DANYLO HALYTSKY LVIV NATIONAL MEDICAL UNIVERSITY
DEPARTMENT of GENERAL, BIOINORGANIC, PHYSICAL and
COLLOIDAL CHEMISTRY
V.V. Ogurtsov, O.M. Roman, O.V. Klenina
MULTIPLY CHOICE QUESTIONS
ON MEDICAL CHEMISTRY
(Module 1. Acid-Base Equilibrium and Coordination Compounds
Formation Processes in Biological Liquids)
For the 1st year students
оf medical faculty
L’VIV – 2012
Chapter 1. Solutions. Ways of Expressing Concentrations of
Solutions. Preparation of Solution With the
Known Concentration
1.1. What shows a curve of solubility
of a gas?
А. dependence solubility of a gas
with temperature
B. dependence solubility of a gas
with pressure
C. dependence solubility of a gas
with nature of compound
D. dependence solubility of
a gas with presence of
another substances
E. dependence solubility of a gas
with nature of solvent
1.2. How changes the solubility of
gases with increasing a pressure?
А. decrease
B. does not change
C. increase proportionally
D. solubility doesn’t depend on
pressure
E. decrease proportionally
E. decrease
1.5. How changes the solubility of a
gas with decreasing a
temperature?
А. does not change
B. increase proportionally
C. decrease
D. increase
E. 1.6. How changes the solubility of an
oxygen in a blood with increasing
a pressure?
А. increase
B. decrease proportionally
C. D. decrease
E. does not change
1.3. How changes the solubility of
gases with decreasing a pressure?
А. does not change
B. decrease
C. decrease proportionally
D. solubility doesn’t depend on
pressure
E. increase proportionally
1.7. Mass percentage of solute – that
is:
А. the percentage by mass of
solute contained in a solution
B. relation between number of
solute and mass of solvent
C. gram of solute in 1000g of
solution
D. relation between mass of
solute and volume of solution
E. number of moles of solute that
are in 100g of solution
1.4. How changes the solubility of
gases in water with increasing a
temperature?
А. increase
B. increase proportionally
C. D. does not change
1.8. Molarity – that is:
А. number of moles of solute that
are in 1kg of solvent
B. number of moles of solute that
are in 1kg of solution
C. number of moles of solute that
are in 100сm3 of solution
D. number of moles of solute that
are in 1сm3 of solution
E. number of moles of solute that
are in 1L of solution
1.9. Molality – that is:
А. number of moles of solute that
are in 1kg of solution
B. number of moles of solute that
are in 100сm3 of solution
C. number of moles of solute that
are in 1L of solution
D. number of moles of solute that
are in 1сm3 of solution
E. number of moles of solute that
are in 1kg of solvent
1.10. Normality (molar concentration of
equivalent) – that is:
А. number of mol-equivalen of
solute that are in 1 cm3of
solution
B. number of mol-equivalen of
solute that are in 100 сm3 of
solution
C. number of mol-equivalen of
solute that are in 1kg of
solution
D. number of mol-equivalen of
solute that are in 1kg of
solvent
E. number of mol-equivalen of
solute that are in 1L of
solution
1.11. Titr – that is:
А. number of gram of solute in 1
L of solution
B. number of gram of solute in 1
cm3 of solution
C. number of gram of solute in 1
kg of solution
D. number of gram of solute in 1
сm3 of solvent
E. number of gram of solute in 1
g of solvent
1.12. Mole fraction of a solute – that is:
А. moles of solute divided by the
moles of solvent
B. moles of component substance
divided by the total moles of
solution
C. moles of solvent divided by
the moles of solute
D. moles of solvent divided by
the total moles of solution
E. relation between number of
particles in a system solute and
mass
1.13. How many grams of AgNO3 are
required to prepare 10 g of 2%
solution?
А. 0.2
B. 20
C. 0.1
D. 10
E. 2
1.14. How many grams of NaCl are
required to prepare 200 g of 0.9 %
solution?
А. 0.18
B. 1.8
C. 9
D. 0.9
E. 18
1.15. How many grams of glucose are
required to prepare 500 g of 5%
solution?
А. 25
B. 50
C. 100
D. 5
E. 15
1.16. How many grams of NaCl are
required to prepare 50 g of 10%
hypertonic solution?
А.
B.
C.
D.
E.
5g
0,5 g
1g
10 g
50 g
1.17. How many grams of glucose are
required to prepare 200 g of 4%
hypotonic solution?
А. 8 g
B. 2 g
C. 20 g
D. 200 g
E. 80 g
1.18. How many grams of glucose are
required to prepare 200 g of 5%
isotonic solution?
А. 20 g
B. 5 g
C. 100 g
D. 50 g
E. 10 g
1.19. What is the mass percentage (%)
of C12H22O11 in a solution that
contains 30.0 g of C12H22O11 in
570 g of water?
А. 10
B. 5
C. 20
D. 30
E. 15
1.20. What is the mass percentage (%)
of glucose in a solution that
contains 20 g of glucose in 180 g
of water?
А. 10
B. 20
C. 5
D. 30
E. 15
1.21. What is the mass percentage (%)
of glycerin in a solution that
contains 40.0 g of glycerin in 360
g of water?
А. 10
B. 15
C. 40
D. 30
E. 20
1.22. What is the molarity of a solution
containing 4.0 g of NaOH in 500
ml of solution?
А. 0.25
B. 0.2
C. 0.1
D. 0.3
E. 0.15
1.23. What is the molarity of a solution
containing 40.0 g of NaOH in 800
ml of solution?
А. 2.50
B. 0.50
C. 1.50
D. 1.00
E. 1.25
1.24. What is the molarity of a solution
containing 9.8 g of H2SO4 in 200
ml of solution?
А. 1.00
B. 0.25
C. 0.10
D. 0.50
E. 0.75
1.25. What is the molarity of a solution
containing 98 g of H2SO4 in 600
ml of solution?
А. 1.50
B. 1.25
C. 1.83
D. 1.67
E. 1.00
1.26. What is the molarity of a solution
containing 5,6 g of KOH in 400
ml of solution?
А. 0.50
B. 0.25
C. 0.75
D. 1.00
E. 0.10
glucose and 18 mole Н2О?
А. 0.01
B. 2.0
C. 0.1
D. 0.2
E. 1.0
1.27. What is the molarity of a solution
containing 56 g of KOH in 500 ml
of solution?
А. 2.5
B. 0.5
C. 1.0
D. 2.0
E. 1.5
1.30. What is the mole fraction of a
solution containing 4 moles of
glucose and 36 mole Н2О?
А. 1. 0
B. 0.1
C. 4
D. 0.4
E. 2.0
1.28. What is the mole fraction of a
solution containing 2 moles of
NaOH and 18 mole Н2О?
А. 0.2
B. 0.02
C. 0.1
D. 2.0
E. 0.01
1.31. What is the mole fraction of a
solution containing 5 moles of
C12H22O11 and 45 mole Н2О?
А. 0.1
B. 0.01
C. 5
D. 0.05
E. 0.5
1.29. What is the mole fraction of a
solution containing 2 moles of
Chapter 2. Colligative Properties of solutions. Experimental
Determination of the Osmotic Concentration of
Solutions by the Method of Cryometry
2.1. Colligative properties depend on
the:
А. nature of solvent
B. temperature
C. number of solute and solvent
molecules (or ions)
D. percent of ionization
E. nature of solute
2.2. Colligative properties are:
А. diffusion
B. –
C. solubility
D. osmosis and diffusion
E. osmosis
2.3. Oncotic pressure – is:
А. osmotic pressure that is caused
by albumen molecules,
dissolved in a biological
liquids
B. osmotic pressure that is caused
by electrolytes in biological
liquids
C. total osmotic pressure of
biological liquids
D. E. osmotic pressure that is caused
by ions in biological liquids
2.4. Osmotic concentration
(osmolarity) – that is:
А. total concentration of solute
and solvent molecules in a
solution
B. molar concentration of
albumen molecules
C. concentration of electrolytes
D. mass percentage of
electrolytes
E. concentration of albumen
molecules
2.5. Solutions, which have the same
osmotic pressure are:
А. saturated
B. concentrated
C. hypotonic
D. isotonic
E. hypertonic
2.6. Value of an oncotic pressure (кPa)
is:
А. 3.5·102 – 3.9·102
B. 3.5 – 3.9
C. 0.35 – 0.39
D. 3.5·102 – 3.9·103
E. 3.5 – 3.9·102
2.7. Value of an osmotic pressure
(кPa) of a blood:
А. 7.4·103 – 7,8·102
B. 7.4 – 7.8
C. 7.4·10 – 7,8·102
D. 74 – 78
E. 7.4·102 – 7,8·102
2.8. What happen with red blood cells,
when they are placed in a
hypertonic solution?
А. hemolysis and crenation
B. C. diffusion
D. hemolysis
E. crenation
2.9. What happen with red blood cells,
when they are placed in a
hypotonic solution?
А. hemolysis and crenation
B. crenation
C. diffusion
D. hemolysis
E. osmosis
2.10. How to calculate osmotic pressure
of electrolytes solution?
А. π = νRT
B. π = iCNRT
C. π = iCmRT
D. π = CMRT
E. π = iCMRT
2.11. How to calculate osmotic pressure
of non-electrolytes solution?
А. π = CMRT
B. π = iCNRT
C. π = iCMRT
D. π = CNRT
E. π = (m/M)RT
2.12. Isotonic solutions are:
А. 0,9% NaCl and 0,5% glucose
B. 9% NaCl and 5% glucose
C. 9% NaCl and 0,5% glucose
D. 0,9% NaCl and 5%-glucose
E. 5% NaCl and 0,9% glucose
2.13. What happen with red blood cells,
when they are placed into a 10%
NaCl solution?
А. crenation
B. hemolysis
C. does not change
D. E. hemolysis and crenation
2.14. What happen with red blood cells,
when they are placed in a 1%
glucose solution?
А. crenation
B. does not change
C. hemolysis and crenation
D. hemolysis
E. 2.15. What happen with red blood cells,
when they are placed in a 5%
glucose solution?
А. does not change
B. hemolysis and crenation
C. diffusion
D. hemolysis
E. crenation
2.16. Freezing point depression
constant depend on the:
А. presence of catalyst
B. concentration of solution
C. nature of solute
D. temperature
E. nature of solvent
2.17. What is the freezing point of
solution (0С) containing 1 mol of
maltose and 2000 g of water?
А. +1.86
B. –1.86
C. –3.72
D. –0.93
E. +3.72
2.18. Boiling point elevation constant
depend on the:
А. temperature
B. concentration of solution
C. nature of solute
D. presence of catalyst
E. nature of solvent
2.19. What is the boiling point of
solution (0С) containing 2 mol of
glucose and 2000 g of water?
А. 101. 04
B. 101.,86
C. 100.00
D. 100.52
E. 101.00
2.20. What is the boiling point of
solution (0С) containing 1 mol of
urea and 500 g of water?
А. 101.04
B. 101.00
C. 101.86
D. 100.52
E. 100.00
Chapter 3. The Equilibrium and Processes Involving
Coordination Compounds. Preparation and
Properties of Coordination Compounds.
Complexonometry
3.1. The most stable coordination
compounds exist for:
А. alkaline earth metals
B. alkali metals
C. lantanoids
D. transition metals
E. s-elements
3.2. Point out the formula of the
coordination compound for which
the empirical formula is
PtCl4·4NH3 and the coordination
number of Pt(IV) is 6.
А. [PtCl4]
B. [Pt(NH3)2Cl4]
C. [Pt(NH3)4Cl2]Cl2
D. [PtCl3(NH3)3]Cl
E. [Pt(NH3)2Cl2]Cl2
3.3. Point out the formula of the
coordination compound for which
the empirical formula is
PtCl4·6NH3 and the coordination
number of Pt(IV) is 6.
А. [PtCl3(NH3)3]Cl
B. [Pt(NH3)2Cl4]
C. К2[PtCl6]
D. [Pt(NH3)4Cl2]Cl2
E. [Pt(NH3)6]Cl4
3.4. Point out the formula of the
coordination compound for which
the empirical formula is 2NH4Cl·
PtCl4?
А. [Pt(NH3)4Cl2]Cl2
B. [Pt(NH3)2Cl3]Cl
C. [Pt(NH3)6]Cl4
D. [Pt(NH3)2Cl4]
E. (NH4)2[PtCl6]
3.5. Select the anion complex ion from
the given ones:
А. [Cu(NH3)4]
B. [Cr(H2O)3Br]
C. [Cr(H2O)3(CN)3]
D. [Zn(OH)4]
E. [Ag(NH3)2]
3.6. Select the cation complex ion
from the given ones:
А. [Cu(СNS)4]
B. [Ag(СN)2]
C. [Al(OH)6]
D. [Zn(OH)4]
E. [Cr(H2O)4(CN)2]
3.7. Select the anion complex ion from
the given ones:
А. [Cu(NH3)4]
B. [Al(OH)6]
C. [Cu(H2O)4]
D. [Cr(NH3)3(CN)3]
E. [Cu(NH3)2Cl2]
3.8. Select the cation complex ion
from the given ones:
А. [HgI4]
B. [Cr(NH3)4(CNS)2]
C. [Cu(H2O)(CN)3]
D. [Cu(СN)4]
E. [Zn(OH)4]
3.9. What are the oxidation states of
the central metal ions in the
complex ions [Fe(CN)6]4– and
[Cr(H2O)4F2]+ ?
А.
B.
C.
D.
E.
+4, +3
+3, +3
+2, +3
+2, +2
+3, +2
3.10. What are the oxidation states of
the central metal ions in the
coordination compounds
[Cu(NH3)4]SO4 and
K2[Pt(OH)2Cl4]?
А. +2, +4
B. +2, +2
C. +1, +2
D. +2, +3
E. +1, +4
3.11. What are the oxidation state of the
central metal ion and the charge of
the complex ion for the
coordination compound
Na3[Cr(OH)6]?
А. +3, –2
B. +2, +4
C. +3, –3
D. +3, +3
E. +3, –4
3.12. What are the oxidation state of the
central metal ion and the charge of
the complex ion for the
coordination compound
[Co(NH3)4(CNS)2]Cl ?
А. +2, 4
B. +2, 6
C. +3, 6
D. +3, 2
E. +3, 4
3.13. What are the oxidation state of the
central metal ion and the charge of
the complex ion for the
coordination compound
K2[Pt(OH)2Cl4] ?
А. +2, –4
B. +4, +2
C. +4, 0
D. +2, –2
E. +4, –2
3.14. Select the most stable complex
ion of mercury through the listed
ones, if the complex ions have the
given values of the constants of
dissociation:
А. [HgBr4]2–, Кd = 1·10–21
B. [HgI4]2– ,Кd = 1.38·10–30
C. [Hg(СN)4]2–,Кd = 3·10–42
D. [HgCl4]2– ,Кd = 6·10–16
E. [Hg(CNS)4]2–, Кd = 1.3·10–22
3.15. Select the least stable complex ion
of zinc through the listed ones, if
the complex ions have the given
values of the constants of
dissociation:
А. [Zn(NH3)4]2+, Кd = 2.0·10–9
B. [Zn(CNS)4]2–,Кd = 5·10–2
C. [ZnЕДТА]2–, Кd = 3.2·10–17
D. [Zn(OH)4]2–, Кd = 2.2·10–15
E. [Zn(CN)4]2–, Кd = 1.0·10–10
3.16. Select the most stable complex
ion of Ag through the listed ones,
if the complex ions have the given
values of the constants of
dissociation:
А. [Ag(S2O3)2]3–, Кd = 3.5·10–14
B. [Ag(NO2)2]– , Кd = 1.8·10–3
C. [Ag(NH3)2]+ , Кd = 5.8·10–8
D. [Ag(CN)2]– , Кd = 1.4·10–20
E. [AgCl2]– , Кd = 9.1·10–6
3.17. The expression of the constants of
dissociation of complex ion for
the compound K4[Fe(CN)6] is:
А. [Fe 2 + ] ⋅ 6[CN − ]
[[Fe(CN) 6 ] 4− ]
E. [Co 2+ ] + [ NH ] 6
3
B. [Fe 3+ ] ⋅ [CN − ] 6
[[Fe(CN) 6 ]3− ]
C. [Fe 2+ ] ⋅ [CN − ] 6
[[Co( NH 3 ) 6 ] 2+ ]
[[Fe(CN) 6 ] 4− ]
D. [K + ] 4 ⋅ [[Fe(CN ) 6 ] 4 − ]
[K 4 [ Fe(CN ) 6 ]]
E. [Fe 2+ ] + [CN − ]6
4−
[[Fe(CN) 6 ] ]
3.18. The expression of the constants of
dissociation of complex ion for
the compound [Cu(NH3)4]SO4 is:
А. [Cu 2 + ] + [ NH ] 4
3
[[Cu ( NH 3 ) 4 ] 2 + ]
B. [Cu 2+ ] 2 ⋅ [ NH ] 4
3
[[Cu ( NH 3 ) 4 ] 2+ ]
C. [Cu 2 + ] ⋅ [ NH ] 4
3
[[Cu ( NH 3 ) 4 ] 2+ ]
D. [[Cu ( NH ) ]
3 4
2+
] ⋅ [SO 24 − ]
[[Cu ( NH 3 ) 4 ]SO 4 ]
E. [Cu 2 + ] ⋅ 4[ NH ]
3
2+
[[Cu ( NH 3 ) 4 ] ]
3.19. The expression of the constants of
dissociation of complex ion for
the compound [Co(NH3)6]Cl2 is:
А. [Co 2 + ] ⋅ 6[ NH ]
3
2+
[[Co( NH 3 ) 6 ] ]
B. [Co 2 + ] ⋅ 6[ NH ] ⋅ 2[Cl − ]
3
[[Co ( NH 3 ) 6 ]Cl 2 ]
C. [Co( NH ) ] ⋅ [Cl − ] 2
3 6
[[Co( NH 3 ) 6 ]Cl 2 ]
D. [Co
2+
] ⋅ [ NH 3 ]
6
[[Co( NH 3 ) 6 ] 2+ ]
3.20. The expression of the constants of
dissociation of complex ion for
the compound K2[HgI4] is:
А. [ K + ] 2 ⋅ [[HgI ] 2− ]
4
[ K 2 [HgI 4 ]]
B. [ Hg 2 + ] ⋅ [ I − ] 4
[[HgI 4 ] 2− ]
C.
[Hg 2 + ]2 ⋅ [I − ]
[[HgI 4 ]2 − ]
D. [K + ] 2 ⋅ [ Hg 2 + ] ⋅ [ I − ] 4
[ K 2 [ HgI 4 ]]
E. [ Hg
2+
] ⋅ 4[I − ]
[[HgI 4 ] 2− ]
3.21. The expression of the constants of
dissociation of complex ion for
the compound Na2[Zn(OH)4] is:
А. [ Zn 2+ ] + [OH − ] 4
[[Zn (OH) 4 ] 2− ]
B. [ Na + ] 2 ⋅ [ Zn 2 + ] ⋅ [OH − ] 4 ]
[ Na 2 [ Zn (OH ) 4 ]]
2
C. [ Zn + ] ⋅ [OH − ] 4
[[Zn (OH) 4 ] 2− ]
D. [ Zn 2 + ] ⋅ 4[OH − ]
[[ Zn (OH) 4 ] 2− ]
E. [ Na + ] 2 ⋅ [ Zn (OH ) 4 ] 2− ]
[ Na 2 [ Zn (OH ) 4 ]]
3.22. Select the most stable
amminecomplex through the
listed ones, if the complex ions
have the given values of the
constants of dissociation:
А. [Ni(NH3)6]2+, Кd = 1,2·10–8
B. [Zn(NH3)4]2+, Кd = 2,0·10–9
C. [Co(NH3)6]3+, Кd = 6,2·10–36
D. [Hg(NH3)4]2+, Кd = 5,2·10–20
E. [Cu(NH3)4]2+, Кd = 9,3·10–13
3.23. The quantitative characteristic of
complex ions stability in solution
is:
А. the percent of dissociation
B. the constant of dissociation
C. the equilibrium constant
D. the constant of hydrolysis
E. the constant of the complex
formation
3.24. What is the product of the reaction
of interaction of copper sulfate
with the excess of ammonium
hydroxide?
А. [Cu(OH)2(NH3)2]
B. [Cu(NH3)4](OH)2
C. [Cu(NH3)2(H2O)2]SO4
D. (NH4)2[Cu(OH)4]
E. Cu(OH)2
3.25. What is the product of the reaction
of Cu(OH)2 dissolving in the
excess of concentrated КОН?
А. K[Cu(OH)3]
B. [Cu(OH)2(H2O)2]
C. [Cu(H2O)4](OH)2
D. reaction doesn’t pass
E. K2[Cu(OH)4]
3.26. Which coordination compound
through the listed ones will form
when the solution of HgCl2 would
be acted with the excess of KI?
А. K2[HgI2Cl2]
B. [Hg(H2O)4]Cl2
C. K2[HgI4]
D. K2[HgCl4]
E. [HgI2]
3.27. Complete and balance the
equation of the reaction
Cu(OH)2 + NH4OHconc. →. Point
out the sum of the coefficients of
this equation.
А. 9
B. 6
C. 8
D. 10
E. 13
3.28. Complete and balance the
equation of the reaction AgBr +
Na2S2O3 →. Point out the sum of
the coefficients of this equation.
А. 4
B. 6
C. 8
D. 5
E. 7
3.29. Complete and balance the
equation of the reaction
[Cu(H2O)4]SO4 + NH3 →. Point
out the sum of the coefficients of
this equation.
А. 8
B. 9
C. 12
D. 11
E. 10
3.30. What coordination number is the
most common for Fe2+?
А. 5
B. 2
C. 8
D. 6
E. 4
3.31. The most stable coordination
compounds with aminocarbon
acids can form the following ions:
А. Cu, Zn, Co
B.
C.
D.
E.
Mn, Ni, Fe
Fe, Mn, Mg
Mn, Mg, Zn
Co, Fe, Zn
3.32. What is the oxidation state of the
central metal ion in the
coordination compound
Na2[Fe(CN)5NO]?
А. +2
B. 0
C. +3
D. +6
E. +1
3.33. Zinc can dissolve in the excess of
an alkali solution owing to the
complex ion formation:
А. [Zn(NH3)4]2+
B. [Zn(H2O)4]2+
C. [ZnCl4]2–
D. [Zn(OH)4]2–
E. ZnO22–
3.34. What is the geometry of the
hybrid orbitals in the coordination
compounds with the coordination
number 2 of the central metal ion
like [Ag(NH3)2]+?
А. octahedral
B. square planar
C. linear
D. tetrahedral
E. square pyramid
3.35. What will be the product of the
reaction between ZnCl2 and
potassium hexacyanoferrate (II)?
А. Zn3[Fe(CN)6]2
B. Fe[Zn(CN)4]
C. K2[Zn(CN)4]
D. Zn2[Fe(CNS)6]
E. Zn2[Fe(CN)6]
3.36. Complete and balance the
equation of the reaction
K4[Fe(CN)6] + Cl2 →. Point out
the sum of the coefficients of this
equation.
А. 4
B. 7
C. 8
D. 6
E. 16
3.37. Which ligands through the listed
ones are monodentate?
А. NH3 and CN–
B. OH– and SO42–
C. Cl– and P2O74–
D. Н2O and CO32–
E. NH3 and SO42–
3.38. Which ligands through the listed
ones are bidentate?
А. NH3 and CN–
B. Н2O and Br–
C. Н2O and CNS–
D. Cl– and CN–
E. CO32– and P2O74–
3.39. Which ligands through the listed
ones are monodentate?
А. С2О42–, CNS–, CN–
B. CO32–, Cl–, OH–
C. CO, NO, SO42–
D. NH3, CO32–, CNS–
E. NH3, CO, CN–
3.40. The components of coordination
compounds are:
А. the central metal ion and the
complex cation
B. the central metal ion and the
complex anion
C. the complex ion and the
external coordination sphere
D. the central metal ion and
ligands
E. the central metal ion and
positively or negatively
charged ions
3.41. What kind of chemical bonding is
obligatory in coordination
compounds?
А. ionic bonding
B. hydrogen bonding
C. covalent bonding
D. donor-acceptor bonding
E. metallic bonding
3.44. What is the molecular formula of
the coordination compound
diaquadiamminenicol(ІІ) nitrateт?
А. [Ni(OH)2(NH3)2](NO3)2
B. [Ni(H2O)2(NO3)2]
C. [Ni(H2O)2(NH3)2]NO3
D. [Ni(H2O)2(NH3)2](NO3)2
E. [Ni(H2O)2(NH3)2]NO2
3.42. What is the molecular formula of
the coordination compound
diammineditiocyanocopper(ІІ)?
А. (NH4)2[Cu (CN)2]
B. [Cu(NH3)2(CNS)2]
C. [Cu(NH3)2(CN)2]S
D. [Cu(NH3)2](CNS)2
E. (NH4)2[Cu (CNS)4]
3.45. What is the molecular formula of
the coordination compound
potassium
dihydroxotetrachlorochromate(ІІІ)
А. K[Cr(OH)2Cl2]
B. K[Cr(H2O)2Cl4]
C. K3[Cr(H2O)2(OH)2Cl2]
D. K3[Cr(OH)2Cl4]
E. [KCrCl4](OH)2
3.43. What is the molecular formula of
the coordination compound
pentaamminebromocobalt(ІІІ)
sulfate?
А. [Co(NH3)5Br]SO3
B. [Co(NH4)5Br](SO4)2
C. [Co(NО2)5Br]SO4
D. [Co(NH3)5Br]SO4
E. [Co(NH3)5SO4]Br
3.46. What is the molecular formula of
the coordination compound
dichloroaquatriamminecobalt(ІІІ)
bromide?
А. [CoCl2(NH3)3H2O]Br2
B. [Co(NH3)3(H2O)Br]Cl2
C. [Co(H2O)Cl2(NH3)3]Br
D. [Co(H2O)Br 2(NH3)3]Cl
E. [Co(H2O)BrCl2(NH3)2]
Chapter 4. Bioelements and Their Classification. Chemical
Properties and Biological Role of Macroelements
4.1. Hydrogen can be referred to as the
element of the following groups of
elements according to its chemical
properties:
А. halogens
B. alkaline earth metals and
halogens
C. alkaline metals
D. alkaline and alkaline earth
metals
E. alkaline metals and halogens
4.2. The bio-metals are able:
А. to adjust the acidic properties
of bio-systems only
B. to take part in reductionoxidation processes only
C. to take part in reductionoxidation reactions and
coordination compounds
formation processes
D. to take part in coordination
compounds formation
processes only
E. to adjust the acid-base
properties of bio-systems
4.3. Write down the molecular
formulas for sodium sulfide and
lithium hydrosulfate. What are the
valences of sulfur in these
compounds? Point out the sum of
these values.
А. 4
B. 8
C. 7
D. 6
E. 5
4.4. Write down the electronic formula
of Mg2+ion. What is the total
number of electrons in this ion?
А. 7
B. 8
C. 10
D. 12
E. 9
4.5. What chemical element
corresponds to the electronic
formula ns2?
А. Cu
B. Zn
C. Ba
D. K
E. Na
4.6. What is the number of the valence
electrons for the calcium atom?
А. 3
B. 4
C. 6
D. 1
E. 2
4.7. Which of the listed elements has
the lowest value of the ionization
energy?
А. Mg
B. Ca
C. P
D. K
E. N
4.8. What type of the crystal lattice do
the most salts of the alkaline
metals have?
А. metallic
B. ionic
C. molecular
D. atomic
E. –
E. K
4.9. What compounds are used in
medicine as soothing drugs?
А. NaCl, KBr, KF
B. KJ, NaJ, NaCl
C. NaBr, KBr, NaCl
D. KCl, NaCl, KF
E. NaBr, KBr, NH4Br
4.14. What reactant is used for the
identification of K+ion?
А. Na2S
B. (NH4)2C2O4
C. Na2CO3
D. NaH2SbO4
E. NaHC4H4O6
4.10. What chemical element is the most
abundant in hydrosphere?
А. Mg
B. Fe
C. Na
D. Ca
E. K
4.15. What reactant is used for the
identification of Na+ion?
А. NH4Cl
B. NaH2PO4
C. H2S
D. NH4SCN
E. KH2SbO4
4.11. Which ones through the listed
compounds are used as acid
reducers?
А. NaHCO3, MgO, Al(OH)3
B. NaOH, Ca(OH)2, NaHCO3
C. KOH, Fe(OH)3 , Al(OH)3
D. Na2CO3, MgO, Na2SiO3
E. NaHCO3, MgO, Fe(OH)3
4.16. What reactant is used for the
identification of Ca2+ion?
А. H2S
B. HNO3
C. NH4SCN
D. HCl
E. (NH4)2C2O4
4.12. The ion of which metal through
the listed ones is the most
abundant in biological liquids and
support the osmotic pressure and
the action of buffer systems?
А. magnesium
B. barium
C. calcium
D. potassium
E. sodium
4.13. Which s-element through the
listed ones is contained in the
greatest amounts in living
organisms?
А. Ca
B. Ba
C. Na
D. Mg
4.17. What reactant is used for the
identification of Mg2+ ion?
А. NaH2PO4
B. NaHC4H4O6
C. HCl
D. H2S
E. KH2SbO4
4.18. Which compounds through the
listed ones should be added to
water to decrease its hardness?
А. KI, Al2(SO4)3
B. Na2CO3, Na3PO4
C. MgSO4, Na2SO4
D. Ca(OH)2, CaSO4
E. NaCl, CaCl2
4.19. Which element through the listed
ones gives oxide Е2О when it
burns in the air or in the
atmosphere of oxygen?
А. K
B. Cs
C. Li
D. Rb
E. Na
4.20. Which salt of the s-elements
through the listed ones give the
alkali solution under the
hydrolysis?
А. CaCl2
B. Na2CO3
C. KNO3
D. LiBr
E. CaSO4
4.21. Whist s-element through the listed
ones does not react with water
under STP?
А. Ca
B. K
C. Ba
D. Na
E. Mg
4.22. The chemical activity of the
oxides in the row BeO – MgO –
CaO – BaO will:
А. decrease
B. firstly decrease, then increase
C. doesn’t change
D. increase
E. firstly increase, then decrease
4.23. The presence of which ions causes
the hardness of water?
А. Ba2+, Mg2+
B. K+, Mg2+
C. Na+, Ca2+
D. K+, Ca2+
E. Ca2+, Mg2+
4.24. Which elements through the listed
ones are organogen elements?
А. N, P, S, Fe, C
B.
C.
D.
E.
N, P, K, Mg, S
S, K, Mg, O, C
C, H, O, N, P, S
C, H, O, Ca, S
4.25. The majority of bioelements are
the elements of such periods of the
Periodic table:
А. III and IV periods
B. V and VI periods
C. I and II periods
D. III and V periods
E. IV and V periods
4.26. Point out the valence of chlorine
in its compounds KClO3 and
KClO.
А. 3, 2
B. 7, 3
C. 7, 1
D. 5, 1
E. 7, 5
4.27. Which chemical elements through
the listed ones is the most
abundant in the earth crust?
А. Ca
B. Fe
C. Si
D. O
E. Al
4.28. Which of the halogens is used in
medicine as a simple substance?
А. bromine
B. chlorine, iodine
C. chlorine, iodine, bromine
D. bromine, iodine
E. iodine
4.29. Which compound through the
listed ones is used for the
identification of the halogens
ions?
А. Mg(NO3)2
B. KNO3
C. AgNO3
D. Ba(NO3)2
E. NaNO3
4.30. Which elements of the VIА group
of the Periodic table are the
organogen elements?
А. S, Te
B. O, Se
C. O, Te
D. Po, S
E. O, S
4.31. Which oxygen compound through
the listed ones is used as
disinfection means in medicine?
А. potassium perchlorate
B. calcium hypochlorite
C. ozone
D. hydrogen peroxide
E. hydrogen oxide
4.32. What compounds of nitrogen
through the listed ones are toxic
and therefore their concentrations
in water and food should be
controlled?
А. nitrites, ammonium ions
B. nitrites, amines
C. nitrites, nitrates
D. amines, nitrates
E. nitrates, ammonium ions
4.33. The main pollutions of the
atmospheric air are:
А. NO2, CO, SO2, NO
B. NO2, CO, N2O, CH4
C. NO2, CO, CH4, NH3
D. CO2, Cl2 ,NH3, CH4
E. CO, CH4, N2O, Cl2
4.34. In which of the given rows the
chemical elements are listed in the
consequence of their relative
electronegativity decreasing?
А. O, Cl, F, P, S
B.
C.
D.
E.
F, Cl, H, O, P
Cl, F, O, P, S
F, O, Cl, S, P
S, P, F, O, Cl
4.35. The properties of chemical
elements and their compounds
depends on:
А. the nuclei charge of their
atoms
B. the atoms radii
C. the values of the relative
electronegativies
D. the values of the ionization
energies
E. the values of the standard
reduction-oxidation potentials
потенціалу
4.36. What reactant is used for the
identification of sulfate-ion?
А. NH4SCN
B. Ba(NO3)2
C. NaH2PO4
D. KNO3
E. HCl
4.37. What reactant is used for the
identification of carbonate-ion?
А. KNO3
B. HCl
C. Na2S
D. NaH2PO4
E. NH4Cl
4.38. Point out the carbides through the
listed compounds.
А. CaC2 and Al4C3
B. СаСО3 and СаС2
C. СН4 and В4С
D. CS2 and CaC2
E. SiC and CH4
4.39. Which salts through the listed ones
can hydrolyze?
А. Ba(NO3)2
B.
C.
D.
E.
MgSO4
CaCl2
CaSO4
Ba(CH3COO)2
4.40. Which compound through the
listed ones is the most toxic?
А. CO
B. CO(NH2)2
C. CO2
D. Na2SiO3
E. SiO2
4.43. Which salt through the listed ones
can decompose under heating into
products, which can form the
initial compound under cooling?
А. NH4Cl
B. NH4NO3
C. NH4HCO3
D. NaHCO3
E. Na2CO3
4.41. What reactant should be used to
detect carbon dioxide in the air?
А. aqueous solution of Ca(OH)2
B. Fe(OH)2
C. crystalline NaOH
D. CaO
E. aqueous solution of NaOH
4.44. Point out for which of the listed
pairs of an acid and a base the
reaction of neutralization will not
take place?
А. H2SO4 and Ba(OH)2
B. H3PO4 and Ca(OH)2
C. H2SiO3 and Fe(OH)2
D. KOH and CH3COOH
E. H3PO4 and Mg(OH)2
4.42. What type of hybridization the
atoms of carbon in graphite have?
А. sp
B. sp3
C. dsp3
D. sp3d2
E. sp2
4.45. What is the electronic
configuration of S2- ion?
А. [Ne]2s23p3
B. [Ne]2s23p2
C. [Ne]2s23p5
D. [Ne]2s23p6
E. [Ne]2s23p4
Chapter 5. Chemical Properties and Biological Role of
Microelements
5.1. The biometals are able to take
part:
А. in the oxidation-reduction
processes only
B. in the processes of the acidbase equilibrium
C. in the oxidation-reduction
processes and in the processes
of coordination compounds
formation
D. in the processes of the
regulation of acid-base
properties of bio-systems
E. in the processes of
coordination compounds
formation only
5.2. The molecules of hemoglobin and
chlorophyll includes the atoms of
the following elements:
А. Fe, Ca
B. Mg i, Ca
C. Fe, Mg
D. Mg, Co
E. Fe, Co
5.3. The molecules of insulin and
vitamin В12 includes the atoms of
the following elements:
А. Fe, Co
B. Zn, Co
C. Cu, Co
D. Zn, Cu
E. Fe, Zn
5.4. The reactions of coordination
compounds formation are used for
the identification of the following
ions:
А. Са2+, Fe2+
B. Cu2+, Fe2+
C. Cu2+, Са2+
D. Ag+, Fe2+
E. Cu2+, Ag+
5.5. What ion through the listed one is
impossible to identify with the
reduction-oxidation reaction?
А. Zn2+
B. Cr6+
C. Mn2+
D. Cr3+
E. Al3+
5.6. The presence of reducing agents
in water can be determined using
the following reactant:
А. H2C2O4
B. K2Cr2O7
C. KMnO4
D. K2MnO4
E. H2O2
5.7. What elements of the IІВ group
have amphoteric properties?
А. zinc and cadmium
B. all elements of IIB group
C. cadmium and mercury
D. zinc only
E. mercury only
5.8. Point out the product of the
diluted HNO3 reduction with zinc.
А. NO2
B. N2
C. NO
D. NH4NO3
E. N2O
5.9. Which salt through the listed ones
should be dissolved in water to
increase the concentration of
hydrogen ions?
А. Zn2CO3
B. Zn(CH3COO)2
C. Zn3(PO4)2
D. ZnSO4
E. ZnS
5.10. Point out the product of the
reduction of diluted sulfuric acid
with zinc.
А. SO3
B. SO2
C. H2S
D. H2
E. S
5.11. Point out the product of the
reduction of concentrated sulfuric
acid with zinc.
А. SO3, S
B. SO3, H2S
C. SO2, S
D. S, H2S
E. SO2, H2S
5.12. What coordination numbers are
common for Cu2+ as a central ion?
А. 2, 6
B. 6, 8
C. 4, 6
D. 4, 8
E. 2, 4
5.13. Which compound of manganese
doesn’t exist in free state?
А. HMnO4
B. Mn2O3
C. MnO
D. H2MnO4
E. MnO2
5.14. What regularity corresponds to the
changing of acid-base properties
in the row of chromium
compounds CrO–Cr2O3–CrO3?
А. acidic properties increases
B. acid-base properties does not
change
C. basic properties increases
D. acid-base properties are not
typical
E. acidic properties decreases
5.15. The transformation Cr3+ →
Cr2O72– is:
А. the process of reduction in
acidic solution
B. the process of oxidation in
acidic solution
C. 
D. the process of oxidation in
basic solution
E. the process of reduction in
basic solution
5.16. What is the oxidation state of the
central ion in the coordination
compound Na2[Fe(CN)5NO]?
А. 0
B. +2
C. +1
D. +6
E. +3
5.17. What is the electronic
configuration of Fe3+ ion?
А. [Ar] 3d4 4s1
B. [Ar] 3d5 4s1 4p1
C. [Ar] 3d5 4s0
D. [Ar] 3d3 4s1 4p1
E. [Ar] 3d3 4s2
5.18. Which equation through the listed
ones corresponds to the reaction
of iron with hot concentrated
sulfuric acid?
А. 2Fe + 6H2SO4 = Fe2(SO4)3 +
3SO2 + 6H2O
B. iron turn inactive and the
reaction doesn’t pass
C. Fe + H2SO4 = FeSO4 + H2
D. Fe + 3H2SO4 = Fe2(SO4)3 +
3H2
E. Fe + 2H2SO4 = FeSO4 + SO2 +
2H2O
5.19. What is the electronic
configuration of Fe atom?
А. 3d74s2
B. 3d64s2
C. 4d65s2
D. 3d84s2
E. 3d54s1
5.20. What is the electronic
configuration of Co2+ ion?
А. 3d64s2
B. 3d74s0
C. 3d74s2
D. 3d54s2
E. 4d75s2
5.21. What is the electronic
configuration of Ni atom?
А. 3d74s2
B. 4d85s2
C. 3d84s0
D. 3d64s2
E. 3d84s2
D. Fe + NaOH
E. FeCl3 + NaOH
5.22. Complete and balance the
equation of the reaction: FeCl2 +
K3[Fe(CN)6] →. What is the sum
of the coefficients?
А. 9
B. 5
C. 10
D. 6
E. 12
5.27. What two compounds are the
reactants if the products of this
reaction are: ... + ... → Fe2(SO4)3
+ SO2 + H2O?
А. Fe and H2SO4 (dilut.)
B. FeO and H2SO4 (conc.)
C. Fe(OH)3 and H2SO4 (dilut.)
D. Fe2O3 and H2SO4 (conc.)
E. F2O3 and H2SO4 (dilut.)
5.23. What is the highest oxidation
number that Fe may have in its
compounds?
А. +6
B. +2
C. +3
D. +8
E. +4
5.28. Co can reduce the following metal
from its salt solution:
А. KNO3
B. NiSO4
C. AlCl3
D. CaCl2
E. Zn(NO3)2
5.24. The atom of what chemical
element has the electronic
configuration 3d74s2?
А. Co
B. Fe
C. Mn
D. Ni
E. Rh
5.25. In which of the given chemical
reactions iron (III) chloride will
form?
А. Fe(OH)3 + HCl →
B. Fe2O3 + Cl2 →
C. Fe(NO3)3 + HCl →
D. Fe + HCl →
E. Fe2(SO4)3 + HCl →
5.26. Iron(ІІІ) hydroxide will be the
product of the following chemical
reaction:
А. Fe2O3 + NaOH
B. FeCl3 + H2O
C. Fe2O3 + H2O
5.29. The molecules of which
biologically active compound
include cobalt?
А. citochrom
B. vitamin В6
C. hemoglobin
D. chlorophyll
E. vitamin В12
5.30. Red prussiate of potash
K3[Fe(CN)6] is the reactant for the
identification of:
А. Ca2+ ions
B. FeO42– ions
C. FeO2– ions
D. Fe2+ ions
E. Fe3+ ions
5.31. Yellow prussiate of potash
K4[Fe(CN)6] is the reactant for the
identification of:
А. Fe3+ ions
B. FeO2– ions
C. Ca2+ ions
D. FeO42– ions
E. Fe2+ ions
5.32. What is the medium in the
solution of the salt FeCl2?
А. slightly basic
B. neutral
C. acidic
D. basic
E. strongly acidic
5.33. What is the medium in the
solution of the salt CoCl2?
А. strongly acidic
B. acidic
C. basic
D. slightly basic
E. neutral
5.34. What is the medium in the
solution of the salt Ni(NO3)2?
А. strongly acidic
B. basic
C. acidic
D. slightly basic
E. neutral
5.35. The equation of the dissociation
constant of the complex ion for
the compound K4[Fe(CN)6] is:
3+
− 6
А.
Кd = [Fe ] ⋅ [CN ]
4−
[[Fe(CN) 6 ] ]
+ 4
4−
B.
[
Кd = K ] ⋅ [[Fe(CN) 6 ] ]
[[Fe(CN) 6 ] 4− ]
2+
−
C.
Кd = [Fe ] ⋅ 6[CN ]
[[Fe(CN) 6 ] 4− ]
2+
− 6
D.
Кd = [Fe ] + [CN ]
[[Fe(CN ) 6 ] 4− ]
2+
− 6
E.
Кd = [Fe ] ⋅ [CN ]
[[Fe(CN) 6 ] 4− ]
5.36. The equation of the dissociation
constant of the complex ion for
the compound [Со(NН3)6]Cl2 is:
2+
6
А.
Кd = [Co ] ⋅ [ NH 3 ]
2+
[[Co( NH 3 ) 6 ] ]
2+
− 2
B.
Кd = [[Co( NH 3 ) 6 ] ] ⋅ [Cl ]
[[Co( NH 3 ) 6 ]Cl 2 ]
2+
C.
Кd = [Co ] ⋅ 6[ NH 3 ]
[[Co( NH 3 ) 6 ] 2+ ]
D. К = [Co 2+ ] ⋅ [ NH 3 ] 6 ⋅ [Cl − ] 2
d
[[Co( NH 3 ) 6 ]Cl 2 ]
E.
2+
6
Кd = [Co ] + [ NH 3 ]
[[Co( NH 3 ) 6 ] 2+ ]
5.37. Iron (ІІІ) hydroxide has
amphoteric properties as it can:
А. react with acids only
B. decompose under heating
C. react with bases only
D. take part in self-oxidation selfreduction reactions
E. react with both acids and bases
5.38. What is the electronic
configuration of Cr6+ ion?
А. [Ar]3d54s0
B. [Ar]3d54s0
C. [Ar]3d04s1
D. [Ar]3d44s0
E. [Ar]3d04s0
5.39. What is the electronic
configuration of Cr3+ ion?
А. [Ar]3d44s0
B. [Ar]3d54s0
C. [Ar]3d44s1
D. [Ar]3d34s0
E. [Ar]3d54s1
5.40. What is the electronic
configuration of Cr2+ ion?
А. [Ar]3d44s0
B. [Ar]3d54s0
C. [Ar]3d34s0
D. [Ar]3d44s1
E. [Ar]3d24s0
5.41. What is the electronic
configuration of the chromium
atom?
А. [Ar]3d54s1
B. [Ar]3d44s2
C. [Ar]3d44s1
D. [Ar]3d64s1
E. [Ar]3d54s2
5.42. What is the electronic
configuration of the molybdenum
atom?
А. [Kr]4d45s1
B. [Kr]4d55s2
C. [Kr]4d45s2
D. [Kr]4d65s1
E. [Kr]4d55s1
5.43. What is the electronic
configuration of the tungsten
atom?
А. [Xe]5d66s1
B. [Xe]5d56s1
C. [Xe]5d46s2
D. [Xe]5d46s1
E. [Xe]5d56s2
5.46. What regularity corresponds to the
changing of acid-base properties
in the row of manganese
compounds MnO – MnO2 –
Mn2O7:
А. basic properties increases
B. acid-base properties are not
typical
C. acidic properties increases
D. acidic properties decreases
E. acid-base properties does not
change
5.47. The transformation Cr3+ → CrO42–
is:
А. –
B. the process of reduction in
acidic solution
C. the process of reduction in
basic solution
D. the process of oxidation in
basic solution
E. the process of oxidation in
acidic solution
5.44. The most common oxidation
states of chromium in its
compounds are:
А. +2; +3: +4
B. +2; +4: +6
C. +2; +3: +6
D. +1; +5: +6
E. +1; +2: +6
5.48. The transformation MnO4– →
MnO2 is:
А. the process of reduction in
neutral solution
B. the process of reduction in
acidic solution
C. the process of oxidation in
acidic solution
D. the process of oxidation in
basic solution
E. the process of reduction in
basic solution
5.45. What compound of chromium has
amphoteric properties?
А. CrO
B. K2CrO4
C. CrO3
D. Cr(OH)2
E. Cr2O3
5.49. What regularity corresponds to the
changing of ionization energy in
the row Cr–Mo–W?
А. the highest value for Mo
B. increases from W to Cr
C. increases
D. decreases
E. doesn’t change
5.50. What regularity corresponds to the
changing of reduction properties
in the row Cr–Mo–W?
А. increases from W to Cr
B. doesn’t change
C. decreases
D. Mo is the most strong
reduction agent
E. increases
Chapter 6. Acid-Base Equilibrium. Calculation and
Experimental Determination of the рН of
Solutions
6.1. Concentration of hydrogen-ion in
a pure water is:
А. 10–10
B. 10–14
C. 10–7
D. 10–1
E. 10–3
6.2. Which of the listed correlations is
true for the process of selfionization of water at 25 ºС?
А. [H+]+[ОН-]=10-7mol/L
B. [H+]/[ОН-]=10-7mol/L
C. [H+] =[ОН-]=10-14mol/L
D. [H+]+[ОН-]=10-14mol/L
E. [H+]=[ОН-]=10-7mol/L
6.3. What is the concentration of [H+]
in pure water at 25 ºС
А. 10-14
B. 107
C. 10-7
D. 1014
E. 10-1
6.4. What is the concentration of [OH] in pure water at 25 ºС
А. 10-7
B.
C.
D.
E.
107
10-1
10-14
1014
6.5. Which of the following is the
stronger acid?
А. HClO2
B. HClO
C. HClO4
D. chlorous acid
E. HClO3
6.6. Which electrolytes HCl, AgCl,
HNO3, NH4Cl, NH4OH,
CH3COOH, CH3COON are weak
ones:
А. HCl, AgCl
B. AgCl, NH4Cl
C. NH4Cl, NH4OH
D. CH3COOH, CH3COONa
E. NH4OH, CH3COOH
6.7. Which pair of ions cannot be
found in a neutral solution?
А. Ag+ and NO3–
B. K+ and OH–
C. Ca2+ and HCO–
D. Na+ and SO42–
E. H+ and CO32–
6.8. Choose the pair of electrolytes,
which do not react in an aqueous
solution?
А. K2CO3 and H2SO4
B. NaBr and KOH
C. Na2S and HCl
D. Fe(NO3)3 and NaOH
E. MgSO4 and (NH4)3PO4
6.9. Which reaction of the given ones
is impossible:
А. KI + Br2 → KBr + I2
B. KCl + Br2 → KBr + Cl2.
C. NaI + Cl2 → NaCl + I2
D. KCl + І2 → KІ + Cl2
E. NaBr+ Cl2 → NaCl + Br2
6.10. Which base is weak electrolite?
А. KOH
B. Ca(OH)2
C. Ba(OH)2
D. NaOH
E. Mg(OH)2
6.11. Which acid is weak electrolite?
А. HCl
B. H3BO3
C. HBr
D. H2SO4
E. HNO3
6.12. Mistaken statement, that concern
to iron (III) hydroxide: Fe(OH)3 –
it is …
А. strong electrolite
B. brown color of compound
C. insoluble in a water
D. weak base
E. amphoteric hydroxide
6.13. Which one of the given molecular
equation corresponds to the short
ionic equation Сu2+ + S2– = CuS?
А. CuCO3 + H2S = CuS + CO2 +
H2O
B. CuBr2 + K2S = CuS + 2KBr
C. Cu(OH)2 + Na2S = CuS +
2NaOH
D. Cu3(PO4)2 + 3(NH4)2S = 3CuS
+ 2(NH4)3PO4
E. CuCl2 + H2S = CuS + 2HCl
6.14. Point out the row in which pH of
compounds with the same molar
concentration decrease:
А. CH3COOH, HCl, NaOH, NH3,
H2SO4
B. NaOH, NH3, CH3COOH, HCl,
H2SO4
C. HCl, H2SO4, NH3, CH3COOH,
NaOH
D. H2SO4, HCl, NaOH,
CH3COOH, NH3
E. NH3, CH3COOH, NaOH, HCl,
H2SO4
6.15. How many ions are forming at the
dissociation of (NH4)2SO4?
А. 6
B. 5
C. 3
D. 4
E. 2
6.16. Which particle of the given ones
is an anion?
А. Ca2+
B. NO3C. K+
D. Fe3
E. Na+
6.17. Which compounds form ions of
Mn2+ at the dissociation?
А. Na2MnO4
B. MnCl2
C. MnO2
D. KMnO4
E. H2MnO4
6.18. How many ions are forming at the
dissociation of FeCl3?
А. 4
B. 5
C. 6
D. 10
E. 4
6.19. Which of the following
dissociation constant values of
polyprotic acid is always larger?
А. first
B. last
C. the same
D. third
E. second
6.20. Percent of dissociation NH4OH
increase with:
А. cooling
B. concentrating of solution
C. adding base
D. adding salt of ammonium
E. dilution of solution
6.21. Point out an aqueous solution
which has the worst electrical
conductivity? Molarity of the
solutions is equal.
А. H2SO4
B. KCN
C. HCN
D. KOH
E. K2SO4
6.22. Percent of dissociation of weak
electrolytes increase with:
А. cooling
B. heating
C. increasing of concentration
D. decreasing of acidity
E. increasing of acidity
6.23. 0,1 М solution of which
compound has the smallest
concentration of ions?
А. НCl
B. СН3СООН
C. NaNO3
D. СаCl2
E. H2SO4
6.24. In the basic medium рН and рОН
are equal:
А. рН > 7, рОН >7
B. рН = 7, рОН = 7
C. рН > 7, рОН < 7
D. рН < 7, рОН >7
E. рН < 7, рОН < 7
6.25. pH of 0,001 М solution of HCl
equal:
А. 0
B. 7
C. 10
D. 5
E. 3
6.26. What is the concentration of
hydroxide-ion in a solution, if
рОН of its equal 9?
А. 10–7
B. 10–9
C. 10–5
D. 10–11
E. 10–3
6.27. pH equal zero in a solution of:
А. 0.1M KOH
B. 1M HCl
C. 1M H2SO4
D. 1M Ba(OH)2
E. 0.1M HCl
6.28. Units of measurement of
hydrogen-ion concentration in
equation pH = -lg[H+] are:
А. mol/L
B. mol/кg
C. mol
D. mol/mL
E. mol/cm3
6.29. In the acidic solution the values of
[H+] and рН are:
А. [H+] = 10-7; рН = 7
B. [H+]>10-7; рН.> 7
C. [H+] >10-7; рН < 7
D. [H+]< 10-7; рН< 7
E. [H+]>10-7; рН= 7
6.30. Which of the following pH values
indicate an acidic solution at 25
ºС?
А. 7,4
B. 9,5
C. 11,2
D. 1,2
E. 10
6.31. Which of the following pH values
indicate a basic solution at 25 ºС?
А. 5,5
B. 4
C. 1,2
D. 4,5
E. 7,3
6.32. In the acidic medium рН and рОН
are equal:
А. рН < 7, рОН<7
B. рН < 7, рОН >7
C. рН > 7, рОН >7
D. рН =7, рОН = 7
E. рН > 7, рОН<7
6.33. In the neutral medium рН and
рОН are equal:
А. рН > 7, рОН >7
B. рН > 7, рОН<7
C. рН =7, рОН = 7
D. рН < 7, рОН<7
E. рН < 7, рОН >7
6.34. Which of the following pH values
indicate a neutral solution at
25ºС?
А. 7
B. 5
C. 9,5
D. 13
E. 2,5
6.35. What is the pH of a sample of
gastric juice (digestive juice in the
stomach):
А. 0,9– 2,0
B. 2,5 – 3,5
C. 1,5 – 2,5
D. 1,5 – 3,0
E. 0,5 – 1,5
6.36. pH of the blood plasma is:
А. 7,65 – 7,85
B. 7,35 – 7,45
C. 7,15 – 7,35
D. 6,80 – 7,0
E. 8,01 – 8,25
6.37. What is the рН values range of the
urine?
А. 2,0 – 3,5
B. 5,0 – 6,5
C. 2,5 – 3,5
D. 8,5 – 10,5
E. 7,5 – 9,5
Chapter 7. Protolytical Processes in Living Organisms.
Hydrolysis of Salts
7.1. According to the Bronsted-lowry
concept of acids and bases
amphoteric properties have the
next electrolites:
А. H2O, HI, H3O+
B. HClO, H2S, CH3NO2
C. NH3, H3O+, HPO4D. HS-, NO2-, HSO4E. H2O, HCO3-, HPO427.2. According to the Bronsted-Lowry
concept of acids and bases, an
acid is the species which:
А. donates a proton
B. accepts the proton
C. has a free electron pair
D. molecule contains a
hydrogen-ion
E. donates the electron
7.3. According to the Bronsted-Lowry
concept of acids and bases, an
base is the species which:
А. B. accepts the proton
C. donates the electron
D. accepts the electron
E. donates the proton
7.4. Which of the given compounds do
not belong to Lewis acid?
А. no one through the listed
compounds
B. AlCl3
C. С5H5N
D. ZnCl2
E. FeCl3
7.5. In acid-base reaction molecules of
solvent:
А. transfer proton from base to
acid
B. transfer proton from acid to
base
C. D. transfer electron from
reducing agent to oxidizing
agent
E. transfer electron from
oxidizing agent to reducing
agent
7.6. Which of the given species is a
Lewis base?
А. CH4
B. F–
C. Ca2+
D. CO2
E. H+
7.7. Which of the given species is a
Lewis acid?
А. Cl–
B. NH3
C. SO42–
D. CN–
E. BF3
7.8. Which one of the aqueous
solution of the given salts has an
acidic pH?
А. NaCl
B. Na2B4O7
C. ZnSO4
D. K2SO3
E. Na3PO4
7.9. Which one of the given salts
cannot exist in an aqueous
solution?
А. NH4Cl
B.
C.
D.
E.
Cr2S3
NaNO3
FeCl3
K3PO4
7.10. Color of litmus in a solution of
iron (ІІІ) nitrate is:
А. red
B. colorless
C. blue
D. violet
E. pink
7.11. Select the salt, which do not
hydrolyze:
А. CrCl3
B. KI
C. Al2(SO4)3
D. KNO2
E. FeSO4
7.12. Point out the salt which hydrolyze
particularly:
А. K2S
B. NaBr
C. BaSO4
D. Al2S3
E. Ca(NO3)2
7.13. Point out the salt which hydrolyze
to the end:
А. Na3PO4
B. KNO3
C. Cr2S3
D. Al2(SO4)3
E. Cr(NO3)3
7.14. Which one of the given salts has a
basic solution?
А. NaNO3
B. KCl
C. Cr2(SO4)3
D. AlCl3
E. Na2CO3
7.15. Which one of the given salts has
an acidic solution?
А. BaCl2
B. Fe(NO3)3
C. K3PO4
D. NaI
E. K2CO3
7.16. Color of methyl orange in a
solution of zinc sulfate is:
А. blue
B. colorless
C. orange
D. yellow
E. pink
7.17. Color of methyl orange in a
solution of K2CO3 is:
А. red
B. yellow
C. blue
D. orange
E. pink
7.18. Color of methyl orange in a
solution of AlCl3 is:
А. blue
B. pink
C. purple
D. yellow
E. colorless
7.19. Color of phenolphthalein in a
solution of Na3PO4 is:
А. colorless
B. red
C. pink
D. blue
E. orange
7.20. Color of methyl red in a solution
of Cr2(SO4)3 is:
А. yellow
B. blue
C. colorless
D. orange
E. red
7.21. Select the salt, which do not
hydrolyze:
А. K2HPO4
B. Ba(NO3)2
C. KNO2
D. ZnCl2
E. AlCl3
7.22. Point out the salt which can form
as a product of hydrolysis a basic
salt.
А. BaI2
B. KNO2
C. Na2CO3
D. AgNO3
E. AlCl3
7.23. Complete and balance the
equation of the hydrolysis of
CaC2. What is the pH of the
solution of CaC2 and what is the
sum of the coefficients in the
equation of hydrolysis?
А. рН<7; 5
B. рН>7; 6
C. рН>7; 5
D. рН>7; 4
E. рН<7; 4
7.24. Which one of the given salts
forms as a product of hydrolysis a
basic salt?
А. K2CO3
B. Cr2(SO4)3
C. CaCO3
D. AgNO3
E. Na2SO4
7.25. Which one of the given salts
forms a neutral solution?
А. NH4NO3
B. NH4Cl
C. CH3COONH4
D. NH4Br
E. (NH4)2SO4
7.26. Select the salt which increases the
hydrogen-ion concentration, when
dissolved in water?
А. NaCl
B. K2SO4
C. K3PO4
D. Na2CO3
E. ZnCl2
7.27. Select the salt, which do not
hydrolyze:
А. AlBr3
B. K2SO3
C. K2SO4
D. MnCl2
E. CuSO4
7.28. Point out the salt which hydrolyze
in one step completely:
А. CuS
B. no one through the listed salts
C. AlCl3
D. Na2S
E. Cr2S3
7.29. Which one from the given salts
has a basic solution?
А. KCl
B. CuCl2
C. Na2SO4
D. FeCl3
E. Na2S
7.30. What is the product of reaction
between H2O and PCl5?
А. P2O5 + HCl
B. HCl + H3PO3
C. HCl + H3PO4
D. P2O3 + HCl
E. Cl2 + H3PO4
7.31. Select the salt, which hydrolyze in
an aqueous solution:
А. LiBr
B. KI
C. NaCl
D. KI
E. NaF
7.32. Which one of the given salts
reacts with an acid and forms as a
product of reaction a gas?
А. Na2CO3
B. CuSO4
C. Ca3(PO4)2
D. Na2SiO3
E. K2SO4
7.33. Some medicine can destroy in
acidic medium. Which one of the
given salt is incompatible with the
medicine in an aqueous solution?
А. NaCl
B. ZnSO4
C. K3PO4
D. NaHCO3
E. KI
7.34. Some antibiotics can destroy in
acidic medium. Which one of the
given salt is incompatible with the
antibiotics in an aqueous solution?
А. KI
B. Na3PO4
C. CaCl2
D. NH4Cl
E. Na2CO3
7.35. Select the salt, which hydrolyze in
an aqueous solution:
А. Sr(NO3)2
B. NH4NO3
C. NaNO3
D. KNO3
E. Ba(NO3)2
7.36. Point out the salt which hydrolyze
to the end:
А. CuSO4
B. Na2CO3
C. Zn(NO3)2
D. K2S
E. Аl2S3
7.37. Which ions can be at the same
time in a solution?
А. Fe2+, OH–
B. Ag+, Cl–
C. Ba2+, SO42–
D. Fe3+, OH–
E. Fe3+, Cl–
7.38. The expression of the constant of
hydrolysis Кh = Кw/Kb is for a salt
of:
А. CuSO4
B. CH3COONa
C. (NH4)2S
D. KCN
E. NaCl
7.39. The expression of the constant of
hydrolysis Кh = Кw/(Ка ·Kb) is for
a salt of:
А. Fe(NO3)3
B. (NH4)2S
C. Li2S
D. NaCN
E. NH4Cl
7.40. The expression of the constant of
hydrolysis Кh = Kw/(Ka· Kb) is for
a salt of:
А. FeCl3
B. NH4Cl
C. CH3COONH4
D. CH3COONa
E. К3PO4
7.41. The expression of the constant of
hydrolysis Кh = Кw/Kb is for a salt
of:
А. LiNO3
B. K3PO4
C. Na2CO3
D. K2SO4
E. NH4Cl
7.42. The expression of the constant of
hydrolysis Кh = Кw/Ka is for a salt
of:
А. (NH4)3PO4
B. CH3COONH4
C. Na2SO4
D. NaCN
E. (NH4)2SO4
7.43. Percent of hydrolysis of CuSO4
decrease with adding solution of:
А. BaSO4
B. KOH
C. H2O
D. Na2CO3
E. H2SO4
7.44. The direction of protolytical
reaction СН3СООН + С6Н5ОNa
⇄ C6H5OH + CH3COONa is
shifted:
А. dynamic equilibrium
B. reverse
C. D. reaction is impossible
E. forward
Chapter 8. Buffer Solutions, Their Classification and the
Mechanism of the Buffer Action. Preparation of
Buffer Solutions. Determination of the Buffer
Capacity and the pH Values of Buffer Solutions.
The Biological Role of Buffer Systems
8.1. The acidic buffer system is the
mixture of the following
compounds solutions:
А. ammonium chloride and
ammonium hydroxide
B. acetic acid and potassium
acetate
C. carbonic acid and potassium
chloride
D. hydrochloric acid and sodium
chloride
E. phosphoric acid and sodium
sulfate
8.2. The acidic buffer system is the
mixture of the following
compounds solutions:
А. phosphoric acid and sodium
sulfate
B. formic acid and sodium sulfate
C. sodium acetate and sodium
chloride
D. hydrochloric acid and sodium
chloride
E. formic acid and potassium
formiate
8.3. The acidic buffer system is the
mixture of the following
compounds solutions:
А. carbonic acid and sodium
hydrogen carbonate
B. hydrochloric acid and sodium
chloride
C. carbonic acid and potassium
chloride
D. ammonium chloride and
ammonium hydroxide
E. sodium carbonate and sodium
phosphate
8.4. The acidic buffer system is the
mixture of the following
compounds solutions:
А. ammonium chloride and
ammonium hydroxide
B. phosphoric acid and sodium
sulfate
C. sodium acetate and sodium
chloride
D. sodium dihydrogen phosphate
and sodium hydrogen
phosphate
E. sulfuric acid and potassium
hydrosulfate
8.5. The acidic buffer system is the
mixture of the following
compounds solutions:
А. anions of dihydrogen
phosphate and hydrogen
phosphate
B. hydrochloric acid and sodium
chloride
C. sodium acetate and sodium
chloride
D. ammonium chloride and
ammonium hydroxide
E. phosphoric acid and sodium
sulfate
8.6. The acidic buffer system is the
mixture of the following
compounds solutions:
А. acetic acid and sodium sulfate
B. sodium acetate and sodium
chloride
C. acetic acid and acetate anion
D. ammonium chloride and
ammonium hydroxide
E. sulfuric acid and potassium
hydrosulfate
8.7. The basic buffer system is the
mixture of the following
compounds solutions:
А. ammonium chloride and
ammonium sulfate
B. potassium hydroxide and
sodium hydroxide
C. ammonium chloride and
ammonium hydroxide
D. potassium hydroxide and
potassium chloride
E. potassium hydroxide and
ammonium hydroxide
8.8. The basic buffer system is the
mixture of the following
compounds solutions:
А. ammonium chloride and
ammonium sulfate
B. ammonium sulfate and
ammonium hydroxide
C. potassium hydroxide and
sodium hydroxide
D. sodium hydroxide and sodium
sulfate
E. potassium sulfate and
ammonium hydroxide
8.9. The ampholytic buffer system is
the mixture of the following
compounds solutions:
А. ammonium chloride and
ammonium hydroxide
B. glucose
C. sodium dihydrophosphate and
sodium hydrogenphosphate
D. proteins
E. acetic acid and acetate anion
8.10. The ampholytic buffer system is
the mixture of the following
compounds solutions:
А. forming acid and potassium
formiate
B. ammonium hydroxide and
ammonium cation
C. glucose
D. acetic acid and acetate anion
E. aminoacids
8.11. The basic buffer system is the
mixture of the following
compounds solutions:
А. potassium sulfate and
ammonium hydroxide
B. potassium hydroxide and
potassium sulfate
C. ammonium chloride and
ammonium sulfate
D. potassium hydroxide and
sodium hydroxide
E. ammonium hydroxide and
ammonium cation
8.12. The basic buffer system is the
mixture of the following
compounds solutions:
А. ammonium nitrate and
ammonium hydroxide
B. potassium sulfate and
ammonium hydroxide
C. nitrate anions and acetate
anions
D. potassium hydroxide and
ammonium hydroxide
E. ammonium nitrate and
ammonium sulfate
8.13. The concentration of hydrogen
ions in the acetic buffer solution
may be calculated according to
the equation:
А.
n(acid )
[H + ] = K d n(salt )
B.
n
(acid)
[H + ] = K d
n(salt )
C. +
n( base )
[H ] = K d
n(salt )
D.
n(salt )
n( acid )
E.
n(salt )
[H + ] = K d
n( acid )
[H + ] = K W
8.14. The concentration of hydrogen
ions in the phosphate buffer
solution may be calculated
according to the equation:
А. +
n( base )
[H ] = K d
B.
n(salt )
n(salt )
n( acid )
C.
n(acid )
[H + ] = K d n(salt )
D.
n(acid )
[H + ] = K d
n(salt )
E.
n(salt )
[H + ] = K d
n( acid )
[H + ] = K W
8.15. The concentration of hydrogen
ions in the hydrogen carbonate
buffer solution may be calculated
according to the equation:
А.
n(acid )
[H + ] = K d
n(salt )
B.
n(acid )
[H + ] = K d n(salt )
C. +
n( base )
[H ] = K d
D.
n(salt )
n(salt )
n( acid )
E.
n(salt )
+
[H ] = K d
n( acid )
[H + ] = K W
8.16. The concentration of hydroxyl
ions ОН– in the ammonium buffer
solution may be calculated
according to the equation:
А.
[OH − ] = K d
B.
[ОH − ] = K W
n(acid)
n(salt )
n( base )
n(salt )
C.
n( base )
[OH − ] = K d n(salt )
D.
n
(
base
)
−
[OH ] = K d
n(salt )
E.
n(salt )
[OH − ] = K d
n( base )
8.17. The рН value in the acetic buffer
solution may be calculated
according to the equation:
А. pH= pK + lgCacid/Csalt
B. pH= 14 + pKbase. + lgCbase/Csalt
C. pH= 14 + pKbase. – lgCbase./Csalt
D. pH= pK – lgCsalt/Cacid
E. pH= рК– lg(Сacid/Сsalt)
8.18. The рН value in the ammonium
buffer solution may be calculated
according to the equation:
А. pH=рК – lg(Сacid/Сsalt)
B. pH= 14 – pK. + lgCbase/Csalt
C. pH= pK + lgCacid/Csalt
D. pH= 14 + pKbase. + lgCbase./Csalt
E. pH= pK - lgCacid/Csalt
8.19. The рН value in the hydrogen
carbonate buffer solution may be
calculated according to the
equation:
А. pH= pK + lgCacid/Csalt
B. pH= рК – lg(Сacid/Сsalt)
C. pH= pK – lgCsalt/Cacid
D. pH= 14 – pKbase + lgCbase/Csalt
E. pH= 14 + pKbase. + lgCbase./Csalt
8.20. The рН value in the phosphate
buffer solution may be calculated
according to the equation:
А. pH= 14 + pKbase. + lgCbase./Csalt
B. pH= pK – lgCsalt/Cacid
C. pH= pK + lgCacid/Csalt
D. pH= рК – lg(Сacid/Сsalt)
E. pH= 14 – pKbase + lgCbase/Csalt
8.21. The buffer systems may be
characterized with:
А. the uninfluenced pH value on
temperature
B. the considerable change of the
pH value while diluting
C. the change of the pH value
while water is added
D. –
E. the resistance in changing pH
while adding the small
amounts of acids and alkalis
8.22. The pH value of an acidic buffer
solution depends on:
А. the number of moles ratio of
the acid and the salt in the
solution
B. the concentration of the acid
C. the concentration of the salt in
the solution
D. the product of the molarity
concentrations of the acid and
the salt
E. the ionization constant of the
acid and the number of moles
ratio of the acid and the salt in
the solution
8.23. The pH value of a basic buffer
solution depends on:
А. the concentration of the salt in
the solution
B. the ionization constant of the
base and the number of moles
ratio of the base and the salt in
the solution
C. the number of moles ratio of
the base and the salt in the
solution
D. the product of the molarity
concentrations of the base and
the salt
E. the concentration of the base
8.24. One of the buffer systems of the
blood is the mixture of the
following components:
А. СО32– and НСО3–
B. H2PO4– and HPO42–
C. НРО32– and РО33–
D. NH4OH and NH4+
E. СН3СООН and СН3СОО–
8.25. One of the buffer systems of the
blood is the mixture of the
following components:
А. СО32– and НСО3–
B. НРО32– and РО33–
C. Na2B4O7 and H3BO3
D. NH4OH and NH4+
E. HCO3– and Н2СО3
8.26. One of the buffer systems of the
blood is the mixture of the
following components:
А. СО32– and НСО3–
B. СН3СООН and СН3СОО–
C. НРО32– and РО33–
D. NH4OH and NH4+
E. НHb and Hb–
8.27. One of the buffer systems of the
blood is the mixture of the
following components:
А. NH4OH and NH4+
B. НРО32– and РО33–
C. НHbО2 and HbО2–
D. СН3СООН and СН3СОО–
E. СО32– and НСО3–
8.28. Which buffer solution through the
listed ones is not included into the
buffer systems of the blood:
А. phosphate buffer
B. hemoglobin buffer
C. hydrogencarbonate buffer
D. acetate buffer
E. protein buffer
8.29. Which buffer solution through the
listed ones is not included into the
buffer systems of the blood:
А. ammonium buffer
B. phosphate buffer
C. oxyhemoglobin buffer
D. protein buffer
E. hydrogencarbonate buffer
8.30. Which buffer solution through the
listed ones is the ampholytic
buffer system of the blood:
А. phosphate buffer
B. protein buffer
C. oxyhemoglobin buffer
D. hemoglobin buffer
E. hydrogen carbonate buffer
8.31. What is the pH of the buffer
solution which is prepared by
mixing of 200 ml 0.2 М
СН3СООН solution and 200 ml
0.2 М CН3СООNa solution? (Ka
= 1.75 ·10-5 )
А. 5.31
B. 4.76
C. 4.21
D. 4.54
E. 3.97
8.32. What is the pH of the buffer
solution which is prepared by
mixing of 200 ml 0.1 М
СН3СООН solution and 100 ml
0.2 М СН3СООNa solution? (Ka
= 1.75 ·10-5 )
А. 3.97
B. 4.21
C. 5.31
D. 4.76
E. 4.54
B. 7.20
C. 8.10
D. 7.90
E. 7.53
8.33. What is the pH of the buffer
solution which is prepared by
mixing of 500 ml 0.2 М
СН3СООН solution and 200 ml
0.5 М СН3СООNa solution? (Ka
8.37. What is the pH of the buffer
solution which is prepared by
mixing of 100 ml 0.1 М NH4OH
solution and 100 ml 0.1 М NH4Cl
= 1.75 ·10-5 )
А. 4.76
B. 4.54
C. 3.97
D. 4.21
E. 5.31
8.34. What is the pH of the buffer
solution which is prepared by
mixing of 100 ml 0.3 М NаH2РО4
solution and 100 ml 0.3 М
Nа2НРО4 solution? (Ka = 6.3 ·10
)
А. 6.81
B. 7.90
C. 7.53
D. 7.20
E. 8.10
-8
8.35. What is the pH of the buffer
solution which is prepared by
mixing of 200 ml 0.3 М NаH2РО4
solution and 300 ml 0.2 М
Nа2НРО4 solution? (Ka = 6.3 ·10-8
)
А. 8.10
B. 7.53
C. 7.20
D. 7.90
E. 6.81
8.36. What is the pH of the buffer
solution which is prepared by
mixing of 100 ml 0.4 М NаH2РО4
solution and 200 ml 0.2 М
Nа2НРО4 solution? (Ka = 6.3 ·10-8
)
А. 6.81
solution? (Kb=1.8 ·10-5)
А. 10.27
B. 9.83
C. 9.54
D. 8.61
E. 9.25
8.38. What is the pH of the buffer
solution which is prepared by
mixing of 300 ml 0.1 М NH4OH
solution and 100 ml 0.3 М NH4Cl
solution? (Kb=1.8 ·10-5)
А. 8.61
B. 9.83
C. 9.25
D. 10.27
E. 9.54
8.39. What is the pH of the buffer
solution which is prepared by
mixing of 100 ml 0.2 М NH4OH
solution and 200 ml 0.1 М NH4Cl
solution? (Kb=1.8 ·10-5)
А. 9.25
B. 10.27
C. 8.61
D. 9.54
E. 9.83
8.40. What is the pH of the buffer
solution which is prepared by
mixing of the equal volumes of
0.2 М NH4OH solution and 0.2 М
NH4Cl solution? (Kb=1.8 ·10-5)
А. 9.54
B. 9.25
C. 10.27
D. 9.83
E. 8.61
8.41. What is the pH of the buffer
solution which is prepared by
mixing of 500 ml 0.1 М NH4OH
solution and 100 ml 0.5 М NH4Cl
solution? (Kb=1.8 ·10-5)
А. 8.61
B. 9.25
C. 9.54
D. 9.83
E. 10.27
8.42. What is the pH of the buffer
solution which is prepared by
mixing of 200 ml 0.3 М NH4OH
solution and 300 ml 0.2 М NH4Cl
solution? (Kb=1.8 ·10-5)
А. 8.61
B. 9.83
C. 10.27
D. 9.25
E. 9.54
8.43. What is the buffer capacity of the
solution on acid?
А. the mass of an acid which
should be added to change pH
of a buffer solution
B. the number of moles of an acid
which is contained in 1 L of a
buffer solution
C. the number of moles of an acid
which should be added to 1 L
of a buffer solution to change
its pH into 1 point
D. the volume of an acid which
should be added to change pH
of 1 L of a buffer solution
E. the number of moles of a
compound which should be
added to change pH of 1 L of a
buffer solution
8.44. What is the buffer capacity of the
solution on base?
А. the number of moles of a
compound which should be
added to change pH of 1 L of a
buffer solution
B. the number of moles of a base
which is contained in 1 L of a
buffer solution
C. the number of moles of a base
which should be added to 1 L
of a buffer solution to change
its pH into 1 point
D. the mass of a base which
should be added to change pH
of a buffer solution
E. the volume of a base which
should be added to change pH
of 1 L of a buffer solution
8.45. The buffer capacity value of the
acidic buffer system depends on:
А. the mole ratio of the buffer
solution components
B. the nature of the components
of the buffer solution
C. the concentration of the acid in
the buffer solution
D. the ionization constant value
of the acid
E. the pH value and the
concentrations of components
of the buffer solution
8.46. The buffer capacity value of the
basic buffer system depends on:
А. the nature of the components
of the buffer solution
B. the mole ratio of the buffer
solution components
C. the ionization constant value
of the base
D. the concentration of the base in
the buffer solution
E. the pH value and the
concentrations of components
of the buffer solution
8.47. The phosphate buffer solution has
the maximum value of the buffer
capacity when pH of the solution
is:
А. 6.8
B. 7.8
C. 7.6
D. 7.0
E. 7.2
8.48. The acetate buffer solution has the
maximum value of the buffer
capacity when pH of the solution
is:
А. 4.0
B. 5.0
C. 4.8
D. 4.2
E. 5.3
8.49. The ammonium buffer solution
has the maximum value of the
buffer capacity when pH of the
solution is:
А. 8.5
B. 9.3
C. 9.6
D. 9.8
E. 9.0
8.50. The phosphate buffer solution has
the maximum value of the buffer
capacity when the concentration
of hydrogen ions H+ in the
solution (in mol×L-1) is equal to:
А. 2.1·10–8
B. 1.7·10–10
C. 7.3·10–7
D. 6.3·10–8
E. 4.3·10–9
8.51. The acetate buffer solution has the
maximum value of the buffer
capacity when the concentration
of hydrogen ions H+ in the
solution (in mol×L-1) is equal to:
А. 2.3·10–4
B. 4.1·10–6
C. 5.8·10–6
D. 1.8·10–5
E. 9.1·10–5
8.52. The ammonium buffer solution
has the maximum value of the
buffer capacity when the
concentration of hydroxyl ions
OH− in the solution (in mol×L-1) is
equal to:
А. 4.1·10–6
B. 5.8·10–6
C. 2.3·10–4
D. 9.1·10–5
E. 1.8·10–5
8.53. A buffer solution will have the
maximum value of the buffer
capacity when the concentrations
of its components (in mol×L-1)
would be equal to:
А. С(NaH2PO4)= 0.1 and
С(Na2HPO4)= 0.2
B. С(NaH2PO4)= 0.1 and
С(Na2HPO4)= 0.2
C. С(NaH2PO4)= 0.3 and
С(Na2HPO4)= 0.03
D. С(NaH2PO4)= 0.2 and
С(Na2HPO4)= 0.2
E. С(NaH2PO4)= 0.2 and
С(Na2HPO4)= 0.1
8.54. A buffer solution will have the
maximum value of the buffer
capacity when the concentrations
of its components (in mol×L-1)
would be equal to:
А. С(СН3СООNa)= 0.5 and
С(СН3СООН)= 0.05
B. С(СН3СООNa)= 0.2 and
С(СН3СООН)= 0.3
C. С(СН3СООNa)= 0.2 and
С(СН3СООН)= 0.1
D. С(СН3СООNa)= 0.1 and
С(СН3СООН)= 0.1
E. С(СН3СООNa)= 0.1 and
С(СН3СООН)= 0.2
8.55. A buffer solution will have the
maximum value of the buffer
capacity when the concentrations
of its components (in mol×L-1)
would be equal to:
А. С(NH4OH)= 0.4 and
С(NH4Cl)= 0.3
B. С(NH4OH)= 0.3 and
С(NH4Cl)= 0.2
C. С(NH4OH)= 0.01 and
С(NH4Cl)= 0.4
D. С(NH4OH)= 0.3 and
С(NH4Cl)= 0.3
E. С(NH4OH)= 0.2 and
С(NH4Cl)= 0.02
8.56. A buffer solution will have the
maximum value of the buffer
capacity when the concentrations
of its components (in mol×L-1)
would be equal to:
А. С(H2CO3)= 0.6 and
С(NaHCO3)= 0.4
B. С(H2CO3)= 0.1 and
С(NaHCO3)= 0.4
C. С(H2CO3)= 0.4 and
С(NaHCO3)= 0.6
D. С(H2CO3)= 0.7 and
С(NaHCO3)= 0.4
E. С(H2CO3)= 0.5 and
С(NaHCO3)= 0.5
8.57. A buffer solution will have the
maximum value of the buffer
capacity when the concentrations
of its components (in mol×L-1)
would be equal to:
А. С(NaH2PO4)= 0.3 and
С(Na2HPO4)= 0.03
B. С(NaH2PO4)= 0.5 and
С(Na2HPO4)= 0.1
C. С(NaH2PO4)= 0.4 and
С(Na2HPO4)= 0.4
D. С(NaH2PO4)= 0.3 and
С(Na2HPO4)= 0.4
E. С(NaH2PO4)= 0.4 and
С(Na2HPO4)= 0.3
8.58. A buffer solution will have the
maximum value of the buffer
capacity when the concentrations
of its components (in mol×L-1)
would be equal to:
А. С(СН3СООNa)= 0.2 and
С(СН3СООН)= 0.1
B. С(СН3СООNa)= 0.1 and
С(СН3СООН)= 0.2
C. С(СН3СООNa)= 0.5 and
С(СН3СООН)= 0.05
D. С(СН3СООNa)= 0.2 and
С(СН3СООН)= 0.3
E. С(СН3СООNa)= 0.2 and
С(СН3СООН)= 0.2
8.59. A buffer solution will have the
maximum value of the buffer
capacity when the concentrations
of its components (in mol×L-1)
would be equal to:
А. С(NaH2PO4)= 0.1 and
С(Na2HPO4)= 0.1
B. С(NaH2PO4)= 0.2 and
С(Na2HPO4)= 0.2
C. С(NaH2PO4)= 0.2 and
С(Na2HPO4)= 0.1
D. С(NaH2PO4)= 0.05 and
С(Na2HPO4)= 0.05
E. С(NaH2PO4)= 0.3 and
С(Na2HPO4)= 0.03
8.60. A buffer solution will have the
maximum value of the buffer
capacity when the concentrations
of its components (in mol×L-1)
would be equal to:
А. С(СН3СООNa)= 0.1 and
С(СН3СООН)= 0.3
B. С(СН3СООNa)= 0.5 and
С(СН3СООН)= 0.05
C. С(СН3СООNa)= 0.2 and
С(СН3СООН)= 0.2
D. С(СН3СООNa)= 0.3 and
С(СН3СООН)= 0.1
E. С(СН3СООNa)= 0.3 and
С(СН3СООН)= 0.3
8.61. A buffer solution will have the
maximum value of the buffer
capacity when the concentrations
of its components (in mol×L-1)
would be equal to:
А. С(NH4OH)= 0.4 and
С(NH4Cl)= 0.4
B. С(NH4OH)= 0.4 and
С(NH4Cl)= 0.3
C. С(NH4OH)= 0.2 and
С(NH4Cl)= 0.2
D. С(NH4OH)= 0.2 and
С(NH4Cl)= 0.02
E. С(NH4OH)= 0.01 and
С(NH4Cl)= 0.4
8.62. A buffer solution will have the
maximum value of the buffer
capacity when the concentrations
of its components (in mol×L-1)
would be equal to:
А. С(H2CO3)= 0.4 and
С(NaHCO3)= 0.6
B. С(H2CO3)= 0.3 and
С(NaHCO3)= 0.3
C. С(H2CO3)= 0.1 and
С(NaHCO3)= 0.4
D. С(H2CO3)= 0.7 and
С(NaHCO3)= 0.4
E. С(H2CO3)= 0.5 and
С(NaHCO3)= 0.5
8.63. A buffer solution will have the
maximum value of the buffer
capacity when the concentrations
of its components (in mol×L-1)
would be equal to:
А. С(NaH2PO4)= 0.4 and
С(Na2HPO4)= 0.4
B. С(NaH2PO4)= 0.3 and
С(Na2HPO4)= 0.4
C. С(NaH2PO4)= 0.3 and
С(Na2HPO4)= 0.3
D. С(NaH2PO4)= 0.5 and
С(Na2HPO4)= 0.1
E. С(NaH2PO4)= 0.1 and
С(Na2HPO4)= 0.1
8.64. A buffer solution will have the
maximum value of the buffer
capacity when the concentrations
of its components (in mol×L-1)
would be equal to:
А. С(СН3СООNa)= 0.1 and
С(СН3СООН)= 0.2
B. С(СН3СООNa)= 0.2 and
С(СН3СООН)= 0.2
C. С(СН3СООNa)= 0.1 and
С(СН3СООН)= 0.1
D. С(СН3СООNa)= 0.5 and
С(СН3СООН)= 0.05
E. С(СН3СООNa)= 0.2 and
С(СН3СООН)= 0.1
8.65. The adding of 20 ml of 0.1 M
solution of hydrochloric acid HCl
to 200 ml of a buffer solution
caused the change of its pH from
5.4 to 5.1. What is the buffer
capacity of the solution (in
mmol×mL-1) on acid?
А. 48
B. 33
C. 45
D. 38
E. 29
8.66. The adding of 15 ml of 0.3 M
solution of hydrochloric acid HCl
to 300 ml of a buffer solution
caused the change of its pH from
7.8 to 6.5. What is the buffer
capacity of the solution (in
mmol×ml-1) on acid?
А. 15.2
B. 8.7
C. 11.5
D. 19.4
E. 7.6
8.67. The adding of 50 ml of 0.2 M
solution of hydrochloric acid HCl
to 150 ml of a buffer solution
caused the change of its pH from
8.6 to 7.9. What is the buffer
capacity of the solution (in
mmol×mL-1) on acid?
А. 95
B. 76
C. 105
D. 40
E. 81
8.68. The adding of 10 ml of 0.1 M
solution of hydrochloric acid HCl
to 200 ml of a buffer solution
caused the change of its pH from
6.8 to 6.2. What is the buffer
capacity of the solution (in
mmol×mL-1) on acid?
А. 10
B. 8
C. 4
D. 11
E. 6
8.69. The adding of 50 ml of 0.1 M
solution of hydrochloric acid HCl
to 500 ml of a buffer solution
caused the change of its pH from
5.9 to 5.1. What is the buffer
capacity of the solution (in
mmol×mLl-1) on acid?
А. 19.0
B. 15.5
C. 16.4
D. 12.5
E. 9.8
8.70. The adding of 25 ml of 0.2 M
solution of hydrochloric acid HCl
to 250 ml of a buffer solution
caused the change of its pH from
7.6 to 6.8. What is the buffer
capacity of the solution (in
mmol×mL-1) on acid?
А. 50
B. 34
C. 30
D. 45
E. 25
8.71. The adding of 14 ml of 0.2 M
solution of hydrochloric acid HCl
to 150 ml of a buffer solution
caused the change of its pH from
8.2 to 7.3. What is the buffer
capacity of the solution (in
µmol×ml-1) on acid?
А. 20.7
B. 12.3
C. 15.4
D. 29.1
E. 24.6
8.72. The adding of 12 ml of 0.1 M
solution of hydrochloric acid HCl
to 100 ml of a buffer solution
caused the change of its pH from
6.5 to 5.8. What is the buffer
capacity of the solution (in
mmol×mL-1) on acid?
А. 12
B. 10
C. 21
D. 15
E. 17
8.73. The adding of 18 ml of 0.3 M
solution of hydrochloric acid HCl
to 200 ml of a buffer solution
caused the change of its pH from
5.8 to 5.2. What is the buffer
capacity of the solution (in
mmol×mL-1) on acid?
А. 34
B. 45
C. 64
D. 20
E. 55
8.74. The adding of 25 ml of 0.2 M
solution of hydrochloric acid HCl
to 300 ml of a buffer solution
caused the change of its pH from
6.9 to 6.1. What is the buffer
capacity of the solution (in
mmol×mL-1) on acid?
А. 20.8
B. 15.4
C. 10.1
D. 28.5
E. 18.2
8.75. The adding of 30 ml of 0.1 M
solution of hydrochloric acid HCl
to 400 ml of a buffer solution
caused the change of its pH from
7.9 to 6.7. What is the buffer
capacity of the solution (in
mmol×mL-1) on acid?
А. 10.75
B. 6.25
C. 5.25
D. 12.45
E. 4.15
8.76. The adding of 17 ml of 0.1 M
solution of hydrochloric acid HCl
to 200 ml of a buffer solution
caused the change of its pH from
6.5 to 4.8. What is the buffer
capacity of the solution (in
mmol×mLl-1) on acid?
А. 5
B. 12
C. 7
D. 2
E. 10
8.77. What is the рН values range of the
blood plasma at acidosis?
А. 4.50 – 5.35
B. 7.65 – 7.85
C. 6.50 – 7.00
D. 7.35 – 7.45
E. 7.00 – 7.35
8.78. What is the рН values range of the
blood plasma at alkalosis?
А. 6.50 – 7.00
B. 8.00 – 8.40
C. 7.00 – 7.35
D. 7.35 – 7.45
E. 7.45 – 7.80
8.79. For the correction of acid-base
equilibrium at the acidosis is
recommended solution of:
А. HCl
B. glucose
C. NaCl
D. Na2SO4
E. NaHCO3
Chapter 9. The Basic Principles of the Volumetric Analysis.
Acid-Base Titration. Determination the Gastric
Juice Acidity
9.1. How to name curve of change the
pH value during titration process?
А. the range of change
B. C. the range of acidity
D. the range of alkality
E. titration curve
9.2. The point in a titration when a
stoichiometric amount of reactant
has been added is:
А. end point
B. –
C. equivalence point
D. neutral point
E. 9.3. A solution of exactly known
concentration is named:
А. molar
B. equimolar
C. D. normal
E. titrant
9.4. Which of the given equation
express the law of equivalents?
А. V1C1 = V2 C 2
B. V1 = V2
C1
C2
C. V1C 2 = V2 C1
D. V1 = V2
m1
m2
E. V1 m1 = V2 m 2
9.5. Method of neutralization is based
on the reaction:
А. HCl + OH– → H2O + Cl–
B.
C.
D.
E.
KOH + HCl → КCl + Н2О
H3O+ + OH– → 2H2O
NaOH + HCl → NaCl + H2O
KOH + H+ → К+ + Н2О
9.6. Which of the given acids is used
as a titrant of neutralization
method?
А. H2CO3
B. HCN
C. CH3COOH
D. HCl
E. H3PO4
9.7. Which of the given acids is used
as a titrant of neutralization
method?
А. H2SO4
B. H3PO3
C. H2CO3
D. HClO
E. CH3COOH
9.8. Which of the given bases is used
as a titrant of neutralization
method?
А. NaOH and NH4OH
B. NH4OH and КОН
C. Са(OH)2 and NH4OH
D. KOH and NaOH
E. –
9.9. Solution of HCl is used as a titrant
for determination of:
А. H2SO4
B. КОН
C. NaCl
D. CH3COOH
E. KCl
9.10. Solution of HCl is used as a titrant
for determination of:
А. H2SO4
B. NaCl
C. NaОН
D. KCl
E. CH3COOH
9.11. Solution of HCl is used as a titrant
for determination of:
А. H2SO4
B. NaCl
C. K2SO4
D. CH3COOH
E. Na2CO3
9.12. Solution of KOH is used as a
titrant for determination of:
А. NaOH
B. K2SO4
C. NaCl
D. Na2CO3
E. H2SO4
9.13. Solution of NaOH is used as a
titrant for determination of:
А. KOH
B. NaCl
C. K2SO4
D. Na2CO3
E. HCl
9.14. Solution of KOH is used as a
titrant for determination of :
А. NH4OH
B. K2SO4
C. NaCl
D. Na2CO3
E. CH3COOH
9.15. Primary standart for
standartisation of HCl solution is:
А. NaCl
B. H2C2O4
C. K2SO4
D. NH4OH
E. Na2CO3
9.16. Primary standart for
standartisation of H2SO4 solution
is:
А. H2C2O4
B. NH4OH
C. K2SO4
D. Na2CO3
E. NaCl
9.17. Primary standart for
standartisation of HCl solution is:
А. K2SO4
B. NaCl
C. NH4OH
D. H2C2O4·2H2O
E. Na2B4O7·10H2O
9.18. Primary standart for
standartisation of H2SO4 solution
is:
А. NaCl
B. Na2B4O7·10H2O
C. K2SO4
D. NH4OH
E. H2C2O4·2H2O
9.19. Primary standart for
standartisation of KOH solution
is:
А. CH3COOH
B. HCl
C. H2C2O4·2H2O
D. Na2CO3
E. K2SO4
9.20. Primary standart for
standartisation of NaOH solution
is:
А. K2SO4
B. H2C2O4·2H2O
C. Na2CO3
D. CH3COOH
E. HCl
9.21. Solution of HCl is used as a titrant
for determination of:
А. NaCl
B. H2C2O4·2H2O
C. K2SO4
D. KOH
E. CH3COOH
9.22. Solution of HCl is used as a titrant
for determination of:
А. K2SO4
B. NaCl
C. CH3COOH
D. H2C2O4·2H2O
E. NaOH
9.23. Solution of HCl is used as a titrant
for determination of:
А. NaCl
B. K2SO4
C. K2CO3
D. CH3COOH
E. H2C2O4
9.24. Solution of KOH is used as a
titrant for determination of:
А. NaOH
B. K2CO3
C. NaCl
D. CH3COOH
E. K2SO4
9.25. Solution of KOH is used as a
titrant for determination of:
А. K2SO4
B. NaCl
C. K2CO3
D. NaOH
E. H2SO4
9.26. Solution of KOH is used as a
titrant for determination of:
А. NaOH
B. K2CO3
C. NaCl
D. HCl
E. K2SO4
9.27. Equivalent of H2SO4 (М(H2SO4)
= 98 g/mole) equal:
А. 56.5
B. 40.0
C. 49.0
D. 32.6
E. 98.0
9.28. Equivalent of H3РO4 (М(H3РO4)
= 98 g/mole) equal:
А. 98.0
B. 49.0
C. 32.6
D. 56.5
E. 68.4
9.29. Equivalent of HCl (М(HCl ) =
36.5 g/mole) equal:
А. 42.5
B. 36.5
C. 35.5
D. 73
E. 18.25
9.30. Equivalent of NaOH (М(NaOH) =
40 g/mole) equal:
А. 60
B. 40
C. 30
D. 20
E. 50
9.31. Equivalent of KOH (М(KOH) =
56 g/mole) equal:
А. 112
B. 14
C. 56
D. 30
E. 28
9.32. Equivalent of Na2CO3
(М(Na2CO3) = 106 g/mole) equal:
А. 35.5
B.
C.
D.
E.
53.0
106.0
44.0
26.5
9.33. The range pH of a changes in
color of phenophthalein (Кa = 10–
9
) is:
А. 8–9
B. 10–11
C. 8–10
D. 9–10
E. 8–11
9.34. The range pH of a changes in
color of methyl orange (рК = 3.5):
А. 4.5–5.0
B. 3.0–4.0
C. 2.5–4.5
D. 3.5–4.5
E. 2.5–3.5
9.35. What color of methyl orange in a
solution with pH=3.5 (рКa = 3.5)?
А. raspberry
B. orange
C. pink
D. yellow
E. red
9.36. What color of methyl orange in a
solution with рН = 1.5 (рКa =
3.5)?
А. orange
B. raspberry
C. yellow
D. pink
E. green
9.37. What color of methyl orange in a
solution with рН = 5.5 (рКa=
3.5)?
А. yellow
B. orange
C. pink
D. red
E. raspberry
9.38. What color of phenolphthalein in
a solution with рН = 7.9 (рКa =
9)?
А. red
B. yellow
C. orange
D. colorless
E. raspberry
9.39. What color of methyl orange in a
solution with pН = 9 (рКa = 9)?
А. colorless
B. red
C. pink
D. raspberry
E. yellow
9.40. What color of methyl orange in a
solution with рН=11 (рКa = 3.5)?
А. colorless
B. raspberry
C. green
D. yellow
E. orange
9.41. How many grams of NaOH (in g)
are required to prepare 800 mL of
0.1 N solution?
А. 6.4
B. 1.5
C. 2.5
D. 1.6
E. 3.2
9.42. How many grams of NaOH (in g)
are required to prepare 300 mL of
0.1 N solution?
А. 2.4
B. 1.2
C. 0.6
D. 1.8
E. 2.8
9.43. How many grams of KOH (in g)
are required to prepare 300 mL of
0.2 N solution?
А. 5.60
B. 0.68
C. 1.68
D. 3.36
E. 4.57
9.44. How many grams of KOH (in g)
are required to prepare 900 mL of
0.1 N solution?
А. 5.60
B. 5.04
C. 2.01
D. 3.48
E. 1.98
9.45. How many grams of H2SO4 (in g)
are required to prepare 900 mL of
0.1 N solution?
А. 8.82
B. 9.80
C. 2.20
D. 4.41
E. 7.56
9.46. How many grams of Na2CO3 (in
g) are required to prepare 300 mL
of 0.2N solution?
А. 10.6
B. 4.68
C. 5.60
D. 6.36
E. 3.18
9.47. For titration of 56 mL of HCl is
used 42 mL of 0.2N NaOH
solution. Calculate normality
(denoted as N or CN) of analysed
HCl solution.
А. 0.1000
B. 0.2500
C. 0.2200
D. 0.1500
E. 0.1600
9.48. For titration of 15 mL of HCl is
used 12 mL of 0.1N NaOH
solution. Calculate normality
(denoted as N or CN) of analysed
HCl solution.
А. 0.1200
B. 0.0400
C. 0.1400
D. 0.0600
E. 0.0800
9.49. For titration of 25 mL of HCl is
used 30 mL of 0.2N NaOH
solution. Calculate normality
(denoted as N or CN) of analysed
HCl solution.
А. 0.2400
B. 0.3400
C. 0.2500
D. 0.1500
E. 0.1600
9.50. For titration of 30 mL of HCl is
used 45 mL of 0.1N NaOH
solution. Calculate normality
(denoted as N or CN) of analysed
HCl solution.
А. 0.1600
B. 0.2500
C. 0.1500
D. 0.2200
E. 0.1000
9.51. For titration of 60 mL of HCl is
used 46 mL of 0.3N NaOH
solution. Calculate normality
(denoted as N or CN) of analysed
HCl solution.
А. 0.2500
B. 0.1500
C. 0.1600
D. 0.3400
E. 0.2300
9.52. For titration of 34 mL of HCl is
used 17 mL of 0.1N NaOH
solution. Calculate normality
(denoted as N or CN) of analysed
HCl solution.
А. 0.0500
B. 0.1400
C. 0.0400
D. 0.1200
E. 0.0600
9.53. For titration of 3 mL of gastric
juice is used 2.4 mL of 0.1 M of
alkali. Calculate the acidity of
gastric juice.
А. 60.0
B. 60.5
C. 75.0
D. 80.0
E. 90.0
9.54. For titration of 8.4 mL of gastric
juice is used 5.6 mL of 0.1 M of
alkali. Calculate the acidity of
gastric juice.
А. 98.2
B. 66.7
C. 55.4
D. 78.5
E. 84.3
9.55. For titration of 25 mL of gastric
juice is used 12.3 mL of 0.1 M of
alkali. Calculate the acidity of
gastric juice.
А. 98.2
B. 60.3
C. 55.4
D. 49.2
E. 84.3
9.56. For titration of 15 mL of gastric
juice is used 13.7 mL of 0.1 M of
alkali. Calculate the acidity of
gastric juice.
А. 53.7
B. 85.2
C. 62.8
D. 66.2
E. 91.3
9.57. For titration of 18 mL of gastric
juice is used 17.1 mL of 0.1 M of
alkali. Calculate the acidity of
gastric juice.
А. 62.8
B. 66.2
C. 53.7
D. 85.2
E. 95.0
9.58. For titration of 4.8 mL of gastric
juice is used 4.2 mL of 0.1 M of
alkali. Calculate the acidity of
gastric juice.
А. 87.5
B. 91.3
C. 62.8
D. 66.2
E. 53.7
The correct answers to test questions
1.1.
1.2.
1.3.
1.4.
1.5.
1.6.
1.7.
1.8.
1.9.
1.10.
1.11.
1.12.
1.13.
1.14.
1.15.
1.16.
1.17.
1.18.
1.19.
1.20.
1.21.
1.22.
1.23.
1.24.
1.25.
1.26.
1.27.
1.28.
1.29.
1.30.
1.31.
2.1.
2.2.
2.3.
2.4.
2.5.
2.6.
2.7.
2.8.
A
C
C
E
D
A
A
E
E
E
B
B
A
B
A
A
A
E
B
A
A
B
E
D
D
B
D
C
C
B
A
C
D
A
A
D
B
E
E
2.9.
2.10.
2.11.
2.12.
2.13.
2.14.
2.15.
2.16.
2.17.
2.18.
2.19.
2.20.
3.1.
3.2.
3.3.
3.4.
3.5.
3.6.
3.7.
3.8.
3.9.
3.10.
3.11.
3.12.
3.13.
3.14.
3.15.
3.16.
3.17.
3.18.
3.19.
3.20.
3.21.
3.22.
3.23.
3.24.
3.25.
3.26.
3.27.
D
E
A
D
A
D
A
E
D
E
D
A
D
C
E
E
D
E
B
B
C
A
C
C
E
C
B
D
C
C
D
B
C
C
B
B
E
C
D
3.28.
3.29.
3.30.
3.31.
3.32.
3.33.
3.34.
3.35.
3.36.
3.37.
3.38.
3.39.
3.40.
3.41.
3.42.
3.43.
3.44.
3.45.
3.46.
4.1.
4.2.
4.3.
4.4.
4.5.
4.6.
4.7.
4.8.
4.9.
4.10.
4.11.
4.12.
4.13.
4.14.
4.15.
4.16.
4.17.
4.18.
4.19.
4.20.
D
E
D
A
C
D
C
E
B
A
E
E
C
D
B
D
D
D
C
E
C
B
C
C
E
D
B
E
C
A
E
A
E
E
E
A
B
C
B
4.21.
4.22.
4.23.
4.24.
4.25.
4.26.
4.27.
4.28.
4.29.
4.30.
4.31.
4.32.
4.33.
4.34.
4.35.
4.36.
4.37.
4.38.
4.39.
4.40.
4.41.
4.42.
4.43.
4.44.
4.45.
5.1.
5.2.
5.3.
5.4.
5.5.
5.6.
5.7.
5.8.
5.9.
5.10.
5.11.
5.12.
5.13.
5.14.
E
D
E
D
A
D
D
E
C
E
D
C
A
D
A
B
B
A
E
A
A
E
A
C
D
C
C
B
B
A
C
D
D
D
D
E
C
D
A
5.15.
5.16.
5.17.
5.18.
5.19.
5.20.
5.21.
5.22.
5.23.
5.24.
5.25.
5.26.
5.27.
5.28.
5.29.
5.30.
5.31.
5.32.
5.33.
5.34.
5.35.
5.36.
5.37.
5.38.
5.39.
5.40.
5.41.
5.42.
5.43.
5.44.
5.45.
5.46.
5.47.
5.48.
5.49.
5.50.
6.1.
6.2.
6.3.
B
E
C
A
B
B
E
B
A
A
A
E
B
B
E
D
A
C
B
C
E
A
E
E
D
A
A
E
C
C
E
C
D
A
C
C
C
E
C
6.4.
6.5.
6.6.
6.7.
6.8.
6.9.
6.10.
6.11.
6.12.
6.13.
6.14.
6.15.
6.16.
6.17.
6.18.
6.19.
6.20.
6.21.
6.22.
6.23.
6.24.
6.25.
6.26.
6.27.
6.28.
6.29.
6.30.
6.31.
6.32.
6.33.
6.34.
6.35.
6.36.
6.37.
7.1.
7.2.
7.3.
7.4.
7.5.
7.6.
7.7.
7.8.
7.9.
A
C
E
E
B
B
E
B
A
B
B
C
B
B
A
A
E
C
B
B
C
E
B
B
A
C
D
E
B
C
A
A
B
B
E
A
B
C
B
B
E
C
B
7.10.
7.11.
7.12.
7.13.
7.14.
7.15.
7.16.
7.17.
7.18.
7.19.
7.20.
7.21.
7.22.
7.23.
7.24.
7.25.
7.26.
7.27.
7.28.
7.29.
7.30.
7.31.
7.32.
7.33.
7.34.
7.35.
7.36.
7.37.
7.38.
7.39.
7.40.
7.41.
7.42.
7.43.
7.44.
8.1.
8.2.
8.3.
8.4.
8.5.
8.6.
8.7.
8.8.
A
B
A
C
E
B
E
B
B
C
E
B
E
C
B
C
E
C
E
E
C
E
A
B
D
B
E
E
A
B
C
E
D
E
E
B
E
A
D
A
C
C
B
8.9.
8.10.
8.11.
8.12.
8.13.
8.14.
8.15.
8.16.
8.17.
8.18.
8.19.
8.20.
8.21.
8.22.
8.23.
8.24.
8.25.
8.26.
8.27.
8.28.
8.29.
8.30.
8.31.
8.32.
8.33.
8.34.
8.35.
8.36.
8.37.
8.38.
8.39.
8.40.
8.41.
8.42.
8.43.
8.44.
8.45.
8.46.
8.47.
8.48.
8.49.
8.50.
8.51.
D
E
E
A
B
D
A
D
E
B
B
D
E
E
B
B
E
E
C
D
A
B
B
D
A
D
C
B
E
C
A
B
B
D
C
C
E
E
E
C
B
D
D
8.52.
8.53.
8.54.
8.55.
8.56.
8.57.
8.58.
8.59.
8.60.
8.61.
8.62.
8.63.
8.64.
8.65.
8.66.
8.67.
8.68.
8.69.
8.70.
8.71.
8.72.
8.73.
8.74.
8.75.
8.76.
8.77.
8.78.
8.79.
9.1.
9.2.
9.3.
9.4.
9.5.
9.6.
9.7.
9.8.
9.9.
9.10.
9.11.
9.12.
9.13.
9.14.
9.15.
E
D
D
D
E
C
E
B
E
A
E
A
B
B
C
A
B
D
E
A
E
B
A
B
A
E
E
E
E
C
E
A
C
D
A
D
B
C
E
E
E
E
E
9.16.
9.17.
9.18.
9.19.
9.20.
9.21.
9.22.
9.23.
9.24.
9.25.
9.26.
9.27.
9.28.
9.29.
9.30.
9.31.
9.32.
9.33.
9.34.
9.35.
9.36.
9.37.
9.38.
9.39.
9.40.
9.41.
9.42.
9.43.
9.44.
9.45.
9.46.
9.47.
9.48.
9.49.
9.50.
9.51.
9.52.
9.53.
9.54.
9.55.
9.56.
9.57.
9.58.
D
E
B
C
B
D
E
C
D
E
D
C
C
B
B
C
B
C
C
B
D
A
D
E
D
E
B
D
B
D
E
D
E
A
C
E
A
D
B
D
E
E
A
CONTENTS
Chapter 1. Solutions. Ways of Expressing Concentrations of Solutions.
Preparation of Solution With the Known Concentration ........................... 2
Chapter 2. Colligative Properties of solutions. Experimental Determination of
the Osmotic Concentration of Solutions by the Method of
Cryometry .................................................................................................. 5
Chapter 3. The Equilibrium and Processes Involving Coordination
Compounds. Preparation and Properties of Coordination
Compounds. Complexonometry ................................................................ 8
Chapter 4. Bioelements and Their Classification. Chemical Properties and
Biological Role of Macroelements .......................................................... 14
Chapter 5. Chemical Properties and Biological Role of Microelements ..................... 18
Chapter 6. Acid-Base Equilibrium. Calculation and Experimental
Determination of the рН of Solutions ..................................................... 24
Chapter 7. Protolytical Processes in Living Organisms. Hydrolysis of Salts .............. 28
Chapter 8. Buffer Solutions, Their Classification and the Mechanism of the
Buffer Action. Preparation of Buffer Solutions. Determination
of the Buffer Capacity and the pH Values of Buffer Solutions.
The Biological Role of Buffer Systems ................................................... 32
Chapter 9. The Basic Principles of the Volumetric Analysis. Acid-Base
Titration. Determination the Gastric Juice Acidity .................................. 44
The correct answers to test questions .......................................................................... 50