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 INORGANIC CHEMISTRY
(Module 1. General Chemistry)
For the 1st year students
оf pharmaceutical faculty
L’VIV – 2012
1
Chapter 1. Atomic-molecule concept. Nomenclature and
classification of inorganic compounds
1.1. Compound aluminum sulfate is
classified as:
А. neutral salt
B. acidic salt
C. basic salt
D. amphotheric hydroxide
E. hydroxide
1.6. Compound potassium nitrate is
classified as:
А. acidic salt
B. amphotheric hydroxide
C. neutral salt
D. basic salt
E. hydroxide
1.2. Compound sodium
hydrogencarbonate is classified
as:
А. acidic salt
B. hydroxide
C. basic salt
D. amphotheric hydroxide
E. neutral salt
1.7. Compound potassium
hydrogencarbonate is classified
as:
А. hydroxide
B. neutral salt
C. acidic salt
D. amphotheric hydroxide
E. basic salt
1.3. Compound aluminium hydroxide
is classified as:
А. hydroxide
B. basic salt
C. amphotheric hydroxide
D. middle salt
E. acidic salt
1.8. Compound calcium phosphate is
classified as:
А. basic salt
B. amphotheric hydroxide
C. acidic salt
D. hydroxide
E. neutral salt
1.4. Compound lithium hydroxide is
classified as:
А. amphotheric hydroxide
B. acidic salt
C. basic salt
D. neutral salt
E. hydroxide
1.9. Compound strontium hydroxide is
classified as:
А. acidic salt
B. hydroxide
C. neutral salt
D. amphotheric hydroxide
E. basic salt
1.5. Compound beryllium hydroxide is
classified as:
А. amphotheric hydroxide
B. acidic salt
C. neutral salt
D. basic salt
E. hydroxide
1.10. Compound potassium sulfide is
classified as:
А. hydroxide
B. amphotheric hydroxide
C. neutral salt
D. acidic salt
E. basic salt
2
1.17. Give the name of an ion C2O4–:
А. carbide
B. hydrogencarbonate
C. oxalate
D. acetate
E. carbonate
1.11. Compound ammonium carbonate
is classified as:
А. hydroxide
B. neutral salt
C. amphotheric hydroxide
D. basic salt
E. acidic salt
1.18. Give the name of an ion NO2–:
А. ammonium
B. nitride
C. –
D. nitrite
E. nitrate
1.12. Compound ammonium phosphate
is classified as:
А. basic salt
B. hydroxide
C. acidics alt
D. amphotheric hydroxide
E. neutral salt
1.19. Give the name of an ion SO32–:
А. sulfate
B. sulfite
C. sulfide
D. thiosulphate
E. sulphonate
1.13. Compound caesium hydroxide is
classified as:
А. neutral salt
B. hydroxide
C. basic salt
D. amphotheric hydroxide
E. acidic salt
1.20. Give the name of an ion SO42–:
А. sulfite
B. thiosulphate
C. sulfide
D. sulphonate
E. sulfate
1.14. Give the name of an ion
CH3COO–:
А. hydrogencarbonate
B. acetate
C. formiate
D. oxalate
E. carbonate
1.21. Give the name of an ion S2–:
А. sulfate
B. thiosulphate
C. sulfite
D. sulphonate
E. sulfide
1.15. Give the name of an ion CO32–:
А. hydrogencarbonate
B. carbonate
C. oxalate
D. acetate
E. carbide
1.22. Give the name of an ion S2O32–:
А. sulfite
B. sulfate
C. sulfide
D. thiosulphate
E. sulphonate
1.16. Give the name of an ion HCO3–:
А. carbonate
B. oxalate
C. carbide
D. acetate
E. hydrogencarbonate
1.23. Give the name of an ion PO43–:
А. metaphosphate
B. diphosphate
3
C. phosphate
D. hypophosphite
E. phosphite
1.30. Ions of perchlorate and nitrate are
in a pair:
А. Cl–, NH4+
B. ClO–, NO2–
C. ClO4–, NO3–
D. Cl–, NO3–
E. ClО–, NО3–
1.24. Give the name of an ion ClO–:
А. chlorate
B. perchlorate
C. chlorite
D. hypochlorite
E. chloride
1.31. Ions of nitrate and cyanide are in a
pair:
А. NO3–, SCN–
B. NO3–, CN–
C. NO2–, CN–
D. NO2–, CSN–
E. NO3–, CN–
1.25. Give the name of an ion ClO4–:
А. chlorite
B. hypochlorite
C. chlorate
D. chloride
E. perchlorate
1.32. Determine the valency of Chlorine
in the following compounds
KClO3 and KClO.
А. VII, III
B. III, II
C. VII, V
D. VII, I
E. V, I
1.26. Give the name of an ion ClO2–:
А. chlorate
B. perchlorate
C. chloride
D. hypochlorite
E. chlorite
1.27. Give the name of an ion ClO3–:
А. chlorite
B. perchlorate
C. chlorate
D. chloride
E. hypochlorite
1.33. Write a molecular formula of
sodium sulfide and lithium
hydrogensulfate. Determine the
valency of Sulfur in
compounds.What is the sum of
these values?
А. 5
B. 6
C. 7
D. 8
E. 4
1.28. Give the name of an ion Cl–:
А. perchlorate
B. hypochlorite
C. chlorite
D. chlorate
E. chloride
1.34. What is the oxidation number of a
Nitrogen in the compound
(NH4)2CO3 ?
А. +4
B. +3
C. –3
D. –4
1.29. In which pair ions of hypochlorite
and nitrite are present:
А. Cl–, NO3–
B. ClO4–, NO3–
C. ClО–, NО3–
D. ClO3–, NO2–
E. ClO–, NO2–
4
E. +5
E. –4
1.35. What is the oxidation number of a
Nitrogen in the compound NaNO3
?
А. –3
B. +5
C. +2
D. +3
E. +4
1.40. What is the oxidation number of a
Nitrogen in the compound HNO2
?
А. +5
B. +3
C. –3
D. +2
E. +4
1.36. What is the oxidation number of a
Nitrogen in the compound
Ca(NО3)2 ?
А. +2
B. +4
C. +3
D. +5
E. –3
1.41. What is the oxidation number of a
Nitrogen in the compound NH3 ?
А. +4
B. –5
C. 0
D. +3
E. –3
1.42. What is the oxidation number of a
Chlorine in the compound
NH4ClO4 ?
А. +5
B. +1
C. –1
D. +4
E. +7
1.37. What is the oxidation number of a
Nitrogen in the compound
Mg(NO2)2 ?
А. +3
B. +4
C. –3
D. +5
E. +2
1.43. What is the oxidation number of a
Sulfur in the compound Na2SO4 ?
А. –2
B. +6
C. +4
D. 0
E. +2
1.38. What is the oxidation number of a
Nitrogen in the compound KNO2
?
А. +2
B. +5
C. –3
D. +3
E. +4
1.44. What is the oxidation number of a
Sulfur in the compound NaHSO3
?
А. –2
B. +6
C. +4
D. +2
E. 0
1.39. What is the oxidation number of a
Nitrogen in the compound NH4Cl
?
А. +3
B. +4
C. –3
D. +5
1.45. What is the oxidation number of a
5
Sulfur in the compound(NH4) 2S ?
А. –2
B. +4
C. +6
D. +2
E. 0
ortophosphoric acid?
А. +1
B. +4
C. +3
D. +5
E. +2
1.46. What is the oxidation number of
an Oxygen in the compound
hydrogen peroxide H2O2 ?
А. –1
B. +2
C. –2
D. +1
E. 0
1.51. What is the oxidation number of a
Carbon in the compound calcium
hydrogencarbonate ?
А. –2
B. 0
C. +4
D. –4
E. +2
1.47. What is the oxidation number of a
Bromine in the compound calcium
bromide ?
А. +3
B. +5
C. +7
D. –1
E. +1
1.52. What is the oxidation number of a
Carbon in the compound
ammonium carbonate ?
А. –2
B. 0
C. +2
D. +4
E. –4
1.48. What is the oxidation number of a
Phosphorus in the compound
magnesium hydrogenphosphate?
А. +5
B. +2
C. +4
D. +3
E. +1
1.53. What is the oxidation number of
Chlorine in the compound barium
chloride?
А. +1
B. +5
C. +7
D. –1
E. +3
1.49. What is the oxidation number of a
Phosphorus in the compound
ammonium phosphate?
А. +1
B. +4
C. +3
D. +2
E. +5
1.54. What is the oxidation number of
Chlorine in the compound
potassium chlorate?
А. +1
B. +7
C. –1
D. +3
E. +5
1.50. What is the oxidation number of a
Phosphorus in the compound
1.55. What is the oxidation number of
Chlorine in the compound calcium
6
hypochlorite?
А. +5
B. +7
C. –1
D. +3
E. +1
D. +7
E. –1
1.57. What is the oxidation number of
Chlorine in the compound
potassium perchlorate?
А. +5
B. –1
C. +1
D. +3
E. +7
1.56. What is the oxidation number of
Chlorine in the compound
potassium hypochlorite?
А. +3
B. +1
C. +5
Chapter 2. Structure of atoms. The Periodic law and Periodic
table by D. Mendeleev
2.1.
2.2.
2.3.
E. [Kr] 4d105s25p3
What is the electronic
configuration of As atom?
А. [He] 2s223
B. [Kr] 4d105s25p3
C. [Ar]3d104s24p3
D. [Ne] 3s23p3
E. [Xe] 4f145d106s26p3
What is the electronic
configuration of Sb atom?
А. [Ar]3d104s24p3
B. [Kr] 4d105s25p3
C. [He] 2s223
D. [Ne] 3s23p3
E. [Xe] 4f145d106s26p3
What is the electronic
configuration of Bі atom?
А. [Ar]3d104s24p3
B. [Ne] 3s23p3
C. [Xe] 4f145d106s26p3
D. [He] 2s223
7
2.4.
What is the electronic
configuration of As(+3) ion?
А. [Ar]3d104s24p6
B. [Ar]3d94s14p3
C. [Ar]3d104s14p1
D. [Ar]3d74s24p3
E. [Ar]3d104s24p0
2.5.
What is the electronic
configuration of As(-3) ion?
А. [Ar]3d94s14p3
B. [Ar]3d104s24p6
C. [Ar]3d104s14p1
D. [Ar]3d74s24p3
E. [Ar]3d104s24p0
2.6.
What is the electronic
configuration of Sb(+3) ion?
А. [Kr] 4d95s05p3
B. [Kr] 4d105s25p6
C. [Kr] 4d85s15p3
D. [Kr] 4d95s25p1
E. [Kr] 4d105s25p0
2.7.
2.8.
2.9.
А. [Xe] 6s26p0
B. [Xe] 6s26p2
C. [Xe] 6s16p1
D. [Xe] 6s16p0
E. [Xe] 6s26p1
What is the electronic
configuration of Bi(+3) ion?
А. [Xe] 4f145d106s06p2
B. [Xe] 4f115d106s26p3
C. [Xe] 4f145d76s26p3
D. [Xe] 4f145d106s26p6
E. [Xe] 4f145d106s26p0
2.13. What is the electronic
configuration of Pb4+ ion:
А. [Xe] 6s16p0
B. [Xe] 6s26p0
C. [Xe] 6s16p0
D. [Xe] 6s16p1
E. [Xe] 6s06p0
What is the electronic
configuration of Sb(-3) ion?
А. [Kr] 4d105s25p0
B. [Kr] 4d95s05p3
C. [Kr] 4d85s15p3
D. [Kr] 4d105s25p6
E. [Kr] 4d95s25p1
2.14. What is the electronic
configuration of Bromine atom
in potassium bromate?
А. 4s24p0
B. 4s24p5
C. 4s14p6
D. 4s04p5
E. 4s24p3
What is the electronic
configuration of As(+3) ion?
А. [Xe] 4f145d106s26p6
B. [Xe] 4f145d76s26p3
C. [Xe] 4f115d106s26p3
D. [Xe] 4f145d106s06p2
E. [Xe] 4f145d106s26p0
2.15. What is the electronic
configuration of Chlorine atom
in potassium perchlorate?
А. 3s03p0
B. 3s23p0
C. 3s1p6
D. 3s13p5
E. 3s23p5
2.10. What is the electronic
configuration of As atom?
А. [Kr] 4d105s25p3
B. [He] 2s223
C. [Xe] 4f145d106s26p3
D. [Ar]3d104s24p3
E. [Ne] 3s23p3
2.16. What is the electronic
configuration of Chlorine atom
in chlorous acid?
А. 3s23p5
B. 3s23p0
C. 3s23p2
D. 3s13p5
E. 3s1p6
2.11. Which of the listed electronic
configurations corresponds to
Fe3+ion
А. [Ar] 3d5 4s1 4p1
B. [Ar] 3d4 4s1
C. [Ar] 3d5 4s0
D. [Ar] 3d3 4s1 4p1
E. [Ar] 3d3 4s2
2.17. What is the electronic
configuration of Bromine atom
in potassium hypobromite?
А. 4s24p5
2.12. What is the electronic
configuration of Pb2+ ion:
8
B.
C.
D.
E.
5s25p4
4s24p0
5s25p5
4s24p4
E. [Xe]4f145d106s0
2.23. Which of the listed electronic
configurations corresponds to
29Сu atom?
А. [Ar] 3d10 4s1
B. [Ar] 3d7 4s2
C. [Ar] 3d8 4s2
D. [Ar] 3d9 4s2
E. [Ar] 3d6 4s2
2.18. What is the electronic
configuration of І– ion?
А. 6s26p4
B. 5s25p4
C. 6s26p5
D. 5s25p5
E. 5s25p6
2.24. Which of the listed electronic
configurations corresponds to
Cu2+ ion ?
А. [Ar]3d104s1
B. [Ar]3d84s1
C. [Ar]3d104s2
D. [Ar]3d84s2
E. [Ar]3d94s0
2.19. What is the electronic
configuration of F– ion?
А. 2s22p4
B. 2s22p5
C. 2s02p6
D. 2s02p5
E. 2s22p6
2.25. Which of the listed electronic
configurations corresponds to
47Ag atom?
А. [Kr]4d105s0
B. [Kr]4d105s1
C. [Kr]4d95s2
D. [Kr]4d85s1
E. [Kr]4d85s2
2.20. What is the electronic
configuration of Br– ion?
А. 4s04p5
B. 4s24p6
C. 5s25p6
D. 4s14p6
E. 4s24p5
2.21. Which of the listed electronic
configurations corresponds to
Cd2+ ion?
А. [Kr]4d105s2
B. [Kr]4d105s0
C. [Kr]4d95s0
D. [Kr]4d105s1
E. [Kr]4d85s2
2.26. What is the electronic
configuration of Ag+ ion?
А. [Kr]4d105s2
B. [Kr]4d85s2
C. [Kr]4d105s0
D. [Kr]4d85s1
E. [Kr]4d95s1
2.27. Which of the listed electronic
configurations corresponds to
79Au atom?
А. [Xe]4f145d96s2
B. [Xe]4f145d86s2
C. [Xe]4f145d96s1
D. [Xe]4f145d106s1
E. [Xe]4f145d106s2
2.22. Which of the listed electronic
configurations corresponds to
Hg1+ ion?
А. [Xe]4f145d106s1
B. [Xe]4f145d86s1
C. [Xe]4f145d96s2
D. [Xe]4f145d106s1
9
configuration of atom
corresponds to Cu2+ ion?
А. [Ar]3d84s1
B. [Ar]3d104s1
C. [Ar]3d104s2
D. [Ar]3d94s0
E. [Ar]3d84s2
2.28. What is the electronic
configuration of ion Au3+?
А. [Xe]4f145d96s2
B. [Xe]4f145d96s1
C. [Xe]4f145d106s0
D. [Xe]4f145d86s0
E. [Xe]4f145d86s1
2.34. What from the given electronic
configuration of atom
corresponds to 47Ag atom?
А. [Kr]4d105s1
B. [Kr]4d85s2
C. [Kr]4d95s2
D. [Kr]4d105s0
E. [Kr]4d85s1
2.29. Which of the listed electronic
configurations corresponds to
13Al atom?
А. [Ne] 3s23p1
B. [Ne] 3s13p0
C. [Ne] 3s23p3
D. [Ne] 3s03p0
E. [Ne] 3s23p4
2.35. What from the given electronic
configuration of atom
corresponds to Ag+ ion?
А. [Kr]4d85s2
B. [Kr]4d85s1
C. [Kr]4d95s1
D. [Kr]4d105s2
E. [Kr]4d105s0
2.30. Which of the listed electronic
configurations corresponds to 5B
atom?
А. [He] 2s22p4
B. [He] 2s22p1
C. [He] 2s22p2
D. [He] 2s22p3
E. [He] 2s22p5
2.36. What from the given electronic
configuration of atom
corresponds to 79Au atom?
А. [Xe]4f145d106s2
B. [Xe]4f145d96s2
C. [Xe]4f145d106s1
D. [Xe]4f145d86s2
E. [Xe]4f145d96s1
2.31. Which of the listed electronic
configurations corresponds to
Al3+ ion?
А. [Ne] 3s23p4
B. [Ne] 3s23p1
C. [Ne] 3s13p0
D. [Ne] 3s23p3
E. [Ne] 3s03p0
2.37. What from the given electronic
configuration of atom
corresponds to Au3+ ion?
А. [Xe]4f145d86s1
B. [Xe]4f145d86s0
C. [Xe]4f145d96s1
D. [Xe]4f145d106s0
E. [Xe]4f145d96s2
2.32. Which of the listed electronic
configurations corresponds to the
р-elements of IVA groups?
А. ns2np2
B. ns2np3
C. ns2np1
D. ns2np0
E. ns1np3
2.38. Which of the listed electronic
2.33. What from the given electronic
10
configurations corresponds to
Mn6+ ion?
А. [Ar]3d44s1
B. [Ar]3d54s0
C. [Ar]3d54s0
D. [Ar]3d04s2
E. [Ar]3d04s1
configurations corresponds to the
atom of Nitrogen?
А. 1s22s22p3
B. 1s22s22p4
C. 1s22s22p2
D. 1s22s22p5
E. 1s22s22p63p1
2.39. Which of the listed electronic
configurations corresponds to
Mn4+ ion?
А. [Ar]3d24s2
B. [Ar]3d44s1
C. [Ar]3d44s0
D. [Ar]3d24s1
E. [Ar]3d14s2
2.44. Which of the listed electronic
configurations corresponds to the
atom of nitrogen in a nitrogen
oxide (ІІІ) N2O3?
А. [He] 2s22p2
B. [He] 2s22p0
C. [He] 2s22p1
D. [He] 2s22p3
E. [He] 2s12p1
2.40. Which of the listed electronic
configurations corresponds to
Mn 7+ ion?
А. [Ar]3d54s0
B. [Ar]3d04s0
C. [Ar]3d44s0
D. [Ar]3d04s1
E. [Ar]3d54s1
2.45. Which of the listed electronic
configurations corresponds to the
atom of nitrogen in a nitric acid
HNO3?
А. [He] 2s22p3
B. [He] 2s12p1
C. [He] 2s12p2
D. [He] 2s22p2
E. [He] 2s02p0
2.41. Which of the listed electronic
configurations corresponds to
Mn2+ ion?
А. [Ar]3d24s1
B. [Ar]3d34s2
C. [Ar]3d54s0
D. [Ar]3d04s2
E. [Ar]3d44s1
2.46. Which of the listed electronic
configurations corresponds to
Cr6+ ion?
А. [Ar]3d04s0
B. [Ar]3d54s0
C. [Ar]3d44s0
D. [Ar]3d54s0
E. [Ar]3d04s1
2.42. Which of the listed electronic
configurations corresponds to
atom of Mn?
А. [Ar]3d34s2
B. [Ar]3d44s2
C. [Ar]3d44s1
D. [Ar]3d64s1
E. [Ar]3d54s2
2.47. Which of the listed electronic
configurations corresponds to
Cr3+ ion?
А. [Ar]3d54s0
B. [Ar]3d44s1
C. [Ar]3d54s1
D. [Ar]3d34s0
E. [Ar]3d44s0
2.43. Which of the listed electronic
11
2.48. Which of the listed electronic
configurations corresponds to
Cr2+ ion?
А. [Ar]3d44s1
B. [Ar]3d24s0
C. [Ar]3d54s0
D. [Ar]3d34s0
E. [Ar]3d44s0
2.53. The same number of energy
levels have atoms of elements
with atomic numbers:
А. 11 and 4
B. 11 and 32
C. –
D. 11 and 13
E. –
2.49. Which of the listed electronic
configurations corresponds to the
atom of Chromium?
А. [Ar]3d64s1
B. [Ar]3d44s2
C. [Ar]3d44s1
D. [Ar]3d54s1
E. [Ar]3d54s2
2.54. The same number of energy
levels have atoms of elements
with atomic numbers:
А. 4 and 53
B. –
C. 4 and 5
D. 4 and 20
E. –
2.50. Which of the listed electronic
configurations corresponds to
Molybdenum atom?
А. [Kr]3d64s1
B. [Kr]3d44s1
C. [Kr]3d44s2
D. [Kr]3d54s2
E. [Kr]3d54s1
2.55. The same number of energy
levels have atoms of elements
with atomic numbers:
А. –
B. 20 and 1
C. 20 and 19
D. –
E. 20 and 7
2.51. Which of the listed electronic
configurations corresponds to the
atom of Tungsten?
А. [Xe]4d45s1
B. [Xe]4d65s1
C. [Xe]4d55s2
D. [Xe]4d55s1
E. [Xe]4d45s2
2.56. The same number of energy
levels have atoms of elements
with atomic numbers:
А. 6 and 4
B. 6 and 19
C. –
D. 6 and 35
E. –
2.52. The same number of energy
levels have atoms of elements
with atomic numbers:
А. 3 and 4
B. 3 and 40
C. –
D. –
E. 3 and 20
2.57. The same number of energy
levels have atoms of elements
with atomic numbers:
А. 16 and 17
B. 16 and 3
C. 16 and 5
D. –
E. –
12
2.58. The same number of energy
levels have atoms of elements
with atomic numbers:
А. –
B. –
C. 12 and 32
D. 12 and 11
E. 12 and 53
2.63. How many protons contain the
nucleus of an atom of element
with atomic number 7?
А. 3
B. 7
C. 6
D. 2
E. 4
2.59. How many protons contain the
nucleus of an atom of element
with atomic number 21?
А. 20
B. 26
C. 12
D. 25
E. 21
2.64. How many protons contain the
nucleus of an atom of element
with atomic number 9?
А. 4
B. 6
C. 9
D. 7
E. 2
2.60. How many protons contain the
nucleus of an atom of element
with atomic number 2?
А. 4
B. 2
C. 6
D. 5
E. 3
2.65. How many protons contain the
nucleus of an atom of element
with atomic number 10?
А. 13
B. 14
C. 10
D. 12
E. 5
2.61. How many protons contain the
nucleus of an atom of element
with atomic number 4?
А. 2
B. 5
C. 6
D. 3
E. 4
2.66. How many protons contain the
nucleus of an atom of element
with atomic number 11?
А. 12
B. 14
C. 11
D. 10
E. 13
2.62. How many protons contain the
nucleus of an atom of element
with atomic number 6?
А. 2
B. 3
C. 4
D. 5
E. 6
2.67. How many protons do contain
the kernel of atom of element
with a sequence number 12?
А. 12
B. 9
C. 11
D. 10
E. 8
13
2.68. How many protons contain the
nucleus of an atom of element
with atomic number 14?
А. 12
B. 11
C. 9
D. 14
E. 10
2.73. How many protons contain the
nucleus of an atom of element
with atomic number 23?
А. 25
B. 23
C. 26
D. 22
E. 24
2.69. How many protons contain the
nucleus of an atom of element
with atomic number 16?
А. 17
B. 18
C. 15
D. 16
E. 14
2.74. How many protons contain the
nucleus of an atom of element
with atomic number 25?
А. 22
B. 25
C. 26
D. 24
E. 23
2.70. How many protons contain the
nucleus of an atom of element
with atomic number 17?
А. 15
B. 18
C. 19
D. 16
E. 17
2.75. How many protons contain the
nucleus of an atom of element
with atomic number 26?
А. 22
B. 25
C. 26
D. 23
E. 24
2.71. How many protons contain the
nucleus of an atom of element
with atomic number 20?
А. 16
B. 18
C. 19
D. 20
E. 17
2.76. How many protons contain the
nucleus of an atom of element
with atomic number 27?
А. 28
B. 26
C. 29
D. 25
E. 27
2.72. How many protons contain the
nucleus of an atom of element
with atomic number 22?
А. 21
B. 16
C. 22
D. 19
E. 20
2.77. How many protons contain the
nucleus of an atom of element
with atomic number 28?
А. 28
B. 27
C. 30
D. 29
E. 31
14
B. 10
C. 34
D. 12
E. 7
2.78. How many protons contain the
nucleus of an atom of element
with atomic number 29?
А. 31
B. 28
C. 32
D. 30
E. 29
2.83. What is the atomic number of
element, the atom of which has 1
electrons at external energy
level?
А. 15
B. 20
C. 18
D. 34
E. 19
2.79. What is the atomic number of
element, the atom of which has 2
electrons at external energy
level?
А. 11
B. 20
C. 16
D. 23
E. 19
2.84. What is the atomic number of
element, the atom of which has 1
electrons at external energy
level?
А. 31
B. 15
C. 26
D. 38
E. 37
2.80. What is the atomic number of
element, the atom of which has 2
electrons at external energy
level?
А. 11
B. 32
C. 12
D. 16
E. 13
2.85. What is the atomic number of
element, the atom of which has 1
electrons at external energy
level?
А. 56
B. 34
C. 14
D. 55
E. 54
2.81. What is the atomic number of
element, the atom of which has 2
electrons at external energy
level?
А. 6
B. 15
C. 3
D. 17
E. 4
2.86. What is the atomic number of
element, the atom of which has 3
electrons at external energy
level?
А. 34
B. 13
C. 7
D. 12
E. 14
2.82. What is the atomic number of
element, the atom of which has 1
electrons at external energy
level?
А. 11
15
А. 20
B. 50
C. 51
D. 2
E. 49
2.87. What is the atomic number of
element, the atom of which has 3
electrons at external energy
level?
А. 32
B. 30
C. 31
D. 15
E. 7
2.92. What is the atomic number of
element, the atom of which has 5
electrons at external energy
level?
А. 14
B. 15
C. 20
D. 4
E. 16
2.88. What is the atomic number of
element, the atom of which has 3
electrons at external energy
level?
А. 48
B. 50
C. 3
D. 49
E. 11
2.93. What is the atomic number of
element, the atom of which has 5
electrons at external energy
level?
А. 2
B. 19
C. 32
D. 33
E. 34
2.89. What is the atomic number of
element, the atom of which has 4
electrons at external energy
level?
А. 3
B. 14
C. 20
D. 15
E. 13
2.94. What is the atomic number of
element, the atom of which has 5
electrons at external energy
level?
А. 52
B. 3
C. 51
D. 50
E. 19
2.90. What is the atomic number of
element, the atom of which has 4
electrons at external energy
level?
А. 16
B. 32
C. 31
D. 11
E. 33
2.95. What is the atomic number of
element, the atom of which has 6
electrons at external energy
level?
А. 17
B. 16
C. 15
D. 3
E. 20
2.91. What is the atomic number of
element, the atom of which has 4
electrons at external energy
level?
16
B. 8
C. 10
D. 20
E. 11
2.96. What is the atomic number of
element, the atom of which has 6
electrons at external energy
level?
А. 35
B. 4
C. 34
D. 19
E. 33
2.99. What is the atomic number of
element, the atom of which has 7
electrons at external energy
level?
А. 20
B. 16
C. 19
D. 3
E. 17
2.97. What is the atomic number of
element, the atom of which has 6
electrons at external energy
level?
А. 53
B. 11
C. 51
D. 20
E. 52
2.100. What is the atomic number of
element, the atom of which has 7
electrons at external energy
level?
А. 20
B. 34
C. 11
D. 36
E. 35
2.98. What is the atomic number of
element, the atom of which has
7electrons at external energy
level?
А. 9
Chapter 3. Equivavlents of substances in chemical reactions
is 20 g/mole?
А. 4.5
B. 12
C. 5
D. 7
E. 28
3.1. What is the equivalent mass of a
metal if its oxide equivalent mass
is 64.2 g/mole?
А. 26.4
B. 16.0
C. 56.2
D. 13.2
E. 32.1
3.3. What is the equivalent mass of a
metal if its oxide equivalent mass
is 31 g/mole?
А. 23
B. 5
3.2. What is the equivalent mass of a
metal if its oxide equivalent mass
17
C. 12
D. 7
E. 4.5
C. 7
D. 5
E. 12
3.4. What is the equivalent mass of a
metal if its oxide equivalent mass
is 12.5 g/mole?
А. 5
B. 8
C. 7
D. 1
E. 4.5
3.9. What is the equivalent mass of an
element if its oxide equivalent
mass is 14.2 g/mole?
А. 12
B. 5
C. 7
D. 6.2
E. 4.5
3.5. What is the equivalent mass of a
metal if its oxide equivalent mass
is 51.8 g/mole?
А. 26.4
B. 32.1
C. 13.2
D. 16.0
E. 43.8
3.10. What is the equivalent mass of an
element if its oxide equivalent
mass is 115 g/mole?
А. 26.4
B. 32.1
C. 56.2
D. 16.0
E. 107
3.6. What is the equivalent mass of an
element if its oxide equivalent
mass is 16 g/mole?
А. 4.5
B. 8
C. 12
D. 7
E. 5
3.11. What is the equivalent mass of a
metal if its sulfate equivalent mass
is 60.2 g/mole?
А. 28
B. 12.2
C. 7
D. 4.5
E. 5
3.7. What is the equivalent mass of an
element if its oxide equivalent
mass is 13.3 g/mole?
А. 4.5
B. 7
C. 28
D. 5.3
E. 5
3.12. What is the equivalent mass of a
metal if its sulfate equivalent mass
is 68 g/mole?
А. 5
B. 4.5
C. 12
D. 20
E. 7
3.8. What is the equivalent mass of an
element if its oxide equivalent
mass is 11 g/mole?
А. 4.5
B. 3
3.13. What is the equivalent mass of a
metal if its sulfate equivalent mass
is 57 g/mole?
А. 7
B. 9
18
C. 12
D. 5
E. 4.5
C. 5
D. 23
E. 12
3.14. What is the equivalent mass of a
metal if its nitrate equivalent mass
is 85 g/mole?
А. 4.5
B. 23
C. 7
D. 5
E. 12
3.19. What is the equivalent mass of a
metal if its carbonate equivalent
mass is 98.7 g/mole?
А. 56.2
B. 68.7
C. 32.1
D. 16.0
E. 26.4
3.15. What is the equivalent mass of a
metal if its nitrate equivalent mass
is 94.7 g/mole?
А. 7
B. 23
C. 12
D. 5
E. 32.7
3.20. What is the equivalent mass of a
metal if its chloride equivalent
mass is 58.5 g/mole?
А. 4.5
B. 7
C. 12
D. 5
E. 23
3.16. What is the equivalent mass of a
metal if its nitrate equivalent mass
is 118.2 g/mole?
А. 26.4
B. 13.2
C. 16.0
D. 32.1
E. 56.2
3.21. What is the equivalent mass of a
metal if its chloride equivalent
mass is 104.2 g/mole?
А. 26.4
B. 68.7
C. 56.2
D. 32.1
E. 16.0
3.17. What is the equivalent mass of a
metal if its carbonate equivalent
mass is 50 g/mole?
А. 12
B. 20
C. 30
D. 7
E. 5
3.22. What is the equivalent mass of a
metal if its chloride equivalent
mass is 40 g/mole?
А. 1
B. 5
C. 8
D. 7
E. 4.5
3.18. What is the equivalent mass of a
metal if its carbonate equivalent
mass is 53 g/mole?
А. 7
B. 30
3.23. What is the equivalent mass of a
metal if its hydroxide equivalent
mass is 37 g/mole?
А. 20
B. 12
19
C. 5
D. 7
E. 30
C. 16.0
D. 26.4
E. 56.2
3.24. What is the equivalent mass of a
metal if its hydroxide equivalent
mass is 49.7 g/mole?
А. 5
B. 23
C. 32.7
D. 12
E. 7
3.29. What is the equivalent mass of a
metal hydroxide if the metal
equivalent mass is 68.7 g/mole?
А. 26.4
B. 32.1
C. 85.7
D. 68.7
E. 56.2
3.25. What is the equivalent mass of a
metal if its hydroxide equivalent
mass is 40 g/mole?
А. 12
B. 7
C. 23
D. 4.5
E. 5
3.30. What is the equivalent mass of a
metal hydroxide if the metal
equivalent mass is 9 g/mole?
А. 23
B. 7
C. 12
D. 5
E. 26
3.26. What is the equivalent mass of a
metal if its hydroxide equivalent
mass is 60.7 g/mole?
А. 26.4
B. 32.1
C. 43.8
D. 13.2
E. 16.0
3.31. Calculate the number of
equivalents of potassium
hydroxide KOH which will react
completely with 1 mole of sulfuric
acid H2SO4.
А. 0.25
B. 2
C. 4
D. 1
E. 0.5
3.27. What is the equivalent mass of a
metal hydroxide if the metal
equivalent mass is 56.2 g/mole?
А. 73.2
B. 26.4
C. 56.2
D. 32.1
E. 68.7
3.32. Calculate the number of
equivalents of sodium hydroxide
NaOH which will react
completely with 1 mole of sulfuric
acid H2SO4.
А. 1
B. 2
C. 0.5
D. 0.25
E. 4
3.28. What is the equivalent mass of a
metal hydroxide if the metal
equivalent mass is 39 g/mole?
А. 13.2
B. 32.1
3.33. Calculate the number of
20
equivalents of calcium hydroxide
Ca(OH)2 which will react
completely with 1 mole of sulfuric
acid H2SO4.
А. 4
B. 0.5
C. 1
D. 0.25
E. 2
Ca(OH)2 which will react
completely with 1 mole of nitric
acid HNO3.
А. 0.5
B. 1
C. 2
D. 0.25
E. 3
3.38. Calculate the number of
equivalents of calcium hydroxide
Ca(OH)2 which will react
completely with 1 mole of orthophosphoric acid H3PO4.
А. 0.25
B. 2
C. 3
D. 0.5
E. 1
3.34. Calculate the number of
equivalents of aluminium
hydroxide Al(OH)3 which will
react completely with 1 mole of
sulfuric acid H2SO4.
А. 0.5
B. 0.25
C. 1
D. 4
E. 2
3.39. Calculate the number of
equivalents of aluminium
hydroxide Al(OH)3 which will
react completely with 1 mole of
ortho-phosphoric acid H3PO4.
А. 0.25
B. 0.5
C. 2
D. 3
E. 1
3.35. Calculate the number of
equivalents of aluminium
hydroxide Al(OH)3 which will
react completely with 1 mole of
nitric acid HNO3.
А. 0.25
B. 1
C. 3
D. 2
E. 0.5
3.40. Calculate the number of
equivalents of sodium hydroxide
NaOH which will react
completely with 1 mole of orthophosphoric acid H3PO4.
А. 0.25
B. 0.5
C. 1
D. 2
E. 3
3.36. Calculate the number of
equivalents of zinc hydroxide
Zn(OH)2 which will react
completely with 1 mole of nitric
acid HNO3.
А. 0.25
B. 1
C. 0.5
D. 2
E. 3
3.41. Calculate the number of
equivalents of zinc hydroxide
Zn(OH)2 which will react
3.37. Calculate the number of
equivalents of calcium hydroxide
21
completely with 1 mole of orthophosphoric acid H3PO4.
А. 2
B. 1
C. 0.25
D. 0.5
E. 3
B.
C.
D.
E.
1
3
2
5
3.46. For calculation the equivalent
mass of sodium oxide Na2O its
molar mass should be divided by:
А. 2
B. 4
C. 1
D. 3
E. 5
3.42. Calculate the number of
equivalents of zinc hydroxide
Zn(OH)2 which will react
completely with 1 mole of
hydrochloric acid HCl.
А. 0.5
B. 2
C. 3
D. 1
E. 0.25
3.47. For calculation the equivalent
mass of beryllium oxide BeO its
molar mass should be divided by:
А. 3
B. 5
C. 4
D. 1
E. 2
3.43. Calculate the number of
equivalents of aluminium
hydroxide Al(OH)3 which will
react completely with 1 mole of
hydrochloric acid HCl.
А. 0.25
B. 2
C. 1
D. 3
E. 0.5
3.48. For calculation the equivalent
mass of aluminium oxide Al2O3
its molar mass should be divided
by:
А. 2
B. 5
C. 6
D. 3
E. 4
3.44. Calculate the number of
equivalents of calcium hydroxide
Ca(OH)2 which will react
completely with 1 mole of
hydrochloric acid HCl.
А. 3
B. 1
C. 0.25
D. 0.5
E. 2
3.49. For calculation the equivalent
mass of iron (III) oxide Fe2O3 its
molar mass should be divided by:
А. 6
B. 5
C. 4
D. 3
E. 2
3.45. For calculation the equivalent
mass of calcium oxide CaO its
molar mass should be divided by:
А. 4
3.50. For calculation the equivalent
mass of chromium (III) oxide
Cr2O3 its molar mass should be
22
divided by:
А. 6
B. 3
C. 4
D. 2
E. 5
mass of phosphorus (III) oxide
P2O3 its molar mass should be
divided by:
А. 2
B. 5
C. 6
D. 4
E. 3
3.51. For calculation the equivalent
mass of sulfur (IV) oxide SO2 its
molar mass should be divided by:
А. 2
B. 1
C. 4
D. 8
E. 6
3.56. For calculation the equivalent
mass of arsenic (V) oxide As2O5
its molar mass should be divided
by:
А. 5
B. 2
C. 1
D. 3
E. 10
3.52. For calculation the equivalent
mass of carbon (IV) oxide CO2 its
molar mass should be divided by:
А. 4
B. 8
C. 1
D. 6
E. 2
3.57. For calculation the equivalent
mass of arsenic (III) oxide As2O3
its molar mass should be divided
by:
А. 2
B. 5
C. 3
D. 4
E. 6
3.53. For calculation the equivalent
mass of sulfur (VI) oxide SO3 its
molar mass should be divided by:
А. 4
B. 8
C. 6
D. 2
E. 1
3.58. For calculation the equivalent
mass of a reactant in the following
chemical transformation: HNO3
→ NO2, its molar mass should be
divided by …
А. 1
B. 3
C. 5
D. 4
E. 2
3.54. For calculation the equivalent
mass of phosphorus (V) oxide
P2O5 its molar mass should be
divided by:
А. 2
B. 5
C. 10
D. 3
E. 1
3.59. For calculation the equivalent
mass of a reactant in the following
chemical transformation: H2SO3
→ H2SO4, its molar mass should
be divided by …
3.55. For calculation the equivalent
23
А. 2
B. 4
C. 5
D. 3
E. 1
B.
C.
D.
E.
3
2
5
4
3.64. For calculation the equivalent
mass of a reactant in the following
chemical transformation: N2 →
NO , its molar mass should be
divided by …
А. 3
B. 1
C. 5
D. 2
E. 4
3.60. For calculation the equivalent
mass of a reactant in the following
chemical transformation: S0 →
H2S, its molar mass should be
divided by …
А. 4
B. 3
C. 1
D. 5
E. 2
3.65. For calculation the equivalent
mass of a reactant in the following
chemical transformation: O2 →
CuO , its molar mass should be
divided by …
А. 4
B. 3
C. 2
D. 1
E. 5
3.61. For calculation the equivalent
mass of a reactant in the following
chemical transformation: NO →
NO2, its molar mass should be
divided by …
А. 4
B. 3
C. 1
D. 2
E. 5
3.66. For calculation the equivalent
mass of sulfuric acid H2SO4 its
molar mass should be divided by:
А. 4
B. 1
C. 2
D. 3
E. 5
3.62. For calculation the equivalent
mass of a reactant in the following
chemical transformation: MgO →
Mg0 , its molar mass should be
divided by …
А. 2
B. 5
C. 1
D. 3
E. 4
3.67. For calculation the equivalent
mass of hydrochloric acid HCl its
molar mass should be divided by:
А. 4
B. 2
C. 5
D. 1
E. 3
3.63. For calculation the equivalent
mass of a reactant in the following
chemical transformation: HNO3
→ NO , its molar mass should be
divided by …
А. 1
24
3.68. For calculation the equivalent
mass of phosphoric acid H3PO4 its
molar mass should be divided by:
А. 4
B. 3
C. 1
D. 5
E. 2
3.73. For calculation the equivalent
mass of sodium hydroxide NaOH
its molar mass should be divided
by:
А. 4
B. 5
C. 3
D. 1
E. 2
3.69. For calculation the equivalent
mass of acetic acid CH3COOH its
molar mass should be divided by:
А. 4
B. 2
C. 5
D. 1
E. 3
3.74. For calculation the equivalent
mass of potassium hydroxide
KOH its molar mass should be
divided by:
А. 4
B. 2
C. 5
D. 1
E. 3
3.70. For calculation the equivalent
mass of nitric acid HNO its molar
mass should be divided by:
А. 3
B. 2
C. 1
D. 4
E. 5
3.75. For calculation the equivalent
mass of calcium hydroxide
Ca(OH)2 its molar mass should be
divided by:
А. 5
B. 4
C. 1
D. 3
E. 2
3.71. For calculation the equivalent
mass of perchloric acid HClO4 its
molar mass should be divided by:
А. 5
B. 2
C. 1
D. 4
E. 3
3.76. For calculation the equivalent
mass of barium hydroxide
Ba(OH)2 its molar mass should be
divided by:
А. 2
B. 3
C. 1
D. 5
E. 4
3.72. For calculation the equivalent
mass of sulfide acid H2S its molar
mass should be divided by:
А. 4
B. 5
C. 2
D. 3
E. 1
3.77. For calculation the equivalent
mass of magnesium hydroxide
Mg(OH)2 its molar mass should
be divided by:
25
А. 4
B. 2
C. 5
D. 1
E. 3
mass of calcium carbonate CaCO3
its molar mass should be divided
by:
А. 4
B. 5
C. 1
D. 3
E. 2
3.78. For calculation the equivalent
mass of aluminium hydroxide
Al(OH)3 its molar mass should be
divided by:
А. 4
B. 1
C. 5
D. 2
E. 3
3.83. For calculation the equivalent
mass of copper sulfate CuSO4 its
molar mass should be divided by:
А. 2
B. 5
C. 4
D. 1
E. 3
3.79. For calculation the equivalent
mass of sodium chloride NaCl its
molar mass should be divided by:
А. 1
B. 5
C. 2
D. 4
E. 3
3.84. For calculation the equivalent
mass of sodium carbonate Na2CO3
its molar mass should be divided:
А. 1
B. 3
C. 2
D. 5
E. 4
3.80. For calculation the equivalent
mass of potassium bromide KBr
its molar mass should be divided
by:
А. 2
B. 4
C. 5
D. 1
E. 3
3.85. For calculation the equivalent
mass of aluminium chloride AlCl3
its molar mass should be divided
by:
А. 3
B. 1
C. 5
D. 2
E. 4
3.81. For calculation the equivalent
mass of silver nitrate AgNO3 its
molar mass should be divided by:
А. 1
B. 3
C. 5
D. 4
E. 2
3.86. For calculation the equivalent
mass of aluminium bromide AlBr3
its molar mass should be divided
by:
А. 2
B. 3
C. 5
D. 1
3.82. For calculation the equivalent
26
E. 4
3.89. For calculation the equivalent
mass of iron (II) phosphate
Fe3(PO4)2 its molar mass should
be divided by:
А. 5
B. 6
C. 1
D. 2
E. 4
3.87. For calculation the equivalent
mass of aluminium nitrate
Al(NO3)3 its molar mass should be
divided by:
А. 2
B. 3
C. 4
D. 1
E. 5
3.90. For calculation the equivalent
mass of iron (III) sulfate
Fe2(SO4)3 its molar mass should
be divided by:
А. 3
B. 6
C. 2
D. 4
E. 5
3.88. For calculation the equivalent
mass of calcium phosphate
Ca3(PO4)2 its molar mass should
be divided by:
А. 3
B. 1
C. 5
D. 2
E. 6
Chapter 4. Solutions. Ways of expressing concentration of
solutions
4.1. What shows a curve of solubility
of a gas?
А. dependence solubility of a gas
with pressure
B. dependence solubility of a gas
with temperature
C. dependence solubility of a gas
with presence of another
substances
D. dependence solubility of a gas
with nature of compound
E. dependence solubility of a gas
with nature of solvent
4.2. How changes the solubility of a
gas with increasing a pressure?
А. decrease
B. increase proportionally
C. decrease proportionally
D. does not change
E. спадає
4.3. How changes the solubility of a
gas with decreasing a pressure?
А. decrease
B. decrease proportionally
C. increase proportionally
D. solubility doesn’t depend on
27
pressure
E. does not change
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
4.4. How changes the solubility of a
gas with increasing a temperature?
А. does not change
B. increase proportionally
C. decrease
D. E. increase
4.9. Molality – that is:
А. number of moles of solute that
are in 1сm3 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 1kg of solvent
E. number of moles of solute that
are in 1kg of solution
4.5. How changes the solubility of a
gas with decreasing a
temperature?
А. does not change
B. increase proportionally
C. increase
D. decrease
E. 4.6. How changes the solubility of a
oxygen in a blood with increasing
a pressure?
А. increase
B. decrease proportionally
C. decrease
D. E. does not change
4.10. Normality (molar concentration of
equivalent) – that is:
А. number of mol-equivalen of
solute that are in 1L of
solution
B. number of mol-equivalen of
solute that are in 100 сm3of
solution
C. number of mol-equivalen of
solute that are in 1kg of
solution
D. number of mol-equivalen of
solute that are in 1 cm3of
solution
E. number of mol-equivalen of
solute that are in 1kg of
solvent
4.7. Mass percentage of solute – that
is:
А. relation between number of
solute and mass of solvent
B. relation between mass of
solute and volume of solution
C. number of moles of solute that
are in 100g of solution
D. gram of solute in 1000g of
solution
E. the percentage by mass of
solute contained in a solution
4.11. Titr – that is:
А. number of gram of solute in 1
L of solution
B. number of gram of solute in 1
сm3 of solvent
C. number of gram of solute in 1
4.8. Molarity – that is:
А. number of moles of solute that
are in 1kg of solvent
28
cm3 of solution
D. number of gram of solute in 1
g of solvent
E. number of gram of solute in 1
kg of solution
E. 15
4.16. How many grams of NaCl are
required to prepare 50 g of 10%
hypertonic solution?
А. 50 g
B. 5 g
C. 10 g
D. 0,5 g
E. 1 g
4.12. Mole fraction of a solute – that is:
А. moles of solute divided by the
moles of solvent
B. relation between number of
particles in a system solute
and mass
C. moles of component substance
divided by the total moles of
solution
D. moles of solvent divided by
the total moles of solution
E. moles of solvent divided by
the moles of solute
4.17. How many grams of glucose are
required to prepare 200 g of 4%
hypotonic solution?
А. 20 g
B. 8 g
C. 200 g
D. 2 g
E. 80 g
4.13. How many grams of AgNO3 are
required to prepare 10 g of 2%
solution?
А. 10
B. 20
C. 2
D. 0,2
E. 0,1
4.18. How many grams of glucose are
required to prepare 200 g of 5%
isotonic solution?
А. 5 g
B. 100 g
C. 20 g
D. 50 g
E. 10 g
4.14. How many grams of NaCl are
required to prepare 200 g of 0,9 %
solution?
А. 1,8
B. 0,9
C. 18
D. 0,18
E. 9
4.19. 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. 20
C. 5
D. 15
E. 30
4.15. How many grams of glucose are
required to prepare 500 g of 5%
solution?
А. 25
B. 5
C. 50
D. 100
4.20. What is the mass percentage (%)
of glucose in a solution that
contains 20 g of glucose in 180 g
of water?
А. 10
B. 15
29
C. 5
D. 30
E. 20
B.
C.
D.
E.
1,83
1,67
1,25
1,00
4.21. What is the mass percentage (%)
of glicerine in a solution that
contains 40.0 g of glicerine in 360
g of water?
А. 40
B. 10
C. 15
D. 30
E. 20
4.26. What is the molarity of a solution
containing 5,6 g of KOH in 400
ml of solution?
А. 1,00
B. 0,75
C. 0,10
D. 0,25
E. 0,50
4.22. What is the molarity of a solution
containing 4.0 g of NaOH in 500
ml of solution?
А. 0,15
B. 0,2
C. 0,1
D. 0,3
E. 0,25
4.27. What is the molarity of a solution
containing 56 g of KOH in 500 ml
of solution?
А. 2,0
B. 0,5
C. 2,5
D. 1,0
E. 1,5
4.23. What is the molarity of a solution
containing 40.0 g of NaOH in 800
ml of solution?
А. 2,50
B. 1,25
C. 1,00
D. 1,50
E. 0,50
4.28. What are the mole fraction of a
solution containing 2 mole of
NaOH and 18 mole Н2О?
А. 2,0
B. 0,1
C. 0,01
D. 0,02
E. 0,2
4.24. What is the molarity of a solution
containing 9.8 g of H2SO4 in 200
ml of solution?
А. 0,50
B. 0,75
C. 1,00
D. 0,25
E. 0,10
4.29. What are the mole fraction of a
solution containing 2 mole of
glucose and 18 mole Н2О?
А. 1,0
B. 0,1
C. 2,0
D. 0,2
E. 0,01
4.25. What is the molarity of a solution
containing 98 g of H2SO4 in 600
ml of solution?
А. 1,50
4.30. What are the mole fraction of a
solution containing 4 mole of
glucose and 36 mole Н2О?
А. 0,1
30
B.
C.
D.
E.
C12H22O11 and 45 mole Н2О?
А. 0,5
B. 0,05
C. 0,1
D. 5
E. 0,01
2,0
1,0
0,4
4
4.31. What are the mole fraction of a
solution containing 5 mole of
Chapter 5. Colligative properties of solutions
5.1. Colligative properties depend on
the:
А. nature of solvent
B. number of solute and solvent
molecules (or ions)
C. percent of ionization
D. nature of solute
E. temperature
5.4. Osmotic concentration
(osmolarity)– that is:
А. total concentration of solute
and solvent molecules in a
solution
B. mass percentage of
electrolytes
C. molar concentration of
albumen molecules
D. concentration of electrolytes
E. concentration of albumen
molecules
5.2. Colligative properties are:
А. osmosis
B. diffusion
C. osmosis and diffusion
D. solubility
E. –
5.5. Solutions, that have the same
osmotic pressure are:
А. hypotonic
B. isotonic
C. hypertonic
D. concentrated
E. saturated
5.3. Oncotic preassure – is:
А. total osmotic preassure of
biological liquids
B. C. osmotic preassure that is
caused by electrolytes in
biological liquids
D. osmotic preassure that is
caused by albumen molecules,
dissolved in a biological
liquids
E. osmotic preassure that is
caused by iones in biological
liquids
5.6. Value of an oncotic pressure (кPa)
are:
А. 3.5·102 – 3.9·103
B. 0.35 – 0.39
C. 3.5·102 – 3.9·102
D. 3.5 – 3.9·102
E. 3.5 – 3.9
5.7. Value of an osmotic pressure
31
(кPa) of a blood:
А. 7.4·103 – 7,8·102
B. 7.4·102 – 7,8·102
C. 7,4 – 7,8
D. 7.4·10 – 7,8·102
E. 74 – 78
D. 0,9% NaCl and 0,5% glucose
E. 0,9% NaCl and 5%-glucose
5.13. What happen with red blood cells,
when they are placed in a 10%
NaCl solution?
А. B. crenation
C. hemolysis
D. does not change
E. hemolysis and crenation
5.8. What happen with red blood cells,
when they are placed in a
hypertonic solution?
А. diffusion
B. hemolysis and crenation
C. D. hemolysis
E. crenation
5.14. What happen with red blood cells,
when they are placed in a 1%
glucose solution?
А. does not change
B. C. hemolysis and crenation
D. crenation
E. hemolysis
5.9. What happen with red blood cells,
when they are placed in a
hypotonic solution?
А. diffusion
B. hemolysis
C. hemolysis and crenation
D. osmosis
E. crenation
5.15. What happen with red blood cells,
when they are placed in a 5%
glucose solution?
А. diffusion
B. hemolysis and crenation
C. does not change
D. crenation
E. hemolysis
5.10. How to calculate osmotic pressure
of electrolytes solution?
А. π = iCNRT
B. π = νRT
C. π = iCmRT
D. π = CMRT
E. π = iCMRT
5.16. Freezing point depression
constant depend on the:
А. concentration of solution
B. nature of solvent
C. nature of solute
D. temperature
E. presence of catalyst
5.11. How to calculate osmotic pressure
of non-electrolytes solution?
А. π = CMRT
B. π = iCMRT
C. π = CNRT
D. π = iCNRT
E. π = (m/M)RT
5.17. What is the freezing point of
solution (0С) containing 1 mol of
maltose and 2000 g of water?
А. –0.93
B. –1.86
C. +1.86
D. –3.72
5.12. Isotonic solutions are:
А. 5% NaCl and 0,9% glucose
B. 9% NaCl and 5% glucose
C. 9% NaCl and 0,5% glucose
32
E. +3.72
C. 100.52
D. 100.00
E. 101.,86
5.18. Boiling point elevation constant
depend on the:
А. presence of catalyst
B. nature of solvent
C. nature of solute
D. temperature
E. concentration of solution
5.20. What is the boiling point of
solution (0С) containing 1 mol of
urea and 500 g of water?
А. 101.04
B. 100.00
C. 101.00
D. 100.52
E. 101.86
5.19. What is the boiling point of
solution (0С) containing 2 mol of
glucose and 2000 g of water?
А. 101. 04
B. 101.00
Chapter 6. The basic terms of chemical thermodynamics.
Thermochemistry. The direction of chemical
processes passage
B. T=const, U=const
C. P=const, U=const
D. V=const, Q=const
E. P=const, T=const
6.1. The mass of the substance (m) and
its volume (V) are:
А. intensive properties
B. state functions of the system
C. thermodynamic potentials
D. thermodynamic properties
E. extensive properties
6.4. Thermochemistry is the study of:
А. transformations between
different kinds of matter
B. different kinds of energy
changing associated with
physical and chemical
processes
C. transformations of internal
energy into work under
chemical reactions
D. different kinds of energy
changing associated with
chemical reactions
E. transformations of heat into
internal energy under chemical
6.2. Temperature (Т) and pressure (Р)
are:
А. kinetic properties
B. extensive properties
C. thermodynamic potentials
D. intensive properties
E. state functions of the system
6.3. The isothermal – isochoric
thermodynamic process is carried
out under:
А. T=const, V=const
33
reactions
according to the way of their
interaction with the surroundings:
А. homogeneous and
heterogeneous
B. isolated, closed, open
C. physical and chemical
D. one-, two- and threecomponents
E. equilibrium and nonequilibrium
6.5. The isothermal – isobaric
thermodynamic process is carried
out under:
А. T=const, U=const
B. P=const, U=const
C. T=const, V=const
D. T=const, P=const
E. V=const, P=const
6.6. A system which can exchange
energy only with the surroundings
is called:
А. isolated
B. equilibrium
C. open
D. closed
E. thermodynamic
6.10. Chemical thermodynamics is
based on:
А. the main laws of physics and
chemistry
B. two main laws of
thermodynamics
C. three main laws of
thermodynamics
D. different physical laws and
equations
E. one main laws of
thermodynamics
6.7. What is the kind of a system when
metal plate of zinc is dipped into
the test-tube with the sulfuric acid
H2SO4 solution?
А. physical, heterogeneous,
closed
B. chemical, heterogeneous, open
C. chemical, heterogeneous,
isolated
D. chemical, homogeneous,
isolated
E. chemical, homogeneous, open
6.11. State functions are the parameters
of systems which depend on:
А. the initial and final states of
the system
B. the ability of a system to come
back to its initial state
C. the path by which the process
occurs
D. the equilibrium constant value
E. the exchange by mass and
energy with the surroundings
6.8. What is the kind of a system when
calcium carbonate CaCO3 is
heated in a test-tube?
А. heterogeneous, two-phases
B. heterogeneous, equilibrium
C. heterogeneous, three-phases
D. heterogeneous, nonequilibrium
E. homogeneous, one-phase
6.12. Heat and work depends on:
А. the initial and final states of
the system
B. the exchange by mass and
energy with the surroundings
C. the ability of a system to come
back to its initial state
D. the equilibrium constant value
E. the path by which the process
6.9. Thermodynamic systems may be
divided into following types
34
occurs
А. 1, 2, 3
B. 1, 3
C. 3
D. 2
E. 1
6.13. Does the ∆Н°298 value for a
chemical reaction depends on the
presence of a catalyst in a system?
А. depends of nature of a catalyst
B. doesn’t depend
C. depends in homogeneous
systems
D. depends
E. depends in heterogeneous
systems
6.18. Which reactions through the listed
ones are endothermic? 1. N2 + O2
= 2NO 2. H2 + Cl2 = 2HCl 3. H2 +
S = H2S
А. 1, 2, 3
B. 1
C. 2, 3
D. 3
E. 2
6.14. The main law of thermochemistry
is:
А. Hess’ law
B. Nernst’ law
C. Henry’s law
D. Avogadro’ law
E. law of mass action
6.19. Point out the correct consequence
of the thermal stability increasing
for hydrogen halogenides. The
standard enthalpies of formation
values for hydrogen halogenides
(in kJ/mol) are: ∆H°(HBr) = –
36,3; ∆H°(HI) = 26,6; ∆H°(HF)
= −270,7; ∆H°(HCl) = −92,3.
А. HF < HBr < HCl < HI
B. HI > HBr > HCl > HF
C. HI < HBr < HCl < HF
D. HF < HCl < HBr < HI
E. HBr < HCl < HF < HI
6.15. The standard enthalpy of
formation for which of the
following substances is equal to
zero?
А. O3
B. О2
C. СО2
D. Н2О
E. С6Н12О6
6.20. Which compound through the
listed ones can be more easily
decomposed under heating?
А. N2O3(g)
B. all compounds are readily
decompose identically
C. N2О(g)
D. NO(g)
E. NO2(g)
6.16. The standard enthalpy of
formation for which of the
following substances is equal to
zero?
А. H2O(g)
B. HF(g)
C. HF(liquid)
D. N2(solid)
E. N2 (g)
6.21. What will be the standard
enthalpy change for the reaction:
С(graphite) + 2 Н2(g) = СН4(g)?
А. it will increase at 75 kJ
B. it will decrease at 51 kJ
6.17. Which reactions through the listed
ones are exothermic? 1. N2 + O2 =
2NO 2. H2 + Cl2 = 2HCl 3. H2 + I2
= 2HI
35
C. it will decrease at 175 kJ
D. it will increase at 186 kJ
E. it will decrease at 75 kJ
the internal energy of the system:
Q= ∆U?
А. for equilibrium processes
B. for isochoric processes
C. for isobaric processes
D. for adiabatic processes
E. for isothermal processes
6.22. The mathematical equation for the
first law of thermodynamics is:
А. Q = ∆U + W
B. ∆U = Q – W
C. Q = ∆U – W
D. Q = – ∆Н
E. ∆U = Q + W
6.27. For what kind of thermodynamic
processes the heat effect of the
reaction equals to the change of
the enthalpy: Q = ∆H?
А. for isobaric processes
B. for equilibrium processes
C. for isochoric processes
D. for adiabatic processes
E. for isothermal processes
6.23. For which of the given substances
the standard enthalpy of formation
doesn’t equal to zero?
А. С(diamond)
B. I2(solid)
C. Р(white)
D. N2(g)
E. С(graphite)
6.28. The heat effect for the process of
water transformation from liquid
to steam equals to:
А. - 44 kJ/mol
B. 4.4 kJ/mol
C. 40 kJ/mol
D. 44 kJ/mol
E. -241.8 kJ/mol
6.24. 10.5 kJ of heat released when 11.2
L of H2S was formed. What is the
standard enthalpy of formation for
H2S?
А. 10.5 kJ/mol
B. –21.0 kJ/mol
C. 21.0 kJ/mol
D. 5.25 kJ/mol
E. –5.25 kJ/mol
6.29. For which of the listed
compounds the standard
enthalpies of combustion
(∆Н°comb.) are equal to zero?
А. СО, NН3
B. NO, NH3
C. О2, Н2
D. СО2, Н2О
E. СО, Н2
6.25. Which reactions through the listed
ones are exothermic: 1. N2O4 =
2NO2 2. 1/2 N2 + 1/2 O2 = NO 3.
H2 + 1/2 O2 =H2O
А. 2
B. no one through the listed
reactions
C. 1
D. 1, 2, 3
E. 3
6.30. In which of the given cases a
reaction is possible at any
temperatures?
А. ∆H0 > 0 і ∆S0 < 0
B. |∆H0| = |T∆S0|
C. ∆H0 < 0 і ∆S0 > 0
D. no one
6.26. For what kind of thermodynamic
processes the heat effect of the
reaction equals to the change of
36
E. ∆H0 > 0, T=0
FeCl3(solid)
B. CO(g) + Cl2(g) = COCl2(g)
C. 4 Al(solid) + 3 C(solid) =
Al4C3(solid)
D. CH4(g) + Cl2(g) =
CH3Cl(liquid) + HCl(g)
E. 2 NH3(g) = N2(g) + 3 H2(g)
6.31. Point out for which of the given
processes ∆S0 > 0.
А. 2H2S(g) + 3O2(g) → 2H2O(g)
+ 2SO2(g)
B. for none of the given reactions
C. H2(g) + F2(g) → 2HF(g)
D. NH4NO2(solid) → 2H2O(g) +
N2(g)
E. 2CO(g) + O2(g) → 2CO2(g)
6.36. The change of free Gibbs’ energy
may be calculated as:
А. F = U – TS
B. ∆G = T∆S – ∆U
C. ∆G = ∆H – T∆S
D. ∆G = T∆S – ∆H
E. G = H + T∆S
6.32. Point out for which of the given
processes the entropy increases?
А. water freezing
B. ethylene polymerization
C. association of ions
D. evaporation of alcohol
E. transformation of graphite into
diamond
6.37. Free Gibbs’ energy is the measure
of:
А. internal energy
B. dispersal energy
C. non-reversible process
D. the energy which can be used
for fulfilling a work
E. thermodynamic stability of the
system
6.33. What is the standard entropy
change for the process of graphite
transformation into diamond?
SС(diamond)= 2,4 J/(mol•К)?
А. - 8.1 J/(mol•К)
B. 5.7 J/(mol•К)
C. 8.1 J/(mol•К)
D. -3.3 J/(mol•К)
E. 3.3 J/(mol•К)
6.38. Point out without any calculations
for which of the given processes
the entropy increases?
А. 4 HСl(g) + О2(g) = 2Cl2(g) + 2
H2O(g)
B. 2СО(g) + О2(g) = 2СО(g)
C. С(graphite) + СО2(g) =
2СО(g)
D. 2SO2(g) + 2NO2(g) = 2SO2(g)
+ N2(g)
E. H2(g) + Сl2(g) = 2HCl(g)
6.34. The entropy of elements may be
equal to zero only under the
conditions of:
А. normal conditions
B. the temperature of absolute
zero (T=0 °K)
C. STP
D. P = const
E. T = const
6.39. A chemical reaction is impossible
at any temperature in the case of:
А. ∆H < 0, ∆S < 0, ∆G < 0
B. ∆H < 0, ∆S < 0, ∆G > 0
C. ∆H > 0, ∆S < 0, ∆G > 0
D. ∆H < 0, ∆S > 0, ∆G > 0
6.35. Point out without any calculations
for which of the given processes
the entropy increases?
А. 2 Fe(solid) + 3 Cl2(g) = 2
37
E. ∆H > 0, ∆S > 0, ∆G > 0
compounds in the organism?
А. CO2, N2, H2O
B. CO, H2O, SO3
C. CO, NO, H2O
D. CO2, NO2, SO3
E. CO2, NO, SO2
6.40. Is it possible to determine the
absolute value of the enthalpy and
free Gibbs’energy?
А. possibly to determine at STP
B. possibly to determine at
normal conditions
C. it is possibly to determine
experimentally
D. impossible
E. possible
6.45. What kind of system are
biological systems?
А. homogeneous closed
B. heterogeneous nonequilibrium
C. homogeneous open
D. heterogeneous isolated
E. homogeneous equilibrium
6.41. Entropy is the measure of:
А. internal energy
B. heat capacity of the system
C. the energy which can be used
for fulfilling a work
D. dispersal energy
E. reservation of energy of a
system
6.46. What kind of system are the living
organism cells?
А. open
B. non-equilibrium
C. equilibrium
D. closed
E. isolated
6.42. Is the forward reaction
C(graphite) + CO2(g) = 2 CO(g)
possible? At what conditions?
А. possible at steady pressure
B. possible at high temperature
C. possible at normal conditions
D. impossible even at high
temperature
E. possible at STP
6.47. The main source of energy for the
human’s organism is:
А. ATP
B. carbohydrates
C. proteins
D. vitamins and minerals
E. fats
6.43. The decreasing of Gibbs’ free
energy shows that the forward
reaction is spontaneous at the
conditions of:
А. m = constant, heat capacity is
const
B. P = const
C. P = const, V = const
D. T = const, P = const
E. V = const, T = const
6.48. The daily ration of proteins for an
adult is:
А. 50–80 g
B. 150-200 g
C. 60–70 g
D. 75–85 g
E. 30–50 g
6.49. The daily ration of fats for an
adult is:
А. 70–80 g
B. 60–70 g
C. 110–120 g
6.44. What substances are the final
products of metabolism of organic
38
D. 30–50 g
E. 90-110 g
6.53. What kind of thermodynamic
system is the living organism?
А. opened system in the state of
thermodynamic equilibrium
B. closed system in stationary
state
C. closed system in the
equilibrium state
D. opened system in stationary
state
E. isolated system in the
equilibrium state
6.50. The daily ration of carbohydrates
for an adult is:
А. 60–70 g
B. 90–100 g
C. 250–280 g
D. 300–370 g
E. 380–390 g
6.51. Energy which is accumulated in
the organism may be released
under the process of:
А. photosynthesis
B. bio-polymers synthesis
C. foods metabolism
D. enzyme catalysis
E. ATP hydrolysis
6.54. Which one of the given equations
is the expression of the second
law of thermodynamics for
biological systems?
А. S = Smax
B. ∆Q = T ⋅ ∆S
C. ∆S > 0
6.52. The molecules of what
compounds can act as energy
storage in bio-systems?
А. DNA
B. RNA
C. АDP
D. ATP
E. glucose
∆τ
D. ∆S = ∆Q
T
E. ∆S = 0
Chapter 7. The rate and mechanism of chemical reactions
7.2. Сhose the reaction from the given
ones that has the highest rate:
t
→
А. MgCO3 
MgO + CO2
+
B. H2O + H = H3O+
C. 2SO2 + O2 = 2SO3
D. H2 + I2 = 2HI
E. 3H2 + N2 = 2NH3
7.1. The units of the rate of a chemical
reaction in homogeneous
systems?
А. mol⋅m2⋅min–1
B. mol⋅L–1⋅min.
C. mol⋅м3⋅s–1
D. mol⋅L–1⋅s–1
E. mol⋅mL–1⋅s–1
7.3. Сhose the reaction from the given
39
ones that has the highest rate:
Kt
А.
C2H12O6 → 2C2H5OH +
2CO2
Kt
B. CO + 2H →
CH3OH
2
t
C.

→
2NH3
N2 +3H2
D. NaOH + HCl = NaCl + H2O
E. 2NO + Cl2 = 2NOCl
is:
А.
B.
C.
D.
E.
7.8. Chose the reaction that take place
with the highest rate, if for the
same interval of time 3,0 grams of
products were forms?
7.4. The expression of the Rate Law
for reaction 2NO (g)+O2(g) =
2NO2(g) is:
А. v = [2NO] 2 ·[O2]
B. v =k[NO]2·[O2]
C. v =k[NO] + [O2]
D. v =k[NO2]2·[O2]
E. v = [NO]2 + [O2]
I.
1
2
1
2
Cl2(g) = HCl(g)
O2(g) = H2O(g)
1
7.9. Сhose the reaction from the given
ones that has the highest rate:
А. 2SO2+ O2 = 2SO3
B. Ва(OH)2 + 2HCl = ВаCl2 +
2H2O
C. (C6H10O5)n + nH2O
+
,t
H

→ nC6H12O6
∆τ
∆c
υ =−
∆τ
C.
c −c
υ= 2 1
τ 2 − τ1
D.
B.
υ =±
H2(g) +
1
υ=
E.
2
III. 2 H2(g) + 2 F2(g) = HF(g)
А. B. rate is the same
C. II
D. I
E. III
7.6. The instantaneous rate may be
calculated according to equation:
А.
∆c
υ = kc 2
1
II. H2(g) +
7.5. The units of the rate of a chemical
reaction in heterogeneous
systems:
А. molּmLּs-1
B. molּLּs-1
C. kmolּм3ּmin-1
D. mol/(cm3ּs)
E. molּL/min
D.
v = k[SO2] + [O2]
v = k[SO2]2 [O2]
v = [SО2] [O2]
v = [SO2] [O2]2
v = k[SO3]
2NH3
t

→
N2 + 3H2
Kt
E. 2C H OH →
(C2H5)2O +
2 5
H2O
7.10. The expression of the Rate Law
for reaction 2CO(g) + O2(g) =
2CO2(g) is:
А. v = k[CO]2⋅[O2]
B. v = k[CO2]2
C. v = [CО]⋅ [O2]
D. v = [CO]2⋅[O2]
E. v = k[2CO] ⋅[O2]
dc
dτ
7.7. The expression of the Rate law for
reaction 2SO2(g) + O2(g) = 2SO3(g)
40
СаСО3(s) → СаО(s) + СО2(g)
correct expression of the rate law
is:
А. v = k[СаО] + [СO2]
B. v = k[СаО ][СO2]
C. v = k[СаСО3 ]
D. v = k
E. v = [СаСО3 ]
7.11. The rate increases in a
heterogeneous systems with:
А. increasing surface area
B. decreasing of concentration of
reactant
C. irradiation
D. all methods
E. cooling
7.17. Decomposition of HI (hydrogen
iodide) on the surface of gold is
the reaction of:
А. first order
B. higher order
C. zero order
D. E. second order
7.12. The expression of the Rate Law
for reaction С(gr) + СО2(g) = 2СО(g)
is:
А. v = k[С] [СO]
B. v = k [С] [СO2]
C. v = k[С]
D. v = k [СO2]
E. v = k[СО2]
7.18. Decomposition of NH3 on the
surface of tungsten (W) is the
7.13. The expression of the Rate Law
for reaction Н2О(g) + СО(g) =
СО2(g) +Н2(g) is:
А. v = k[Н2О ] [СO]
B. v = k ([Н2О ] + [СO])
C. v = k [Н2 ] [СO2]
D. v = k [СO]
E. v = [Н2О ] [СO]
reaction of: 2NH3
+3H2
А. higher order
B. second order
C. first order
D. zero order
E. -
7.14. The expression of the Rate Law
for reaction N2(g) + 3Н2(g) =
2NH3(g) is:
А. v = k[N2 ] [H2]3
B. v = k[N2 ]+ [H2]3
C. v = k[NH3 ]2
D. v = 2[N2 ] 3[H2]
E. v = [N2 ] [H2]3
t

→N
2
7.19. The given reaction of hydrolysis
С12Н22О11 + Н2О = С6Н12О6 (gl) +
С6Н12О6(fr) is:
А. bimolecular reaction of the
zero order
B. monomolecular reaction of the
second order
C. bimolecular reaction of the
first order
D. bimolecular reaction of the
second order
E. monomolecular reaction of the
first order
7.15. How to name the main law of the
chemical kinetics?
А. Rate law
B. Ostwald’s law
C. D. The law of equivalents
E. Henry’s law
7.20. The reaction CO + Cl2 = COCl2 is
a reaction:
7.16. According to the reaction
41
А. bimolecular reaction of the
second order
B. monomolecular reaction of the
first order
C. bimolecular reaction of the
first order
D. monomolecular reaction of the
second order
E. monomolecular reaction of the
zero order
Ea in the most of chemical
reactions:
А. 100-300 kJ/mol
B. 150-300 kJ/mol
C. 50-150 kJ/mol
D. 100-200 kJ/mol
E. 40-200 kJ/mol
7.25. Which of the given reactions take
place by the molecular
mechanisms
А. 2NO + O2 = 2NO2
B. 2H2 + O2 = 2H2O
C. H3O+ + OH– = 2H2O
D. H2 + Cl2 = 2HCl
E. Ba2+ + SO42– = BaSO4
7.21. The reaction CuO(s) + H2(g) = Cu(s)
+ H2O(l) is a reaction:
А. bimolecular reaction of the
first order реакція
B. bimolecular reaction of the
second order
C. heterogeneous, second order
D. monomolecular reaction of the
first order
E. homogeneous, second order
7.26. Which of the given reactions take
place by the radical mechanisms?
А. CH4 + Cl2 = CH3Cl + HCl
B. HNO3 + KOH = KNO3 + H2O
C. 2NO + O2 = 2NO2
D. AgNO3 + HCl = AgCl↓ +
HNO3
E. H2 + I2 = 2HI
7.22. When the value of rate constant
and rate of reaction are equal?
А. reaction take place in
homogeneous system
B. reaction take place in
homogeneous system
C. concentrations of reactants are
equal 1 mol/L
D. concentrations of reactants are
the same, but not equal 1
mol/L
E. in all cases
7.27. If the activation energy of the
chemical reaction is Еа > 120
kJ/mol, its rate is:
А. high
B. very high
C. average
D. low
E. very low
7.23. When the order and the
molecularity are congruent?
А. for photochemical reaction
B. for complicated reaction
C. always are congruent
D. E. only for simple, one step
reaction
7.28. If the activation energy of the
chemical reaction is Еа ≈ 40
kJ/mol, its rate is:
А. very low
B. low
C. high
D. very high
E. average
7.24. The range of the activation energy
7.29. The solubility of a slightly
42
dissolved salt AmBn, which
dissociate according to the scheme
→
AmBn ← mAn+ + nBm– may be
calculated as:
А.
Ksp
S=
form?(IP – ion product)
А. ІP = Ksp
B. ІP> Ksp
C. ІP ≈ Ksp
D. E. ІP< Ksp
m+n
7.34. Solubility product constant Ksp
depends on:
А. B. presence of catalyst
C. molar concentration of ions
D. concentration of salt
E. temperature
B. S = K
sp
C.
S= (m⋅n)
D.
S= (m+n)
E.
S= (m+n)
Ksp
m⋅n
Kp
m+n
Ksp
7.35. The solubility product constant
Ksp of a slightly dissolved salt
AmBn, which dissociate according
→
to the scheme AmBn ← mAn+ +
nBm– may be calculated as:
А. Ksp = [A]m⋅[В]n
B. Ksp = [An+]m⋅[Bm–]n
C.
a n+ ⋅ aBmKsp = A
D.
a n + + a B mKsp = A
E. Ksp = [An+]⋅[Bm–]
mm ⋅ nn
7.30. What is the relations between
Gibbs energy and the solubility
product constant Ksp?
А. log Ksp =∆G/(2,303RT)
B. ∆G = - RTln Ksp
C. ∆G = RTlog Ksp
D. ∆G = RTln Ksp
E. log Ksp =–∆G/(2,303RT)
(
7.31. In which case the solution of
BaSO4 is over-saturated?
А. [Ba2+]⋅[SO42–] = Ksp
B. [Ba] ⋅[SO4]= Ksp
C. [Ba2+]⋅[SO42–] > Ksp
D. [Ba2+]⋅[SO42–] ≈ Ksp
E. [Ba2+]⋅[SO42–] < Ksp
) (
)
7.36. The solubility of a slightly
dissolved salt is expressed by the:
А. dissociation constant
B. coefficient of absorption
C. solubility product constant
D. percent of solubility
E. coefficient of solubility
7.32. In which case the solution of AgI
is saturated?
А. [Ag+]⋅[I–] < Ksp
B. [Ag+]⋅[I–]≈ Ksp
C. [Ag+]⋅[I–] > Ksp
D. [Ag+]⋅[I–] = Ksp
E. [Ag+]+[I–] < Ksp
7.37. The expression of the solubility
product constant Ksp for Ca3
(PO4)2 is:
А. Ksp = 3[Ca2+]3· 2[PO43–]2
B. Ksp = [Ca2+]3·[PO43–]2
C. Ksp = 3[Ca2+]3+2[PO43–]2
D. Ksp = ([Ca2+]3·[PO43–]2)/
[Ca3(PO4)2]
7.33. In which case the precipitate of
slightly dissolved salt will
43
E. Ksp = [Ca2+]3 + [PO43–]2
D. Ksp = a(Ca2+) a(F–)
E. Ksp = [Ca2+][2F–]
7.38. Compare the values for Ksp next
salts HgS, PbS, CdS, SnS, TlS2
and choose one, which is the least
soluble in a water.
А. Ksp (HgS) = 4,0·10–53
B. Ksp (TlS2) = 5·10–21
C. Ksp (PbS) = 2,5·10–27
D. Ksp (CdS) = 1,2·10–28
E. Ksp (SnS) = 1,0·10–27
7.43. The expression of the solubility
product constant Ksp for Ag2CrO4:
А. Ksp = [Ag+]+[Cr2O42–]
B. Ksp = 2[Ag+]•[CO42–]
C. Ksp = [Ag+]2⋅[CrO42–]
D. Ksp = [Ag+]⋅[CrO42–]
2
E.
(a ) ⋅ aCrO
Ksp = Аg
+
2-
4
7.44. The solubility of Ag2S (in mol/L)
may be calculated according to
the equation:
А. S= K
sp
7.39. Which ions can not be present
simultaneous (одночасно) in a
solution?
А. Na+, SO42–
B. Cu2+, SO42–
C. Fe2+, OH–
D. NH4+, Cl–
E. K+, NO3–
B.
S= 3
Ksp
4
C. S= 3 4K
sp
7.40. Choose the pair of compound,
which ions can not be present
simultaneous in a solution:
А. Ba(OH)2 and CO2
B. NaOH and P2O5
C. AgNO3 and HCl
D. Al(NO3)3 and HCl
E. CuSO4 and BaCl2
D.
Ksp
S=
2
E.
S= 3
Ksp
27
7.45. The solubility of Fe(OH)3 (in
mol/L) may be calculated
according to the equation:
А.
Ksp
S= 3
4
B. S= 3 4K
7.41. The expression of the solubility
product constant Ksp for
Mg(OH)2:
А.
= aMg 2+ ⋅ a _
OH
Ksp
2+
B. Ksp = [Mg ]⋅[OH–]
C. Ksp = [Mg2+]⋅[OH–]2
D. Ksp = [Mg2+]•2[OH–]
E. Ksp = 2[Mg2+]•2[OH–]
sp
C.
S= 3
Ksp
27
D. S= K
sp
E.
7.42. The expression of the solubility
product constant Ksp for CaF2:
А. Ksp = [Ca2+] + [F–]
B. Ksp = [Ca2+][F–]2
C. Ksp = [Ca2+] / [F–]2
S= 4
K sp
27
7.46. Expression of the equilibrium
constant for the reaction 2SO2 +
O2 ⇄ 2SO3 is:
44
[SO 2 ]2 ⋅ [O 2 ]
[SO 3 ]2
[SO3 ]
B.
Kp =
[SO 2 ] ⋅ [O 2 ]
А.
Kp =
[SO3 ]2 ⋅ [O 2 ]
[SO 2 ]2
C.
Kp =
[SO 2 ]2
[SO3 ]2 ⋅ [O 2 ]
D.
А.
C.
D.
E.
Kp =
Kp =
B.
Kp
Kp
Kp
2
[SO3 ]
[SO 2 ]2 ⋅ [O 2 ]
E.
[H 2 ]
[H 2 O]
[FeO] ⋅ [H 2 ]
=
[Fe] ⋅ [H 2 O]
[H О]
= 2
[H 2 ]
[H 2 O] ⋅ [Fe]
=
[H 2 ] ⋅ [FeO]
[H 2 O]
=
[H 2 ] ⋅ [FeO]
Kp =
Kp
7.47. Expression of the equilibrium
constant for the reaction FeO(s) +
H2(g) ⇄ Fe(s) + H2O(g) ?
Chapter 8. The equilibrium in feebly soluble electrolytes
solutions
product constant Ksp?
А. log Ksp =–∆G/(2,303RT)
B. ∆G = - RTln Ksp
C. ∆G = RTln Ksp
D. ∆G = RTlog Ksp
E. log Ksp =∆G/(2,303RT)
8.1. The solubility of a slightly
dissolved salt AmBn, which
dissociate according to the scheme
AmBn ⇄ mAn+ + nBm– may be
calculated as:
А. (m+n) Ksp
S=
8.3. In which case the solution of
BaSO4 is over-saturated?
А. [Ba2+]⋅[SO42–] < Ksp
B. [Ba2+]⋅[SO42–] ≈ Ksp
C. [Ba2+]⋅[SO42–] > Ksp
D. [Ba] ⋅[SO4]= Ksp
E. [Ba2+]⋅[SO42–] = Ksp
mm ⋅ nn
B. S = K
sp
C.
S=
Ksp
m+n
D.
S= (m+n)
E.
S= (m⋅n)
Kp
m+n
8.4. In which case the solution of AgI
is saturated?
А. [Ag+]⋅[I–] > Ksp
B. [Ag+]⋅[I–] < Ksp
C. [Ag+]+[I–] < Ksp
Ksp
m⋅n
8.2. What is the relations between
Gibbs energy and the solubility
45
А. Ksp = 3[Ca2+]3· 2[PO43–]2
B. Ksp = [Ca2+]3 + [PO43–]2
C. Ksp = 3[Ca2+]3+2[PO43–]2
D. Ksp = ([Ca2+]3·[PO43–]2)/
[Ca3(PO4)2]
E. Ksp = [Ca2+]3·[PO43–]2
D. [Ag+]⋅[I–] = Ksp
E. [Ag+]⋅[I–]≈ Ksp
8.5. In which case the precipitate of
slightly dissolved salt will
form?(IP – ion product)
А. ІP ≈ Ksp
B. ІP< Ksp
C. D. ІP = Ksp
E. ІP> Ksp
8.10. Compare the values for Ksp next
salts HgS, PbS, CdS, SnS, TlS2
and choose one, which is the least
soluble in a water.
А. Ksp (TlS2) = 5·10–21
B. Ksp (PbS) = 2,5·10–27
C. Ksp (CdS) = 1,2·10–28
D. Ksp (HgS) = 4,0·10–53
E. Ksp (SnS) = 1,0·10–27
8.6. Solubility product constant Ksp
depends on:
А. B. molar concentration of ions
C. temperature
D. concentration of salt
E. presence of catalyst
8.11. Which ions can not be present
simultaneous (одночасно) in a
solution?
А. K+, NO3–
B. Cu2+, SO42–
C. NH4+, Cl–
D. Na+, SO42–
E. Fe2+, OH–
8.7. The solubility product constant
Ksp of a slightly dissolved salt
AmBn, which dissociate according
→
to the scheme AmBn ← mAn+ +
nBm– may be calculated as:
А.
a n + + a B mKsp = A
B. Ksp = [An+]m⋅[Bm–]n
C. Ksp = [An+]⋅[Bm–]
D. Ksp = [A]m⋅[В]n
E.
a n+ ⋅ aBmKsp = A
(
) (
8.12. Choose the pair of compound,
which ions can not be present
simultaneous in a solution:
А. AgNO3 and HCl
B. CuSO4 and BaCl2
C. NaOH and P2O5
D. Al(NO3)3 and HCl
E. Ba(OH)2 and CO2
)
8.8. The solubility of a slightly
dissolved salt is expressed by the:
А. percent of solubility
B. solubility product constant
C. coefficient of absorption
D. coefficient of solubility
E. dissociation constant
8.13. The expression of the solubility
product constant Ksp for
Mg(OH)2:
А. Ksp = [Mg2+]⋅[OH–]
B. Ksp = [Mg2+]⋅[OH–]2
C.
= aMg 2+ ⋅ a _
OH
Ksp
D. Ksp = 2[Mg2+]•2[OH–]
E. Ksp = [Mg2+]•2[OH–]
8.9. The expression of the solubility
product constant Ksp for Ca3
(PO4)2 is:
46
E.
8.14. The expression of the solubility
product constant Ksp for CaF2:
А. Ksp = [Ca2+] / [F–]2
B. Ksp = a(Ca2+) a(F–)
C. Ksp = [Ca2+] + [F–]
D. Ksp = [Ca2+][F–]2
E. Ksp = [Ca2+][2F–]
O2 ⇄ 2SO3 is:
А.
[SO 2 ]2
Kp =
B.
C.
2-
8.16. The solubility of Ag2S (in mol/L)
may be calculated according to
the equation:
А.
Ksp
S= 3
27
B.
Ksp
S= 3
4
C.
Ksp
S=
2
D. S= 3 4K
[SO3 ]2
[SO2 ]2 ⋅ [O 2 ]
Kp =
[SO 2 ]2 ⋅ [O 2 ]
[SO 3 ]2
Kp =
8.19. Point out, which of the given
reactions should be held at the
increased pressure according to Le
Chatelier's principle.
А. CO(gas) + Cl2(gas) =
COCl2(gas)
B. 3H2(gas) + N2(gas) =
2NH3(gas)
C. N2(gas) + O2(gas) = NO2(gas)
D. H2(gas) + Cl2(gas) =
2HCl(gas)
E. Fe + H2O(gas) = FeO +
H2(gas)
sp
E. S= K
sp
8.17. The solubility of Fe(OH)3 (in
mol/L) may be calculated
according to the equation:
А.
Ksp
S= 4
27
B. S= K
8.20. Which of the given statements is
true for the system in the
equilibrium state?
А. The rates of the direct and
reverse reactions are equal
B. permanent losses of free
Gibbs’ energy are needed
C. the reactants concentrations
are equal
D. the reactants masses do not
change
sp
S= 3
Kp =
[SO3 ]2 ⋅ [O 2 ]
[SO3 ]2 ⋅ [O 2 ]
[SO 2 ]2
[SO3 ]
E.
Kp =
[SO 2 ] ⋅ [O 2 ]
D.
4
C.
4
8.18. Expression of the equilibrium
constant for the reaction 2SO2 +
8.15. The expression of the solubility
product constant Ksp for Ag2CrO4:
А. Ksp = [Ag+]⋅[CrO42–]
B. Ksp = [Ag+]2⋅[CrO42–]
2
C.
(a ) ⋅ aCrO
Ksp = Аg
D. Ksp = [Ag+]+[Cr2O42–]
E. Ksp = 2[Ag+]•[CO42–]
+
Ksp
S= 3
Ksp
27
D. S= 3 4K
sp
47
E. the permanent exchange of the
substance and energy between
the system and surroundings
takes place
Chapter 9. Chemical equilibrium
D.
9.1. Select the true definition for the
equilibrium constant through the
given ones:
А. the product of the reaction
products equilibrium
concentrations raised to the
powers of their stoichiometric
coefficients
B. the product of the reactants
equilibrium concentrations
raised to the powers of their
stoichiometric coefficients
C. the rate constants of the
reverse and direct reactions
ratio
D. the rate constants of the direct
and reverse reactions ratio
E. the product of the reactants
concentrations changes
E.
[SO3 ]2 ⋅ [O 2 ]
[SO 2 ]2
[SO 2 ]2
K eq =
[SO3]2 ⋅ [O 2 ]
K eq =
9.3. Select the true mathematical
expression for the reaction
FeO(solid) + H2(gas) ⇄ Fe(solid)
+ H2O(gas) equilibrium constant.
А.
[FeO] ⋅ [H 2 ]
K eq =
[Fe] ⋅ [H 2 O]
B. K = [H 2 O]
eq
9.2. Select the true mathematical
expression for the reaction 2SO2 +
O2 ⇄ 2SO3 equilibrium constant.
А.
[SO3 ]2
K eq =
[SO 2 ]2 ⋅ [O 2 ]
B.
[SO 3 ]
K eq =
[SO 2 ] ⋅ [O 2 ]
C.
[SO 2 ]2 ⋅ [O 2 ]
K eq =
[SO3 ]2
[H 2 ] ⋅ [FeO]
C.
K eq =
D.
K eq =
E.
K eq =
[H 2 O]
[H 2 ]
[H 2 ]
[H 2O]
[H 2 O] ⋅ [Fe]
[H 2 ] ⋅ [FeO]
9.4. Methanol synthesis according to
the equation of the reaction CO(g)
+ 2H2(g) ⇄ CH3OH(l) is the
exothermal process. What
variables and conditions should be
changed for the product yield
increasing?
А. temperature increasing,
pressure increasing
48
B. temperature increasing,
methanol concentration
increasing
C. temperature decreasing,
withdrawal of CO from the
reaction area
D. temperature increasing,
withdrawal of hydrogen from
the reaction area
E. temperature decreasing,
withdrawal of methanol from
the reaction area
C. temperature decreasing,
nitrogen and hydrogen
concentrations increasing
D. the reacting mixture volume
increasing, applying of a
catalyst
E. applying of a catalyst,
temperature increasing
9.7. For which of the reactions given
below the temperature and
pressure increasing will shift the
equilibrium toward the products
formation:
9.5. What variables and conditions
should be changed for the product
SО3 yield increasing according to
the reaction chemical equation
1. N2(gas) + 3H2(gas) ⇄
2NH3(gas) Q;
2. C(solid) + O2(gas) ⇄ CO2(gas)
+ Q;
SO2 + 1/2O2 ⇄ SO3 ; ∆H°298 = –
98.9 kJ/mol?
А. temperature increasing, the
reacting mixture volume
decreasing
B. temperature increasing, the
reacting mixture volume
increasing
C. temperature decreasing,
oxygen concentration
decreasing
D. temperature increasing,
pressure decreasing
E. temperature decreasing,
pressure increasing
3. N2O4(liquid) ⇄ 2NO2(gas) –
Q?
А. 1
B. 2,3
C. для всіх наведених реакцій
D. 1, 3
E. 2
9.8. The system state which does not
change in time under the
unchangeable variables and
conditions, is called:
А. equilibrium
B. non-equilibrium
C. isobaric
D. stationary
E. isothermal
9.6. What variables and conditions
should be changed for the
ammonium yield increasing
according to the reaction chemical
9.9. For which of the given processes
the temperature decreasing will
cause the reaction rate increasing?
А. endothermal
B. exothermal
C. isochoric
D. adiabatic
equation N2 + 3H2 ⇄ 2NH3 ;
∆H°298 = –92.4 kJ/mol?
А. temperature decreasing,
ammonium concentration
increasing
B. temperature increasing,
pressure decreasing
49
E. isobaric
9.14. Will the equilibrium be shifted in
the given reacting system under
the temperature decreasing: N2 +
9.10. For which of the given reacting
systems the pressure increasing
will cause the equilibrium shifting
towards direct reaction?
А. H (g) + I (g) ⇄ 2HI(g)
2
3Н2 ⇄ 2NН3 + Q?
А. –
B. will shift right
C. will not be shifted
D. will shift left
E. –
2
B. COCl (g) ⇄ CO(g) + Cl (g)
2
2
C. NH Cl(s) ⇄ HCl(g) + NH (g)
4
3
D. CO (g) + H (g) ⇄ CO(g) +
2
2
H2O(g)
E. 2NO(g) + O (g) ⇄ 2NO (g)
2
9.15. Will the equilibrium be shifted in
the given reacting system under
the temperature decreasing:
2
СОCl2 ⇄ CO + Cl2 – Q?
А. will shift left
B. will not be shifted
C. –
D. will shift right
E. –
9.11. For which of the given processes
the temperature increasing will
cause the product yield
increasing?
А. isobaric
B. endothermal
C. adiabatic
D. isochoric
E. exothermal
9.16. Will the equilibrium be shifted in
the given reacting system under
the hydrogen concentration
9.12. Will the equilibrium be shifted in
the given reacting system under
the temperature increasing: 2NO +
increasing: Н2 + S ⇄ Н2S?
А. –
B. will shift right
C. will not be shifted
D. will shift left
E. –
O2 ⇄ 2NO2 + Q?
А. –
B. will shift left
C. –
D. will shift right
E. will not be shifted
9.17. Will the equilibrium be shifted in
the given reacting system under
the hydrogen concentration
9.13. Will the equilibrium be shifted in
the given reacting system under
the temperature increasing: N2O4
increasing: Н2 + Cl2 ⇄ 2НCl?
А. –
B. will not be shifted
C. –
D. will shift right
E. will shift left
⇄ 2NO2 – Q?
А. –
B. –
C. will shift left
D. will not be shifted
E. will shift right
9.18. Will the equilibrium be shifted in
the given reacting system under
the pressure increasing: Н2 + І2 ⇄
50
2НІ?
А. will shift left
B. –
C. –
D. will shift right
E. will not be shifted
D. will shift left
E. –
9.23. Will the equilibrium be shifted in
the given reacting system under
the oxygen concentration
decreasing: 3О2 ⇄ 2О3 + Q?
А. –
B. will shift left
C. –
D. will shift right
E. will not be shifted
9.19. Will the equilibrium be shifted in
the given reacting system under
the pressure increasing: 2NO2 ⇄
2NO + O2?
А. –
B. will not be shifted
C. –
D. will shift left
E. will shift right
9.24. Will the equilibrium be shifted in
the given reacting system under
the temperature increasing: NH3 +
H2O ⇄ NH4OH + Q?
А. will not be shifted
B. –
C. –
D. will shift left
E. will shift right
9.20. Will the equilibrium be shifted in
the given reacting system under
the pressure increasing: N2 + 3H2
⇄ 2NH3?
А. will shift left
B. –
C. will shift right
D. will not be shifted
E. –
9.25. Will the equilibrium be shifted in
the given reacting system under
the pressure decreasing: NH3 +
H2O ⇄ NH4OH + Q?
А. will not be shifted
B. will shift right
C. –
D. –
E. will shift left
9.21. Will the equilibrium be shifted in
the given reacting system under
the temperature increasing: 3О2 ⇄
2О3 + Q?
А. –
B. –
C. will shift right
D. will not be shifted
E. will shift left
9.26. Will the equilibrium be shifted in
the given reacting system under
the ammonium concentration
increasing: NH3 + H2O ⇄ NH4OH
+ Q?
А. –
B. will shift right
C. will shift left
D. will not be shifted
E. –
9.22. Will the equilibrium be shifted in
the given reacting system under
the oxygen concentration
increasing: 3О2 ⇄ 2О3 + Q?
А. will shift right
B. will not be shifted
C. –
51
the equilibrium shifting right for
the following reversible reaction
9.27. What variable change will cause
the product yield increasing for
the ethane hydration reaction:
N2O4(г)⇄2 NO2(г), ∆H > 0
А. the reactant concentration
decreasing
B. the reaction product
concentration increasing
C. temperature increasing and
pressure decreasing
D. temperature increasing and
pressure increasing
E. temperature decreasing and
pressure increasing
С2Н4(g) + Н2⇄С2Н6(g)
А. Н2 concentration decreasing
B. reacting system volume
increasing
C. pressure decreasing
D. pressure increasing
E. С2Н4 concentration decreasing
9.28. What variable change will cause
the equilibrium shifting left for
the following reversible reaction
9.31. Chemical reactions which may
occur in direct and reverse
directions are called:
А. catalytical
B. kinetical
C. thermochemical
D. non-reversible
E. reversible
СО(g) + Н2О(g)⇄ СО2(g)+ Н2(g),
∆H < 0
А. temperature decreasing
B. pressure increasing
C. temperature increasing and
pressure increasing
D. temperature increasing
E. reacting system volume
change
9.32. What variable change will cause
the equilibrium shifting right for
the following reversible reaction
9.29. What variable change will cause
the equilibrium shifting right for
the following reversible reaction
N2(g)+ О2(g)⇄2NО(g), ∆H > 0
А. temperature decreasing
B. temperature increasing, the
reaction product concentration
decreasing
C. nitrogen concentration
decreasing
D. pressure increasing
E. oxygen concentration
decreasing
N2⇄2N, ∆H > 0
А. pressure increasing
B. temperature increasing and
pressure decreasing
C. temperature decreasing
D. the reactant concentration
decreasing
E. temperature decreasing and
pressure increasing
9.30. What variable change will cause
52
Chapter 10. The concept of strong and weak electrolytes
10.1. Concentration of hydrogen-ion
in a pure water is:
А. 10–7
B. 10–10
C. 10–3
D. 10–14
E. 10–1
HNO3, NH4Cl, NH4OH,
CH3COOH, CH3COON are
weak ones:
А. NH4Cl, NH4OH
B. CH3COOH, CH3COONa
C. AgCl, NH4Cl
D. NH4OH, CH3COOH
E. HCl, AgCl
10.2. 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-]=10-14mol/L
C. [H+] =[ОН-]=10-14mol/L
D. [H+]/[ОН-]=10-7mol/L
E. [H+]=[ОН-]=10-7mol/L
10.7. Which pair of ions cannot be
found in a neutral solution?
А. K+ and OH–
B. Ca2+ and HCO–
C. Na+ and SO42–
D. H+ and CO32–
E. Ag+ and NO3–
10.3. What is the concentration of [H+]
in pure water at 25 ºС
А. 10-1
B. 107
C. 10-14
D. 10-7
E. 1014
10.8. Choose the pair of electrolytes,
which do not react in an aqueous
solution?
А. Fe(NO3)3 and NaOH
B. NaBr and KOH
C. K2CO3 and H2SO4
D. MgSO4 and (NH4)3PO4
E. Na2S and HCl
10.4. What is the concentration of
[OH-] in pure water at 25 ºС
А. 10-7
B. 107
C. 1014
D. 10-14
E. 10-1
10.9. Which reaction of the given ones
is impossible:
А. KCl + Br2 → KBr + Cl2.
B. KI + Br2 → KBr + I2
C. NaI + Cl2 → NaCl + I2
D. KCl + І2 → KІ + Cl2
E. NaBr+ Cl2 → NaCl + Br2
10.5. Which of the following is the
stronger acid?
А. HClO2
B. HClO
C. HClO3
D. HClO4
E. chlorous acid
10.10. Which base is weak electrolyte?
А. NaOH
B. Ca(OH)2
C. Mg(OH)2
D. Ba(OH)2
E. KOH
10.6. Which electrolytes HCl, AgCl,
10.11. Which acid is weak electrolyte?
А. HCl
53
B.
C.
D.
E.
H2SO4
HBr
H3BO3
HNO3
C. 5
D. 2
E. 3
10.16. Which particle of the given ones
is an anion?
А. Ca2+
B. K+
C. Fe3
D. NO3E. Na+
10.12. Mistaken statement, that concern
to iron (III) hydroxide: Fe(OH)3
– it is …
А. strong electrolyte
B. amphoteric hydroxide
C. weak base
D. insoluble in a water
E. brown color of compound
10.17. Which compounds form ions of
Mn2+ at the dissociation?
А. MnCl2
B. MnO2
C. KMnO4
D. Na2MnO4
E. H2MnO4
10.13. Which one of the given
molecular equation corresponds
to the short ionic equation Сu2+ +
S2– = CuS?
А. CuCO3 + H2S = CuS + CO2 +
H2O
B. Cu(OH)2 + Na2S = CuS +
2NaOH
C. Cu3(PO4)2 + 3(NH4)2S =
3CuS + 2(NH4)3PO4
D. CuBr2 + K2S = CuS + 2KBr
E. CuCl2 + H2S = CuS + 2HCl
10.18. How many ions are forming at
the dissociation of FeCl3?
А. 10
B. 5
C. 6
D. 4
E. 4
10.14. Point out the row in which pH of
compounds with the same molar
concentration decrease:
А. HCl, H2SO4, NH3,
CH3COOH, NaOH
B. CH3COOH, HCl, NaOH,
NH3, H2SO4
C. NaOH, NH3, CH3COOH,
HCl, H2SO4
D. H2SO4, HCl, NaOH,
CH3COOH, NH3
E. NH3, CH3COOH, NaOH,
HCl, H2SO4
10.19. Which of the following
dissociation constant values of
polyprotic acid is always larger?
А. last
B. first
C. second
D. the same
E. third
10.20. Percent of dissociation NH4OH
increase with:
А. adding salt of ammonium
B. concentrating of solution
C. adding base
D. dilution of solution
E. cooling
10.15. How many ions are forming at
the dissociation of (NH4)2SO4?
А. 6
B. 4
10.21. Point out an aqueous solution
54
which has the worst electrical
conductivity? Molarities of
solutions are equal.
А. HCN
B. KCN
C. KOH
D. H2SO4
E. K2SO4
А.
B.
C.
D.
E.
10–7
10–3
10–9
10–5
10–11
10.27. pH equal zero in a solution of:
А. 1M HCl
B. 0.1M KOH
C. 1M Ba(OH)2
D. 1M H2SO4
E. 0.1M HCl
10.22. Percent of dissociation of weak
electrolytes increase with:
А. increasing of concentration
B. decreasing of acidity
C. cooling
D. increasing of acidity
E. heating
10.28. Units of measurement of
hydrogen-ion concentration in
equation pH = -lg[H+] are:
А. mol/cm3
B. mol/mL
C. mol/L
D. mol
E. mol/кg
10.23. 0,1 М solution of which
compound has the smallest
concentration of ions?
А. НCl
B. H2SO4
C. NaNO3
D. СаCl2
E. СН3СООН
10.29. 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
10.24. 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
10.30. Which of the following pH
values indicate an acidic solution
at 25 ºС?
А. 9,5
B. 1,2
C. 11,2
D. 10
E. 7,4
10.25. pH of 0,001 М solution of HCl
equal:
А. 0
B. 5
C. 7
D. 10
E. 3
10.31. Which of the following pH
values indicate a basic solution
at 25 ºС?
А. 4,5
B. 7,3
C. 1,2
10.26. What is the concentration of
hydroxide-ion in a solution, if
рОН of its equal 9?
55
D. 4
E. 5,5
the stomach):
А. 0,5 – 1,5
B. 0,9– 2,0
C. 1,5 – 3,0
D. 1,5 – 2,5
E. 2,5 – 3,5
10.32. 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
10.36. pH of the blood plasma is:
А. 6,80 – 7,0
B. 7,35 – 7,45
C. 7,15 – 7,35
D. 8,01 – 8,25
E. 7,65 – 7,85
10.33. 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
10.37. What is the рН values range of
the urine?
А. 8,5 – 10,5
B. 2,0 – 3,5
C. 2,5 – 3,5
D. 7,5 – 9,5
E. 5,0 – 6,5
10.34. Which of the following pH
values indicate a neutral solution
at 25ºС?
А. 9,5
B. 5
C. 7
D. 2,5
E. 13
10.38. Concentration of hydrogen-ion
in a pure water is:
А. 10–10
B. 10–1
C. 10–14
D. 10–3
E. 10–7
10.35. What is the pH of a sample of
gastric juice (digestive juice in
Chapter 11. Acids and bases theories. Self-ionization of
water. pH
E. рН = 7, рОН = 7
11.1. 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
11.2. pH of 0,001 М solution of HCl
equal:
А. 10
B. 5
C. 0
56
D. 3
E. 7
values indicate a basic solution
at 25 ºС?
А. 4
B. 4,5
C. 7,3
D. 1,2
E. 5,5
11.3. What is the concentration of
hydroxide-ion in a solution, if
рОН of its equal 9?
А. 10–7
B. 10–3
C. 10–9
D. 10–5
E. 10–11
11.9. 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
11.4. pH equal zero in a solution of:
А. 0.1M HCl
B. 1M H2SO4
C. 1M HCl
D. 1M Ba(OH)2
E. 0.1M KOH
11.10. 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
11.5. Units of measurement of
hydrogen-ion concentration in
equation pH = -lg[H+] are:
А. mol/кg
B. mol/cm3
C. mol
D. mol/L
E. mol/mL
11.11. Which of the following pH
values indicate a neutral solution
at 25ºС?
А. 13
B. 9,5
C. 7
D. 5
E. 2,5
11.6. 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
11.12. What is the pH of a sample of
gastric juice (digestive juice in
the stomach):
А. 1,5 – 2,5
B. 1,5 – 3,0
C. 2,5 – 3,5
D. 0,9– 2,0
E. 0,5 – 1,5
11.7. Which of the following pH
values indicate an acidic solution
at 25 ºС?
А. 9,5
B. 10
C. 1,2
D. 7,4
E. 11,2
11.13. pH of the blood plasma is:
А. 6,80 – 7,0
B. 8,01 – 8,25
11.8. Which of the following pH
57
C. 7,35 – 7,45
D. 7,15 – 7,35
E. 7,65 – 7,85
Lowry concept of acids and
bases, an base is the species
which:
А. accepts the electron
B. C. donates the electron
D. accepts the proton
E. donates the proton
11.14. What is the рН values range of
the urine?
А. 2,5 – 3,5
B. 8,5 – 10,5
C. 7,5 – 9,5
D. 2,0 – 3,5
E. 5,0 – 6,5
11.19. Which of the given compounds
do not belong to Lewis acid?
А. AlCl3
B. С5H5N
C. ZnCl2
D. FeCl3
E. no one through the listed
compounds
11.15. Concentration of hydrogen-ion
in a pure water is:
А. 10–7
B. 10–10
C. 10–14
D. 10–3
E. 10–1
11.20. In acid-base reaction molecules
of solvent:
А. B. transfer electron from
reducing agent to oxidizing
agent
C. transfer proton from acid to
base
D. transfer electron from
oxidizing agent to reducing
agent
E. transfer proton from base to
acid
11.16. According to the Bronsted-lowry
concept of acids and bases
amphoteric properties have the
next electrolites:
А. HClO, H2S, CH3NO2
B. HS-, NO2-, HSO4C. H2O, HCO3-,HPO42D. NH3, H3O+, HPO4E. H2O, HI, H3O+
11.17. According to the BronstedLowry concept of acids and
bases, an acid is the species
which:
А. accepts the proton
B. donates a proton
C. molecule contains a
hydrogen-ion
D. donates the electron
E. has a free electron pair
11.21. Which of the given species is a
Lewis base?
А. CO2
B. Ca2+
C. F–
D. CH4
E. H+
11.18. According to the Bronsted-
58
Chapter 12. Protolytic processes
А. transfer electron from
reducing agent to oxidizing
agent
B. transfer electron from
oxidizing agent to reducing
agent
C. D. transfer proton from base to
acid
E. transfer proton from acid to
base
12.1. According to the Bronsted-lowry
concept of acids and bases
amphoteric properties have the
next electrolites:
А. H2O, HCO3-,HPO42B. HClO, H2S, CH3NO2
C. H2O, HI, H3O+
D. HS-, NO2-, HSO4E. NH3, H3O+, HPO412.2. According to the BronstedLowry concept of acids and
bases, an acid is the species
which:
А. donates the electron
B. has a free electron pair
C. accepts the proton
D. molecule contains a
hydrogen-ion
E. donates a proton
12.6. Which of the given species is a
Lewis base?
А. H+
B. F–
C. CO2
D. CH4
E. Ca2+
12.7. Which of the given species is a
Lewis acid?
А. BF3
B. NH3
C. SO42–
D. CN–
E. Cl–
12.3. According to the BronstedLowry concept of acids and
bases, an base is the species
which:
А. accepts the proton
B. donates the electron
C. D. donates the proton
E. accepts the electron
12.8. Which one of the aqueous
solution of the given salts has an
acidic pH?
А. K2SO3
B. ZnSO4
C. Na3PO4
D. Na2B4O7
E. NaCl
12.4. Which of the given compounds
do not belong to Lewis acid?
А. ZnCl2
B. С5H5N
C. FeCl3
D. AlCl3
E. no one through the listed
compounds
12.9. Which one of the given salts
cannot exist in an aqueous
solution?
А. FeCl3
B. K3PO4
12.5. In acid-base reaction molecules
of solvent:
59
C. NH4Cl
D. NaNO3
E. Cr2S3
А.
B.
C.
D.
E.
12.10. Color of litmus in a solution of
iron (ІІІ) nitrate is:
А. red
B. pink
C. violet
D. blue
E. colorless
NaI
Fe(NO3)3
BaCl2
K3PO4
K2CO3
12.16. Color of methyl orange in a
solution of zinc sulfate is:
А. yellow
B. pink
C. blue
D. colorless
E. orange
12.11. Select the salt, which does not
hydrolyze:
А. Al2(SO4)3
B. CrCl3
C. KNO2
D. KI
E. FeSO4
12.17. Color of methyl orange in a
solution of K2CO3 is:
А. orange
B. yellow
C. red
D. pink
E. blue
12.12. Point out the salt which
hydrolyze particularly:
А. NaBr
B. K2S
C. Ca(NO3)2
D. BaSO4
E. Al2S3
12.18. Color of methyl orange in a
solution of AlCl3 is:
А. colorless
B. yellow
C. purple
D. blue
E. pink
12.13. Point out the salt which
hydrolyze to the end:
А. Al2(SO4)3
B. Na3PO4
C. Cr(NO3)3
D. Cr2S3
E. KNO3
12.19. Color of phenolphthalein in a
solution of Na3PO4 is:
А. colorless
B. blue
C. pink
D. red
E. orange
12.14. Which one of the given salts has
a basic solution?
А. Cr2(SO4)3
B. KCl
C. NaNO3
D. AlCl3
E. Na2CO3
12.20. Color of methyl red in a solution
of Cr2(SO4)3 is:
А. yellow
B. orange
C. red
D. blue
E. colorless
12.15. Which one of the given salts has
an acidic solution?
60
E. NH4Br
12.21. Select the salt, which do not
hydrolyze:
А. AlCl3
B. Ba(NO3)2
C. KNO2
D. ZnCl2
E. K2HPO4
12.26. Select the salt which increases
the hydrogen-ion concentration,
when dissolved in water?
А. Na2CO3
B. K2SO4
C. ZnCl2
D. NaCl
E. K3PO4
12.22. Point out the salt which can form
as a product of hydrolysis a basic
salt.
А. KNO2
B. BaI2
C. AlCl3
D. Na2CO3
E. AgNO3
12.27. Select the salt, which do not
hydrolyze:
А. K2SO4
B. AlBr3
C. MnCl2
D. K2SO3
E. CuSO4
12.23. 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; 5
C. рН>7; 4
D. рН<7; 4
E. рН>7; 6
12.28. Point out the salt which
hydrolyze in one step
completely:
А. Cr2S3
B. AlCl3
C. CuS
D. no one through the listed
salts
E. Na2S
12.29. Which one from the given salts
has a basic solution?
А. Na2S
B. CuCl2
C. FeCl3
D. KCl
E. Na2SO4
12.24. Which one of the given salts
forms as a product of hydrolysis
a basic salt?
А. Cr2(SO4)3
B. Na2SO4
C. AgNO3
D. CaCO3
E. K2CO3
12.30. What is the product of reaction
between H2O and PCl5?
А. HCl + H3PO3
B. HCl + H3PO4
C. Cl2 + H3PO4
D. P2O3 + HCl
E. P2O5 + HCl
12.25. Which one of the given salts
forms a neutral solution?
А. NH4Cl
B. NH4NO3
C. (NH4)2SO4
D. CH3COONH4
12.31. Select the salt, which hydrolyze
61
in an aqueous solution:
А. KI
B. LiBr
C. NaCl
D. KI
E. NaF
12.36. Point out the salt which
hydrolyze to the end:
А. CuSO4
B. Zn(NO3)2
C. K2S
D. Na2CO3
E. Аl2S3
12.32. Which one of the given salts
reacts with an acid and forms as
a product of reaction a gas?
А. Na2CO3
B. CuSO4
C. Na2SiO3
D. K2SO4
E. Ca3(PO4)2
12.37. Which ions can be at the same
time in a solution?
А. Fe3+, OH–
B. Fe3+ , Cl–
C. Ba2+, SO42–
D. Fe2+, OH–
E. Ag+, Cl–
12.33. Some medicine can destroy in
acidic medium. Which one of the
given salt is incompatible with
the medicine in an aqueous
solution?
А. NaHCO3
B. K3PO4
C. KI
D. ZnSO4
E. NaCl
12.38. The expression of the constant of
hydrolysis Кh = Кw/Kb is for a
salt of:
А. CH3COONa
B. CuSO4
C. (NH4)2S
D. KCN
E. NaCl
12.39. The expression of the constant of
hydrolysis Кh = Кw/(Ка · Kb) is
for a salt of:
А. (NH4)2S
B. NH4Cl
C. Li2S
D. NaCN
E. Fe(NO3)3
12.34. Some antibiotics can destroy in
acidic medium. Which one of the
given salt is incompatible with
the antibiotics in an aqueous
solution?
А. Na3PO4
B. CaCl2
C. NH4Cl
D. Na2CO3
E. KI
12.40. The expression of the constant of
hydrolysis Кh = Kw/(Ka· Kb) is for
a salt of:
А. CH3COONa
B. NH4Cl
C. К3PO4
D. CH3COONH4
E. FeCl3
12.35. Select the salt, which hydrolyze
in an aqueous solution:
А. Sr(NO3)2
B. KNO3
C. NaNO3
D. Ba(NO3)2
E. NH4NO3
12.41. The expression of the constant of
hydrolysis Кh = Кw/Kb is for a
62
salt of:
А. Na2CO3
B. K2SO4
C. K3PO4
D. NH4Cl
E. LiNO3
А.
B.
C.
D.
E.
H2O
H2SO4
BaSO4
KOH
Na2CO3
12.44. The direction of protolytical
reaction СН3СООН + С6Н5ОNa
→
← C6H5OH + CH3COONa is
shifted:
А. reaction is impossible
B. dynamic equilibrium
C. forward
D. E. reverse
12.42. The expression of the constant of
hydrolysis Кh = Кw/Ka is for a
salt of:
А. NaCN
B. (NH4)3PO4
C. Na2SO4
D. CH3COONH4
E. (NH4)2SO4
12.43. Percent of hydrolysis of CuSO4
decrease with adding solution of:
Chapter 13. Reactions with electrons transferring
reaction with an iron sulfate in
acidic medium find out
properties of:
А. B. oxidizing agent
C. does not show the redox
properties
D. oxidizing agent and reducing
agent
E. reducing agent
13.1. How will change the redox
properties in a row: Cl– – Br– – I–
А. does not change
B. C. increased
D. decreases
E. a bromine is a stronger
reduction agent, than chlorine
13.2. What is the oxidation number of
a molybdenum in the compound
(NH4)6Mo7O24 ?
А. +3
B. +2
C. +5
D. +1
E. +6
13.4. Mercury has the oxidation
number +2 in the following
compound?
А. Hg2SO4
B. Hg2(NO3)2•2H2O
C. Hg2O
D. Hg2Cl2
E. K2[HgI4]
13.3. Potassium permanganate in a
63
+ H2O
13.5. What is the oxidation number of
a Arsenic in the compound
AsH3?
А. +3
B. –3
C. +5
D. –5
E. +1
13.9. What is the oxidation state of the
central ion in the coordination
compound [Cr(H2O)4Cl2]Cl.
А. +4
B. 0
C. +2
D. +3
E. +6
13.6. Nitrogen(ІІ) oxide has redox
properties. What properties it
finds out in the reaction NO+
KMnO4 + H2SO4 → ?
А. B. oxidizing properties
C. oxidizing and reducing
properties
D. does not change the oxidation
number
E. reducing properties
13.10. How many electrons gains the
potassium dichromate.K2Cr2O7.
What is the oxidation number of
a Chromium when it reduced in
the acidic medium?
А. 3, +3
B. 3, +4
C. 8, +2
D. 6, +3
E. 4, +2
13.7. Which reaction through the listed
ones correspondsto the
intermolecular oxidationreduction reaction.
А. HCl + CrO3 = CrCl3 + Cl2 +
H2O
B. Cl2 + H2O = HCl + HClO
C. 2CuCl +Cl2 = 2CuCl2
D. KMnO4 + HCl = MnCl2 + Cl2
+ KCl + H2O
E. Au2O3 = Au + O2
13.11. Which compound through the
listed ones has both oxidizing
and reducing properties?
А. CrO3
B. PbO2
C. CO2
D. SO3
E. SO2
13.12. Which equation through the
listed ones corresponds to the
disproportionation?
А. I2O5 + H2O = 2HIO3
B. Cl2O7 + H2O = 2HClO4
C. Cl2O + H2O = 2HClO
D. Br2O + H2O = 2HBrO
E. ClO2 + H2O = HClO2 +
HClO3
13.8. Which reaction through the listed
ones correspondsto the
disproportionation oxidationreduction reaction.
А. Au2O3 → Au + O2
B. MnO2 + HCl → MnCl2 + Cl2
+ H2O
C. S + KOH → K2SO3 + K2S +
H2O
D. FeCl2 + Cl2 → FeCl3
E. HCl + Cr2O3 → CrCl3 + Cl2
13.13. Which compound through the
listed ones has both oxidizing
and reducing properties? :
А. NO2
64
B. N2O5
C. NH3
D. HNO3
E. NH4Cl
13.18. Which reaction through the listed
ones is impossible:
А. NaI + Cl2 → NaCl + I2
B. KCl + І2 → KІ + Cl2
C. NaBr+ Cl2 → NaCl + Br2
D. KCl + Br2 → KBr + Cl2
E. KI + Br2 → KBr + I2
13.14. Which equation through the
given ones corresponds to the the
reaction of disproportionation?
А. MnO2 + HCl → MnCl2 + Cl2
+ H2O
B. FeCl2 + Cl2 → FeCl3
C. S + KOH → K2SO3 + K2S +
H2O
D. Au2O3 → Au + O2
E. HCl + Cr2O3 → CrCl3 + Cl2
+ H2O
13.19. In which of the given
compounds iron can show
reducing properties only?
А. Fe2O3
B. FeCl2
C. K2FeO4
D. Fe
E. FeCl3
13.15. NaNO2 has reducing properties
when rescts with:
А. KMnO4
B. NaHCO3
C. KI
D. NH3
E. H2S
13.20. In which of the given
compounds iron can show
oxidizing properties only?
А. FeCl2
B. Fe2O3
C. K2FeO4
D. Fe
E. FeCl3
13.16. What is the oxidation state of the
central ion in the coordination
compound Na2[Fe(CN)5NO] ?
А. +1
B. +3
C. +6
D. 0
E. +2
13.21. In which of the given
compounds iron can show both
oxidizing and reducing
properties? 1. K2FeO4 2. Fe 3.
FeCl2 4. FeCl3 5. Fe2O3 Give an
answer as the sum of numbers of
these compounds.
А. 12
B. 10
C. 9
D. 11
E. 13
13.17. The transformation Cr+3 →
CrO42– is:
А. the process of oxidation in
basic solution
B. the process of reduction in
acidic solution
C. the process of reduction in
basic solution
D. E. the process of oxidation in
acidic solution
13.22. In which of the given
compounds iron can show both
oxidizing and reducing
properties? 1. K2FeO4 2. Fe 3.
FeO 4. FeCl3 5. Fe2O3 Give an
65
answer as the sum of numbers of
these compounds.
А. 13
B. 10
C. 9
D. 11
E. 12
C. CrCl3
D. K2CrO4
E. Cr
13.27. In which of the given
compounds Chromium can show
oxidizing properties only?
А. CrCl2
B. K2CrO4
C. Cr2O3
D. CrCl3
E. Cr
13.23. In which of the given
compounds Manganese can
show reducing properties only?
А. Mn
B. K2MnO4
C. KMnO4
D. Mn2O7
E. MnO2
13.28. In which of the given
compounds Chromium can show
oxidizing properties only?
А. Cr2O3
B. CrCl3
C. K2Cr2O7
D. Cr
E. CrCl2
13.24. In which of the given
compounds Manganese can
show oxidizing properties only?
А. K2MnO4
B. MnO2
C. Mn
D. Mn2O3
E. KMnO4
13.29. In which from the stated below
matters Chromium can show
oxidizing properties only?
А. Cr2O3
B. Cr
C. CrO
D. CrCl3
E. CrO6
13.25. In which of the given
compounds Manganese can
show both oxidizing and
reducing properties? 1. KMnO4
2. K2MnO4 3. Mn 4. MnO2 5.
Mn2O7 Give an answer as the
sum of numbers of these
compounds.
А. 6
B. 4
C. 7
D. 8
E. 5
13.30. In which of the given
compounds Chromium can show
both oxidizing and reducing
properties? 1. K2CrO4 2. CrCl3 3.
Cr 4. Cr2O3 5. CrO Give an
answer as the sum of numbers of
these compounds.
А. 9
B. 10
C. 8
D. 11
E. 7
13.26. In which of the given
compounds Chromium can show
reducing properties only?
А. CrCl2
B. K2Cr2O7
13.31. In which of the given
66
compounds Chromium can show
both oxidizing and reducing
properties? 1. K2CrO4 2. CrCl3 3.
Cr 4. K2Cr2O7 5. CrO Give an
answer as the sum of numbers of
these compounds.
А. 8
B. 10
C. 11
D. 9
E. 7
oxidizing properties only?
А. CoSO4
B. CoCl2
C. [Co(NH3)6]Cl3
D. CoO
E. Co
13.36. In which of the given
compounds Cobalt can show
both oxidizing and reducing
properties? 1. CoO 2. CoCl3 3.
Co 4. [Co(NH3)6]Cl3 5. CoCl2
Give an answer as the sum of
numbers of these compounds.
А. 7
B. 9
C. 4
D. 5
E. 6
13.32. In which of the given
compounds Chromium can show
both oxidizing and reducing
properties? 1. CrO3 2. CrCl3 3.
Cr 4. K2Cr2O7 5. CrCl2 Give an
answer as the sum of numbers of
these compounds.
А. 11
B. 7
C. 9
D. 10
E. 8
13.37. In which of the given
compounds Cobalt can show
both oxidizing and reducing
properties? 1. CoO 2. CoCl3 3.
Co 4. [Co(NH3)6]Cl3 5. CoSO4
Give an answer as the sum of
numbers of these compounds.
А. 6
B. 7
C. 5
D. 9
E. 4
13.33. In which of the given
compounds Cobalt can show
reducing properties only?
А. CoCl3
B. [Co(NH3)6]Cl3
C. CoO
D. Co
E. CoCl2
13.38. In which of the given
compounds Copper can show
reducing properties only?
А. CuO
B. CuCl2
C. Cu2O
D. CuCl
E. Cu
13.34. In which of the given
compounds Cobalt can show
oxidizing properties only?
А. Co
B. CoO
C. CoCl2
D. CoSO4
E. CoCl3
13.39. In which of the given
compounds Copper can show
oxidizing properties only?
13.35. In which of the given
compounds Cobalt can show
67
А. CuCl2
B. CuCl
C. Cu
D. Cu2O
E. K[Cu(CN)2]
D. 3
E. 1
13.44. What is the number of electrons,
losted or gained according with
the transformation: NO→ NO2.
А. 2
B. 5
C. 1
D. 3
E. 4
13.40. In which of the given
compounds Copper can show
both oxidizing and reducing
properties? 1. K[Cu(CN)2] 2.
CuCl2 3. Cu 4. [Co(NH3)6]Cl3 5.
CuCl Give an answer the sum of
numbers of these matters.
А. 6
B. 7
C. 5
D. 4
E. 8
13.45. What is the number of electrons,
losted or gained according with
the transformation: MgO→ Mg0
.
А. 1
B. 2
C. 5
D. 4
E. 3
13.41. What is the number of electrons,
losted or gained according with
the transformation: HNO3 →
NO2.
А. 3
B. 4
C. 2
D. 5
E. 1
13.46. What is the number of electrons,
losted or gained according with
the transformation: HNO3 →
NO.
А. 5
B. 3
C. 1
D. 2
E. 4
13.42. What is the number of electrons,
losted or gained according with
the transformation: H2SO3 →
H2SO4 .
А. 4
B. 1
C. 2
D. 5
E. 3
13.47. What is the number of electrons,
losted or gained according with
the transformation: N2 → NO.
А. 5
B. 1
C. 4
D. 3
E. 2
13.43. What is the number of electrons,
losted or gained according with
the transformation: S0 → H2S.
А. 4
B. 5
C. 2
13.48. What is the number of electrons,
losted or gained according with
the transformation: O2 → CuO.
А. 1
68
B. 4
C. 2
D. 5
E. 3
13.53. What is the number of electrons,
losted or gained according with
the transformation: HNO3 →
NH4Cl.
А. 7
B. 6
C. 9
D. 8
E. 5
13.49. What is the number of electrons,
losted or gained according with
the transformation: H2SO4 → S0.
А. 4
B. 7
C. 5
D. 8
E. 6
13.54. What is the number of electrons,
losted or gained according with
the transformation: HNO3 →
NH3.
А. 5
B. 7
C. 8
D. 6
E. 9
13.50. What is the number of electrons,
losted or gained according with
the transformation: S0 → H2SO4
.
А. 8
B. 6
C. 5
D. 4
E. 7
13.55. What is the number of electrons,
losted or gained according with
the transformation: HNO3 →
N2O
А. 8
B. 6
C. 4
D. 5
E. 7
13.51. What is the number of electrons,
losted or gained according with
the transformation: H2S → SO2 .
А. 7
B. 4
C. 5
D. 6
E. 3
13.56. What is the number of electrons,
losted or gained according with
the transformation: H2SO4 →
H2S.
А. 5
B. 6
C. 7
D. 4
E. 8
13.52. What is the number of electrons,
losted or gained according with
the transformation: NH3 → N2.
А. 7
B. 3
C. 5
D. 6
E. 4
69
Chapter 14. Experimental studying of reduction-oxidation
reactions
the transformation: MgO→ Mg0
.
А. 4
B. 5
C. 3
D. 2
E. 1
14.1. What is the number of electrons,
losted or gained according with
the transformation: HNO3 →
NO2.
А. 5
B. 2
C. 4
D. 3
E. 1
14.6. What is the number of electrons,
losted or gained according with
the transformation: HNO3 →
NO.
А. 1
B. 2
C. 4
D. 5
E. 3
14.2. What is the number of electrons,
losted or gained according with
the transformation: H2SO3 →
H2SO4 .
А. 5
B. 3
C. 4
D. 2
E. 1
14.7. What is the number of electrons,
losted or gained according with
the transformation: N2 → NO.
А. 1
B. 2
C. 4
D. 5
E. 3
14.3. What is the number of electrons,
losted or gained according with
the transformation: S0 → H2S.
А. 5
B. 4
C. 3
D. 2
E. 1
14.8. What is the number of electrons,
losted or gained according with
the transformation: O2 → CuO.
А. 3
B. 4
C. 5
D. 1
E. 2
14.4. What is the number of electrons,
losted or gained according with
the transformation: NO→ NO2.
А. 2
B. 5
C. 4
D. 3
E. 1
14.9. What is the number of electrons,
losted or gained according with
the transformation: H2SO4 → S0.
А. 5
B. 7
14.5. What is the number of electrons,
losted or gained according with
70
C. 6
D. 8
E. 4
B.
C.
D.
E.
14.10. What is the number of electrons,
losted or gained according with
the transformation: S0 → H2SO4
.
А. 6
B. 5
C. 4
D. 8
E. 7
6
7
5
9
14.14. What is the number of electrons,
losted or gained according with
the transformation: HNO3 →
NH3.
А. 8
B. 7
C. 5
D. 6
E. 9
14.11. What is the number of electrons,
losted or gained according with
the transformation: H2S → SO2 .
А. 4
B. 3
C. 7
D. 6
E. 5
14.15. What is the number of electrons,
losted or gained according with
the transformation: HNO3 →
N2O
А. 4
B. 7
C. 6
D. 8
E. 5
14.12. What is the number of electrons,
losted or gained according with
the transformation: NH3 → N2.
А. 3
B. 5
C. 4
D. 6
E. 7
14.16. What is the number of electrons,
losted or gained according with
the transformation: H2SO4 →
H2S.
А. 7
B. 5
C. 8
D. 6
E. 4
14.13. What is the number of electrons,
losted or gained according with
the transformation: HNO3 →
NH4Cl.
А. 8
71
Chapter 15. Coordination compounds. Reactions of
coordination compounds formation
15.1. The most stable coordination
compounds exist for:
А. transition metals
B. alkali metals
C. alkaline earth metals
D. lantanoids
E. s-elements
15.5. Select the anion complex ion
from the given ones:
А. [Cr(H2O)3(CN)3]
B. [Zn(OH)4]
C. [Cu(NH3)4]
D. [Cr(H2O)3Br]
E. [Ag(NH3)2]
15.2. 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. [Pt(NH3)2Cl4]
B. [Pt(NH3)2Cl2]Cl2
C. [PtCl4]
D. [Pt(NH3)4Cl2]Cl2
E. [PtCl3(NH3)3]Cl
15.6. Select the cation complex ion
from the given ones:
А. [Zn(OH)4]
B. [Cr(H2O)4(CN)2]
C. [Ag(СN)2]
D. [Cu(СNS)4]
E. [Al(OH)6]
15.7. Select the anion complex ion
from the given ones:
А. [Cr(NH3)3(CN)3]
B. [Cu(H2O)4]
C. [Al(OH)6]
D. [Cu(NH3)4]
E. [Cu(NH3)2Cl2]
15.3. 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. К2[PtCl6]
B. [Pt(NH3)6]Cl4
C. [PtCl3(NH3)3]Cl
D. [Pt(NH3)4Cl2]Cl2
E. [Pt(NH3)2Cl4]
15.8. Select the cation complex ion
from the given ones:
А. [HgI4]
B. [Cr(NH3)4(CNS)2]
C. [Zn(OH)4]
D. [Cu(СN)4]
E. [Cu(H2O)(CN)3]
15.4. Point out the formula of the
coordination compound for
which the empirical formula is
2NH4Cl· PtCl4?
А. [Pt(NH3)4Cl2]Cl2
B. [Pt(NH3)6]Cl4
C. (NH4)2[PtCl6]
D. [Pt(NH3)2Cl4]
E. [Pt(NH3)2Cl3]Cl
15.9. What are the oxidation states of
the central metal ions in the
complex ions [Fe(CN)6]4– and
[Cr(H2O)4F2]+ ?
А. +2, +2
B. +4, +3
C. +2, +3
D. +3, +2
72
E. +3, +3
15.14. 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. [Hg(СN)4]2– Кd = 3·10–42
B. [Hg(CNS)4]2– Кd = 1,3·10–22
C. [HgI4]2– Кd = 1,38·10–30
D. [HgBr4]2– Кd = 1·10–21)
E. [HgCl4]2– Кd = 6·10–16
15.10. What are the oxidation states of
the central metal ions in the
coordination compounds
[Cu(NH3)4]SO4 and
K2[Pt(OH)2Cl4]?
А. +1, +2
B. +2, +3
C. +2, +4
D. +2, +2
E. +1, +4
15.15. 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(OH)4]2– Кd = 2,2·10–15
B. [Zn(CNS)4]2– Кd = 5·10–2
C. [Zn(CN)4]2– Кd = 1,0·10–10
D. [Zn(NH3)4]2+ Кd = 2,0·10–9
E. [ZnЕДТА]2– Кd = 3,2·10–17
15.11. 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, –4
B. +3, –2
C. +3, –3
D. +3, +3
E. +2, +4
15.16. 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(NO2)2]– Кd = 1,8·10–3
B. [Ag(S2O3)2]3– Кd = 3,5·10–14
C. [Ag(CN)2]– Кd = 1,4·10–20
D. [AgCl2]– Кd = 9,1·10–6
E. [Ag(NH3)2]+ Кd = 5,8·10–8
15.12. 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. +3, 6
B. +2, 4
C. +3, 4
D. +3, 2
E. +2, 6
15.17. 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− ]
B. [ Fe 2 + ] + [CN − ] 6
15.13. 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. +2, –2
C. +4, +2
D. +4, 0
E. +4, –2
[[Fe(CN) 6 ] 4 − ]
C. [Fe 2+ ] ⋅ [CN − ]6
[[Fe(CN) 6 ] 4 − ]
73
А. [Hg 2+ ] ⋅ [I − ] 4
D. [Fe 3+ ] ⋅ [CN − ]6
[[HgI 4 ] 2− ]
3−
[[Fe(CN ) 6 ] ]
B. [K + ] 2 ⋅ [Hg 2+ ] ⋅ [I − ] 4
E. [ K + ] 4 ⋅ [[Fe(CN ) 6 ] 4− ]
[ K 2 [ HgI 4 ]]
[K 4 [Fe (CN ) 6 ]]
2+ 2
15.18. The expression of the constants
of dissociation of complex ion for
the compound [Cu(NH3)4]SO4 is:
А. [Cu 2+ ] ⋅ [ NH 3 ] 4
2+
C. [Hg ] ⋅ [I − ]
[[HgI 4 ]2 − ]
D. [ K + ] 2 ⋅ [[HgI 4 ] 2 − ]
[ K 2 [HgI 4 ]]
E. [Hg 2+ ] ⋅ 4[I − ]
[[Cu ( NH 3 ) 4 ] ]
B. [Cu 2+ ] 2 ⋅ [ NH 3 ] 4
[[Cu ( NH 3 ) 4 ] 2+ ]
C. [Cu 2+ ] ⋅ 4[ NH 3 ]
[[HgI 4 ] 2− ]
15.21. The expression of the constants
of dissociation of complex ion for
the compound Na2[Zn(OH)4] is:
А. [ Na + ] 2 ⋅ [ Zn 2+ ] ⋅ [OH − ] 4 ]
[[Cu ( NH 3 ) 4 ] 2+ ]
D. [Cu 2+ ] + [ NH 3 ] 4
[ Na 2 [ Zn(OH) 4 ]]
[[Cu ( NH 3 ) 4 ] 2+ ]
+ 2
B. [ Na ] ⋅ [ Zn(OH) 4 ] 2− ]
E. [[Cu ( NH 3 ) 4 ] 2+ ] ⋅ [SO 24− ]
[ Na 2 [ Zn(OH) 4 ]]
[[Cu ( NH 3 ) 4 ]SO 4 ]
15.19. The expression of the constants
of dissociation of complex ion for
the compound [Co(NH3)6]Cl2 is:
А. [Co 2+ ] ⋅ [ NH 3 ] 6
[[Co( NH 3 ) 6 ] 2+ ]
C. [ Zn 2 + ] + [OH − ] 4
[[Zn(OH) 4 ] 2− ]
D. [ Zn 2+ ] ⋅ 4[OH − ]
[[Zn(OH) 4 ] 2− ]
E. [Zn 2+ ] ⋅ [OH − ] 4
[[Zn(OH) 4 ] 2− ]
B. [Co 2 + ] + [ NH ] 6
3
[[Co( NH 3 ) 6 ] 2 + ]
C. [Co( NH 3 ) 6 ] ⋅ [Cl − ] 2
[[Co( NH 3 ) 6 ]Cl 2 ]
D. [Co 2+ ] ⋅ 6[ NH ]
3
[[Co( NH 3 ) 6 ] 2+ ]
E. [Co 2 + ] ⋅ 6[ NH 3 ] ⋅ 2[Cl − ]
[[Co ( NH 3 ) 6 ]Cl 2 ]
15.20. The expression of the constants
of dissociation of complex ion for
the compound K2[HgI4] is:
74
15.22. Select the most stable
amminecomplex through the
listed ones, if the complex ions
have the given values of the
constants of dissociation:
А. [Co(NH3)6]3+ Кd = 6,2·10–36
B. [Cu(NH3)4]2+ Кd = 9,3·10–13
C. [Ni(NH3)6]2+ Кd = 1,2·10–8
D. [Zn(NH3)4]2+ Кd = 2,0·10–9
E. [Hg(NH3)4]2+ Кd = 5,2·10–20
15.23. The quantitative characteristic of
complex ions stability in solution
is:
А. the equilibrium constant
B. the constant of the complex
formation
C. the constant of hydrolysis
D. the percent of dissociation
E. the constant of dissociation
D. 10
E. 6
15.28. Complete and balance the
equation of the reaction AgBr +
Na2S2O3 → Point out the sum of
the coefficients of this equation.
А. 5
B. 4
C. 8
D. 6
E. 7
15.24. What is the product of the
reaction of interaction of copper
sulfate with the excess of
ammonium hydroxide?
А. [Cu(NH3)4](OH)2
B. [Cu(NH3)2(H2O)2]SO4
C. Cu(OH)2
D. [Cu(OH)2(NH3)2]
E. (NH4)2[Cu(OH)4]
15.25. What is the product of the
reaction of Cu(OH)2 dissolving in
the excess of concentrated КОН?
А. [Cu(H2O)4](OH)2
B. reaction doesn’t pass
C. [Cu(OH)2(H2O)2]
D. K2[Cu(OH)4]
E. K[Cu(OH)3]
15.26. 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[HgCl4]
D. K2[HgI4]
E. [HgI2]
15.29. Complete and balance the
equation of the reaction
[Cu(H2O)4]SO4 + NH3 → Point
out the sum of the coefficients of
this equation.
А. 11
B. 9
C. 12
D. 8
E. 10
15.30. What coordination number is the
most common for Fe2+?
А. 6
B. 4
C. 8
D. 2
E. 5
15.31. The most stable coordination
compounds with aminocarbon
acids can form the following
ions:
А. Mn, Mg, Zn
B. Mn, Ni, Fe
C. Co, Fe, Zn
D. Cu, Zn, Co
E. Fe, Mn, Mg
15.27. 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. 13
C. 8
15.32. What is the oxidation state of the
central metal ion in the
coordination compound
75
Na2[Fe(CN)5NO]?
А. +6
B. +1
C. +2
D. +3
E. 0
D. 16
E. 4
15.37. Which ligands through the listed
ones are monodentate?
А. OH– and SO42–
B. Cl– and P2O74–
C. NH3 and SO42–
D. NH3 and CN–
E. Н2O and CO32–
15.33. Zinc can dissolve in the excess of
an alkali solution owing to the
complex ion formation:
А. [Zn(OH)4]2–
B. [Zn(H2O)4]2+
C. [ZnCl4]2–
D. [Zn(NH3)4]2+
E. ZnO22–
15.38. Which ligands through the listed
ones are bidentate?
А. Н2O and CNS–
B. Н2O and Br–
C. Cl– and CN–
D. CO32– and P2O74–
E. NH3 and CN–
15.34. 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. square pyramid
B. linear
C. Tetrahedral
D. square planar
E. octahedral
15.39. Which ligands through the listed
ones are monodentate?
А. NH3, CO32–, CNS–
B. CO, NO, SO42–
C. CO32–, Cl–, OH–
D. NH3, CO, CN–
E. С2О42–, CNS–, CN–
15.40. The components of coordination
compounds are:
А. the central metal ion and
positively or negatively
charged ions
B. the central metal ion and the
complex cation
C. the complex ion and the
external coordination sphere
D. the central metal ion and the
complex anion
E. the central metal ion and
ligands
15.35. What will be the product of the
reaction between ZnCl2 and
potassium hexacyanoferrate (II)?
А. K2[Zn(CN)4]
B. Fe[Zn(CN)4]
C. Zn2[Fe(CNS)6]
D. Zn2[Fe(CN)6]
E. Zn3[Fe(CN)6]2
15.36. Complete and balance the
equation of the reaction
K4[Fe(CN)6] + Cl2 → Point out
the sum of the coefficients of this
equation.
А. 6
B. 8
C. 7
15.41. What kind of chemical bonding is
obligatory in coordination
compounds?
А. ionic bonding
76
B. metallic bonding
C. covalent bonding
D. donor-acceptor bonding
E. hydrogen bonding
А. [Ni(OH)2(NH3)2](NO3)2
B. [Ni(H2O)2(NH3)2]NO2
C. [Ni(H2O)2(NH3)2]NO3
D. [Ni(H2O)2(NH3)2](NO3)2
E. [Ni(H2O)2(NO3)2]
15.42. What is the molecular formula of
the coordination compound
diammineditiocyanocopper(ІІ)?
А. (NH4)2[Cu (CN)2]
B. (NH4)2[Cu (CNS)4]
C. [Cu(NH3)2(CN)2]S
D. [Cu(NH3)2](CNS)2
E. [Cu(NH3)2(CNS)2]
15.45. What is the molecular formula of
the coordination compound
potassium
dihydroxotetrachlorochromate(ІІІ
)
А. [KCrCl4](OH)2
B. K[Cr(H2O)2Cl4]
C. K[Cr(OH)2Cl2]
D. K3[Cr(H2O)2(OH)2Cl2]
E. K3[Cr(OH)2Cl4]
15.43. What is the molecular formula of
the coordination compound
pentaamminebromocobalt(ІІІ)
sulfate?
А. [Co(NО2)5Br]SO4
B. [Co(NH3)5Br]SO4
C. [Co(NH4)5Br](SO4)2
D. [Co(NH3)5Br]SO3
E. [Co(NH3)5SO4]Br
15.46. What is the molecular formula of
the coordination compound
dichloroaquatriamminecobalt(ІІІ)
bromide?
А. [Co(H2O)BrCl2(NH3)2]
B. [Co(H2O)Br 2(NH3)3]Cl
C. [Co(H2O)Cl2(NH3)3]Br
D. [CoCl2(NH3)3H2O]Br2
E. [Co(NH3)3(H2O)Br]Cl2
15.44. What is the molecular formula of
the coordination compound
diaquadiamminenicol(ІІ)
nitrateт?
Chapter 16. Experimental studying of coordination
compounds properties
16.1. The expression of the constants of
dissociation of complex ion for
the compound K4[Fe(CN)6] is:
А. [Fe 2 + ] ⋅ [CN − ] 6
[[Fe(CN) 6 ] 4− ]
B. [K + ] 4 ⋅ [[Fe(CN) 6 ] 4 − ]
[K 4 [ Fe(CN) 6 ]]
C. [Fe 2+ ] + [CN − ]6
[[Fe(CN) 6 ] 4 − ]
D. [Fe 3+ ] ⋅ [CN − ] 6
[[Fe(CN ) 6 ]3− ]
77
D. [Hg 2 + ]2 ⋅ [I − ]
E. [Fe 2+ ] ⋅ 6[CN − ]
[[HgI 4 ]2 − ]
4−
[[Fe(CN ) 6 ] ]
E. [K + ] 2 ⋅ [[HgI 4 ] 2− ]
16.2. The expression of the constants of
dissociation of complex ion for
the compound [Cu(NH3)4]SO4 is:
А. [Cu 2+ ] ⋅ [ NH 3 ] 4
[[Cu ( NH 3 ) 4 ] 2 + ]
B. [Cu 2+ ] + [ NH 3 ] 4
B. [ Na + ] 2 ⋅ [ Zn 2+ ] ⋅ [OH − ] 4 ]
C. [Cu 2+ ] 2 ⋅ [ NH 3 ]4
[ Na 2 [ Zn (OH) 4 ]]
[[Cu ( NH 3 ) 4 ] 2+ ]
C. [ Zn 2+ ] ⋅ 4[OH − ]
D. [Cu 2+ ] ⋅ 4[ NH 3 ]
[[Zn(OH) 4 ] 2− ]
[[Cu ( NH 3 ) 4 ] 2+ ]
D. [ Na + ] 2 ⋅ [ Zn(OH) 4 ] 2− ]
E. [[Cu ( NH 3 ) 4 ] 2 + ] ⋅ [SO 24 − ]
[ Na 2 [ Zn (OH) 4 ]]
[[Cu ( NH 3 ) 4 ]SO 4 ]
E.
16.3. The expression of the constants of
dissociation of complex ion for
the compound [Co(NH3)6]Cl2 is:
А. [Co 2+ ] ⋅ 6[ NH 3 ]
[[Co ( NH 3 ) 6 ] 2 + ]
B. [Co 2 + ] ⋅ 6[ NH3 ] ⋅ 2[Cl− ]
[[Co( NH3 )6 ]Cl 2 ]
C. [Co 2+ ] ⋅ [ NH 3 ]6
[[Co ( NH 3 ) 6 ] 2 + ]
D. [Co( NH 3 ) 6 ] ⋅[Cl − ] 2
[[Co( NH 3 ) 6 ]Cl 2 ]
E. [Co 2+ ] + [ NH 3 ]6
[[Co( NH 3 ) 6 ] 2+ ]
16.4. The expression of the constants of
dissociation of complex ion for
the compound K2[HgI4] is:
А. [Hg 2+ ] ⋅ [I − ] 4
[[HgI 4 ] 2− ]
[ Hg 2 + ] ⋅ 4[ I − ]
[ Zn 2 + ] ⋅ [OH − ] 4
[[Zn (OH) 4 ] 2− ]
16.6. Select the most stable
amminecomplex through the
listed ones, if the complex ions
have the given values of the
constants of dissociation:
А. [Cu(NH3)4]2+ Кd = 9,3·10–13
B. [Hg(NH3)4]2+ Кd = 5,2·10–20
C. [Co(NH3)6]3+ Кd = 6,2·10–36
D. [Zn(NH3)4]2+ Кd = 2,0·10–9
E. [Ni(NH3)6]2+ Кd = 1,2·10–8
16.7. 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(CNS)2]
D. [Cu(NH3)2(CN)2]S
E. (NH4)2[Cu (CNS)4]
16.8. What is the molecular formula of
the coordination compound
pentaamminebromocobalt(ІІІ)
sulfate?
[[ HgI 4 ] 2 − ]
C.
16.5. 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− ]
[[Cu ( NH 3 ) 4 ] 2+ ]
B.
[K 2 [HgI 4 ]]
[ K + ] 2 ⋅ [Hg 2+ ] ⋅ [ I − ] 4
[K 2 [HgI 4 ]]
78
А. [Co(NH4)5Br](SO4)2
B. [Co(NH3)5Br]SO4
C. [Co(NH3)5Br]SO3
D. [Co(NО2)5Br]SO4
E. [Co(NH3)5SO4]Br
16.9. What is the molecular formula of
the coordination compound
diaquadiamminenicol(ІІ) nitrateт?
А. [Ni(OH)2(NH3)2](NO3)2
B. [Ni(H2O)2(NH3)2]NO2
C. [Ni(H2O)2(NH3)2]NO3
D. [Ni(H2O)2(NO3)2]
E. [Ni(H2O)2(NH3)2](NO3)2
16.10. What is the molecular formula of
the coordination compound
potassium
dihydroxotetrachlorochromate(ІІІ)
А. K[Cr(OH)2Cl2]
B. K3[Cr(OH)2Cl4]
C. [KCrCl4](OH)2
D. K[Cr(H2O)2Cl4]
E. K3[Cr(H2O)2(OH)2Cl2]
16.11. What is the molecular formula of
the coordination compound
dichloroaquatriamminecobalt(ІІІ)
bromide?
А. [Co(H2O)BrCl2(NH3)2]
B. [Co(H2O)Cl2(NH3)3]Br
C. [Co(NH3)3(H2O)Br]Cl2
D. [Co(H2O)Br 2(NH3)3]Cl
E. [CoCl2(NH3)3H2O]Br2
16.13. 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, +3
C. +1, +2
D. +2, +2
E. +1, +4
16.14. 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, –3
B. +3, –2
C. +2, +4
D. +3, –4
E. +3, +3
16.15. 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, 6
B. +3, 6
C. +3, 4
D. +3, 2
E. +2, 4
16.16. 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. +4, +2
B. +4, –2
C. +4, 0
D. +2, –2
E. +2, –4
16.12. What are the oxidation states of
the central metal ions in the
complex ions [Fe(CN)6]4– and
[Cr(H2O)4F2]+ ?
А. +3, +3
B. +2, +3
C. +2, +2
D. +3, +2
E. +4, +3
79
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.
1.32.
1.33.
1.34.
1.35.
1.36.
1.37.
1.38.
1.39.
1.40.
A
A
C
E
A
C
C
E
B
C
B
E
B
B
B
E
C
D
B
E
E
D
C
D
E
E
C
E
E
C
E
E
D
C
B
D
A
D
C
B
1.41.
1.42.
1.43.
1.44.
1.45.
1.46.
1.47.
1.48.
1.49.
1.50.
1.51.
1.52.
1.53.
1.54.
1.55.
1.56.
1.57.
2.1.
2.2.
2.3.
2.4.
2.5.
2.6.
2.7.
2.8.
2.9.
2.10.
2.11.
2.12.
2.13.
2.14.
2.15.
2.16.
2.17.
2.18.
2.19.
2.20.
2.21.
2.22.
2.23.
E
E
B
C
A
A
D
A
E
D
C
D
D
E
E
B
E
C
B
C
E
B
E
E
D
A
D
C
A
E
A
A
C
E
E
E
B
B
D
A
2.24.
2.25.
2.26.
2.27.
2.28.
2.29.
2.30.
2.31.
2.32.
2.33.
2.34.
2.35.
2.36.
2.37.
2.38.
2.39.
2.40.
2.41.
2.42.
2.43.
2.44.
2.45.
2.46.
2.47.
2.48.
2.49.
2.50.
2.51.
2.52.
2.53.
2.54.
2.55.
2.56.
2.57.
2.58.
2.59.
2.60.
2.61.
2.62.
2.63.
E
B
C
D
D
A
B
E
A
D
A
E
C
B
E
E
B
B
E
A
B
E
A
D
E
D
E
E
A
D
C
C
A
A
D
E
B
E
E
B
80
2.64.
2.65.
2.66.
2.67.
2.68.
2.69.
2.70.
2.71.
2.72.
2.73.
2.74.
2.75.
2.76.
2.77.
2.78.
2.79.
2.80.
2.81.
2.82.
2.83.
2.84.
2.85.
2.86.
2.87.
2.88.
2.89.
2.90.
2.91.
2.92.
2.93.
2.94.
2.95.
2.96.
2.97.
2.98.
2.99.
2.100.
3.1.
3.2.
3.3.
C
C
C
A
D
D
E
D
C
B
B
C
E
A
E
B
C
E
A
E
E
D
B
C
D
B
B
B
B
D
C
B
C
E
A
E
E
C
B
A
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.
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.
E
E
B
D
B
D
E
B
D
B
B
E
E
B
D
B
E
B
E
A
C
C
C
A
E
C
E
B
B
E
E
B
B
B
C
D
E
E
D
C
3.44.
3.45.
3.46.
3.47.
3.48.
3.49.
3.50.
3.51.
3.52.
3.53.
3.54.
3.55.
3.56.
3.57.
3.58.
3.59.
3.60.
3.61.
3.62.
3.63.
3.64.
3.65.
3.66.
3.67.
3.68.
3.69.
3.70.
3.71.
3.72.
3.73.
3.74.
3.75.
3.76.
3.77.
3.78.
3.79.
3.80.
3.81.
3.82.
3.83.
3.84.
3.85.
3.86.
B
D
A
E
C
A
A
C
A
C
C
C
E
E
A
A
E
D
A
B
E
A
C
D
B
D
C
C
C
D
D
E
A
B
E
A
D
A
E
A
C
A
B
3.87.
3.88.
3.89.
3.90.
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.
4.21.
4.22.
4.23.
4.24.
4.25.
4.26.
4.27.
4.28.
4.29.
4.30.
4.31.
5.1.
5.2.
5.3.
5.4.
5.5.
5.6.
5.7.
5.8.
B
E
B
B
B
B
B
C
C
A
E
E
D
A
C
C
D
A
A
B
B
E
C
A
B
B
B
A
C
D
A
B
B
A
C
B
C
D
A
B
E
B
E
5.9.
5.10.
5.11.
5.12.
5.13.
5.14.
5.15.
5.16.
5.17.
5.18.
5.19.
5.20.
6.1.
6.2.
6.3.
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.
B
E
A
E
B
E
C
B
A
B
C
A
E
D
A
D
D
D
B
C
B
C
A
E
B
A
B
E
D
B
C
D
E
A
A
B
E
B
A
D
D
C
D
81
6.32.
6.33.
6.34.
6.35.
6.36.
6.37.
6.38.
6.39.
6.40.
6.41.
6.42.
6.43.
6.44.
6.45.
6.46.
6.47.
6.48.
6.49.
6.50.
6.51.
6.52.
6.53.
6.54.
7.1.
7.2.
7.3.
7.4.
7.5.
7.6.
7.7.
7.8.
7.9.
7.10.
7.11.
7.12.
7.13.
7.14.
7.15.
7.16.
7.17.
7.18.
7.19.
7.20.
D
D
B
E
C
D
C
C
D
D
B
D
A
B
A
B
D
E
E
E
D
D
C
D
B
D
B
D
E
B
C
B
A
A
E
A
A
A
D
C
D
C
A
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.
7.45.
7.46.
7.47.
8.1.
8.2.
8.3.
8.4.
8.5.
8.6.
8.7.
8.8.
8.9.
8.10.
8.11.
8.12.
8.13.
8.14.
8.15.
8.16.
A
C
E
E
A
A
E
D
E
E
C
D
B
E
B
C
B
A
C
D
C
B
C
B
E
E
C
A
A
C
D
E
C
B
B
E
D
E
D
B
D
B
B
8.17.
8.18.
8.19.
8.20.
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.
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.
10.1.
10.2.
10.3.
10.4.
10.5.
10.6.
10.7.
A
B
B
A
D
A
C
E
E
C
D
A
B
E
B
B
E
B
A
B
D
E
D
C
E
A
B
D
E
B
D
A
B
C
E
B
A
E
D
A
D
D
D
10.8.
10.9.
10.10.
10.11.
10.12.
10.13.
10.14.
10.15.
10.16.
10.17.
10.18.
10.19.
10.20.
10.21.
10.22.
10.23.
10.24.
10.25.
10.26.
10.27.
10.28.
10.29.
10.30.
10.31.
10.32.
10.33.
10.34.
10.35.
10.36.
10.37.
10.38.
11.1.
11.2.
11.3.
11.4.
11.5.
11.6.
11.7.
11.8.
11.9.
11.10.
11.11.
11.12.
B
A
C
D
A
D
C
E
D
A
E
B
D
A
E
E
D
E
C
A
C
C
B
B
E
A
C
B
B
E
E
B
D
C
C
D
E
C
C
C
B
C
D
11.13.
11.14.
11.15.
11.16.
11.17.
11.18.
11.19.
11.20.
11.21.
12.1.
12.2.
12.3.
12.4.
12.5.
12.6.
12.7.
12.8.
12.9.
12.10.
12.11.
12.12.
12.13.
12.14.
12.15.
12.16.
12.17.
12.18.
12.19.
12.20.
12.21.
12.22.
12.23.
12.24.
12.25.
12.26.
12.27.
12.28.
12.29.
12.30.
12.31.
12.32.
12.33.
12.34.
C
E
A
C
B
D
B
C
C
A
E
A
B
E
B
A
B
E
A
D
B
D
E
B
B
B
E
C
C
B
C
B
A
D
C
A
A
A
B
E
A
D
C
82
12.35.
12.36.
12.37.
12.38.
12.39.
12.40.
12.41.
12.42.
12.43.
12.44.
13.1.
13.2.
13.3.
13.4.
13.5.
13.6.
13.7.
13.8.
13.9.
13.10.
13.11.
13.12.
13.13.
13.14.
13.15.
13.16.
13.17.
13.18.
13.19.
13.20.
13.21.
13.22.
13.23.
13.24.
13.25.
13.26.
13.27.
13.28.
13.29.
13.30.
13.31.
13.32.
13.33.
E
E
B
B
A
D
D
A
B
C
C
E
B
E
B
E
E
C
D
D
E
E
A
C
A
B
A
D
D
C
A
E
A
E
A
E
B
C
E
D
E
B
D
13.34.
13.35.
13.36.
13.37.
13.38.
13.39.
13.40.
13.41.
13.42.
13.43.
13.44.
13.45.
13.46.
13.47.
13.48.
13.49.
13.50.
13.51.
13.52.
13.53.
13.54.
13.55.
13.56.
14.1.
14.2.
14.3.
14.4.
14.5.
14.6.
14.7.
14.8.
14.9.
14.10.
14.11.
14.12.
14.13.
14.14.
14.15.
14.16.
15.1.
15.2.
15.3.
15.4.
E
C
E
A
E
A
A
E
C
C
A
B
B
C
B
E
B
D
D
D
C
A
E
E
D
D
A
D
E
C
B
C
A
D
D
A
A
D
C
A
D
B
C
15.5.
15.6.
15.7.
15.8.
15.9.
15.10.
15.11.
15.12.
15.13.
15.14.
15.15.
15.16.
B
B
C
B
C
C
C
A
E
A
B
C
15.17.
15.18.
15.19.
15.20.
15.21.
15.22.
15.23.
15.24.
15.25.
15.26.
15.27.
15.28.
C
A
A
A
E
A
E
A
D
D
D
A
15.29.
15.30.
15.31.
15.32.
15.33.
15.34.
15.35.
15.36.
15.37.
15.38.
15.39.
15.40.
E
A
D
D
A
B
D
C
D
D
D
C
83
15.41.
15.42.
15.43.
15.44.
15.45.
15.46.
16.1.
16.2.
16.3.
16.4.
16.5.
16.6.
D
E
B
D
E
C
A
A
C
A
E
C
16.7.
16.8.
16.9.
16.10.
16.11.
16.12.
16.13.
16.14.
16.15.
16.16.
C
B
E
B
B
B
A
A
B
B
CONTENTS
Chapter 1. Atomic-molecule concept. Nomenclature and classification of
inorganic compounds ................................................................................. 2
Chapter 2. Structure of atoms. The Periodic law and Periodic table by D.
Mendeleev ................................................................................................. 7
Chapter 3. Equivavlents of substances in chemical reactions .................................... 17
Chapter 4. Solutions. Ways of expressing concentration of solutions ....................... 27
Chapter 5. Colligative properties of solutions ........................................................... 31
Chapter 6. The basic terms of chemical thermodynamics. Thermochemistry.
The direction of chemical processes passage ........................................... 33
Chapter 7. The rate and mechanism of chemical reactions........................................ 39
Chapter 8. The equilibrium in feebly soluble electrolytes solutions .......................... 45
Chapter 9. Chemical equilibrium............................................................................... 48
Chapter 10. The concept of strong and weak electrolytes ......................................... 53
Chapter 11. Acids and bases theories. Self-ionization of water. pH .......................... 56
Chapter 12. Protolytic processes................................................................................ 59
Chapter 13. Reactions with electrons transferring ..................................................... 63
Chapter 14. Experimental studying of reduction-oxidation reactions ....................... 70
Chapter 15. Coordination compounds. Reactions of coordination compounds
formation ................................................................................................. 72
Chapter 16. Experimental studying of coordination compounds properties .............. 77
84