Pharamaceutical Analysis Unit-1 Semester-1 MCQs
1.Intermediate precision is done by.
Different analysts
Different days
Different equipment
All of the above
SOLUTION
All of the above
2.Which one always acts as reducing agent.
H2O2
H2S
HNO3
SO2
SOLUTION
H2S
3.For the titration of HCl and NH4OH, the suitable indicator is
Methyl Orange
EBT
Phenolphthalein
None of the above
SOLUTION
Methyl Orange
4.The oxidation number of Cr in K2Cr2O7 is
+6
+7
+5
+4
SOLUTION
+6
Q-5
The electrochemical method which is used to measure electro motive force is called as
Amperometry
Conductometry
Polarography
Potentiometry
SOLUTION
Potentiometry
6.Polarography is developed by which of the following scientist
Hull
Jaroslav heyrovsky
Schiebold
Einstein
SOLUTION
Jaroslav heyrovsky
7.Precision is usually expressed in terms of.
Variance
Standard deviation
Sigma method
RSD
SOLUTION
RSD
8.EDTA method of determining hardness of water can be used to detamine
All types of hardness
Temporary hardness only
Permament hardness only
Alkaline hardness only
SOLUTION
All types of hardness
9.In Gas-liquid phase chromatography, the stationary phase is composed of _____ and the mobile phase is made of _____
Solid, liquid
Liquid, liquid
Liquid, gas
Solid, gas
SOLUTION
Liquid, gas
10.The precision under the same operating conditions over a short interval of time is called as
Reproducibility
Intermediate precision
Repeatability
Robustness
SOLUTION
Repeatability
11.The number of moles of a solute per liter of a solution is
Molality
Normality
Molarity
None
SOLUTION
Molarity
12.Which one always acts as oxidizing agent
HNO3
MnO2
H2O2
SO2
SOLUTION
HNO3
13.Which method is used for the Limit test for arsenic
Gutzeit method
Oswald method
Arrhenius method
Karl-Fischer method
SOLUTION
Gutzeit method
14.Which of the following cannot be used as adsorbent in Column adsorption chromatography
Magnesium oxide
Silica gel
Activated alumina
Potassium permanganate
SOLUTION
Potassium permanganate
15.In which of the following type of paper, chromatography does the mobile phase move horizontally over a circular sheet of paper?
Ascending paper chromatography.
Descending paper chromatography.
Radial paper chromatography.
Ascending – descending chromatography.
SOLUTION
Radial paper chromatography
16.The closeness of agreement between a series of measurement obtained from multiple sampling of the homogenous sample is?
Accuracy
Precision
Ruggedness
Robustness
SOLUTION
Precision
17. The equivalent weight of NaoH is
36
20
40
13
SOLUTION
40
18. Phenolphthalein indicator is used for titration of
CH3COOH VS Na2CO3
CH3COOH VS NaOH
HNO3 VS NH4OH
H2SO4 VS Na2CO3
SOLUTION
CH3COOH VS NaOH
19. is used as primary standard for standardization of NaOH.
A. Sodium carbonate
B. Sodium bicarbonate
C. Sodium chloride
D. Potassium dichromate
Ans. B
20. Phenolphthalein has a pH range of
A. 6.8-8.4
B. 1.2-2.8
C. 8.3 11.0
D. 4.2-6.3
Ans. C
21. Errors arise due to the individual analyst is responsible for them
A. Method error
B. Instrumental error
C. Personal error
D. Random error
Ans. C
22. Solution of known concentration
A. Standard solution
B. Concentration
C. Solution
D. Concentrated solution
Ans. A
23. Acid is a substance which dissociates in water to produce hydrogen ions
A. Arrhenius theory
B. Lewis theory
C. Bronsted theory
D. Lowry theory
Ans. A
24. The colour change is due to ionisation of the acid base indicators
A. Ostwald theory
B. Chromophore theory
C. Quinonoid theory
D. Resonance theory
Ans. A
25.the individual oxidized and reduced forms
A. Redox indicators
B. Redox potential
C. Redox number
D. Redox state
Ans. A
26. 20gm NaOH in 500 ml =
A. 0.1 N
B. 1 N
C. 0.5 M
D. 0.05 N
Ans. B
27. In oxidation reduction change in . of reacting element takes place.
A. Volume
B. pH
C. Absorbance
D. Valency
Ans. D
28. is not an amphiprotic solvent.
A. Water
B. Alcohol
C. Acetic acid
D. None
Ans. D
29…… is not type of co-precipitation.
A. Surface adsorption
B. Occlusion
C. Crystallization
D. Mechanical entrapment
Ans. D
30. Oxidation-Reduction titration is also known as
A. complexometric titration
B. Gravimetric titration
C. Redox titration
D. Gasometric titration
Ans. C
31. Potentiometry is type of, method.
A. Qualitative
B. Chromatographic
C. Classical
D. Electro-chemical1
Ans. D
32. is chelating agent
A. Salicylic acid
B. EDTA
C. Benzoic acid
D. Glycerol
Ans. B
33. used as titrant in non-aqueous titration.
A. EDTA
B. Perchloric acid
C. Sodium nitrite
D. Silver nitrite
Ans. B
33.Conductometry used for the measurement of
A. Conductivity
B. Potential
C. Temperature
D. Concentration
Ans. A
34. Standardization oflodine is carried out using.
A. Sodium thiosulphate
B. Oxalic acid
C. Perchloric acid
D. None of these
Ans. A
35.The degree of agreement between measured value and accepted true value is
A. Precision
B. Accuracy
C. Range
D. Average deviation
Ans. A
36. Behavior of indicator is explained by . theory.
A. Chromospheres
B. lonic
C. Color
D. Resonance
Ans. D
37. pH is defined as
A. -log [OH-1
B. -log [H+
C. pH +pOH
D. log pOH
Ans. B
38. The titration carries out between KCl and AgNO3 is termed as titration.
A. Oxidation-Reduction
B. Precipitation
C. Acid-Base
D. None of these
Ans.B
39.. 8.5 ml HCl in 1
litre = .
A. 0.1 M
B.0.1 N
C. Both A and B
D. 0.5 M
Ans. A
40. The number of gm-equivalent of the solute per liter of solution is known as
A. Normality
B. Molarity
C. Molality
D. Mole Fraction
Ans.A
41. The number of gm-mole of the solute per kg of solution is known as
A. Normality
B. Molarity
C. Molality
D. Mole fraction
Ans.C
42. The ratio of number of gm-mole ofa component to total number of gm-mole in mixture or solution is known as
A. Normality
B. Molarity
C. Molality
D. Mole fraction
Ans.D
43. The number of gms of solute per 100 ml of solvent is known as
A. Normality
B. % weight by volume
C. Molality
D. Mole fraction
Ans.B
44. The chemical reagent from which solution of required concentration can be prepared is
A. Secondary standard
B. Dilute solution
C. Concentrated solution
D. Primary standard
Ans.C
45. In Standard solution which ofthe following is accurately known,
A. Normality, strength or % of chemicals
B. Volume
C. Pressure
D. Temperature
Ans.A
46. The process of adding known concentration until it complete the reaction with known
volume is called as
A. Titrant
B. Analysis
C. Titration
D. Titrend
Ans.C
47. In titration end point can be determined by change in colour by
A. Measuring cylinder
B. Burette
C. Instrument
D. Indicator
Ans.D
48. The Quantity of chemical in each liter of solution is known as
A. Normality
B. Strength
C. Molecular Weight
D. Equivalence Weight
Ans.B
49. An example of a primary standard substance is
A. FeS04
B. Na2CO03
C. NH4OH
D. NaOH
Ans.B
50. A normal solution is one which contains
A. Gram molecular weight/L
B. Gram equivalence weight/L
C. Gram formula weight/L
D. Gram molecular weight/Kg
Ans.B
51. A buffer solution can be formed by dissolving equal moles of
A. HF and NaF
B. HCl and NaOH
C. KBrandNa3P04
D. CH3COOH and NaCl
Ans. A
52. The conjugate acid ofHAs04 is
A. H30*
B. AS04+
C. H3AS04
D. H2ASO4*
Ans.B
53. Which of the following indicators has a transition point closest to the equivalence point for the titration of a weak acid by a strong base?
A. Orange IV
B. Tliymol blue
C. Methyl orange
D. Bromcresol green
Ans.B
54. A solution of known concentration is the definition of a
A. Buffer solution.
B. Neutral solution.
C. Standard solution.
D. Saturated solution.
Ans.C
55. Which ofthe following is the strongest Bronsted-Lowry base?
A. NH3
B. CO3 2
C. HSO3
D. H2BO3
Ans.B
56. An Arrhenius acid is defined as a chemical species that
A. is a proton donor.
B. is a proton acceptor.
C. Produces hydrogen ions in solution.
D. Produces hydroxide ions in solution.
Ans.C
56. Consider the following reaction:
H3BO3 (aq) +HS (aq)>H2BO3 (aq) + H2S (aq)
The order of Bronsted-Lowry acids and bases in this equation is
A. Acid, base, base, add.
B. Acid, base, acid, base.
C. Base, acid, acid, base.
D. Base, acid, base, acid.
Ans.D
57. Which of the following indicators is yellow at a pH of 10.0?
A. Methyl red
B. Phenol red
C. Thymol blue
D. Methyl violet
Ans.A
58. Which of the following is a general property of bases?
A. Taste sour
B. Turns litmus red
C. Conduct electric current in solution
D. Concentration of H30+ is greater than concentration of OH-
Ans.C
59. The conjugate base of an acid is produced by
A. Adding a proton to the acid.
B. Adding an electron to the acid.
C. Removing a proton from the acid.
D. Removing an electron from the acid
Ans.C
60. A buffer solution may contain equal moles of
A. Weak add and strong base.
B. Strong acid and strong base.
C. Weak acid and its conjugate base.
D. Strong acid and its conjugate base.
Ans.C
61. Which of the folowing are general properties of bases in aqueous solution?
A. Feel slippery and increase H30+
B. Turn litmus red and accept a proton
C Conduct electricity and turn littmus blue
D. Feel slippery and react with Au to produce H2 (g)
Ans.C
62. Pure sodium hydrogen phthalate is used to standardize a solution of NaOH for
acid-base titration. What term is used to describe the sodium hydrogen phthalate?
A. Titrant base
B. Standard buffer
C. Equivalent base
D. Primary standard
Ans.D
63. An Arrhenius base is defined as a compound that
A. Accepts OH- in solution.
B. Releases OH-in solution.
C. Accepts protons in solution.
D. Donates protons in solution.
Ans.B
64. A Bronsted-Lowry acid is defined as a substance that
A. releases H+ (aq)
B. releases OH-(aq)
C. accepts proton in solution
D. donates proton in solution
Ans.D
65. A basic solution can be defined as one in which
[H3O+] is not present
[H3O+] is equal to [OH-|
[H30+] is less than [OH:]
[H30+] is greater than [OH-]
Ans.C
66. A chemical indicator in solution consists of
A. A weak acid and its conjugate acid.
B. A weak acid and its conjugate base.
C. A strong acid and its conjugate acid.
D. A strong acid and its conjugate base.
Ans.B
67. What do a chemical indicator and a buffer solution typically both contain?
A. A strong acid and its conjugate acid
B. A strong acid and its conjugate base
C. A weak acid and its conjugate acid.
D. A weak acid and its conjugate base
Ans.D
68. When performing a titration experiment, the indicator must always have
A distinct colour change at pH =7.0.
B. The ability to change from colourless to pink,
C. A transition point that is close to the equivalence point.
D.An equivalence point that is close to the stoichiometric point.
Ans.C
69. Which of the following is not a good use for an acid-base titration curve?
A. to determine the concentration of the base
B. to select a suitable indicator for the titration
C. to determine whether the acid is strong or weak
D. to select a suitable primary standard for the titration
Ans.D
70. Which of the following acids has the weakest conjugate base?
A. HIO3
B. HNO2
C. H3P04
D.CH3COOH
Ans.A
71. Which ofthe followiing 1.0M salt solutions will be acidic?
A. NaNO3
B.NaHCO3
C. NaHS04
D. NaHPO4
Ans.C
72. The pH at which an indicator changes colour is known as its
A. Standard point.
B. Transition point.
C. Equivalence point.
D. Stoichiometric point.
Ans.B
73. A buffer solution can be prepared by dissolving equal moles of
A. A weak base and a strong base.
B. A weak acid and its conjugate base.
C. A strong base and its conjugate acid.
D. A strong acid and its conjugate base.
Ans. B
74. A Bronsted-Lowry acid is defined as a substance that
A. releases
B. releases OH (aq)
C. accepts a proton
D. donates a proton
Ans.D
75. A chemical indicator in solution consists of
A. A weak acid and is conjugate acid.
B. A weak acid and its conjugate base
C. A strong acid and its conjugate acid.
D. A strong acid and its conjugate base.
Ans.C
76. Which is the conjugate base of H2PO4-?
A. OH-
B. PO4
C. HPO4
D. H3PO4
Ans.B
77. What do a chemical indicator and a buffer solution typically both contain?
A. a strong acid and its conjugate acid
B. a strong add and its conjugate base
C. a weak add and its conjugate acid
D. a weak add and its conjugate base
Ans.D
78. Non aqueous titration is carried out for
A. Water insoluble drug
B. Weakly acidic drug
C. Weakly basic drug
D. All the above
Ans. D
79. Which one is aprotic solvent?
A. Chloroform
B. Benzene
C. Both
D. None
Ans. B
80. Prototogenic solvent is
A. Sulphuric acid
B. Hydrochloric acid
C. Nitric acid
D. All the above
Ans. D
81. Protophilic solvent is
A. Sodium hydroxide
B. Lithium methoxide
C. Sodium methoxide
D. All
Ans. D
82. Which one is useful in non aqueous titration?
A. Leveling solvent
B. Differentiating solvent
C. Both
D. None
Ans. A
83. Water may interfere with non aqueous titration by
Acting as Strong acid than the weakly acidic drug
B. Acting as Strong base than the weakly basic drug
C. Both
D. None
Ans.C
84. In the preparation of the 0.l (N) perchloric acid amotmt of acetic anhydride should be
optimum. Why?
A. If added more quantity then amine drug may acetylate and causes erroneous result
B. If added less quantity then water may interfere with the titration,
C. Formation of acetyl perchlorate can cause explosion
D. All
Ans.B
85. Perchloric acid can be standardized by using
A. Benzoic acid
B. Oxalic acid
C. Potassium hydrogen phthalate
D. Tartaric add
Ans.C
86. Which one is used as indicator for non aqueous titration?
A. Crystal violet
B. Thymol blue
C. Oracet blue B
D. All
Ans.A
87. Potentiometric titration is used in nonaqueous titration, when
A. Colour of the solution is high
B. Colour of the solution is low
C. Both
D. None
Ans.C
88. Sodium Acetate, NaC2H302, is a water soluble salt that forms an aqueous solution that is
A. Acidic
B. Basic
C. Neutral
Ans.B
89. All the compounds given can be assayed by NAT except
A. Piperazine citrate
B. Diethylcarbamazine
C. Niclosamide
D. Metrifonate
Ans.D
90. Example for amphiprotic solvent
A. Methanol
B. Glacial acetic add
C. Water
D. All of the above
E. None of the above
Ans.D
91. Nature of amphiprotic solvent
P) Acts as a base in strong addic environment
Q) Acts as a acid in strong basic environment
R) Acts as a base in weak basic environment
S) Neutral in nature
A. P.R
B. P,S
C. Q.R
D. P.Q
Ans.D
92. Principle involved in non aqueous titration of weakly basic drug
A. Proton donation from acetic acid to drug
B. Proton donation from onium ion to acetic acid
C. Proton donation from perchloric acid to acetie acid
D. All of the above
Ans.D
93. AgCl has to be filtered off before titration using
A. Modified Volhard’s method
B. Mohr’s method
C. Fajan’s method
D. None of the above
Ans.A
94. The adsorption indicator in Fajan’s method has to be;
A. Of the same charge as titrant
B. Of the opposite charge as titrant
C. Has no charge. D. None
Ans.A
95. Titrations based on the use of silver nitrate are called
A. Argentometric
B. Complexometric
C. Amperometric
D. Conductometric
Ans.A
96. Adsorption indicators are used in
A. Fajan’s method
B. Mohr’s method
C. Volhard’s method
D. All
Ans.A
97. Which method follows the principle of formation of coloured precipitate at the end point?
A. Fajan’s method
B. Volhard’s method
C. Modified Volhard’s metlrod
D. All
Ans.D
98. In Which method, ferric ammonium sulphate is used as an indicator?
A. Fajan s method
B. Mohr’s method
C. Volhard’s method
D. None
Ans.B
99. Potassium chromate (K2Cr04) is used as an indicator in
A. Mohr’s method
B. Volhard’s method
C. Fajan’s method
D. None
Ans.A
100. Which of the following is an example of adsorption indicators?
A. Eosin
B. Phenolphthalein
C. Methyl red
D. Ninhydrin
Ans.A
101. Which method is used in water analysis
A. Fajan’s method
B. Mohr’s method
C. Volhard’s method
D. None
Ans. B