1. There is no unit

2. mol/l

3. g/mol

4. mol

5. g

18. Unit of the molar mass of the substance A

1. g/mol

2. there is no unit

3. mol/l

4. mol

5. g

19. Unit of the molar mass of an equivalent of the substance A

1. g/mol

2. there is no unit

3. mol/l

4. mol

5. g

20. Unit of a number of equivalence of the substance A

1. There is no unit

2. mol/l

3. g/mol

4. mol

5. g

21. Unit of the factor of equivalence

1. There is no unit

2. mol/l

3. g/mol

4. mol

5. g

22. Unit of a density of a solution A

1. g/ml

2. g

3. mol/l

4. mg / mol

5. there is no unit

23. Unit of the mass of the substance A

1. g

2. mol/l

3. mg / l

4. there is no unit

5. g/ml

24. Specify the molecular mass of air

А) 29 g/mole

В) 16 g/mole

С) 2 g/mole

D) 32 g/mole

25. Specify the molar volume of a gas at normal condition

А) 22,4

В) 2,24

С) 224

D) 0,224

Е) 0,02

26. Define the number of equivalence of the phosphoric acid for the following reaction: H₃PO₄+NaOH=NaH₂PO₄+H₂O

1. 1

2. 1/2

3. 2

4. 1/3

5. 3

27. Determine the equivalent of soda for the reaction: Na₂CO₃ + 2 HCI = 2 NaCI + CO₂ + H₂O

1. 1/2 Na₂CO₃

2. 2

3. 1/2

4. Na₂CO₃

5. 3

28. Determine the equivalent of soda for the reaction: Na₂CO₃ + HCI = NaHCO₃ + NaCI

1. Na₂CO₃

2. 1/2 Na₂CO₃

3. 2

4. 1/2

5. 3

29. Determine the number of equivalence of soda for the reaction: Na₂CO₃ + 2 HCI = 2 NaCI + CO₂ + H₂O

1. 2

2. HCI

3. 1/2

4. 1

5. Na₂CO₃

30. Determine the factor of equivalence of soda for the reaction: Na₂CO₃ + 2 HCI = 2 NaCI + CO₂ + H₂O

1. 1/2

2. 1

3. Na₂CO₃

4. HCI

5. 2

31. Determine the number of equivalence of soda for the reaction: Na₂CO₃ + HCI = NaHCO₃ + NaCI

1. 1

2. 1/2

3. 1/3

4. 2

5. 3

32. Determine the factor of equivalence of soda for the reaction: Na₂CO₃ + HCI = NaHCO₃ + NaCI

1. 1

2. 1/2

3. 1/3

4. 2

5. 3

33. Determine the equivalent of permanganate ion for the reaction: MnO₄^-+ 8 H ⁺ + 5 e = Mn^{2 +} + 4 H₂O

1. 1/5 MnO₄^-

2. MnO₄^-

3. 1/2

4. 1/7

5. 1/2 Mn^{2 +}

34. Determine the equivalent of iron for the reaction: 5 Fe^{2 +} + MnO₄^-+ 8 H ⁺ = 5 Fe^{3 +} + Mn^{2 +} + 4 H₂O

1. Fe

2. 1/2 Fe

3. 1/2

4. 1/3 Fe

5. 1

35. Determine the equivalent of dichromate ion for the reaction: Cr₂O₇^2-+ 14 H ⁺ + 6 e = 2 Cr^{3 +} + 7 H₂O

1. 1/6 Cr₂O₇^2-

2. 1/6

3. 1/3

4. Cr₂O₇^2-

5. 1/3 Cr₂O₇^2-

36. Determine the equivalent of calcium phosphate for the reaction: 3 Ca^{2 +} + 2 PO₄^3- = Ca₃ (PO₄) ₂

1. 1/6 Ca₃ (PO₄) ₂

2. 1/3

3. 1/6

4. 1/3Ca₃ (PO₄) ₂

5. Ca₃ (PO₄) ₂

37. Determine the number of equivalence of permanganate ion for the reaction: MnO₄ ^-+ 8 H ⁺ + 5 e = Mn^{2 +} + 4 H₂O

1. 5

2. 1/5 MnO₄^-

3. MnO_4-

4. 1/2

5. 2

38. Determine the factor of equivalence of permanganate ion for the reaction: MnO₄^-+ 8 H ⁺ + 5 e = Mn^{2 +} + 4 H₂O

1. 1/5

2. 1/5 MnO₄^-

3. MnO₄^-

4. 1/2

5. 1/7

39. Determine the number of equivalence of iron for the reaction: 5 Fe^{2 +} + MnO₄^-+ 8 H ⁺ = 5 Fe^{3 +} + Mn^{2 +} + 4 H₂O

1. 1

2. Fe

3. 1/2 Fe

4. 1/2

5. 3

40. Determine the factor of equivalence of iron for the reaction: 5 Fe^{2 +} + MnO₄^-+ 8 H ⁺ = 5 Fe^{3 +} + Mn^{2 +} + 4 H₂O

1. 1

2. Fe

3. 1/2 Fe

4. 1/2

5. 1/3 Fe

41. Determine the number of equivalence of dichromate ion for the reaction: Cr₂O₇^2-+ 14 H ⁺ + 6 e = 2 Cr^{3 +} + 7 H₂O

1. 6

2. 1/6 Cr₂O₇^2-

3. 3

4. 1/6

5. 1/3 Cr₂O₇^2-

42. Determine the factor of equivalence of dichromate ion for the reaction: Cr₂O₇^2- + 14 H ⁺ + 6 e = 2 Cr^{3 +} + 7 H₂O

1. 1/6

2. 6

3. 1/3

4. Cr₂O₇^2-

5. 1/3 Cr₂O₇^2-

43. Determine the number of equivalence of calcium phosphate for the reaction: 3 Ca^{2 +} + 2 PO₄^3- = Ca₃ (PO₄) ₂

1. 6

2. 1/6 Ca₃ (PO₄) ₂

3. 1/3

4. 3

5. 1/3Ca₃ (PO₄) ₂

44. Determine the factor of equivalence of calcium phosphate for the reaction: 3 Ca^{2 +} + 2 PO₄^3- = Ca₃ (PO₄) ₂

1. 1/6

2. 1/3

3. 6

4. 1/3Ca₃ (PO₄) ₂

5. Ca₃ (PO₄) ₂

45. Calculate the normal concentration of 12 % H₂SO₄ (density 1.080).

1. 2.6

2. 1.0

3. 3.5

4. 6.0

5. 5.0

46. Calculate the mass fraction (%) of the 6.5 M phosphoric acid (density 1.32).

1. 48.3

2. 53.1

3. 25.3

4. 17.8

5. 33.5

47. Calculate the mass fraction (%) of the sulfuric acid in its 10 n. solution (density 1.29).

1. 38

2. 30

3. 41

4. 29

5. 56

48. Calculate the mass fraction (%) of HCl in its 7.98 M solution (density 1.13).

1. 26

2. 18

3. 9

4. 30

5. 20

49. Calculate the mass fraction (%) of HNO₃ in its 4.85 M solution (density 1.16).

1. 26

2. 18

3. 11

4. 32

5. 21

50. Calculate the mass fraction (%) of КОН in its 8.55 M solution (density 1.35).

1. 35.5

2. 42.1

3. 26.8

4. 30.7

5. 40.5

51. Calculate the mass fraction (%) of NaOH in its 0.7 M solution (density 1.03).

1. 2.7

2. 1.5

3. 1.0

4. 3.2

5. 2.0

52. Calculate the mass fraction (%) of Na₂CO₃ in its 3.07 n. solution (density 1.15).

1. 14

2. 24

3. 10

4. 12

5. 13

53. Calculate the mass fraction (%) of NH₃ in its 14.8 M solution (density of 0.9g/ml).

1. 28

2. 20

3. 17

4. 32

5. 15

54. Calculate the normal concentration of the sulfuric acid if its titer is equal 0.02446 g/ml.

1. 0.4988

2. 0.5321

3. 0.1954

4. 0.2555

5. 0.7820

55. Calculate the molar concentration of sodium hydroxide if its titer is equal 0.004020 g/ml.

1. 0.1005

2. 0.4563

3. 0.5619

4. 0.6721

5. 0.2968

56. Calculate the titer of the sulfuric acid, if its normal concentration is 0.1008 mol/l.

1. 0.004943

2. 0.001115

3. 0.007819

4. 0.003985

5. 0.006178

57. Calculate the titer of sodium hydroxide, if its molar concentration is 0.09981 mol/l.

1. 0.003992

2. 0.007881

3. 0.001078

4. 0.002354

5. 0.005541

58. Calculate the molar concentration of the sulfuric acid if its titer is equal 0.004852 g/ml.

1. 0.04947

2. 0.01591

3. 0.07895

4. 0.06341

5. 0.02317

59. Calculate the normal concentration of the sulfuric acid if its titer is equal 0.004852 g/ml

1. 0.09895

2. 0.04563

3. 0.07811

4. 0.05560

5. 0.06113

60. The titer of the hydrochloric acid is equal to 0.003592 g/ml, determine the molar concentration of the solution.

1. 0.09841

2. 0.01282

3. 0.00400

4. 0.00100

5. 0.02536

61. Determine the titer of 0.1205 n. of the sulfuric acid solution.

1. 0.00590

2. 0.0180

3. 0.00245

4. 0.1205

5. 0.01216

62. Determine the titer of 1 M of the milk acid (CH₃CHOHCOOH) solution.

1. 9·10^-2

2. 9·10^-3

3. 9·10^-4

4. 9·10^-5

5. 9·10^-6

63. Calculate the molar concentration of the acetic acid (С₂Н₄О₂) with the titer 0.000016 g/ml.

1. 0.0002667

2. 0.001334

3. 0.002672

4. 0.02672

5. 0.01334

64. Calculate the titer of 0.21 M of the sodium hydroxide solution.

1. 0.008400

2. 0.004200

3. 0.21000

4. 0.05250

5. 0.003672

65. Calculate the titer of 1 M of the wine acid (СО₂Н (СНОН) ₂СО₂Н) solution.

1. 0.1500

2. 0.0150

3. 0.0075

4. 0.0015

5. 0.0750

66. Determine the normal concentration of H₂SO₄ solution which titer is 0.004278 g/ml.

1. 0.0873

2. 0.0980

3. 0.1746

4. 0.0434

5. 0.1517

67. Determine the molar concentration of 35 % H₂SO₄ (density 1.26).

1. 4.5

2. 5.0

3. 3.0

4. 4.0

5. 3.5

68. Calculate the titer of 0.02 M of acetone ((CH₃) ₂CO) solution.

1. 1,16·10^-3

2. 1,16·10^-4

3. 5,8·10^-2

4. 5,8·10^-3

5. 5,8·10^-4

69. Calculate the titer of 0.1420 n. of the sulfuric acid solution.

1. 0.006958

2. 0.005112

3. 0.004840

4. 0.142000

5. 0.012360

70. Determine the normal concentration of the sulfuric acid if its titer is equal to 0.00590 g/ml.

1. 0.1204

2. 0.2410

3. 0.0100

4. 0.0180

5. 0.1518

71. Calculate the titer of 0.1101 M solution of the hydrochloric acid.

1. 0.004019

2. 0.003563

3. 3.9636

4. 0.001101

5. 0.03963

72. Determine the titer of 0.12 n. of the sulfuric acid solution.

1. 0.005880

2. 0.017601

3. 0.002440

4. 0.001482

5. 0.03568

73. Calculate the titer of 0.12 n. of sodium tetra borate (Na₂B₄O₇) solution.

1. 0.01207

2. 22.8841

3. 0.0005203

4. 0.003485

5. 2.2884

74. Determine the molar concentration of nitric acid which titer is equal to 0.006300 g/ml?

1. 0.1

2. 6.3

3. 0.001

4. 0.6

5. 0.63

75. Calculate the mass of iodine in 0.1923 g of chemically pure AgI.

1. 0.1039

2. 0.4156

3. 0.2387

4. 0.5145

5. 0.3026

76. Calculate the mass of chromium in 0.5844 g of chemically pure BaCrO₄.

1. 0.1199

2. 0.3248

3. 0.3591

4. 0.2845

5. 0.2911

77. What is the number (mol) of formaldehyde (НСНО) contained in 5 litres 0.2 M solutions?

1. 1.0

2. 2.0

3. 3.0

4. 4.0

5. 5.0

78. What is the number (mol) of ascorbic acid (С₆Н₈О₆) contained in 500 ml of 0.02 M solution?

1. 0.010

2. 0.176

3. 0.352

4. 0.020

5. 0.256

79. How many grams of benzaldehyde (С₆Н₅СНО) are necessary for preparation 200 ml of 0.01 M solution?

1. 0.212

2. 0.021

3. 2.120

4. 0.424

5. 0.106

80. How many grams of furfural (С₄Н₃ОСНО) are necessary for preparation of 0.1 litre 0.002 M solution?

1. 0.0192

2. 0.0019

3. 1.9200

4. 0.1920

5. 19.200

81. How many grams of the waterless sodium carbonate are necessary to receive 2 litres 0.1 n. solution?

1. 10.6

2. 15.3

3. 5.5

4. 21.4

5. 30.0

82. How many grams of potassium chloride are necessary to dissolve in 100 g of water to receive 5 % solution?

1. 5.26

2. 2.41

3. 7.15

4. 4.66

5. 3.18

83. How many grams of sodium sulfate are necessary to dissolve in 400 g of water to receive 8 % solution?

1. 34.78

2. 36.98

3. 30.45

4. 33.12

5. 31.77

84. How many grams of water should be added to 40 g of KBr to receive 4 % solution?

1. 960

2. 1000

3. 850

4. 500

5. 270

85. How many grams of water should be added to 5.7 g of the boric acid to receive 3 % solution?

1. 184.3

2. 200.2

3. 150.0

4. 360.1

5. 180.0

86. How many grams of the sulfuric acid are in 1 litre of 0.1 n. solutions?

1. 4.9

2. 8.5

3. 3.7

4. 6.8

5. 5.6

87. How many grams of soda are in 1 litre of 0.5 n. solutions?

1. 26.5

2. 30.1

3. 20.8

4. 23.6

5. 29.2

88. How many grams of the phosphoric acid are in 1 litre of 0.3 n. solutions?

1. 9.8

2. 5.5

3. 6.7

4. 11.9

5. 4.8

89. How many grams of magnesium sulfate are in 1 litre of 0.2 n. solutions?

1. 12

2. 20

3. 31

4. 15

5. 28

90. How many grams of aluminium chloride are in 1 litre of 0.3 n. solutions?

1. 13.35

2. 15.17

3. 21.03

4. 10.11

5. 18.52

91. How many grams of aluminium sulfate are in 1 litre of 0.1 M solutions?

1. 34.2

2. 30.1

3. 25.0

4. 36.3

5. 28.4

92. How many grams of aluminium sulfate are in 1 litre of 1.8 n. solutions?

1. 102.6

2. 116.0

3. 125.3

4. 98.5

5. 73.9

93. How many grams of Na₂CO₃·10H₂O are necessary to receive 3 litres of 0.2 n. solution?

1. 85.8

2. 20.6

3. 40.0

4. 97.3

5. 60.0

94. How many grams of water should be added to 100 g of Na₂CO₃ ·10H₂O to receive 10 % salt solution?

1. 270.6

2. 300.1

3. 250.7

4. 425.1

5. 125.6

95. What the number (mol) of NaCN should be dissolved in 100 g of water to receive 5 % solution?

1. 0.1073

2. 1.0730

3. 0.9521

4. 0.7735

5. 0.6517

96. What the number of water (mol) should be added to 50 g of H₂SO₄ to receive 10 % solution?

1. 25

2. 15

3. 10

4. 30

5. 35

97. 400 ml of 1.2 M NaOH and 600 ml of 1.8 M NaOH are mixed; determine the molar concentration of the received solution.

1. 1.56

2. 2.25

3. 1.15

4. 1.96

5. 2.11

98. How many ml of 0.1 n. of phosphoric acid can be prepared from 80 ml of 0.75 n. solution of the same acid?

1. 600

2. 800

3. 700

4. 500

5. 900

99. Up to what volume (liters) is it necessary to dilute 2.4 litres of 1.6 M HCl by water to receive 0.25 M solution?

1. 15.4

2. 17.6

3. 11.5

4. 13.0

5. 10.9

100. Up to what volume (litre) is it necessary to evaporate 3.5 litres of 0.04 M KOH to receive 0.1 M solution?

1. 1.4

2. 0.9

3. 2.0

4. 3.2

5. 0.5

101. What volume (ml) 0.5 n. of sulfuric acid is necessary to add to 1 litre of 0.11 n. solution of the same acid to receive 0.2 n. solutions?

1. 300

2. 200

3. 100

4. 400

5. 500

102. How many litres of 8 M КОН are necessary to add to 5 litres of 3.2 М КОН to receive 4 М solutions?

1. 1

2. 2

3. 3

4. 4

5. 5

103. How many ml of 2 М NaOH are necessary to add to 750 ml of water to receive 0.4 M solution NaOH?

1. 187.5

2. 100.0

3. 125.3

4. 200.0

5. 145.5

104. What volume of water (ml) should be added to 1 litre of 0.5300 M HCI to receive 0.5000 M solution?

1. 60

2. 100

3. 40

4. 120

5. 80

105. What volume (ml) of 38.32 % solution HCI (density 1.19) is necessary for preparation 1 litre of 0.1 M solution?

1. 8.0

2. 10.0

3. 6.5

4. 5.5

5. 4.0

106. What volume (ml) of 95.72% H₂SO₄ (density 1.84) is necessary for preparation 2.5 litres of 0.1 M H₂SO₄?

1. 14

2. 45

3. 30

4. 36

5. 58

107. 20.00 ml of 7.4 M HCI has been taken for preparation of 500 ml of solution HCI, calculate the molar concentration of the received solution.

1. 0.3

2. 0.8

3. 1.0

4. 0.1

5. 1.5

108. Up to what volume (ml) is it necessary to dilute 200 ml of 0.01 M solution to receive 0.005 M solution?

1. 400

2. 800

3. 500

4. 750

5. 1000

109. How many ml of 1 M solution HCI is it necessary to prepare 1 litre of 0.1 M solution of HCI?

1. 100.0

2. 50.0

3. 10.0

4. 500.0

5. 200.0

110. Up to what volume (ml) is it necessary to dilute 10 ml of 0.5 M solution to receive 0.05 M solution?

1. 100.0

2. 50.0

3. 1000.0

4. 500.0

5. 200.0

111. Up to what volume (ml) is it necessary to dilute100 ml 0.01 M solution of formaldehyde to receive 0.005 M solution of formaldehyde (НСНО)?

1. 200.0

2. 500.0

3. 1000.0

4. 250.0

5. 750.0

112. How many ml of 2.0 M HCI is it necessary to add to 1.1 litres of 0.1880 M HCI to receive 0.2000 M solution?

1. 7.3

2. 10.0

3. 5.0

4. 3.7

5. 5.8

113. How many ml of water are necessary to be added to 1.2 litres of 0.24 M HCI to receive 0.20 M solution?

1. 240

2. 500

3. 320

4. 150

5. 200

114. Up to what volume (ml) is it necessary to dilute100 ml 0.2 M solution to receive 0.02 M solution?

1. 1000.0

2. 500.0

3. 250.0

4. 900.0

5. 750.0

115. 1.5 M solution of CaCI₂ has been diluted in 18 times, determine its molar concentration.

1. 0.083

2. 0.125

3. 0.063

4. 0.045

5. 0.008

116. 0.37 M solution of NaCI has been evaporated to 1/4 initial volume, calculate the molar concentration of the received solution.

1. 1.48

2. 2.31

3. 0.98

4. 3.45

5. 2.84

117. 0.05 M solution of AgNO₃ has been evaporated to 1/7 initial volume, determine the molar concentration of the received solution.

1. 0.35

2. 0.55

3. 0.21

4. 0.53

5. 0.82

118. 0.2 M solution of K₂SO₄ has been diluted in 17 times, determine the molar concentration of potassium cations?

1. 0.024

2. 0.105

3. 0.083

4. 0.077

5. 0.051

119. 0.7 M solution of NaCI has been diluted in 27 times, determine the molar concentration of chlorine anions.

1. 0.026

2. 0.078

3. 0.089

4. 0.057

5. 0.046

120. 1.5 M solution of Al(NO₃) ₃ has been diluted in 75 times, determine the molar concentration of nitrates ions.

1. 0.06

2. 0.05

3. 0.09

4. 0.03

5. 0.01

121. How many ml of 14.6 M of nitric acid are necessary to be taken to receive 4 litres of 0.1 M solution?

1. 27.40

2. 40.21

3. 1089

4. 33.75

5. 20.11

122. 25 ml of 9.5 M H₂SO₄ were diluted up to 3 litres, determine the titer of the received solution.

1. 0.007758

2. 0.07710

3. 0.7715

4. 0.0007714

5. 7.7150

123. How many ml of water is it necessary to add to 3 litres of H₂SO₄ solution with the titer 0.007714 to receive the solution with the titer 0.007351?

1. 148

2. 156

3. 132

4. 113

5. 160

124. How many ml of H₂SO₄ solution with the titer 0.007714 is it necessary to receive 1.5 litres of 0.05 n. solutions?

1. 476

2. 598

3. 321

4. 119

5. 405

125. How many ml of water is it necessary to add to 3754 ml of HNO₃ solution with the titer 0.006497 to receive 0.1 M solution?

1. 117

2. 234

3. 157

4. 193

5. 205

126. How many the ml of water is it necessary to add to 3753 ml solution of nitric acid with the titer 0.006316 to receive 0.1 M solution?

1. 9.5

2. 2.8

3. 5.5

4. 6.3

5. 1.9

127. How many ml of HNO₃ with the titer 0.006479 is it necessary to receive 5 litres of 0.01 M solution?

1. 486.4

2. 523.3

3. 126.8

4. 348.9

5. 293.2

128. How many ml of the nitric acid solution with the titer 0.006497 is it necessary to add to 500 ml solution of the same acid with the titer 0.005601 to receive 0.1 M solution?

1. 1774

2. 2000

3. 1978

4. 1525

5. 1601

129. How many ml of nitric acid solution with the titer 0.005601 is it necessary to add to 500 ml solution of the same acid with the titer 0.006479 to receive 0.1 M solution?

1. 128.0

2. 140.1

3. 398.2

4. 225.0

5. 115.3

130. How many litres of water must be added to 1 litre of HNO₃ solution with the titer 0.006396 to receive 0.01 M solution?

1. 9

2. 20

3. 35

4. 10

5. 30

131. How many litres of water must be added to 3.9 litres of KOH solution with the titer 0.02817 to receive 0.05 M solution?

1. 35

2. 20

3. 11

4. 25

5. 33

132. How many litres of water must be added to 3.9 litres of NaОН solution with the titer 0.02034 to receive 0.05 M solution?

1. 36

2. 99

3. 25

4. 67

5. 50

133. How many grams of KCl are necessary to be added to 450 g of 8 % solution of the same salt to receive 12 % solution?

1. 20

2. 30

3. 42

4. 11

5. 25

134. How many kg of water is it necessary to add to 1 kg of 40 % solution of the sulfuric acid to receive 25 % solution?

1. 0.6

2. 2.0

3. 1.0

4. 0.5

5. 1.5

135. How many mole of water should be added to 1.6 kg of 25 % NaOH solution to receive 16 % solution?

1. 50

2. 20

3. 30

4. 10

5. 60

136. 300 g of 40 % solution of the sulfuric acid and 700 g of 10 % solution of the same acid are mixed; calculate the mass fraction (%) of the received solution.

1. 19

2. 25

3. 11

4. 38

5. 48

137. How many grams of 32 % solution of nitric acid are necessary to be added to 600 g of 80 % solution of the same acid to receive 64 % solution?

1. 300

2. 500

3. 100

4. 400

5. 200

138. 300 kg of water was evaporated from 750 kg of 48 % solution of the sulfuric acid, determine the mass fraction (%) of sulfuric acid in the received solution.

1. 80

2. 100

3. 60

4. 50

5. 30

139. How many kg of water is it necessary to evaporate from 1 тon of 60 % sulfuric acid solution to receive 96 % solution?

1. 375

2. 450

3. 300

4. 200

5. 350

140. It is necessary to prepare 1 М solution from 1 kg of 63 % nitric acid solution, determine the volume (litres) of the received solution.

1. 10

2. 20

3. 15

4. 30

5. 35

141. It is necessary to prepare 1 M solution of HCI from 20 ml of 20 % HCl (density 1.1), determine the volume (ml) of the received solution.

1. 120.5

2. 100.5

3. 142.3

4. 101.9

5. 115.0

142. It is necessary to prepare 1 M H₃PO₄ solution from 120 ml of 30 % H₃PO₄ (density 1.19), determine the volume (ml) of the received solution.

1. 437

2. 500

3. 425

4. 378

5. 516

143. 800 ml of 3 M КОН solution and 1.2 litres of 12 % КОН solution (density 1.1) are mixed; calculate the molar concentration of the received solution.

1. 2.6

2. 3.0

3. 2.1

4. 0.8

5. 1.5

144. 3 litres of 0.1 M H₃PO₄ solution and 2 litres of 9 % solution of the same acid (density 1.05) are mixed; calculate the normal concentration of the received solution.

1. 1.34

2. 2.25

3. 0.78

4. 1.98

5. 2.15

145. How many ml of 20 % HCl solution (density 1.1) should be added to 4 litres of 0.6 M HCl solution to receive 1 M solution?

1. 320

2. 450

3. 125

4. 350

5. 170

146. How many litres of 0.2 M NH₃ solution are necessary to be added to 20 ml of 35 % NH₃ solution (density 0.88) to receive 0.5 M solution?

1. 1.2

2. 1.8

3. 0.9

4. 0.5

5. 1.6

147. How many litres of 0.1 n. solution of the sulfuric acid is it possible to prepare from 70 ml of 50 % solution of the same acid (density 1.4)?

1. 10

2. 20

3. 30

4. 40

5. 50

148. How many litres of 8 M NaOH is it possible to prepare from 1 kg of 42 % NaOH solution?

1. 1.3

2. 2.5

3. 0.9

4. 2.7

5. 3.1

149. How many litres of 8 M NaOH is it possible to prepare from 1 litre of 42 % NaOH solution (density 1.45)?

1. 1.9

2. 2.5

3. 0.6

4. 2.8

5. 0.2

150. How many ml of 40 % solution of the phosphoric acid (density 1.25) are required for preparation of 400 ml of 0.25 M solution of the same acid?

1. 19.6

2. 21.0

3. 15.3

4. 11.5

5. 21.8

151. How many ml of 40 % phosphoric acid solution (density 1.25) are required for preparation of 3 litres of 0.15 n. solution of the same acid?

1. 29

2. 35

3. 16

4. 13

5. 33

152. Calculate the thermal effect of reaction (кJ) of methanol synthesis from hydrogen and carbon oxide on solid catalyst at 298К 2Н₂ (г) +СО → СН₃ОН (г), if = –201,2 кJ/mol; Н⁰_f(CO) = –110,5 кJ/mol ;

1. –90,7

2. 311,7

3. 90,2

4. 60,9

5. –73,2

153. Determine thermal effect of reaction: СН  СН + СО + Н₂О (ж) → СН₂=СНСООН (ж) at standard pressure if warmth of formation is known

Substance	[kJ/mol ]
СН  СН	226,75
СО	–110,50
Н2О (ж)	–285,84
СН2 = СНСООН (ж)	–384,37

1. -214,78

2. 107,36

3. 1007,36

4. –623,09

5. –154,2

154. To calculate thermal effect of reaction (kJ) at Т=298К CuCl₂ + Zn = ZnCl₂ + Cu Values are resulted in the table:

Substance
ZnCl2	–478,2
CuCl2	–262,3

1. -215,9

2. 740,5

3. –903,6

4. 904,2

5. 370,2

155. Calculate entropy change under standard conditions for reaction 2H₂S + SO₂ = 2 Н₂О (ж) + 3S. Values S are given in the table.

Substance	[J/molК]
Н2О	69,96
S	32,55
SO2	248,1
H2S	205,64

1. –421,81

2. –102,50

3. 513,24

4. 350,72

5. 231,11

156. Calculate thermal effect of reaction (кJ) at Т=298К, Р=1,01310⁵ Па

Cd (тв) + 2AgCl (тв) = 2Ag (тв) + CdCl₂ (тв), if warmth of formation of substances are known

Substance	298 [kJ/mol ]
Сd	0
Ag	0
AgCl	–126,8
CdCl2	–389,0

1. –135,4

2. –263,2

3. –515,8

4. 443,2

5. 344,8

157. Calculate standard change of energy of Gibbs (kJ) for reaction Cd (тв) + 2AgCl (тв) = 2Ag (тв) + CdCl₂ (тв),

if are known Н₂₉₈ = –135,4 kJ; S₂₉₈ = –76,84 J/К.

1. –112,5

2. 1393,55

3. –141,7

4. 24,61

5. 41,42

158. Calculate standard change of entropy for reaction H_2(г)+ O_2(г) H₂O_ж under standard conditions:

Substance	S [J/mol К]
H2	130.6
O2	205.03
H2O	69.96

1. -163.155 J/к

2. 144.39 J/к

3. 450.59 J/к

4. 370.25 J/к

5. 265.67 J/к

159. Calculate standard thermal effect (kJ/mol) reactions of dissolution of zinc in the diluted water solution copper vitriol Zn_(т)+CuSO₄=Cu_(т)+ZnSO₄; H _ZnSO4=-978,2 kJ/mol; kJ/mol.

1. -207,1;

2. -211,66;

3. -316,1;

4. 213,61;

5. 166,19;

160. Calculate thermal effect of reaction (kJ/mol) synthesis methanol from hydrogen and carbon oxide on the solid catalyst at 298 K 2H_2(г)+CO_(г) → CH₃OH_(г), =-201,2 kJ/mol; kJ/mol.

1. -90,7;

2. -60,9;

3. -90,2;

4. -73,2;

5. -86,1;

161. Define thermal effect of chemical reaction at 298 K CH₃OH_(г)+3/2 O₂ → CO₂+2H₂O_(г), if

-201,2 кJ/mol, -393,51 кJ/mol, -241,84 кJ/mol:

1. -675,99 кJ/mol;

2. 398,11 кJ/mol;

3. 1764,2 кJ/mol;

4. -575,25 кJ/mol;

5. -834,78 кJ/mol;

162. Calculate thermal effect of reaction (kJ/mol) synthesis methanol from hydrogen and carbon oxide on the solid catalyst at 298 K 2H_2(г)+CO_2(г) → CH₃OH_(г), -201,2 кJ/mol, -110.5 кJ/mol:

1. -90,7;

2. -60,9;

3. -90,2;

4. -73,2;

5. 86,1;

163. Define standard change of entropy for reaction: C₂H₂+2H₂O_(ж) → CH₃COOH_(ж)+H₂,

200,8 J/molК, 69,96 J/molК, 159,8 J/molК, 130,6 J/molК:

1. -50,32 J/molК;

2. -65,48 J/molК;

3. -45,93 J/molК;

4. -33,75 J/molК;

5. -74,18 J/molК;

164. Calculate energy of Gibbs (J/mol) under standard conditions for reaction: C₂H₂+2H₂O_(ж) → CH₃COOH_(ж)+H₂, 209,25 10³ J/mol, -237,2310³ J/mol, -389,3610³ J/mol, 0

1. -124,1510³;

2. -113,6110³;

3. -121,5310³;

4. -135,9310³;

5. -109,1510³;

165. Calculate thermal effect of reaction under standard conditions for reaction: C₂H₂+2H₂O_(ж) → CH₃COOH_(ж)+H₂,

226,75 10³ J/mol, -285,8410³ J/mol, -484,910³ J/mol, 0:

1. -139,9710³ J/mol;

2. -145,3210³ J/mol;

3. -151,6410³ J/mol;

4. 125,8610³ J/mol;

5. 108,5210³ J/mol;

166. Calculate ΔU under standard conditions for reaction: C₂H₂+2H₂O_(ж) → CH₃COOH_(ж)+H₂

at 298,2 К and 139,97 10³ J/mol:

1. 139,97 10³ J/mol;

2. 145,32 10³ J/mol;

3. 151,64 10³ J/mol;

4. 125,8610³ J/mol;

5. 108,5210³ J/mol;