PHARMACEUTICAL ANALYSIS (BP102TP) MCQs with Answer
1. _________ is used as primary standard for standardization of NaOH.
A. Sodium carbonate
B. Sodium bicarbonate
C. Sodium chloride
D. Potassium dichromate
Ans. B
2. 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
3. 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
4. Solution of known concentration
A. Standard solution
B. Concentration
C. Solution
D. Concentrated solution
Ans. A
5. 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
6. 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
7. Substance that can be reversibly oxidized or reduced, having different distinct colour in the individual oxidized and reduced forms
A. Redox indicators
B. Redox potential
C. Redox number
D. Redox state
Ans. A
8. 20 gm NaOH in 500 ml =
A. 0.1 N
B. 1 N
C. 0.5 M
D. 0.05 N
Ans. B
9. In oxidation reduction change in __________ of reacting element takes place.
A. Volume
B. pH
C. Absorbance
D. Valency
Ans. D
10. __________ is not an amphiprotic solvent.
A. Water
B. Alcohol
C. Acetic acid
D. None
Ans. D
11. __________ is not type of co-precipitation.
A. Surface adsorption
B. Occlusion
C. Crystallization
D. Mechanical entrapment
Ans. D
12. Oxidation-Reduction titration is also known as
A. Complexometric titration
B. Gravimetric titration
C. Redox titration
D. Gasometric titration
Ans. C
13. Potentiometry is type of ________ method.
A. Qualitative
B. Chromatographic
C. Classical
D. Electro-chemical
Ans. D
14. ________ is chelating agent
A. Salicylic acid
B. EDTA
C. Benzoic acid
D. Glycerol
Ans. B
15. __________ used as titrant in non-aqueous titration.
A. EDTA
B. Perchloric acid
C. Sodium nitrite
D. Silver nitrite
Ans. B
16. Conductometry used for the measurement of
A. Conductivity
B. Potential
C. Temperature
D. Concentration
Ans. A
17. Standardization of Iodine is carried out using ________________
A. Sodium thiosulphate
B. Oxalic acid
C. Perchloric acid
D. None of these
Ans. A
18. The degree of agreement between measured value and accepted true value is _____________
A. Precision
B. Accuracy
C. Range
D. Average deviation
Ans. A
19. Behavior of indicator is explained by ___________ theory.
A. Chromospheres
B. Ionic
C. Color
D. Resonance
Ans. D
20. pH is defined as
A. –log [OH–]
B. –log [H+]
C. pH + pOH
D. log pOH
Ans. B
21. 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
22. 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
23. 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
24. The number of gm-mole of the solute per liter of solution is known as
A. Normality
B. Molarity
C. Molality
D. Mole fraction
Ans.B
25. 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
26. The ratio of number of gm-mole of a 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
27. 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
28. 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
29. In strong acid – strong base titration, the pH of mixture at initial stage is find out by formula
A. PH=-log[H+]
B. [H+]=NaVa-NbVb/(Va + Vb)
C. POH = -log[OH-l
D. [OH-] = NbVb – NaVa/ (Va+ Vb)
Ans.A
30. In Standard solution which of the following is accurately known ,
A. Normality, strength or % of chemicals
B. Volume
C. Pressure
D. Temperature
Ans.A
31. 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
32. In titration end point can be determined by change in colour by
A. Measuring cylinder
B. Burette
C. Instrument
D. Indicator
Ans.D
33. The Quantity of chemical in each liter of solution is known as
A. Normality
B. Strength
C. Molecular Weight
D. Equivalence Weight
Ans.B
34. Exactly required concentration can be prepared from chemical reagent is called as
A. Primary standard
B. Secondary standard
C. Both A & B
D. None of this
Ans.A
35. An example of a primary standard substance is
A. FeS04
B. Na2C03
C. NH40H
D. NaOH
Ans.B
36. 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
37. A buffer solution can be formed by dissolving equal moles of
A. HF and NaF
B. HCl and NaOH
C. KBr and Na3P04
D. CH3COOH and NaCl
Ans. A
38. The conjugate acid of HAs042- is
A. H3O*
B. AS04’+
C. H3ASO4
D. H2ASO4*
Ans.B
39. 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
40. A solution of known concentration is the definition of a
A. Buffer solution.
B. Neutral solution.
C. Standard solution.
D. Saturated solution.
Ans.C
41. Which of the following is the strongest Bronsted-Lowry base?
A. NH3
B. CO3 2+
C. HSO3
D. H2BO3
Ans.B
42. 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
43. 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
44. 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
45. 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 H3O+ is greater than concentration of OH-
Ans.C
46. 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
47. 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
48. Which of the following are general properties of bases in aqueous solution?
A. Feel slippery and increase H3O+
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
49. 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
50. 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
51. 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
52. A basic solution can be defined as one in which
[H3O+] is not present
[H3O+] is equal to [OH-]
[H3O+] is less than [OH:]
[H3O+] is greater than [OH-]
Ans.C
53. 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
54. 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
55. 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
56. 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
57. Which of the following acids has the weakest conjugate base?
A. HIO3
B. HNO2
C. H3PO4
D.CH3COOH
Ans.A
58. Which of the followiing 1.0 M salt solutions will be acidic?
A. NaNO3
B.NaHCO3
C. NaHS04
D. NaHPO4
Ans.C
59. 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
60. 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
61. 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
62. 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.C
63. Which is the conjugate base of H2PO4-?
A. OH-
B. PO4 3-
C. HPO42-
D. H3PO4
Ans.B
64. 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
65. 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
66. Which one is aprotic solvent?
A. Chloroform
B. Benzene
C. Both
D. None
Ans. B
67. Prototogenic solvent is
A. Sulphuric acid
B. Hydrochloric acid
C. Nitric acid
D. All the above
Ans. D
68. Protophilic solvent is
A. Sodium hydroxide
B. Lithium methoxide
C. Sodium methoxide
D. All
Ans. D
69. Which one is useful in non aqueous titration?
A. Leveling solvent
B. Differentiating solvent
C. Both
D. None
Ans. A
70. Water may interfere with non aqueous titration by
A. 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
71. In the preparation of the 0.1 (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
72. Perchloric acid can be standardized by using
A. Benzoic acid
B. Oxalic acid
C. Potassium hydrogen phthalate
D. Tartaric add
Ans.C
73. Which one is used as indicator for non aqueous titration?
A. Crystal violet
B. Thymol blue
C. Oracet blue B
D. All
Ans.A
74. 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
75. Sodium Acetate, NaC2H302, is a water soluble salt that forms an aqueous solution that is
A. Acidic
B. Basic
C. Neutral
Ans.B
76. All the compounds given can be assayed by NAT except
A. Piperazine citrate
B. Diethylcarbamazine
C. Niclosamide
D. Metrifonate
Ans.D
77. Example for amphiprotic solvent
A. Methanol
B. Glacial acetic add
C. Water
D. All of the above
E. None of the above
Ans.D
78. 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
79. 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 acetic acid
D. All of the above
Ans.D
80. 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
81. 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.
Ans.A
82. Titrations based on the use of silver nitrate are called
A. Argentometric
B. Complexometric
C. Amperometric
D. Conductometric
Ans.A
83. Adsorption indicators are used in
A. Fajan’s method
B. Mohr’s method
C. Volhard’s method
D. All
Ans.A
84. 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
85. 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
86. Potassium chromate (K2CrO4) is used as an indicator in
A. Mohr’s method
B. Volhard’s method
C. Fajan’s method
D. None
Ans.A
87. Which of the following is an example of adsorption indicators?
A. Eosin
B. Phenolphthalein
C. Methyl red
D. Ninhydrin
Ans.A
88. Which method is used in water analysis
A. Fajan’s method
B. Mohr’s method
C. Volhard’s method
D. None
Ans. B
89. EDTA has_____binding sites and therefore it is also called as multidentate ligand.
A. Six
B. Five
C. Four
D. Seven
Ans.C
90. _______agent forms the complex with the metal ions that are not required in the estimation
A. Masking
B. Demasking
C. Both
Ans.B
91. The endpoint for an EDTA titration is usually found by using a indicator
A. Metallochromic
B. Redox
C. Acid base
D. All
Ans.A
92. Which one is polydentale
A. Ethylene diamine
B. EDTA
C. Both
D. None
Ans.C
93. Which one is sequestering agent?
A. Salicylaldoxime
B. 8-hydroxy quinolilne
C. EDTA
D. All
Ans.C
94. The complexometric titration where EDTA is used carried out at basic pH. Why?
A. For the stability of complex formed
B. Reaction rate is optimum in basic pH
C. There is less number of side reaction
D. All
Ans.D
95. Which is used as masking agent for lead in complexometrric titration?
A. Sod. Sulphide
B. Oxalate
C. Thiocetanaide
D. All
Ans.C
96. Dimercaprol is used as complexing agent for complexion of
A. Mercury
B. Arsenic
C. Lead
D. All
Ans.D
97. Indicator used in complexometric titration is
A. Erichrome black T
E- Xylenolorange
C. Mordant black II
D. All
Ans.D
98. Name the assay method for the drud calcium gluconate
A. Non aq titration
B. Acid base titaration
C. Complexometric
D. lodometric
Ans.C
99. Number of rings observed in the tetravalent ion EDTA complex
A. 4
B. 5
C. 6
D. 3
Ans.B
100. Following are properties of good precipitate except:
A. Easily filtered and washed free of contamination.
B. Significant loss of the analyte occurs during filtration and washing.
C. Unreactive with constituents of the atmosphere.
D. both a and b
Ans.B
101. In ____________, analyte is separated from a solution of the sample as a precipitate and is converted into a compound of known composition
A. Volatilization gravimetry
B. Precipitation gravimetry
C. Electrogravimetry
D. Precipitation point
Ans.B
102. ___________is the weight of analyte per unit weight of the precipitate.
A. Gravimetric factor
B. Precipitation factor
C. Electrogravimetry factor
D. None of the above
Ans.A
103. Digestion of precipitate also known as
A. Ageing
B. Gravimetric factor
C. Co – precipitation
D. Ostwald ripening
Ans.D
104. SI unit of conductance is
A. Mho
B. Seimens
C. Volt
D. None of the above
Ans.B
105. Current used for measured of conductance is
A. A.C
B. D.C
C. Both A and B
D. None of these
Ans.A
106. Hydrogen and Hydroxyl ions are potent_____
A. Conductivity
B. Molar conductance
C. Conductance Enhancers
D. None of the above
Ans.C
107. _______is the product of specific conductance and volume of electrolyte
A. Conductivity
B. Molar conductance
C. Conductance Enhancers
D. None of the above
Ans.B
108. _____is the conductance offered by 1 cm^ of an electrolytic solution
A. Molar conductjince
B. Conductance Enhancers
C. Specific conductance
D. Specific Resistance
Ans.C
109. Potentiometry is an_____method of analysis
A. Spectroscopic
B. Electrometric
C. Analytical
D. None of the abobe
Ans.B
110. Example for reference electrode except
A. Antimony electrode
B. Silver-silver electrode
C. Calomel electrode
D. None of the above
Ans.A
111. The indicator used in estimation of hardness of water by potentiometiy
A. PH
B. PM
C. Both a and b
D. None of the above
Ans.B
112. Which of the following two are used reference electrodes in polentiometry?
P) Glass membrane
Q) Hg-calomel
R) Ag-silver chloride
S) Ion selective
A)P,Q B)P,S C)Q,R D)P,R
Ans.C
• Hydrogen electrode can be used as
A. Indicator electrode
B. Reference electrode
C. Secondary reference electrode
D. Both A and b
Ans.D
113. __________electrode is employed as a secondary reference electrode
A. Hydrogen electrode
B. Droping Mercury Electrode
C. Calomel electrode
D. None of the above
Ans.C
114. Each electrochemical cell is composed of
A. Two half cells
B. Half cells
C. Both A and B
D. None of the above
Ans.A
115. An electrode, whose electrode potential is well known and stable is a
A. Indicator electrode
B. Reference electrode
C. Both A and B
D. None of the above
Ans.B
116. In polarography, when limiting current is achieved, one of the following process takes place. Choose that.
A-The rate of electron transfer just matches the rate of mass transfer
B. The rate of electron transfer is slower than the rate of mass transfer
C. The rate of electron transfer becomes independent of the rate of mass transfer
D. The rate of electron transfer far exceeds the rate of mass transfer
Ans.B
117. Which of the following is used as indicator electrode in polarography?
A. Glass
B. Dropping mercury
C. Platinum
D. Silver
Ans.B
118. For Qualitative analysis by polarography, characteristic parameter used is
A, Diffusion current
B. Half wave potential
C. Voltage
D. None of the above
Ans.B
119. Limiting current is sum of diffusion current and
A. Residual current
B. Faradic current
C. Migration current
D .Additional current
Ans.B
120. Gradual rising in current in polarography is called
A.Weak current
R Higher current
C Migration Currerrt
D.Residual current
Ans.D
121. Reason for generation of migration current in polarogram is
A. Migration and diffusion of charged particles
B. Migration of charged particles
C. Diffusion of charged particle
D. None of the above
Ans.A
122. The D and L isomeric forms can be distinguished by
A. Polarimetry
B. Refractometry
C. Potentiometry
D. Conductometry
Ans.A
123. Sodium vapor lamp used in Polarlmeter emit light of wavelcngth (in Angstrom)
A. 5890 & 5896
B. 4368 & 4916
C 5770 & 5791
D.5461 & 4368
Ans.A
124. Oxidation involves
A. loss of hydrogen
B. loss of oxygen
C. gain in hydrogen
D. gain in electrons
Ans.A
125. In a reaction between CuS04(aq) and Zi(aq)
A. Zinc experiences an increase in the oxidation state
B. undergoes oxidation
C. Zinc undergoes oxidation
D. all of these
Ans.D
126. Oxidizing agents
A. are mostly non-metals
B. are mostly metals
C. decrease in oxidation state
D. are mostly transition metals
Ans.A
127. Upon oxidation of acidified potassium manganate (VII), the puiple color of Manganese
A. stays
B. changes to pink
C. becomes colorless
D. becomes blue
Ans.C
128. Hydrogen acts as a reducing agent,
A. by taking oxygen
B. by giving electron
C. by taking hydrogen
D. Both A and B
Ans.D
129. Reduction involves
A. loss of oxygen
B. gain in hydrogen
C gain in oxygen
D. loss of electrons
Ans.A
130. Oxidizing agents does not include
A. potassium iodide
B. potassium manganate
C. potassium dichromate
D. bromine solutions
Ans.A
