Solutions Notes and MCQ

by | Aug 14, 2021 | CHEMISTRY

SOLUTIONS

Solutions MCQs

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Questions Option A Option B Option C Option D

1. The homogeneous mixture of two or more components is called a

Suspension Solution Heterogeneous mixture Adsorbtion

2. Solutions has

same composition throughout same property both 1 and 2 None

3. Almost all processes in our body occur in some kind of

Solid solution liquid solution Gaseous solution None

4. Brass is a solution of

Cu and Zn Cu, Zn and Ni Cu and Tin None

5. German silver is a solution of

Cu and Zn Cu, Zn and Ni Cu and Tin None

6. Bronze is a solution of

Cu and Zn Cu, Zn and Ni Cu and Tin None

7. Solution consist of

Solute  and solvent Solute and absorbant Solvent and another solvent Solute and another solute

8. Cocacola is a

Solution Suspension Colloid None

9. The component present in large quantity in solution is called

Solute Solvent Ellutant Pollutant

10. The component present in small quantity in solution is called

Solute Solvent Ellutant Pollutant

11. Solutions can be expressed

Qualitatively Quantitatively both 1 and 2 None

12. Composition of a solution can be described by expressing its

Weight Volume Concentration None

13. Which of the following is not a quantitative way of expressing the solution?

ppm mole fraction W/W percentage Dilute

14. Which of the following is  a qualitative way of expressing the solution?

 Concentrated Dilute both 1 and 2 None

15. The ratio of the volume of component to the volume of solution multiplied by 100 is called its

 w/w pecentage v/v percentage w/v percentage Mole fraction

16. The ratio of the mass of component to the mass of solution multiplied by 100 is called its

 w/w pecentage v/v percentage w/v percentage Mole fraction

17. The ratio of the mass of component to the volume of solution multiplied by 100 is called its

 w/w pecentage v/v percentage w/v percentage Mole fraction

18. The number of moles of solute divided by the total number of moles of solution is it’s

 Molarity Molality Mole fraction Mass percentage

19. Million times the number of parts of component to divided by total number of parts of all component in the solution is called

 ppm mole fraction w/v percentage None

20. The number of moles of solute present in one litre of solution is called

 ppm Mole fraction w/v percentage Molarity

21. The number of moles of solute present per kg of solvent is called it’s

 Molarity Molality Mole fraction None

22. Irrespective of the solute when the solvent is a gas, the solution is a

 Liquid solution Solid solution Gaseous solution None

23. Irrespective of the solute when the solvent is a liquid, the solution is a

 Liquid solution Solid solution Gaseous solution None

24. Irrespective of the solute when the solvent is a solid, the solution is a

 Liquid solution Solid solution Gaseous solution None

25. Oxygen dissolved in water is an example of which type of solution ?

 Gas-liquid Gas-solid Solid-liquid Liquid-gas

26. Alcohol dissolved in water is an example of which type of solution ?

 Gas-liquid Liquid-liquid Solid-liquid Liquid-gas

27. NaCl in water is an example of which type of solution ?

 Gas-liquid Liquid-liquid Solid-liquid Liquid-gas

28. Dust particles in air is an example of which type of solution ?

 Gas-liquid Solid-gas Solid-liquid Liquid-gas

29. Water vapour in air is an example of which type of solution ?

 Liquid-gas Solid-gas Solid-liquid Solid-solid

30. Mixture of oxygen and nitrogen is an example of which type of solution ?

 Liquid-gas Solid-gas Solid-liquid Gas-gas

31. Hydrogen in palladium is an example of which type of solution ?

 Gas-liquid Gas-solid Solid-liquid Gas-gas

32. Zinc-amalgam is an example of which type of solution ?

 Gas-liquid Gas-solid liquid-solid Gas-gas

33. Copper dissolved in gold is an example of which type of solution ?

 Gas-liquid Solid-solid liquid-solid Gas-gas

34. Which of the following concentration of Flouride ion in water prevents tooth decay ?

 1 ppm 1.5 ppm 2ppm 5ppm

35. Which of the following concentration of Flouride ion in water causes tooth to become mottled ?

 2 ppm 1.5 ppm 2ppm 5ppm

36. High concentration of flouride ion

 Prevent tooth decay Causes mottling of tooth is poisonous None

37. Which of the following is used in rat poison ?

 NaCl NaF NaBr NaI

38. The solution containing two components only is called a

 Binary solution Diary solution Ternary solution Quaternary solution

39. The number of components present in a binary solution is called

 1 2 3 4

40. The number of components present in a binary solution is called

 1 2 3 4

41. What is the unit of mass percentage ?

 kg L Mole Unit less

42. What is the unit of volume percentage ?

 kg L Mole Unit less

43. The sum of the mole fractions of all the components of a solution is

 1 1.5 0.5 2

44. The mole fraction of solute in a solution is generally

 >1 <1 1 2

45. The mole fraction of solvent in a solution is generally

 >2 <2 1 2

46. Mole fraction is generally denoted by the symbol

 s x y z

47. Molarity is denoted by

 m x M z

48. Molality is denoted by

 m s M y

49. Unit of molarity is

 mole per litre mole per kg Mole Litre

50. Unit of molality is

 mole per litre mole per kg Mole Litre

51. What is the volume percentage of solution containing 10ml of solute in 40ml of solvent ?

 10 percent 15 percent 20 percent 25 percent

52. What is the mass percentage of solution containing 80g of solute in 240g of solvent ?

 10 percent 16 percent 21 percent 25 percent

53. What is the mass by volume percentage of a solution of 10g sugar dissolved in 200 ml of solution ?

 5 percent 10 percent 20 percent 40 percent

54. What is the mole fraction of ethylene glycol in its 20 percent by mass solution in water ?

 0.932 0.048 0.068 0.052

55. Find the mole fraction of water in above solution.

 0.932 0.048 0.068 0.052

56. Find the molarity of a solution of 10g NaOH in 450ml solution.

 .278 mole per dm cube .556 mole per dm cube .45 mole per dm cube .1 mole per dm cube

57. Find the molality of a solution of 2.5g of ethanoic acid in 75g of benzene.

 .256 mole per kg .556 mole per kg .444 mole per kg None

58. The maximum amount of a substance that can be dissolved in specified amount of solvent at contant T and P is its

 Solubility Affinity Mole fraction None

59. Polar solute mostly dissolve in

 Polar solvent Non-polar solvent Both 1 and 2 None

60. Non-polar solute mostly dissolve in

 Polar solvent Non-polar solvent Both 1 and 3 None

61. Like dissolves

 Like Unlike Both perfectly None

62. What is the process called when a added solute get dissolved in solvent increasing its concentration ?

 Crystallization Dissolution Equillibrium None

63. When equillibrium is established , the relation between the rate of crystallization(Rc) and rate of dissolution(Rd) is

 Rc=Rd Rc < Rd Rc > Rd Rc = 2Rd

64. A solution in which no more solute can be dissolved at that T and P is called

 Saturated solution Unsaturated solution Ideal solution None

65. A solution in which more solute can be dissolved at that T and P is called

 Saturated solution Unsaturated solution Ideal solution None

66. The concentration of solute in a saturated solution is called its

 Permeability Solubility Both 1 and 2 None

67. The solubility depends on

 Nature of solute Nature of solvent Temperature All the above

68. When dissolution process is endothermic, then on increasing temperature solubility

 Increases Decreases Remain the same can’t be said

69. Which of the following can’t be dissolved in benzene ?

 Sugar NaCl Both 1 and 2 Naphthalene

70. Which of the following can be dissolved in water ?

 Sugar NaCl Both 1 and 2 None

71. When dissolution process is exothermic, then on increasing temperature solubility

 Increases Decreases Remain the same can’t be said

72. Which of the following doesn’t have significant effect on solubility of solids in liquids ?

 Nature of solute Nature of solvent Temperature Pressure

73. 6mg of oxygen is dissolved in 1litre water, calculate in ppm unit.

 5 ppm 6 ppm 7 ppm 3 ppm

74. Solubility of gases in liquid is greatly effected by

 Pressure only Temperature only Both 1 and 2 None

75. With increase of pressure , the solubility of gas in liquid

 Increases Decreases Remain the same can’t be predicted

76. What is the unit of mass by volume percentage ?

 g/ml L Kg Metre

77. What is the unit of mole fraction ?

 Mole Mole per litre 1/Mole Unit less

78. Who was the first to give a quantitative relationship between pressure and solubility of a gas in a solvent ?

 De Broglie Raoult Henry Newton

79. The solubility of a gas in a liquid is directly proportional to the pressure of the gas. This is called as

 Henry’s law Newton’s law Einstein’s law None

80. In which of the following solution Henry’s law is a special case of Raolt’s law ?

 Ethanol in water Oxygen in water water in milk none

81. The graph between the partial pressure of the gas and the mole fraction of gas in solution is a

 Circle Parabola Straight line Constant

82. When a highly volatile solute dissolves in a non-volatile solvent, then

 Henry law is dominant Raoult’s law is dominant Insuffient data none

83. At the same temperature the values of Henry’s law constant for different gases is

 Same Different can’t be predicted Have no relation to T.

84. Higher the value of Henry’s law constant for a given pressure, the solubility of gas in the liquid is

 Higher Lower Remain the same None

85. With decrease of temperature, the solubility of gases in liquid

 Increases Decreases Remain the same can’t be predicted

86. People living in high altitudes generally develop a symptom due to low oxygen concentration known as

 Anoxia Acne Axis Proximata

87. The partial pressure of each component in volatile liquid solution is directly proportional to its mole fraction. This is called

 Henry’s law Raoult’s law Newton’s law None

88. The graph between the total vapour pressure of liquid solution and mole fraction of its solvent is a

 Straight line Quadratic equation Parabola None

89. Under equillibrium condition the pressure exerted by the vapours of the liquid over the liquid phase is called

 Vapour pressure Critical pressure Atmospheric pressure None

90. In a solution of non-volatile solute and volatile solvent, the vapour pressure of the solution is due to

 Solute only Solvent only Both 1 and 2 None

91. Solutions which obey Raoult’s law over the entire range of concentration are known as

 Raoult solution Non ideal solution Ideal solution All the above

92. Solutions which do not obey Raoult’s law over the entire range of concentration are known as

 Raoult solution Non ideal solution Ideal solution All the above

93. Compare to the vapour pressure of pure solvent, the vapour pressure of the solution is

 More Less Both are equal None

94. For an ideal solution the enthalpy of mixing of the pure components to form the solution is

 Positive Negative Zero None

95. For an ideal solution the volume of mixing of the pure components to form the solution is

 Positive Negative Zero None

96. The decrease in the vapour pressure of the solvent depends on

 Nature of solute Nature of solvent Quantity of solute All the above

97. The ratio between the decrease in the vapour pressure of water on adding one mole of sucrose to that on adding one mole urea is

 1 4 6 Can’t be predicted

98. Liquid-liquid solutions can be classified into ideal and non-ideal solutions on the basis of

 Henry’s law Raoult’s law Newton’s law None

99. Solution of benzene and toluene is

 Ideal solution Non ideal solution Both 1 and 2 None

100. The ratio between the A-B type of interaction and A-A and B-B type of interaction in an ideal solution is

 more than one nearly 1 less than one more than 2

101. Which of the following solution is not an ideal solution ?

 n-hexane and n-heptane Benzene and Toluene Bromoethane and Chloroethane Chloroform and acetone

102. As compare to the prediction by Raoult’s law the vapour pressure of a non-ideal solution is

 Lower Higher May be lower or higher Equal

103. Solution with higher vapour pressure than expected by Raoult’s law are called

 Negative deviation Positive deviation No deviation All the above

104. Solution with lower vapour pressure than expected by Raoult’s law are called

 Negative deviation Positive deviation No deviation All the above

105. Compare to graph predicted by Raoult’s law the graph of vapour pressure vs mole fraction for a solution with positive deviation

 Will lie above Lie below Lie in the same line None

106. Compare to graph predicted by Raoult’s law the graph of vapour pressure vs mole fraction for a solution with negative deviation

 Will lie above Lie below Lie in the same line None

107. Mixture of ethanol and acetone is an example of _______ deviation from Raoult’s law.

 Positive Negative No All the above

108. Which of the following is not a non ideal solution ?

 Bromoethane and chloroethane Chloroform and acetone Carbon disulphide and acetone All the above

109. The A-B interactions are weaker than those between A-A or B-B in

 Positive deviation Negative deviation No deviation All the above

110. The A-B interactions are stronger than those between A-A or B-B in

 Positive deviation Negative deviation No deviation All the above

111. The binary mixture having the same composition in liquid and vapour phase and boil at a constant temperature are called

 Isotopes Azeotropes Allotropes Boltrope

112. The azeotropes can be separated by

 Extractive distillation Fractional distillation Chromatography both 2 and 3

113. How many types of azeotropes are there ?

 1 2 3 4

114. At a specific composition solutions which show a large positive deviation from Raoult’s law are

 Minimum boiling azeotropes Maximum boiling azeotropes Both 1 and 2 None

115. At a specific composition solutions which show a large positive deviation from Raoult’s law are

 Minimum boiling azeotropes Maximum boiling azeotropes Both 1 and 2 None

116. _______ pecentage by volume of ethanol in water is an azeotrope composition.

 80 85 5 95

117. Nitric acid and water can form

 Minimum boiling azeotropes Maximum boiling azeotropes Both 1 and 2 None

118. The percentage composition of nitric acid and water in its azeotrope form are

 68 and 32 by mass 32 and 68 by mass 42 and 58 by volume 56 and 44 by volume

119. The boiling point of azeotrope formed  by nitric acid and water is

 293.5 K 393.5 K 493.5 K 593.5 K

120. The properties which depends on the number of solute particles in solution, irrespective of their nature are called

 Chemical properties General properties Colligative properties All the above

121. With respect to solvent, which of the following is not a colligative property ?

 Relative lowering of vapour P. Depression of freezing point Elevation of boiling point Relative increase in vapour P

122. The word ‘colligative’ is a

 Latin word Greek word American word French word

123. The lowering of vapour pressure of solution depends on

 Nature of solute Nature of solvent Quantity of solute None

124. In a binary solution of solid in liquid the relative lowering of vapour pressure is equal to

 Mole fraction of solute Mole fraction of solvent Volume of solution None

125. For a very dilute solution, the relation between relative lowering of vapour pressure and  weight of the solvent is

 Directly proportional Directly vary as square of it Inversely vary as cube of it Inversely proportional

126. For a very dilute solution, the relation between relative lowering of vapour pressure and molecular weight of the solute is

 Directly proportional Directly vary as square of it Inversely vary as cube of it Inversely proportional

127. The ratio between the atmospheric pressure and vapour pressure of a liquid at its boiling point is

 One Two Zero Infinite

128. What is the boiling point of water ?

 100 K 173 K 273.15 K 373.15 K

129. Latin meaning of colligative is

 Bind together Come here Divide Move faster

130. The vapour pressure of water at its boiling point is

 1.013 bar 2.026 bar 5 atm 10 atm

131. The boiling point of the pure solvent is always ________ the boiling point of solution.

 Greater than Less than Equal to Half

132. The boiling point of a solution of one mole of sucrose in 1kg of water is

 100 K 273.15 K 373.15 K 373.52 K

133. Boiling point of a solution depends on the

 Number of solute molecules Volume of solution Nature of solute All the above

134. For dilute solutions, the elevation of boiling point is directly proportional to

 It’s molarity It’s molality It’s Normality All the above

135. The constant of proportionality in the expression of elevation in boiling point is called

 Cryoscopic constant Ebullioscopic constant Molar depression constant None

136. The constant of proportionality in the expression of depression of freezing point is called

 Cryoscopic constant Ebullioscopic constant Molar depression constant Both 1 and 3

137. The elevation in boiling point of solution is directly proportional to the

 Weight of the solute Molecular mass of solute Weight of the solvent None

138. The elevation in boiling point of solution is inversely proportional to the

 Molecular mass of the solvent Molecular mass of solute Weight of the solvent both 2 and 3

139. 18g of sucrose is dissolved in 1kg of water. What is the boiling point of solution, given Kb of water is 0.52 K kg per mole?

 373.15 K 370.15 K 373.202 K 100.052 K

140. The depression in the freezing point of the solution is directly proportional to it’s

 Molarity Molality Normality None

141. The elevation in boiling point of solution is independent of

 Nature of solute Number of moles of solute Quantity of solute All the above

142. The lowering of vapour pressure of solution causes ________ in the f p compare to that of the pure solvent.

 Increase Decrease Uneffected None

143. The unit of Kb is

 K kg per mole K kg mol K mol per kg Mole per kg per Kelvin

144. The unit of Kf is

 K kg per mole K kg mol K mol per kg Mole per kg per Kelvin

145. The unit of elevation of boiling point is

 K kg per mole K Mole per kg kg per K

146. The unit of depression of freezing point is

 K kg mole K Mole per kg Unitless

147. The unit of relative lowering of vapour pressure is

 Bar atm Both 1 and 2 Unitless

148. The relation between Kb and enthalpy of vapourisation is

 Directly proportional Inversely proportional Vary as square of it None

149. The relation between Kf and enthalpy of fusion is

 Directly proportional Inversely proportional Vary as square of it None

150. The relation between Kb and boiling point of the pure solvent is

 Directly proportional Inversely proportional Vary as square of it None

151. The relation between Kf and freezing point of the pure solvent is

 Directly proportional Inversely proportional Vary as square of it None

152. 45g of ethylene glycol  is  mixed with 600g of water. What is the freezing point depression ?

 2.2 K 272.95 K 100.2 K 102.2 K

153. 45g of ethylene glycol  is  mixed with 600g of water. What is the freezing point of the solution ?

 2.2 K 272.95 K 100.2 K 102.2 K

154. Wilted flowers revive when placed in fresh water. It is due to

 Diffusion Osmosis Guttation Adsorbtion

155. The process of movement of solvent from dilute solution to concentrated solution through a semipermeable membrane is called

 Osmosis Guttation Diffusion Adsorbtion

156. The pressure that just stops the flow of solvent moving due to osmosis is called

 Osmotic pressure Atmospheric pressure Critical pressure None

157. The flow of solute from concentrated region to dilute region is called

 Osmosis Guttation Diffusion Adsorbtion

158. In osmosis, the direction of movement of solvent molecule is

 From low to high concentration From high to low concentration To same concentration region All the above

159. Blood cells collapse when suspended in saline water due to

 Diffusion Osmosis Guttation Adsorbtion

160. Osmotic pressure depends upon the

 Number of solute molecules Nature of solute Both 1 and 2 None

161. For a dilute solution at a given temperature, the osmotic pressure is proportional to the

 Molarity of solution Molality of solution Normality of solution None

162. Osmotic pressure is equal to

 CRT 2CRT 3.14RT 3/2RT

163. The relation between molecular mass of solute and osmotic pressure of the solution is

 Directly proportional Inversely proportional Vary as square of it Have no relation

164. On increasing the temperature the osmotic pressure of a given solution

 Increase Decrease Remain the same None

165. Molar masses of polymers and other macromolecules are better measure by

 Elevation in b p method Depression of f p method Osmotic pressure method None

166. Molecular mass of solute of a solution can be determined from its

 Elevation in boiling point Depression in Freezing point Osmotic pressure All the above

167. Two solutions having same osmotic pressure at a given temperature are called

 Isotopic solution Isotonic solution Hypotonic solution Hypertonic solution

168. Two solutions with same osmotic pressure are joined by a semipermeable membrane, the solvent moves from

  Solution with high volume Solution with less volume No movement occur None

169. The osmotic pressure associated to the fluid inside the blood cell is equivalent to which solution?

 0.5 percent W/V NaCl solution 0.6 percent W/V NaCl solution 1.2 percent W/V NaCl solution 0.9 percent W/V NaCl solution

170. Solvent of blood cell flow out when place in a

 Hypotonic solution Hypertonic solution Isotonic solution All the above

171. Solvent of solution flow into the blood cells when it is place in a

 Isotopic solution Hypertonic solution Hypotonic solution Isotonic solution

171. People taking lot of salt in diet have

 Typhoid Goiter Edema Malaria

172. The process used in desalination of sea water is

 Adsorbtion Diffusion Osmosis Reverse osmosis

173. When there is a dissociation of solute into ions, the experimental value of molar mass is

 Higher than true value Lower than true value Twice the true value Equal to the true value

174. When there is a association of solute, the experimental value of molar mass is

 Higher than true value Lower than true value Twice the true value Equal to the true value

175. The molar mass we get due to dissociation or association of molecule is called

 Normal molar mass Common molar mass Abnormal molar mass True molar mass

176. Who introduced the factor I in abnormal colligative properties ?

 Dalton Henry Raoult Van’t Hoff

177. Which factor account for the extent of association or dissociation of molecule in solution ?

 Van’t Hoff factor Henry’s constant Raoult’s factor Avogadro’s number

178. Van’t Hoff factor is denoted as

 i J K mol per kg x

179. When did van’t Hoff introduced van’t Hoff’s factor ?

 In 1880 In 1980 In 1800 In 1899

180. The ratio between normal molar mass by abnormal molar mass is

 Van’t Hoff factor Factor i Extent of association All the above

181. The ratio between calculated colligative properties and observed colligative properties is

 Van’t Hoff factor 1/van’t Hoff factor 2* van’t Hoff factor Square of van’t Hoff factor

182. The ratio between the number of moles of particles before dissociation/association to that after dissociation/association is

 Frequency factor Van’t Hoff factor 1/van’t Hoff factor None

183. The study of conversion of electrical energy to chemical energy and chemical energy to produce electricity is called

 Electricity Chemical equillibrium Electrochemistry Electrostatics

184. Batteries convert

 Chemical to electrical energy Electrical to chemical energy Chemical energy to heat Chemical energy to light

185. Reactions carried out electrochemically can be

 Ecofriendly Energy efficient Less polluting All the above

186. The transmission of sensory signals through cells to brain have

 Electrochemical origin chemical origin Electical origin None

187. The Zn/Cu cell that convert chemical energy to electrical energy is called as

 Daniel cell electrolytic cell Photovoltaic cell All the above

188. Fuel cells convert

 Chemical to electrical energy Electrical to chemical energy Chemical energy to heat None

189. The device that converts chemical energy to electrical energy is called a

 Galvanic cell Voltaic cell Both 1 and 2 electrolytic cell

190. The device that converts electrical energy to chemical energy is called a

 Galvanic cell Voltaic cell Both 1 and 3 electrolytic cell

191. In the Galvanic cell Gibbs energy of the spontaneous redox reaction is converted into

 Electrical work Heat Light Mechanical work

192. In the Daniel cell Zn is

 Oxidised Reduced Both 1 and 2 Remains  unaffected

193. In the Daniel cell Cu is

 Oxidised Reduced Both 1 and 3 Remains  unaffected

194. The electrolyte of the two half cells are connected internally through a

 Voltmeter Switch Salt bridge None

195. The electrolyte of the two half cells are connected externally through a

 Voltmeter Switch Both 1 and 2 Salt bridge

196. The potential difference develop between the electrode and the electrolyte is called

 Redox potential Oxidation potential Reduction potential Electrode potential

197. When the concentration of all the species involved in a half cell is unity then the electrode process is known as

 Standard electrode potential Oxidation potential Redox potential Electrode potential

198. According to IUPAC convention, which of the following is called as the standard electrode potential

 Reduction potential Oxidation potential Redox potential All the above

199. In a galvanic cell, the half cell in which oxidation takes place is called

 Anode Cathode Both 1 and 2 Electrode

200. In daniel cell, the reaction in which Cupric ion is converted to solid Cu is called

 Oxidation half reaction Reduction half reaction Redox reaction None

201. In daniel cell, the reaction in which solid Zn is converted to Zinc ion is called

 Oxidation half reaction Reduction half reaction Redox reaction None

202. In a galvanic cell, the half cell in which reduction takes place is called

 Anode Cathode Both 1 and 2 Electrode

203. With respect to the solution cathode has

 A positive potential A negative potential The same potential None

204. With respect to the solution Anode has

 A positive potential A negative potential The same potential None

205. The direction of flow of current and that of electron are

 7 Opposite Perpendicular to each other 45 degree to each other

206. The potential difference between the two electrodes of a galvanic cell is called the

 Cell potential Shell potential Redox potential Oxidation potential

207. The unit of potential difference is

 Ampere Volt Volt per ampere Volt square

208. The potential of a individual half cell is

 Zero Positive Negative Can’t be measured

209. Standard hydrogen electrode consist of

 Cu electrode Gold electrode Pt electrode Silver electrode

210. In SHE the pressure of hydrogen gas is maintained at

 One bar Two bar Zero bar 3 bar

211. In SHE the concentration of hydrogen ion is maintained at

 1 M Dilute 5 M 3 M

212. In SHE the electrode is dipped in

 A basic solution An acidic solution A neutral solution All the above

213. The standard electrode potential corresponding  to the reaction Cu2+ (aq, 1M) + 2e —> Cu(s) is

 0 V 0.34 V -0.76 1 V

214. The standard electrode potential corresponding  to the reaction Zn2+ (aq, 1M) + 2e —> Cu(s) is

 1 V 0.34 V -0.76 0 V

215. The standard electrode potential corresponding  to the reaction Cu2+ (aq, 1M) + 2e —> Cu(s) is

 2 V 0.34 V -0.76 0 V