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MDCAT Chemistry Electrochemistry Test Online

Malik TahirLast Updated: May 24, 2025

Chemistry Electrochemistry MCQS Online Test

MDCAT Chemistry Electrochemistry Chapter Online Test

Total Questions:	192
Time Allowed:	60 Minutes
Total Marks:	192
How to Attempt Test:	Please choose the right Option in MCQ-type question.
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MDCAT Chemistry Electrochemistry Test

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Page 1 of 8

Chemistry

1. Reaction takes place at anode is

Oxidation

Ionization

Reduction

Hydrolysis

2. Corrosion reactions are

Spontaneous redox reactions

Non-spontaneous redox reactions

None of these

Spontaneous acid–base reactions

3. Which of the following element act as inert electrode?

None

4. In the conversion of Br2 to BrO₃¯¹ the oxidation state of bromine changes from

1 to 5

0 to 5.

0 to –3

2 to 5

5. In electrolytic cell, electricity in carried out by

All

Non-spontaneous reaction

Neutralization

Spontaneous reaction

6. A solution of sodium sulphate was electrolyzed using some inert electrodes. The products at the electrodes are

None of these

O₂,H₂

O₂, SO₂

O₂, Na

7. Time required to deposit one millimole of aluminum metal by the passage of 9.65 amperes through molten electrolyte containing aluminum ion is

30 s

10,000 s

30,000 s

10 s

8. Anode electrode element always have _________ position in electrochemical series

Higher

In middle

Not particular

Lower

9. Partial pressure of a solution component is directly proportional to its mole fraction. This statement is known as

Henry’s law

Ostwald’s dilution law

Distribution law

Raoult’s law

10. Equal volumes of 0.1 M AgNO₃ and 0.2 M NaCl are mixed. The concentration of NO¯₃ ions in the mixture will be

0.05 M

0.1 M

0.15 M

0.2 M

11. If 5.85 g of NaCl are dissolved in 90 g of water, the mole fraction of NaCl is

0.1

0.0196

0.01

0.2

12. What will be the density of H₂SO₄ when lead accumulator is recharged?

1.25 cm¯³

1.81 cm¯³

1.15 cm¯³

2.15 cm¯³

13. What are the ions present in water?

H and OH

H+ and OH-

H2O

H2 and O

14. The temperature at which the vapour pressure of a liquid becomes equal to external pressure is

Inversion point

Boiling point

Melting point

Sublimation point

15. If 5.85 g of NaCl are dissolved in 90g of water, the mole fraction of NaCl is

0.2

0.01

0.1

0.0196

16. Half cells are interconnected through

Wire

Electric circuit

No connection exists

Salt Bridge

17. Calculate the amount of charge flowing in 2 minute in a wire of resistance 10 Ω when a potential difference of 20 V is applied

4 C

120 C

20 C

240 C

18. After adding a solute freezing point of solvent decreases to -0.186. Calculate ∆ Tb if Kf = 1.86 and Kb = 0.521

0.0521

1.86

0.0186

0.521

19. Solution with same osmotic pressures are called

Normal

Hypertonic

Isotonic

Hypotonic

20. Which of the following will have the highest boiling point at 1 atm pressure?

0.1 M NaCl

0.1 M BaCl₂

0.1 M Sucrose

0.1 M Glucose

21. The process of electrical coating of one metal on another to protect, decorate or to have a greater resistance to corrosion is called

Electroplating

Induction

Electrolysis

Conduction

22. Separation of azeotropic mixture into pure components is carried out by

Fractional distillation

None of these

Vacuum distillation

Distillation

23. The + 1 oxidation state of P is found in

H₃PO₂

H₄P₃O₇

H₃PO₃

H₃PO₄

24. The solubility of a gas in water depends upon

Temperature

All of these

Pressure of the gas

Nature of the gas

25. A cell constant is generally found by measuring the conductivity of aqueous solution of

MgCl₂

KCl

BaCl₂

NaCl

Page 2 of 8

26. The limiting molar conductivities ʌ’ for NaCl, KBr and KCl are 126, 152 and 150 S cm² respectively. The ʌ’ for NaBr is

302 S cm² mol¯¹

128 S cm² mol¯¹

176 S cm² mol¯¹

278 S cm² mol¯¹

27. Which of the following solution of H₂SO₄ is more concentrated?

1 normal

1 molar

1 molal

All

28. Choose the cell among the following list in which conversation of electrical energy into chemical energy takes place

Daniel cell

Electrolytic cell

Fuel cell

Galvanic cell

29. The conductivity of strong electrolyte

Decreases on dilution

Does not change on dilution

Depends on density of electrolyte itself.

Increases on dilution slightly

30. Which of the substances Na, Hg, S Pt and graphite can be used as electrodes in electrolytic cells having aqueous solution?

Pt and graphite only

Na, Pt and graphite

Na and S only

Na and Hg

31. Which one of the following substance when dissolved in water give acidic solution

NaCl

CH₃ CooNH₄

NH₄Cl

Na₂SO₄

32. Hydrogen gas is not liberated when the following metal is added to dil. HCI.

33. In electrolysis of NaCl when Pt electrode is taken then H₂ is liberated at cathode while with Hg cathode it forms sodium amalgam

Na is dissolved in Hg while it does not dissolve in Pt

More voltage is required to reduce H⁺ at Hg than at Pt

Conc. Of H⁺ ions is when Pt electrode is taken

Hg is more inert than Pt

34. Specific conductivity of a solution

Increases with dilution

Depends on mass of electrolyte

Decreases with dilution

Remains unchanged with dilution

35. When during electrolysis of a solution of AgNO₃, 9650 coulombs of charge pass through the electroplating bath, the mass of silver deposited on the cathode will be

108 g

10.8 g

21.6 g

1.08 g

36. A 0.001 molal solution of [Pt(NH₃)₄Cl₄] in water had a freezing point depression of 0.0054°C. If Kf for water is 1.80, the correct formulation for the above molecule is

[Pt(NH₃)₄Cl]Cl₃

[Pt(NH₃)₄Cl₄]

[Pt(NH₃)₄Cl₂]Cl₂

[Pt(NH₃)₄Cl₃]Cl

37. When electricity is passed through molten Al₂O₃ + Na₃AIF₆ and 13.5 gms of Al are deposited, the number of faraday must be

1.5

2.0

0.5

1.0

38. In a hydrogen-oxygen fuel cell, combustion of hydrogen occurs to

Generate heat

Remove adsorbed oxygen from electrode surfaces

Produce high purity water

Create potential difference between two electrodes

39. Voltaic cell can be recharged by

By addition of fresh solution

By removal of solution

By heating it

By replacing external circuit with external source of electricity

40. When a metal is dipped in 1 molar of its solution at 298k, then potential set up is called

Standard electrode potential

Electroplating

Ionization potential

Electric change

41. Which substances are mixed to form a buffer solution?

Strong acid and its salt of weak base

Weak acid and its salt of weak base

Weak acid and its salt of strong base

A strong acid and its salt of a strong base

42. Which of the following is the strongest oxidizing agent?

I₂

Pb²⁺

Ag⁺

43. The strength of solution an element whose electrode potential is to be measured

1 N

1 M

2 M

1 f

44. The best reducing agent is

Cl¯

I¯

F¯

Br¯

45. Calculate the percentage by weight if NaCl, if 2.0 g of NaCl is dissolved in 20g of water

11.2%

14.25%

9.09%

13.1%

46. 18g of glucose is dissolved in 90g of water. The relative lowering of vapour pressure is equal to

1/5

5.1

1/51

47. Choose the best reducing agent among the following

I¯¹

Br¯¹

F¯¹

Cl¯¹

48. The osmotic pressure of a dilute solution is directly proportional to the

Diffusion rate of the solute

Elevation in boiling point

Flow of solvent from a concentrated to a dilute solution

Ionic concentration

49. The substance having highest conductivity at room temperature among the following is

Glass

0.1 N HCl

Graphite

0.1 N NaCl

50. In alkaline battery the anode is made up of

AgO2

Cadmium

MnO2

Page 3 of 8

51. The cathodic reaction in the electrolysis of dil. H₂SO₄ with Pt electrodes is

Oxidation

Reduction

Neither oxidation and reduction

Both oxidation and reduction

52. Colligative properties are the properties of

Both a and b

Neither a nor b

Concentration solutions behave as nearly non – ideal solutions

Dilute solution which behave as nearly ideal solution

53. The ionic strength of a solution containing 0.1 mole/kg of KCl and 0.2 mole/kg of CuSO₄ is

0.6

0.2

0.9

0.3

54. Alkaline battery has a voltage of

4.5V

1.5V

3.5V

2.5V

55. Standard reduction electrode potential of three metals A, B and C are respectively + 0.05 V, - 3.0 and -1.2V. The reducing power of

B > C > A

A > C > B

C > B > A

A > B > C

56. At room temperature, the mole fraction of a solution in 0.25 and the vapour pressure of the solvent is 0.80 atm. Then the lowering of vapour pressure is

0.80

0.20

0.60

0.75

57. The specific conductance of 0.1 M NaCl solution is 1.06 x 10¯² ohm¯¹mol¯¹. Its molar conductance in ohm¯¹ cm² mol¯¹ is

1.06 x 10⁴

1.06 x 10²

1.06 x 10³

58. Potential of Zn is called

Redox

It has not potential

Oxidation

Reduction

59. Which oxide has +2 oxidation number of oxygen?

Na₂O₂

F₂O

Cl₂O

Na₂O

60. Mole fraction of pure water is

None of these

Exactly equal to one

Slightly greater than one

Slightly less than one

61. 1.0 g of pure calcium carbonate was found to require 50 ml of dilute HCl for complete reaction. The strength of HCl solution is given by

0.2 N

4 N

2 N

0.4 N

62. Electrolysis is the process in which a chemical reaction takes place at the expense of

None of these

Electrical energy

Chemical energy

Heat energy

63. Which of the following statement is correct for electrolytic cell?

Migration of ions along with oxidation reaction at anode and reduction reaction at cathode

Electrons flow from cathode to anode through the external battery

None of these

Electrons flow cathode to anode within the electrolytic solution

64. In galvanic cell Zn acts as an anode so its value of standard reduction potential in comparison to coupled electrode would be

Sum of reduction and oxidation potentials

Lesser

None

Greater

65. An electric current is passed through silver voltmeter connected to a water voltmeter. The cathode of the silver voltammeter is 0.108 g more at the end of the electrolysis. The volume of oxygen evolved at STP is

5.6 cm³

11.2 cm³

56 cm³

550 cm³

66. Electrochemical series is a list of elements arranged into increasing order to either

Cell voltage

Standard reduction potential

Standard oxidation potential

Ionization potential

67. The relative lowering of vapour pressure is equal to mole fraction of the solute. This law is called:

Raoult’s law

Henry’s law

Ostwald’s law

Arrhenius law

68. The pressure at which water boils at 101.5 °c is

760 mm of Hg

Slightly more than 1 atom

2.5 atom

750 torr

69. The volume of 0.1 M H₂SO₄ required to neutralize completely 40 ml of 0.2 M NaOH solution is

20 ml

80 ml

40 ml

10 ml

70. The osmotic pressure of 1 m solution at 27°C is

24.6 atm

12.1 atm

2.46 atm

1.21 atm

71. When Cu, Ag, Au and Pt are reacted with acids, these metals do not liberate hydrogen, this is due to the reason that

Very high positive value of reduction potential

Very high negative values reduction potential

Reduction potentials are negative

Very low ionization potential values

72. Electrode potential of Zn is

Depends on the nature of the coupled electrode

Oxidation

Oxidation-reduction

Reduction

73. If the salt bridge is not used between two half cells, then the voltage

Does not change

Decrease rapidly

Decreases slowly

Drops to zero

74. The vapour pressure of two liquids ‘P’ and ‘Q’ are 80 and 60 torr respectively. The total vapour pressure of solution obtained by mixing 3 mole of P and 2 mol of Q would be

140 torr

72 torr

68 torr

20 torr

75. An oxidizing agent in a chemical reaction in the substance which

Gains electrons

pH is changed

Acts as a catalyst

Loses electrons

Page 4 of 8

76. The EMF of the cell rection Fe²⁺ + zn = Zn²⁺ + feis

– 1.17 V

+ 1.17 V

– 0.35 V

+ 0.35

77. The art of electroplating was given by

Brugan

Edison

Thomas Gradam

Faraday

78. Salt bridge transfers

Current

Solvent particles

Anions

Electrons

79. 0.5 M of H₂SO₄ is diluted from 1 liter to 10 liter, normality of resulting solution is

10 N

11 N

0.1N

1 N

80. A smuggler could not carry gold by chemically depositing iron on the gold surface since

Gold has higher reduction potential then iron

Gold has lower reduction potential then iron

Iron rusts

Gold is denser

81. Wen quantity of electricity passed is one faraday then the mass deposited at the electrode is equal to

One gm. atomic weight

None of these

One gm. Equivalent weight

Electrochemical equivalent

82. In the electrolysis of molten sodium chloride, what is the yellow green gas formed?

Hydrogen

Chloride

Chlorine

Oxygen

83. Electricity in voltaic cell is produced due to

Oxidation

Reduction

Neutralization

B + C

84. Strong reducing agents have

Lesser positive value of standard reduction potential

None of these

Greater negative value of standard reduction potential

Greater positive value of standard reduction potential

85. The number of moles of a solute in 500 cm³, 3M solution is

1.5

86. If α is the degree of dissociation of Na₂SO₄ the Vant Hoff’s factor (i) used for calculating the molecular mass is

1 + 2 α

1 + α

1 – 2 α

1 – α

87. A solution contains 1.2046 x 10²⁴ hydrochloric acid molecules in one dm³ of the solution. The strength of the solution is

6 N

2 N

8 N

4 N

88. In a solution of CuSO₄ how much time will be required to precipitate 2g copper by 0.5 ampere current?

510 sec

12157.48 sec

102 sec

642 sec

89. Which one of the following is a colligative property?

Surface tension

Osmotic pressure

Refractive index

Viscosity

90. Pure water does not conduct electricity because it

Is almost unionized

Is readily decomposed

Is neutral

Has low boiling point

91. A certain current liberate 0.5 g of hydrogen in 2 h. How many grams of copper can be liberated by the same current flowing for the same time in a copper sulphate solution?

15.9 gm

63.5 gm

12.7 gm

31.8 gm

92. Oxidation number of carbon in NaHCO₃ is

-6

93. Which of the following is the use of electrolysis?

Both A and B

Electroplating

None of these

Electrorefining

94. Of the following, the metal that cannot be obtained by electrolysis of aqueous solution of their salts are:

95. Units of molarity are

Mol/lit

None of these

Gm/lit

Kg/lit

96. What is the molarity of H₂SO₄ solution that has density of 1.84 gm/cm³ which was at 35°C and contains 98% by weight?

4.18 M

18 M

8.14 M

18.4 M

97. When electricity is passed through molten electrolyte consisting of alumina and cryolite, 13.5 g of Al are deposited. The number of faradays of electricity passed must be

1.5

1.0

2.0

0.5

98. How many g of dibasic acid (mol. wt. 200) should be present in 100 ml of the aqueous solution to give 0.1 Normality?

1 g

20 g

10 g

2 g

99. Molton NaCl conducts electricity due to the presence of

Free molecules

Free electrons

Atoms of Na and Cl.

Free ions

100. The molality of 2% NaCl. W/W solution is approximately

0.05

0.25

0.5

2.05

Page 5 of 8

101. Which of the following (IM) conducts more electricity?

Nitric acid

Phosphorus acid

Sulphuric acid

Boric acid

102. Maximum freezing point falls in

Benzene

Naphthalene

Camphor

Water

103. H₂ gas in SHE is filled at a pressure of

800 mm of Hg

760 mm of Hg

780 mm of Hg

750 mm of Hg

104. Which of the following statements is FALSE?

Reduction occurs at cathode

All voltaic (galvanic) cells involve the use of electricity to initiate nonspontaneous chemical reactions

All electrochemical reactions involve the transfer of electrons

Oxidation and reduction half-reactions occur at electrodes in electrochemical cells.

105. An electrolyte

Gives ions only when dissolved in water

Forms complex ions in solution

Gives ions only when electricity is passed

Possesses ions even in solid state

106. When common salt is dissolved in water

B.P of water decrease

Any possibility

B.P of water increase

B.P of water remain constant

107. Li occupies higher position in the electrochemical series of metals as compared to Cu since

Li is smaller in size as compared to Cu

The standard oxidation potential of Li/Li⁺ is lower than that of CuCu²⁺

The standard reduction potential of Cu²+/Cu is lower than that of Li⁺/Li

The standard reduction potential of Li⁺/Li is lower than that of Cu²+/Cu

108. Secondary cell is

Daniel cell

Non rechargeable

Rechargeable

Electrolytic cell

109. If liquids A and B form an ideal solution

The free energy of mixing is zero

The enthalpy of mixing is zero

The free energy as well as the entropy of mixing are each zero

The entropy of mixing is zero

110. 8 g of NaOh is dissolved in 500 cm³ of solution, its molarity is:

0.04 M

0.8 M

0.2 M

0.4 M

111. 96500 C electricity is passed through CuSO₄. The amount of copper precipitated is

1.0 mole

0.5 mole

2.00 mole

0.25 mole

112. By means of fuel cells, chemical energy may be converted into

Electrical energy

Magnetic energy

Heat energy

Sound energy

113. Temperature for standard electrode potential is

25 C°

300 K

273 K

310 K

114. The standard e.m.f. of a galvanic cell involving cell reaction with n = 2 is found to be 0.295 V at 25°C. The equilibrium constant of the reaction would be

1.0 x 10²

2.0 x 10¹¹

4.0 x 10¹²

1.0 x 10¹⁰

115. In alkaline battery anode is made up of

Cadmium

MnO₂

AgO₂

116. The weight of pure NaOH required to prepare 250 cm³ of 0.1 N solution is

4 g

5 g

1 g

2 g

117. The Vant Hoff factor (i) accounts for

The extent of dissolution of solute

The extent of dissociation of solute

Degree of solubilization of solute

The degree of decomposition of solution

118. Prevention of corrosion of iron by Zn coating is called

Photo electrolysis

Electrolysis

Galvanization

Cathodic protection

119. If a salt bridge is removed between the two half cells, the voltage

Drops to zero

Increases gradually

Does not change

Increases rapidly

120. The unit of specific conductivity is

Ohm¯¹ cm

Ohm¯¹ cm¯¹

Ohm cm¯¹

Ohm cm¯²

121. The cryoscopic constant of water is 1.86. The elevation of B.P for a 0.1m solution of a solute in water is

0.186 c°

18.6 c°

1.86 c°

Sufficient date not given

122. Corrosion is basically a

Interaction

Electrochemical phenomenon

Union between two light metals and a heavy metal

Altered reaction in presence of H₂O

123. If 18 g of glucose (C₆H₁₂C₆) is present in 1000 g of an aqueous solution of glucose it is said to be

0.1 molal

1.1 molal

0.5 molal

1 molal

124. It azeotropic mixture showing positive deviation from Rault’s law, the volume of the mixture is

Slightly more than the total volume of the components

None of these

Slightly less than the total volume of the components

Equal to the total volume of the components

125. For spontaneity of a cell, which is correct?

∆ G = +ve, ∆ E = 0

∆ G = -ve, ∆ E = 0

∆ G = 0, ∆E = 0

∆ G = -ve

Page 6 of 8

126. In a chemical reaction, oxidation process involves

Increase in oxidation number of the elements in reactants

Oxidation number neither increases nor decreases

Decrease in oxidation number of element

Increase in oxidation number of element

127. The amount of electricity that can deposit 108 g of silver from silver nitrate solution is

1 coulomb

1 ampere

2 ampere

1 faraday

128. Same amount of electric current is passed through solution if AgNO₃ and HCl. If 1.08 g of silver is obtained in the first case, the amount of hydrogen liberated as S.T.P. in the second case is:

1.008 g

22400 cm³

224 cm³

112 cm³

129. What will be the weight of deposited silver on passing 965 coulombs of electricity in solution of AgNO₃?

2.16 g

0.54 g

1.08 g

0.27 g

130. Out of Cu, Ag, Fe and Zn the metal which can displace all others from their salt solutions is

131. Under the process of rusting of iron, 4Fe + 3O₂ → 2Fe₂O₃, iron is

Precipitated

Hydrolyzed

Reduced

Oxidized

132. Density of H₂SO₄ in lead accumulator is

120 g Cm³

1.25g/Cm³

1.15 g/Cm³

1.2 g/Cm³

133. Conductivity (Unit : siemen’s S) is directly proportionally to the area of the vessel and the concentration of the solution in it and is inversely proportional to the length of vessel, then the unit of constant of proportionality is

S² m² mol¯²

S² m² mol

S m mol¯¹

S m² mol¯¹

134. An aqueous solution of ethanol in water has vapour pressure

Less than that of water

More than that of H₂O

Equal to that of water

Equal to that of ethanol

135. Azeotropic mixture of HCl and water has

22.2% HCl

20.2% HCl

48% HCl

36% HCl

136. During a redox reaction, an oxidizing agent

Gains electrons

Is hydrolysed

Loses electrons

Is oxidized

137. A cell in which chemical energy is converted into electrical energy is called

Galvanic cell

Dry cell

Electrolytic cell

Fuel cell

138. Pick out the wrong statement. In electrochemical cell

Chemical energy is converted into electrical energy

Salt bridge maintains the electrical neutrality of the solution

Electrons are released at anode

Cathode is regarded as negative electrode

139. In an electrolytic cell current flows

From anode to cathode in an outer circuit

From anode to cathode inside the cell

From cathode to anode in outer circuit

From cathode to anode inside the cell

140. When the solute is present in trace quantities the following expression is used?

Gram per million

Milligram percent

Microgram percent

Parts per million

141. Salt bridge transfers

Current

Electrons

Ions

Anion

142. The standard EMF of Daniel cell is 1.10 volt. The maximum electrical work obtained from the Daniel cell is

212.3 kJ

106.15 kJ

175.4 kJ

53.07 kJ

143. If the ionic product of a solution is less than the solubility product, the solution is

Supersaturated

Saturated

Ideal

Unsaturated

144. A current of 9.65 ampere flowing for 10 minutes deposits 3.0 g of the metal which is monovalent. The atomic mass of the metal is

96.5

145. A redox reaction involves

Ion combination reaction

Electron transfer

Proton transfer

A reaction in a solution

146. The half-reaction that occurs at the anode during the electrolysis of molten sodium bromide is:

2Br– → Br₂ + 2e –

Na⁺ + e– → Na

Na → Na⁺ + e–

Br₂ + 2e – → 2Br –

147. Decrease in oxidation number is called

Oxidation

All of these

Redox

Reduction

148. The degree of dissociation of weak electrolyte increases as

Dilution increases

None

Pressure increases

Dilution decreases

149. Stronger the oxidizing agent, greater is the

e.m.f of cell

Oxidation potential

Redox potential

Reduction potential

150. Standard hydrogen electrode has an arbitrarily fixed potential

1.00 volt

0.00 volt

None of these

0.10 volt

Page 7 of 8

151. Density of H₂SO₄ in lead accumulator is

1.15g/cm3

1.3g/cm3

1.20g/cm3

1.25g/cm3

152. Chemical used in salt bridge is

KOH

KBr

KCI

KNO3

153. Which of the statements given below concerning properties of solution, describe a colligaive effect?

Vapour pressure of pure benzene decreases by the addition of naphthalene

Vapour pressure of pure water decreases by the addition of nitric acid

Boiling point of pure benzene increases by the addition of toluene

Boiling point of pure water decreases by the addition of ethanol

154. Metals usually conduct electricity because

Metals are decomposed by current

In metals the ions are free to more

They are mobile electrons in the metallic structure

Metals have high resistance

155. How much of NaOH is required to neutralize 1500 cm³ of 0.1 N HCl?

60 g

40 g

6 g

4 g

156. Which of the following is a strong electrolyte?

HCN

NH₄OH

CH₃COOH

Ca(NO₃)₂

157. A solution contains A, B and C components. The mole fraction A and C are 0.25 and 0.35 respectively. The mole fraction B will be

0.30

0.35

0.40

0.25

158. Oxidation in a chemical reaction involves

Decrease in oxidation number

Increase in oxidation number

Increase in oxidation number of all the elements on reactant side

Both are possible

159. The reference calomel electrode is made from which of the following?

HgCl₂

ZnCl₂

Hg₂Cl₂

CuSO₄

160. Best way to prevent rusting iron is by

None of these

Both of these

Putting it in saline water

Making iron cathode

161. The specific conductance of a 0.1 N KCl solution at 23°C is 0.012 ohm¯¹ cm¯¹. The resistance of cell containing the solution at the same temperature was found to be 55 ohm. The cell constant will be

1.12 cm¯¹

0.142 cm¯¹

0.918 cm¯¹

0.66 cm¯¹

162. The molarity of the solution containing x grams (NH₄)SO₄ in 500 cm³ of the solution is 0.6. What is x

39.6

42.7

45.1

40.5

163. Camphor is often used in molecular mass determination because

It is solvent for organic substances

It has a very high cryoscopic constant

It is readily available

It is volatile

164. A 20% solution of NaCl by weight means that

10.0g NaCl/100ml

58.5g NaCl/100ml

5.58g NaCl/100m

20g NaCl/100ml

165. Molarity of water is

55.5

166. Oxidation state of hydrogen in CaH₂ is

-1

-2

167. 2.5 faradays of electricity is passed through solution of CuSO₄. The number of gram equivalents of copper deposited on the cathode would be

1.25

None of these

1 2

2.5

168. What is the molality of a solution prepared by dissolving 5 g of toluene in 250 g of Benzene.

7.20

3.12

4.10

0.217

169. Cathode provides electrons to

Does not provide any electron

Neutral atom

-Ve ion

+Ve ion

170. The number of coulombs required for the deposition of 107.870 g of silver is

193000

10000

48250

96500

171. In a Galvanic cell

Chemical energy is converted into electricity

Electrical energy is converted into heat

Electrical energy is converted into chemical energy

Chemical energy is converted into heat

172. The electrode with more negative value of reduction potential acts as

None of these

Cathode

Electrode

Anode

173. When molten sodium undergoes electrolysis, the ion reduces is

Both Na⁺ and CI¯

Na⁺

Cl¯

None of these

174. Equal volumes of ethylene glycol (molar mass = 62) and water (molar mass = 18) are mixed. The depression in freezing point of water is (given Kf of water 1.86 K mol¯¹ kg and specific gravity of ethylene glycol is 1.11)

33.3

0.333

3.33

0.0033

175. 50 mL of 10 N H₂SO₄. 25 mL of 12 N HCl and 40 mL of 5N HNO₃ are mixed and the volume of the mixture is made 1000 mL by adding water. The normality of resulting solution will be

1 N

2 N

3 N

9 N

Page 8 of 8

176. Which of these is not an application of electrolysis?

Manufacture of bleach

Making leather

Rust removal

Electroplating

177. A dry alkaline cell has porous Zn anode & MnO₂ as cathode the electrolyte used is

NH₄OH

Ca(OH)₂

KOH

NaOH

178. An electric current is passed through silver nitrate solution using silver electrodes. 10.79 g of silver was found to be deposited on the cathode if the same amount of electricity is passed through copper sulphate solution using copper electrodes, the weight of copper deposited on the cathode is

6.4 g

12.8 g

2.3 g

3.2 g

179. In a Galvanic cell, the electrons flow from

Cathode to anode through the external circuit

Anode to cathode through the external circuit

Anode to cathode through the solution

Cathode to anode through the solution

180. Reduction always occurs

Both A and B

None of these

At anode

At cathode

181. Sea water has 5.65 x 10¯³ g of dissolved oxygen calculate the conclusion of oxygen in sea water in ppx

6.1

5.51

5.65

1.32

182. The reference electrode is made by using

HgCl₂

ZnCl₂

Hg₂Cl₂

CuSO₄

183. A device which converts electrical energy into chemical energy is called

An electrolytic cell

A galvanic cell

A chemical cell

A voltaic cell

184. Which one of the following will be good conductor of electricity?

Molten NaCl

Chloroform

Dilute solution of glucose

Pure distilled water

185. If the standard electrode potential of CU²⁺/Cu electrode is 0.34 V, what is the electrode potential of 0.01 M concentration of Cu²⁺? (T = 298 K)

0.281 V

0.176 V

0.399 V

0.222 V

186. Cathodic reaction in the electrolysis of dil. H₂SO₄ is always

Reduction

Oxidation

Reduction

Both

187. 96500 C of electricity liberates from CuSO₄ solution

31.75 g of Cu

100 g of Cu

96500 g of CU

63.5 g of Cu

188. The depression of freezing point is directly proportional to

Molarity of the solution

Molality of the solution

Molarity of the solvent

Mole fraction of the solution

189. Which has maximum oxidation number

190. An aqueous solution freezes at -0.186°C. (Kf = 1.86, Kb = 0.512). What is the elevation in boiling point?

0.512

0.80

0.186

0.0512

191. Vant Hoff’s factor of Ca(NO₃)₂ is

192. The equivalent conductivity of 0.1 M week acid is 100 times less than that at infinite dilution. The degree of dissociation is

0.01

100

0.001

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Malik TahirLast Updated: May 24, 2025

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