermolecular forces (hydrogen bonds) are
both greater. Ethanol’s OH group also forms hydrogen bonds,
but the hydrocarbon portion of the molecule cannot interact
favorably with water, and weaker London dispersion forces form
instead.
b. The kinetic energy of the water molecules increases when tem-
perature increases. Intermolecular forces are weaker in strength as
a consequence of the increased molecular motion. Because sur-
face tension increases when the strength of intermolecular forces
increases as described in part (a), surface tension decreases when
temperature increases.
21. The waxed car is a hydrophobic surface. To minimize its inter-
action with the hydrophobic molecules (wax), each water drop mini-
mizes its surface area by becoming a sphere (the geometrical shape
with the lowest possible ratio of surface to volume). Water does not bead
on glass, because the glass presents a hydrophilic surface with which the
water molecules can interact. This allows the water to spread out.
22. The paper clip, although composed of a metal with a greater
density than water, fl oats due to the strong hydrogen bonding that
occurs among water molecules on the surface of the liquid. Soap dis-
rupts these strong intermolecular forces and as a result the paper clip
sinks to the bottom of the container.
23. Polar and nonpolar regions of the detergents are indicated.
Hexadecyltrimethylammonium
HO
OH
O
O
nonpolar
polar
OH
Cholate
CH3
CH 3
CH 3
(H2C) 15
polar
nonpolar
H 3C
CH 3
CH 3
CH3
N

24. Polar and nonpolar regions of the detergents are indicated.
Dimethyldecylphosphine oxide
O
OH
H
H
H
H
O
OH
OH
CH2 OH
(CH2 )7 CH3
n-Octylglucoside
Nonpolar
(CH2)9H3 C P
O
CH3
CH3
Nonpolar
Polar
Polar
25. Compounds A and D are amphiphilic, compound B is nonpolar,
and compounds C and E are polar.
26. Compound A has a polar head and a nonpolar tail as indicated
and can form a micelle (see Fig. 2.9). Compound D has a polar head
B
C
E
N
N
CH 2 OH3 C
H
N
H
H
H
CH2 OH 3C H
N
N
H
H
CH3O CH2
CH3
H2 C
11. a. van der Waals forces (dipole–dipole interactions); b. hydrogen
bonding; c. van der Waals forces (London dispersion forces); d. ionic
interactions.
12. a. hydrogen bonding; b. ionic interactions; c. van der Waals
forces (London dispersion forces).
13. Solubility in water decreases as the number of carbons in the
alcohol increases. The hydroxyl group of the alcohol is able to form
hydrogen bonds with water, but water cannot interact favorably with
the hydrocarbon chain. Increasing the length of the chain increases
the number of potentially unfavorable interactions of the alcohol with
water and solubility decreases as a result.
14. Solubility in water and dielectric constants are correlated; low
molecular weight alcohols are miscible with water and have a high
dielectric constant; high molecular weight alcohols are not very sol-
uble in water and have a low dielectric constant.
15. Aquatic organisms that live in the pond are able to survive the
winter. Since the water at the bottom of the pond remains in the liquid
form instead of freezing, the organisms are able to move around. The
ice on top of the pond also serves as an insulating layer from the cold
winter air.
16. Water is unique in that its liquid form is more dense than its solid
form. The weight of the skater puts pressure on the thin blade of the
ice skate. The ice melts under the blade because of this increased
pressure. A higher pressure favors the liquid form of water over the
solid form because the liquid form is more dense and takes up less
volume.
17. The positively charged ammonium ion is surrounded by a shell of
water molecules that are oriented so that the partially negatively
charged oxygen atoms interact with the positive charge on the am-
monium ion. Similarly, the negatively charged sulfate ion is hydrated
with water molecules oriented so that the partially positively charged
hydrogen atoms interact with the negative charge on the sulfate anion.
(Not shown in the diagram is the fact that the ammonium ions out-
number the sulfate ions by a 2:1 ratio. Also note that the exact number
of water molecules shown is unimportant.)
O
O
O
O
NH4
SO 4
2
H
H H
O
H
H
O
H
H
H
O
H
H
O
H
H
H
H
H
H
O HH O HH

Solutions 5
c. The hydrophobic grease moves into the hydrophobic core of the
water-soluble soap micelle. The “dissolved” grease can then be
washed away with the micelle.
29. a. The nonpolar core of the lipid bilayer helps prevent the passage
of water since the polar water molecules cannot easily penetrate the
hydrophobic core of the bilayer. b. Most human cells are surrounded
by a fluid containing about 150 mM Na + and slightly less Cl – (see
Fig. 2.12). A solution containing 150 mM NaCl mimics the extracel-
lular fluid and therefore helps maintain the isolated cells in near-
normal conditions. If the cells were placed in pure water, water
would tend to enter the cells by osmosis; this might cause the cells to
burst.
30. In reverse osmosis, water moves from an area of low concen-
tration (high solute concentration) to an area of high concentration
(low solute concentration). This movement is opposite that described
for osmosis in Problem 29. This is a non-spontaneous process that
requires an input of energy in order to proceed, unlike osmosis, which
occurs spontaneously without input of energy.
31. a. CO2 is nonpolar and would be able to cross a bilayer. b. Glu-
cose is polar and would not be able to pass through a bilayer because
the presence of the hydroxyl groups means glucose is highly hydrated
and would not be able to pass through the nonpolar tails of the mol-
ecules forming the bilayer. c. DNP is nonpolar and would be able
to cross a bilayer. d. Calcium ions are charged and are, like glucose,
highly hydrated and would not be able to cross a lipid bilayer.
32. Vesicles consist of a lipid bilayer that closes up to enclose an
aqueous compartment. The polar drug readily dissolves in this
aqueous compartment. Delivery to the cell is accomplished when the
vesicle membrane fuses with the cell membrane, releasing the drug
into the cytosol.
33. Substances present at high concentration move to an area of low
concentration spontaneously, or “down” a concentration gradient in
a process that increases their entropy. The export of Na + ions from
the cell requires that the sodium ions be transported from an area
of low concentration to an area of high concentration. The same is
true for potassium transport. Thus, these processes are not sponta-
neous, and an input of cellular energy is required to accomplish the
transport.
34. The amount of Na+ (atomic weight 23 g · mol–1
) lost in 15 minutes,
assuming a fluid loss rate of 2 L per hour and a sweat Na+ concentration
of 50 mM (Box 2.B), is
0.25 h × 2 L
h × 0.05 mol
L × 23 g
mol × 1000 mg Na +
g Na + × l oz chips
200 mg Na + = 2.9 oz chips
It would take 2.9 ounces of potato chips (about a handful) to replace
the lost sodium ions.
35. a. In a high-solute medium, the cytoplasm loses water and there-
fore its volume decreases. b. In a low-solute medium, the cytoplasm
gains water and therefore its volume increases.
36. E. coli accumulates water when grown in a low-salt medium.
However, regulation of water content only would cause a large in-
crease in cytoplasmic volume. To avoid this large increase in volume,
E. coli also exports K + ions. The opposite occurs when E. coli is
grown in a high-salt medium: The cytoplasmic water content is de-
creased, but cytoplasmic osmolarity increases as E. coli imports K+
ions. [From Record, M.T., et al., Trends Biochem. Sci. 23, 143–148
(1998).]
37. Since the molecular mass of H2O is 18.0 g · mol –1 , a given volume
(for example, 1 L or 1000 g) has a molar concentration of 1000 g · L–1 ÷
18.0 g · mol –1 = 55.5 M. By definition, a liter of water at pH 7.0 has
and two nonpolar tails as indicated and can form a bilayer (see Fig.
2.10). Compounds B, C, and E form neither micelles nor bilayers.
A
D
H 3C (CH2) 11
(CH2 )11
CH3
CH3
CH3
(CH 2) 11 CH3
CH2
CH2
N CH2 COO
HC
C
C
O
O
OHO
O
Polar head
Polar head
Nonpolar tail
Nonpolar
tails
27. a. In the nonpolar solvent, AOT’s polar head group faces the interior
of the micelle, and its nonpolar tails face the solvent.
Nonpolar
tails
Polar
head
H3 C (CH 2)3 CH
CH2CH 3
CH 2
H3 C (CH 2)3 CH
CH2CH 3
CH 2
CH2
CH
O
O
O
O O
O O
C
C S
AOT
b. The protein, which contains numerous polar groups, interacts
with the polar AOT groups in the micelle interior.
Water
Protein
Isooctane
28.
a.
b.
a)
b)
Nonpolar tail H 3C (CH2 ) 11 ONa Polar headO
O
O
S
NaO S
O
O
O(H2 C)11 CH 3
S
O
O
O(CH2) 11
CH3
NaO
NaO
S
O
O
O(CH 2) 11
CH3
S
O
O
H 3 C (CH 2) 11 O ONa
S OO
CH3
(CH2 ) 11 O
ONa
SO O
CH3
(CH2 ) 11 O
ONa
S
O
O
H3C
ONa
(CH 2) 11O
S
O
O
H3 C
ONa
(CH2) 11O

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6 Solutions
itself, 1.0 × 10−7 M, can be ignored because it is much smaller
than the hydroxide ion concentration contributed by the KOH.)
Kw = 1.0 × 10−14 = [H + ] [OH − ]
[H + ] = 1.0 × 10−14
[OH − ]
[H + ] = 1.0 × 10−14
(0.029 M)
[H + ] = 3.4 × 10−13 M
pH = −log[H + ]
pH = −log(3.4 × 10−13 )
pH = 12.5
48. a. The final concentration of HCl is (0.0015 L)(3 mol/L) ÷ 1 L
= 0.0045 M. Since HCl is a strong acid and dissociates com-
pletely, the added [H + ] is equal to [HCl]. (The existing hydrogen
ion concentration in the water itself, 1.0 × 10–7 M, can be ignored
because it is much smaller than the hydrogen ion concentration
contributed by the hydrochloric acid.)
pH = −log[H + ]
pH = −log(0.0045)
pH = 2.3
b. The final concentration of NaOH is (0.0015 L)(3 mol/L) ÷ 1
L = 0.0045 M. Since NaOH dissociates completely, the added
[OH–
] is equal to the [NaOH]. (The existing hydroxide ion con-
centration in the water itself, 1.0 × 10–7 M, can be ignored because
it is much smaller than the hydroxide ion concentration contrib-
uted by the NaOH.)
Kw = 1.0 × 10−14 = [H + ] [OH − ]
[H + ] = 1.0 × 10−14
[OH − ]
[H + ] = 1.0 × 10−14
(0.0045 M)
[H + ] = 2.2 × 10−12 M
pH = −log[H + ]
pH = −log(2.2 × 10−12 )
pH = 11.6
49.
HO
CH2
CH2
COO H
COO H
COO H
C
Citric acid H
H
N
Piperidine
O
O HH O C
O
C
Oxalic acid
CH2 CH2
O
O
O
O SNH
O HCH
CH2
CH2
CH2
CH2
O
C
H
H
H2 N
H2N
Lysine
N
H
NH
O
O O
Barbituric acid
4-Morphine ethanesulfonic acid (MES)

a hydrogen ion concentration of 1.0 × 10 –7 M. Therefore the ratio of
[H2 O] to [H+
] is 55.5 M/(1.0 × 10–7 M) = 5.55 × 10 8
.
38. [H + ] = [OH − ] = 1.47 × 10 −14
[H + ] = √1.47 × 10 −14
[H + ] = 1.21 × 10 −7 M
pH = −log(1.21 × 10 −7 M)
pH = 6.92
39. The HCl is a strong acid and dissociates completely. This means
that the concentration of hydrogen ions contributed by the HCl is
1.0 × 10 –9 M. But the concentration of the hydrogen ions contrib-
uted by the dissociation of water is 100-fold greater than this: 1.0 ×
10 –7 M. The concentration of the hydrogen ions contributed by the
HCl is negligible in comparison. Therefore, the pH of the solution
is equal to 7.0.
40. The pH of this solution is 7.0 (see Solution 39).The concen-
tration of hydroxide ions contributed by the dissociation of water
is 100-fold greater than that contributed by the dissociation of the
dilute NaOH.
41. −
42.
Acid, base,
or neutral? pH [H+ ] (M) [OH–
] (M)
Blood base 7.42 3.8 × 10–8 2.6 × 10–7
Saliva neutral 7.00 1.0 × 10–7 1.0 × 10–7
Urine acid 6.80 1.6 × 10–7 6.3 × 10–8
Gastric juice acid 2.10 7.9 × 10–3 1.3 × 10–12
43. The stomach contents have a low pH due to the contribution of
gastric juice (pH 1.5–3.0). When the partially digested material enters
the small intestine, the addition of pancreatic juice (pH 7.8–8.0) neu-
tralizes the acid and increases the pH.
44. The carbonate ions accept protons from water and form hydrox-
ide ions (as shown in the equation below), resulting in basic urine.
CO 2−
3 (aq) + H 2O(l) → HCO −
3 (aq) + OH − (aq)
45. a. C 2O 4
2− b. SO 3
2− c. HPO 4
2− d. CO 3
2− e. AsO 4
3− f. PO 4
3− g. O 2
2−
46. a. H2C2O4 b. H 2 SO3 c. H3PO 4 d. H 2 CO 3 e. H 2AsO 4
– f. H 2 PO4
–
g. H2 O2
47. a. The final concentration of HNO3 is (0.020 L)(1.0 M)
0.520 L =
0.038 M. Since HNO3 is a strong acid and dissociates completely,
the added [H+
] is equal to [HNO3]. (The existing hydrogen ion
concentration in the water itself, 1.0 × 10−7 M, can be ignored
because it is much smaller than the hydrogen ion concentration
contributed by the nitric acid.)
pH = −log[H + ]
pH = −log(0.038)
pH = 1.4
b. The final concentration of KOH is (0.015 L)(1.0 M)
0.515 L = 0.029 M
Since KOH dissociates completely, the added [OH−
] is equal to
the [KOH]. (The existing hydroxide ion concentration in the water

Loading page 7...

Solutions 7
54. pH = pK + log [A − ]
[ HA ]
log [A − ]
[ HA ] = pH − pK = 5.0 − 4.76 = 0.24
[A − ]
[ HA ] = 1.74 or [A − ] = 1.74 [HA ]
[A − ] = 1.74[HA ] = 1.74(0.05 M − [A − ] )
[A − ] = 0.087 − 1.74[A − ]
2.74[A − ] = 0.087 M
[A − ] = 0.032 M or 32 mM
55. First, determine the ratio of [A− ] to [HA]:
pH = pK + log [A − ]
[ HA ]
log [A − ]
[ HA ] = pH − pK
[A − ]
[ HA ] = 10(pH−pK)
Substitute the values for the desired pH (5.0) and the pK (4.76):
[A − ]
[ HA ] = 10(5.0−4.76) = 100.24 = 1.74
Calculate the number of moles of acetate (A−
) already present:
(0.50 L)(0.20 mol · L−1 ) = 0.10 moles acetate
Calculate the moles of acetic acid needed, based on the calculated ratio:
[A − ]
[ HA ] = 1.74
[ HA ] = 0.10 moles
1.74
[HA ] = 0.057 moles
Finally, calculate the volume of glacial acetic acid needed:
0.057 moles
17.4 mol · L −1 = 0.0033 L, or 3.3 mL
The addition of 3.3 mL to a 500-mL solution dilutes the solution by
less than 1%, which doesn’t introduce significant error.
56. Adding NaOH to the acetic acid will convert some of the acetic
acid (HA) to acetate (A–
):
NaOH + CH 3COOH →Na + + CH 3COO − + H 2O
For every mole of NaOH added, one mole of CH3 COOH will be
consumed, and one mole of CH3COO – will be generated. If x is the
number of moles of NaOH added, then x will also be the number of
moles of A– generated.
Calculate the initial amount of acetic acid:
The initial amount of acetic acid is 0.10 mol (see Solution 55), so the
final amount of acetic acid will be 0.10 mol – x.
[A − ]
[ HA ] = 1.74 = x
0.10 mol − x
x = 1.74(0.10 mol − x) = 0.174 mol − 1.74 x
2.74 x = 0.174 mol
x = 0.174 mol/2.74 = 0.0635 mol
Calculate the mass of NaOH to add:
0.0635 mol × 40.0 g · mol −1 = 2.54 g
50. Convert all the data to either Ka or pK values to evaluate (pK =
–logKa). The greater the Ka value, the stronger the acid—that is, the
greater the tendency for the proton to be donated. (The lower the pK
value, the stronger the acid.) From strongest to weakest acid: E, D, B,
A, C. Note that the stronger the acid, the weaker its conjugate base.
For example, citric acid is a stronger acid than citrate, and succinic
acid is a stronger acid than succinate.
Acid Ka pK
A citrate 1.74 × 10−5 4.76
B succinic acid 6.17 × 10–5 4.21
C succinate 2.29 × 10–6 5.64
D formic acid 1.78 × 10–4 3.75
E citric acid 7.41 × 10−4 3.13
51. Calculate the final concentrations of the weak acid (H 2PO −
4 ) and
conjugate base (HPO 4
2− ). Note that K+ is a spectator ion.
[H 2PO −
4 ] = (0.025 L)(2.0 M)
0.200 L = 0.25 M
[HPO 2−
4 ] = (0.050 L)(2.0 M)
0.200 L = 0.50 M
Next, substitute these values into the Henderson–Hasselbalch equa-
tion using the pK values in Table 2.4:
pH = pK + log [A − ]
[ HA ]
pH = 6.82 + log (0.50 M)/(0.25 M)
pH = 6.82 + 0.30
pH = 7.12
52. Use the pK value in Table 2.4 and the Henderson–Hasselbalch
equation to calculate the ratio of the concentrations of imidazole (A–
)
and the imidazolium ion (HA):
pH = pK + log [A − ]
[ HA ]
log [A − ]
[ HA ] = pH − pK
[A − ]
[ HA ] = 10(pH−pK)
[A − ]
[ HA ] = 10(7.4−7.0)
[A − ]
[ HA ] = 2.5
1
53. The fi nal volume is 500 mL + 10 mL + 20 mL = 0.53 L
[boric acid] = [HA ] = (0.01 L)(0.05 M)
0.53 L = 9.4 × 10−4 M
[borate] = [A − ] = (0.02 L)(0.02 M)
0.53 L = 7.5 × 10−4 M
pH = pK + log [A − ]
[ HA ]
= 9.24 + log 7.5 × 10−4
9.4 × 10−4
= 9.24 − 0.10 = 9.14

Loading page 8...

8 Solutions
0.5 1.0 1.5 2.0 2.5 3.0
H+ ions dissociated
pH
14
12
10
8
6
4
2
0
[H3PO4 ]
[H2 PO4
]
[HPO4
2]
[PO 4
3−]
pK1
Midpoint one
[H3PO 4] [H2PO4
]
pK2
Midpoint two
[H 2PO 4
] [HPO 4
2]
pK3
Midpoint three
[HPO 4
2−] [PO4
3−]
b. H 3PO 4 →H + + H 2PO −
4
H 2PO −
4 →H + + HPO 2−
4
HPO 2−
4 →H + + PO 3−
4
c. The dissociation of the second proton has a pK of 6.82, which
is closest to the pH of blood. Therefore the weak acid present in
blood is H2PO4
– and the weak base is HPO4
2–
.
d. The dissociation of the third proton has a pK of 12.38. There-
fore, a buffer solution at pH 11 would consist of the weak acid
HPO 4
2− and its conjugate base, PO 4
3− (supplied as the sodium salts
Na2HPO4 and Na3PO4).
64. The aspirin is more likely to be absorbed in the stomach at pH 2.
At this pH, the carboxylate group is mostly protonated and uncharged.
This allows the aspirin to pass more easily through the nonpolar lipid
bilayer. At the pH of the small intestine, the carboxylate group is
mostly in the ionized form and will be negatively charged. Charged
species are more polar than uncharged species (and are likely to be
hydrated) and will have difficulty traversing a lipid bilayer.
65. a. HO (H2 C)2 HN N (CH2) 2 SO3

Weak acid (HA)
Conjugate base (A)
HO (H2 C)2 (CH 2) 2 SO3
H
NN

b. The pK for HEPES is 7.55; therefore, its effective buffering
range is 6.55–8.55.
c. 1.0 L × 0.10 mole
L × 260.3 g
mol = 26 g
Weigh 26 g of the HEPES salt and add to a beaker. Dissolve in
slightly less than 1.0 liter of water (leave “room” for the HCl solu-
tion that will be added in the next step).
d. At the final pH,
[A − ]
[ HA ] = 10(pH−pK) = 10(8.0−7.55) = 100.45 = 2.82
For each mole of HCl added, x, one mole of HEPES salt (A–
) will
be converted to a mole of HEPES acid (HA). The starting amount
of A– is (1.0 L)(0.10 mol · L–1
) = 0.10 moles. After the HCl is
added, the amount of A− will be 0.10 moles – x, and the amount
of HA will be x. Consequently,
57. a. H 2CO 3 →H + + HCO −
3
HCO −
3 →H + + CO 2−
3
b. The pK of the first dissociation is closer to the pH; therefore
the weak acid present in blood is H2CO3 and the conjugate base
is HCO3
–
.
c. pH = pK + log [HCO −
3 ]
[H 2CO 3]
7.40 = 6.35 + log 24 × 10−3 M
[H 2CO 3]
1.05 = log 24 × 10−3 M
[H 2CO 3]
11.2 = 24 × 10−3 M
[H 2CO 3]
[H 2CO 3] = 2.1 × 10−3 M = 2.1 mM
58. The pK of the fluorinated compound would be lower (it is 9.0);
that is, the compound becomes less basic and more acidic. This
occurs because the F atom, which is highly electronegative, pulls on
the nitrogen’s electrons, loosening its hold on the proton.
59. a. CH3
C O
COO
Pyruvate
b. Pyruvate predominates in the cell at pH 7.4. The pK values for
carboxylic acid groups are typically in the 2–3 range; therefore,
the carboxylate group will be unprotonated at physiological pH.
60. pH 2 + H 3NCH 2COOH
pH 7 + H 3NCH 2COO −
pH 10 H 2NCH 2COO −
The carboxylic acid group has a pK of 2.35, and the amino group has
a pK of 9.78. The Henderson–Hasselbalch equation can be used to
calculate the exact percentage of protonated/unprotonated forms of
each functional group, but that really isn’t necessary. Instead, the pK
values for each group should be compared to the pH. At pH = 2, the
pH is below both pK values, so both functional groups are mostly pro-
tonated. At pH = 7, the pH is well above the pK for the carboxylic acid
group but below the pK for the amino group. Therefore the carboxylic
acid group is unprotonated and the amino group is protonated. At
pH = 10, the pH is above the pK values of both functional groups.
Thus, both groups are mostly unprotonated.
61. a. 10 mM glycinamide buffer, because its pK is closer to the
desired pH. b. 20 mM Tris buffer, because the higher the concen-
tration of the buffering species, the more acid or base it can neutral-
ize. c. Neither. Both a weak acid and a conjugate base are required
buffer constituents. Neither the weak acid alone (boric acid) nor
the conjugate base alone (sodium borate) can serve as an effective
buffer.
62. a. 10 mM acetic acid buffer, because its pK is closer to the
desired pH. b. 20 mM acetic acid buffer, because the higher concen-
tration of buffer species will allow it to neutralize a greater amount
of acid or base. c. Neither. Both a weak acid and a conjugate base
are required buffer constituents. Neither the weak acid alone (acetic
acid) nor the conjugate base alone (sodium acetate) can serve as an
effective buffer.
63. a. The three ionizable protons of phosphoric acid have pK values
of 2.15, 6.82, and 12.38 (Table 2.4). The pK values are the mid-
points of the titration curve:

Loading page 9...

Solutions 9
pH = pK + log [A − ]
[ HA ]
pH = 8.3 + log 48.5 mmol ÷ 1001.5 mL
51.5 mmol ÷ 1001.5 mL
pH = 8.3 + (−0.026)
pH = 8.27
The buffer is effective: The pH increases only 0.07 unit (from 8.2
to 8.27) with the addition of the strong base. In comparison, the
addition of the same amount of base to water, which is not buf-
fered, results in a pH change from approximately 7.0 to 11.6 (see
Problem 48b).
67. pH = pK + log [A − ]
[ HA ]
log [A − ]
[ HA ] = pH − pK
[A − ]
[ HA ] = 10(pH−pK)
[A − ]
[ HA ] = 10(6.5−7.0) = 10−0.5 = 0.316
Since the starting solution contains (0.5 L)(0.01 mol · L −1
) = 0.005
mole of imidazole (A–
), the amount of imidazolium chloride (HA)
needed is 0.005 mol/0.316 = 0.016 moles. The stock imidazolium
chloride is 1 M, so the volume of imidazolium chloride to be added is
0.016 mol
1.0 mol · L −1 = 0.016 L or16 mL
68. a. First, calculate the ratio of [A−
] to [HA]. Rearranging the
Henderson–Hasselbalch equation gives
[A − ]
[ HA ] = 10(pH−pK) = 10(2.0−8.3) = 10−6.3 = 5 × 10−7
Virtually all of the Tris is in the weak acid form. Therefore, the
concentration of the weak acid, HA, is 0.10 M and the concentra-
tion of the conjugate base, A−
, is 5.0 × 10−8 M.
b. The added HCl dissociates completely, so the amount of H+
added is (0.0015 L)(3.0 mol · L−1
) = 0.0045 mol. In an effective
buffer, the acid would convert some of the conjugate Tris base to
weak acid. But the concentration of conjugate base is already neg-
ligible. Therefore, the moles of additional H+ should be added to
the concentration of hydrogen ions already present (1.0 × 10−2 M),
for a total concentration of 0.0145 M.
pH = −log[H + ] = log (0.0145 M) = 1.84
The buffer has not functioned effectively. There was not enough
conjugate base to react with the additional hydrogen ions added.
The result is a decrease in pH from 2.0 to 1.84.
c. When NaOH is added, an equivalent amount of Tris acid (HA)
is converted to Tris base (A−
). Let x = moles of OH− added =
(0.0015 L)(3.0 mol · L−1
) = 0.0045 moles = 4.5 mmol.
The final amount of A− is 5.0 × 10−8 mol + 4.5 mmol = 4.5 mmol.
The final amount of HA is 100 mmol – 4.5 mmol = 95.5 mmol.
The new pH is determined by substituting the new concentrations
of H− and HA into the Henderson–Hasselbalch equation:
pH = pK + log [A − ]
[ HA ]
pH = 8.3 + log (4.5 mmol ÷ 1001.5 mL)
(95.5 mmol ÷ 1001.5 mL)
pH = 8.3 + (−1.3) = 7.0
[A − ]
[ HA ] = 2.82 = 0.10 mole − x
x
2.82x = 0.10 mol − x
3.82x = 0.10 mol
x = 0.10 mol/3.82 = 0.0262 mol
Calculate how much 6.0 M HCl to add:
0.0262 mol
6.0 mol · L −1 = 0.0044 L, or 4.4 mL
To make the buffer, dissolve 26 g of HEPES salt [see part c] in less
than 1.0 L. Add 4.4 mL of 6.0 M HCl, then add water to bring the
final volume to 1.0 L.
66. a.
Weak acid (HA)
CH 2OH
CH2OH
HOH2C C NH 3

Conjugate base (A)
H
NH2
CH2 OH
CH2 OH
HOH2 C C
b. The pK of Tris is 8.30; therefore, its effective buffering range
is 7.30–9.30.
c. Rearranging the Henderson–Hasselbalch equation gives
[A − ]
[ HA ] = 10(pH−pK) = 10(8.2−8.3) = 10−0.1 = 0.79
Since [A − ] + [HA] = 0.10 M, [A − ] = 0.10 M − [HA ],
and (0.10 M − [HA ] )
[ HA ] = 0.79
0.79 [HA ] = 0.10 M − [HA ]
1.79[HA ] = 0.10 M
[ HA ] = 0.10 M
1.79 = 0.056 M = 56 mM
[A − ] + [HA ] = 0.10 M = 100 mM, so [A − ] = 44 mM
d. When HCl is added, an equivalent amount of Tris base (A–
) is
converted to Tris acid (HA).
Let x = moles of H+ added = (0.0015 L)(3.0 mol · L–1
) = 0.0045
moles = 4.5 mmol.
The final amount of A– is 44 mmol – 4.5 mmol = 39.5 mmol.
The final amount of HA is 56 mmol + 4.5 mmol = 60.5 mmol.
Use the Henderson–Hasselbalch equation to calculate the new pH:
pH = pK + log [A − ]
[ HA ]
pH = 8.3 + log 39.5 mmol ÷ 1001.5 mL
60.5 mmol ÷ 1001.5 mL
pH = 8.3 + (−0.2)
pH = 8.1
The buffer is effective: The pH decreases about 0.1 unit (from
8.2 to 8.1) with the addition of the strong acid. In comparison,
the addition of the same amount of acid to water, which is not
buffered, results in a pH change from approximately 7.0 to 2.3
(see Problem 48a).
e. When NaOH is added, an equivalent amount of Tris acid (HA)
is converted to Tris base (A–
). Let x = moles of OH– added =
(0.0015 L)(3.0 mol · L–1
) = 0.0045 moles = 4.5 mmol.
The final amount of A– is 44 mmol + 4.5 mmol = 48.5 mmol.
The final amount of HA is 56 mmol – 4.5 mmol = 51.5 mmol.
Use the Henderson–Hasselbalch equation to calculate the new pH:

Loading page 10...

10 Solutions
101.05 = [HCO −
3 ]
[H 2CO 3 ]
[HCO −
3 ]
[H 2CO 3 ] = 11.2
1
In order to serve as an effective buffer (i.e., absorb both added H+
and OH– ), both a conjugate base and a weak acid must be present.
In the patient, the ratio of conjugate base to weak acid does not lie
within an effective buffering range. The bicarbonate concentration
(conjugate base) is too high relative to the carbonic acid (weak acid)
concentration; thus the relative amount of weak acid is insufficient.
[Krause, D. S., Wolf, B. A., and Shaw, L. M., Ther. Drug Monit. 14,
441– 451 (1992).]
73. Ammonia and ammonium ions are in equilibrium, as represented
by the following equation:
NH +
4 ⇌ H + + NH 3
Carbonic acid and bicarbonate ions are in equilibrium, as represented
by the following equation:
H 2CO 3 ⇌ H + + HCO −
3
Phosphate ions are in equilibrium, according to the following equation:
H 2PO −
4 ⇌ H + + HPO 2−
4
In metabolic acidosis, the concentration of protons increases, so the
equilibrium shifts to form H2PO 4
–
, carbonic acid, and ammonium
ions. In order to bring the pH back to normal, the kidney excretes
H2 PO 4
– and ammonium ions, and bicarbonate ions are reabsorbed. The
result is a decrease in the concentration of protons and an increase
in blood pH.
74. The relevant equations are shown in Solution 73. In metabolic
alkalosis there is an excess of hydroxide ions, which react with pro-
tons to form water. This causes the equilibria to shift to form HPO 4
2–
,
NH 3 , and HCO 3
– . In order to bring the pH back to normal, the kidney
reabsorbs NH4
+ and H 2PO 4
– and excretes HCO3
– .
75. The concentrations of both Na+ and Cl– are greater outside the
cell than inside (see Fig. 2.12). Therefore the movement of these ions
into the cell is thermodynamically favorable. Na+ movement into the
cell drives the exit of H+ via an exchange protein in the plasma mem-
brane (the favorable movement of Na+ into the cell “pays for” the
unfavorable movement of H+ out of the cell). Similarly, the move-
ment of Cl– into the cell drives the movement of HCO 3
– out of the cell
through another exchange protein.
76. Acetoacetate and 3-hydroxybutyrate are acids (they are ionized
at physiological pH). The accumulation of the ketone bodies there-
fore causes metabolic acidosis. The body attempts to compensate by
increasing the breathing rate in order to eliminate more CO2.
77. The cell-surface carbonic anhydrase can catalyze the conversion
of H+ + HCO3
– to CO2 , which can then diffuse into the cell (the ionic
H + and HCO3
– cannot cross the hydrophobic lipid bilayer on their
own). Inside the cell, carbonic anhydrase converts the CO2 back to
H + + HCO3
–
.
78. The lungs can compensate for metabolic acidosis through an
increase in the breathing rate in order to eliminate more CO2. The
kidneys can compensate for respiratory acidosis by increasing the
breakdown of glutamine to produce NH3 (excreted in urine as NH 4
+ ,
see Solution 73); however, this mechanism requires the synthesis of
enzymes, which takes several hours at least.
Tris is not an effective buffer at pH 2.0, a pH more than 6 units
lower than its pK value. Virtually all of the Tris is in the weak acid
form at this pH. If acid is added, there is not enough base to absorb
the excess added hydrogen ions, and the pH decreases. If base is
added, some of the weak acid is converted to the conjugate base
and the pH approaches the value of the pK.
69. H + (aq) + HCO −
3 (aq) ⇌ H 2CO 3 (aq) ⇌ H 2O (l) + CO 2 (aq)
Failure to eliminate CO2 in the lungs would cause a buildup of CO2 (aq).
This would shift the equilibrium of the above equations to the left.
The increase in CO2 (aq) would lead to the increased production of
carbonic acid, which would in turn dissociate to form additional hy-
drogen ions, causing acidosis.
70. a. Mechanical hyperventilation removes CO 2 from the patient’s
lungs. Carbonic acid in the blood would produce more water and
CO2 to make up for the loss of CO2. This in turn would cause
additional hydrogen ions and bicarbonate ions to form more
carbonic acid. The loss of hydrogen ions would result in an in-
creased pH, bringing the patient’s pH back to normal.
b. The additional bicarbonate would combine with hydrogen ions
to form carbonic acid. The additional carbonic acid would disso-
ciate to form water and carbon dioxide. This helps alleviate the
acidosis because the bicarbonate combines with excess hydrogen
ions, thus decreasing the hydrogen ion concentration and increas-
ing the pH. However, it is not acceptable for use in patients with
ALI because of the increased production of aqueous CO2 in the
blood. The CO2 produced would need to be exhaled in the lungs,
which would be difficult in patients with ALI.
c. Tris becomes protonated to form its conjugate acid. This re-
moves H+ from circulation and brings the pH back to normal. The
protonated form of Tris is excreted in the urine. This method of
acidosis treatment does not involve exhalation of CO2 and is there-
fore an acceptable treatment for patients with ALI.
CH 2OH
CH 2OH
HOH 2 C C NH 3

NH2
CH2 OH
CH2 OH
HOH 2C C H

[From Kallet, R. H., et al., Am. J. Respir. Crit. Care Med. 161,
1149–1153 (2000).]
71. During hyperventilation, too much CO 2 (which is equivalent to
H+ in the form of carbonic acid) is given off, resulting in respiratory
alkalosis. By repeatedly inhaling the expired air, the individual can
recover some of this CO2 and restore acid–base balance.
72. The ratio of bicarbonate to carbonic acid in the patient’s blood
can be determined using the Henderson–Hasselbalch equation:
pH = pK + log [A − ]
[ HA ]
7.55 = 6.35 + log [HCO −
3 ]
[H 2CO 3 ]
101.2 = [HCO −
3 ]
[H 2CO 3 ]
[HCO −
3 ]
[H 2CO 3 ] = 15.8
1
Similarly, the ratio of bicarbonate to carbonic acid in a normal person’s
blood can be determined:
pH = pK + log [A − ]
[ HA ]
7.4 = 6.35 + log [HCO −
3 ]
[H 2CO 3 ]

Loading page 11...

Solutions 11
8-Chloroadenosine
NH 2
N N
N N
Cl
O
H H
HH
OH OH
CH 2 OH
12. The compound is a thymidine analog. [From Maity, J. and Stromberg,
R., Molecules 18, 12740–12750 (2013).]
5-Bromo-2′-deoxyuridine
O
NO
HN Br
O
H H
HH
OH H
CH2OH
13. a. A diphosphate bridge links the ribose groups in each dinuc-
leotide. This linkage is a variation of the monophosphate bridge
(phosphodiester linkage) in DNA and RNA. b. The adenosine group
in CoA bears a phosphoryl group on C3ʹ.
14. O
O
H H
HH
O OH
CH2
O
O
O P NH 2
N
N
O
NH 2
O
H H
HH
OH OH
CH 2
O
O
O P
N
N
N N
Phosphodiester
bond
If the dinucleotide were DNA, it would lack OH groups at each ribose
C2ʹ position.
15.
O
OH
OH
O
O
OO
NH2
NH
NH2
N
H H
H H
H H
H H
N N
G
NN
N N
A
CH2
O
O
O P
OO
O
P
3
5
CH25
2
Chapter 3
1. The heat treatment destroys the polysaccharide capsule of the wild-
type Pneumococcus, but the DNA survives the heat treatment. The
DNA then “invades” the mutant Pneumococcus and supplies the genes
encoding the enzymes needed for capsule synthesis that the mutant
lacks. The mutant is now able to synthesize a capsule and has the ca-
pacity to cause disease, which results in the death of the mice and the
appearance of encapsulated Pneumococcus in the mouse tissue.
2. These experiments showed that the transforming factor was
neither a protein nor RNA.
3. Some of the labeled “parent” DNA appears in the progeny, but
none of the labeled protein appears in the progeny. This indicates
that the bacteriophage DNA is involved in the production of progeny
bacteriophages, but bacteriophage protein is not required.
4. The triple-helical model is not consistent with the hydrophobic
effect, which suggests that the nonpolar nitrogenous bases would reside
in the center of the DNA structure and the hydrophilic phosphates
would reside on the surface. The triple-helical model also assumes
that the phosphate groups are protonated and form stabilizing hydro-
gen bonds in the DNA interior. But the pK value for phosphate is
well below 7, so the phosphate groups would not be protonated at
physiological pH. In the absence of hydrogen bonds, there are no ad-
ditional forces that would hold the strands of the triple helix together.
5. Thymine (5-methyl uracil) contains a methyl group attached to C5
of the pyrimidine ring of uracil.
6.
P
OO H
H H
O OH
H
O
O
H2
C
Adenine
7.
N
H
N
H 3C
O
5-Methylcytosine
NH2
8. a.
N
N N
H
N
H CH 3
N
N6-Methyladenine
b. The N 6
-DNA methyltransferase might be a good drug target. If
methylation of certain adenine residues is required for virulence,
then it is possible that inhibition of the bacterial transferase enzyme
might prevent adenine methylation and thus prevent disease caused
by pathogenic bacteria.
9. The base 5-chlorouracil is a substitute for thymine (5-methyluracil).
10. A chlorine is substituted for a hydrogen in 5-chorouracil, which
closely resembles thymine (see Solution 9). Therefore, the culture
containing 5-chlorouracil will incorporate this base in place of thymine
as the DNA replicates. The 5-chlorouracil has a greater mass than
thymine, so DNA isolated from this culture will have a greater mass
than DNA isolated from the control culture.
11. [From Jordheim, L. P., Durantel, D., Zoulim, F., and Dumontet,
C. Nat. Rev. Drug Discov. 12, 447–464 (2013).]

Loading page 12...

12 Solutions
25. The sugar–phosphate backbone is on the outside of the molecule.
The polar sugar groups can form hydrogen bonds with the surround-
ing water molecules. The negatively charged phosphate groups inter-
act favorably with positively charged ions. The nonpolar nitrogenous
bases are found on the inside of the molecule and interact favorably
via stacking interactions. In this way, contact with the aqueous solu-
tion is minimized, as described by the hydrophobic effect.
26. a. Proteins are more likely to bind to the major groove, which
can easily accommodate proteins. The larger surface area of the ma-
jor groove allows multiple favorable interactions between the DNA
and protein. b. The positively charged side chains of the Lys and Arg
residues form ion pairs with the negatively charged phosphate groups
on the DNA backbone. These are strong interactions, so the histones
have a high affinity for DNA.
27. a. The Tm is approximately 72°C. b. The melting curves are
shown below.
1.0
1.4
1.3
1.2
1.1
Temperature (°C)
5030
Relative absorbance at 260 nm
70
Tm Tm
D. discoideum S. albus
90
28. a. The DNA contains 50% G + C, so its melting point would be
approximately 90°C. b. The DNA would need to be cooled gradually
to 65–70°C (20–25°C below its melting temperature).
GC content (%)
700 10 20 30 40 50 60 70 80
80
90
100
110
Tm (°C)
29. The DNA from the organisms that thrive in hot environments
would contain more G and C than DNA from species living in a more
temperate environment. The higher GC content increases the stability
of DNA at high temperatures.
30. The positively charged sodium ions can form ion pairs with the
negatively charged phosphate groups on the DNA backbone and
“shield” the negative charges from one another. This increases the
overall stability of DNA and makes it more difficult to melt.
31. a. You should increase the temperature to melt out imperfect
matches between the probe and the DNA. b. You should decrease the
temperature to increase the chances that the two strands will align,
despite the mismatch.
32. Heating denatures the target DNA (separates its two strands) so
that a single-stranded probe can more easily form sequence-specific
hydrogen bonds with it.
16.
O
O
OH OH
O
H
H H
H
N 1
NH
OH OH
N NH
H H
H
N
9
O
CH 2OPO O P
O O
H2C
17. The organism must also contain 19% A (since [A] = [T] accord-
ing to Chargaff’s rules) and 62% C + G (or 31% C and 31% G, since
[C] = [G]). Each cell is a diploid, containing 60,000 kb or 6 × 107
bases. Therefore,
[A] = [T] = (0.19)(6 ×107 bases) = 1.14 × 107 bases
[C] = [G] = (0.31)(6 × 107 bases) = 1.86 × 107 bases
18. a. Using Chargaff’s rules (see Solution 17), the number of C
residues must also be 24,182. Subtracting (2 × 24,182) from 97,004
yields 48,640 (A + T) residues. Dividing this number by 2 yields
24,320 residues each of A and T. b. GenBank reports only the sequence
of a single strand of DNA, since the sequence of the complementary
strand can easily be deduced using Watson–Crick base-pairing.
19. The total amount of purines (A + G) in DNA must equal the
total amount of pyrimidines (C + T) because each base pair in the
double-stranded DNA molecule consists of a purine and a pyrimidine.
This is not true for RNA, which is single-stranded.
20. The genome contains 28.7% T, 21.5% G, 29.3% A, and 20.6% C.
Chargaff ’s rules do not apply because the viral genome is composed
of single-stranded DNA.
21. It is a G:C base pair.
22.
N
H
N
N
NH
N
H
O
N
N HH
O
Cytosine
Hypoxanthine
N
N
N
H
N
N
NH
N
H
O
N
N HH
Adenine
Hypoxanthine
N
H
N
O
Uracil
N
NH
N
H
O
N
H
O
Hypoxanthine
23. The statement is false because the greater stability of GC-rich
DNA is due to the stronger stacking interactions involving G:C base
pairs and does not depend on the number of hydrogen bonds in the
base pairs.
24. It is certainly the case that hydrogen bonds hold A:T and G:C
base pairs together and that these interactions are very favorable. But
upon denaturation of the DNA, each nitrogenous base has the oppor-
tunity to form equally favorable hydrogen bonds with water. There-
fore, forces other than hydrogen bonds must contribute to the overall
stability of the DNA molecule.

Loading page 13...

Solutions 13
35. a. 3′-TGTGGTACCACGTAGACTGA-5′
b. 5′-ACACCAUGGUGCAUCUGACU-3′
36. a. The top strand is the coding strand and the bottom strand is
the noncoding strand. b. Only coding strands are published because
the mRNA sequence is identical to the sequence of the coding strand,
with the exception that U replaces T in the mRNA.
37. a. A poly-Phe polypeptide was produced. b. Poly A produces
poly-Lys; poly C yields poly-Pro; and poly G yields poly-Gly.
38. a. The cell-free system produces polypeptides consisting of al-
ternating Val and Cys residues. Some of the polypeptides begin with
Val; others begin with Cys, depending on which reading frame is
used. b. The production of this peptide does not allow one to un-
ambiguously assign the GUG and UGU codons. Additional experi-
mental data are required to make this assignment.
39. The number of possible sequences of four different nucleotides
taken n at a time is 4n; here n is the number of nucleotides in the
sequence. a. 4 1 = 4 b. 4 2 = 16 c. 4 3 = 64 d. 4 4 = 256. At least three
nucleotides are necessary to code for 20 amino acids.
40. There are 216 codons possible: 63 = 216. [From Malyshev, D. A.,
Dhami, K., Lavergne, T., Chen, T., Dai, N., Foster, J. M., Corrêa Jr., I.
R., and Romesberg, F. E., Nature 509, 385–388 (2014).]
41. a. First reading frame:
AGG TCT TCA GGG AAT GCC TGG CGA GAG GGG AGC
Arg - Ser - Ser - Gly - Asn - Ala - Trp - Arg - Glu - Gly - Ser-
AGC TGG TAT CGC TGG GCC CAA AGG C
Ser - Trp - Tyr - Arg - Trp - Ala - Gln - Arg
Second reading frame:
A GGT CTT CAG GGA ATG CCT GGC GAG AGG GGA GCA
- Gly - Leu - Gln - Gly - Met - Pro - Gly - Glu - Arg - Gly - Ala-
GCT GGT ATC GCT GGG CCC AAA GGC
Ala - Gly - Ile - Ala - Gly - Pro - Lys - Gly
Third reading frame:
AG GTC TTC AGG GAA TGC CTG GCG AGA GGG GAG CAG
--Val - Phe - Arg - Glu - Cys - Leu - Ala - Arg - Gly - Glu - Gln-
CTG GTA TCG CTG GGC CCA AAG GC
Leu - Val - Ser - Leu - Gly - Pro - Lys-
b. The second reading frame, which produces a protein in which every
third amino acid is Gly, is the correct reading frame.
42. a. Asparagine has two codons, AAU and AAC (see Table 3.3).
An A→G mutation at the second position could generate a codon
for serine (AGU or AGC). b. The CGA codon codes for the amino
acid arginine; the mutation (C→T in the DNA) converts the codon
to a Stop codon. When the mRNA for the gene is translated, pro-
tein synthesis terminates prematurely and the truncated protein is
nonfunctional.
43. The genetic code (shown in Table 3.3) is redundant. Since there
are 64 different possibilities for 3-base codons and only 20 amino
acids, most amino acids have more than one codon. If a mutation
happens to occur in the third position (3ʹ end), the mutation might not
alter the protein sequence. For example, GUU, GUC, GUA, and GUG
all code for valine. A mutation in the third position of a valine codon
would still result in the selection of valine and would have no effect
on the amino acid sequence of the protein.
44. The same segment of DNA can encode two different proteins if
each strand is a coding strand.
45. First, identify the translation start site, the Met residue whose
codon is AUG in the mRNA (see Table 3.3) or ATG in the DNA.
Translation stops at the DNA sequence TAA, which corresponds to
33. a. An inherited characteristic could be determined by more than
one gene. b. Some sequences of DNA encode RNA molecules that are
not translated into protein (for example, rRNA and tRNA). c. Some
genes are not transcribed during a cell’s lifetime. This can occur if the
gene is expressed only under certain environmental conditions or in cer-
tain specialized cells in a multicellular organism.
34. a. The DNA isolated after one generation is a homogeneous
sample of DNA with a density intermediate between DNA containing
all 14
N and all 15
N. b. The DNA isolated after the second generation is
heterogeneous. Half of the DNA has the same density as the first gener-
ation; half of the DNA consists of all 14
N DNA and has a lower density.
15 N
14 N
First-generation
daughter molecules
Second-generation
daughter molecules

c. A hypothetical scheme for conservative DNA replication is shown
below. The DNA isolated after both the first and the second genera-
tions is heterogeneous. Half of the DNA has the same high density as
the original DNA (all 15
N); half of the DNA consists of all 14
N DNA
and has a lower density.
15
N
14
N
First-generation
daughter molecules
Second-generation
daughter molecules

Loading page 14...

14 Solutions
• How many copies of each gene are in the organism’s genome?
• What is the amount of noncoding DNA in the genome? Is the non-
coding DNA really “junk DNA,” or does it have some biological role?
• How many transposable elements are in the noncoding DNA?
53. a. The fi rst reading frame is the longest ORF.
First reading frame:
TAT GGG ATG GCT GAG TAC AGC ACG TTG AAT GAG
Tyr - Gly - Met - Ala - Glu - Tyr - Ser - Thr - Leu - Asn - Glu-
GCG ATG GCC GCT GGT GAT G
Ala - Met - Ala - Ala - Gly - Asp-
Second reading frame:
T ATG GGA TGG CTG AGT ACA GCA CGT TGA ATG AGG
-Met - Gly - Trp - Leu - Ser - Thr - Ala - Arg -Stop - Met - Arg-
CGA TGG CCG CTG GTG ATG
Arg - Trp - Pro - Leu - Val - Met
Third reading frame:
TA TGG GAT GGC TGA GTA CAG CAC GTT GAA TGA GGC
---Trp - Asp - Gly - Stop - Val - Gln - His - Val - Glu - Stop - Gly-
GAT GGC CGC TGG TGA TG
Asp - Gly - Arg - Trp - Stop
b. Assuming the reading frame has been correctly identified, the most
likely start site is the first Met residue in the first ORF.
54. Like the symbiont described in Problem 49, the bacteriophage
is parasitic and makes use of the host cell’s tRNAs, protein-synthe-
sizing machinery, and replication proteins.
55. If a SNP occurs every 300 nucleotides or so, and if there are
about 3 million kb (3 × 10 9 nucleotides) in the human genome (see
Table 3.4), then there are (3 × 109 bp ÷ 300 bp/SNP) = 1 × 10 7
(10 million) total SNPs in the human genome. [Source: ghr.nlm.nih.
gov/handbook/genomicresearch/snp]
56. Because ~1.4% of the human genome consists of protein-coding
genes, about 1.4% of the 10 million SNPs, or 140,000, are likely to
affect these genes. Since the total number of genes is only ~21,000, in
theory, every gene would differ.
57. a. The strongest associations are located between positions
67,370,000 and 67,470,000. b. Gene B contains SNPs associated
with the disease whereas Genes A and C do not. [From Duerr, R. H.,
et al., Science 314, 1461–1463 (2006).]
58. Chromosomes 10, 11, and 13 have genes carrying SNPs that are
correlated with the colon disease. [From Garcia-Barcelo, M., et al.,
Proc. Natl. Acad. Sci. USA 106, 2694–2699 (2009).]
59. MspI, AsuI, EcoRI, PstI, SauI, and NotI generate sticky ends.
AluI and EcoRV generate blunt ends.
60. The restriction enzyme with the longer recognition sequence
would be a rare cutter, because it is likely to encounter this sequence
less often and therefore will cleave the DNA less frequently than a
restriction enzyme with a shorter recognition sequence.
61. AluI cleaves the sequence at two locations and EcoRI and NotI
cleave the sequence at one location each. The other enzymes listed in
Table 3.5 do not cleave this segment of the plasmid DNA.
CGCGGATCCGAATTCGAGCTCCGTCGACAAGCTTGCGGCCGCACTCGAG
EcoRI AluI AluI NotI
62. The enzyme MspI generates sticky ends. The single-stranded re-
gions are then removed by the action of the exonuclease, releasing the
free nucleotides C and G:
the stop codon UAA in the mRNA. Use Table 3.3 to decode the inter-
vening codons, substituting U for T.
CTCAGAGTTCACC ATG GGC TCC ATC GGT GCA GCA AGC
Met Gly Ser Ile Gly Ala Ala Ser
ATG GAA ··· 1104 bp ·· TTC TTT GGC AGA TGT GTT TCC
Met Glu ···················· Phe Phe Gly Arg Cys Val Ser
CCT TAA AAAGAA
Pro *
46. a. The siRNA is an “antisense” mRNA, so its sequence should be
complementary to that of the mRNA. The solution below shows an
siRNA that corresponds to the 5ʹ end of the mRNA:
mRNA 5ʹ→3ʹ AUG GGC UCC AUC GGU GCA GCA AGC AUG GAA
siRNA 3ʹ→5ʹ UAC CCG AGG UAG CCA CGU CGU UCG UAC CUU
b. When the antisense RNA binds to the mRNA, the mRNA can no
longer serve as a template for protein synthesis. (In the cell, the bind-
ing of antisense RNA to mRNA involves an enzyme that degrades
the mRNA into smaller fragments.) c. The siRNA molecules must be
able to cross the cell membrane to enter the cell and find the target
mRNA.
47. a. The normal protein sequence is ····Glu-Asn-Ile-Ile-Phe-Gly-
Val-Ser-Tyr····. The mutant protein sequence is the same except the
Phe at position 508 is deleted. Note that although the deletion of Phe
affects codons 507 and 508, the redundancy of the genetic code means
that the Ile at position 507 is not affected, and the amino acids down-
stream of the mutation are also unaffected. b. The sequence of the
normal protein in this region of the gene is ····Asn-Ile-Asp-Thr····. The
amino acid sequence of the mutated CF gene (in which two bases, A
and T, are missing), is ····Asn-Arg-Tyr····. This is a frameshift muta-
tion and all of the amino acids past the deletion will differ from the
amino acids in the normal protein.
48. In order for a single nucleotide change to switch an arginine
codon to a glutamine codon, either a CGA or a CGG Arg codon must
have been replaced with a CAA or CAG glutamine codon. In either
case, the middle G has been changed to an A. The correct reading
frame with the amino acid sequences for the normal and mutant pro-
teins are shown below. [From Ludwig, E. H. and McCarthy, B. J. Am.
J. Hum. Genet. 47, 712–720 (1990).]
Normal gene · · · CT GGC CGG CTC AAT GGA GAG TCC · · ·
Gly Arg Leu Asn Gly Glu Ser
Mutated gene · · · CT GGC CAG CTC AAT GGA GAG TCC · · ·
Gly Gln Leu Asn Gly Glu Ser
49. C. ruddii, with such a small genome and only 182 genes, must be
some sort of parasite rather than a free-living bacterium. (In fact, C.
ruddii is an insect symbiont.)
50. Prokaryotes tend to have smaller genomes than eukaryotes, so
evolution has shaped the prokaryote genome to pack in genes more
efficiently. Eukaryotes, with larger genomes and more noncoding
DNA, have more space to arrange genes.
51. The 35 million differences out of 3.0 billion total nucleotides
represent approximately 1%, or a bit less than the original claim.
(This number reflects single-base differences and does not account
for insertions and deletions of multiple bases.)
52. Questions that need to be addressed in order to solve the C-value
paradox:
• How does one define organismal complexity? Perhaps humans are
not the most complex organisms.
• How much of the organism’s genome codes for RNA? For protein?
What are the biological roles of these gene products?

Loading page 15...

Solutions 15
In practice, however, you’d want to embed the recognition sequence
rather than having the recognition sequence on the ends; the reason for
this will be explained in Chapter 20.
69. Primers with high GC content have high Tm values. If the annealing
temperature is much lower than the melting temperature, improper
base pairing may occur (see Figure 3.8) and the desired gene frag-
ment may not be amplified.
70. You can use a DNA polymerase that is not heat-stable. You
would have to cool the reaction mixture to a temperature at which the
polymerase works best and you would have to add the enzyme at each
reaction cycle because it would be destroyed every time the temper-
ature was raised to melt the double-stranded DNA.
71. To amplify the protein-coding DNA sequence, the primers
should correspond to the first three and last three residues of the pro-
tein (each amino acid represents three nucleotides, so the primers
would each be nine bases long). Use Table 3.3 to find the codons that
correspond to the first three residues:
Met Gly Ser
AUG GGU UCU
GGC UCC
GGA UCA
GGG UCG
AGU
AGC
Using just the topmost set of codons, a possible DNA primer would
therefore have the sequence 5ʹ-ATGGGTTCT-3ʹ. This primer could
base pair with the gene’s noncoding strand, and its extension from
its 3ʹ end would yield a copy of the coding strand of the gene (see
Fig. 3.18). The other primer must correspond to the last three amino
acids of the protein:
Val Ser Pro
GUU UCU CCU
GUC UCC CCC
GUA UCA CCA
GUG UCG CCG
AGU
AGC
Again, considering just the topmost set of codons, a probable DNA
coding sequence would be 5ʹ-GTTTCTCCT-3ʹ. This sequence cannot
be used as a primer. However, a suitable primer would be the comple-
mentary sequence 5ʹ-AGGAGAAAC-3ʹ, which can then be extended
from its 3ʹ end to yield a copy of the noncoding strand of the gene.
The number of possible primer pairs is quite large, because all but
one of the amino acids has more than one codon. For the first primer,
there are 1 × 4 × 6 = 24 possibilities; for the second, 4 × 6 × 4 = 96
possibilities. There are 24 × 96 = 2304 different pairs of primers that
could be used to amplify the gene by PCR.
72. To design an oligonucleotide probe for a gene, the researcher must
apply the genetic code in reverse, that is, select codons that correspond
to the amino acids in the protein. Most amino acids can be encoded
by more than one codon, so the researcher would have to choose one
of them and hope that it matched the DNA well enough for the probe
to successfully hybridize with the DNA (see Solution 71). Met and
Trp, however, are encoded by only one codon each, so by using these
codons as part of the probe, the researcher can be assured of a perfect
match with the DNA, at least for these three nucleotides.
73. ATTGTTCCCACAGACCG
CGGCGAAGCATTGTTCC ACCGTGTTTCCGACCG
TTGTTCCCACAGACCGTG
TG C T TA G C
A C G A ATC G G C
C G G A A C G A
C T TGC T
Exonuclease
cleavage
63. a. A HaeII digest of the linear 2743-bp pGEM-3Z plasmid (see
Figure 3.16) would produce four bands, as shown below (1–323 pro-
duces a 323-bp band, 324–693 produces a 370-bp band, 694–2564
produces an 1871-bp band, and 2565–2743 produces a 179-bp band).
b. A digest of the circular plasmid produces the 370-bp band and the
1871-bp band but also produces a 502-bp band (2565–323) in place
of the 323-bp band and the 179-bp band. [From Promega.]
Linear
Circular
3000 bp
1500 bp
1000 bp
500 bp
100 bp
64.
2 kb 7 kb
Pst I
8 kb 3 kb
EcoRI Pst I
65. Polymerization occurs in the 5ʹ→3ʹ direction and a 3ʹ OH group
must be available, so the primer must be complementary to the sequence
as shown.
5ʹ-AGTCGATCCCTGATCGTACGCTACGGTAACGT-3ʹ
3ʹ-TGCCATTGCA-5ʹ
66. A restriction endonuclease is often used to prepare fragments of
DNA for insertion into a cloning vector. Since the cloned DNA con-
tains the recognition site (whose sequence is known), this sequence can
be used as a starting point to sequence the unknown DNA segment.
67. The primers are shown in red below.
5ʹ-ATGATTCGCCTCGGGGCTCCCCAGTCGCTGGTGCTGCT GACGCTGCTCGTCG-3ʹ
← 3ʹ-ACGACT GCGACGAGCAGC-5ʹ
5ʹ-ATGATTCGCCTCGGGGCT-3ʹ →
3ʹ-TACTAAGCGGAGCCCCGAGGGGTCAGCGACCACGACGACTGCGACGAGCAGC-5ʹ
68. a. The primers are shown in red below.
5ʹ-ATGGGCTCCATCGGTGCAGCAAGCATGGAA · · ·
TTCTTTGGCAGATGTGT T TCCCCTTAAAAAGAA-3ʹ
3ʹ-CAAAGGGGAATT T T TCT T-5ʹ
5ʹ-AT GGGCTCCAT CGGT GCA-3ʹ
3ʹ-TACCCGAGGTAGCCACGTCGTTCGTACCTT · · ·
AAGAAACCGTCTACACAAAGGGGAATTTTTCTT-5ʹ
b. Add the sequence recognized by the EcoRI endonuclease
(GAATTC; see Table 3.5) to the 5ʹ end of each primer. So the forward
primer (on the left) would have a sequence of 5ʹ-GAATTCATGG-
GCTCCATCGGTGCA-3ʹ and the reverse primer (on the right) would
have a sequence of 5ʹ-GAATTCTTCTTTTTAAGGGGAAAC-3ʹ.

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