Chapter 7 – Multiple Ch0ice Questions

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Multiple Ch0ice Questions

1. A homogenous mixture of two or more than two or more than chemical substances is called

(i) Solute

(ii) Solution

(iii) Solvent

(iv) Solvation

 

2. Number of gram- equivalents of solute dissolved per dm³ of the solution is known as

(i) Molarity

(ii) Molality

(iii) Normality

(iv) None of these

 

3. Number of moles of the solute dissolved per dm³ of the solution is known as

(i) Molarity

(ii) Formality

(iii) %

(iv) None of these

 

4, Number of moles of the solute dissolved in 1 kg of solvent is known as

(i) Molarity

(ii) Formality

(iii) Molatity

(iv) Mole fraction

 

5. The ratio of the number of moles of a particular component of the solution to the total number of moles of all the components of the solution is called

(i) %

(ii) Mole fraction

(iii) Formality

(iv) Molality

 

6. The process in which water molecules surround and interact with solute ions or molecules is called

(i) Hydration

(ii) Salvation

(iii) Hydrolysis

(iv) Dehydration

 

7. Which substance yield ions when dissolved in water?

(i) Acids

(ii) Salts

(iii) Bases

(iv) All

 

8. The degree of dissociation depends upon

(i) Nature of electrolyte

(ii) Dilution of solution

(iii) The temperature

(iv) All factors

9. Which is the example of a sparingly soluble salt?

(i) AgC1

(ii) KC1

(iii) NaCO 3

(iv) HC1

 

10. The rate of a chemical reaction is determined by

(i) Physical methods

(ii) Chemical methods

(iii) Both methods

(iv) None of these

 

11. The amount of chemical produced by an electric current is directly proportional to the quantity of electricity passed. This fact is known as

(i) Faradays

(ii) Ohm’s law

(iii)Newton’s law

(iv) Coulmb’s law

 

12. A cell in which a redox reaction produces an electric current is known as

(l) Reversible cell

(ii) Galvanic cell

(iii) Electrolytic cell

(iv) Irreversible cell

 

13. The cell which converts electrical energy to chemical energy is called

(i) Galvanic cell

(ii) Dry cell

(iii) Electrolytic cell

(iv) None of these

 

14. The potential difference is measured by a device known as

(i) Spectrometer

(ii) Viscometer

(iii) Voltmeler

(iv) Voltammeter

 

15. The electrode at which oxidation takes place is called

(i) Cathode

(ii) Anode

(iii) Diode

(iv) Dynode

 

16. The electrode at which reduction takes place is called

(i) Cathode

(ii) Anode

(iii) Diode

(iv) Dynode

 

17. Which elements has greater reduction potential?

(i) Li

(ii) Cu

(iii) C1

(iv) F

 

18. The oxidation number of Mn in KMnO4is

(i) + 3

(ii) + 5

(iii) + 7

(iv) + 9

 

19. Generally the oxidation number of oxygen is

(i) + 2

(ii) – 2

(iii) -1

(iv) +1/2

 

20. The ions product of water at 25 ° C is

(i) 10-12

(i) 10-13

(iii) 10-14

(iv) 10-7

 

21. A solution which contains H+ = 10-7 M is said to be

(i) Amphoteric

(ii) Acidic

(iii) Basic

(iv) Neutral

 

22. The concentration of H+ and OH ions in an aqueous solution can vary from

(i) 1 to14

(ii) 1to1014

(iii) 1 to 12

(iv) 1 to10-12

 

23. The pH of 0.01 M HC1 is

(i) 4

(ii) 3

(iii) 1

(iv) 2

 

24. The concentration of H+ ions in a solution having pH 7 is equal to

(i) 10-5

(ii) 10-6

(iii) 10-8

(iv) 10-7

 

25. Which of the following pair acts as a buffer?

(i) Na C1 + NaOH

(ii) H2SO4 + Na2SO4

(iii) Mg NO3 + HNO 3

(iv) NH4C1 + NH4OH

 

26. Loss of electrons is called

(i) Reduction

(ii) Oxidation

(iii) Hydrolysis

(iv) Electrolysis

 

27. Gain of electron is called

(i) Reduction

(ii) Oxidation

(iii) Hydrolysis

(iv) Electrolysis

 

28. 4.0 g Na OH has been dissolved per dm³ of the solution. The strength of the solution is

(i) 0.5 M

(ii) 0.6 M

(iii) 0.1 M

(iv) 1.0 m

 

29. 5% w/v Na OH solution means

(i) 59 Na OH +100 g H2O

(ii) 5g Na OH + 100 g H2O

(iii) 5g Na OH + 100ml H2O

(iv) 5g Na OH + 100 cm3 solution

 

30. pH of 0.0001 M Na OH is

(i) 3

(ii) 11

(iii) – 3

(iv) 7

 

31. Which salt gives neutral solution?

(i) CuSO4

(ii) NaHCO 3

(iii) Na2CO 3

(iv) NaCl

 

32. What kind of buffer would be a mixture of CH3COOH and CH3COONa ?

(i) Neutral buffer

(ii) Acidic buffer

(iii) Basic butler

(iv) None of these

 

33. pH of human blood is

(i) 7

(ii) 7.4

(iii) 7.8

(iv) 8.4

 

34. Which of the following reactions is correct one?

(i) Zn + Cu —-> Zn + Cu 2+

(ii) Zn + Cu2+ —->Zn + Cu 2+ + Cu 2+

(iii) Zn + Cu 2+ —->Zn2+ + Cu

(iv) Zn2+ +Cu2+—->Zn+ Cu

 

35. Which of the following elements have large oxidation potential?

(i) C u

(ii) Li

(iii) K

(iv) F

 

36. The oxidation number of N is NHO3 is

(i) +1

(ii) +3

(iii) +5

(iv) -5

 

37. pH of a solution is equal to V

(i) Log [OH]

(ii) – log [OH]

(iii) log [ H]

(iv) log [H]

 

38. The sums of pH is equal to

(i) 10

(ii) 14

(iii) 12

(iv) 7

 

39. pH is determined by

(i) Litmus paper

(ii) Indicator

(iii) pH meter

(iv) All of these methods

 

110. These organic compounds whose color change depends on pH of the solution are known as

(i) Pigment

(ii) Dyes

(iii) Indicators

(iv) None of these

 

41. Indicators are

(i) Strong acids

(ii) Strong bases

(iii) Weak acids

(iv) Weak acids or weak base

 

42. The color of phenolphthalein in basic medium is

(i) Colorless

(ii) Green

(iii) Blue

(iv) Red

 

43. Hydrogen ions are more readily reduced than

(i) Ag

(ii) Cu++

(iii) Cl2

(iv) Zn+1

 

44. The oxidation number of Cr in K2CrO4 is

(i) + 5

(ii) + 7

(iii) + 3

(iv) + 6

 

45. Component of solution in large amount is called:

(i) Solvent

(ii) Solute

(iii) Solution

(iv) Minority

 

46. Oxidation state of sulphur in SO2 is:

(i) – 4

(ii) + 22

(iii) + 2

(iv) + 4

 

47. One of the following formulate contains nitrogen with oxidation state +5

(i) NH 4+1

(ii) NH 3

(iii) NHO3

(iv) NO 2

 

48. One of the following aqueous solution has the lowest pH :

(i) 0.1M NaOH

(ii) 0.1 M KOH

(iii) 0.1 M HCL

(iv) 0.001 M HNO3

 

49. Sum of oxidation number of natural compound is always:

(i) -v e

(ii) +v e

(iii) Zero

(iv) Infinite

 

50. One of the following salts dissolved in H2O to form a solution with a pH greater than 7:

(i) NaCL

(ii) CuSO4

(iii) Na2CO3

(iv) NH4CL

 

51. pH of pureH2O is:

(i) KMnO

(ii) K2MnO4

(iii) M n O4

(iv) M n O

 

52. Hydrolysis of a salt occurs in an aqueous solution, which:

(i) Has p H = 7

(ii) Is neutral

(iii) is either acidic or basic

(iv) Does not contain ions

53. What is hydrolysis of salts?

(i) Interaction of the salt with OH ions obtained from water

(ii) Interaction of the anions of the salt with H ions obtained from water

(iii) Interaction of the ions of the salt with the ions of the water

(iv) None of the above

 

54. A 10% solution of NaCl means that in 100 g of solution there is:

(i) 5.85 g NaCl

(ii) 58.5g of NaCl

(iii) 10g Nacl

(iv) 10g of H20

 

55. 26.5 g sodium carbonate is added to 250 ml of distilled water to yield a concentration equal to:

(i) 1.0 M

(ii) O. 5 M

(iii) 1.0 N

(iv) 1.5 M

 

55. Molarity of solution which contains 0.5 moles in 500 ml is:

(i) 1.0 M

(ii) 1.0 N

(iii) 0.5 M

(iv) 1.5 M

 

56. Molarity of solution which contains 0.5 mole in 500ml is:

(i) 0.5 M

(ii) 1.0 M

(iii) 1.5 M

(iv) 2 M

 

57. 500 ml of the solution contains 49 gm of H2SO4 the molarity of the solution:

 

58. l lit of 0.5N AgNO3solution contains : [molecular wt of Ag NO3 = 169.9]

(i) 50 gm of Ag NO3

(ii) 100 gm of Ag NO3

(iii) 84. gm of Ag NO3

(iv) 65 gm of Ag NO3

 

59. 0.1 M solution of different substance contains:

(i) Different mole of substance

(ii) Different amount of substance

(iii) Different amount of solution

(iv) All of these

 

60. 0. 5 moles of NaCl dissolve in 250 ml of solution, 2 lit of this solution contains:

(i) 234 gm of Na Cl

(ii) 250 gm of Na Cl

(iii) 150 gm of Na Cl

(iv) 300 gm of Na Cl

 

61. The molarity of H2 SO is 0.5 M. its normality will be:

(i) 0.5 N

(ii) 1.0 N

(iii) 0.25 N

(iv) 2.0 N

 

62. The volume of 4M HCl needed to prepare one liter of 0.5 M solution is:

(i) 0.125

(ii) 0.0125

(iii) 0. 875

(iv) 0.0875

 

63. A mixture contains 1 mole of A, 3 moles of B and 6 moles of C moles fraction of

A is:

(i) 0.1

(ii) 0.3

(iii) 0.6

(iv) 0.8

 

64. How many gm of HC1 needed to prepare 4 M HCl solution in 1 lit:

(i) 109.5 g

(ii) 73 g

(iii) 146 g

(iv) 200 g

 

65. A 10 N solution stands for :

(i) Normal Solution

(ii) Decanormal solution

(iii) Decinormal solution

(iv) Semi normal solution

 

66. What is the volume of 0.5 M HCl solution which reacts with 50 ml of 0.1 M NaOH solution:

(i) 50 ml

(ii) 5 ml

(iii) 25 ml

(iv) 10 ml

 

67. Theory of ionization was put forward by:

(i) Arrhenius

(ii) Hess

(iii) Le- Chatelier

(iv) Avogadro

 

58. The charge from ferrous to ferric involves the:

(i) Loss of electron

(ii) Gain of electron

(iii) Loss of proton

(iv) Gain of proton

 

69. The addition of oxygen is known as

(i) Reduction

(ii) Oxidation

(iii) Combustion

(iv) None of these

 

70. A reducing agent

(i) Always forms hydrogen

(ii) Always removes hydrogen

(iii) Is an electron donor

(iv) Is an electron acceptor

 

71. An oxidizing agent is that which can:

(i) Gain electrons

(ii) Lose electrons

(iii) Share electrons

(iv) Gain positron

 

72. The conversion of an atom into an anion is called as:

(i) Oxidation

(ii) Reduction

(iii) Hydration

(iv) None of these

 

73. When neutral atom change into cation than:

(i) It gains proton

(ii) It gains electrons

(iii) It losses proton

(iv) It losses electrons

 

74, Oxidation number oxygen in hydrogen peroxide is:

(i) + 2

(ii) – 2

(iii) +1

(iv) -1

 

75. Oxidation state of sulphur in sulphate radical is:

(i) + 4

(ii) + 5

(iii) + 6

(iv) + 7

 

76. The oxidation state of nitrogen in N3 H is:

(i) +1/3

(ii) + 3

(iii) – 3

(iv) – 1/ 3

 

77. At the end of redox reaction, oxidation state of the oxidizing agent:

(i) Decrease

(ii) Increase

(iii) Some time increase, some time decrease

(iv) Remains same

 

78. Cell reaction for the cell

Zn / Zn2+ (1.0M) || Cd2+ (1.0M) / Cd is given by

(i) cd —————-> Cd2+ +2e

(ii) Zn2+ —————->Znº – 2e

(in) Zn 2+ + cd —————-> Zn + cd2+

(av) Zn + cd2+ —————-> Zn2+ + cd

 

79. Electrical conductance depends upon which of the following factors:

(i) Numbers of ions

(ii) Mobility of ions

(iii) Both of the above

(iv) None of the above

 

80. A voltaic cell shown as

Pt/ H2/ H+ || Cu2+ / Cu

Which of the following is incorrect.

(i) Copper is getting deposited

(ii) Hydrogen electrode is a negative end

(iii) Hydrogen is getting reduced

(iv) Cu+2 / Cu half cell has a higher redox potential

 

81. According to Lewis acid base theory base is a/an:

(i) Electron donor

(ii) Electron acceptor

(iii) Proton donor

(iv) Proton acceptor

 

82. Acids and base are:

(i) Proton acceptor

(ii) Proton_donor, proton acceptor

(iii) Proton donor, proton donor

(iv) Proton acceptor, proton acceptor

 

83. Which of the following formula represent and acid with a basicity of 2 :

(i) HC1

(ii) NHO3

(iii) HCO2 H

(iv) H2 SO 4

 

84. An alkali is abase which

(i) Is decomposed by heating

(ii) Forms acid salts

(iii) Is neutral

(iv) Dissolves in water

 

85. Which of the following has pH higher than 7:

(i) 100ml H2SO4 (0.1 M) + 100ml Na C1 (0.1 M)

(ii) 100 ml HC1(0.1 M)+100 ml Na C1 (0.1 M)

(iii) 100 ml HNO3 (0.1 M)+200 ml Na C1(0.1 M)

(iv) 100 ml HNO3 (0.1 M)+ 200 ml Na OH (0.1 M)

 

 

86. CO 2 passed through water after the combustion of hydrocarbons p H of the water will be:

(i) 5

(ii) 7

(iii) 8

(iv) 2

 

87. The p l-l of a solution is 8.07 its hydrogen ion concentration is approximately:

(i) 8 x 10-9

(ii) 8 x 109

(iii) 8 x 10-10

(iv) 8 x 1010

 

88. If H ion concentration in the solution is 0. 0004, what is the solution:

(i) +4

(ii) -4

(iii) -3

(iv) Between 3 and 4

 

89. Methyl orange is used as an indicator in acid base titration to record change of pH in the range:

(i) Large quantity of acid

(ii) Large quantity of water

(iii) Small amount of base

(iv) Large amount of base

 

90. Drops of methyl orange in the strong base shows:

(i) Pink Color

(ii) No color

(iii) Red Color

(iv) Yellow color

 

91. Which indicator is suitable for titrating strong acid against a weak base?

(i) Phenolphthalein

(ii) Methyl orange

(iii) Any indicator

(iv) No indicator

 

92. Buffer solution is made from weak acid with:

(i) Weak base

(ii) Acidic salt

(iii) Strong base

(iv) Basic salt

 

93. The range of p H for phenolphthalein indicators is:

(i) 8-10.3

(ii) 3. -5.5

(iii) 6.8-8.4

(iv) 10.1-13.0

 

04. A buffer solution

(i) Change p H rapidly with the addition of an acid

(ii) Does not change p H at all

(iii) Resists changes in p H

(iv) Change pH only with the addition of a strong base

 

95. Which one is a neutralization reaction?

(i) SO3 + H 2 O ———–> H2SO4

(ii) Zn CO3 ———–> ZnO + CO2

(iii) Zn + CuSO4———–>ZnS04 + Cu

(iv) HC1 + KOH ———–>KC1 + H20

 

96. Reaction of an acid like HC and a base like NaOH always

(i) Forms a precipitate

(ii) Forms a volatile salt

(iii) Forms a soluble salt and water

(iv) Forms a salt and water

 

07. If 10 ml of 0.1 M HC1 is mixed with 5.0 ml 0.2 M Na GH, the solution will be

(i) Neutral

(ii) Acids

(iii) Basic

(iv) Difficult to predict gps cell phone tracking free

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