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Practice Test
: Biochemistry Chapter 2
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what ability is crucial to the understanding of water's properties
phosphate system
examples of amphiphilic molecules
carbonic anhydrase
what are some of the unexpected properties of water?
Amount of H3O+ or OH- in 1 L of pure H2O at 25ºC is
what is water's structure in liquid
Buffer the intracellular fluid of cells at physiological pH because pK2 likes near pH value. Phosphate abundant anion in cells in both inorganic form and functional group
Salts of fatty acids: carboxylate functional group hydrates, long hydrophobic tails insoluble.
1 x 10^-7 mol
hydrogen bonds
Enzyme that mediates hydration of CO2. Facilitates the equilibrium by rapidly catalyzing the reaction H2O + CO2(d) H2CO3
Disorderly bonded network. Many (at least half) of H bonds in liquid are in nonideal orientations. This makes liquid lack the structured order of ice. Each molecule connected to every other in fluid network of H bonds. Strain because of nonideal hydrogen bonds in liquid state. Creates kinetic situation in which H2O molecules can switch H-bond allegiances, creating fluidity
High boiling point, melting point, heat of vaporization and surface tension.
Short Answer
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buffers
what ways do cells prevent losing or gaining fluid through osmosis
describe water and nonpolar solvents
weak electrolytes
what are some examples of strong electrolytes
Multiple Choice
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Bicarbonate Buffer System of Blood Plasma
The ability of a substance to surround ions in dipole interactions and diminish their attraction for each other. D. What ionization in solution depends on.
Three dissociable H+ lost in discrete steps, each dissociation showing a characteristic pKa
Disorderly bonded network. Many (at least half) of H bonds in liquid are in nonideal orientations. This makes liquid lack the structured order of ice. Each molecule connected to every other in fluid network of H bonds. Strain because of nonideal hydrogen bonds in liquid state. Creates kinetic situation in which H2O molecules can switch H-bond allegiances, creating fluidity
Concentration of H2CO3 maintained through equilibrium with dissolved CO2, produced in tissues and available as gaseous in the lungs. Buffers concentration of H2CO3. Overall buffer system: CO2(d) + H2O H2CO3. H2CO3 H+ + HCO3 -. Where Kh = equilibrium constant for hydration of CO2 and Ka = first acid dissociation constant for H2CO3.
Another name for Ka. States the extent to which a substance forms ions in water.
describe water's dielectric constant
Buffer system of blood plasma. H2CO3 H+ + HCO3 -. Concentration of H2CO3 small fraction of HCO3 - concentration, because pKa1 is 3.77.
Region of pKa, pH remains relatively unaffected as increments of OH- (or H+) are added. Acts as a buffer.
Water has high D. Attractions between H2O and ions is stronger than between ions.
pH = pKa + log [A-]/[HA]. pH of a solution can be calculated, provided Ka and the concentrations of the weak acid HA and its conjugate base A- are known. Provides a general solution to the quantitative treatment of acid-base equilibria in biological systems.
Three dissociable H+ lost in discrete steps, each dissociation showing a characteristic pKa
titration curve for polyprotic acid
Three dissociable H+ lost in discrete steps, each dissociation showing a characteristic pKa
= pH + pOH = 14
F = e1e2/Dr^2 where F is force, r is distance and e1 and e2 are the charges of the two ions.
Breathing rate more rapid than necessary for normal CO2 elimination from the body. Can result in inappropriately low [CO2(g)] in the blood. Causing blood pH to rise
negative log of the hydrogen ion concentration pH = -log [H+] pH scale: Based on negative logarithms, low pH values represent high H+ concentrations.
Overall equilibrium constant for ionization of H2CO3 in equilibrium with CO2(d)
= pH + pOH = 14
Analytical method used to determine the amount of acid in a solution. Experimental method of determining pKa values of weak electrolytes: Where half the HAc has been neutralized, concentrations of HAc and Ac- are equal and pH = pKa for HAc.
H-bonded water network rearranged toward formation of a local cage structure surrounding each solute molecule. Accompanied by significant ordering (negative entropy). H2O next to solvent have limited structural options. Straddle nonpolar solute so two of three H-bonding vectors available (tangential to solute). Allows H2O to retain H-bonding possibilities because no H-bond acceptor/donator directed towards solute.
KaKh = [H+][HCO3 -] / Kh[CO2(d)]
The ability of a substance to surround ions in dipole interactions and diminish their attraction for each other. D. What ionization in solution depends on.
hydration shells
Buffer system of blood plasma. H2CO3 H+ + HCO3 -. Concentration of H2CO3 small fraction of HCO3 - concentration, because pKa1 is 3.77.
H-bonded water network rearranged toward formation of a local cage structure surrounding each solute molecule. Accompanied by significant ordering (negative entropy). H2O next to solvent have limited structural options. Straddle nonpolar solute so two of three H-bonding vectors available (tangential to solute). Allows H2O to retain H-bonding possibilities because no H-bond acceptor/donator directed towards solute.
Nonpolar solutes: do not H bond. Only sparingly soluble in water. Dissolving nonpolar solutes needs significant reorganization of water surrounding the solute
salts, nonionic but polar substances and carbonyl-containing molecules
water molecules surrounding ions. Stable structures but also dynamic.
True or False
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Kw / Ion product of water
Concentration of H2O in pure water Reciprocal relationship between H+ and OH- concentrations in aqueous solutions
True
False
Henderson-Hasselbalch equation
pH = pKa + log [A-]/[HA]. pH of a solution can be calculated, provided Ka and the concentrations of the weak acid HA and its conjugate base A- are known. Provides a general solution to the quantitative treatment of acid-base equilibria in biological systems.
True
False
respiratory acidosis
Substances capable of generation ions in solution and thereby causing an increase in electrical conductivity of the solution.
True
False
bicarbonate/carbonic acid couple
The ability of a substance to surround ions in dipole interactions and diminish their attraction for each other. D. What ionization in solution depends on.
True
False
clathrate
H-bonded water network rearranged toward formation of a local cage structure surrounding each solute molecule. Accompanied by significant ordering (negative entropy). H2O next to solvent have limited structural options. Straddle nonpolar solute so two of three H-bonding vectors available (tangential to solute). Allows H2O to retain H-bonding possibilities because no H-bond acceptor/donator directed towards solute.
True
False
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Practice Test: Biochemistry Chapter 2