Acid-basic equilibrium and complex compound in biological liquids
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.
n( solute)
V ( solution )
n solute 
E. Cm 
m(solvent )
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. *
D. * CM 
n solute 
m(solvent )
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. *
D. Cm 
n( solute)
V ( solution )
n solute 
D. Cm 
m(solvent )
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 ...........
A. The ratio between the volume solute and total volume of solution.
C. CM 
16.
17.
18.
19.
20.
21.
22.
23.
24.
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.
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.
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.
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.
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.
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.
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.
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.
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.
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 )
C. M 
n(compound )
m solute 
T
V (solution )
D.
n solute 
E. * Cm 
m(solvent )
26. For calculation mole mass (weight) of compound is used such formula:
m solute 

m(solution )
A.
m(compound )
B. * M 
n(compound )
n( solute)
C. CM 
V ( solution )
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 )
B. M 
n(compound )
m solute 
T
V (solution )
C. *
m solute 
E ( solute)  V ( solution )
D.
n solute 
E. Cm 
m(solvent )
28. For calculation normality of solution is used such formula:
m(compound )
A. M 
n(compound )
n solute 
B. Cm 
m(solvent )
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.


B. *
V solute 
V( solvent )  V solute 
m(compound )
n(compound )
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. *
C. M 
V solute 
V( solvent )  V solute 
B.
m solute 
Cn 
E ( solute)  V ( solution )
C.
m(compound )
D. M 
n(compound )
m solute 

m(solution )
E.
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.
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.
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.
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.
Colligative properties is all except:
A. Vapor-pressure lowering.
B. Boiling-point elevation.

31.
32.
33.
34.
35.
36.
37.
38.
39.
40.
41.
42.
C. Freezing-point depression.
D. Osmotic pressure.
E. *Mole mass.
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.
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.
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.
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.
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.
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.
Hypotonic solutions are:
43.
44.
45.
46.
47.
48.
49.
50.
51.
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.
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.
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.
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.
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.
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.
Colligative property is:
A. Temperature.
B. *Boiling-point elevation.
C. Volume.
D. Mole.
E. Molecule weight.
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 %.
Colligative properties is:
A. Temperature.
B. Normality.
C. Volume.
D. *Osmotic pressure.
E. Molecule weight.
Neutralization reaction is the reaction between:
A. Strong acids.
B. Weak acids.
C. *Acid and base.
52.
53.
54.
55.
56.
57.
58.
59.
D. Weak bases.
E. Strong base.
What compounds is formed in neutralization reaction?
A. Strong acids.
B. Weak acids.
C. Acid and base.
D. *Salt and water.
E. Strong base.
For determination of рН solution is used:
A. Voltmiter.
B. Centrifuger.
C. Photoelectrocolorimetr.
D. *рН-meter.
E. Calorimeter.
What is color of methyl orange in acidic medium?
A. *Red.
B. Blue.
C. Violet.
D. Orange.
E. Colorless.
What is color of methyl red (indicator) in basic medium?
A. Red.
B. Blue.
C. *Yellow.
D. Orange.
E. Colorless.
What is color of phenolphalein in basic medium?
A. Yellow.
B. Blue.
C. Orange.
D. *Crimson.
E. Colorless.
Acid - base titration indicators is:
A. *Weak acids or weak bases.
B. Strong acids.
C. Strong bases.
D. Derivative of mineral acids.
E. Salt.
What is color of litmus in basic medium?
A. Yellow.
B. *Blue.
C. Orange.
D. Crimson.
E. Colorless.
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.
61.
62.
63.
64.
65.
66.
67.
68.
69.
70.
E. Strong acidic.
What is composition of phosphate buffer solutions?
A. HHb/Hb-.
B. HHbO2/HbO2-.
C. *H2PO4-/HPO42-.
D. H2CO3/HCO3-.
E. NH3/NH4+
What is composition of oxihemoglobin buffer solutions?
A. HHb/Hb-.
B. *HHbO2/HbO2-.
C. H2PO4-/HPO42-.
D. H2CO3/HCO3-.
E. NH3/NH4+
What is composition of bicarbonate buffer solutions?
A. HHb/Hb-.
B. HHbO2/HbO2-.
C. H2PO4-/HPO42-.
D. *H2CO3/HCO3-.
E. NH3/NH4+
What is composition of ammonia buffer solutions?
A. HHb/Hb-.
B. HHbO2/HbO2-.
C. H2PO4-/HPO42-.
D. H2CO3/HCO3-.
E. *NH3/NH4+
What is composition of hemoglobin buffer solutions?
A. *HHb/Hb-.
B. HHbO2/HbO2-.
C. H2PO4-/HPO42-.
D. H2CO3/HCO3-.
E. NH3/NH4+
What is composition of acetic buffer solutions?
A. *CH3COOH/CH3COO-.
B. H2CO3/HCO3-.
C. HHbO2/HbO2-.
D. H2PO4-/HPO42-.
E. NH3/NH4+
What is composition of protein buffer solutions?
A. HHb/Hb-.
B. H2PO4-/HPO42-.
C. *NH2RCOOH/NH2RCOOD. HHbO2/HbO2-.
E. H2CO3/HCO3-.
Blood buffer solution is all except:
A. HHb/Hb-.
B. HHbO2/HbO2-.
C. H2PO4-/HPO42-.
D. H2CO3/HCO3-.
E. *NH3/NH4+
Blood buffer solution is:
A. CH3COOH/CH3COO-.
B. *H2CO3/HCO3-.
C. HCl/Cl-.
D. H2SO4/HSO4-.
E. NH3/NH4+.
Blood buffer solution is all except:
A. HHb/Hb-.
71.
72.
73.
74.
75.
76.
77.
78.
79.
B. H2PO4-/HPO42-.
C. NH2RCOOH/NH2RCOO-.
D. *NH3/NH4+.
B. HHbO2/HbO2-.
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.
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.
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.
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.
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.
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.
What solution has the great buffer capacity?
A. 10/20.
B. 5/10.
C. 50/100.
D. 20/40.
E. *200/400.
What solution has the great buffer capacity?
A. 10/20.
B. 5/10.
C. *50/50.
D. 20/40.
E. 7/3.
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+].
83.
84.
85.
86.
87.
C. *
.
D. рН = lg[Н+] lg[ОН-].
E. рН = - lg[Н+] lg[ОН-].
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
рН =9 of solution. What is acidity of this solution?
A. *Strong basic.
B. Neutral.
C. Weak acidic.
D. Weak basic.
E. Strong acidic.
What is value of water product?
A. Кw = 10-7.
B. Кw = 107.
C. Кw = 10.
D. *Кw = 10-14.
E. Кw = 10-10.
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-].
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:
89.
90.
91.
92.
93.
94.
95.
96.
97.
A. pH = 2.
B. pH = 10.
C. pH = 4.
D. *H = 7.
E. pH = 12.
What value рН of basic medium:
A. рН = - 7.
B. рН < 7.
C. рН = 7.
D. *рН >7.
E. рН < - 7.
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.
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.
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.
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.
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.
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.
It is used as titrant in acid-base titration such compound:
A. KCl.
B. NaHCO3.
C. Na2SO4.
D. *HCl.
E. CuOH.
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. Ca(HCO3)2
107. The method of chelatometry is used for determination concentration of :
A. Acids.
B. *Metal ions.
C. Bases.
D. Carboxylic acids.
E. Anions.
108. Water hardness is ordinarily determined by........
A. HCl.
B. NaOH.
C. KMnO4.
D. CuSO4.
E. *EDTA.
109. In the chelatometry use such indicator:
A. Ion-indicator.
B. Adsorb -indicator.
C. Redox-indicator.
D. Acid-base indicator.
E. *Complex indicator.
110. For determination of total hardness of water use:
A. 0.1 M solution of sodium hydroxide.
B. 0.05 M solution of potassium permanganate.
C. 0.1M solution of acid salt.
D. *Solution of trilonium B.
E. 0.1n solution of calcium hydroxide.
111. Solubility product of AgI is:
A. *Кsp = [Ag+ ][I-].
B. Кsp = [Ag+].
C. Кsp = [Ag+][NO4-]
D. Кsp = [I-]
E. Кsp = [Ag] [K]
112. As titrant in precipitation titration is used:
A. NaCl.
B. KMnO4.
C. *AgNO3.
D. CaSO4.
E. KBr.
113. As titrant in argentometry is used:
A. *AgNO3.
B. KMnO4.
C. NaCl.
D. CaSO4.
E. KBr.
114. As indicator in Mor’s method is used:
A. AgNO3.
B. *K2CrO4.
C. NaCl.
D. CaSO4.
E. KBr.
115. Solutions of permanganate as titrant using in:
A. Acid-base titration.
B. Chelatometry.
C. Precipitation.
D. Sedimentation.
E. *Oxidation - reduction titration.
116. As primary standard in permanganatometry is used:
A. *H2C2O4.
B. NaCl.
C. K2CrO4.
D. H2SO4.
E. KBr.
117. Temporal hardness of water this:
A. Amount of Na hydrocarbonates.
B. Amount of Ca and Mg sulfates and chlorides.
C. Amount of Ca and Mg hydrocarbonates, sulfates and chlorides.
D. *Amount of Ca and Mg hydrocarbonates.
E. Total amount of salts.
118. A neutralization reaction it is reaction between:
A. Strong acids.
B. Weak acids.
C. Strong bases.
D. Weak bases.
E. *Acid and basis.
119. The water products this:
A. Products of solubility.
B. Sum of concentration of ions of Н+ and ОН-.
C. Change of concentrations.
D. *Products of concentration of hydrogen and hydroxide ions.
E. Difference of concentration of ions of Н+ and ОН-.
120. The oxidizing-restoration reactions are reaction in which:
A. Molecules are dissociated into ions.
B. Acid-basic interaction.
C. *Change of oxidation number of elements.
D. Hydrolyzed of salt.
E. Dissociate of acids.
121. Concentration of potassium permanganate is determined in?
A. In basic medium.
B. In neutral medium.
C. In weak bases medium.
D. *In acidic medium.
E. In alcohol solution.
122. Titrimetric analysis is used different reactions. What kind reaction is used for argentometry?
A. Oxidization reaction.
B. *Precipitation reaction.
C. Reduction reactions.
D. Neutralization reaction.
E. Chelatometry.
123. What elements are d-elements?
A. Sodium, Potassium
B. Calcium, Aluminum
C. Fluorine, Chlorine
D. Bromine, Iodine
E. *Iron, Manganese
124. What elements are p-elements?
A. Sodium, Potassium.
B. Calcium, Aluminum.
C. *Fluorine, Chlorine.
D. Lithium, Beryllium.
E. Iron, Manganese.
125. What elements are s-elements?
A. *Sodium, potassium.
B. Vanadium, Aluminum.
C. Fluorine, Chlorine.
D. Bromine, Iodine.
E. Iron, Manganese.
126. Basic metals this:
A. Calcium, Magnesium.
B. *Potassium, Sodium.
C. Iron, Manganese.
D. Sulfur, carbon.
E. Aluminum, Bromine.
127. How many maximally electrons can be on the 3 p sub-shull (electronic energetic level)?
A. 8.
B. 2.
C. 4.
D. *6.
E. 1.
128. What element is macro element?
A. *S.
B. I.
C. Br.
D. F.
E. Al.
129. What element is macro element?
A. Cd.
B. Cu.
C. *Na.
D. Mn.
E. Co.
130. What element is macro element?
A. Hg.
B. Mn.
C. Cu.
D. Br.
E. *Ca
131. What element is micro element?
A. C.
B. S.
C. *I.
D. K.
E. Ca.
132. What element is micro element?
A. *F.
B. Cl.
C. Ca.
D. O.
E. C.
133. Sodium dihydrogenphosphate is:
A. Na3PO4.
B. Na2HPO4.
C. *NaH2PO4.
D. Na3PO3.
E. NaH2PO5.
134. Chlorine ion is with such element in nature:
A. Hydrogen.
B. *Sodium, potassium, magnesium.
C. Oxigen and fluorine.
D. Oxigen, sulfur.
E. Copper.
135. For ditermine Fe2+ is used such complex compound:
A. Potassium cyanide cuprate(II).
B. Cupper potassium tetracyanate.
C. *Potassium hexacyanoferate(III).
D. Potassium hexacyanoferate(II).
E. Potassium tetracuprate(II)
136. For ditermine Fe3+is used such complex compound:
A. Potassium cyanide cuprate(II).
B. Cupper potassium tetracyanate.
C. Potassium hexacyanoferate(III).
D. *Potassium hexacyanoferate(II).
E. Potassium tetracuprate(II)
137. What micro element is in erythrocytes?
A. Sodium.
B. Vanadium.
C. Fluorine.
D. Bromine.
E. *Iron.
138. What element is in bones?
A. Sodium.
B. Vanadium.
C. Fluorine.
D. *Calcium.
E. Iron.
139. What element is privation in organism decopmost activiti of thyroid gland:
A. Sodium.
B. Vanadium.
C. *Iodine.
D. Calcium.
E. Iron.
140. What reagent is used for determination Ca2+ in solution?
A. *(NH4)2C2O4.
B. NaBr.
C. HCl.
D. HNO3.
E. KCl.
141. Aluminium is:
A. s - element.
B. d - element.
C. f - element.
D. *p - element.
E. g - element
142. Sodium is:
A. *s - element.
B. d - element.
C. f - element.
D. p - element
E. g - element
143. Potassium is:
A. *s - element.
B. d - element.
C. f - element.
D. p - element.
E. g - element
144. Iron is:
A. s - element.
B. *d - element.
C. f - element.
D. p - element.
E. g - element.
145. Magnesium is:
A. *s - element.
B. d - element.
C. f - element.
D. p - element.
E. g - element.
146. Iodine is:
A. s - element.
B. d - element.
C. f - element.
D. *p - element.
E. g - element.
147. Calcium is:
A. *s - element.
B. d - element.
C. f - element.
D. p - element.
E. g - element.
148. Fluorine is:
A. s - element.
B. d - element.
C. f - element.
D. *p - element.
E. g - element.
149. Chlorine is:
A. s - element.
B. d - element.
C. f - element.
D. *p - element.
E. g - element.
150. Bromine is:
A. s - element.
B. d - element.
C. f - element.
D. *p - element.
E. g - element.
151. Manganese is:
A. s - element.
B. *d - element.
C. f - element.
D. p - element.
E. g - element.
152. Zinc is:
A. s - element.
B. *d - element.
C. f - element.
D. p - element.
E. g - element.
153. What is name of K2[Cu (CN)4]?
A. Potassium cyanide cuprate(II).
B. Cupper potassium tetracyanate.
C. *Potassium tetracyanocuprate(II).
D. Potassium cyanatecuprate(II).
E. Potassium tetracuprate(II).
154. What is name of [Ag(NH3)2]OH?
A. *Diamminesilver(I) hydroxide.
B. Ammine argentums.
C. Silver hydroxide.
D. Ammine hydroxide.
E. Silver amide.
155. What is name of [Ag(NH3)2]Cl?
A. Diamminesilver(I) hydroxide.
B. Ammine argentums.
C. Silver hydroxide.
D. Ammine hydroxide.
E. *Diamminesilver(I) chloride.
156. What is name of [Cr(H2O)6](NO3)3?
A. Sodium hexahydroxochromate (IV).
B. *Hexaaquachromium(III)nitrate.
C. Tetracorbonylnickel.
D. Sodium tetrahydroxoaluminate.
E. Sodium hexahydroxostannate (IV).
157. What is name of [Ni(CO)4]?
A. *Tetracorbonylnickel.
B. Nickel carbonate.
C. Nickel carbon.
D. Nickel carbon monoxide.
E. Tetraammine nicol(II)bromite.
158. What is name of [Pt (NH3)4][PtCl6]?
A. Hexachloroplatinum(II) platinate (IV).
B. Platinum(II)hexachloroplatinate (IV).
C. *Tetraammineplatinum(II)hexachloroplatinate (IV).
D. Tetraccholoplatinum(III) chloride.
E. Tetraamminecopper(II)bromite.
159. What is name of [Cu(NH3)4]Br2?
A. Hexaaquachromium(III)nitrate.
B. Diamminesilver(I) chloride.
C. Tetraammineplatinum(II)hexachloroplatinate (IV).
D. Tetracorbonylnickel.
E. *Tetraamminecopper(II)bromite
160. What is name of Na[Al(OH)4]?
A. Aluminum sodium.
B. *Sodium tetrahydroxoaluminate.
C. Potassuin bicyanobis(oxalo)nikelate(II).
D. Sodium hydroxide.
E. Aluminum sulfate.
161. What is name of Na2[Sn(OH)6]?
A. *Sodium hexahydroxostannate (IV).
B. Tetraammineplatinum(II)hexachloroplatinate (IV).
C. Diamminesilver(I) hydroxide.
D. Hexaamminenickel(II) bromide.
E. Sodium tetrahydroxoaluminate.
162. What is name of K4[Ni(CN)2(OOC-COO)2]?
A. Diamminenicel(I) hydroxide.
B. Tetraammineaquachlorocobalt(III) chloride
C. Tetraammineplatinum(II)hexachloroplatinate (IV).
D. Hexaamminenickel(II) bromide.
E. *Potassuin bicyanobis(oxalo)nikelate(II).
163. What is name of [Co(NH3)4(H2O)Cl]Cl2?
A. Potassium cyanide cuprate(II).
B. Cupper potassium tetracyanate.
C. Potassium tetracyanocobalt(II).
D. *Tetraammineaquachlorocobalt(III) chloride.
E. Diamminesilver(I) hydroxide.
164. What is ligand name in following complex compound K2[Cu (CN)4]?
A. Cyanide.
B. *Cyano.
C. Nitroso.
D. Nitro.
E. Ammine.
165. What is central ion in complex compound [Cu(NH3)4]CrO4?
A. Ammine.
B. *Cupper.
C. Chromium.
D. Oxygen.
E. Hydrogen.
166. What is dentaty of ligand in following complex compound [Ni(CO)4]?
A. *1.
B. 2.
C. 0.
D. 4.
E. 6.
167. What kind is the following complex compound [Cr(Н2О)6](OH)3?
A. Acidic complex.
B. *Cationic complex.
C. Anionic complex.
D. Basic complex.
E. Neutral complex.
168. What is oxidation number of central ion for the following complex compound [Ni(CO)4]?
A. 1.
B. *0.
C. 4.
D. 3.
E. 6.
169. What is ligand name in following complex compound [Cu(NH3)4]CrO4?
A. Ammonia.
B. *Amino.
C. Chromo.
D. Chromate.
E. Ammine.
170. What is central ion in complex compound [Co(NH3)6]CrO4?
A. Ammine.
B. *Cobalt.
C. Chromium.
D. Oxygen.
E. Hydrogen.
171. What is dentaty of ligand in following complex compound [Co(NH3)6]CrO4?
A. 8.
B. 2.
C. *1.
D. 4.
E. 6.
172. What is coordination number of Ag in the [Ag(NH3)2]OH?
A. 1.
B. *2.
C. 8.
D. 4.
E. 6.
173. What kind is the following complex compound [Co(NO2)(NH3)3]SO4?
A. Acidic complex.
B. Anionic complex.
C. *Cationic complex.
D. Basic complex.
E. Neutral complex.
174. What is oxidation number of central ion for the following complex compound [Co(NO2)2(NH3)3]2+?
A. 0.
B. 1.
C. 3.
D. *4.
E. 6.
175. What ligand name, which is in following complex compound K2[Pt C16]?
A. Potassium.
B. Platinum.
C. *Chloro.
D. Chloral.
E. Platinate.
176. What is central ion in complex compound K2[Pt C16]?
A. Potassium.
B. *Platinum.
C. Chloro.
D. Chloral.
E. Paladium.
177. What is coordination number of Co in the [Co(NH3)4(H2O)Cl]Cl2?
A. 1.
B. 2.
C. 8.
D. 4.
E. *6.
178. What is dentaty of ligand in following complex compound K2[Pt C16]?
A. *1.
B. 2.
C. 0.
D. 4.
E. 6.
179. Coordination number of Ni in the K4[Ni(CN)6]:
A. 1.
B. 2.
C. 8.
D. 4.
E. *6.
180. What kind is the following complex compound K4[Ni(CN)2(OOC-COO)2]?
A. Acidic complex.
B. Cation complex.
C. *Anionic complex.
D. Basic complex.
E. eutral complex.
181. What is dentaty of -OOC-COO- in following complex compound K4[Ni(CN)2(OOC-COO)2]?
A. 1.
B. *2.
C. 0.
D. 4.
E. 6.
182. What is coordination number of Sn in the [Sn(NH3)2Cl2]Cl2?
A. 1.
B. 2.
C. 8.
D. *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.
B. +3.
C. +4.
D. +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. 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. Potassium chloride.
B. Sugar.
C. Oil.
D. D.*Carbon (II) oxide.
E. Sulfuric acid.
256. When cells are placed in 5 % solution of sodium chloride so red blood cells will:
A. Hemolisis.
B. No changes
C. *Plasmolisis.
D. The swell and rupture.
E. Electrophoresis.
257. A supersaturated:
A. *Solution is in which the concentration of solute is greater than its concentration in a saturated solution.
B. Solution is in which the concentration of solute is less than its concentration in a saturated solution.
C. Solution is in which the concentration of solute is less than 1 mole.
D. Solution is in which the concentration of solute same as solubility.
E. Solution is in which the concentration of solute less then solubility.
258. It is used 20 g of magnums nitrate for prepare 400 g solution. What is mass percent of this solution?
A. 40 %.
B. 20 %.
C. 0,1 %.
D. 10 %.
E. *5 %.
259. What is unit of gas solubility in water:
A. By mole per 1000g of solvent.
B. By mole.
C. By percent solute.
D. *By mole per milliliter of solvent.
E. By grams.
260. Hemolysis is phenomenon when cells are placed in а sodium chlorate solution with:
A. 0,9 %.
B. 2,9 %.
C. *0,5 %.
D. 1,5 %.
E. 2,5 %.
261. Value of osmotic pressure is charecterised by:
A. Mendeleev-Сlapeyron law.
B. Raoult’s law.
C. Henry’s law.
D. Henderson-Hasselbalch law.
E. *van’t Hoff law.
262. Choose the substance solubility which is increase with increasing temperature:
A. *Sodium sulfate.
B. Carbon (ІV) oxide.
C. Oxygen.
D. Sulfur (ІV) oxide.
E. Nitrogen.
263. Solid solution is:
A. Mixture of NH3 and H2.
B. Mixture of clay and water.
C. Solution of sand and oil.
D. *Alloy of copper and aluminum.
E. Solution of sodium sulfate.
264. True solution is solution with:
A. *The sizes of particles less than 10-9 m.
B. The sizes of particles 10-7-10-9 m.
C. 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.
Question to pictures
1. What measurement is represented on fig. 1.a?
A. *Areometer.
B. Alcohol gauge.
C. Saccharometer.
D. Thermometer.
E. Manometer.
2. What measurement is represented on fig. 1a?
A. *Areometer.
B. Alcohol gauge.
C. Saccharometer.
D. Thermometer.
E. Manometer.
3. What measurement is represented on fig. 1.a?
A. *Areometer.
B. Alcohol gauge.
C. Saccharometer.
D. Thermometer.
E. Manometer.
4. What measurement is represented on fig. 2 in active position?
A. *Areometer.
B. Alcohol gauge.
C. Saccharometer.
D. Thermometer.
E. Manometer.
5. What factors is influence for solubility process, which is represented on figure 3?
A. Density.
B. Temperature.
C. *Pressure.
D. Concentration.
E. Area of surface.
6. Equation, which is represented on figure 4, it is ….. law equation.
A. *Mendeleev-Klauperon.
B. Raoult's
C. Henry's
D. Henderson-Hasselbalch
E. van’t Hoff
7. Mendeleev-Klauperon law equation is represented on figure 4. Letter “V” is marked ….. in this formula.
A. Pressure
B. *Volume
C. Temperature
D. Density
E. Universal gas constant
8. Mendeleyev-Klauperon law equation is represented on figure 4. Letter “p” is marked ….. in this formula.
A. *Pressure.
B. Volume.
C. Temperature.
D. Density.
E. Universal gas constant.
9. Mendeleyev-Klauperon law equation is represented on figure 4. Letter “R” is marked ….. in this formula.
A. Pressure.
B. Volume.
C. Temperature.
D. Density.
E. *Universal gas constant.
10. Mendeleyev-Klauperon law equation is represented on figure 4. Letter “T” is marked ….. in this formula.
A. Pressure.
B. Volume.
C. *Temperature.
D. Density.
E. Universal gas constant.
11. Mendeleyev-Klauperon law equation is represented on figure 4. Letter “n” is marked ….. in this formula.
A. Pressure.
B. Volume.
C. *Amount mole of compound.
D. Density.
E. Universal gas constant.
12. Mathematical expression, which is represented on figure 5, it is ….. law equation.
A. *First Raoult's law.
B. Second Raoult's law.
C. Henry's.
D. Henderson-Hasselbalch.
E. van’t Hoff.
13. Mathematical expression, which is represented on figure 6, it is ….. law equation.
A. *First Raoult's law.
B. Second Raoult's law.
C. Henry's law.
D. Arrhenius law.
E. van’t Hoff law.
14. Mathematical expression, which is represented on figure 7, it is ….. law equation.
A. First Raoult's law.
B. *Second Raoult's law.
C. Henry's law.
D. Arrhenius law.
E. van’t Hoff law.
15. Second Raoult's law equation is represented on figure 7. Letter “K” is marked ….. in this formula.
A. Pressure.
B. Temperature.
C. *Cryoscopic constant.
D. Ebullioscopic constant.
E. Molality.
16. Phase diagram of the water is represented on figurer 8. The “O” point is:
A. The milting curve.
B. The boiling curve.
C. The sublimation curve.
D. *The triple point.
E. The milting point.
17. What is graph name which is represented on figure 9?
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.
18. Phase diagram of the water is represented on figurer 9. 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.
19. Phase diagram of the water is represented on figurer 9. The “OS” curve is named:
A. *The milting curve.
B. The boiling curve.
C. The sublimation curve.
D. The triple point.
E. The milting point.
20. Phase diagram of the water is represented on figurer 9. 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.
21. Mathematical expression, which is represented on figure 10, it is formula for calculation:
A. *The molar fraction of sulute.
B. The mass fraction.
C. The volume fraction.
D. The molar concentration (malarity).
E. The mass concentration.
22. Mathematical expression, which is represented on figure 10, it is formula for calculation the molar fraction
of solute. Letter “n1” is marked:
A. *The number mole of solvent.
B. The number mole of solute.
C. The mole fraction.
D. The molar concentration.
E. The volume fraction.
23. Mathematical expression, which is represented on figure 10, it is formula for calculation the molar fraction
of solute. Letter “n2” is marked:
A. The number mole of solvent.
B. *The number mole of solute.
C. The mole fraction.
D. The molar concentration.
E. The volume.
24. Equation which is represented on figure 11, 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.
25. The formula which represented on figure 12 is used for calculation:
A. Pressure.
B. Mass fraction.
C. *Density.
D. Molar fraction.
E. Molarity.
26. Formulas of some compounds are represented on figure 13. To choose the matter which is used for
standardize sodium hydroxide solution.
A. *1.
B. 2.
C. 3.
D. 4.
E. 5.
27. 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. 13).
A. 1.
B. 2.
C. 3.
D. 4.
E. *5.
28. Acid-base titration is the titrimetrical analysis method. What are you use as secondary standard solutions in
this method (fig. 14)?
A. 1.
B. *2.
C. 3.
D. 4.
E. 5.
29. What is process name which is represented on figure 15?
A. Preparation of solution.
B. Measuring of solution temperature.
C. *Titration of solution.
D. Determination of electrode potential.
E. Determination of pH solution.
30. Analytical chemists use a variety of glassware to measure volume. Typical instrumentation for performing
titration is on figure 15. Glassware which is represented by a number 1 is named:
A. Volumetric flask.
B. Conical retort.
C. Pipette.
D. *Burette.
E. Cylinder.
31. Typical instrumentation for performing titration is on figure 15. Glassware which is represented by a
number 2 is named:
A. Volumetric flask.
B. *Conical retort.
C. Pipette.
D. Burette.
E. Cylinder.
32. A variety of glassware is used in analytical chemistry to measure volume. What is glassware name which is
represented on figure 16.а.
A. *Measured glass.
B. Measured pipette.
C. Burette.
D. Cylinder.
E. Volumetric flask.
33. What is glassware name which is represented on figure 16.b.
A. Measured glass.
B. Measured pipette.
C. Burette.
D. *Cylinder.
E. Volumetric flask.
34. A variety of glassware is used in analytical chemistry to measure volume. What is glassware name which is
represented on figure 16.c.
A. Measured glass.
B. Measured pipette.
C. Burette.
D. Cylinder.
E. *Volumetric flask.
35. A variety of glassware is used in analytical chemistry to measure volume. What is glassware name which is
represented on figure 16.d.
A. Measured glass.
B. *Measured pipette.
C. Burette.
D. Cylinder.
E. Volumetric flask.
36. A variety of glassware is used in analytical chemistry to measure volume. What is glassware name which is
represented on figure 16.e.
A. Measured glass.
B. Measured pipette.
C. *Burette.
D. Cylinder.
E. Volumetric flask.
37. A variety of chemical reaction is used in analytical chemistry. What is method name, which uses reaction 1
(fig. 17).
A. *Acid-basic titration.
B. Precipitation method.
C. Chelatometry.
D. Oxidation-restoration titration.
E. Complexometric titration.
38. A variety of chemical reaction is used in analytical chemistry. What is method name, which uses reaction 2
(fig. 17).
A. Acid-basic titration.
B. *Precipitation method.
C. Chelatometry.
D. Oxidation-restoration titration.
E. Complexometric titration.
39. A variety of chemical reaction is used in analytical chemistry. What is method name, which uses reaction 3
(fig. 17).
A. Acid-basic titration.
B. Precipitation method.
C. Chelatometry.
D. *Oxidation-restoration titration.
E. Complexometric titration.
40. A variety of chemical reaction is used in analytical chemistry. What is method use reaction 3 (fig. 17) for
standardization secondary standard?
A. Acid-basic titration.
B. Precipitation method.
C. Chelatometry.
D. *Oxidation-restoration titration.
E. Complexometric titration.
41. What compound you can standardization, if is used reaction 3 (fig. 17)?
A. Sulfuric acid.
B. Carbon oxide (IV).
C. *Potassium permanganate.
D. Oxalic acid.
E. Potassium sulfate.
42. End point is indicated by instrumentation. What analytical method is used galvanic element which is
represented on figure 18?
A. Precipitation method.
B. Chelatometry.
C. Gravimetric analysis.
D. *Acid-basic titration.
E. Complexometric titration.
43. Formula, which is represented on fig. 19.1, is used for a calculation:
A. Molar concentration (molarity).
B. *Titre (mass concentration).
C. Normality (molar concentration of equivalent).
D. Molar concentration of equivalent.
E. The mass of the determined compound in titrimetrical analysis.
44. Formula, which is represented on fig. 19.(2), is used for a calculation:
A. *Molar concentration (molarity).
B. Titre (mass concentration).
C. Mass fraction.
D. Molar concentration of equivalent (normality).
E. The mass of the determined compound in titrimetrical analysis.
45. Formula, number 3, which is represented on fig. 19, is used for a calculation:
A. Molar concentration (molarity).
B. Titre (mass concentration).
C. *Molar concentration of equivalent (normality).
D. The mass of the determined compound in titrimetrical analysis.
E. Molar concentration of investigation solution in titrimetrical analysis.
46. Formula, which is represented on fig. 19.4, is used for a calculation:
A. Molar concentration (molarity).
B. Titre (mass concentration).
C. Molar concentration of equivalent (normality).
D. Mass fraction.
E. *Molar concentration of investigation solution in titrimetrical analysis.
47. On fig. 19.5 is represented formula, which is used for a calculation:
A. Molar concentration.
B. Titre (mass concentration).
C. Mass fraction..
D. Molar concentration of equivalent (normality).
E. *Equivalent law.
48. Which volumetric analysis is used the compound (fig. 20.4) as the secondary standard?
A. *Acid-basic titration.
B. Precipitation method.
C. Chelatometry.
D. Oxidation-restoration titration.
E. Complexometric titration.
49. Which volumetric analysis is used the compound (fig. 20.2) as the secondary standard?
A. Acid-basic titration.
B. Precipitation method.
C. *Oxidation-restoration titration.
D. Complexometric titration.
E. Alkalimetry.
50. Which volumetric analysis is used the compound (fig. 20.5) as the secondary standard?
A. Acid-basic titration.
B. *Precipitation method.
C. Chelatometry.
D. Oxidation-restoration titration.
E. Complexometric titration.
51. Which volumetric analysis is used the compound (fig. 20.3) as the secondary standard?
A. Argentometry.
B. Precipitation method.
C. *Alkalimetry.
D. Oxidation-restoration titration.
E. Complexometric titration.
52. Which volumetric analysis is used the compound number 1 (fig. 20.) as the secondary standard?
A. Acid-basic titration.
B. Precipitation method.
C. *Oxidation-restoration titration.
D. Complexometric titration.
E. Alkalimetry.
53. On figure 21.1 is represent:
A. *The ionic coordinating sphere.
B. The coordinating sphere.
C. The coordination number.
D. The ligand.
E. The central metal ion.
54. On figure 21.2 is represent:
A. The ionic coordinating sphere.
B. *The coordinating sphere.
C. The coordination number.
D. The ligand.
E. The central metal ion.
55. On figure 21 number3 is represent:
A. The ionic coordinating sphere.
B. The coordinating sphere.
C. The coordination number.
D. The ligand.
E. *The central metal ion.
56. On figure 21.4 is represent:
A. The ionic coordinating sphere.
B. The coordinating sphere.
C. *The coordination number.
D. The ligand.
E. The central metal ion.
57. On figure 21.5 is represent:
A. The ionic coordinating sphere.
B. The coordinating sphere.
C. The coordination number.
D. *The ligand.
E. The central metal ion.
58. Name of compound (fig.21) is:
A. *Potassium hexacianoferrate (III)
B. Potassium hexacianoferrate (II)
C. Potassium irone (III) hexacianate
D. Potassium irone (III)cianade
E. Potassium cianade ferrate (III)
59. The oxidation number of central atom ion in compound (fig. 21) is:
A. +1.
B. +2.
C. *+3.
D. +4.
E. -2.
60. The coordination number of central atom ion in compound (fig. 21) is:
A. 3.
B. 2.
C. *6.
D. 4.
E. 5.
61. Name of compound (fig.22) 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.
62. The oxidation number of central atom ion in compound (fig. 22) is:
A. +1.
B. *+2.
C. +3.
D. +4.
E. -2.
63. The coordination number of central atom ion in compound (fig. 22) is:
A. 3.
B. 2.
C. 6.
D. *4.
E. 5.
64. On figure 22.1 is represent:
A. The ionic coordinating sphere.
B. The coordinating sphere.
C. The coordination number.
D. The ligand.
E. *The central metal ion.
65. On figure 22.2 is represent:
A. The ionic coordinating sphere.
B. The coordinating sphere.
C. The coordination number.
D. *The ligand.
E. The central metal ion.
66. On figure 22.3 is represent:
A. The ionic coordinating sphere.
B. The coordinating sphere.
C. *The coordination number.
D. The ligand.
E. The central metal ion.
67. On figure 22(4) is represented:
A. *The ionic coordinating sphere.
B. The coordinating sphere.
C. The coordination number.
D. The ligand.
E. The central metal ion.
68. On figure 22.5 is represent:
A. The ionic coordinating sphere.
B. *The coordinating sphere.
C. The coordination number.
D. The ligand.
E. The central metal ion.
69. What is the product of reaction, which is represented on figure 23?
A. KHSO4
B. *K3[Al(OH)6]
C. K[Al(OH)4]
D. K3AlO3
E. Al2O3
70. What is the product of reaction, which is represented on figure 24?
A. K2SO4
B. Fe(CN)2
C. Fe(CN)3
D. *K4[Fe(CN)6]
E. K3[Fe(CN)6]
71. What is the product of reaction, which is represented on figure 25?
A. Fe(CN)4
B. *Na3[Fe(CN)6]
C. NaSO4
D. Fe(CN)2
E. Fe(CN)3
72. The name of compound (fig.26) 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)
73. The oxidation number of central atom ion in compound (fig. 26) is:
A. +1.
B. +2.
C. +3.
D. *+4.
E. -2.
74. The coordination number of central atom ion in compound (fig. 26) is:
A. 3.
B. 2.
C. *6.
D. 4.
E. 5.
75. The name of compound (fig.27) is:
A. *The aquadiaminochloropalladium (ІІ) chloride.
B. The diaminohydroxochloride palladium (ІІ).
C. The palladium (ІІ) chloroaquaammonium.
D. The dichlorodiaminoaquapalladiate.
E. The palladium (ІІ) diaminoaquachloride.
76. The oxidation number of central atom ion in compound (fig. 27) is:
A. +1.
B. *+2.
C. +3.
D. +4.
E. -2.
77. The coordination number of central atom ion in compound (fig. 27) is:
A. 3.
B. 2.
C. 6.
D. *4.
E. 5.
78. Ligands are in the complex compound, which is represented on figure 28:
A. NH3, NO2-.
B. Ni2+, NH3, NO2-.
C. Ni2+, NH3, Cl-.
D. *NH3, NO2-, Cl-.
E. Ni2+, NO2-, Cl-.
79. The oxidation number of central atom ion in compound (fig. 28) is:
A. +1.
B. *+2.
C. +3.
D. +4.
E. -2.
80. The name of compound (fig.29) is:
A. The dihydroxodiaminocopper (ІІ) dibrom.
B. The diaminodihydroxocopper (ІІ) bromide
C. The copper (ІІ) diaminodihydroxo bromide.
D. The dibromodiaquadiamino cuprate.
E. *The diaquadiaminocopper (ІІ) bromide.
81. The name of compound (fig.30) 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.
82. The electron configurations of atoms are represented on figure 31. What is electron configuration of
univalent atom state?
A. 1.
B. 2.
C. 3.
D. *4.
E. 5.
83. The electron configurations of atoms are represented on figure 31. What is electron configuration of bivalent
atom state?
A. *1.
B. 2.
C. 3.
D. 4.
E. 5.
84. The electron configurations of atoms are represented on figure 31. What is electron configuration of
trivalent atom state?
A. 1.
B. *2.
C. 3.
D. 4.
E. 5.
85. The electron configurations of atoms and ion are represented on figure 31. What is electron configuration of
quadrivalent atom state?
A. 1.
B. 2.
C. 3.
D. *4.
E. 5.
86. The electron configurations of atoms and ion are represented on figure 31. What is electron configuration of
fivevalency atom state?
A. 1.
B. 2.
C. 3.
D. 4.
E. *5.
87. What element can form crystals in cell which are represented on figure 32?
A. Potassium.
B. *Calcium.
C. Sodium.
D. Aluminium.
E. Chlorine.
88. What buffer solution has composition which is represented on figure 33?
A. Bicarbonate.
B. Phasphate.
C. Acetate.
D. *Protein.
E. Ammoniacate.
89. Formula which is represented on figure 34 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.
90. Formula which is represented on figure 34 is used for the calculation рН value of solution. To calculate рН
value of solution if concentration of hydroxonium ions is 0,01 mole/l?
A. *2.
B. 1.
C. 10.
D. 3.
E. 0,1.
91. The shrinkage of red blood cells in hypertonic solution is represented on figure 36:
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.
92. Red blood cells will swell and rupture when they are immersed in pure water. On figure 36 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.
93. The effect of isotonic solutions cause no changes in cell volume is represented on figure 36:
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.
94. Plasmolysis (crenation) is represented on figure 36:
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.
95. Hemolysis is represented on figure 36:
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.
96. What phenomenon is represented on the left in figure 36?
A. The effect 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.
97. What phenomenon is represented on the right in figure 36?
A. *The effect 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
98. What phenomenon is represented in the middle of figure 36?
A. The effect of isotonic solutions causes 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.
99. What is instrument represent on fig. 37?
A. Barometer.
B. *Osmometer.
C. Areometer.
D. Dialyser.
E. Saccharometer .
100. The standard test solutions (fig.38) is used for measure рН solutions. What is method use this test?
A. *The colorimetric method.
B. The potentiometric method.
C.
D.
E.
101.
A.
B.
C.
D.
E.
102.
A.
B.
C.
D.
E.
The photometric method.
The polarimetric method
The conductometric method
What is name compound, formula which is represented on fig. 39?
Sodium sulfate.
Sodium sulfite.
*Sodium hydrogen sulfate.
Sodium hydrogen sulfite.
Sodium thiosulfate.
What is ions form, if compound (fig.39) is dissociated?
Sodium cation and sulfate anion.
Sodium cation and sulfite anion.
*Sodium cation and hydrogen sulfate anion.
Sodium cation and hydrosulfite anion.
Sodium cation and thiosulfate anion.