Pharmaceutical Chemistry of Inorganic Medicals

INORGANIC PHARMACEUTICAL PHARMACY

D

1. Ammoniated mercury is also known as: a. calomel c. lunar caustic

b. corrosive sublimate d. white precipitate

C

2. The rays which have no mass and no charge but of very high energy and excellent penetrating power: a. alpha b. beta c. gamma d. x-ray

D

3. Antacids that cause “rebound” hyperacidity are: a. Mg(OH)2 & Al(OH)2 b. Na2CO3 c. NA2S2O3 & MgSO4 d. NaHCO3 & CaCO3

A

4. Evolves a gas with a fruity odor odor when treated with concentrated sulfuric acid and ethanol: a. acetate b. chlorate c. sulfate d. silicate

A

5. A buffer system that has been modified to include NaCl to make it isotonic with physiologic fluid: a. Sorensen phosphate buffer c. Feldman’s buffer b. Gifford’s buffer d. Atkin & Pentin buffer

B

6. An orange-red sulfide insoluble in NH3 but soluble in excess (NH4)2S: a. CdS b. Sb2S3 c. HgS d. MnS

B

7. “Artificial Air” is used therapeutically to alleviate difficult respiration and contains: a. 60% oxygen & 40% helium b. 20% oxygen & 80% helium c. 20% helium & 80% oxygen d. 40% helium & 60% oxygen

B

8. A mixture composed chiefly of potassium polysulfide and potassium thiosulfate: a. sulfur lac b. sulfurated potash c. sublimed sulfur d. washed sulfur

C

9. The energy required to remove an electron from a neutral atom is: a. electron affinity b. kinetic energy c. ionization potential d. electrical energy

A

10. These elements form basic anhydrides except one: a. S b. Na c. Mg d. Ca

B/C 11. Simethicone-containing antacids contain simethicone as: a. antacid b. antiflatulent c. antifoaming agent d. protective A

12. This element is used as a glucose tolerance factor: a. Cr b. Si c. Mg d. Mn

C

13. The first element produced artificially is: a. Rn c. Tc

b. Ta d. Pt

A

14. The reason reason why BaSO4 can be used or taken internally without causing any toxicity is that: a. it does not dissociate in the GIT b. it is soluble in the GIT c. the GI fluids can neutralize it d. it does not reach the GIT since it is a powerful emetic

D

15. Acids have the following properties except: a. sour taste c. neutralize bases

b. donor of protons d. pH above 7

16. Drug of choice to combat systemic acidosis: a. KHCO3 c. Na2CO3

b. NaHCO3 d. K2CO3

B

B

17. This metal, in the form of thin foil, is used as a protective for burn treatment due to its property of conserving fluids and of stimulating tissue growth;

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a. Sn c. Zn

b. Al d. Pd

B

18. Both iron and copper are found in which respiratory enzyme: a. trisinase b. cytochrome oxidase c. peroxide d. oxidase

D

19. Plaster of Paris is chemically: a. CaO b. CaSO4 c. CaSO4.1 1/2H2O d. CaSO4.2 H2O e. (CaSO4)2 H2O 20. The gas considered officially as pharmaceutical inhalant: a. oxygen d. a & b only b. nitrous oxide e. all of the above c. carbon dioxide

E

D

21. Also known as salt-forming group of elements are the: a. alkali metals d. halogens b. alkaline earth metals e. coinage metals c. chalcogen

B

22. The major side effect from the use of barium barium sulfate suspension as radiopaque is: a. diarrhea b. constipation c. vomiting d. dizziness

C

23. The alum a. b. c.

silicate which is antidiarrheal: pumice bentonite kaolin

C

24. Fehling’s a. b. c.

& Benedict’s reagent, reagent, used to determine the presence of reducing sugars contain which which salt: CaSO4 d. MgSO4 NiSO4 e. SrSO4 CuSO4

B

25. Substance added to glass to improve its coefficient of expansion: a. MnO2 b. B c. K d. Pb

D

26. Which vitamin enhance the physiological utilization of Ca in the body? a. Vitamin B12 d. Vitamin D b. Vitamin C e. Vitamin E c. Vitamin C

B

27. A thyroid disorder known as goiter is caused by the lack of: a. calcium b. iodine c. sodium d. potassium

A

28. Salts of these alkaline metals are used as sedative depressant in psychiatry: a. lithium b. iridium c. potassium d. calcium

C

29. The element present in hemoglobin of the blood which plays plays an important role in red blood cell-oxygen transport is: a. Ca b. Mg c. Fe d. P

A

30. Besides activated charcoal and tannic acid, the other component of universal antidote is: a. MgO d. MgCl2 b. MgCO3 e. Mg(OH)2 c. Mg3(PO4)2

B

31. In the form of its salt, salt, this ion is essential to life being the structural basis of skeleton, an important factor in blood coagulation: a. Mg b. Ca c. Zn d. PO4

D

32. This element is present in insulin:

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d. attapulgite e. calamine

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a. Cu b. Fe c. Mg D

C

33. Oxygen and ozone are: a. isotopes c. polymorphs 34. Softest mineral known: a. calamine b. kaolin c. talc

d. Zn e. Co

b. isobars d. allotropes

d. bentonite e. silica

A

35. A 10 volume hydrogen peroxide is equivalent to ______% H2O2: a. 3% b. 9% c. 20% d. 30%

B

36. Mineral chameleon is the synonym of the powerful oxidizing agent: a. NaI b. KMnO4 c. MnO2 d. KNO3

B

37. This ion is used very effectively as astringent, protective and antiperspirant: a. Mg b. Al c. Zn d. Cu

C

38. Strong iodine solution contains KI for the purpose of: a. preservation b. reducing agent c. preventing precipitation d. none of the above

D

39. Prepared chalk or precipitated chalk is chemically known as: a. MgCO3 b. Na2CO3 c. Ca3(PO4)2 d. CaCO3

B

40. Rochelle salt which is used as a cathartic and also as sequestering agent is: a. KHC4H4O6 b. NaKC4H4O6 c. KSbOC4H4O6 d. Na2C4H4O6

C

41. A metal which is unaffected by body fluids and attaches itself to bones, is now used in surgical repairs of bones, nerves and muscles: a. aluminum b. iron c. tantalum d. tin

D

42. Blue vitriol, an effective astringent and emetic is chemically: a. FeSO4-7H2O b. CaCl2 c. CU(C2H3O2)2 d. CuSO4 5H2O

B

43. All of the following ions are present in the intracellular fluids except: + + a. K b. Na 2+ -3 c. Mg d. HPO4

C

44. Bordeaux mixture used as fungicide contains: a. selenium sulfide b. magnesium sulfate c. cupric sulfate d. silver nitrate

A

45. Calomel is: a. HgCl c. stannous fluoride

b. HgCl2 d. ZnCl

46. Amalgams are alloys of: a. iron c. copper

b. zinc d. mercury

D

D

47. The most electronegative element in the periodic table is: a. sulfur b. oxygen c. chlorine d. fluorine

C

48. White vitriol is referred to:

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a. CuSO4-5H2O c. ZnSO4-7H2O

b. FeSO4-7H2O d. H2SO4

D

49. Saltpeter, a meat preservative is the synonym for: a. KNO2 b. NaNO3 c. NaNO2 d. KNO3

A

50. Most abundant and essential of all elements: a. oxygen c. hydrogen

b. silicon d. nitrogen

51. The following are aluminum salts except: a. alum c. kaolin

b. borax d. pumice

B

D

52. Electrolyte replenisher in dehydration: a. sodium iodide b. potassium iodide c. sodium bromide d. sodium chloride e. sodium sulfate

A

53. Cream of tartar is: a. potassium bitartrate c. KCl

b. sodium bitartrate d. sodium carbonate

C

54. Employed topically as astringent and protectant in ointment: a. HgS b. CdO c. ZnO d. HgO

D

55. A substance which takes up water or moisture but does not dissolve is: a. dehydrating agent b. deliquescent c. efflorescent d. hygroscopic

D

56. Ammonia is used as: a. anesthetic c. respiratory depressant

b. expectorant d. respiratory stimulant

C

57. To kill microorganism in inanimate objects we simply used: a. antiseptic b. corrosive c. disinfectant d. sterilization

A

58. Laughing gas is a: a. general anesthetic c. disinfectant

b. caustic d. local anesthetic

59. Increases osmotic load of the GIT: a. bulk-forming laxative c. saline cathartic

b. emollient laxative d. stimulant laxative

60. Inert gas with anesthetic properties: a. argon c. krypton

b. helium d. neon

C

C

A

61. The ion that gives a Turnbulls’ blue precipitate with potassium ferricyanide: a. ferrous b. ferric c. cobalt d. nickel

B

62. It forms white precipitate with HCl but blackens upon addition of ammonium hydroxide: a. cupric b. mercurous c. plumbous d. silver

D

63. The ion that gives a purple solution with sodium bismuthate: a. cobalt b. ferrous c. ferric d. manganese

A

64. Which of the following is a native of hydrous magnesium silicate: a. talc b. pumice c. kaolin d. bentonite

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A

65. The ion that gives a Prussian blue precipitate with potassium ferrocyanide: a. ferric b. ferrous c. cobalt d. nickel

B

66. The mechanism of action in the use of carbon as anti-diarrheal is: a. absorption b. adsorption c. precipitation d. oxidation

A

67. Physiologically inert substances added to the main component of the tablet so it will be convenient to swallow are termed as: a. diluent b. lubricant c. surfactants d. thickening agent

D

68. Some of the uses of astringent are: a. anti-perspirant c. styptic

b. caustic d. all of these

D

69. Best radiopharmaceutical agent for bone imaging: a. Tc99m IDA b. Tc99m albumin colloid c. Tc99m Ferpentate d. Tc99m etidronate

C

70. All of the following are mechanisms of anti-microbial action, except: a. oxidation b. halogenation c. hydrolysis d. precipitation

A

71. The ion that gives a white precipitate with HCl which is soluble in excess ammonium hydroxide but reprecipitated upon addition of nitric acid: a. silver b. plumbous c. mercurous d. cupric

D

72. The ion that gives positive result to Rinman’s Green Test: a. aluminum b. chromium c. manganese d. zinc

C

73. According to this law, the rate of the reaction is proportional to the product of the concentrate of the reactants to the power of its coefficient in a balanced equation: a. Law of Conservation of Mass c. Law of Mass Action b. Law of Definite Proportion d. Le Chatelier’s Principle

B

74. An agent that loses one or more electrons in a redox reaction: a. oxidizing agent b. reducing agent c. catalyst d. inhibitor

C

75. Nickel ion in solution is colored: a. colorless c. green

b. blue d. yellow

A

76. Describes a process or reaction that absorbs heat: a. endothermic b. exothermic c. miscible d. immiscible

B

77. Aluminum reagent is chemically known as: a. aluminum salt of carboxylic acid b. aluminum salt of aurintricarboxylic acid c. aluminum salt of tricarboxylic acid d. none of the above

B

78. The ion that produces an intense blue colored solution with an excess ammonia and a reddish brown precipitate with potassium ferrocyanide: a. cuprous b. cupric c. cadmium d. zinc

A

79. The ion that gives positive result to Thenard’s Blue Test: a. aluminum b. chromium c. manganese d. zinc

B

80. The ion that gives a yellow precipitate with NaOH and scarlet red precipitate with an excess KI: a. mercurous b. mercuric c. plumbous d. bismuth

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A

81. The following can cause a shift of equilibrium except: a. catalyst b. concentration c. pressure d. temperature

A

82. They are called the “soluble group”: a. alkali metals c. aluminum-iron group

b. alkaline earth metals d. silver group

A

83. In the cation analysis, group I ions are often called: a. insoluble chloride group b. soluble chloride group c. soluble sulfide group d. insoluble sulfide group

B

84. In semi-micro procedures, the process of filtration is replaced by the use of: a. vacuum b. centrifuge c. buchner funnel d. all of the above

A

85. It shows a similar properties to that of sodium and potassium: a. ammonium b. barium c. calcium d. magnesium

A

86. A state in which the rate of forward and reverse reactions are the same: a. chemical equilibrium b. equilibrium c. bond length d. bond order

B

87. A rule that states that when a stress is applied to a system in equilibrium, the equilibrium shifts to relieve the stress: a. Law of Mass Action b. Le Chatelier’s Principle c. Law of Conservation of mass d. Law of Definite Proportion

A

88. Blood red colorization with CNS but a blue precipitate with hexacyanoferrate(II): a. ferric b. calcium c. magnesium d. cobalt

A

89. A measure of a solution’s acid strength, the negative common log of the [H3O ]: a. pH b. pOH c. Ka d. Kb

A

90. The isotope used in the determination of the volume of red blood cells and total blood volume: a. Cr-51 b. Co-58 c. Fe-59 d. Ra-226

A

91. The amphoteric property of this compound prevents systemic alkalosis: a. Al(OH)3 b. Ca(OH)2 c. Mg(OH)2 d. Pb(OH)2

A

92. Radiopharmaceutical agent for thyroid function a. sodium iodide 1-131 b. Tc-99m-Entidronate c. Tc-99m-Phytate d. Tc-99

A

93. Substance that shows strong conductivity property and a high degree of ionization: a. Strong electrolyte b. Non-electrolyte c. weak electrolyte d. buffer

C

94. The chemical properties of the elements depend upon the extent to which their electrons are: a. replaced b. completed c. lost d. redistributed

B

95. It gives the spatial orientation of the electron cloud with respect to the three areas in space: a. Spin quantum number b. Magnetic quantum number c. Principal quantum number d. Azimuthal

C

96. An acid which is a proton donor yield a:

+

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a. base c. conjugate base

b. salt d. conjugate acid

A

97. Substances that absorb moisture from the atmosphere and dissolve in it is said to be: a. deliquescent b. efflorescent c. hydrolysis d. none of the above

B

98. This compound when mixed with the hemoglobin of the blood, results in asphyxial death: a. carbon dioxide b. carbon monoxide c. nitrogen oxide d. sulfur dioxide

B

99. The following are oxidizing agents, except: a. K2Cr2O7 c. I2

b. Na2C2O4 d. KMnO4

D

100. The sum of the number of protons and neutrons of an atom: a. atomic weight b. isotopes c. atomic number d. mass number

C

101. All are iodine-containing preparations, except: a. Betadine b. Iodine tincture c. Formol d. Lugol’s solution

B

102. The _______ of any liquid is the temperature at which the liquid phase and the solid phase are in equilibrium under a pressure of one atmosphere: a. vapor pressure b. freezing point c. evaporating point d. boiling point

A

103. Epsom salt is synonymous to: a. Magnesium sulfate c. Cadmium sulfate

b. Calcium sulfate d. Zinc sulfate

B

104. A preparation made by incorporating a solution of lead subacetate with an ointment base consisting of wool fat, white wax, white petroleum and camphor: a. white lead b. Goulard’s cerate c. sugar of lead d. Goulard’s extract

C

105. The smallest particle of matter which enters into a chemical combination a. molecule b. element c. atom d. compound

D

106. Halogen used as a common water disinfectant a. iodine b. bromine c. fluorine d. chlorine

C

107. Transfer of solvent molecules thru a semi permeable membrane a. diffusion b. distillation c. osmosis d. condensation

A

108. Weight of a solute in a given quantity of water is known as ________ of solution: a. concentration b. weight c. volume d. dissolution

C

109. The chloride of this metal is an astringent, antiperspirant and deodorant: a. Mn b. Ga c. Al d. Ca

A

110. Copper imparts a characteristic _________ color to a nonluminous flame a. emerald green b. scarlet c. blue d. golden yellow

C

111. Weak electrolytes are: a. unstable solution b. strong conductor of electricity

c. poor conductors of electricity d. non-conductors of electricity

D

112. Examples of protective from inorganic compounds except: a. Kaolin b. Calamine c. Zinc oxide d. Glycerol

B

113. Laughing gas is for _________ preparation

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a. sedative c. protective B

B

A

B

b. anesthetic d. antacid

114. Heavy water is: a. H2O2 c. T3O

b. D2O d. H2O

115. Element common to all acids: a. oxygen c. chlorine

b. hydrogen d. all of the above

116. For treatment of mental ailments: a. Li2CO3 c. CaCO3

b. Na2CO3 d. K2CO3

117. Cinnabar is chemically: a. HgCl c. Zn

b. HgS d. ZnSO4

C

118. Oxides of typically non-metallic elements are: a. neutral b. basic c. acidic d. ampheteric

D

119. The law that expresses the relationship between pressure, volume and temperature of gases in the equation, PV = nRT, where n = no. of moles of gas and R is constant which is the same for all gases that behave ideally is known as: a. Gay-Lussac’s Law b. Boyle’s Law c. Charles’ Law d. Ideal Gas Law

A

120. Most active of metallic elements: a. alkali metals c. base metals

b. oxidizing agent d. solubilizing agent

C

121. Attractive forces created by the polarizability of molecules and are exerted when two uncharged atoms approach very closely: a. carbon bond b. protein binding c. Van der Waals Forces d. covalent bond

D

122. This element is poisonous even in free metal form: a. magnesium b. silver c. aluminum d. mercury

A

123. These are salts of chlorine except: a. salt peter c. bleaching powder

b. rock salt d. calomel

C

124. Benzalkonium chloride is a germicidal surfactant which is rendered inactive in the presence of: a. organic acid b. gram negative organism c. soaps (anion agents) d. inorganic salts

C

125. It is the gas liberated upon the action of water on acids or metals whenever phosphorus is present as a contaminant: a. hydrogen sulfide b. methane c. phosphine d. carbon tetrachloride e. formaldehyde

B

126. The technique used to detect the presence of trace amounts of metal a. mass spectroscopy b. atomic absorption spectroscopy c. NMR spectrophotometry d. UV-visible spectrophotometry

contaminants:

C 127. Dimercaprol (BAL) acts as an antidote by a process called: a. oxidation b. reduction c. chelation d. absorption e. adsorption www.brex.us

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A

128. A solution made up of a weak base and its salt which resists changes in pH is called: a. buffer solution b. isotonic solution c. neutral solution d. normal solution

D

129. Calcium absorption and distribution are under a complex hormonal control of: a. parathyroid hormone b. calcitonin c. thyrocalcitonin d. all of the above

B

130. Potassium supplements are administered in all of the following manners except: a. IV infusion b. rapid IV injection c. elixir p.o. d. effervescent salts e. slow release p.o

B/C 131. After oral administration, the greatest amount of iron absorption occurs in the: a. duodenum b. stomach c. sigmoid portion of the large intestine d. ascending portion of the large intestine C

132. Copper imparts a characteristics ____ color to a nonluminous flame: a. blue b. scarlet c. green d. emerald green

D

133. A specific antidote for the treatment of poisoning due to oral ingestion of silver nitrate would be the oral administration of: a. KMnO4 solution b. vegetable oil c. acetic acid solution d. normal saline e. sodium bicarbonate

B

134. The following will react with water to form basic solution: a. sulfur trioxide b. ammonia c. nitrogen dioxide d. carbon dioxide

A

135. An ion that often shows expectorant action is: a. iodide d. iodate b. phosphate e. perchlorate c. fluoride

A

136. W hich of the following reduces iodine? a. sodium thiosulfate b. potassium chloride c. sodium hydroxide d. magnesium sulfate e. none of the above

B

137. Radioisotopes decay: a. at the same rate b. randomly c. rapidly

d. slowly e. only when catalyzed

D

138. Lugol’s solution contains this element as its active component: a. fluorine d. iodine b. chlorine e. potassium c. bromine

A

139. The composition of aqua regia is: a. 3HCL and HNO3 c. 2HNO3 and 1HCl

b. 2HNO3 and 2HCl d. 1HNO3 and 2H2SO4

140. Index of protective power of colloids: a. zigmondy c. dolomite

b. nuggets d. none of the above

A

D

141. This halogen is employed in the prevention of dental caries:

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a. chlorine c. iodine A

D

b. bromine d. fluorine

142. Burrows solution is also known as: a. aluminum acetate solution c. sodium borate

b. lead acetate d. none of the given choices

143. Densest element in the periodic table: a. rubefacient c. Pd

b. Pb d. Os

D

144. This instrument used to measure sodium and potassium in quantitatively: a. polarimeter b. spectrophotometer c. refractometer d. flame photometer

C

145. Hard water does not lather with soap. This is due to: a. K b. Al and O c. Mg and Ca d. Zn and Pb

C

146. The acid found in the stomach is: a. lactic c. hydrochloric

b. acetic d. citric

D

147. Occurs when either the salts of various organic acids or organic substituted ammonium salts are added to aqueous solutions of non-electrolytes: a. clathrate formation b. salting out c. solid-in-solid complex d. salting in

C

148. The major physiological ions include the following except for: a. sodium d. phosphorus b. potassium e. calcium c. manganese

C

149. The following are photometric methods of analysis, except: a. turbidimetry b. spectrophotometry c. chromatography d. flame photometry

D

150. Science that deals with the methods of extracting the metal from their ores: a. thermochemistry b. mineralogy c. electrochemistry d. metallurgy

B

151. Universal antidote includes: a. sodium bicarbonate c. magnesium hydroxide

b. activated charcoal d. none of the above

152. Sulfate of this metal is an emetic: a. calcium c. copper

b. gold d. silver

C

D

153. A homogenous molecular dispersion of two or more substances: a. suspension b. emulsion c. gel d. solution

B

154. Group of elements which is considered to be the most reactive of all metallic elements: a. Group O b. Group I-A c. Group I-B d. Group II

D

155. A powerful reducing agent used in medicinal preparation: a. oxygen b. hydrogen peroxide c. nitrogen d. hypophosphorous acid

B

156. Irritative phenomenon to the skin and mucus membrane exhibited by rashes and headaches when excessive amount of Iodine is administered: a. Hyperiodism d. any of the given b. Iodism e. none of the above c. Hypoiodism

C

157. Salts are formed as a result of the reaction between except: a. inorganic acid and as inorganic base b. water and a metal

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c. water and non-metallic element d. an organic acid and an inorganic base D

158. Epsom salt is used as: a. antiphlogistic c. cathartic

b. anticonvulsant d. any of these

D

159. The following are official combinations of electrolyte infusions except: a. Oral Electrolyte Solutions b. Lactated Ringer’s Injection c. Ringer’s Injection USP XX d. Dextrose 5% Injection

B

160. Antidote for Wilson’s disease: a. deferoxamine mesylate c. dimercaprol

b. penicillamine d. physostigmine

B

161. Which of the following Group O elements is recovered form the radioactive decay of radium: a. helium b. radon c. krypton d. argon

B

162. Nitrogen a. respirable air c. St. Elmos Fire

b. mephitic air d. dephlogisticated air

A

163. An organic compound which may either be a weak acid or a weak base that can change color at a definite pH value. a. indicator b. catalyst c. buffers d. tablets

C

164. Sodium citrate a. germicidal c. reduce blood clotting time

D

D

D

b. solubilizer of iodine d. acidifier

165. These ions are cathartic in action except: a. phosphate b. Sulfate c. tartrate

d. acetate e. magnesium

166. Chemical name of Green Vitriol: a. Copper Sulfate b. Magnesium Sulfate c. Sodium Sulfate

d. Ferrous Sulfate e. None of the above

167. Chemical name of Caustic soda: a. Potassium Hydroxide b. Magnesium Hydroxide c. Calcium Hydroxide

d. Sodium Hydroxide e. None of the above

E

168. Commercial preparations of Simethicone containing antacids: a. Di-gel d. a and c only b. Mylanta e. all of the above c. Simeco

C

169. Official water used for the extemporaneous compounding of the parenterals for either IV or IM injection is: a. water for injection b. bacteriostatic water for injection c. sterile water for injection d. none of these

D

170. An aqueous solution of this acid will color turmeric paper brownish red: a. sulfuric acid b. hydrochloric acid c. nitric acid d. boric acid

C

171. Which of the following is a coinage metal: a. barium c. copper

A

b. magnesium d. strontium

172. Gas responsible for the oxidative changes in fats, paints and oil:

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a. oxygen c. carbon dioxide

b. carbon monoxide d. hydrogen

E

173. Reasons for controlling pH within certain specified limits are: a. chemically stability d. a and c only b. solubility of the drug e. all of the above c. patient’s comfort

D

174. Chemical name of China Clay: a. Lead acetate b. Copper sulfate c. Magnesium Trisilicate

d. Kaolin e. none of the above

E

175. Pharmaceutic aid used to displace air to increase the shelf life of an oxidizable product: a. oxygen d. nitrous oxide b. carbon dioxide e. nitrogen c. helium

B

176. A measure of the acidity of a solution a. pOH c. buffer

b. pH d. density

C

177. Preparations used for brain scanning to determine the presence and location of neo-plastic lesions: a. Gold Au 198 Injection b. Chlormerodrin Hg 197 Injection c. Technetium Tc99 Injection d. Sodium Phosphate P32 Solution

B

178. Tartar emetic a. syphilis c. scabicide

b. schistosomiasis d. all of these

A

179. It is used as an inhalant in all pathological conditions accompanied by cyanosis and dyspnea: a. oxygen d. nitrous oxide b. carbon dioxide e. nitrogen c. helium

D

180. Produced by filling an orbital by an electron which is not removed from its atom but is held mutually or “shared” by 2 atoms concerned: a. coordinate bond b. chemical bonds c. hydrogen bond d. covalent bond

C

181. Which of the following elements imparts a characteristics violet color to non-luminous flame: a. sodium b. ferric c. potassium d. copper

D

182. Generic term referring to vitreous material: a. plastic b. tin c. vitriol

d. glass e. none of the above

A

183. The syllable “bi” in sodium bicarbonate and sodium bi-phosphate indicates that they are: a. acids salts b. compounds composed of two elements c. neutral salts d. basic salts

B

184. They are chemical compounds containing elements of high atomic numbers which will stop the passage of x-rays: a. roentgen rays b. radiopaque contrast media c. radiopharmaceuticals d. isotopes

A

185. Brand name of Al(OH)3 a. amphogel c. alum

A

b. phosphagel d. all of these

186. Are compounds which have the capability of functioning chemically as reducing agents: a. antioxidants d. both a and c b. buffers e. none of the above c. preservatives

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A

187. They are preparations containing radioisotopes which are used internally for therapeutic and diagnostic purposes: a. radiopharmaceuticals b. roentgen rays c. radiopaque contrast media d. isotopes

A

188. Which of the following ions is colored blue in solution? a. cupric b. cuprous c. ferric d. ferrous

C

189. The formation of dental caries is distributed to the action of acids, mostly _____, obtained from oral bacterial metabolism of dietary carbohydrates: a. narcotic acid b. citric acid c. lactic acid d. malic acid

B

190. When too much fluoride is present in the tissue fluid, it can develop condition known as “dental fluorosis” which is also known as: a. mottled teeth b. mottled enamel c. mottled dentin d. dental caries

D

191. Compound responsible for the pink color of Calamine USP 24: a. Talc d. Ferric oxide b. Zinc oxide e. FD and C Red c. zinc stearate

B

192. It is administered in an ice-cold condition to lessen its disagreeable bitter taste; parenterally used as an anticonvulsant: a. Rochelle salt b. Epsom salt c. Glauber’s salt d. Purgative lemonade

B

193. Pharmaceutical ingredient of Calamine USP 24: a. Talc b. Zinc oxide c. Zinc stearate d. Ferric oxide

C

194. Which of a. b. c. d.

E

195. The equilibrium constant for the dissociation of a weak acid of the type, HA=H+ + A , would be: a. [A ][HA] d. [H+][A ] b. [HA][A ]/[HA+] e. [H+][A ]/[HA] c. [HA]/[[H+][A ]

D

196. An anti-microbial used in the preparation of white lotion: a. ammoniated mercury d. sulfurated potash b. sublimed sulfur e. selenium sulfide c .precipitated sulfur

D

197. The cation/s that cause/s this group of antacids to have constipating property: +3 a. Al d. a ad c +2 b. Mg e. none of them +2 c. Ca

C

198. An antacid with a very rapid onset of action but relatively short duration; can cause belching and flatulence due to the production of gas: a. magnesium hydroxide b. aluminum hydroxide c. sodium bicarbonate d. calcium phosphate

A

199. It is the basis of smelling salts and occasionally used as leavening agent hence the name of “Baker’s Ammonia”: a. Ammonium Carbonate d. Ammonium Hydroxide b. Aromatic Spt. of Ammonia e. All of them c. Ammonium Chloride

C

200. An anti-microbial agent that may be used to disinfect drinking water in 3 drops per quart; will kill amoeba and bacteria in 15 mins:

the following are examples of covalent bonds? The bond that hold water molecules together The bonds that hold the two strands of a double-stranded DNA molecules together Peptide bonds and glycosidic bond The bonds that hold Na and Cl together in molecules of table salt -

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a. Pot. Permanganate b. Sod. Hypochlorite c. iodine

d. hydrogen e. all of them

B

201. Used as respiratory stimulant by inhaling the vapors: a. ammonium carbonate d. ammonium hydroxide b. aromatic spt. Of ammonia e. all of them c. ammonium chloride

A

202. A compound added to some antacids to serve as defoaming agent to prevent flatulence a. simethicone b. magaldrate c. alginic acid d. sodium bicarbonate

A

203. The molarity of a solution is: a. The number of moles of solute per liter of solution b. The number of moles of solute dissolved in kg solvent c. The number of equivalent weights per liter of solution d. The number of moles of solvent per kg of solution e. The weight in g of solute per 100 ml of a solution

E

204. The form of water most commonly used as a solvent during the manufacture of parenterals is: a. Bacteriostatic water for injection USP b. Deionized water c. Distilled water d. Sterile water of injection USP e. Water for injection

A

205. This is used to describe the approximate measure of the sized of the electron cloud a. principal quantum number d. spin quantum number b. azimuthal quantum number e. all of the above c. magnetic quantum number

B

206. If the ion product is less than Ksp, the solution is: a. saturated d. concentrated b. unsaturated e. diluted c. supersaturated

D

207. Which of the following acid/conjugate base pairs would function best as a buffer at physiological pH? a. lactic acid / lactate ion, -pKa = 3.86 b. carbonic acid / bicarbonate ion, -pKa = 6.37 c. bicarbonate ion / carbonate ion, -pKa = 10.25 d. dihydrogen phosphate / monhydrogen phosphate ion. –pKa = 6.86 e. acetic acid / acetate ion, -pKa = 4.76

B

208. A type or structure of complex where the interactant is a surfactant, a molecule possessing both a nonpolar and a polar portion: a. self-associated aggregate b. micelle c. inclusion complex d. inclusion complex

D

209. The method of preparation must be indicated on labels for: a. Bacteriostatic water for injection, USP b. Milk of Magnesia c. Sterile water for injection, USP d. Purified water, USP e. Water for injection USP

A

210. Conformation of organic molecules is most commonly determined by which of the following analytical method? a. nuclear magnetic resonance d. biological assay b. optical rotation e. mass specrtrophotometry c. pKa determination

D

211. Which of a. b. c.

C

212. Elements that are found as diatomic molecules include all except:

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the following is an example of triprotic acid? acetic acid d. phosphoric acid carbonic acid e. sulfuric acid sulfuric acid

14


a. oxygen b. fluorine c. potassium

d. iodine e. hydrogen

D

213. The Henderson-Hasselbach equation allows us to a. Calcualte the pKa of an acid from the pH of a solution of an acid b. Calculate the pH of the solution of an acid from the pKa of the acid c. Calculate the molar ratio of an acid from the pKa of its conjugate base d. Calculate the molar ratio of an acid and its conjugate base from the pKa of the acid and the pH of the solution of the acid e. Calculate the pH of the solution of a base from the pKa of its conjugate acid

C

214. Atoms in which two outermost electron shells are incomplete refer to: a. nobel or inert gases d. lanthanide series b. representative elements e. actinide series c. transition elements

E

215. If HCl is added to water until the solution contains 1 x 10 mole/L of the H ion, the concentration of OH ions is: -14 -6 a. 1 x 10 mole/L d. 1 x 10 mole/L -4 -10 b. 1 x 10 mole/L e. 1 x 10 mole/L -11 c. c. 1 x 10 mole/L

E

216. The following are properties of soft bases. Which does not belong to these bases? a. with low electronegativities d. with high polarizabilities b. have empty low-lying orbitals e. none of the above c. easily oxidized

A

217. It is equal to the product of the ionic concentrations (in moles per liter of saturated solution), with each concentration raised to the power indicated by the number of ions in the formula: a. Ksp d. Ki b. Ke e. any of the above c. Kw

E

218. The degree of dissociation of acids is often expressed in terms of pKa. pka then is a. directly measured by titration of the acid with sodium hydroxide b. calculated by determining the acid’s buffer capacity c. directly determined by conductivity measurement d. the natural log of the acid’s dissociation constant e. the reciprocal log of the dissociation constant

E

219. The solubility of a chemical in a given solvent is influenced by many factors. Which of the following physicochemical constants may not be useful in predicting the solubility of a chemical? a. pH of a solution d. solubility parameters b. dielectric constants e. valence of the chemical c. pKa of the chemical

A

220. Which of the following glass types does not contain soda lime? a. Type I d. Type IV or NP b. Type II e. all of the above c. Type III

C

221. The shrinkage occurring between the mixture of alcohol and purified water is primarily due to a. van der Waals forces d. ionic bonding b. covalent bonding e. temperature changes c. hydrogen bonding

A

222. Calculate the pH of a 0.08F solution of HCN. Ka is 7.2 x 10 a. 5.12 d. 7.26 b. 6.00 e. none of the above c. 7.60

B

223. A disease found in Japan caused by drinking water contaminated with cadmium: a. Minamata disease d. Addison’s disease b. Itai-itai disease e. none of the above c. Crohn’s disease

E

224. Which of the following is not a factor in influencing equilibrium of a chemical reaction?

-4

+

-

-10

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a. nature of reactant b. changes in pressure c. temperature changes

d. concentration changes e. none of the above

B

225. It contains iron in solution or in suspension and are characterized by a ferruginous taste. a. carbonated water d. Lithia water b. chalybeate water e. siliceous water c. saline water

B

226. Which of the following glass types makes use of water attack test type? a. Type I d. Type IV or NP b. Type II e. none of the above c. Type III

B

227. This refers to an electrically neutral unit formed when two or more atoms are joined together by covalent bond: a. ion d. element b. molecule e. mixture c. compound

E

228. Which of the following is not an action of sulfur? a. cathartic d. depilatories b. parasiticide e. Reye’s syndrome c. fumigation

A

229. This compound is primarily used in the preparation of Vleminck’s solution a. sublimed sulfur d. lithium carbonate b. milk of sulfur e. chlorine dioxide c. zinc oxide

E

230. Iron sorbitex is a chemical complex of: a. iron b. sorbitol c. citric acid

d. dextrin e. all of the above

D

231. The following are constituents of Ladd’s paste, except: a. aluminum powder d. silver nitrate b. liquid petrolatum e. none of the above c. zinc oxide

A

232. Which of the following is not an indication of hypophosphatemia? a. hypervitaminosis D b. hyperparathyroidism c. lack of phosphate reabsorption d. all of the above e. none of the above

C

233. This formula can be determined given the percent composition by mass of the compound a. molecular formula b. structural formula c. empirical formula d. electronic formula

B

234. The unit for molar mass of carbon-12 is a. mole c. atomic mass unit

b. gram d. gram/mL

235. If enthalpy is positive, the reaction is: a. exothermic c. spontaneous

b. endothermic d. reversible

B

B

A

236. The color of the flame produced by lithium a. yellow green b. crimson red c. brick red

d. violet e. intense yellow

237. Hyperphosphatemia may be found in a. hypoparathyroidism b. rickets c. hyperparathyroidism d. possible long term use of aluminum hydroxide gel antacid e. all of the above

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A

238. It is an official antidote for phosphorous poisoning a. blue vitriol d. oil vitriol b. white vitriol e. all of the above c. green vitriol

B

239. Which of the following elements acts as a catalyst for the storage and release of iron? a. chromium d. iodine b. copper e. manganese c. magnesium

D

240. Which of the following minerals is important in the antioxidant capabilities of vitamin E? a.. iron d. selenium b. zinc e. silicon c. chromium

C

241. In a REDOX reaction, the oxidizing agent a. is oxidized c. is reduced

b. loses electrons d. increased in oxidation state

D

242. Radioactive substances are characterized by: a. unstable nucleus b. emitting radiation c. low proton-neuron ratio d. all of the above

A

243. The rate of decay of radioactive substance is expressed in terms of: a. half-life b. angstrom c. curie d. amu

D

244. Crystallization in a supersaturated solution may be induced by: a. stirring the solution b. seeding c. scratching the inside wall of the test tube d. all of the above

D

245. Different nuclides having the same mass number: a. isotopes b. isotones c. isomer d. isobars

C

246. Principle which states that it is impossible to accurately determine simultaneously the position and motion of an electron a. Pauli’s Exclusion Principle c. Heisenberg Uncertainty Principle b. Aufbau Principle d. Planck’s Exclusion Principle

D

247. Which is not a colligative property? a. freezing point depression b. boiling point elevation

c. vapor pressure lowering d. melting point

C

248. When orbitals are of the same energy, electrons distribute themselves one to each orbital before pairing according to: a. Aufbau Principle b. Pauli’s principle c. Hund’s rule d. building principle

D

249. The following underlined elements has +5 oxidation state, except: a. IF5 b. H3SbO4 c. Bi(NO3)3 d. Na2Sn4O6

D

250. If one mole of oxygen molecule weighs 32 grams, how many molecules are present in one mole of O2? a. 8 b. 16 23 c. 32 d. 6.02 x 10

D

251. A reducing agent a. gains electrons c. is reduced

b. decreases in oxidation number d. is oxidized

A

252. Anode is a. b. c. d.

A

253. No two electrons in an atom can have all four quantum numbers the same.

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an electrode where oxidation takes place where reduction takes place where displacement takes place where decomposition takes place

17


a. b. c. d.

Pauli’s exclusion principle Planck’s exclusion principle Hund’s rule Aufbau principle

C

254. These are physical properties except: a. malleability of metals b. volatility of alcohols c. oxidation of iron d. solubility of sugar

A

255. A system in which two opposing reactions are proceeding at the same rate: a. chemical equilibrium b. chemical reaction c. chemical constant d. chemical kinetics

D

256. Going across a period from left to right and from bottom to top a group in the periodic table, which of the following periodicity laws decreases? a. electron affinity b. electronegativity c. ionization energy d. atomic size

B

257. The most abundant metal and the third most abundant element in the earth’s crust: a. sodium b. aluminum c. carbon d. copper

A

258. Which of the following is a polyatomic molecule and a compound? a. O2 b. CO2 –2 c. CO d. Co3

B

259. Which of the following statements is true of a 2 M HA, a weak acid at equilibrium: a. pH=2 b. [H+]=[A-] c. [H+]>[A-] d. HA = 2 M

D

260. Which of the following body fluids is least acidic? a. gastric juice = pH 1.2 b. urine = pH 5.5 c. saliva = pH 6.5 d. tears = pH 7.4

B

261. What is the effect of adding NH4Cl to a solution of NH4OH? a. increased [OH-] conc. b. decreased [OH-] conc. c. decreased NH4OH conc. d. conc. of NH4OH remains the same

D

262. Which hydroxide is not amphoteric? a. Al(OH)3 c. Cr(OH)3

b. Zn(OH)2 d. Mn(OH)2

263. Which of the following is not yellow? a. CdS c. Ag3PO4

b. Ag2CrO4 d. Ag3AsO3

264. Nessler’s reagent is used to identify + a. K + c. Na

b. NH4 + d. Al3

B

B

+

C

265. Used in the treatment of cystitis with methenamine a. sodium phosphate b. sodium sulfate c. sodium biphosphate d. sodium bicarbonate

A

266. Prolonged use of silver nitrate may lead to this undesirable discoloration of the skin a. argyria b. silverism c. Wilson’s disease d. hydrargyrism

D

267. This ion produces violet color to the non-luminous flame a. calcium b. sodium c. barium d. potassium

C

268. Radioisotopes can be produced from the following except:

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a. nuclear pile c. x-ray machine

b. cyclotron d. radioisotope cow

B

269. The radiopharmaceutical which is used as a diagnostic aid to determine blood plasma volume and cardiac output a. Chlormerodrin Hg 197 c. Sodium chromate 51 b. I131 Serum Albumin [Human] d. Gold 198

C

270. Which of the following salts has a pH>7? a. Na2SO4 c. CaC2O4

b. NH4CH3COO d. C2H5NHCl

B

271. Oxidation is a half-reaction a. that involves a gain of electrons b. that involves a loss of electrons c. takes place in the cathode d. where element decreases in oxidation no.

A

272. The ionization constant of the strongest acid is a. HA Ka = 7.2 x 10-4 b. HB Ka = 8.5 x 10-8 c. HC Ka = 7.5 x 10-5 d. HD Ka = 6.5 x 10-10

B

273. Used for a. b. c. d.

C

274. The following oxides are acidic with water except: a. Cl2O7 b. N2O3 c. FeO d. SO2

D

275. A mixture containing 30% ZnS and 70% BaS: a. hausemonite b. braunite c. copperas d. lithopone

D

276. Sb in the presence of HCl gives a violet precipitate with this pink dye a. dimethyl glyoxime b. p-nitorbenzene azoresorcinol c. aluminum reagent d. rhodamine B

D

277. Method of sterilizing sodium bicarbonate for parenteral use: a. autoclaving b. heating in an open vessel & re-saturating with sterile CO2 c. bacteriological filtration d. all of the above

B

278. The following are non-systemic antacids except: a. aluminum hydroxide b. sodium bicarbonate c. dihydroxy aluminum sodium carbonate d. calcium carbonate

C

279. NH4Cl is contraindicated in patients with a. diabetes mellitus c. impaired hepatic function

kidney imaging or determining renal function Technetium 99m-phytate Technetium 99 Heptagluconate Technetium 99 HIDA Technetium 99 Etidronate

+

b. diabetes insipidus d. alkalosis

D

280. The radiopharmaceutical used for the hepatobiliary studies a. sodium iodophippurate I-131 b. Tc-99m DTPA c. Tc-99m-ascorbic acid complex d. Tc-99m-HIDA

D

281. The indicator used for the USP limit test for arsenic a. methyl orange b. silver sulfadiazine c. eriochrome black

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d. Ag diethyldithiocarbamate D

282. Povidone-Iodine, a water soluble, non-toxic, non-staining and a slow releasing antiseptic is a complex of iodine with: a. EDTA b. Silver c. potassium d. polyvinyl pyrrolidone

B

283. Zinc deficiency characterized by thickened scaly inflammed skin is known as: a. seborrheic dermatitis b. parakeratosis c. skin ulcer d. none of the above

B

284. Primary HCO3 excess a. metabolic acidosis c. respiratory acidosis

-

b. metabolic alkalosis d. respiratory alkalosis

A

285. Dehydration and decreased renal blood flow are conditions of: a. hyperchloremia b. hypochloremia c. hyperkalemia d. hypokalemia

A

286. The following are respiratory stimulants except: a. soda lime b. carbon dioxide c. ammonium carbonate d. aromatic ammonia spirit

D

287. Anemia due to decreased blood formation can be caused by deficiencies of key materials a. cobalamin b. folic acid c. pyridoxine d. all

D

288. Used as wet dressing for persons suffering from third degree burns a. H2O2 b. NaOCl c. AgNO3 d. KMnO4

C

289. A dentrifice which contains formalin and reduces the sensitivity of teeth to heat and cold a. Sensodyne b. pumice c. Thermodent d. none of the above

A

290. A halogen characterized as a dark, reddish brown, fuming liquid with suffocating odor: a. bromine b. iodine c. chlorine d. fluorine

B

291. Tartar emetic, known to be an effective antischistosomal agent is: a. KHC4H4O6 b. KSbOC4H4O6 c. NaKC4H4O6 d. KHC4H4O6

D

292. Use of sodium bisulfite a. protective c. dentrifice

b. cleansing agent d. anti-oxidant

293. Slaked lime is a. CaO c CaCO3

b. CaSO4 d. Ca(OH)2

D

D

294. Mechanism of antibacterial action of potassium permanganate solutions a. protein precipitation b. astringent c. halogenation d. oxidation

C

295. He discovered oxygen and called it empyreal air a. Priestly b. Beckerel c. Scheele d. Cavendish

C

296. MgNH4PO4 is the only __________ phosphate. a. yellow b. orange c. white d. blue

B

297. White precipitate is also known as: a. calomel c. calcium oxide

A

b. ammoniated mercury d. zinc sulfide

298. It acts as antacid in small doses, and as a laxative in large doses.

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a. magnesium b. manganese c. aluminum

d. iron e. copper

D

299. This compound is used as carbon dioxide absorber. a. ammonium carbonate b. potassium iodide c. barium hydroxide d. soda lime

C

300. The radiopharmaceutical that is used for kidney imaging or determining renal function. a. I-131-NaI c. Tc-99m-Heptagluconate b. I-131-Human Serum Albumin d. Tc-99m-Phytate

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Pharmaceutical Chemistry of Inorganic Medicals

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