Basis of medical chemistry
1. What compound can’t dissolve in water at standard state?
A. Acetic acid.
B. Ethanol.
C. Sodium chloride.
D. Oil.
E. Sugar.
ANSWER: D
2. Solution is it:
A. Heterogeneous system which consists of two components.
B. Homogeneous system which consists of two or more components and their products.
C. Heterogeneous system which consists of two or more components and their products.
D. Heterogeneous system in which it is impossible to distinguish component parts.
E. Homogeneous system which consists of one component.
ANSWER: B
3. What is a mole?
A. It is the ratio of the mass solute to the mass of solution mass of a solvent
B. It is the quantity grams of solute which percentage in 100 g of solution.
C. The quantity of matter contains such quantity atoms, molecules, ions, as is atoms in 0,012 kgs of an
isotope Carbon 12C.
D. The ratio of mass compound to numbers mole compound.
E. The ratio of the number of moles of that component to the total number of moles of all components.
ANSWER: C
4. What is a molar concentration (a molarity)?
A. The ratio between of the mole of solute and the total mole of solution.
B. The quantity of one component of a solution expressed as a percentage of the total mass.
C. The number of moles of solute dissolved per liter of solution.
D. The number of moles of solute dissolved per kilogram of solvent.
E. Quantity mole-equivalent of solute per one liter of solution.
ANSWER: C
5. When cells are placed in а solution with а lower solute concentration (hypotonic solution), water will move
into the cells. Red blood cells, for example, will swell and rupture in а process called:
A. Plasmolysis.
B. Osmosis.
C. Hemolysis.
D. Solubility.
E. Diffusion.
ANSWER: C
6. In hypertonic solutions, those with higher solute concentrations, cells shrivel because there is а net
movement of water out of the cell. The shrinkage of red blood cells in hypertonic solution is called:
A. Plasmolysis.
B. Osmosis.
C. Hemolysis.
D. Solubility.
E. Diffusion.
ANSWER: A
7. Colligative properties is all except:
A. Vapor-pressure lowering.
B. Boiling-point elevation.
C. Freezing-point depression.
D. Osmotic pressure.
E. Mole mass.
ANSWER: E
8. Hemolysis is:
A. In hypertonic solutions, those with higher solute concentrations, cells shrivel because there is а net
movement of water out of the cell. The shrinkage of red blood cells in hypertonic solution.
B. When cells are placed in а solution with а lower solute concentration (hypotonic solution), water will
move into the cells. Red blood cells, for example, will swell and rupture.
C. The method for determination of molar mass of compounds by freezing-point depression.
D. The solubility of a gas dissolved in a liquid is proportional to the partial pressure of the gas above the
liquid.
E. The spontaneous mixing of the particles of the solute (present in the solution) and the solvent (present
above the solution) to form а homogeneous mixture.
ANSWER: B
9. Plasmolysis is:
A. In hypertonic solutions, those with higher solute concentrations, cells shrivel because there is а net
movement of water out of the cell. The shrinkage of red blood cells in hypertonic solution.
B. When cells are placed in а solution with а lower solute concentration (hypotonic solution), water will
move into the cells. Red blood cells, for example, will swell and rupture.
C. The method for determination of molar mass of compounds by freezing-point depression.
D. The solubility of a gas dissolved in a liquid is proportional to the partial pressure of the gas above the
liquid.
E. The spontaneous mixing of the particles of the solute (present in the solution) and the solvent (present
above the solution) to form а homogeneous mixture.
ANSWER: A
10. Diffusion is:
A. In hypertonic solutions, those with higher solute concentrations, cells shrivel because there is а net
movement of water out of the cell. The shrinkage of red blood cells in hypertonic solution.
B. When cells are placed in а solution with а lower solute concentration (hypotonic solution), water will
move into the cells. Red blood cells, for example, will swell and rupture.
C. The method for determination of molar mass of compounds by freezing-point depression.
D. The solubility of a gas dissolved in a liquid is proportional to the partial pressure of the gas above the
liquid.
E. The spontaneous mixing of the particles of the solute (present in the solution) and the solvent (present
above the solution) to form а homogeneous mixture.
ANSWER: E
11. Isotonic solutions are:
A. Those which have lest osmotic pressure then blood plasma.
B. Those which have the same osmotic pressure as blood plasma.
C. Those which have the greater osmotic pressure then blood plasma
D. That solution in which the concentration of solute is greater than in a saturated solution.
E. Solution in which the concentration of solute is less than in a saturated solution.
ANSWER: B
12. Hypertonic solutions are:
A. Those which have lest osmotic pressure then blood plasma.
B. Those which have the same osmotic pressure as blood plasma.
C. Those which have the greater osmotic pressure then blood plasma
D. Solution in which the concentration of solute is greater than in a saturated solution
E. Solution in which the concentration of solute is less than in a saturated solution.
ANSWER: C
13. Hypotonic solutions are:
A. Those which have lest osmotic pressure then blood plasma.
B. Those which have the same osmotic pressure as blood plasma.
C. Those which have the greater osmotic pressure then blood plasma
D. Solution in which the concentration of solute is greater than in a saturated solution
E. Solution in which the concentration of solute is less than in a saturated solution.
ANSWER: A
14. Physiological solution of sodium chloride is solution, which percent by weight is:
A. 0.89 %.
B. 2.61 %.
C. 1.63 %.
D. 8.9 %.
E. 98 %.
ANSWER: A
15. What compounds is formed in neutralization reaction?
A. Strong acids.
B. Weak acids.
C. Acid and base.
D. Salt and water.
E. Strong base.
ANSWER: D
16. For determination of рН solution is used:
A. Voltmiter.
B. Centrifuger.
C. Photoelectrocolorimetr.
D. рН-meter.
E. Calorimeter.
ANSWER: D
17. What is color of methyl orange in acidic medium?
A. Red.
B. Blue.
C. Violet.
D. Orange.
E. Colorless.
ANSWER: A
18. What is color of methyl red (indicator) in basic medium?
A. Red.
B. Blue.
C. Yellow.
D. Orange.
E. Colorless.
ANSWER: C
19. What is color of phenolphalein in basic medium?
A. Yellow.
B. Blue.
C. Orange.
D. Crimson.
E. Colorless.
ANSWER: D
20. What is color of litmus in basic medium?
A. Yellow.
B. Blue.
C. Orange.
D. Crimson.
E. Colorless.
ANSWER: B
21. What is value of рН blood human body?
A. 7,93-9,45.
B. 7,36-7,45.
C. 6,20-7,30.
D. 2,10-4,15.
E. 5,70-6,74.
ANSWER: B
22. What factor is influence for pH of buffer solution:
A. Water product.
B. Ratio between solution component concentrations.
A. Heat capacity.
B. Temperature of solution.
C. Atmospheric pressure.
ANSWER: B
23. The capacity of а buffer solution depends on:
A. The ratio of acid-conjugate base pair concentrations.
B. Name of components.
C. Temperature solution.
D. Pressure.
E. Concentration of water.
ANSWER: A
24. How рН of buffer solution is changed, if add 50 mls of water?
A. Once.
B. Twice.
C. Three times.
D. Four times.
E. Do not change
ANSWER: E
25. What method are you used for determination total hardness of water?
A. Acid-base titration.
B. Chelatometry.
C. Precipitation.
D. Oxidation - reduction titration.
E. Sedimentation.
ANSWER: B
26. What method are you used for determination concentration of NaCl in solution?
A. Acid-base titration.
B. Chelatometry.
C. Precipitation.
D. Oxidation - reduction titration.
E. Sedimentation.
ANSWER: C
27. What method are you used for determination concentration of potassium permanganate in solution?
A. Acid-base titration.
B. Chelatometry.
C. Precipitation.
D. Oxidation - reduction titration.
E. Sedimentation.
ANSWER: D
28. It is used as titrant in acid-base titration such compound:
A. KCl.
B. NaHCO3.
C. Na2SO4.
D. HCl.
E. CuOH.
ANSWER: D
29. In the titrimetric analysis use the method of neutralization. What titrants are used in this method?
A. NaNO3, Na2S2O3.
B. AgNO3, BaCl2.
C. NaOH, HCl.
D. KI, K2Cr2O7.
E. KI, KMnO4.
ANSWER: C
30. Solutions of permanganate as titrant using in:
A. Acid-base titration.
B. Chelatometry.
C. Precipitation.
D. Sedimentation.
E. Oxidation - reduction titration.
ANSWER: E
31. What elements are p-elements?
A. Sodium, Potassium.
B. Calcium, Aluminum.
C. Fluorine, Chlorine.
D. Lithium, Beryllium.
E. Iron, Manganese.
ANSWER: C
32. What elements are s-elements?
A. Sodium, potassium.
B. Vanadium, Aluminum.
C. Fluorine, Chlorine.
D. Bromine, Iodine.
E. Iron, Manganese.
ANSWER: A
33. What element is macro element?
A. Hg.
B. Mn.
C. Cu.
D. Br.
E. Ca
ANSWER: E
34. Sodium dihydrogenphosphate is:
A. Na3PO4.
B. Na2HPO4.
C. NaH2PO4.
D. Na3PO3.
E. NaH2PO5.
ANSWER: C
35. What micro element is in erythrocytes?
A. Sodium.
B. Vanadium.
C. Fluorine.
D. Bromine.
E. Iron.
ANSWER: E
36. What element is in bones?
A. Sodium.
B. Vanadium.
C. Fluorine.
D. Calcium.
E. Iron.
ANSWER: C
37. Sodium is:
A. s - element.
B. d - element.
C. f - element.
D. p - element.
E. g - element
ANSWER: A
38. Calcium is:
A. s - element.
B. d - element.
C. f - element.
D. p - element.
E. g - element.
ANSWER: A
39. Calcium has different biological functions. What main function is essential for calcium?
A. In blood coagulation.
B. Activates the conversion of prothrombin to thrombin.
C. In milk clotting.
D. Bones and teeth formation.
E. In muscle contraction.
ANSWER: D
40. What element with phosphorus is present in teeth?
A. Copper.
B. Cobalt.
C. Calcium.
D. Chlorine.
E. Zinc.
ANSWER: C
41. Physiological solution is:
A. Those solutions, which have lest osmotic pressure then blood plasma.
B. Those solutions, which have the same osmotic pressure as blood plasma.
C. Those solutions, which have the greater osmotic pressure then blood plasma.
D. Solution is one in which the concentration of solute is greater than its concentration in a saturated
solution.
E. Solution in which the concentration of solute is less than its concentration in a saturated solution.
ANSWER: B
42. The partical size of true solution is:
A. The less than 10-9 m.
B. 10-7-10-9 m.
C. The more then 10-5 m.
D. 10-5-10-3 m.
E. 10-7-10-5 m.
ANSWER: A
43. А system usually consists of а definite amount of one or more substances and is separated from the
surroundings by а real or imaginary boundary through which matter and energy can flow from the
system to the surroundings or vice versa:
A. Exogenous and endogenous.
B. One, two, three compounds.
C. Homogenous and heterogeneous.
D. Isolated, opened, closed.
E. Reversible and irreversible.
ANSWER: D
44. It is used stable temperature and pressure for the most processes in chemical technology. What is process
name?
A. Isochoric - Isothermel.
B. Isobar - Isothermic.
C. Isobar - Isochoric.
D. Isochoric - Adiabatic.
E. Isothermal - Adiabatic.
ANSWER: B
45. State in which both reactants and products are present in concentrations which have no further tendency to
change with time. is called:
A. Isochoric.
B. Adiabatic
C. Isothermal.
D. Isobar.
E. Equilibrium.
ANSWER: E
46. Thermodynamics systems are classified by amount of phases into:
A. Exogenous and endogenous.
B. Solid, liquid, gas.
C. Homogeneous and heterogeneous.
D. Isolated, opened, closed
E. Reversible and irreversible.
ANSWER: C
47. If а system can exchange only energy with the surroundings but not matter, it is called:
A. Exogenous.
B. Closed
C. Homogenous.
D. Isolated.
E. Opened.
ANSWER: B
48. If system can exchange both matter and energy with the surroundings, it is called:
A. Exogenous.
B. Closed
C. Homogenous.
D. Isolated.
E. Opened.
ANSWER: E
49. If а system can neither exchange matter nor energy with the surroundings, it is called
A. Exogenous.
B. Closed
C. Homogenous.
D. Isolated.
E. Opened
ANSWER: D
50. Closed thermodynamics systems are systems, which can exchange with the surroundings:
A. Matter.
B. Energy.
C. Both matter and energy.
D. Temperature.
E. Neither exchange matter nor energy.
ANSWER: B
51. Opened thermodynamics systems are systems, which can exchange with the surroundings:
A. Matter.
B. Energy.
C. Both matter and energy
D. Temperature.
E. Neither exchange matter nor energy.
ANSWER: C
52. If all reagent and products of reaction are in same phase, this reaction is called:
A. Homogeneous
B. Single-phased
C. Multi-phased
D. Heterogeneous
E. Different-phased
ANSWER: A
53. Heterogeneous system is:
A. System which consists of one phase.
B. System which consists of two or more phases.
C. Contain liquid.
D. System which consists of a single phase.
E. System in which is distilled water .
ANSWER: B
54. All factors influence for rate of reaction except:
A. Concentration of the reactants.
B. Temperature.
C. Presence of Catalyst.
D. Surface area of the reactants.
E. Color of indicator.
ANSWER: E
55. Rate of chemical reaction is:
A. The change in the concentration of any one of the reactants or products per unit of time.
B. The change of the coloring of indicator.
C. The change of volume.
D. The change of pH value.
E. The change of temperature.
ANSWER: A
56. Branch of chemistry which deals with the study of the speeds or the rates f chemical reactions, the factors
affecting the rates of the reactions and the mechanism by which the reactions proceed is:
A. Thermodynamics.
B. Chemical kinetics.
C. Analytical chemistry.
D. Electrochemistry.
E. Inorganic chemistry.
ANSWER: B
57. If all reagent and products of reaction are in different phases, this reaction is called:
A. Homogeneous
B. Single-phased
C. Different-phased
D. Heterogeneous
E. Similar.
ANSWER: D
58. For rate constant influence all factors except:
A. Concentration of the reactants.
B. Temperature.
C. Pressure.
D. Surface area of the reactants.
E. Nature of reagents.
ANSWER: A
59. What factors are influence for rate constant?
A. Concentration of the reactants.
B. Indicator.
C. Dispersed phase.
D. Surfactant.
E. Nature of reagents.
60. What factors influence for rate of reaction?
A. Concentration of the reactants.
B. Indicator.
C. Dispersed phase.
D. Surfactant
E. Surface tension.
ANSWER: A
61. The processes in which both catalyst and reagents are in same phase is called:
A. Heterogeneous catalysis.
B. Homogeneous catalysis.
C. Positive catalysis.
D. Negative catalysis.
E. Autocatalysis.
ANSWER: B
62. The process in which reagents react with surface of catalyst is named:
A. Heterogeneous catalysis.
B. Homogeneous catalysis.
C. Positive catalysis.
D. Negative catalysis.
E. Autocatalysis.
ANSWER: A
63. The nature of enzyme is:
A. Carbohydrate.
B. Lipid
C. Protein.
D. Mineral acid
E. Vitamin.
ANSWER: C
64. A substance which can change the speed of а chemical reaction without being used up in that reaction and
the phenomenon is known as:
A. Polymers.
B. Hormones.
C. Catalysts.
D. Indicators
E. Vitamin.
ANSWER: C
65. Biological catalysts are:
A. Polymers.
B. Vitamin.
C. Hormones.
D. Indicators.
E. Enzymes.
ANSWER: E
66. Hydrogen electrode is:
A. Metal-metal ion electrode.
B. Gas-ion electrodes.
C. Metal-insoluble salt-anion electrode.
D. Inert "oxidation-reduction" electrode.
E. Membrane electrode.
ANSWER: B
67. Standard EMF of the cell equaled:
A. pH.
B. Oxidation number.
C. Standard oxidation potential of the oxidation half reaction + Standard reduction potential of the reduction
half reaction.
D. Solubility product.
E. Heat effect.
ANSWER: C
68. Processes, which are between interfaces of two systems is:
A. Coagulation.
B. Surface phenomena.
C. Surface tension.
D. Absorption.
E. Boiling.
ANSWER: B
69. The surfactants are compound, except:
A. Alcohols.
B. Alkalis.
C. Salts of fat acids.
D. Protein.
E. Hydrochloric acid.
ANSWER: E
70. The surfactant is:
A. Hydrochloric acid.
B. Calcium hydroxide.
C. Sodium chloride.
D. Isoamil alcohol.
E. Potassium.
ANSWER: D
71. The concentrated one component in the surface other is named:
A. Absorption.
B. Adsorption.
C. Disorbsion.
D. Solubility.
E. Capillary condensation.
ANSWER: B
72. Adsorption is:
A. The phenomenon of concentrated the molecules of а substance on the surface of а liquid or а solid
resulting.
B. Chemical reaction between adsorbed and adsorbate.
C. When molecules have hydrophilic and hydrophobic groups simultaneously.
D. The separation of mixtures.
E. The chromatography analysis.
ANSWER: A
73. What method is used for separation dispersion particles by sizes?
A. Electrophoreses.
B. Brownian motion.
C. Diffusion.
D. Sedimentation.
E. Osmotic pressure
ANSWER: A
74. These methods involve the joining together of а large number of smaller particles to form particles of
colloidal size.
A. Peptization.
B. Polymerisation
C. Condensation.
D. Titration
E. Dispersion.
ANSWER: C
75. In а gravitational field, heavy particles settle towards the foot of а column of solution by the process called:
A. Ultracentrifugation.
B. Sedimentation.
C. Coagulation.
D. Flocculation.
E. Dialysis.
ANSWER: B
76. Blood is dispersed system, once of dispersed phase particles are erythrocytes with size 10-4 m. What type of
dispersed system is it?
A. True solution.
B. Macroheterogeneous.
C. Microheterogeneous.
D. Ultramicroheterogeneous.
E. Colloidal solution.
ANSWER: C
77. Blood serum is dispersed system. What type dispersed system is it?
A. True solution.
B. Solid.
C. Macroheterogeneous.
D. Microheterogeneous.
E. Colloidal solution.
ANSWER: E
78. System with size dispersed phase particle equal 10-9 - 10-7 is:
A. True solution.
B. Microheterogeneous.
C. Macroheterogeneous.
D. Homogeneous.
E. Colloidal solution.
ANSWER: E
79. What polymer is natural?
A. Polyethylene.
B. Kapron.
C. Polypropilen.
D. Starch.
E. Polyformaldehyde.
ANSWER: D
80. If in the half cell, the metal rod is suspended in а solution of one molar concentration, and the temperature is
kept at 298 К, the electrode potential is called:
A. Membrane potential.
B. Diffuse potential.
C. Electro-kinetic potential.
D. Concentration potential.
E. Standard electrode potential.
ANSWER: E
81. The kinetic energy that reactant molecules must have allows them to reach the transition state so that a
reaction can occur.
A. Heat effect reaction.
B. Potential energy.
C. Activation energy.
D. Enthalpy.
E. Free Gibbs’ energy.
ANSWER: C
82. The study of rates and mechanisms of chemical reactions and of the factors on which they depend is:
A. Thermodynamics.
B. Electrochemistry.
C. Colloidal chemistry.
D. Chemical kinetics.
E. Gravimetric analysis.
ANSWER: D
83. The part of the universe chosen for thermodynamic consideration (to study the effect of temperature,
pressure etc.) is called:
A. System.
B. Surroundings.
C. Entropy.
D. Reaction.
E. Energy.
ANSWER: A
84. What compounds cannot form solution?
A. Silicon (II) oxide and water.
B. NaOH and water.
C. Aluminum and copper.
D. NaCl and water.
E. Sugar and water.
ANSWER: A
85. Mass concentration, titer is ……..
A. The ratio between the volume solute and total volume of solution.
B. Number grams of solute per one milliliter of solution.
C. The number of moles of solute dissolved per liter of solution.
D. The number of moles of solute dissolved per kilogram of solvent.
E. Quantity gram-equivalent of solute per one liter of soluti
ANSWER: B
86. What is a percentage by weight (mass)?
A. The ratio between of the mole of solute and the total mole of solution.
B. The quantity of one component of a solution expressed as a percentage of the total mass.
C. The number of moles of solute dissolved per liter of solution.
D. The number of moles of solute dissolved per kilogram of solvent.
E. Quantity mole-equivalent of solute per one liter of solution.
ANSWER: B
87. Neutralization reaction is the reaction between:
A. Strong acids.
B. Weak acids.
C. Acid and base.
D. Weak bases.
E. Strong base.
ANSWER: C
88. What is composition of acetic buffer solutions?
A. CH3COOH/CH3COO-.
B. H2CO3/HCO3-.
C. HHbO2/HbO2-.
D. H2PO4-/HPO42-.
E. NH3/NH4+
ANSWER: A
89. What solution has the great buffer capacity?
A. 10/20.
B. 5/10.
C. 50/100.
D. 20/40.
E. 200/400.
ANSWER: E
90. pH of neutral medium is:
A. pH = 2.
B. pH = 10.
C. pH = 4.
D. pH = 7.
E. pH = 12.
ANSWER: D
рН of basic medium:
рН = - 7.
A.
рН < 7.
B.
рН = 7.
C.
рН >7.
D.
рН < - 7.
ANSWER: D
91. The concept “Total general of energy is stable in all isolated system” is:
A. First law of thermodynamics.
B. Second law of thermodynamics.
C. Third law of thermodynamics.
D. Hess’s law.
E. Kirchhoff’s law.
ANSWER: A
What process is name when stable temperature?
A. Isolated.
B. Isobaric.
C. Isochoric.
D. Adiabatic.
E. Isothermic.
ANSWER: E
92. A substance which can change the speed of а chemical reaction without being used up in that reaction and
the phenomenon is known as:
A. Polymers.
B. Hormones.
C. Catalysts.
D. Indicators
E. Vitamin.
ANSWER: C
93. What kind of dispersion systems is fog (G-gas, L-Liquid, S-solid)?
A. G/S.
B. S/S.
C. L/L.
D. G/G.
E. L/G.
ANSWER: E
94. What kind of dispersion systems is smoke (G-gas, L-Liquid, S-solid)?
A. G/S.
B. S/S.
C. L/L
D. .S/G.
E. G/L
ANSWER: D
95. The study of rates and mechanisms of chemical reactions and of the factors on which they depend is:
A. Thermodynamics.
B. Electrochemistry.
C. Colloidal chemistry.
D. Chemical kinetics.
E. Gravimetric analysis.
ANSWER: D
96. "k" in rate law equation υ =k[A][B] is:
A. Rate constant.
B. Mass-action expression.
C. Chemical equilibrium constant.
D. Rate.
E. Temperature reaction.
ANSWER: A
97. υ in rate law equation υ =k[A][B] is:
A. Rate constant.
B. Mass-action expression.
C. Chemical equilibrium constant.
D. Rate.
E. Temperature reaction.
ANSWER: D
98. The part of the universe chosen for thermodynamic consideration (to study the effect of temperature,
pressure etc.) is called:
A. System.
B. Surroundings.
C. Entropy.
D. Reaction.
E. Energy.
ANSWER: A
99. The remaining portion of the universe, excluding the system, is called:
A. System.
B. Surroundings.
C. Entropy.
D. Reaction.
E. Energy.
ANSWER: B
100. Isothermal process is:
A. А process is carried out in such а manner that the temperature remains constant throughout the process.
B. A process is carried out in such а manner that no heat can flow from the system to the surroundings or vice
versa i.e. the system is completely insulated from the surroundings.
C. А process during which the volume of the system is kept constant.
D. А process during which the pressure of the system is kept constant.
E. А process which is carried out infinitesimally slowly so that all changes occurring in the direct process can
be exactly reversed.
ANSWER: A