Basis of medical chemistry
Text teat assesments
1. What compound cannot dissolve in water at standard state?
A. Acetic acid.
B. Ethanol.
C. Sodium chloride.
D. * Oil.
E. Sugar.
2. What is compound increased solubility, if temperature is increased also?
A. CO2.
B. Sulfuric acid.
C. Oxygen.
D. Carbon monoxide.
E. Sulfur oxide.
3. 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.
4. Such compounds cannot form solution:
A. Hydrogen and nitrogen.
B. * Silver and water.
C. Sugar and water.
D. Oxygen and helium.
E. Sodium and water.
5. 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.
6. How many mole of solute is dissolved in 4 litres of solution with a concentration 1 mole per 1 liter of
solution?
A. 0.4 mole.
B. 1 mole.
C. * 4 mole.
D. 3 mole.
E. 2 mole.
7. By the chemical theory solution is:
A. *Chemical non-stabile compounds, which is formed when solvent interact with solute.
B. System, which is formed when solute scattered in solvent.
C. Mixture with two compounds.
D. System which changes.
E. System which has stable state.
8. By the physical theory solution is:
A. Chemical non-stabile compound, which is formed when solvent interact with solute.
B. * System, which is formed when solute interact with solvent.
C. Mixture with two compounds.
D. System which changes.
E. System which has stable state.
9. 30 g of sodium hydroxide is dissolved in 270 g of water. What is a mass fraction of this solution?
A. *10 %
B. 2 %
C. 25 %
D. 100 %
E. 12 %
10. 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.
11. For calculation molarity of solution is used such formula:
A.
B.
C.
CM 
D. *
n( solute)
V ( solution )
n solute 
m(solvent )
E.
12. Choose the formula which is used for calculation percentage by weight (mass percent):
n( solute)
A. CM 
V ( solution )
m solute 
Cn 
E ( solute)  V ( solution )
B.
m solute 

 100%
m( solution )
C. *
Cm 
n solute 
m(solvent )
D.
m solute 
T
V (solution )
E.
13. For calculation mass fraction used such formula:
m solute 
Cn 
E ( solute)  V ( solution )
A.
m solute 

m(solution )
B. *
Cm 
n( solute)
V ( solution )
C.
n solute 
Cm 
m(solvent )
D.
m solute 
T
V (solution )
E.
14. Volume fraction (percentage by volume) of a component in solution is ……..
A. The number of moles of the component divided by the total number of moles making up the solution.
B. *The volume of the component divided by the total volume making up the solution
C. The number of grams of the component divided by the number of milliliters of solution.
D. The number of moles of solute dissolved per kilogram of solvent.
E. The number of moles of solute per volume (liter) of solution.
15. Percentage by weight (mass) or mass percent is ...........
CM 
A. The ratio between the volume solute and total volume 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 gram-equivalent of solute per one liter of solution.
16. Molar concentration of an equivalent (normal concentration), normality ……
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, which is in per one liter of solution.
17. 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 solution.
18. Molarity, or molar concentration 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 solution.
19. Molality is ……………
A. The ratio between the volume of 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 solution.
20. What is a mass fraction?
A. The ratio between the volume of solute and total volume of solution.
B. *The ratio between the mass of solute and total mass 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 solution.
21. What is a molar fraction?
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 gram-equivalent of solute per one liter of solution.
22. 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 gram-equivalent of solute per one liter of solution.
23. What is a normal concentration (a normality)?
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 gram-equivalent of solute per one liter of solution.
24. 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 gram-equivalent of solute per one liter of solution.
25. For calculation molality of solution is used such formula:
m solute 

m(solution )
A.
m solute 
Cn 
E ( solute)  V ( solution )
B.
m(compound )
M
n(compound )
C.
m solute 
T
V (solution )
D.
n solute 
Cm 
m(solvent )
E. *
26. For calculation mole mass (weight) of compound is used such formula:
m solute 

m(solution )
A.
m(compound )
M
n(compound )
B. *
n( solute)
V ( solution )
C.
m solute 
Cn 
E ( solute)  V ( solution )
D.
  solute 
Cm 
m(solvent )
E.
27. Choose the formula which is used for calculation mass concentration (titr):
m solute 

m(solution )
A.
m(compound )
M
n(compound )
B.
m solute 
T
V (solution )
C. *
CM 
m solute 
E ( solute)  V ( solution )
D.
n solute 
Cm 
m(solvent )
E.
28. For calculation normality of solution is used such formula:
m(compound )
A. M 
n(compound )
n solute 
Cm 
m(solvent )
B.
m solute 
Cn 
E ( solute)  V ( solution )
C. *
Cn 
m solute 
m(solution )
D.
m solute 

 100%
m
(
solution
)
E.
29. For calculation volume fraction of solution is used such formula:

m solute 
m(solution )
A.
V solute 

V( solvent )  V solute 
B. *
m(compound )
M
n(compound )
C.
m solute 
Cn 
E ( solute)  V ( solution )
D.
m solute 
T
V( solution )
E.
30. For calculation mole fraction (percentage by mole) of solution is used such formula:
  solute 
X
 ( solvent )    solute 
A. *

V solute 
V( solvent )  V solute 
B.
m solute 
Cn 
E ( solute)  V ( solution )
C.
m(compound )
M
n(compound )
D.
m solute 

m(solution )
E.
31. Cryoscopy this:
A. *The method for determination of molar mass of compounds by freezing-point depression.
B. The method for determination boiling temperature.
C. The method for determination boiling-point elevation.
D. The method for determination osmosis.
E. The method for determination solubility of compounds.
32. 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.
33. 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.
34. Henry’s law 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. A supersaturated solution is one in which the concentration of solute is greater than its concentration in a
saturated solution.
35. Colligative properties is all except:

A. Vapor-pressure lowering.
B. Boiling-point elevation.
C. Freezing-point depression.
D. Osmotic pressure.
E. *Mole mass.
36. 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.
37. 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 ffreezing-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.
38. 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.
39. Raoult's Law:
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 partial vapor pressure of a component in liquid solution is proportional to the mole fraction of that
component, the constant of proportionality being the vapor pressure of the pure component.
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.
40. 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.
41. 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.
42. 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.
43. This formula PV= nRT is formula of:
A. Henry's law equation.
B. Freezing point determination equation.
C. *Van’t Hoff law equation.
D. Raoult's law equation.
E. Boiling-point elevation equation.
44. This formula ∆Tboiling= Kboiling* m is formula of:
A. Henry's law equation.
B. Freezing point determination equation.
C. Van’t Hoff law equation.
D. Raoult's law equation.
E. *Boiling-point elevation equation.
45. This formula is ∆Tfreezing= Kfreezing*m formula of::
A. Henry's law equation.
B. *Freezing point depretion equation.
C. Van’t Hoff law equation.
D. Raoult's law equation.
E. Boiling-point elevation equation.
46. This formula P1 = X1 P10 is formula of:
A. Henry's law equation.
B. Freezing point determination equation.
C. Van’t Hoff law equation.
D. *Raoult's law equation.
E. Boiling-point elevation equation.
47. This formula X = KP is formula of:
A. *Henry's law equation.
B. Freezing point determination equation.
C. Van’t Hoff law equation.
D. Raoult's law equation.
E. Boiling-point elevation equation.
48. Colligative property is:
A. Temperature.
B. *Boiling-point elevation.
C. Volume.
D. Mole.
E. Molecule weight.
49. 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 %.
50. Colligative properties is:
A. Temperature.
B. Normality.
C. Volume.
D. *Osmotic pressure.
E. Molecule weight.
51. Neutralization reaction is the reaction between:
A. Strong acids.
B. Weak acids.
C. *Acid and base.
D. Weak bases.
E. Strong base.
52. What compounds is formed in neutralization reaction?
A. Strong acids.
B. Weak acids.
C. Acid and base.
D. *Salt and water.
E. Strong base.
53. For determination of рН solution is used:
A. Voltmiter.
B. Centrifuger.
C. Photoelectrocolorimetr.
D. *рН-meter.
E. Calorimeter.
54. What is color of methyl orange in acidic medium?
A. *Red.
B. Blue.
C. Violet.
D. Orange.
E. Colorless.
55. What is color of methyl red (indicator) in basic medium?
A. Red.
B. Blue.
C. *Yellow.
D. Orange.
E. Colorless.
56. What is color of phenolphalein in basic medium?
A. Yellow.
B. Blue.
C. Orange.
D. *Crimson.
E. Colorless.
57. Acid - base titration indicators is:
A. *Weak acids or weak bases.
B. Strong acids.
C. Strong bases.
D. Derivative of mineral acids.
E. Salt.
58. What is color of litmus in basic medium?
A. Yellow.
B. *Blue.
C. Orange.
D. Crimson.
E. Colorless.
59. What formula is used for calculate pH of solution:
A. КW = [Н+][ОН-]
B. *рН = - lg[Н+]
C.
D. рН = lg[Н+] lg[ОН-]
E. рН = - lg[Н+] lg[ОН-]
60. рН = 6.5. What is medium of solution:
A. Strong basic.
B. Neutral
C. *Weak acidic.
D. Weak-basic.
E. Strong acidic.
61. What is composition of phosphate buffer solutions?
A. HHb/Hb-.
B. HHbO2/HbO2-.
C. *H2PO4-/HPO42-.
D. H2CO3/HCO3-.
E. NH3/NH4+
62. What is composition of oxihemoglobin buffer solutions?
A. HHb/Hb-.
B. *HHbO2/HbO2-.
C. H2PO4-/HPO42-.
D. H2CO3/HCO3-.
E. NH3/NH4+
63. What is composition of bicarbonate buffer solutions?
A. HHb/Hb-.
B. HHbO2/HbO2-.
C. H2PO4-/HPO42-.
D. *H2CO3/HCO3-.
E. NH3/NH4+
64. What is composition of ammonia buffer solutions?
A. HHb/Hb-.
B. HHbO2/HbO2-.
C. H2PO4-/HPO42-.
D. H2CO3/HCO3-.
E. *NH3/NH4+
65. What is composition of hemoglobin buffer solutions?
A. *HHb/Hb-.
B. HHbO2/HbO2-.
C. H2PO4-/HPO42-.
D. H2CO3/HCO3-.
E. NH3/NH4+
66. What is composition of acetic buffer solutions?
A. *CH3COOH/CH3COO-.
B. H2CO3/HCO3-.
C. HHbO2/HbO2-.
D. H2PO4-/HPO42-.
E. NH3/NH4+
67. What is composition of protein buffer solutions?
A. HHb/Hb-.
B. H2PO4-/HPO42-.
C. *NH2RCOOH/NH2RCOOD. HHbO2/HbO2-.
E. H2CO3/HCO3-.
68. Blood buffer solution is all except:
A. HHb/Hb-.
B. HHbO2/HbO2-.
C. H2PO4-/HPO42-.
D. H2CO3/HCO3-.
E. *NH3/NH4+
69. Blood buffer solution is:
A. CH3COOH/CH3COO-.
B. *H2CO3/HCO3-.
C. HCl/Cl-.
D. H2SO4/HSO4-.
E. NH3/NH4+.
70. Blood buffer solution is all except:
A. HHb/Hb-.
B. H2PO4-/HPO42-.
C. NH2RCOOH/NH2RCOO-.
D. *NH3/NH4+.
E. HHbO2/HbO2-.
71. What is value of рН blood human body?
A. 7,93-9,45.
B. *7,36-7,40.
C. 6,20-7,30.
D. 2,10-4,15.
E. 5,70-6,74.
72. The number of moles of а strong acid or а strong base that causes 1.00 L of the buffer to undergo а 1.00unit change in pH is called:
A. Water product.
B. The concentration of H+.
C. Heat capacity.
D. *The buffer capacity of а solution.
E. Acidity of solution.
73. What factor is influence for pH of buffer solution:
A. Water product.
B. *Ratio between solution component concentrations.
C. Heat capacity.
D. Temperature of solution.
E. Atmospheric pressure.
74. The capacity of а buffer systems depends on:
A. Name of components.
B. Temperature solution.
C. Pressure.
D. *The molar concentration of the acid-conjugate base pair.
E. Concentration of water.
75. 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.
76. Buffer capacity is directly proportional to the…….
A. Temperature solution.
B. Pressure.
C. *Concentration of the buffer solution components.
D. Pressure.
E. Concentration of water.
77. What solution has the great buffer capacity?
A. 10/20.
B. 5/10.
C. 50/100.
D. 20/40.
E. *200/400.
78. What solution has the great buffer capacity?
A. 10/20.
B. 5/10.
C. *50/50.
D. 20/40.
E. 7/3.
79. What solution has the great buffer capacity?
A. 10/20.
B. *500/1000.
C. 50/100.
D. 20/40.
E. 2/4.
80. What solution has the great buffer capacity?
A. 10/20.
B. 1/2.
C. 25/50.
D. 20/40.
E. *20/20.
81. Formula
is used to calculate:
A. *pH buffer solution.
B. Molarity.
C. Mass Fraction.
D. Solubility product.
E. Normality.
82. What formula is used for calculate pH of buffer solution:
A. КW = [Н+][ОН-].
B. рН = - lg[Н+].
C. *
.
D. рН = lg[Н+] lg[ОН-].
E. рН = - lg[Н+] lg[ОН-].
83. 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 non change
84. рН =9 of solution. What is acidity of this solution?
A. *Strong basic.
B. Neutral.
C. Weak acidic.
D. Weak basic.
E. Strong acidic.
85. What is value of water product?
A. Кw = 10-7.
B. Кw = 107.
C. Кw = 10.
D. *Кw = 10-14.
E. Кw = 10-10.
86. What formula is used for calculate pOH of solution?
A. КW = [Н+][ОН-].
B. рН = - lg[Н+].
C. *рН = - lg[ОН-].
D. рН = lg[Н+] lg[ОН-].
E. рН = - lg[Н+] lg[ОН-].
87. What formula is used for calculate water product:
A. *КW = [Н+][ОН-]
B. рН = - lg[Н+]
C.
D. рН = lg[Н+] lg[ОН-]
E. рН = - lg[Н+] lg[ОН-]
88. pH of neutral medium is:
A. pH = 2.
B. pH = 10.
C. pH = 4.
D. *H = 7.
E. pH = 12.
89. What value рН of basic medium:
A. рН = - 7.
B. рН < 7.
C. рН = 7.
D. *рН >7.
E. рН < - 7.
90. What concentration hydrogen ion is in basic medium:
A. More then10-4.
B. *Lest then10-7.
C. 10-7.
D. 10-1.
E. 10-4.
91. What method are you used you can use for determination an acid concentration in solution?
A. *Acid-base titration.
B. Chelatometry.
C. Oxidation - reduction titration.
D. Precipitation.
E. Sedimentation.
92. 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.
93. What method are you used you can use for determination concentration of NaCl in solution?
A. Acid-base titration.
B. Chelatometry.
C. *Precipitation.
D. Oxidation - reduction titration.
E. Sedimentation.
94. 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.
95. A highly purified compound that serves as а reference material in all volumetric titrimetric methods is:
A. Indicator.
B. Catalyst.
C. Adsorbate.
D. Investigation compounds.
E. *Primary standard.
96. It is used as titrant in acid-base titration such compound:
A. KCl.
B. NaHCO3.
C. Na2SO4.
D. *HCl.
E. CuOH.
97. As titrant in acid-base titration is used:
A. *HCl, NaOH, H2SO4, KOH.
B. BaCl2, NaI, KCl.
C. Na2SO4, KNO4, H2SO4.
D. CuOH, CoCl.
E. K2SO4, KMnO4.
98. As primary standard in acid-base titration is used:
A. KCl, NaBr.
B. *NaHCO3, Na2B4O7, H2C2O4.
C. Ag NO3, Na2SO4.
D. HCl, NaOH.
E. CuOH, ZnCO3.
99. 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.
100. What indicators is used in acid-base titration?
A. *Weak bases and weak acid.
B. AgNO3, BaCl2.
C. NaOH, HCl.
D. KI, K2Cr2O7.
E. KI, KMnO4.
101. In neutralization use such indicator:
A. Erichrom black T.
B. Potassium chromate.
C. *Methyl orange.
D. Potassium permanganate.
E. Iodine.
102. Temporal hardness of water this:
A. Amount of acids in solution.
B. Amount of calcium and magnesium sulfates and chlorides.
C. Amount of calcium and magnesium bicarbonate, sulfates and chlorides and other salt.
D. *Amount of calcium and magnesium bicarbonate.
E. Amount of potassium carbonate.
103. Permanent hardness of water this:
A. Amount of acetic asid in solution.
B. *Amount of calcium and magnesium sulfates and chlorides.
C. Amount of calcium and magnesium bicarbonate, sulfates and chlorides and other salt.
D. Amount of calcium and magnesium bicarbonate.
E. Amount of potassium carbonate.
104. Total hardness of water this:
A. Amount of oxalic acid in solution.
B. Amount of calcium and magnesium sulfates and chlorides.
C. *Amount of calcium and magnesium bicarbonate, sulfates and chlorides and other salt.
D. Amount of calcium and magnesium bicarbonate.
E. Amount of potassium carbonate.
105. What compound influence for temporal hardness of water:
A. CaCO3
B. CaSO4
C. *Ca(HCO3)2
D. Ca(OH)2
E. CaCl2
106. What compound is influence for permanent hardness of water:
A. CaCO3
B. *CaSO4
C. Ca(OH)2
D. Na3РО4
E.
107.
A.
B.
C.
D.
E.
108.
A.
B.
C.
D.
E.
109.
A.
B.
C.
D.
E.
110.
A.
B.
C.
D.
E.
111.
A.
B.
C.
D.
E.
112.
A.
B.
C.
D.
E.
113.
A.
B.
C.
D.
E.
114.
A.
B.
C.
D.
E.
115.
A.
B.
C.
D.
E.
116.
A.
Ca(HCO3)2
The method of chelatometry is used for determination concentration of :
Acids.
*Metal ions.
Bases.
Carboxylic acids.
Anions.
Water hardness is ordinarily determined by........
HCl.
NaOH.
KMnO4.
CuSO4.
*EDTA.
In the chelatometry use such indicator:
Ion-indicator.
Adsorb -indicator.
Redox-indicator.
Acid-base indicator.
*Complex indicator.
For determination of total hardness of water use:
0.1 M solution of sodium hydroxide.
0.05 M solution of potassium permanganate.
0.1M solution of acid salt.
*Solution of trilonium B.
0.1n solution of calcium hydroxide.
Solubility product of AgI is:
*Кsp = [Ag+][I-].
Кsp = [Ag+].
Кsp = [Ag+][NO4-]
Кsp = [I-]
Кsp = [Ag] [K]
As titrant in precipitation titration is used:
NaCl.
KMnO4.
*AgNO3.
CaSO4.
KBr.
As titrant in argentometry is used:
*AgNO3.
KMnO4.
NaCl.
CaSO4.
KBr.
As indicator in Mor’s method is used:
AgNO3.
*K2CrO4.
NaCl.
CaSO4.
KBr.
Solutions of permanganate as titrant using in:
Acid-base titration.
Chelatometry.
Precipitation.
Sedimentation.
*Oxidation - reduction titration.
As primary standard in permanganatometry is used:
*H2C2O4.
B.
C.
D.
E.
117.
A.
B.
C.
D.
E.
118.
A.
B.
C.
D.
E.
119.
A.
B.
C.
D.
E.
120.
A.
B.
C.
D.
E.
121.
A.
B.
C.
D.
E.
122.
A.
B.
C.
D.
E.
123.
A.
B.
C.
D.
E.
124.
A.
B.
C.
D.
E.
125.
A.
B.
C.
D.
NaCl.
K2CrO4.
H2SO4.
KBr.
Temporal hardness of water this:
Amount of Na hydrocarbonates.
Amount of Ca and Mg sulfates and chlorides.
Amount of Ca and Mg hydrocarbonates, sulfates and chlorides.
*Amount of Ca and Mg hydrocarbonates.
Total amount of salts.
A neutralization reaction it is reaction between:
Strong acids.
Weak acids.
Strong bases.
Weak bases.
*Acid and basis.
The water products this:
Products of solubility.
Sum of concentration of ions of Н+ and ОН-.
Change of concentrations.
*Products of concentration of hydrogen and hydroxide ions.
Difference of concentration of ions of Н+ and ОН-.
The oxidizing-restoration reactions are reaction in which:
Molecules are dissociated into ions.
Acid-basic interaction.
*Change of oxidation number of elements.
Hydrolyzed of salt.
Dissociate of acids.
Concentration of potassium permanganate is determined in?
In basic medium.
In neutral medium.
In weak bases medium.
*In acidic medium.
In alcohol solution.
Titrimetric analysis is used different reactions. What kind reaction is used for argentometry?
Oxidization reaction.
*Precipitation reaction.
Reduction reactions.
Neutralization reaction.
Chelatometry.
What elements are d-elements?
Sodium, Potassium
Calcium, Aluminum
Fluorine, Chlorine
Bromine, Iodine
*Iron, Manganese
What elements are p-elements?
Sodium, Potassium.
Calcium, Aluminum.
*Fluorine, Chlorine.
Lithium, Beryllium.
Iron, Manganese.
What elements are s-elements?
*Sodium, potassium.
Vanadium, Aluminum.
Fluorine, Chlorine.
Bromine, Iodine.
E.
126.
A.
B.
C.
D.
E.
127.
A.
B.
C.
D.
E.
128.
A.
B.
C.
D.
E.
129.
A.
B.
C.
D.
E.
130.
A.
B.
C.
D.
E.
131.
A.
B.
C.
D.
E.
132.
A.
B.
C.
D.
E.
133.
A.
B.
C.
D.
E.
134.
A.
B.
C.
D.
E.
135.
A.
Iron, Manganese.
Basic metals this:
Calcium, Magnesium.
*Potassium, Sodium.
Iron, Manganese.
Sulfur, carbon.
Aluminum, Bromine.
How many maximally electrons can be on the 3 p sub-shull (electronic energetic level)?
8.
2.
4.
*6.
1.
What element is macro element?
*S.
I.
Br.
F.
Al.
What element is macro element?
Cd.
Cu.
*Na.
Mn.
Co.
What element is macro element?
Hg.
Mn.
Cu.
Br.
*Ca
What element is micro element?
C.
S.
*I.
K.
Ca.
What element is micro element?
*F.
Cl.
Ca.
O.
C.
Sodium dihydrogenphosphate is:
Na3PO4.
Na2HPO4.
*NaH2PO4.
Na3PO3.
NaH2PO5.
Chlorine ion is with such element in nature:
Hydrogen.
*Sodium, potassium, magnesium.
Oxigen and fluorine.
Oxigen, sulfur.
Copper.
For ditermine Fe2+ is used such complex compound:
Potassium cyanide cuprate(II).
B.
C.
D.
E.
136.
A.
B.
C.
D.
E.
137.
A.
B.
C.
D.
E.
138.
A.
B.
C.
D.
E.
139.
A.
B.
C.
D.
E.
140.
A.
B.
C.
D.
E.
141.
A.
B.
C.
D.
E.
142.
A.
B.
C.
D.
E.
143.
A.
B.
C.
D.
E.
144.
A.
B.
C.
D.
Cupper potassium tetracyanate.
*Potassium hexacyanoferate(III).
Potassium hexacyanoferate(II).
Potassium tetracuprate(II)
For ditermine Fe3+is used such complex compound:
Potassium cyanide cuprate(II).
Cupper potassium tetracyanate.
Potassium hexacyanoferate(III).
*Potassium hexacyanoferate(II).
Potassium tetracuprate(II)
What micro element is in erythrocytes?
Sodium.
Vanadium.
Fluorine.
Bromine.
*Iron.
What element is in bones?
Sodium.
Vanadium.
Fluorine.
*Calcium.
Iron.
What element is privation in organism decopmost activiti of thyroid gland:
Sodium.
Vanadium.
*Iodine.
Calcium.
Iron.
What reagent is used for determination Ca2+ in solution?
*(NH4)2C2O4.
NaBr.
HCl.
HNO3.
KCl.
Aluminium is:
s - element.
d - element.
f - element.
*p - element.
g - element
Sodium is:
*s - element.
d - element.
f - element.
p - element
g - element
Potassium is:
*s - element.
d - element.
f - element.
p - element.
g - element
Iron is:
s - element.
*d - element.
f - element.
p - element.
E.
145.
A.
B.
C.
D.
E.
146.
A.
B.
C.
D.
E.
147.
A.
B.
C.
D.
E.
148.
A.
B.
C.
D.
E.
149.
A.
B.
C.
D.
E.
150.
A.
B.
C.
D.
E.
151.
A.
B.
C.
D.
E.
152.
A.
B.
C.
D.
E.
153.
A.
B.
C.
D.
E.
154.
A.
g - element.
Magnesium is:
*s - element.
d - element.
f - element.
p - element.
g - element.
Iodine is:
s - element.
d - element.
f - element.
*p - element.
g - element.
Calcium is:
*s - element.
d - element.
f - element.
p - element.
g - element.
Fluorine is:
s - element.
d - element.
f - element.
*p - element.
g - element.
Chlorine is:
s - element.
d - element.
f - element.
*p - element.
g - element.
Bromine is:
s - element.
d - element.
f - element.
*p - element.
g - element.
Manganese is:
s - element.
*d - element.
f - element.
p - element.
g - element.
Zinc is:
s - element.
*d - element.
f - element.
p - element.
g - element.
What is name of K2[Cu (CN)4]?
Potassium cyanide cuprate(II).
Cupper potassium tetracyanate.
*Potassium tetracyanocuprate(II).
Potassium cyanatecuprate(II).
Potassium tetracuprate(II).
What is name of [Ag(NH3)2]OH?
*Diamminesilver(I) hydroxide.
B.
C.
D.
E.
155.
A.
B.
C.
D.
E.
156.
A.
B.
C.
D.
E.
157.
A.
B.
C.
D.
E.
158.
A.
B.
C.
D.
E.
159.
A.
B.
C.
D.
E.
160.
A.
B.
C.
D.
E.
161.
A.
B.
C.
D.
E.
162.
A.
B.
C.
D.
E.
163.
A.
B.
C.
D.
Ammine argentums.
Silver hydroxide.
Ammine hydroxide.
Silver amide.
What is name of [Ag(NH3)2]Cl?
Diamminesilver(I) hydroxide.
Ammine argentums.
Silver hydroxide.
Ammine hydroxide.
*Diamminesilver(I) chloride.
What is name of [Cr(H2O)6](NO3)3?
Sodium hexahydroxochromate (IV).
*Hexaaquachromium(III)nitrate.
Tetracorbonylnickel.
Sodium tetrahydroxoaluminate.
Sodium hexahydroxostannate (IV).
What is name of [Ni(CO)4]?
*Tetracorbonylnickel.
Nickel carbonate.
Nickel carbon.
Nickel carbon monoxide.
Tetraammine nicol(II)bromite.
What is name of [Pt (NH3)4][PtCl6]?
Hexachloroplatinum(II) platinate (IV).
Platinum(II)hexachloroplatinate (IV).
*Tetraammineplatinum(II)hexachloroplatinate (IV).
Tetraccholoplatinum(III) chloride.
Tetraamminecopper(II)bromite.
What is name of [Cu(NH3)4]Br2?
Hexaaquachromium(III)nitrate.
Diamminesilver(I) chloride.
Tetraammineplatinum(II)hexachloroplatinate (IV).
Tetracorbonylnickel.
*Tetraamminecopper(II)bromite
What is name of Na[Al(OH)4]?
Aluminum sodium.
*Sodium tetrahydroxoaluminate.
Potassuin bicyanobis(oxalo)nikelate(II).
Sodium hydroxide.
Aluminum sulfate.
What is name of Na2[Sn(OH)6]?
*Sodium hexahydroxostannate (IV).
Tetraammineplatinum(II)hexachloroplatinate (IV).
Diamminesilver(I) hydroxide.
Hexaamminenickel(II) bromide.
Sodium tetrahydroxoaluminate.
What is name of K4[Ni(CN)2(OOC-COO)2]?
Diamminenicel(I) hydroxide.
Tetraammineaquachlorocobalt(III) chloride
Tetraammineplatinum(II)hexachloroplatinate (IV).
Hexaamminenickel(II) bromide.
*Potassuin bicyanobis(oxalo)nikelate(II).
What is name of [Co(NH3)4(H2O)Cl]Cl2?
Potassium cyanide cuprate(II).
Cupper potassium tetracyanate.
Potassium tetracyanocobalt(II).
*Tetraammineaquachlorocobalt(III) chloride.
E.
164.
A.
B.
C.
D.
E.
165.
A.
B.
C.
D.
E.
166.
A.
B.
C.
D.
E.
167.
A.
B.
C.
D.
E.
168.
A.
B.
C.
D.
E.
169.
A.
B.
C.
D.
E.
170.
A.
B.
C.
D.
E.
171.
A.
B.
C.
D.
E.
172.
A.
B.
C.
D.
E.
173.
A.
Diamminesilver(I) hydroxide.
What is ligand name in following complex compound K2[Cu (CN)4]?
Cyanide.
*Cyano.
Nitroso.
Nitro.
Ammine.
What is central ion in complex compound [Cu(NH3)4]CrO4?
Ammine.
*Cupper.
Chromium.
Oxygen.
Hydrogen.
What is dentaty of ligand in following complex compound [Ni(CO)4]?
*1.
2.
0.
4.
6.
What kind is the following complex compound [Cr(Н2О)6](OH)3?
Acidic complex.
*Cationic complex.
Anionic complex.
Basic complex.
Neutral complex.
What is oxidation number of central ion for the following complex compound [Ni(CO)4]?
1.
*0.
4.
3.
6.
What is ligand name in following complex compound [Cu(NH3)4]CrO4?
Ammonia.
*Amino.
Chromo.
Chromate.
Ammine.
What is central ion in complex compound [Co(NH3)6]CrO4?
Ammine.
*Cobalt.
Chromium.
Oxygen.
Hydrogen.
What is dentaty of ligand in following complex compound [Co(NH3)6]CrO4?
8.
2.
*1.
4.
6.
What is coordination number of Ag in the [Ag(NH3)2]OH?
1.
*2.
8.
4.
6.
What kind is the following complex compound [Co(NO2)(NH3)3]SO4?
Acidic complex.
B.
C.
D.
E.
174.
A.
B.
C.
D.
E.
175.
A.
B.
C.
D.
E.
176.
A.
B.
C.
D.
E.
177.
A.
B.
C.
D.
E.
178.
A.
B.
C.
D.
E.
179.
A.
B.
C.
D.
E.
180.
A.
B.
C.
D.
E.
181.
A.
B.
C.
D.
E.
182.
A.
B.
C.
D.
Anionic complex.
*Cationic complex.
Basic complex.
Neutral complex.
What is oxidation number of central ion for the following complex compound [Co(NO2)2(NH3)3]2+?
0.
1.
3.
*4.
6.
What ligand name, which is in following complex compound K2[Pt C16]?
Potassium.
Platinum.
*Chloro.
Chloral.
Platinate.
What is central ion in complex compound K2[Pt C16]?
Potassium.
*Platinum.
Chloro.
Chloral.
Paladium.
What is coordination number of Co in the [Co(NH3)4(H2O)Cl]Cl2?
1.
2.
8.
4.
*6.
What is dentaty of ligand in following complex compound K2[Pt C16]?
*1.
2.
0.
4.
6.
Coordination number of Ni in the K4[Ni(CN)6]:
1.
2.
8.
4.
*6.
What kind is the following complex compound K4[Ni(CN)2(OOC-COO)2]?
Acidic complex.
Cation complex.
*Anionic complex.
Basic complex.
Neutral complex.
What is dentaty of -OOC-COO- in following complex compound K4[Ni(CN)2(OOC-COO)2]?
1.
*2.
0.
4.
6.
What is coordination number of Sn in the [Sn(NH3)2Cl2]Cl2?
1.
2.
8.
*4.
E. 6.
183. Osmotic pressure of blood is:
A. 8.9 atm.
B. 7.0 atm.
C. 1 atm.
D. 4.7 atm.
E. *7.7 atm.
184. Iron in living organism can be in two forms: heme and non-heme in human body. What compound is
containing non-heme iron?
A. Myoglobin.
B. *Ferritin.
C. Catalases.
D. Peroxidase.
E. Cytochromes.
185. Iron is present as porphyrin form in all compounds except:
A. Myoglobin.
B. Catalases.
C. *Ferritin.
D. Peroxidase.
E. Cytochromes.
186. What oxidation number of iron ion which are present in hemoglobin?
A. +2.
B. 0.
C. +3.
D. +4.
E. +6.
187. Calcium has different biological functions. What function has it with phosphorus?
A. In blood coagulation.
B. Activates the conversion of prothrombin to thrombin.
C. *Bones and teeth formation.
D. In milk clotting.
E. In muscle contraction.
188. 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.
189. What element with calcium is present in bones?
A. Copper.
B. Cobalt.
C. Zinc.
D. Chlorine.
E. *Phosphorus.
190. What element with phosphorus is present in teeth?
A. Copper.
B. Cobalt.
C. *Calcium.
D. Chlorine.
E. Zinc.
191. What element has not in amino acids?
A. Copper.
B. Oxygen.
C. Nitrogen.
D. Hydrogen.
E. Carbon.
192. Qualitative reaction on the CaCl2 is reaction with:
A. NH4NO3.
B. NH4Br.
C. NH4Cl.
D. *(NH4)2C2O4.
E. (NH4)2SO4.
193. What oxidation number of calcium ion which are present in human body?
A. +1.
B. 0.
C. +3.
D. +4.
E. *+2.
194. What oxidation number of sodium ion which are present in human body?
A. +3.
B. 0.
C. *+1.
D. +4.
E. +2.
195. What oxidation number of potassium ion which are present in human body?
A. +3.
B. *+1.
C. 0.
D. +4.
E. +2.
196. What oxidation number of chlorine ion which are present in human body?
A. +3.
B. +1.
C. 0.
D. *-1.
E. +5.
197. Phosphorus in living organism is in form:
A. *PO4-3.
B. P-3.
C. P4.
D. PO2-1.
E. P2O5.
198. Complex compounds are all except:
A. [Cu (NH3)4] SO4.
B. [Co(NH3)4(H2O)Cl]Cl2.
C. K2[Pt C16].
D. *CuSO4.
E. [Sn(NH3)2Cl2]Cl2.
199. The donor atoms, molecules or anions, which donate а pair of electrons to the metal atom and form coordinate bond with it are called
A. Central metal.
B. *Ligands.
C. C.Indicator.
D. Titrant.
E. Analyte.
200. Compound in which the central metal atom is linked to а number of ions or neutral molecules by
coordinate bonds.
A. *Coordination compound.
B. Base.
C. Oxide.
D. Alloy.
E. Acid.
201. The species formed by linking of а number of ions or molecules by co-ordinate bonds to the central
metal atom (or ion) carries positive or negative charge, it is called:
A. Acid.
B. Base.
C. *Complex ion.
D. Oxide.
E. Alloy.
202. The total number of monodentate ligands (plus double the number of bi dentate ligands if any) attached
to the central metal ion through coordinate bonds is called:
A. Oxidation number of the metal ion.
B. Oxidation state of the metal ion.
C. Dentaty of the metal ion.
D. Charge of the metal ion.
E. *Coordination number of the metal ion.
203. Neutral ligands are all except:
A. NН3.
B. Н2О.
C. CO.
D. *Cl-.
E. CS.
204. Negative ligand is:
A. NН3.
B. *Cl-.
C. Н2О.
D. CO.
E. CS.
205. Neutral ligand is:
A. NO3-.
B. *Н2О.
C. CO3-.
D. ClO2+.
E. NO+.
206. Positive ligand is:
A. NO3-.
B. Н2О.
C. CO3-.
D. *ClO2+.
E. NO
207. Complex compound is:
A. Cu3(PO4)2.
B. CoCl3.
C. *K2[Pt C16].
D. CuSO4.
E. SnCl4.
208. 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.
209. Henry’s law equation is:
A. ΔTboiling = Tboiling (solution)-Tboiling (solvent)=KbCm.
B. P1 = X1 P10.
C. C.*X = KP.
D. ΔTfreezing=Tfreezing (solvent)-Tfreezing (solution)=KfreezingCm.
E. PV= nRT.
210. Freezing point determination equation is:
A. ΔTboiling = Tboiling (solution)-Tboiling (solvent)=KbCm.
B. P1 = X1 P10.
C. X = KP.
D. *ΔTfreezing=Tfreezing (solvent)-Tfreezing (solution)=KfreezingCm.
E. PV= nRT.
211. Van’t Hoff law equation is:
A. ΔTboiling = Tboiling (solution)-Tboiling (solvent)=KbCm.
B. P1 = X1 P10.
C. X = KP.
D. ΔTfreezing=Tfreezing (solvent)-Tfreezing (solution)=KfreezingCm.
E. *PV= nRT.
212. Raoult’s law equation is:
A. Δ Tboiling = Tboiling (solution)-Tboiling (solvent)=KbCm.
B. *P1 = X1 P10.
C. X = KP.
D. ΔTfreezing=Tfreezing (solvent)-Tfreezing (solution)=KfreezingCm.
E. PV= nRT.
213. Boiling-point elevation equation is:
A. *ΔTboiling = Tboiling (solution)-Tboiling (solvent)=KbCm.
B. P1 = X1 P10.
C. X = KP.
D. ΔTfreezing=Tfreezing (solvent)-Tfreezing (solution)=KfreezingCm.
E. PV= nRT.
214. Properties of a solution which depend only on the concentration of the solute and not upon its identity
are called:
A. *Colligative properties.
B. Physiological properties.
C. Chemical properties.
D. Physical phenomenon.
E. Chemical phenomenon.
215. Ebolyscopy this:
A. The method for determination of molar mass of compounds by freezing-point depression.
B. The method for determination boiling temperature.
C. *The method for determination of molar mass of compounds by boiling-point elevation.
D. The method for determination osmosis.
E. The method for determination solubility.
216. On value freezing-point depression and boiling-point elevation influence …… of solution.
A. Molarity.
B. Normality.
C. Mass fraction.
D. *Molality.
E. Volume fraction.
217. Solution of Na2CO3*10 H2O can use as primary standert on:
A. *Acid-base titration.
B. Chelatometry.
C. Precipitation.
D. Oxidation - reduction titration.
E. Sedimentation.
218. What indicator are you used on permanganatometry?
A. Potassium chromate.
B. Methyl red.
C. *Indicatorless.
D. Erichrom black T.
E. Methil orange.
219. Titrimetric methods are all except:
A. Complexometry.
B. Neutralization.
C. Precipitation.
D. Oxidation-redaction.
E. *Potentiometry.
220. Titrimetric method classified into four groups based on the:
A. *Type of reaction involved.
B. Acidity of reactive medium.
C. Concentration unit of solution.
D. Oxidation number of elements.
E. Physical properties of titrant.
221. Complexometric titrations are methods in which ….
A. An acidic or basic titrant reacts with an analyte that is a base or an acid.
B. Titrant is an oxidizing or reducing agent.
C. *Involving a metal-ligand complexation reaction.
D. The analyte and titrant react to form a precipitate.
E. Titrant reacts with an analyte by diffusion.
222. Acid-base titrations are methods in which ….
A. *An acidic or basic titrant reacts with an analyte that is a base or an acid.
B. Titrant is an oxidizing or reducing agent.
C. Involving a metal-ligand complexation reaction.
D. The analyte and titrant react to form a precipitate.
E. Titrant reacts with an analyte by diffusion.
223. Redox titrations are methods in which ….
A. An acidic or basic titrant reacts with an analyte that is a base or an acid.
B. *Titrant is an oxidizing or reducing agent.
C. Involving a metal-ligand complexation reaction.
D. The analyte and titrant react to form a precipitate.
E. Titrant reacts with an analyte by diffusion.
224. Precipitation titrations are methods in which ….
A. An acidic or basic titrant reacts with an analyte that is a base or an acid.
B. Titrant is an oxidizing or reducing agent.
C. Involving a metal-ligand complexation reaction.
D. *The analyte and titrant react to form a precipitate.
E. Titrant reacts with an analyte by diffusion.
225. Quantitative chemical analysis carried out by determining the volume of solution of accurately known
concentration which is required to react quantitatively with a measured volume of a solution of the
substance to be determined is called:
A. Potentiometry.
B. Sedimentation.
C. Flocculation.
D. *Titrimtric analysis.
E. Gravimetric analysis.
226. End points in acid-base titration were determined using:
A. Erichrom black T.
B. Potassium chromate.
C. *Methil orange.
D. Potassium permanganate.
E. Iodin.
227. End points in argentometry were determined using:
A. Erichrom black T.
B. Potassium chromate.
C. Methil orange.
D. *Potassium chromate.
E. Iodin.
228. End points in complexometric were determined using:
A. *Erichrom black T.
B. Potassium chromate.
C. Methil orange.
D. Potassium chromate.
E. Iodin.
229. Solubility product of PbCl2 is:
A. Ksp = [Pb2+]2[Cl-].
B. Ksp = [Cl-]2.
C. Ksp = [Pb2+][Cl-].
D. *Ksp = [Pb2+][Cl-]2.
E. Ksp = [Pb2+].
230. Solubility product of BaSO4 is:
A. *Ksp = [Ba2+][SO4-2].
B. Ksp = [SO4-]2.
C. Ksp = [Ba+][Cl-].
D. Ksp = [Ba2+][ SO4-]2.
E. Ksp = [Ba2+].
231. Solubility product of Ag2CrO4 is:
A. Кsp = [Ag+] [CrO4-]2.
B. Кsp = [Ag+].
C. Кsp = [Ag+][NO3-].
D. *Кsp = [Ag+ ]2[CrO4-2].
E. Кsp = [Ag]2.
232. What equation is equation of buffers act, when hydrochloric acid is added to the phosphate buffer
solution is?
A. СН3СООН + NaOH = СН3COONa + Н2О.
B. *Na2HPO4 + HCI = NaH2PO4 + NaCl.
C. СН3СООNа + HCI = СН3СООН + NaCI.
D. NaHCO3+ HCI = H2CO3 + NaCI.
E. NH2RCOONa + HCI = NH2RCOOH + NaCI.
233. What equation is equation of buffers act if hydrochloric acid is added to the acetate buffer solution?
A. СН3СООН + NaOH = СН3СООNa + Н2О.
B. Na2HPO4 + HCI = NaH2PO4 + NaCl.
C. *СН3СООNа + HCI = СН3СООН + NaCI.
D. NaHCO3+ HCI = H2CO3 + NaCI.
E. NH2RCOONa + HCI = NH2RCOOH + NaCI.
234. What equation is equation of buffers act, when hydrochloric acid is added to the bicarbonate buffer
solution?
A. СН3СООН + NaOH = СН3СООNa + Н2О.
B. Na2HPO4 + HCI = NaH2PO4 + NaCl.
C. СН3СООNа + HCI = СН3СООН + NaCI.
D. *NaHCO3+ HCI = H2CO3 + NaCI.
E. NH2RCOONa + HCI = NH2RCOOH + NaCI.
235. What equation is equation of buffers act, when hydrochloric acid is added to the protein buffer solution?
A. СН3СООН + NaOH = СН3СООNa + Н2О.
B. Na2HPO4 + HCI = NaH2PO4 + NaCl.
C. СН3СООNа + HCI = СН3СООН + NaCI.
D. NaHCO3+ HCI = H2CO3 + NaCI.
E. *NH2RCOONa + HCI = NH2RCOOH + NaCI.
236. What equation is equation of buffers act, when hydrochloric acid is added to the hemoglobine buffer
solution?
A. *NaHb + HCI = HHb + NaCl.
B. Na2HPO4 + HCI = NaH2PO4 + NaCl.
C. СН3СООNа + HCI = СН3СООН + NaCI.
D. NaHCO3+ HCI = H2CO3 + NaCI.
E. NH2RCOONa + HCI = NH2RCOOH + NaCI.
237. What equation is equation of buffers act, when hydrochloric acid is added to the oxihemoglobine buffer
solution?
A. *NaHbO2 + HCI = HHbO2 + NaCl.
B. Na2HPO4 + HCI = NaH2PO4 + NaCl.
C. СН3СООNа + HCI = СН3СООН + NaCI.
D. NaHCO3+ HCI = H2CO3 + NaCI.
E. NH2RCOONa + HCI = NH2RCOOH + NaCI.
238. What equation is equation of buffers act when, sodium hydroxide is added to the acetate buffer solution?
A. * СН3СООН + NaOH = СН3СООNa + Н2О.
B. NaH2PO4 + NaOH = Na2HPO4 + Н2О.
C. HHbO2+ NaOH = NaHbO2 + Н2О.
D. H2CO3+ NaOH = NaHCO3 + Н2О.
E. NH2RCOOH + NaOH = NH2RCOONa + Н2О.
239. What equation is equation of buffers act when, sodium hydroxide is added to the phosphate buffer
solution?
A. СН3СООН + NaOH = СН3СООNa + Н2О.
B. *NaH2PO4 + NaOH = Na2HPO4 + Н2О.
C. HHbO2+ NaOH = NaHbO2 + Н2О.
D. H2CO3+ NaOH = NaHCO3 + Н2О.
E. NH2RCOOH + NaOH = NH2RCOONa + Н2О.
240. What equation is equation of buffers act when, sodium hydroxide is added to the bicarbonate buffer
solution?
A. СН3СООН + NaOH = СН3СООNa + Н2О.
B. NaH2PO4 + NaOH = Na2HPO4 + Н2О.
C. HHbO2+ NaOH = NaHbO2 + Н2О.
D. *H2CO3+ NaOH = NaHCO3 + Н2О.
E. NH2RCOOH + NaOH = NH2RCOONa + Н2О.
241. What equation is equation of buffers act when, sodium hydroxide is added to the protein buffer solution?
A. HHbO2+ NaOH = NaHbO2 + Н2О.
B. NaH2PO4 + NaOH = Na2HPO4 + Н2О.
C. СН3СООH + NaOH = СН3СООNa + Н2О.
D. H2CO3+ NaOH = NaHCO3 + Н2О.
E. *NH2RCOOH + NaOH = NH2RCOONa + Н2О.
242. What equation is equation of buffers act, when sodium hydroxide is added to the hemoglobine buffer
solution?
A. HHbO2+ NaOH = NaHbO2 + Н2О.
B. NaH2PO4 + NaOH = Na2HPO4 + Н2О.
C. СН3СООН + NaOH = СН3СООNa + Н2О.
D. H2CO3+ NaOH = NaHCO3 + Н2О.
E. *HHb + NaOH = NaHb + Н2О.
243. What equation is equation of buffers act when, sodium hydroxide is added to the oxihemoglobine buffer
solution?
A. СН3СООН + NaOH = СН3СООNa + Н2О.
B. NaH2PO4 + NaOH = Na2HPO4 + Н2О.
C. *HHbO2+ NaOH = NaHbO2 + Н2О.
D. H2CO3+ NaOH = NaHCO3 + Н2О.
E. HHb + NaOH = NaHb + Н2О.
244. What is compound increased solubility, if temperature is increased also?
A. Nitrogen (IV) oxide.
B. *Potassium nitrate.
C. Oxygen.
D. Carbon (II) oxide.
E. Sulfur (ІV) oxide.
245. It is impossible add water into the concentrated sulfuric acid, because:
A. Water has the greater heat capacity then acid.
B. Water has the less viscosity then acid.
C. *Water is boiling in surface of acid and the heat released will cause the acid to spatter.
D. Concentrated sulfuric acid cannot dissolve in such case.
E. Concentrated sulfate acid is a strong oxidant.
246. Saturated solution is:
A. Solution with particles which cannot observe in ultramicroscopes.
B. Solution with particles which can observe in microscopes.
C. *The highest concentration of solute which a solution can have and be in equilibrium with any
undissolved solute with which it is placed in contact.
D. Solution is unstable and its solute tends eventually to crystallize out of solution.
E. Solution with particles which can observe by eye.
247. Solids solubility usually decrease with:
A. Increasing pressure.
B. Decreasing pressure.
C. C.*Decreasing temperature.
D. Increasing size of solute particles.
E. Increasing temperature.
248. As an antiseptic mean in medicine is applied water solution of permanganate potassium with the mass
percent of KMnO4 0.2 %. Haw many grams of KMnO4 is needed for prepare 100 g of this solution?
A. 2 g.
B. 0,02 g.
C. *0,2 g.
D. 0,1 g.
E. 20 g.
249. What amount mole of Ca(OH)2 is necessary for neutralization 0.3 mole of phosphoric acid?
A. 10.5 mole.
B. 1 mole.
C. 0.9 mole.
D. *0.45 mole.
E. 0.6 mole.
250. Choose the substance solubility which is increase with increasing pressure:
A. Sodium sulfate.
B. Ethanol.
C. *Nitrogen.
D. Acetic acid.
E. Calcium hydroxide.
251. Choose the correct definition:
A. Vapor pressure of a solution containing a non-volatile solute is equal to the atmospheric pressure.
B. Vapor pressure of a solution containing a non-volatile solute is equal to the molarity of solute.
C. Vapor pressure of a solution containing a non-volatile solute is proportionally to the mass fraction of the
solute.
D. Vapor pressure of a solution containing a non-volatile solute is proportionally to the molality of solute.
E. * Vapor pressure of a solution containing a non-volatile solute is equal to the vapor pressure of the pure
solvent times the mole fraction of the solvent.
252. How many ions are formed after full dissociation of one molecule of potassium phosphate?
A. 5.
B. 2.
C. 3.
D. *4.
E. 6.
253. Solid solution is:
A. Mixture of N2 and О2.
B. Mixture of clay and water.
C. Solution of sand and oil.
D. Solution of copper sulfate.
E. *Alloy of nickel and copper.
254. When cells are placed in а solution with а lower solute concentration (hypotonic solution), so red blood
cells will:
A. *Swell and rupture.
B. No changes.
C. Plasmolisis.
D. The shrinkage.
E. Electrophoresis.
255. Choose the substance solubility which is increase with increasing pressure:
A.
B.
C.
D.
E.
256.
A.
B.
C.
D.
E.
257.
A.
B.
C.
D.
E.
258.
A.
B.
C.
D.
E.
259.
A.
B.
C.
D.
E.
260.
A.
B.
C.
D.
E.
261.
A.
B.
C.
D.
E.
262.
A.
B.
C.
D.
E.
263.
A.
B.
C.
D.
E.
264.
A.
B.
C.
Potassium chloride.
Sugar.
Oil.
D.*Carbon (II) oxide.
Sulfuric acid.
When cells are placed in 5 % solution of sodium chloride so red blood cells will:
Hemolisis.
No changes
*Plasmolisis.
The swell and rupture.
Electrophoresis.
A supersaturated:
*Solution is in which the concentration of solute is greater than its concentration in a saturated solution.
Solution is in which the concentration of solute is less than its concentration in a saturated solution.
Solution is in which the concentration of solute is less than 1 mole.
Solution is in which the concentration of solute same as solubility.
Solution is in which the concentration of solute less then solubility.
It is used 20 g of magnums nitrate for prepare 400 g solution. What is mass percent of this solution?
40 %.
20 %.
0,1 %.
10 %.
*5 %.
What is unit of gas solubility in water:
By mole per 1000g of solvent.
By mole.
By percent solute.
*By mole per milliliter of solvent.
By grams.
Hemolysis is phenomenon when cells are placed in а sodium chlorate solution with:
0,9 %.
2,9 %.
*0,5 %.
1,5 %.
2,5 %.
Value of osmotic pressure is charecterised by:
Mendeleev-Сlapeyron law.
Raoult’s law.
Henry’s law.
Henderson-Hasselbalch law.
*van’t Hoff law.
Choose the substance solubility which is increase with increasing temperature:
*Sodium sulfate.
Carbon (ІV) oxide.
Oxygen.
Sulfur (ІV) oxide.
Nitrogen.
Solid solution is:
Mixture of NH3 and H2.
Mixture of clay and water.
Solution of sand and oil.
*Alloy of copper and aluminum.
Solution of sodium sulfate.
True solution is solution with:
*The sizes of particles less than 10-9 m.
The sizes of particles 10-7-10-9 m.
The sizes of particles more then 10-5 m.
D. The sizes of particles 10-5-10-3 m.
E. The sizes of particles 10-7-10-5 m.
265. Mass percent is:
A. *Mass of solute which is in 100 g of solution.
B. Mass of solute which is in 100 g of solvent.
C. Amount mole equivalents of solute which is in 1 liter of solution.
D. Amount moles of solute which is in 100 g of solution.
E. Amount moles of solute which is in 100 g of solvent.
266. 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.
267. It is used stable temperature and pressure for the most processes in chemical technology. What name is
process?
A. Isochoric - Isothermel.
B. *Isobar - Isothermic.
C. Isobar - Isochoric.
D. Isochoric - Adiabatic.
E. Isothermal - Adiabatic.
268. Standard state of a system is state when:
A. 101,3 kPa, 0 0K.
B. 101,3 kPa, 273 0K.
C. *101,3 kPa, 298 0K.
D. 50 kPa, 273 0K.
E. 50 kPa, 298 0K.
269. The state of the system, when it composition and function does not change in time is called:
A. Isochoric.
B. Adiabatic
C. Isothermal.
D. Isobar.
E. *Equilibrium.
270. The standard enthalpy of combustion (ΔН°combustion) equal zero for such compound:
A. *O2, Н2.
B. СО2, Н2О.
C. NO, NH3.
D. P2O3, PH3.
E. NO2, N2H4.
271. For an isochoric process the Heat effect equal:
A. Zero.
B. Change of enthalpy.
C. *Change of internal energy.
D. Change of entropy.
E. Change of free Gibbs’s energy.
272. The first law equation is:
A. dH = dQ + dE
B. Q=A+W
C. Q = dHW
D. *Q = U + W
E. S = dG + W
273. 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.
E.
274.
A.
B.
C.
D.
E.
275.
A.
B.
C.
D.
E.
276.
A.
B.
C.
D.
E.
277.
A.
B.
C.
D.
E.
278.
A.
B.
C.
D.
E.
279.
A.
B.
C.
D.
E.
280.
A.
B.
C.
D.
E.
281.
A.
B.
C.
D.
E.
282.
A.
B.
C.
D.
E.
283.
Hess’s law.
Kirchhoff’s law.
Heat effect of reaction oxidation 1 mole of compound at standard state is called:
Standard enthalpy of dissolved.
Standard enthalpy of neutralization
Standard enthalpy of formation.
*Standard enthalpy of combustion.
Standard enthalpy of precipitation.
Thermodynamics systems are classified by amount of phases into:
Exogenous and endogenous.
Solid, liquid, gas.
*Homogeneous and heterogeneous.
Isolated, opened, closed
Reversible and irreversible.
When temperature is stable this process is called?
Isolated.
Isobaric.
Isochoric.
Adiabatic.
*Isothermic.
Normal state is state when:
101,3 kPa, 0 0K.
*101,3 kPa, 273 0K.
101,3 kPa, 298 0K.
50 kPa, 273 0K.
50 kPa, 298 0K.
Measure of randomness or disorder of the system is:
Heat.
Work.
Enthalpy.
*Entropy.
Internal energy.
The equation for pressure-volume work at isobar expansion is:
W= VS
W= pQ
*W = p ΔV
W=nRTln(V2/V1)
W=nRT (V2/V1)
Temperature dependence of heat effect of reaction is studied such law:.
First law of thermodynamics.
Second law of thermodynamics.
Third law of thermodynamics.
*Kirchhoff’s law.
Hess’s law.
If а system can exchange only energy with the surroundings but not matter, it is called:
Exogenous.
*Closed
Homogenous.
Isolated.
Opened.
If system can exchange both matter and energy with the surroundings, it is called:
Exogenous.
Closed
Homogenous.
Isolated.
*Opened.
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
284. 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.
285. 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.
286. The concept “The total amount of heat evolved or absorbed in a reaction depends only upon the nature
of the initial reactants and that of the final products and does not depend upon the path by which this change
is brought about” is:
A. First law of thermodynamics.
B. Second law of thermodynamics.
C. Third law of thermodynamics.
D. *Hess’s law.
E. Kirchhoff’s law.
287. Formula: dS = ΔQ/T is expression of:
A. First law of thermodynamics.
B. Second law of thermodynamics.
C. *Third law of thermodynamics.
D. Hess’s law.
E. Kirchhoff’s law.
288. In spontaneous processes the Gibbs’s energy is:
A. Maximal.
B. Zero.
C. Minimal.
D. *Negative.
E. Positive
289. The spontaneous processes are in such circumstances:
A. G0, S<0.
B. G0, S  0.
C. G=0, S=0.
D. *D. G<0, S>0.
E. G>0, S<0.
290. The non spontaneous processes are in such circumstances:
A. G0, S<0.
B. G0, S  0.
C. G=0, S=0.
D. G<0, S>0.
E. *G>0, S<0.
291. The equilibrium state is in such circumstances:
A. G0, S<0.
B. G0, S  0.
C. G=0, S=0.
D. G<0, S>0.
E. G>0, S<0.
292. Chemical kinetics studies:
A. Properties of solutions.
B. *Speed of chemical reactions and its dependence on the different factors.
C. Buffer systems of blood.
D. pH of solutions.
E. Oxidation- reduction reactions.
293. 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
294. Rate constant is:
A. *k = υ if concentration of reagents equal one unit.
B. Degree of precipitation.
C. Mass constant.
D. k = υ if concentration of reagents equal 0.1.
E. k = υ if concentration of reagents equal 10.
295. 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 .
296. 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.
297. 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.
298. Reversible system is:
A. System which consists of one phase.
B. System which consists of two more phases.
C. Consist liquid and gas phases.
D. System which consists of five phases.
E. *System which is carried out infinitestimally.
299. 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.
300. 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.
301. Vant-Goff rule:
A. *Rate of homogeneous chemical reaction is increase in two - four times when temperature is increase on
10 0С.
B.
C.
D.
E.
302.
A.
B.
C.
D.
E.
303.
A.
B.
C.
D.
E.
304.
A.
B.
C.
D.
E.
305.
A.
B.
C.
D.
E.
306.
A.
B.
C.
D.
E.
307.
A.
B.
C.
D.
E.
308.
A.
B.
C.
D.
E.
309.
A.
B.
C.
D.
E.
310.
A.
B.
C.
D.
Total mass of chemical reaction reagent equal total mass of products.
Energy is stable.
Properties of elements, and they derivative are depended on atoms weight.
Heat effect of reaction is constant, when is formed same reagents.
An empirical quantity, and obtained from thy experimental rate law is:
Rate constant.
Molecularity.
*Reaction order.
Mass constant.
Stoichiometric coefficient.
An elementary reaction proposed as an individual step in а mechanism is:
Rate constant.
*Molecularity.
Reaction order.
Mass constant.
Stoichiometric coefficient.
For rate constant influence all factors except:
*Concentration of the reactants.
Temperature.
Pressure.
Surface area of the reactants.
Nature of reagents.
What factors are influence for rate constant?
Concentration of the reactants.
Indicator.
Dispersed phase.
Surfactant.
*Nature of reagents.
What factors influence for rate of reaction?
*Concentration of the reactants.
Indicator.
Dispersed phase.
Surfactant
Surface tension.
Rate law equation for reaction: 2 SO2 (g) + O2 (g) →2 SO3 (g) is:
υ = k [SO3]2 [O2].
υ = k 2[SO2] [O2].
* υ = k [SO2]2 [O2].
υ = k [O2].
υ = k [SO3].
Rate law equation for reaction: 2 SO3 (g) → 2 SO2 (g) + O2 (g) is:
* υ = k [SO3]2.
υ = k 2[SO2] [O2].
υ = k [SO2]2 [O2].
υ = k [O2].
υ = k [SO2].
Rate law equation for reaction: 2 NO (g) + O2 (g) ↔2 NO2 is:
υ= k [NO2]2.
*υ= k [NO]2 [O2].
υ= k [NO] [O2].
υ = k [O2].
υ = k 2[NO2].
The mass-action expression for reversible reaction: N2 (g) + 3H2 (g) ↔ 2NH3 (g):
K= [N2]2/ [NH3]2
K= [N2]3 [H2].
*K= [NH3]2 / [N2] [H2]3
K=[H2].
E. K=[N2] [H2]3
311. The mass-action expression for reversible reaction: 3O2 (g) + 2H2S (g) → 2H2O (g) + 2SO2 (g):
A. K= [O2]3/ [H2O]2
B. K= [H2S] [O2]3.
C. K= [SO2]2 / [O2] [H2S]
D. K= [O2] /[ H2O]+ [SO2]
E. *K= [SO2]2[H2O]2 / [O2]3[H2S]2
312. Rate law equation for reaction: 2 NH3
2 (g) + 3H2 (g) is:
A. *υ= k [N2] [H2]3
B. υ= k [N]2 [H2].
C. υ= k [NH2]3
D. υ= k [O2].
E. υ= k [N2]2.
313. 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.
314. Matters, which increase activity of catalyst named:
A. *Promoter (activator)
B. Inhibitors
C. Hormones
D. Indicators
E. Enzyme
315. Reactions which are flowing past in two parties: the forward reaction - conducts to formation reaction
product and reverse reaction - decomposing reaction product on mother substances:
A. Series reaction.
B. Parallel reaction.
C. Conjugating reaction.
D. Chain reaction.
E. *Reversible reaction.
316. Reaction, in which products of firs step reaction is reagents for second step reaction is:
A. Reversible reaction.
B. *Series reaction.
C. Parallel reaction.
D. Conjugating reaction.
E. Chain reaction.
317. Reversible reaction is:
A. *А+В ↔ С+D
B. В. А→ В→ С→ D
C.
D.
E.
318.
A.
B.
.
А+В→ М. А+С→N
AВ+О· → АО·+В. СD+AO·→CO·+AD
Chain reaction is:
А+В ↔ С+D
А→ В→ С→ D
C.
D.
E.
319.
A.
.
А+В→ М. А+С→N
*AВ+О· → АО·+В. СD+AO·→CO·+AD
Parallel reaction is:
А+В ↔ С+D
B. А→ В→ С→ D
C.
D.
E.
320.
*
.
А+В→ М. А+С→N
AВ+О· → АО·+В. СD+AO·→CO·+AD
Conjugating reaction is:
A.
B.
C.
D.
E.
321.
A.
B.
C.
D.
.
А+В ↔ С+D
А→ В→ С→ D
*А+В→ М. А+С→N
AВ+О· → АО·+В. СD+AO·→CO·+AD
Series reaction is:
А+В ↔ С+D
*А→ В→ С→ D
А+В→ М. А+С→N
AВ+О· → АО·+В. СD+AO·→CO·+AD
E.
322.
A.
B.
C.
D.
E.
323.
A.
B.
C.
D.
E.
324.
A.
B.
C.
D.
E.
325.
A.
B.
C.
D.
E.
326.
A.
B.
C.
D.
E.
327.
A.
B.
C.
The process in which reagents react with surface of catalyst is named:
*Heterogeneous catalysis.
Homogeneous catalysis.
Positive catalysis.
Negative catalysis.
Autocatalysis.
The catalysis in which rate of reaction increase is named:
Heterogeneous catalysis.
Homogeneous catalysis.
*Positive catalysis.
Negative catalysis.
Autocatalysis.
The catalysis in which rate of reaction decrease is named:
Heterogeneous catalysis.
Homogeneous catalysis.
Positive catalysis.
*Negative catalysis.
Autocatalysis.
The matters which inactive of catalyst named:
Promoters
*Inhibitor
Hormone
Indicator
Enzyme.
The nature of enzyme is:
Carbohydrate.
Lipid
*Protein.
Mineral acid
Vitamin.
Proteins specialized to catalyze biological reactions are:
Polymers.
*Enzymes.
Hormones.
D. Indicators.
E. Vitamin.
328. 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.
329. Catalyst influence for:
A. Ganged of chemical equilibrium.
B. Increase temperature.
C. Increase pressure.
D. *Rate of reaction.
E. Increase volume.
330. It is used as catalyst for hydrolysis starch such compound:
A. *HCl.
B. NaOH.
C. CuSO4.
D. CaCl2.
E. I2.
331. The reaction of hydrolysis starch is:
A. C12H22O11 + H2O → 2C6H12O6.
B. nCO2 + mH2O → Cn(H2O)m + nO2.
C. *(C6H10O5)n + nH2O → nC6H12O6.
D. CH3COOC2H5 + H2O → CH3COOH + C2H5OH.
E. С6Н12О6 + 6О2→ 6СО2+6Н2О
332. Biological catalysts are:
A. Polymers.
B. Vitamin.
C. Hormones.
D. Indicators.
E. *Enzymes.
333. 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.
RT
E  E0 lnQ
nF
334. E in Nernst equation:
is:
A. Mass-action expression.
B. *Electrode potential.
C. Standard electrode potential.
D. EMF.
E. Oxidation potential.
335. The mass-action expression for oxidation-reduction reaction: Fe + CuSO4 = Cu+ FeSO4 is:
A. Q= 1 / [CuSO4].
B. Q= [Fe] / [FeSO4] [Cu].
C. *Q= [Cu][FeSO4] / [CuSO4] [Fe].
D. Q= [Cu] / [CuSO4].
E. Q= [Fe] /[FeSO4].
336. Silver electrode is:
A. *Metal-metal ion electrode.
B. Membrane electrode.
C. Gas-ion electrodes.
D. Metal-insoluble salt-anion electrode.
E. Inert "oxidation-reduction" electrode.
RT
E  E0 lnQ
nF
337. E0 in Nernst equation:
is:
A. Mass-action expression.
B. Electrode potential.
C. *Standard electrode potential.
D. EMF.
E. Oxidation potential.
338. The mass-action expression for half reaction: Zn2+ + 2e- = Zn is:
A. *Q= [Zn] / [Zn2+].
B. Q= [Zn2+]2 / [Zn].
C. Q= [Zn2+] / [Zn].
D. Q= Zn2+ /Zn.
E. Q= 1 / [Zn2+]2.
339. Glass 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.
340. What value of standard electrode potential for standard hydrogen electrode:
A. - 0.34.
B. - 1.22.
C. *0.
D. + 0.15.
E. + 0.220.
341. The mass-action expression for oxidation-reduction reaction 2H+ + 2e- = H2 is:
A. *Q= [H2] / [H+]2
B. Q= pH2 / [H+]
C. Q= pH2 / [H+]2
D. Q= [H+] / pH2
E. Q= [H+]2 / pH2
342. What equation is using for calculated рН solutions in electrochemistry:
A. *Nernst.
B. Arrhenius.
C. Electro-neutrality.
D. Raoult’s.
E. Shredyngare.
343. Diagram of silver-silver chloride electrode is:
A. Pt, H2/2H+.
B. Ме/Меn+.
C. Zn/Zn2+.
D. *Ag/AgCl, KCl.
E. Hg/Hg2Cl2, KCl.
344. Potentiometry is:
A. *Physic-chemical method of research concentration of ions, electrode potential, which used the EMF
measuring.
B. Aggregation of the particles arising from the stabilizing effect of this secondary minimum.
C. Increase of the boiling temperature of solutions.
D. Decline of the freezing temperature of solutions.
E. System, in which a dispersion phase and dispersion medium are liquids, which are non dissolved eth
other.
345. Standard hydrogen electrode this:
A. Platinum lamina is in contact with hydrochloric acid solution.
B. Platinum lamina is in contact with zinc sulfate solution.
C. Platinum lamina is in contact with its ions in solution.
D. *Hydrogen at atmospheric pressure is passed into 1 М НС1 in which foil of the platinized platinum
remains immersed through which inflow or outflow of electrons takes place.
E. A metal is in contact with one of its insoluble salts and also with а solution containing the anion of the
salt
346. What is value of osmotic pressure of blood serum?
A. *7,7 -7,8 atm.
B. 6,2 - 7,3 atm.
C. 8,6-8,9 atm.
D. 2,1 -7,1atm.
E. 10,7-11,4 atm.
347. Standard EMF of the cell equalled:
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.
348. What formula is Nernst equation?
A. E = E0catode - E0anode.
B. *E = E0 - (RT/ nF) ln ([M]/ [Mn+]).
C. pH = - log [H+].
D. pH = 14- pOH.
E. E = 14 - RT/nF
349. The metal - metal ion electrode is electrode, which:
A. Employs а gas in contact with its anion or cation in solution.
B. A metal is in contact with one of its insoluble salts and also with а solution containing the anion of the
salt.
C. Really no more of an oxidation-reduction electrode than any other.
D. Semipermeable membrane.
E. *Consists of а metal in contact with its ions in solution.
350. The gas-ion electrode is electrode, which:
A. *Employs а gas in contact with its anion or cation in solution.
B. A metal is in contact with one of its insoluble salts and also with а solution containing the anion of the
salt.
C. Really no more of an oxidation-reduction electrode than any other.
D. Semipermeable membrane
E. Consists of а metal in contact with its ions in solution.
351. In the metal-insoluble salt-anion electrode is electrode, which:
A. Employs а gas in contact with its anion or cation in solution.
B. *A metal is in contact with one of its insoluble salts and also with а solution containing the anion of the
salt.
C. Really no more of an oxidation-reduction electrode than any other.
D. Semipermeable membrane
E. Consists of а metal in contact with its ions in solution.
352. An inert oxidation-reduction electrode is:
A. Employs а gas in contact with its anion or cation in solution.
B. A metal is in contact with one of its insoluble salts and also with а solution containing the anion of the
salt.
C. *It consists of strip, wire, or of an inert material, say, platinium, in contact with a solution, which
contains ions of a substance, is two different oxidation states.
D. Semipermeable membrane.
E. Consists of а metal in contact with its ions in solution.
353. The difference between the electrode potentials of the two half cell is known as:
A. *Electromotive force (EMF) of the cell or cell potential or cell voltage.
B. Masse-action.
C. Mole mass.
D.
E.
354.
A.
B.
C.
D.
E.
355.
A.
B.
C.
D.
E.
356.
A.
B.
C.
D.
E.
357.
A.
B.
C.
D.
E.
358.
A.
B.
C.
D.
E.
359.
A.
B.
C.
D.
E.
360.
A.
B.
C.
D.
E.
361.
A.
B.
C.
D.
E.
362.
A.
B.
C.
D.
E.
363.
Molarity.
Solubility product.
Processes, which are between interfaces of two systems is:
Coagulation.
*Surface phenomena.
Surface tension.
Absorption.
Boiling.
The equation, which is used for calculate surface tension is:
*σ = G/S.
σ = GS.
σ = S/G.
σ = νRT.
σ = C/RT.
The surfactants are compound, except:
Alcohols.
Alkalis.
Salts of fat acids.
Protein.
*Hidrochloric acid..
Energy, which have molecules on surface is:
Enthalpy.
Entropy.
Heat.
Work.
*Free Gibbs’s energy.
The force in dynes acting upon a line cm long on the surface of the liquid is:
*Surface tension.
Entropy.
Enthalpy.
Heat.
Pressure.
Value of surface free Gibb's energy depends on:
Decrease of pressure.
Volume of liquids.
Form of glass.
*Nature of matter.
Freezing temperature.
What concept is correct?
Surfactant increase surface tension at twice.
Surfactant does not influece on surface tension value.
Surfactant increase surface tension at 4 times.
*Surfactant decrease surface tension.
Surfactant increase surface tension in 3 times.
The surfactant is:
Hydrochloric acid.
Calcium hydroxide.
Sodium chloride.
*Isoamil alcohol.
Potassium.
The surfactant is all compounds except:
Alcohols.
Fatty acids.
*Sodium chloride.
Amino acids.
Proteins.
Surface tension is measured by such unit:
A.
B.
C.
D.
E.
364.
A.
B.
C.
D.
E.
365.
A.
B.
C.
D.
E.
366.
A.
B.
C.
D.
E.
367.
A.
B.
C.
D.
E.
368.
A.
B.
C.
D.
E.
369.
A.
B.
C.
D.
E.
370.
A.
B.
C.
D.
E.
371.
A.
B.
C.
D.
E.
372.
A.
B.
*J/m2
N/m2
J/m
J/sm
N/dm2
Surface tension is measured by such unit:
J/sm
*N/m
J/m
N/sm2
N/dm2
What method is used for determination surface tension:
Potentiometry.
Chelatometry.
*Stalagmometric method.
Chromatography.
Criometry.
The concentrated one component in the surface other is named:
Absorption.
*Adsorption.
Disorbsion.
Solubility.
Capillary condensation.
What concept is correct?
Surfactant increase surface tension at twice.
Surfactant does not change surface tension.
Surfactant increase surface tension at 4 times.
*Surface inactive compound increase surface tension.
Surfactant increase surface tension in 3 times.
Adsorption is:
*The phenomenon of concentrated the molecules of а substance on the surface of а liquid or а solid
resulting.
Chemical reaction between adsorbed and adsorbate.
When molecules have hydrophilic and hydrophobic groups simultaneously.
The separation of mixtures.
The chromatography analysis.
Ionic adsorption this:
The separation of mixtures.
When molecules have hydrophilic and hydrophobic groups simultaneously.
*Chemical reaction between solution ions and ions of adsorbent surface.
The chromatography analysis.
Chemical reaction between adsorbed and adsorbate.
Adsorption of ions is interaction:
Between water and acid.
*Between adsorbent ions and ions of solution.
Between liquids.
Between elements.
Between bases.
At chemical adsorption:
Is formation intramolecule forces between an adsorbed and an adsorbate.
The concentrated one matter in the volume of other.
*Chemical interaction of adsorbent and adsorbate, products to this reaction are in same phase.
There is selective absorption of one kind of electrolyte ions in surface of ion-exchanger.
The separation of compound in mixture at the thin layer of adsorbed.
The rules of selective adsorption are:
Shulce - Hardy.
Duklo - Trauber.
C. *Pescov-Panet-Faiences'.
D. Vant - Goff.
E. Raoult’s.
373. By the rule of selective adsorption an adsorbent must by:
A. To be easily soluble compound.
B. *To have a certain crystalline grate.
C. To be liquid.
D. To be gaseous.
E. To be soluble compound.
374. The phenomenon of attracting and retaining the molecules of а substance on the surface of а liquid or а
solid resulting into a higher concentration of the molecules on the surface is:
A. *Adsorption
B. Adsorbate
C. Adsorbent
D. Desorption
E. Absorption
375. The substance thus adsorbed on the surface is called:
A. Adsorption
B. *Adsorbate
C. Adsorbent
D. Desorption
E. Absorption
376. The substance on which compound is adsorbed is called:
A. Adsorption
B. Adsorbate
C. *Adsorbent
D. Desorption
E. Absorption
377. The reverse processes removal of the adsorbed substance from the surface is called:
A. Adsorption
B. Adsorbate
C. Adsorbent
D. *Desorption
E. Absorption
378. Adsorbate this:
A. *The substance thus adsorbed on the surface.
B. The substance on which compound is adsorbed.
C. Product of reactions.
D. Reagents of reaction.
E. Matter which is absorbed
379. Adsorbent this:
A. The substance thus adsorbed on the surface.
B. *The substance on which compound is adsorbed.
C. Product of reactions.
D. Reagents of reaction.
E. Matter which is absorbed
380. What ion has the greatest adsorptive activity?
A. К+
B. Са+2
C. Fe+3
D. *Sn+4
E. Na+
381. Ion exchange adsorption is:
A. *The adsorption in which ions of solution exchange with surface adsorbent ions.
B. Exchange by electrons
C. The adsorption in which exchange of molecules.
D. Absorption of gases by solids.
E.
382.
A.
B.
C.
D.
E.
383.
A.
B.
C.
D.
E.
384.
A.
B.
C.
D.
E.
385.
A.
B.
C.
D.
E.
386.
A.
B.
C.
D.
E.
387.
A.
B.
C.
D.
E.
388.
A.
B.
C.
D.
E.
389.
A.
B.
C.
D.
E.
390.
A.
B.
C.
D.
E.
391.
A.
The adsorption in which of molecules of solute react with molecules of solvent.
Cation exchange resins is:
OH--exchange resins
СІ- -exchange resins
SO42--exchange resins
*H+- exchange resins
Br -- exchange resins
Anion exchange resins is:
*OH--exchange resins
Na -exchange resins
Ca-exchange resins
H+- exchange resins
K-exchange resins
Adsorption is this:
*Concentrated one matter in surface other.
Transferred matters from solid into the gas state.
Method gravimetry.
Method of separation mixtures into individual compounds.
Chromatography analysis.
Chromatography is this:
Concentrated one matter in surface other.
Transferred matters from solid into the gas state.
Method gravimetry.
*Method of separation mixtures into individual compounds.
Chelatometry analysis.
What ion has the greatest adsorptive activity?
Sr+2
Са+2
*Fe+3
Ba+2
Na+
What ion has the greatest adsorptive activity?
Sr+2
Са+2
Mg+2
*Ba+2
Be+2
Which properties have dispersion systems:
A molecule is structural unit of the system.
Thermodynamics stable system.
Homogeneous system.
*Thermodynamics instable system.
The system has not surface between phases.
What is particle size of colloid solution?
*10-8м.
10-10м.
1015м.
10-3м.
10-1м
Colloid systems have following properties except:
Sedimentation.
*Dinaturation.
Brownian movement effect.
Diffusion.
Osmotic pressure.
Systems, in which particle size10-4 m are:
True solution.
B. *Macroheterogeneous.
C. Microheterogeneous.
D. Ultramicroheterogeneous.
E. Homogeneous.
392. 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.
393. Method preparation of colloid solutions by this reaction 2Н2S+SO2 = 3S+2H2O is called:
A. Peptization..
B. *Oxidation.
C. Electric method.
D. Hydrolysis.
E. Double decomposition.
394. Method preparation of colloid solutions by this reaction 2Na2SO4+CaCl = CaSO4+2NaCl is called:
A. Peptization.
B. Oxidation.
C. Electric method.
D. Hydrolysis.
E. *Double decomposition.
395. Method preparation of colloid solutions by this reaction FeCl3+3H2O= 3HCl + Fe(HO)3 is called:
A. Peptization.
B. Oxidation.
C. Electric method.
D. *Hydrolysis.
E. Double decomposition.
396. What method is used for separation dispersion particles by sizes?
A. *Electrophoreses.
B. Brownian motion.
C. Diffusion.
D. Sedimentation.
E. Osmotic pressure
397. A process of passing of a precipitate into colloidal particles on adding suitable electrolyte is called:
A. *Peptization.
B. Oxidation.
C. Electric method.
D. Hydrolysis.
E. Double decomposition.
398. 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.
399. These methods involve the breaking of the bigger particles to colloidal size.
A. Peptization.
B. Oxidation.
C. Condensation.
D. Hydrolysis.
E. *Dispersion.
400. Systems with dispersed phase particle size between 10-9 to 10-7m are:
A. True solution.
B. Macroheterodisperse solution.
C. Solid.
D. *Colloidal solutions.
E. Mixture.
401. For purification colloidal solution is used such method except:
A. Dialysis
B. *Titration.
C. Electrodialysis.
D. Ultrafiltration.
E. Ultracentrifugation.
402. What purification colloidal solution method is base in “Artificial kidney”?
A. Dialysis.
B. Electrodialysis.
C. *Hemodialysis
D. Ultrafiltration
E. Ultracentrifugation
403. The process which involves the movement of colloidal particles towards one or the other electrode when
placed under the influence of an electric field:
A. *Electrophoresis.
B. Electrodialysis.
C. Hemodialysis.
D. Ultrafiltration.
E. Ultracentrifugation.
404. A phenomenon in which the molecules of the dispersion medium are allowed to move under the
influence of an electric field whereas colloidal particles are not allowed to move:
A. Electrophoresis.
B. Electrodialysis.
C. Hemodialysis.
D. *Electroosmosis.
E. Ultracentrifugation.
405. 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.
406. The minimum amount of an electrolyte (millimoles) that must be added to one liter of а colloidal
solution so as to bring about complete coagulation or flocculation is called:
A. *Coagulation or flocculation value (or threshold) of the electrolyte.
B. Oxidation number.
C. Temperature coefficient.
D. Dissociation degree.
E. Degree of adsorptions.
407. Coagulation this:
A. The process of separating the particles of colloids from those of crystalloids by diffusion of the mixture
through а parchment or an animal membrane.
B. Oxidation of element in colloidal solution.
C. *Aggregation of the particles arising from the stabilizing effect of this secondary minimum.
D. System, in which a dispersion phase and dispersion medium are liquids, which are non dissolved eth
other.
E. Part of chemistry, which studies physical and chemical properties of microheterogeneous system and
HMC.
408. 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.
409. Blood serum is dispersed system. What type dispersed system is it?
A. True solution.
B. Solid.
C. Macroheterogeneous.
D. Microheterogeneous.
E. *Colloidal solution.
410. 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
411. System with size dispersed phase particle equal 10-9 - 10-7 is:
A. True solution.
B. Microheterogeneous.
C. Macroheterogeneous.
D. Homogeneous.
E. *Colloidal solution.
412. Colloidal solutions have some stability. What factors influence for they stability?
A. *Electrokinetic ξ -potential.
B. Pressure.
C. Volume of systems.
D. Catalysts.
E. Indicators.
413. Colloidal solutions have some stability. Stability is the greatest when:
A. Thermodynamics (φ)-potential same as electrokinetic ξ-potential.
B. Thermodynamics (φ)-potential greater then electrokinetic ξ-potential.
C. *Thermodynamics (φ)-potential lest then electrokinetic ξ-potential.
D. Both equal zero.
E. Electrokinetic ξ -potential equal zero.
414. Coagulants and anticoagulants are used in medicine and pharmacy. What coagulation (flocculation)
value?
A. Amount of strong acid.
B. .Amount of base.
C. Minimum amount of non electrolytes.
D. Amount of stabilisator.
E. *The minimum amount of an electrolyte (millimoles) that must be added to one liter of а colloidal
solution so as to bring about complete coagulation or flocculation.
415. The amount of an electrolyte which is added to one liter of а colloidal solution so as to bring about
complete flocculation is called:
A. *Flocculation number.
B. Surface tension.
C. Heat capacity.
D. Acidity.
E. Ion product.
416. Osmotic pressure of colloidal solution is:
A. Very great.
B. Stable all time.
C. Equal zero.
D. *Very small.
E. Chang when change illumination.
417. Phenomenon of mat luminescence of colloid solution at passing of light:
A. Coagulation
B. Peptization.
C. Diffraction
D. *Opalescence
E. Nephelomertry.
418. What polymer is natural?
A. Polyethylene.
B. Kapron.
C. Polypropilen.
D. *Starch.
E. Polyformaldehyde.
419. For swellings influence all factors except:
A. *Time.
B. Temperature.
C. Relation between energies of bond in a polymer and solving energy.
D. Concentrations of polymer
E. Nature polymer.
420. The quantitative measure of swelling is:
A. Change of solution volume.
B. *Swelling degree.
C. Change the nature of polymer.
D. Unchanging amount of polymer.
E. Volume of turgescent polymer.
421. Value of рН solution in which an proteins is in isoelectric state, name ....
A. Solubility of protein.
B. Hydrolysis of protein.
C. *Isoelectric point of protein.
D. Synthesis of protein.
E. Flowdown of protein
422. Hydrogen bonds are typical for such structure of proteins:
A. Quaternary.
B. Primary.
C. *Secondary.
D. Tertiary.
E. Simple.
423. On the swelling process influence all factors except:
A. рН medium.
B. *Catalyst.
C. Nature of polymer and solvent.
D. Molecular mass of polymer.
E. Temperature.
424. What formula is used for determination swelling degree?
A. α = N/n.
B. α = K / C.
C. α = 1- C / m.
D. α = C m / V.
E. *α = (m - m0)/m0 = mp/m0.
425. The amount of liquids which is absorbed one unit of polymer is named:
A. *Swelling degree.
B. Hydrolysis degree.
C. Polymerization degree.
D. Ionizations degree.
E. Condensation degree.
426. High molecular connections (HMC) are compounds with molecular mass of order...
A. 10 - 102 atomic units.
B. *104 – 106 atomic units.
C. 10-1 - 10-2 atomic units.
D. 10 - 103 atomic units.
E. 10-4 - 10-б atomic units.
427. The high molecular compounds (HMC, polymers) are used in pharmacy and medicine. What property of
colloid solution is typical for polymer solutions?
A.
B.
C.
D.
E.
428.
A.
B.
C.
D.
E.
429.
A.
B.
C.
D.
E.
430.
A.
B.
C.
D.
E.
431.
A.
B.
C.
D.
E.
432.
A.
B.
C.
D.
E.
433.
A.
B.
C.
D.
E.
434.
A.
B.
C.
D.
E.
435.
A.
B.
C.
D.
E.
436.
A.
B.
C.
Thermodynamics stability.
Structural viscidity.
*Dispersion of light.
Jeling.
Swelling.
Linked water:
Water which is in the human body.
*Water molecules, which pass to the polymer and form hydrate layers.
Water in food.
Water which is adsorbed polymer after formation hydrate layers.
Creates the compression of the all system.
“Free water”:
Water molecules, which pass to the polymer and form hydrate layers.
Water in the human body.
Water in food.
*Water which is adsorbed polymer after formation hydrate layers.
Creates the compression of the all system.
Silver-silver chloride electrode is:
The metal - metal ion electrode.
The gas-ion electrode is electrode.
*Metal-insoluble salt-anion electrode.
Inert "oxidation-reduction" electrode.
Membrane electrode.
Cu/Cu2+ electrode is:
*The metal - metal ion electrode.
The gas-ion electrode is electrode.
Metal-insoluble salt-anion electrode.
Inert "oxidation-reduction" electrode.
Membrane electrode.
Zn/Zn2+ electrode is:
*The metal - metal ion electrode.
The gas-ion electrode is electrode.
Metal-insoluble salt-anion electrode.
Inert "oxidation-reduction" electrode.
Membrane electrode.
In the metal-insoluble salt-anion electrode is electrode:
Zn/Zn2+ electrode.
*Silver-silver chloride electrode.
Hydrogen electrode.
Glass electrode.
Cu/Cu2+ electrode.
Gas-ion electrode is electrode:
Silver-silver chloride electrode.
Zn/Zn2+ electrode.
*Hydrogen electrode.
Glass electrode.
Cu/Cu2+ electrode.
Membrane electrode is electrode:
Silver-silver chloride electrode.
Zn/Zn2+ electrode.
*Glass electrode.
Hydrogen electrode.
Cu/Cu2+ electrode.
The metal - metal ion electrode is:
Silver-silver chloride electrode.
Calomel electrode.
Hydrogen electrode.
D. Glass electrode.
E. *Cd/Cd2+ electrode.
437. Calomel electrode is:
A. The metal - metal ion electrode.
B. The gas-ion electrode is electrode.
C. *Metal-insoluble salt-anion electrode.
D. Inert "oxidation-reduction" electrode.
E. Membrane electrode.
438. For measuring pH of solution and biological liquids is used such electrode:
A. Zn/Zn2+ electrode.
B. Calomel electrode.
C. *Hydrogen electrode.
D. Ag/Ag+ electrode.
E. Cu/Cu2+ electrode.
439. For measuring pH of solution and biological liquids is used such electrode:
A. Calomel electrode.
B. *Glass electrode.
C. Calomel electrode.
D. Ag/Ag+ electrode.
E. Cu/Cu2+ electrode.
440. 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.
441. An electrochemical cell:
A. *It is а device, which makes use of an oxidation-reduction reaction to produce the interconversion of
chemical and electric energy.
B. It is а device, which makes use of reaction to produce the interconversion of heat and potential energy.
C. It is а device, which makes use of reaction to produce the interconversion of electric and potential
energy.
D. It is а device, which makes use of reaction to produce the interconversion of chemical and potential
energy.
E. It is а device, which makes use of a precipitation reaction to produce the interconversion of chemical
and kinetic energy.
442. Galvanic cell:
is used for measuring:
A. Membrane potential.
B. *pH.
C. Standard electrode potential.
D. Concentration potential.
E. Electro-kinetic potential.
443.
A.
B.
C.
D.
E.
444.
A.
B.
C.
D.
E.
445.
Electrode potential is formed in systems when are such reactions:
Double decomposing reaction.
Hydrolysis reaction.
Precipitation reaction.
*Oxidation - redaction reaction:
Neutralization reaction.
This concept “A state of dynamic balance in which the rate of forward and reverse reaction are equal” is:
*Chemical equilibrium.
Constant of reaction rate.
van’t Hoff law.
First law of thermodynamics.
Hass’s law.
This concept “If a stress (change of conditions) is applied to a system at equilibrium, the system shifts in
the direction that reduces the stress, to move toward a new state equilibrium” is:
A. Schrodinger equation.
B. Bohr’ postulates.
C. Schrodinger equation.
D. *Lechatelier’s principle.
E. van’t Hoff law.
446. Reversible is all reaction except:
A. N2O4(g) ↔ 2NO2(g).
B. *2KClO3 (s)→2KCl(s) + 3O2(g).
C. N2 (g) + 3H2(g) ↔ 2NH3(g).
D. N2(g) + O2(g) ↔ 2NO(g).
E. C2H4 (g) + H2(g) ↔ C2H6(g).
447. Irreversible reaction is:
A. *CaCO3 (s)→CaO(s) + CO2(g).
B. N2O4(g) ↔ 2NO2(g).
C. N2 (g) + 3H2(g) ↔ 2NH3(g).
D. N2(g) + O2(g) ↔ 2NO(g).
E. C3H6 (g) + H2(g) ↔ C3H8(g).
448. The kinetic energy that reactant molecules must have allow them to reach the transition state so that a
reaction can occur.
A. Heat effect reaction.
B. Potential energy.
C. *Activation reaction.
D. Enthalpy.
E. Free Gibbs’ energy.
449. The time required for half of that reactant to the converted into product.
A. Heat effect reaction.
B. Molecularity.
C. Time of reaction.
D. Order reaction.
E. *Half-life a reactant.
450.
A.
B.
C.
D.
E.
451.
A.
B.
C.
D.
E.
The equation:
for this reaction
is:
Rate law equation.
van’t Hoff law equation.
*Rate equation.
Chemical equilibrium constant.
Arhenius’ law equation.
The study of rates and mechanisms of chemical reactions and of the factors on which they depend is:
Thermodynamics.
Electrochemistry.
Colloidal chemistry.
*Chemical kinetics.
Gravimetric analysis.
452.
A.
B.
C.
D.
E.
"k" in rate law equation
*Rate constant.
Mass-action expression.
Chemical equilibrium constant.
Rate.
Temperature reaction.
453.
A.
B.
C.
D.
υ in rate law equation
Rate constant.
Mass-action expression.
Chemical equilibrium constant.
*Rate.
is:
is:
E. Temperature reaction.
454. Inreversible is all reaction except:
A. *N2O4(g) ↔ 2 NO2(g).
B. 2KClO3 (s) →2 KCl(s) + 3O2(g).
C. CaCO3 (s) →CaO(s) + CO2(g).
D. 2NaNO3 → 2 NaNO2 + O2.
E. 2Cu(NO3)2 → 2 CuO + 4NO2 +O2.
455. The mass-action expression for reversible reaction: C2H4 (g) + H2(g) = C2H6(g).
A. K = [C2H4] [H2]/ [C2H6].
B. *K = [C2H6] / [C2H4] [H2].
C. K = [C2H4] + [H2] - [C2H6].
D. K = [C2H4] / [C2H6].
E. K = 1/ [C2H6].
456. Rate law equation for forward reaction: N2O4(g) = 2NO2(g) is:
A. υ= k [2NO2].
B. υ= k [NO2]2.
C. *υ= k [N2O4].
D. υ= k [NO].
E. υ= [NO2].
457. Rate law equation for reverse reaction:
is:
A. υ= k [KClO3]2.
B. *υ= k [KCl]2 [O2]3.
C. υ= k 2 [KCl] 3[O2].
D. υ= k [KCl] [O2].
E. υ= k [KCl] + [O2]3.
458. 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.
459. The remaining portion of the universe, excluding the system, is called:
A. System.
B. *Surroundings.
C. Entropy.
D. Reaction.
E. Energy.
460. The properties of the system whose value depends upon the amount of substance present in the system
are:
A. Reversible properties.
B. Irreversible properties.
C. *Extensive properties.
D. Intensive properties.
E. Spontaneous properties.
461. The properties of the system whose value does not depend upon the amount of substance present in the
system are.
A. Reversible properties.
B. Irreversible properties.
C. Extensive properties.
D. *Intensive properties.
E. Spontaneous properties.
462. Extensive property is:
A. Temperature.
B. Pressure.
C. Viscosity.
D.
E.
463.
A.
B.
C.
D.
E.
464.
A.
B.
C.
D.
E.
465.
A.
B.
C.
D.
E.
466.
A.
B.
C.
D.
E.
467.
A.
B.
C.
D.
E.
468.
A.
B.
C.
D.
E.
469.
A.
B.
C.
D.
E.
470.
A.
B.
C.
Density.
*Mass.
Intensive properties are all except:
Temperature.
*Heat capacity.
Viscosity.
Density.
Pressure.
Extensive properties are all except:
Mass.
Volume.
Heat capacity.
*Density.
Gibbs free energy.
Intensive property is:
Mass.
Volume.
*Viscosity.
Heat capacity.
Gibbs free energy.
Isothermal process is:
*А process is carried out in such а manner that the temperature remains constant throughout the process.
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.
А process during which the volume of the system is kept constant.
А process during which the pressure of the system is kept constant.
А process which is carried out infinitesimally slowly so that all changes occurring in the direct process
can be exactly reversed.
Adiabatic process is:
А process is carried out in such а manner that the temperature remains constant throughout the process.
*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.
А process during which the volume of the system is kept constant.
А process during which the pressure of the system is kept constant.
А process which is carried out infinitesimally slowly so that all changes occurring in the direct process
can be exactly reversed.
Isochoric process is:
А process is carried out in such а manner that the temperature remains constant throughout the process.
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.
*А process during which the volume of the system is kept constant.
А process during which the pressure of the system is kept constant.
А process which is carried out infinitesimally slowly so that all changes occurring in the direct process
can be exactly reversed.
Isobaric process is:
А process is carried out in such а manner that the temperature remains constant throughout the process.
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.
А process during which the volume of the system is kept constant.
*А process during which the pressure of the system is kept constant.
А process which is carried out infinitesimally slowly so that all changes occurring in the direct process
can be exactly reversed.
Reversible process is:
А process is carried out in such а manner that the temperature remains constant throughout the process.
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.
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.
471. Irreversible process is:
A. А process is carried out in such а manner that the temperature remains constant throughout the process.
B. *A process which does not meet the above requirements.
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.
472. For measurement heat is used:
A. Thermometer.
B. pH-meter.
C. Voltmeter.
D. Potentiometer.
E. *Calorimeter.
473. The 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 in the temperature of any one of the reactants or products per unit of time.
C. The change in the pressure of solution any one of the reactants or products per unit of time.
D. The change in the volume of solution any one of the reactants or products per unit of time.
E. The change in the internal energy of any one of the reactants or products per unit of time.
474. The rate of chemical reaction is calculated by formula:
A. W=nRT (V2/V1).
B. W= pQ.
C. W = p ΔV.
D. W=nRTln(V2/V1).
E.
475.
A.
B.
C.
D.
E.
476.
A.
B.
*
Factors affection the reaction rate all except:
Nature of the reactants.
Concentration of the reactants.
*Internal energy of systems.
Presence of Catalyst.
Surface area of the reactants.
Vant-Goff rule equation is:
W= nRT (V2/V1).
*υt2/υt1 = γ t2 - t1/10.
C.
.
D. W= nRTln(V2/V1).
E.
.
477. Arhenius equation is:
A. W= nRT (V2/V1).
B. *
.
(t2 - t1)/10
C. υt2/υt1 = γ
.
D. W= nRTln(V2/V1).
E.
.
478. “A” in Arhenius equation (
) is:
A. Activation energy.
B. *Pre-exponential factor or the frequency factor.
C. Boltzmann distribution.
D. Activation Gibbs energy.
E. Rate constant.
479.
A.
B.
C.
D.
E.
“Ea” in Arhenius equation (
) is:
*Activation energy.
Pre-exponential factor or the frequency factor.
Boltzmann distribution.
Activation Gibbs energy.
Rate constant.
480.
A.
B.
C.
D.
E.
“k” in Arhenius equation (
) is:
Activation energy.
Pre-exponential factor or the frequency factor.
Boltzmann distribution.
Activation Gibbs energy.
*Rate constant.
481.
A.
B.
C.
D.
E.
482.
A.
B.
C.
D.
E.
483.
A.
B.
C.
D.
E.
484.
A.
B.
C.
D.
E.
485.
A.
B.
C.
D.
E.
486.
A.
B.
C.
D.
E.
487.
A.
B.
“е-Ea/RT” in Arhenius equation (
) is:
Activation energy.
Pre-exponential factor or the frequency factor.
*Boltzmann distribution.
Activation Gibbs energy.
Rate constant.
“T” in Arhenius equation (ln k=ln A-Ea/ RT) is:
Activation energy.
Pre-exponential factor or the frequency factor.
Boltzmann distribution.
*Temperature.
Rate constant.
Enzyme is biological catalyst. What is it nature?
Carbohydrate.
Lipid.
*Protein.
Mineral acid.
Vitamin.
HCl is used as catalyst. What is it nature?
Carbohydrate.
Lipid.
Protein.
*Mineral acid.
Vitamin.
Platinum is used as catalyst. What is it nature?
Carbohydrate.
*Metal.
Protein.
Mineral acid.
Vitamin.
Aluminum cloride is used as catalyst. What is it nature?
Carbohydrate.
Metal.
Protein.
Mineral acid.
*Mineral salt.
Cytochrome is biological catalyst. What is it nature?
*Protein.
Metal.
C. Carbohydrate.
D. Mineral acid.
E. Mineral salt.
488. What kind of dispersion systems is emulsions(G-gas, L-Liquid, S-solid)?
A. G/S.
B. S/S.
C. *L/L.
D. S/G.
E. G/L.
489. What kind of dispersion systems is gels (G-gas, L-Liquid, S-solid)?
A. G/S.
B. S/S.
C. L/L.
D. *S/L.
E. G/L.
490. Syspension is dispersed system with size dispersed phase particle equal 10-4. What type system of it
is(G-gas, L-Liquid, S-solid)?
A. G/S.
B. S/S.
C. L/L.
D. *S/L.
E. G/L.
491. What type of dispersed system is blood if size of dispersed phase particle equal 10-4?
A. True solution.
B. Emulsion.
C. *Suspension.
D. Aerosol.
E. Colloidal solution.
492. Aggregation of the particles arising from the stabilizing effect of this secondary minimum is:
A. *Coagulation.
B. Peptization.
C. Opalescence.
D. Diffraction.
E. Nephelomertry.
493. Sedimentation is process in which ….
A. The process of separating the particles of colloids from those of crystalloids by diffusion of the mixture
through а parchment or an animal membrane.
B. Oxidation of element in colloidal solution.
C. Aggregation of the particles arising from the stabilizing effect of this secondary minimum.
D. System, in which a dispersion phase and dispersion medium are liquids, which are non dissolved eth
other.
E. *In а gravitational field, heavy particles settle towards the foot of а column of solution.
494. These methods involve the joining together of а large number of smaller particles to form particles of
colloidal size is called condensation. What method is condensation?
A. *Peptization.
B. Oxidation reaction.
C. Opalescence.
D. Diffraction.
E. Nephelomertry.
495. These condensation methods is all except:
A. Redaction.
B. Oxidation.
C. Double decomposition.
D. Hydrolysis.
E. *Dispersion.
496. Oxidation reaction is used for preparation colloidal solution. What reaction is oxidation?
A. As2O3 + ЗH2S = As2S3 + З H2O.
B. 2 AuCl3 + 3 SnCl2=2 Аu + 3SnCl4.
C. *Br2 + H2S = S + 2HBr.
D. FeCl3 + 3 H2O = Fe(OH)3 + 3 HCl.
E. AlCl3 + 3 H2O = Al(OH)3 + 3 HCl.
497. Double decomposition reaction is used for preparation colloidal solution. What reaction is double
decomposition?
A. *As2O3 + ЗH2S = As2S3 + З H2O.
B. 2 AuCl3 + 3 SnCl2=2 Аu + 3SnCl4.
C. Br2 + H2S = S + 2HBr.
D. FeCl3 + 3 H2O = Fe(OH)3 + 3 HCl.
E. AlCl3 + 3 H2O = Al(OH)3 + 3 HCl.
498. Reduction reaction is used for preparation colloidal solution. What reaction is reduction?
A. As2O3 + ЗH2S = As2S3 + З H2O.
B. *2 AuCl3 + 3 SnCl2=2 Аu + 3SnCl4.
C. Br2 + H2S = S + 2HBr.
D. FeCl3 + 3 H2O = Fe(OH)3 + 3 HCl.
E. AlCl3 + 3 H2O = Al(OH)3 + 3 HCl.
499. Reaction of hydrolysis is used for preparation colloidal solution. What reaction is hydrolysis?
A. As2O3 + ЗH2S = As2S3 + З H2O.
B. 2 AuCl3 + 3 SnCl2=2 Аu + 3SnCl4.
C. Br2 + H2S = S + 2HBr.
D. Fe3O3 + 6 HCl = 2 FeCl3 + 3 H2O.
E. *AlCl3 + 3 H2O = Al(OH)3 + 3 HCl.
500. Colloidal solutions have different properties. Physical properties is all except:
A. Heterogeneous character.
B. Stability.
C. Filterability.
D. Visibility.
E. *Tyndall affect.
501. Colloidal solutions have different properties. Colligative properties is:
A. Heterogeneous character.
B. *Osmotic pressure.
C. Filterability.
D. Visibility.
E. Tyndall affect.
502. Colloidal solutions have different properties. Optical properties is:
A. Heterogeneous character.
B. Osmotic pressure.
C. Filterability.
D. Visibility.
E. *Tyndall affect.
503. Colloidal solutions have different properties. Mechanical properties is:
A. Heterogeneous character.
B. Osmotic pressure.
C. Filterability.
D. *Brownian movement.
E. Tyndall affect.
504. Colloidal solutions have different properties. Electrical properties is:
A. *Electrophoresis.
B. Osmotic pressure.
C. Filterability.
D. Brownian movement.
E. Tyndall affect.
505. Colloidal solutions have different properties. Physical properties is:
A. Electrophoresis.
B. Electrodialisis.
C. *Filterability.
D.
E.
506.
A.
B.
C.
D.
E.
507.
A.
B.
C.
D.
E.
508.
A.
B.
C.
D.
E.
509.
A.
B.
C.
D.
E.
510.
A.
B.
C.
D.
E.
511.
A.
B.
C.
D.
E.
512.
A.
B.
C.
D.
E.
513.
A.
B.
C.
D.
E.
514.
A.
B.
C.
D.
E.
Brownian movement.
Tyndall affect.
For synthesis of polymers is used reaction:
*Addition polymerization.
Oxidation.
Peptization.
Hydrolysis.
Dispersion.
Addition polymerization is reaction……
The process of separating the particles of colloids from those of crystalloids by diffusion of the mixture
through а parchment or an animal membrane.
Oxidation of element in colloidal solution.
Aggregation of the particles arising from the stabilizing effect of this secondary minimum.
*Occurs when unsaturated monomers react to form а polymer.
In а gravitational field, heavy particles settle towards the foot of а column of solution.
Anion exchange resins all except:
OH--exchange resins.
*H+- exchange resins.
SO42--exchange resins.
СІ- -exchange resins.
Br-- exchange resins.
Cation exchange resins all except:
*OH--exchange resins.
Na+-exchange resins.
Ca2+-exchange resins.
H+- exchange resins.
K+-exchange resins.
The occlusion is called:
Concentrated one matter in surface other.
Transferred matters from solid into the gas state.
*The adsorption of gases on the surface of metals.
Method of separation mixtures into individual compounds.
Chromatography analysis.
Surface phenomenon is all except:
Adhesion.
Coatings.
Adsorption.
*Sedimentation.
Occlusion.
What phenomenon is surface phenomenon?
*Adhesion.
Titration.
Neutralization.
Sedimentation.
Absorption.
What compound is surface inactive compound?
Alcohols.
Fatty acids.
*Sodium
Amino acids.
Proteins.
What ion is adsorbed on OH-- exchange resins?
*SO42-.
Na+.
Ca2+.
H+.
K+.
515. What ion is adsorbed on H+- exchange resins?
A. SO42-.
B. *Na+.
C. S2-.
D. OH-.
E. Cl-.
516. On H+- exchange resins are adsorbed all ions except:
A. *PO43-.
B. Na+.
C. Ca2+.
D. H+.
E. K+.
517. On OH-- exchange resins is adsorbed all ions except:
A. SO42-.
B. *Ca2+.
C. S2-.
D. OH-.
E. Cl-.
518. The adsorption in which ions of solution exchange with surface adsorbent ions.
A. Adhesion.
B. Coatings.
C. Sedimentation.
D. Occlusion.
E. *Ion exchange adsorption.
519. Class of compounds, molecule which contain hydrophobic (non-polar) hydrocarbon "tails" and a
hydrophilic (polar) "head" group are called:
A. Mineral acids.
B. Mineral Bases.
C. Oxides.
D. *Surfactants.
E. Mineral salt.
520. Compounds which concentrate at the interface, and modifies (decrease) its surface tension are called
A. Mineral acids.
B. *Surfactants.
C. Mineral Bases.
D. Oxides.
E. Mineral salt.
521. Compounds which accumulates at the interface, and modifies (increase) its surface tension are called:
A. Fatty acids.
B. Proteins.
C. Surfactants.
D. *Surface inactive compound.
E. Phospholipids.
522. The surface phenomenon on which occurs throughout the body of the material is:
A. Adhesion.
B. Adsorption.
C. Neutralization.
D. Sedimentation.
E. *Absorption.
523. The surface phenomenon on which occurs only at the surface of the adsorbent is:
A. Adhesion.
B. *Adsorption.
C. Neutralization.
D. Sedimentation.
E. Absorption.
524. Surface tension depend on:
A. Decrease of pressure.
B.
C.
D.
E.
525.
A.
B.
C.
D.
E.
1.
2.
3.
4.
5.
6.
7.
8.
Volume of liquids.
Form of glass.
*Nature of liquids.
Freezing temperature.
The surface tension can determine by such method:
Potentiaometry.
Chelatometry.
*Stalagmometri method.
Chromatography.
Criometry.
Question to pictures
Equation, which is represented on figure 1, it is ….. law equation.
A. *Mendeleev-Сlapeyron.
B. Raoult's.
C. Henry's.
D. Henderson-Hasselbalch.
E. van’t Hoff.
Mendeleev-Сlapeyron law equation is represented on figure 1. Letter “V” is marked ….. in this formula.
A. Pressure.
B. *Volume.
C. Temperature.
D. Density.
E. Universal gas constant.
Mendeleev- Clapeyron law equation is represented on figure1. Letter “p” is marked ….. in this formula.
A. *Pressure.
B. Volume.
C. Temperature.
D. Density.
E. Universal gas constant.
Mendeleev- Clapeyron law equation is represented on figure 1. Letter “R” is marked ….. in this formula.
A. Pressure.
B. Volume.
C. Temperature.
D. Density.
E. *Universal gas constant.
Mendeleev- Clapeyron law equation is represented on figure 1. Letter “T” is marked ….. in this formula.
A. Pressure.
B. Volume.
C. *Temperature.
D. Density.
E. Universal gas constant.
Mendeleev- Clapeyron law equation is represented on figure 1. Letter “n” is marked ….. in this formula.
A. Pressure.
B. Volume.
C. *Amount of mole matter.
D. Density.
E. Universal gas constant.
Phases diagram of the water is represented on figurer 2. The “O” point is:
A. The milting curve.
B. The boiling curve.
C. The sublimation curve.
D. *The triple point.
E. The milting point.
A graph is represented on figure 2. What is it name?
A. *Phase diagram of the water state.
B. Phase diagram of the metallic system state.
C. Phase diagram of the carbon-iron system state.
D. Diagram of temperature dependence on solubility.
E. Diagram of the catalyst influence on solubility.
9. Phase diagram of the water is represented on figurer 2. The “OA” curve is named:
A. The milting curve.
B. *The boiling curve.
C. The sublimation curve.
D. The triple point.
E. The milting point.
10. Phase diagram of the water is represented on figurer 2. The “AC” curve is named:
A. *The milting curve.
B. The boiling curve.
C. The sublimation curve.
D. The triple point.
E. The milting point.
11. Phase diagram of the water is represented on figurer 2. The “OB” curve is named:
A. The milting curve.
B. The boiling curve.
C. *The sublimation curve.
D. The triple point.
E. The milting point.
12. Equation which is represented on figure 3 , it is mathematical expression of:
A. First Raoult's law.
B. Henry's law.
C. Arrhenius law.
D. van’t Hoff law.
E. Equivalent law.
13. *Some compound formulas are represented on figure 4. To choose the matter which is used for standardize
sodium hydroxide solution.
A. *1.
B. 2.
C. 3.
D. 4.
E. 5.
14. Acid and base standard solutions are used on neutralization titration method as second standard. Choose the
matter which is used for standardize sulfuric acid solution (fig. 4).
A. 1.
B. 2.
C. 3.
D. 4.
E. *5.
15. What is process name which is represented on figure 5?
A. Preparation of solution.
B. Measuring of solution temperature.
C. *Titration of solution.
D. Determination of electrode potential.
E. Determination of pH solution.
16. Analytical chemists use a variety of glassware to measure volume. Typical instrumentation for performing
titration is on figure 5. Glassware which is represented by a number 1 is named:
A. Volumetric flask.
B. Conical retort.
C. Pipette.
D. *Burette.
E. Cylinder.
17. Typical instrumentation for performing titration is on figure 5. Glassware which is represented by a number
2 is named:
A. Volumetric flask.
B. *Conical retort.
C. Pipette.
D. Burette.
E. Cylinder.
18. A variety of glassware is used in analytical chemistry to measure volume. What is glassware name which is
represented on figure 6.а.
A. *Measured beaker.
B. Measured pipette.
C. Burette.
D. Cylinder.
E. Volumetric flask.
19. What is glassware name which is represented on figure 6.b.
A. Measured beaker.
B. Measured pipette.
C. Burette.
D. *Cylinder.
E. Volumetric flask.
20. A variety of glassware is used in analytical chemistry to measure volume. What is glassware name which is
represented on figure 6.c.
A. Measured beaker.
B. Measured pipette.
C. Burette.
D. Cylinder.
E. *Volumetric flask.
21. A variety of glassware is used in analytical chemistry to measure volume. What is glassware name which is
represented on figure 6.d.
A. Measured beaker.
B. *Measured pipette.
C. Burette.
D. Cylinder.
E. Volumetric flask.
22. A variety of glassware is used in analytical chemistry to measure volume. What is glassware name which is
represented on figure 6.e.
A. Measured beaker.
B. Measured pipette.
C. *Burette.
D. Cylinder.
E. Volumetric flask.
23. Which volumetric analysis is used the compound (fig. 7.4) as the secondary standard?
A. *Acid-basic titration.
B. Precipitation method.
C. Chelatometry.
D. Oxidation-restoration titration.
E. Complexometric titration.
24. Which volumetric analysis is used the compound (fig. 7.2) as the secondary standard?
A. Acid-basic titration.
B. Precipitation method.
C. Chelatometry.
D. *Oxidation-restoration titration.
E. Complexometric titration.
25. Which volumetric analysis is used the compound (fig. 7.5) as the secondary standard?
A. Acid-basic titration.
B. *Precipitation method.
C. Chelatometry.
D. Oxidation-restoration titration.
E. Complexometric titration.
26. Which volumetric analysis is used the compound (fig. 7.3) as the secondary standard?
A. Oxidometry.
B. Precipitation method.
C. *Alkalimetry.
D. Oxidation-restoration titration.
E. Complexometric titration.
27. On figure 8.1 is represent:
A. *The ionisation sphere.
B. The coordinating sphere.
C. The coordination number.
D. The ligand.
E. The central metal ion.
28. On figure 8.2 is represent:
A. The ionisation sphere.
B. *The coordinating sphere.
C. The coordination number.
D. The ligand.
E. The central metal ion.
29. On figure 8.3 is represent:
A. The ionisation sphere.
B. The coordinating sphere.
C. The coordination number.
D. The ligand.
E. *The central metal ion.
30. On figure 8.4 is represent:
A. The ionisation sphere.
B. The coordinating sphere.
C. *The coordination number.
D. The ligand.
E. The central metal ion.
31. On figure 8.5 is represent:
A. The ionisation sphere.
B. The coordinating sphere.
C. The coordination number.
D. *The ligand.
E. The central metal ion.
32. The name of compound (fig.8) is:
A. *Potassium hexacianoferrate (III).
B. Potassium hexacianoferrate (II).
C. Potassium irone (III) hexacianate.
D. Potassium irone (III)cianade.
E. Potassium cianade ferrate (III).
33. The oxidation number of central atom ion in compound (fig. 8) is:
A. +1.
B. +2.
C. *+3.
D. +4.
E. -2.
34. The coordination number of central atom ion in compound (fig. 8) is:
A. 3.
B. 2.
C. *6.
D. 4.
E. 5.
35. The name of compound (fig.9) is:
A. The tetraaninocuprate (ІІ) sulfa.
B. The diaminocopper (ІІ) sulfide.
C. The copper (ІІ) diamino sulfite.
D. The tetraaninosulfo cuprate.
E. *The tetraaninocopper (ІІ) sulfate.
36. The oxidation number of central atom ion in compound (fig. 9) is:
A. +1.
B. *+2.
C. +3.
D. +4.
E. -2.
37. The coordination number of central atom ion in compound (fig. 9) is:
A. 3.
B. 2.
C. 6.
D. *4.
E. 5.
38. On figure 9.1 is represent:
A. The ionic coordinating sphere.
B. The coordinating sphere.
C. The coordination number.
D. The ligand.
E. *The central metal ion.
39. On figure 9.2 is represent:
A. The ionic coordinating sphere.
B. The coordinating sphere.
C. The coordination number.
D. *The ligand.
E. The central metal ion.
40. On figure 9.3 is represent:
A. The ionic coordinating sphere.
B. The coordinating sphere.
C. *The coordination number.
D. The ligand.
E. The central metal ion.
41. On figure 9.4 is represent:
A. *The ionic coordinating sphere.
B. The coordinating sphere.
C. The coordination number.
D. The ligand.
E. The central metal ion.
42. On figure 9.5 is represent:
A. The ionic coordinating sphere.
B. *The coordinating sphere.
C. The coordination number.
D. The ligand.
E. The central metal ion.
43. The name of compound (fig.10) is:
A. The chloride of diaminodihydro platinum (ІV).
B. The dihydroxotetrachloroplatinum (ІV) hydroxide.
C. The platinum (ІІ) dihydroxotetrachloroammonium
D. The ammonium dihydroxide of platinum tetrachloride.
E. *The ammonium dihydroxotetrachloroplatinate (ІV).
44. The oxidation number of central atom ion in compound (fig. 10) is:
A. +1.
B. +2.
C. +3.
D. *+4.
E. -2.
45. The coordination number of central atom ion in compound (fig. 10) is:
A. 3.
B. 2.
C. *6.
D. 4.
E. 5.
46. The name of compound (fig.11) is:
A. *The aquadiaminochloropalladium (ІІ) chloride.
B. The diaminohydroxochloride palladium (ІІ).
C. The palladium (ІІ) chloroaquaammonium.
D. The dichlorodiaminoaquapalladiate.
E. The palladium (ІІ) diaminoaquachloride.
47. The oxidation number of central atom ion in compound (fig. 11) is:
A. +1.
B. +2.
C. *+3.
D. +4.
E. -2.
48. The coordination number of central atom ion in compound (fig. 11) is:
A. 3.
B. 2.
C. 6.
D. *4.
E. 5.
49. The name of compound (fig.12) is:
A. *The sodium dinitroargentate (І).
B. The sodium silver nitrate.
C. The sodium silver nitrite.
D. The nitrosilver (І) nitrate.
E. The disodium silverdinitrite.
50. Formula which is represented on figure 13 ([КИСЛОТА] is [acid]; [ОСНОВА] is [base]) is used for the
calculation:
A. The dissociation constant.
B. The dissociation degree.
C. *The pH-value.
D. The mass of matter.
E. The hydrolysis degree.
51. Mathematical expression, which is represented on figure 13 ([КИСЛОТА] is [acid]; [ОСНОВА] is [base]),
it is formula for calculation the pH of buffer solution. “рКа” is marked:
A. *The index of dissociation constant.
B. The dissociation constant.
C. The dissociation degree.
D. The mass of matter.
E. The hydrolysis degree.
52. The shrinkage of red blood cells in hypertonic solution is represented on figure 14:
A. On the right.
B. On the right and in the middle.
C. In the middle.
D. *On the left.
E. On the left and in the middle.
53. Red blood cells will swell and rupture when they are immersed in pure water. On figure 14 this process is
represented:
A. On the right.
B. On the right and in the middle.
C. *In the middle.
D. On the left.
E. On the left and in the middle.
54. The effect of isotonic solutions cause no changes in cell volume is represented on figure 14:
A. *On the right.
B. On the right and in the middle.
C. In the middle.
D. On the left.
E. On the left and in the middle.
55. Plasmolysis (crenation) is represented on figure 14:
A. On the right.
B. On the right and in the middle.
C. In the middle.
D. *On the left.
E. On the left and in the middle.
56. Hemolysis is represented on figure 14:
A. On the right.
B. On the right and in the middle.
C. *In the middle.
D. On the left.
E. On the left and in the middle.
57. What phenomenon is represented on the left in figure 14?
A. The effects of isotonic solutions cause no changes in cell volume.
B. Red blood cells will swell and rupture when they are immersed in pure water.
C. *The shrinkage of red blood cells in hypertonic solution.
D. The effect of isotonic solutions.
E. The effect of 0.9 % of sodium chloride solution.
58. What phenomenon is represented on the right in figure 14?
A. *The effects of isotonic solutions cause no changes in cell volume.
B. Red blood cells will swell and rupture when they are immersed in pure water
C. The shrinkage of red blood cells in hypertonic solution
D. The effect of isotonic solutions
E. The effect of 10 % of sodium chloride solution.
59. What phenomenon is represented in the middle of figure 14?
A. The effects of isotonic solutions cause no changes in cell volume.
B. *Red blood cells will swell and rupture when they are immersed in pure water.
C. The shrinkage of red blood cells in hypertonic solution.
D. The effect of isotonic solutions.
E. The effect of 0.9 % of sodium chloride solution.
60. The test-reagents (fig.15) are used for measure рН solutions. What is method use this test-reagent?
A. *The colorimetric method.
B. The potentiometric method.
C. The photometric method.
D. The polarimetric method.
E. The conductometric method.
61. What is name compound, formula which is represented on fig. 16?
A. Sodium sulfate.
B. Sodium sulfite.
C. *Sodium hydrogen sulfate.
D. Sodium hydrogen sulfite.
E. Sodium thiosulfate.
62. What is ions form, if compound (fig.16) is dissociated?
A. Sodium cation and sulfate anion.
B. Sodium cation and sulfite anion.
C. *Sodium cation and hydrogen sulfate anion.
D. Sodium cation and hydrosulfite anion.
E. Sodium cation and thiosulfate anion.
63. On figure 17 it is shown formation of:
A. *Double electric layer.
B. Contact potential.
C. Diffuse potential.
D. Membrane potential.
E. Concentration potential.
64. What is “?” mean in Nernst equation (figure 18)?
A. Valency of metal ion.
B. *Activity of ions in solution.
C. Volume of solution.
D. Number of electrons.
E. Electrode potential.
65. What is “n” mean in Nernst equation (figure 18)?
A. Absolute temperature.
B. Activity of ions.
C. Faraday constant.
D. *Number of electrons.
E. Electrode potential.
66. What is “F” mean in Nernst equation (figure 18)?
A. Absolute temperature.
B. Activity of ions is in solution.
C. *Faraday constant.
D. Number of electrons.
E. Electrode potential.
67. What is “e” mean in Nernst equation (figure 18)?
A. Absolute temperature.
B. Activity of ions in solution.
C. Faraday constant.
D. Number of electrons.
E. *Electrode potential.
68. What is “e0” mean in Nernst equation (figure 18)?
A. Absolute temperature.
B. Activity of ions in solution.
C. Faraday constant.
D. *Standard electrode potential.
E. Number of electrons.
69. A formula (figure 19) is used for a calculation......
A. *Electrode potential.
B. Amount of solute in solution.
C. The mass of the solute in solution.
D. Molar concentration of solution.
E. Mass fraction of solute in solution.
70. Formula, which is shown on figure 19 it is:
A. Mass-action law equation.
B. Equivalent law equation.
C. *Nernst equation.
D. Arrhenius equation.
E. Faraday equation.
71. What electrode is shown on figure 20?
A. *Hydrogen.
B. Platinum.
C. Glass.
D. Silver-silvercholide.
E. Calomel.
72. Electrode represent on figure 20. What is electrode and what is its standard electrode potential?
A. Hydrogen, 10 V.
B. Platinum, 0 V.
C. Glass, 0 V.
D. *Hydrogen, 0 V.
E. Platinum, 10 V.
73. What galvanic cell is shown on figure 21?
A. Concentration cell.
B. *Daniell cell.
C. Copper cell.
D. Zinc cell.
E. Ionselective cell.
74. What electrode is shown on figure 22?
A. Hydrogen.
B. Platinum.
C. *Glass.
D. Silver-silvercholide.
E. Calomel.
75. Glass electrode is shown on figure 22. It is marked a number 1:
A. Glass tube.
B. Connecting a cable.
C. Thin glass membrane
D. *Internal reference electrode.
E. Standard potassium chloride solution.
76. Glass electrode is shown on figure 22. It is marked a number 2:
A. Glass tube.
B. Connecting a cable.
C. Thin glass membrane
D. Internal reference electrode.
E. *Standard potassium chloride solution.
77. Glass electrode is shown on figure 22. It is marked a number 3:
A. Glass tube.
B. Connecting a cable.
C. *Thin glass membrane
D. Internal reference electrode.
E. Standard potassium chloride solution.
78. What is the end process name, which is shown on figure 23?
A. The osmosis.
B. The dialysis.
C. The coagulation.
D. *The sedimentation.
E. Evaporation.
79. What is intermediate process name, which is shown on figure 23?
A. The osmosis.
B. The dialysis.
C. *The coagulation.
D. The sedimentation.
E. The evaporation.
80. What is the end process name, which is shown on figure 24?
A. The osmosis.
B. The dialysis.
C. The coagulation.
D. The sedimentation.
E. *The coalescence.
81. Dispersed and condensation methods of colloid solutions preparation is shown on figure 25. What method
of colloid solutions preparation is marked by number 1?
A. A particle of macroheterogonous suspension.
B. *A pure matter.
C. A micelle of emulsion.
D. Structural units of colloid solution.
E. A ultramicroheterogonous particle (ion, molecule) of true compounds.
82. Dispersed and condensation methods of colloid solutions preparation is shown on figure 25. What method
of colloid solutions preparation is marked by number 2?
A. *A particle of macroheterogonous suspension.
B. A pure matter.
C. A micelle of emulsion.
D. Structural units of colloid solution.
E. A ultramicroheterogonous particle (ion, molecule) of true compounds.
83. Dispersed and condensation methods of colloid solutions preparation is shown on figure 25. What method
of colloid solutions preparation is marked by number 4?
A. A particle of macroheterogonous suspension.
B. A pure matter.
C. A micelle of emulsion.
D. Structural units of colloid solution.
E. *A ultramicroheterogonous particle (ion, molecule) of true compounds.
84. Dispersed and condensation methods of colloid solutions preparation is shown on figure 25. What method
of colloid solutions preparation is marked by number 3?
A. A particle of macroheterogonous suspension.
B. A pure matter.
C. A micelle of emulsion.
D. *Structural units of colloid solution.
E. An ultramicroheterogonous particle (ion, molecule) of true compounds.
85. What factors is influence for solubility process, which is represented on figure 26?
A. Density.
B. Temperature.
C. *Pressure.
D. Concentration.
E. Area of surface.
86. What is device shown on figure 27?
A. A device for a dialysis.
B. *A device for preparation of colloid solutions by the method of Brediga.
C. A device for a vividialysis.
D. A device for a hemodialysis.
E. A device for a measuring of рН.
87. The micelle structure of some colloidal solution is shown on figure 28. What is the mark fragment name?
A. *A nuclear.
B. A diffuse layer.
C. A granule.
D. An appositive ion.
E. A micelle.
88. The micelle structure of some colloidal solution is shown on figure 29. What is the mark fragment name?
A. A nuclear.
B. A diffuse layer.
C. *A granule.
D. An appositive ion.
E. A micelle.
89. The micelle structure of some colloidal solution is shown on figure 30. What is the mark fragment name?
A. A nuclear.
B. A diffuse layer.
C. A granule.
D. *An appositive ion.
E. A micelle.
90. Which reaction (figure. 32) does not equilibrium displacement if a volume is changed in system?
A. 1.
B. *2.
C. 3.
D. 4.
E. 5.
91. Which reaction (figure. 32) does equilibrium displacement to the right if a volume is increase in system?
A. 1, 2.
B. 2, 3.
C. 3, 4.
D. *4, 5.
E. 2, 5.
92. Which reaction (figure. 32) does equilibrium displacement to the left if a volume is increase in system?
A. 1, 2.
B. *1, 3.
C. 3, 4.
D. 4, 5.
E. 2, 5.
93. Which reaction (figure. 32) does equilibrium displacement to the right if a pressure is decrease in system?
A. 1, 2.
B. 2, 3.
C. 3, 4.
D. *4, 5.
E. 2, 5.
94. Which reaction (figure. 32) does equilibrium displacement to the left if a pressure is decrease in system?
A. 1, 2.
B. *1, 3.
C. 3, 4.
D. 4, 5.
E. 2, 5.
95. Which reaction (figure. 32) does equilibrium displacement to the right if a pressure is increase in system?
A. *1, 3.
B. 2, 3.
C. 3, 4.
D. 4, 5.
E. 2, 5.
96. Which reaction (figure. 32) does equilibrium displacement to the left if a pressure is increase in system?
A. 1, 3.
B. 2, 3.
C. 3, 4.
D. *4, 5.
E. 2,5.
97. How is change speed of favorite reaction (figure. 31) if volume of reaction system decrease in 2 times?
A. *Increased in 4 times.
B. Increased in 2 times.
C. Decreased in 4 times.
D. Decreased in 2 times.
E. Increased in 6 times.
98. How is change speed of favorite reaction (figure. 31) if volume of reaction system increase in 2 times?
A. Increased in 4 times.
B. Increased in 2 times.
C. *Decreased in 4 times.
D. Decreased in 2 times.
E. Increased in 6 times.
99. How will change speed of favorite reaction (figure. 31) if pressure of reaction system decrease in 2 times?
A. Increased in 4 times.
B. Increased in 2 times.
C. *Decreased in 4 times.
D. Decreased in 2 times.
E. Increased in 6 times.
100. How is change speed of favorite reaction (figure. 31) if pressure of reaction system increase in 2 times?
A. *Increased in 4 times.
B. Increased in 2 times.
C. Decreased in 4 times.
D. Decreased in 2 times.
E. Increased in 6 times.
101. How is change speed of favorite reaction (figure. 31) if pressure of reaction system increase in 3 times?
A. Increased in 4 times.
B. Increased in 3 times.
C. Decreased in 4 times.
D. Decreased in 2 times.
E. *Increased in 9 times.
102. How is change speed of favorite reaction (figure. 31) if pressure of reaction system decrease in 3 times?
A. Increased in 4 times.
B. Increased in 3 times.
C. *Decreased in 9 times.
D. Decreased in 2 times.
E. Increased in 9 times.
103. What is a device name which is shown on figure 33?
A. *Calorimeter.
B. Artificial kidney.
C. Dialyser.
D. Coagulator.
E. Potentiometer.
104. The device which is shown on figure 33 is used for determine:
A. *Heat effects of reactions.
B. Concentration of solutions.
C. Density of liquids.
D. Melting point of compounds.
E. Speed of chemical reactions.
105. What is type of chemical reaction which is shown on figure 34?
A. *Parallel reactions.
B. Conjugate reactions.
C. Series reactions.
D. Chain reactions.
E. Reversible reactions.
106. Diagram dependence of surface tension by the concentration of water solutions of different matters is
shown on figure 35. A number 1 is mark dependence of surface tension by the solution of:
A. Surface – adsorption compounds.
B. Surface – electrolyte compounds.
C. Surface – indifferent compounds.
D. *Non surfactant compounds.
E. Surfactants.
107. Diagram dependence of surface tension by the concentration of water solutions of different matters is
shown on figure 35. A number 2 is mark dependence of surface tension by the solution of:
A. Surface – adsorption compounds.
B. Surface – electrolyte compounds.
C. *Surface – indifferent compounds.
D. Non surfactant compounds.
E. Surfactants.
108. Diagram dependence of surface tension by the concentration of water solutions of different matters is
shown on figure 35. A number 3 is mark dependence of surface tension by the solution of:
A. Surface – adsorption compounds.
B. Surface – electrolyte compounds.
C. Surface – indifferent compounds.
D. Non surfactant compounds.
E. *Surfactants.
109. On figure. 36 it is shown diagram of:
A. Dependence of adsorption by a temperature.
B. *Dependence of adsorption by a concentration of solution.
C. Dependence of adsorption by a surface tension.
D. Dependence of surface tension by a temperature.
E. Dependence of surface tension by a concentration of solution.
110. On figure 37 is shown the structure of surfactants. A number 1 is marked:
A. *Hydrophilic part.
B. Hydrocarbon radical.
C. Hydrophoblic part.
D. Nonpolar part.
E. Carbohydrate group.
111. On figure 37 is shown the structure of surfactants. A number 2 is marked:
A. Hydrophilic part.
B. Hydrocarbon radical.
C. *Hydrophoblic part.
D. Carboxylic group.
E. Carbohydrate group.
112. What is number mark the diagram dependence of surface tension by the temperature (figure 42)?
A. 1.
B. *2.
C. 3.
D. 4.
E. 5.
113. What is number mark the diagram dependence of surface tension by the concentration of surfactants in
solution (figure 43)?
A. 1.
B. 2.
C. 3.
D. *4.
E. 5.