Biochemistry Ch 2
The pH of a solution of 0.04 M HCl is: a. 4 b. 1.4 c. 0.4 d. 0.04 e. The pH cannot be determined
b. 1.4
If the pH of 1 liter of a 1.0 M carbonate buffer is 7.0, what is the molar ratio of H2CO3 to HCO3−? (pK = 6.37) a. 0.234 b. 4.27 c. 6.37 d. 7.00 e. 10.20
b. 4.27
The dissociation constant for an acid is 1 × 10− 6 . What is its pKa? a. −6 b. 6 c. 0.6 d. −0.6
b. 6
Using the Henderson-Hasselbalch equation, calculate the pH of an ammonia buffer when the NH3:NH4 + ratio is 0.4 moles:0.6 moles. (pK = 9.75) a. 7.40 b. 9.07 c. 9.25 d. 9.43 e. 11.05
b. 9.07
Which has the greater Ka, a weak acid or a strong acid? a. A weak acid. b. A strong acid c. They should dissociate about the same. d. It's impossible to predict
b. A strong acid
Which will dissociate most in water, a weak acid or a strong acid? a. A weak acid. b. A strong acid c. They should dissociate about the same. d. It's impossible to predict.
b. A strong acid
Which of the following molecules has polar bonds but is itself not polar? a. NH3 b. CO2 c. CH4 d. H2O
b. CO2
Which of the following classes of compounds is hydrophobic? a. Table Salt b. Cholesterol c. Phosphate esters d. Cholesterol and phosphate esters. e. All of these are hydrophobic
b. Cholesterol
The main intracellular buffer system is a. H3PO4/H2PO4− b. H2PO4−/ HPO4 2− c. HPO4 2− /PO4 3− d. H3PO4/PO4 3−
b. H2PO4−/ HPO4 2−
Which of the following equations represents the relationship between the pKa of an acid and the pH of a solution containing the acid and its conjugate base? a. Arrhenius equation b. Henderson-Hasselbalch equation c. Nernst equation d. Butler-Volmer equation
b. Henderson-Hasselbalch equation
The dissociation constant for an acid with a pKa value of 6.0 is a. 1 × 10− 6 b. −1 × 10 6 c. 1 × 106 d. −1 × 10− 6
a. 1 × 10− 6
The ratio of a weak acid and its conjugate base at the point of maximum buffering capacity is a. 1/1 b. 1/10 c. 10/1 d. no definite ratio is needed
a. 1/1
What is the pH of an acetic acid solution where the concentration of acetic acid is 2 mM and the concentration of sodium acetate is 20 mM. The pKa of acetic acid is 4.76. a. 5.76 b. 10.6 c. 12.6 d. 8.8
a. 5.76
An ammonia buffer contains NH3:NH4 + in a ratio of 0.4 moles:0.6 moles (pK = 9.75). What will be the pH if you add 0.01 moles of HCl to this buffer? a. 8.98 b. 9.04 c. 9.25 d. 9.46 e. 9.52
a. 8.98
Which of the following is not true? a. A buffer is a solution which maintains a solution at a neutral pH b. Buffer solutions are made to resist change in pH c. Zwitterion buffers are less likely to interfere with biological reactions than non-zwitterions d. HEPES is a zwitterion buffer
a. A buffer is a solution which maintains a solution at a neutral pH
Which has the greater pKa, a weak acid or a strong acid? a. A weak acid. b. A strong acid c. They should dissociate about the same. d. It's impossible to predict.
a. A weak acid.
The enzyme lysozyme has an optimum pH close to 5. A suitable buffer would be: a. Acetate b. Carbonate c. Phosphate d. Pyruvate e. None of these is a suitable buffer for this reaction.
a. Acetate
Which of the following molecules will not form hydrogen bonds? a. CH4 b. NH3 c. H2O d. HF
a. CH4
The main blood buffer system is a. H2CO3/HCO3− b. HCO3−/CO3 2− c. H2CO3/CO3 2− d. none of the above
a. H2CO3/HCO3−
Which of the following statements about hydrogen bonds is false? a. The donor is a hydrogen atom bonded to a less electronegative atom then hydrogen. b. The more linear the bond, the stronger the attraction. c. The acceptor must contain a non-bonded pair of electrons. d. It is a type of non-covalent bond.
a. The donor is a hydrogen atom bonded to a less electronegative atom then hydrogen.
Which of the following is true? a. The pH of a solution where the A− to HA ratio is 1 has a pH = pKa. b. If the pH does not equal the pKa, the solution is not a buffer. c. The best buffer for any experiment will always have a pH equal to the pKa. d. If a buffer has more weak acid than conjugate base, the pH will be higher than the pKa.
a. The pH of a solution where the A− to HA ratio is 1 has a pH = pKa.
How do hydrogen bonds tend to affect the melting and boiling points of substances? a. They tend to increase both melting and boiling points. b. They tend to decrease both melting and boiling points. c. They tend to increase melting points and decrease boiling points. d. They tend to decrease melting points and increase boiling points. e. They do not have any affect on either melting or boiling points.
a. They tend to increase both melting and boiling points.
Hydrogen bonds can only form when the hydrogen atom is involved in a polar bond. a. True b. False
a. True
The inflection point of the titration curve for a weak monoprotic acid is equal to its pKa a. True b. False
a. True
For an acid that undergoes this reaction: HA ↔ H + + A− Ka = a. [H+ ][A−]/[HA] b. [H+ ][HA]/[A−] c. [HA][A−]/[H+ ] d. [A−]/[HA][H+ ] e. [H+ ]/[HA][A−]
a. [H+ ][A−]/[HA]
Which of the following characteristics makes for a good hydrogen bond donor? a. a high electronegativity b. a nonbonding pair of electrons c. both of the above d. neither of the above
a. a high electronegativity
Consider a reaction that produces a significant amount of hydrogen ion and is to be carried out a pH 7. Only two acids are available for making the buffer solution. The pKa values for acids A and B are 6.3 and 7.3, respectively. Which acid would serve as the optimum buffer for this reaction? Or would carrying out the reaction in water simply serve as well? a. acid A b. acid B c. water d. both acids would be equally effective
a. acid A
A hydrogen bond is a special type of a. dipole - dipole bond b. induced dipole - induced dipole bond c. covalent bond d. ionic bond
a. dipole - dipole bond
A London dispersion force is another name for a(n) a. induced dipole - induced dipole bond b. ionic bond c. covalent bond d. non-polar bond
a. induced dipole - induced dipole bond
Ionic compounds and polar covalent compounds tend to dissolve in water because of a. ion-dipole and dipole-dipole interactions b. dipole-induced dipole interactions c. van der Waals bonds d. hydrophobic interactions
a. ion-dipole and dipole-dipole interactions
A buffer solution a. is used to control the pH of a solution b. contains at least 100 times more of a weak acid than its conjugate base c. contains at least 100 times less of a weak acid than its conjugate base d. always has a pH of 7
a. is used to control the pH of a solution
Hydrogen bonds a. play an important role in the solvent properties of water b. are not involved in protein structure c. play a role in the properties of DNA, but not of RNA d. give water a lower boiling point than expected
a. play an important role in the solvent properties of water
If atoms with greatly differing electronegativities form a bond, that bond will be a. polar. b. nonpolar. c. amphipathic. d. acidic.
a. polar.
Buffers work to maintain pH because a. they obey LeChatlier's principle b. weak acids cannot change the pH of a solution c. weak bases added to strong bases neutralize each other d. they destroy the hydrogen ion that is added
a. they obey LeChatlier's principle
In a hydrogen bond a. three atoms lie in a straight line b. there is stronger bonding than in a covalent bond c. unpaired electrons play no role d. none of the above
a. three atoms lie in a straight line
A buffer solution at pH 10 has a ratio of [HA]/[A−] of 10. What is the pKa of the acid? a. 8 b. 9 c. 10 d. 11 e. 12
d. 11
If a solution has a pH = 9.6, the [H+ ] is a. 2.5 × 10^10 b. 9.6 M c. 2.5 M d. 2.5 × 10− 10 M e. 9.6 × 10− 10 M
d. 2.5 × 10− 10 M
What is the maximum number of hydrogen bonds a single water molecule can form? a. 1 b. 2 c. 3 d. 4 e. 5
d. 4
Calculate the final pH of a solution made by the addition of 10 mL of a 0.5 M NaOH solution to 500 mL of a 0.4 M HA originally at pH = 5.0 (pKa = 5.0) Neglect the volume change. a. 6.10 b. 5.09 c. 7.00 d. 5.55
d. 5.55
Buffers which lack biological activity and are unlikely to interfere with any biochemical reactions include: a. Tris. b. Hepes. c. Phosphate. d. Both Tris and HEPES. e. All of these
d. Both Tris and HEPES.
If the pH of 1 liter of a 1.0 M carbonate buffer is 7.0, what is actual number of moles of H2CO3 and HCO3−? (pK = 6.37) moles of H2CO3 moles of HCO3− I. 0.86 0.14 II. 0.81 0.19 III. 0.76 0.24 IV. 0.19 0.81 V. 0.14 0.86 a. I b. II c. III d. IV e. V
d. IV
Which of the following acids would serve as a good buffer for a reaction at pH = 8.0? K a I. acetic acid 1.76 × 10− 5 II. H2PO4− 6.31 × 10− 8 III. bicarbonate 5.6 × 10− 11 IV. TRIS 5.01 × 10− 9 a. I b. II c. III d. IV
d. IV
Which of the following principles states that if stress is applied to a system in equilibrium, the equilibrium will shift in the direction that relieves the stress? a. Pauli exclusion principle b. Mach's principle c. Fermat's principle d. Le Chatelier's principle
d. Le Chatelier's principle
Which of the following molecules is polar? a. CCl4 b. CH4 c. CO2 d. NH3 e. None of these molecules is polar
d. NH3
Which of the following elements has the highest electronegativity? a. C b. H c. N d. O e. P
d. O
Which of the following compounds is most likely to form a micelle? a. Acetic acid. b. Glucose. c. Glycerol. d. Sodium palmitate. e. Sodium phosphate.
d. Sodium palmitate.
Which of the following is true about ionic compounds? a. They are more likely to dissolve in non-polar solvents than covalent compounds. b. They always dissolve completely in water. c. They never dissolve in polar solvents. d. Some of them dissolve completely in water or other polar solvents, while others do not
d. Some of them dissolve completely in water or other polar solvents, while others do not
Which of the following classes of compounds is hydrophilic? a. Sugars b. Fatty acids c. Amino acids d. Sugars and amino acids. e. All of these
d. Sugars and amino acids
Which of the following is true regarding hydrogen bonds. a. They can only form between two different molecules b. They are important in protein folding but not DNA structure c. They are important in DNA structure but not protein folding d. They can be found within a single molecule
d. They can be found within a single molecule
Many of the properties of water can be accounted for by the fact that a. it is polar b. it forms hydrogen bonds c. it is a bent molecule d. all of these are true
d. all of these are true
Which of the following is a true statement? a. most substances contract when they freeze. b. water expands when it freezes. c. hydrogen bonding is related to water's tendency to expand as it freezes. d. all of these are true
d. all of these are true
Which of the following properties of water are related to its ability to form hydrogen bonds? a. boiling point b. melting point c. density d. solvent potency e. all of the choices
e. all of the choices
Which of the following is important to know when deciding if a given buffer will be effective for an experiment? a. the pKa of the buffer compound b. the buffer capacity c. the concentration of the buffer d. whether the experiment is likely to generate hydrogen ions or hydroxide ions e. all of these are important considerations
e. all of these are important considerations
How does the strength of hydrogen bonds compare with covalent bonds? a. Hydrogen bonds are much stronger than covalent bonds. b. Hydrogen bonds are much weaker than covalent bonds. c. Hydrogen bonds and covalent bonds have similar strengths. d. The question cannot be answered without knowing which covalent bonds are being referred to
b. Hydrogen bonds are much weaker than covalent bonds.
Refer to Exhibit 2A. Which of the functional groups cannot function as a hydrogen donor to water? a. I b. II c. III d. IV e. All can donate a hydrogen to water
b. II
Explain why carbon dioxide is nonpolar.
A carbon dioxide molecule has two C=O polar bonds. However, the bonds in the molecule may be polar, but the molecule itself can be nonpolar because of its geometry. The CO2 molecule is linear; therefore, the attraction of the oxygen for the electrons in one bond is cancelled out by the equal and opposite attraction for the electrons by the oxygen on the other side of the molecule, resulting in a nonpolar molecule.
Distinguish between the hydrogen bonding found in liquid water and ice.
In liquid water, hydrogen bonds are constantly breaking and new ones are constantly forming, with some molecules breaking off and others joining the cluster. An ice crystal, in contrast, has a more or less stable arrangement of hydrogen bonds and its number of molecules is many orders of magnitude greater than 100.
Which of the following statements is true of dipole-induced dipole interactions? a. They occur between molecules that are dipoles, with the partial positive side of one molecule attracting the partial negative side of another molecule. b. They involve a permanent dipole inducing a transient dipole in a nonpolar molecule. c. They are the attraction between two molecules, lacking dipoles, bumping into each other and distorting each other's electron cloud. d. They give rise to a London dispersion force between transient-induced dipoles.
b. They involve a permanent dipole inducing a transient dipole in a nonpolar molecule.
The tendency for an atom to attract electrons to itself in a chemical bond is called a. polarity. b. electronegativity. c. hydrophilicity d. electrophilicity.
b. electronegativity.
Which substance would be the best buffer at pH 8 if it had to be able to buffer against either acid or base? a. one with a pKa of 7 b. one with a pKa of 8 c. one with a pKa of 9 d. The pKa of a substance doesn't tell you whether it would be a good buffer at this pH.
b. one with a pKa of 8
Bases are a. proton donors. b. proton acceptors. c. hydrogen bond donors. d. hydrogen bond acceptors
b. proton acceptors.
The substance most likely to form a micelle is a. acetic acid b. sodium palmitate c. methyl alcohol d. acetone
b. sodium palmitate
Buffering capacity refers to a. the effectiveness of commercial antacids b. the extent to which a buffer solution can counteract the effect of added acid or base c. the pH of a buffer solution d. the molecular weight of the substance used as a buffer
b. the extent to which a buffer solution can counteract the effect of added acid or base
If a solution has a pH = 6, the [H+ ] is a. 6 M b. 10^6 M c. 10 −6 M d. 0.6 M
c. 10 −6 M
The pOH a solution of 0.04 M HCl is: a. 1.4 b. 10 c. 12.6 d. 13.6 e. The pOH cannot be determined
c. 12.6
What is the pH of a solution with [H+] = 10 mM? a. 10 b. 1 c. 2 d. −2
c. 2
A solution at pH 7 contains a weak acid, HA. The pKa of the acid is 6.5. What is the ratio of [A−]:[HA]? a. 1:3 b. 1:1 c. 3:1 d. 10:1
c. 3:1
An ammonium buffer would work well at this pH: a. 5.6 b. 7.0 c. 9.0 d. 11.0 e. None of these
c. 9.0
True hydrogen bonds can NOT form between hydrogen and this element: a. N b. F c. C d. O e. All of these elements can form hydrogen bonds.
c. C
Which of the following is a correct listing of electronegativity values, from low to high? a. C, H, O, N b. N, H, O, C c. H, C, N, O d. H, C, O, N
c. H, C, N, O
Refer to Exhibit 2A. Which of the functional groups is the most electrophilic? a. I b. II c. III d. IV e. The answer cannot be determined without further information.
c. III
Is water an acid or a base? a. Water is an acid. b. Water is a base. c. Water is both an acid and a base. d. Water is neither an acid nor a base.
c. Water is both an acid and a base.
When does a weak acid buffer best? a. From one pH unit below its pKa to its pKa. b. From its pKa to one pH unit above its pKa. c. Within one pH unit of its pKa, both above and below. d. Weak acids do not make good buffers at all.
c. Within one pH unit of its pKa, both above and below.
Which of the following characteristics makes for a good hydrogen bond acceptor? a. a high electronegativity b. a nonbonding pair of electrons c. both of these d. neither of these
c. both of these
The non-covalent interaction below associated with the strongest force in aqueous solution is a. dipole-induced dipole b. hydrophobic interactions c. hydrogen bonding d. van der Waals forces
c. hydrogen bonding
In a titration of a weak acid by a strong base a. two equivalents of base are always needed to neutralize all the acid present b. the equivalence point cannot be defined exactly c. there is a region in which the pH changes slowly d. the equivalence point depends on the nature of the added base
c. there is a region in which the pH changes slowly
Nonphysiological buffers such as HEPES and PIPES have come into common use because a. they are inexpensive b. they can be prepared much more easily than other buffers c. they have less tendency to interfere with reactions d. they contain nitrogen
c. they have less tendency to interfere with reactions
A micelle is a structure which a. aggregates with other micelles in water. b. has its polar groups on the outside and non-polar groups on the inside when in water. c. explains how soaps and detergents work. d. has its polar groups on the outside and non-polar groups on the inside when in water and explains how soaps and detergents work. e. All of these are true
d. has its polar groups on the outside and non-polar groups on the inside when in water and explains how soaps and detergents work.
Which of the following is not considered a van der Waal's force? a. dipole - dipole bond b. dipole - induced dipole bond c. induced dipole - induced dipole bond d. ion - dipole bond
d. ion - dipole bond
Which of the following molecules is amphipathic? a. sodium chloride b. acetic acid c. benzene d. palmitic acid
d. palmitic acid
When a carboxylate side-chain of one amino acid in a protein is in close proximity to a charged amino group of another amino acid, we call the resulting interaction a(n) a. ion - dipole bond b. ionic bond c. van der Waal's bond d. salt bridge
d. salt bridge
The ion product constant for water (Kw) is equal to: a. 10^14 b. 10^7 c. 100 d. 10− 7 e. 10− 14
e. 10 −14
An HCl solution has a pH = 3. If you dilute 10 mL of the solution to 1000mL, the final pH will be: a. 1.0 b. 2.0 c. The pH does not change. d. 4.0 e. 5.0
e. 5.0
A carbonate buffer would work well at this pH: a. 4.0 b. 6.0 c. 8.0 d. 10.0 e. 6.0 and 10.0
e. 6.0 and 10.0
A phosphate buffer would work well at this pH: a. 5.0 b. 7.0 c. 8.0 d. 10.0 e. 7.0 and 8.0
e. 7.0 and 8.0
Refer to Exhibit 2A. Which of the groups could not act as a proton acceptor in a hydrogen bond? a. I b. II c. III d. IV e. All can accept a hydrogen in a hydrogen bond
e. All can accept a hydrogen in a hydrogen bond
Molecules which contain both hydrophilic and hydrophobic regions are: a. Amphipathic b. Amphiphilic c. Able to form micelles d. Both amphipathic and amphiphilic e. All of these
e. All of these
The water molecule is polar because: a. Electrons are not distributed symmetrically in the molecule. b. The hydrogen atoms are found on one "side" of the molecule. c. Hydrogen is less electronegative than oxygen. d. The hydrogen atoms are found on one "side" of the molecule and hydrogen is less electronegative than oxygen. e. All of these are correct
e. All of these are correct
Hydrogen bonds explain which of the following properties of water? a. Water is a great solvent for all ionic and polar molecules. b. Water has high melting and boiling points for its small size. c. Ice expands when frozen. d. Both the abnormal melting and freezing points and that ice expands when frozen. e. Hydrogen bonds explain all of these properties
e. Hydrogen bonds explain all of these properties
Which of the following would make the best buffer at pH =10.0? a. Acetic acid and sodium acetate b. Tris and its acid form c. H2CO3 and NaHCO3 d. Na2HPO4 and NaH2PO4 e. NaHCO3 and Na2CO3
e. NaHCO3 and Na2CO3
