biochem chpt #2

Section 2-5 31) Attractions of oppositely charged functional groups of proteins are sometimes called ________. A) salt bridges or ion pairing B) disulfide bridges C) London bridges D) hydrophilic bridges

A

Section 2-1 3) Which substance do you expect to be most soluble in water? A) Ammonia, NH3. B) Methane, CH4. C) Carbon dioxide, CO2. D) Nitrogen, N2.

A

Section 2-5 33) London dispersion forces are attractive forces that arise due to A) infinitesimal dipoles generated by the constant random motion of electrons. B) permanent dipoles of molecules containing covalent bonds between atoms of very different electronegativities. C) the hydrophobic effect. D) ion pairing between oppositely charged functional groups.

A

Section 2-1 4) Which is NOT a proper way to form a hydrogen bond? (The symbol "R" represents a general organic group. The hydrogen bonding is represented by dashed lines.) A) I B) II C) III D) IV

B

Section 2-7 43) In pure water hydronium ions are formed by ________ attack of oxygen on a proton in an adjacent water molecule. A) ionic B) nucleophilic C) electrophilic D) covalent

B

Section 2-8 53) Compare solution A with pH = 4 to solution B with pH = 6. A) The concentration of hydronium ion in solution A is twice that in solution B. B) Solution A has greater buffering capacity than solution B. C) The concentration of hydronium ion in solution A is 100 times that in solution B. D) The hydroxide concentrations are equal in the two solutions since pH only measures the concentration of H+.

C

Section 2-2 6) Which statement is true about hydrogen bonds between water molecules? A) They are about as strong as the covalent bonds in a water molecule. B) They arise because of the linear geometry of water. C) They cause water to have an unusually low freezing point for its molecular weight. D) They involve the unequal sharing of a proton between water molecules. E) In liquid water the same molecules attract to each other over long time periods.

D

Section 2-3 15) Which is true about the solubility of electrolytes in water? A) They are all insoluble in water. B) They are usually only sparingly soluble in water. C) They often form super-saturated aqueous solutions. D) They readily dissolve and ionize in water.

D

Section 2-7 44) Pure water has a concentration of A) 18 g/ml. B) 1 g/ml. C) 1000 g/ml. D) 55 M.

D

Section 2-1 2) The polarity of small molecules is a result of A) the presence of oxygen. B) the geometry of the bonds in the molecule. C) the polar covalent bonds. D) All of the above. E) B and C.

E

Section 2-9 64) For a weak acid with a pKa = 6.5, the effective buffering range is usually considered to be A) pH 6 to pH 7. B) pH 6.4 to pH 6.6. C) pH 5.5 to pH 7.5. D) dependent on the molarity of the acid. E) B and C.

C

Section 2-5 34) The aggregation of nonpolar molecules or groups in water is thermodynamically due to the A) increased entropy of the nonpolar molecules when they associate. B) decreased enthalpy of the system. C) increased entropy of the water molecules. D) very strong van der Waals forces among the nonpolar molecules or groups.

C

Section 2-10

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Section 2-10 63) Since HCl is a strong acid its value of Ka is ________. A) effectively equal to infinity B) equal to Kw C) zero D) dependent on the concentration of HCl

A

Section 2-10 68) pKa values of phosphoric acid are 2.2, 7.2 and 12.7. A phosphate buffer of pH = 7.4 can be prepared using A) H2PO4- and HPO42-. B) HPO42- and PO43-. C) H3PO4 and HCl. D) None of the above.

A

Section 2-2 8) Compounds that ionize when dissolved in water are called ________. A) electrolytes B) polar compounds C) hydrophobic compounds D) amphipathic compounds

A

Section 2-3 16) What is the difference between a particle being hydrated versus being solvated? A) A hydrated particle is surrounded by a shell of water. A solvated molecule is surrounded by a shell of solvent molecules, not necessarily water. B) The terms hydrated and solvated mean exactly the same thing. C) A hydrated particle has reacted with hydrogen. A solvated particle is dissolved in a solvent. D) The word hydrated is used only when the solute is an electrolyte.

A

Section 2-3 12) Which would you expect to be most soluble in water? A) I B) II C) III D) IV

A

Section 2-4 22) Molecules that are both hydrophobic and hydrophilic are ________. A) amphipathic B) amphoteric C) bipolar D) not possible

A

Section 2-5 28) Which of these noncovalent forces in biological systems is usually the strongest? A) Hydrogen bonds. B) London dispersion forces. C) Hydrophobic interactions. D) Van der Waals forces.

A

Section 2-5 35) Water molecules clustered about nonpolar molecules contribute to hydrophobic interactions because A) their number is minimized to increase the total entropy of water. B) nonpolar molecules are more highly organized than polar molecules. C) water molecules in the cell are more organized in the regions away from the nonpolar molecule. D) All of the above. E) B and C.

A

Section 2-7 41) Which parameter has the greatest correlation to reaction rate? A) Activation energy. B) Gibb's free energy. C) Enthalpy. D) Entropy. E) None of the above.

A

Section 2-7 48) How does the ion-product of water, Kw, relate to the equilibrium constant, Keq, for the dissociation reaction of water? A) Kw is found by multiplying Keq by the concentration of water. B) Kw just another symbol for Keq , so they are equal. C) Kw is found by dividing Keq by the ideal gas constant. D) Kw is found by multiplying Keq by the concentrations of hydronium ion and hydroxide ion.

A

Section 2-7 45) Which statement best characterizes the distribution of charge in the hydronium ion, H3O+? A) The positive charge is distributed over all of the atoms in the ion. B) The positive charge is localized only on the oxygen atom. C) The positive charge is distributed between the three hydrogen atoms only. D) The positive charge is localized on only one of the hydrogen atoms.

A

Section 2-8 50) In pure water, the concentration of H+ plus equals A) 1 × 10-7 M. B) 1 × 10-14 M. C) 1 M. D) .07 M.

A

Section 2-9 56) Two weak acids, A and B, have pKa values of 4 and 6, respectively. Which statement is true? A) Acid A dissociates to a greater extent in water than acid B. B) For solutions of equal concentration, acid B will have a lower pH. C) B is the conjugate base of A. D) Acid A is more likely to be a polyprotic acid than acid B. E) The equivalence point of acid A is higher than that of acid B.

A

Section 2-9 58) What is the approximate pH of a 0.10 M solution of a weak acid that has a Ka of 5 × 10-5 M? A) 2.7 B) 5.3 C) 4.8 D) 11.3 E) Cannot determine from the information given.

A

Section 2-5 37) The oxygen atom of water is nucleophilic because A) it has a negative oxidation number. B) it carries a partial positive charge. C) it has two unshared pair of electrons. D) it seeks electron-rich molecules. E) All of the above.

C

Section 2-10 65) Blood pH is primarily regulated by A) a protein buffer system. B) the carbon dioxide - carbonic acid - bicarbonate buffer system. C) the phosphate buffering system. D) carbonic acid (H2CO3). E) B and C.

B

Section 2-10 69) Acetic acid has a pKa of 4.8. How many milliliters of 0.2 M acetic acid and 0.2 M sodium acetate are required to prepare 1 liter of 0.1 M buffer solution having a pH of 4.8? A) 500 ml acetic acid and 500 ml sodium acetate. B) 250 ml acetic acid and 250 ml sodium acetate, then 500 ml water. C) 250 ml acetic acid and 500 ml sodium acetate, then 250 ml water. D) 500 ml acetic acid and 250 ml sodium acetate, then 250 ml water.

B

Section 2-3 11) A molecule or ion is said to be hydrated when it ________. A) is neutralized by water B) is surrounded by water molecules C) reacts and forms a covalent bond to water D) aggregates with other molecules or ions to form a micelle in water

B

Section 2-3 17) The osmotic pressure of an aqueous solution depends on A) the chemical nature of the solute. B) the molar concentration of solute. C) the hydrophobic effect of the solute. D) All of the above. E) None of the above.

B

Section 2-4 21) Micelles, formed by detergents in water, have A) hydrophilic interiors and hydrophobic exteriors. B) hydrophobic interiors and hydrophilic exteriors. C) hydrophilic interiors and exteriors. D) hydrophobic interiors and exteriors. E) None of the above.

B

Section 2-4 24) Which statement explains the cleaning action of soap on greasy dishes? A) The soap changes the water-solubility of the grease so that it is easily dissolved by the water. B) The grease is trapped inside the hydrophobic interior of micelles made of soap molecules. C) The soap chemically breaks down the grease into smaller, more water-soluble molecules. D) The soap hydrates the grease with its polar head groups and holds it in suspension.

B

Section 2-5 36) The three dimensional structure of most proteins is largely determined by A) other proteins which fold them. B) weak noncovalent interactions. C) denaturation. D) hydrogen bonds. E) All of the above.

B

Section 2-5 30) Which statement is true about the ability of carbon to participate in hydrogen bonds in living organisms? A) There are too many carbon atoms competing for the hydrogens in biomolecules to allow for the stable formation of hydrogen bonds. B) Carbon's electronegativity is too low to participate in hydrogen bonding. C) Most carbons in biomolecules are hydrogen bonded to water. D) Carbon is too large to participate in hydrogen bonding.

B

Section 2-6 39) Enzymes which condense subunits of macromolecules during their synthesis usually A) transfer an acyl or carbonyl group to an electrophile. B) exclude water from the active site. C) contain inhibitors of hydrolases. D) are catalyzing thermodynamically favored reactions. E) All of the above.

B

Section 2-7 47) The self-ionization of water is ________. A) a unimolecular dissociation of a single water molecule to H+ and OH- B) a biomolecular reaction between two water molecules to yield H3O+ and OH- C) a result of hydrophobic interactions D) a termolecular reaction involving the simultaneous collision of H2O, H+ and OH-

B

Section 2-8 51) Basic solutions form when chemicals are dissolved in water and remove A) OH-. B) H+. C) Na+. D) A and B. E) A, B and C.

B

Section 2-9 57) Calculate the value of pKa for an acid when Ka = 2.6 × 10-4. A) -3.59 B) +3.59 C) -8.25 D) +8.25 E) +3800

B

Section 2-9 61) A titration curve for a weak acid is shown. Which point shows the most buffering? A) A B) B C) C D) D E) E

B

Section 2-6 40) The ion-product constant for water, Kw, is A) 1 × 10-7 M2. B) 1 × 10-7 M. C) 1 × 10-14 M2. D) 1 × 10-14 M.

C

1) Which statement does NOT explain the polarity of water? A) Oxygen is more electronegative than hydrogen. B) Water molecules have a bent geometry (V-shaped). C) The oxygen in water has sp2 hybrid orbitals. D) In water the hydrogen carries a partial positive charge (δ+).

C

Section 2-10 66) The pKa of lactic acid is 3.9. A lactate buffer will be useful from pH values A) 3.5 through 4.4. B) 3.0 through 4.5. C) 2.9 through 4.9. D) 3.8 through 4.0.

C

Section 2-2 7) The abundance of water in the cells and tissues helps to minimize temperature fluctuations. This is due to what property of water? A) Density. B) Viscosity. C) Specific heat. D) Boiling point.

C

Section 2-3 13) Solutes diffuse more slowly in cytoplasm than in water because of A) the higher viscosity of water. B) the higher heat of vaporization of water. C) the presence of many crowded molecules in the cytoplasm. D) the absence of charged molecules inside cells.

C

Section 2-3 14) The ________ pressure is the pressure required to prevent the flow of solvent through a solvent-permeable membrane that separates two solutions of different solute concentration. A) hydrostatic B) electromotive C) osmotic D) partial

C

Section 2-3 19) The osmotic pressure of a 0.010 M sucrose (C12H22O11) solution at 25°C is 0.24 atm. How does the osmotic pressure of a 0.010 M glucose (C6H12O6) solution at 25°C compare to this? Note that neither solute is volatile or ionizable. A) The glucose solution has a lower osmotic pressure because its molar mass is lower than sucrose. B) The glucose solution has a higher osmotic pressure because its molar mass is lower than sucrose. C) The osmotic pressures are equal because the solutions have the same molar concentration. D) Nothing can be said about the osmotic pressure of the glucose solution without more information.

C

Section 2-3 9) Poorly soluble molecules such as lipids and nucleoside bases can be made more soluble in cells by attaching ________ to them. A) water B) oxygen C) carbohydrates D) salt ions

C

Section 2-4 23) Which molecule or ion below is amphipathic? A) H2NCH2COOH (glycine) B) H2O C) CH3(CH2)14COO- D) CH3CH2CH2CH2CH3

C

Section 2-4 26) Which of the following is NOT a "weak" interaction? A) Hydrogen bonds B) Van der Waals forces. C) Disulfide bonds. D) Ionic interactions. E) Hydrophobic interactions.

C

Section 2-5 27) Which of the following weak interactions is NOT an electrostatic interaction? A) Hydrogen bonds. B) Charge-charge interactions. C) Hydrophobic interactions. D) Van der Waals forces.

C

Section 2-8 52) The pH of a 10-4 M solution of HCl is A) 3. B) 3.5. C) 4. D) 4.5. E) greater than 4.5.

C

Section 2-10 67) Intracellular buffers include A) proteins. B) inorganic phosphate. C) cellulose. D) Both A and B. E) A, B and C.

D

Section 2-10 70) The pH of human blood is primarily maintained at 7.4 by A) ATP. B) carbon dioxide-carbonic acid buffer systems. C) a bicarbonate buffer system. D) B and C. E) A, B and C.

D

Section 2-2 5) What is the maximum number of hydrogen bonds that one water molecule can have with neighboring water molecules? A) 1 B) 2 C) 3 D) 4

D

Section 2-3 20) Oil and water do not form a solution due to ________. A) the hydrophobic effect B) the inability of oil to hydrogen bond with water C) the nonpolarity of oil D) All of the above. E) A and C only.

D

Section 2-4 25) Some ions such as thiocyanate that are poorly solvated in water and can enhance the solubility of nonpolar compounds in water by disordering the water molecules are called ________. A) azeotropes B) hydrophobic ions C) zeolytes D) chaotropes

D

Section 2-5 29) Hydrogen bonds can occur when hydrogen is covalently bonded to atoms like nitrogen and oxygen. What property of nitrogen and oxygen is important for this? A) Atomic mass. B) Ionizability. C) Hydrophobicity. D) Electronegativity.

D

Section 2-5 32) Which is true about hydrogen bonding for biological molecules? A) Hydrogen bonds are strong enough to confer structural stability, for example in DNA. B) Hydrogen bonds are weak enough to be easily broken (weaker than covalent bonds). C) They contribute to the water solubility of many macromolecules. D) All of the above.

D

Section 2-6 38) Water is a nucleophile, yet it does not usually hydrolyze macromolecules in cells because A) covalent bonds linking macromolecule subunits are stable at cell pH. B) covalent bonds linking macromolecule subunits are stable at cell temperature. C) the concentration of water is much too small in cells. D) A and B.

D

Section 2-7 49) A solution containing 10-8 M HCl and 10-8 M acetic acid contains H+ which is supplied mostly by A) the strong acid. B) the weak acid. C) both the strong and the weak acids. D) water. E) All of the above.

D

Section 2-7 42) What is the concentration of hydroxide ion in an aqueous solution with an H+ concentration of 2 × 10-5 M? A) 2 × 109 M B) 2 × 10-19 M C) 2 × 10-19 M D) 5 × 10-10 M E) Cannot calculate from the information given.

D

Section 2-7 46) Which statement below is true about the relative lifetime of a hydrogen bond, compared to the rate of water's ionization to hydroxide ions and hydronium ions? A) The strength of hydrogen bonding makes its dissociation much slower than the ionization of water. B) The rate of dissociation of a hydrogen bond is the same order of magnitude as the rate of ionization of water. C) The two rates are linked in such a way that the more the water is ionized, the stronger and longer lasting hydrogen bonding will be. D) The lifetime of a water molecule before it is ionized is about 109 greater than the lifetime of a hydrogen bond.

D

Section 2-8 54) If human blood is not maintained at close to pH = 7.4, a person can develop A) acidosis. B) alkalosis. C) diabetes. D) Both A and B. E) None of the above.

D

Section 2-8 55) The Henderson-Hasselbalch equation can be used to calculate A) the pH of a solution of an organic acid. B) the amount of salt and acid to add to form a specific buffer. C) the pKa of a weak acid. D) All of the above. E) A and C only.

D

Section 2-9 62) The imidazolium ion has a pKa = 7.0. Imidazolium buffers can be prepared for pH values of A) 6.5 to 7.5. B) 6.1 to 7.1. C) 5.5 to 8.5. D) 6.0 to 8.0. E) 6.0 to 7.5.

D

Section 2-9 60) At the midpoint of a titration curve A) the concentration of a conjugate base is equal to the concentration of a conjugate acid. B) the pH equals the pKa. C) the ability of the solution to buffer is best. D) All of the above. E) A and B only.

D

Section 2-3 10) Electrolytes dissolve readily in water because A) they are held together by electrostatic forces. B) they are hydrophobic. C) water molecules can cluster about cations. D) water molecules can cluster about anions. E) water molecules can cluster about cations and anions.

E

Section 2-3 18) Cells keep the osmotic pressure from being too great by A) existing in hypertonic solutions. B) making macromolecules from smaller molecules. C) existing in a hypotonic solution. D) existing in an isotonic solution. E) Both B and D.

E

Section 2-9 59) The ratio of the concentration of a ________ over ________ describes the proportions of forms of a weak acid necessary to satisfy the Henderson-Hasselbalch equation. A) conjugate acid; conjugate base B) conjugate base; conjugate acid C) proton donor; proton acceptor D) proton acceptor; proton donor E) B and D

E