Free Printable QC (PQ) 100

1.

Limit of moisture in non-aqueous titrimetric analysis is less than:

a)

0.5%

b)

0.05%

c)

0.2%

d)

0.02%

2.

Standard solution in non-aqueous titrimetric analysis-acidimetry

a)

Perchloric acid

b)

Hydrogen bromide

c)

Both A and B

d)

None of the choices

3.

Which of the following statement/s is/are correct?

I. Non-aqueous alkalimetry is used when the analyte is weakly acidic.

II. Non-aqueous alkalimetry is used when analyte is acid halide.

III. Non-aqueous alkalimetry is used when the analyte contains heterocyclic nitrogen compound.

IV. Non-aqueous alkalimetry is used when analyte is barbiturate.

a)

I only

b)

I and II only

c)

I, II, and III only

d)

I, II, and IV

4.

Indicator/s used in non-aqueous titrimetry:

I. Nile blue III. Malachite green

II. Crystal violet IV. Phenolphthalein

a)

I only

b)

I and II only

c)

I, II, and III only

d)

I, II, III, and IV

5.

Standard solutions in non-aqueous alkalimetry.

I. Lithium methoxide III. Hydrogen bromide

II. Perchloric acid IV. Sodium hydroxide

a)

I only

b)

I and II only

c)

I, II, and III only

d)

I, II, III, and IV

6.

Perchloric acid in glacial acetic acid and perchloric acid in dioxane are volumetric solution used in what type of analysis?

a)

Direct acidimetry

b)

Direct alkalimetry

c)

Non-aqueous acidimetry

d)

Non-aqueous alkalimetry

7.

A characteristic of a substance which is suitable for non-aqueous titrimetry is:

a)

A.

Weakly reactive

b)

B.

Weakly basic

c)

C.

Very soluble in water

d)

A and B

8.

The strongest of the known common acids which gives excellent results in the assay of weak bases and its salts

a)

Nitric acid

b)

Sulfuric acid

c)

Hydrochloric acid

d)

Perchloric acid

9.

A sample of Chlorpheniramine maleate weighing 0.502 g was assayed by non-aqueous titrimetry using 22.2 mL of perchloric acid with normality of 0.1125. Calculate the % purity of the sample. Each mL of 0.1 N perchloric acid is equivalent to 19.54 mg of C₁₆H₁₉ClN₂.C₄H₄O₄.

a)

97.2

b)

72.9

c)

27.9

d)

9.72

10.

This method of precipitation titration with Silver involved the formation of a colored complex.

a)

Mohr

b)

Volhard

c)

Fajan

d)

A and B

11.

Standard solution in precipitation method of analysis.

a)

Disodium edentate

b)

Silver nitrate

c)

Sodium methoxide

d)

Perchloric acid

12.

Use to prevent one element from interfering in the analysis of another element.

a)

Masking agent

b)

Demasking agent

c)

Both A and B

d)

None of the choices

13.

Argentometric titration is titration with _____ ion.

a)

Magnesium

b)

Sodium

c)

Silver

d)

Potassium

14.

Fajans titration uses _____ indicator.

a)

Acid base

b)

Adsorption

c)

Metal-ion

d)

None of the choices

15.

Ferric ammonium sulfate is used as indicator in the standardization of:

a)

Silver nitrate

b)

Ammonium thiocyanate

c)

Edentate disodium

d)

All of the choices

16.

The end point in using ferric ammonium sulfate is:

a)

White precipitate

b)

Red-brown color

c)

Pink color

d)

Blue color

17.

A molecule which provides groups of attachment to metal ions.

a)

Ligand

b)

Chelate

c)

Both A and B

d)

None of the choices

18.

The following is/are true about EDTA titration.

I. EDTA titration is also known as complexometric titration.

II. The equilibrium constant in EDTA titration is called stability constant.

III. For end-point detection, commonly used indicator is called EDTA indicator.

IV. EDTA titration technique includes displacement titration.

a)

I only

b)

II and III

c)

I, II, and III

d)

I, II, and IV

19.

Most of the official drugs containing Calcium and Magnesium are determined by:

a)

Gravimetric

b)

Complexometry

c)

Bioassay

d)

Non-aqueous matter

20.

Adsorption indicators are used in:

a)

Complexation reaction

b)

Acidimetry

c)

Volumetric precipitation

d)

Alkalimetry

21.

The indicator for EDTA titration against CaCO₃ is:

a)

Thymol blue

b)

Hydroxynaphthol blue

c)

Methyl red

d)

Methylene blue

22.

The primary standard used to standardize 0.05 M EDTA:

a)

Calcium carbonate

b)

Potassium biphthalate

c)

Sodium oxalate

d)

Calcium sulfate

23.

The compleximetric method of determining metal ion is:

a)

Volhard titration

b)

EDTA titration

c)

Permanganate titration

d)

Kjeldahl

24.

Adsorption indicators are used in

a)

Neutralization

b)

Precipitation

c)

Complexation

d)

Redox

25.

The end point of a reaction in analysis by precipitation methods may be determined by using an instrument which is

a)

Amperometric

b)

Refractometer

c)

Spectrometric

d)

Chromatographic

26.

A 0.2185 g sample of NaCl was assayed using Volhard method using 50 mL of 0.0998N silver nitrate and 11.9 mL of 0.1350 N ammonium thiocyanate. Calculate the % NaCl in the sample. MW NaCl = 58.45

a)

42.6

b)

62.4

c)

90.5

d)

6.24

27.

A 50 mL aliquot of solution containing 450 g of Magnesium sulfate in 0.5 L required 37.6 mL of EDTA solution for titration. How many mg of Calcium carbonate will react with 1 mL of this EDTA solution? MW Magnesium sulfate = 120.37; MW CaCO₃ = 100

a)

0.9943 mg

b)

9.99 mg

c)

99.94 mg

d)

994.3 mg

28.

The type of chemical reaction involved for Fe²⁺ + Ce^4- Fe³⁺ + Ce^3- is a or an:

a)

Acid base

b)

Precipitation

c)

Complex formation

d)

Oxidation reduction

29.

Other name of ferrous phenanthroline.

a)

Eosin Y

b)

Crystal violet

c)

Ferroin

d)

Ferric alum

30.

Color of the complex resulting from reaction with ferrous phenanthroline

a)

Blue

b)

Red

c)

Pink

d)

Violet

31.

Primary standard in the standardization of ceric sulfate solution

a)

Potassium hydrogen phthalate

b)

Calcium carbonate

c)

Sodium bicarbonate

d)

Arsenic trioxide/Sodium oxalate

32.

A substance which gains electrons in a redox reaction.

a)

Oxidizing agent

b)

Reducing agent

c)

Both A and B

d)

None of the choices

33.

Indicator in Redox Titration using KMnO₄.

a)

Starch TS

b)

KMnO₄

c)

Methyl red TS

d)

Methyl orange

34.

Orthophenanthroline TS is used as indicator in:

a)

Permanganometry

b)

Ceric sulfate titration

c)

Iodometry

d)

Iodimetry

35.

Which of the following statement/s is/are true?

I. KMnO₄ can be standardized using arsenic trioxide.

II. KMnO₄ serves as indicator in acidic solution.

III. Hydrogen peroxide can be analyzed using KMnO₄.

IV. KMnO₄ in acidic solution is reduced to colorless Mn⁺².

a)

I and II

b)

I, II and III

c)

II, III, and IV

d)

I, III, and IV

36.

Koppeschaar’s solution is also known as:

a)

0.1 N Iodine solution

b)

0.1 N Bromine solution

c)

0.1 M sodium nitrite solution

d)

0.1 N sodium thiosulfate solution

37.

0.1N Bromine solution is employed as:

a)

Oxidizing agent

b)

Reducing agent

c)

Masking agent

d)

Demasking agent

38.

Dichlorophenol-indophenol solution is standardized using:

a)

Sulfanilamide USP

b)

Ascorbic acid USP

c)

Sulfathiazole USP

d)

Resorcinol USP

39.

The oxidation number of Mn in KMnO₄ is:

a)

+2

b)

+1

c)

+5

d)

+7

40.

Which of the following standard solutions is not used in redox titration?

a)

Sodium thiosulfate solution

b)

Iodine solution

c)

Bromine solution

d)

Sodium hydroxide solution

41.

This method of analysis involve a change in valence of the reacting substances:

a)

Neutralization

b)

Precipitation

c)

Complexation

d)

Redox

42.

Calculate the weight of oxalic acid required to prepare 1000 mL of 0.5 N of the solution. MW = 126

a)

36.5 g

b)

63.5 g

c)

31.5 g

d)

23.5 g

43.

If starch TS is used as an indicator, the end point is/are:

a)

Appearance of intense blue color

b)

Disappearance of intense blue color

c)

Both of the choices

d)

None of the choices

44.

Use of KI in the preparation of iodine solution.

a)

Solubilizing agent

b)

Change in pH of the solution

c)

As preservative

d)

All of the choices

45.

Indicator in Iodometric method of analysis.

a)

KMnO₄

b)

Methyl red TS

c)

Methyl orange TS

d)

Starch TS

46.

The use of chloroform in sodium thiosulfate solution.

a)

To stabilize the solution

b)

To increase its solubility

c)

To prevent bacterial growth

d)

To maintain the pH of the solution

47.

The use of sodium bicarbonate in the standardization of iodine solution

a)

Increases the solubility

b)

As buffer

c)

As preservatives

d)

To prevent bacterial growth

48.

What is the use of HgI₂ in the preparation of starch TS?

a)

To increase the solubility of starch

b)

To impart color

c)

As a preservative

d)

To stabilize the pH

49.

The active fraction of starch which reacts with the iodine to form an intense blue color

a)

Amylopectin

b)

Amylose

c)

Glucose

d)

Sucrose

50.

When a reducing analyte is titrated directly with iodine, the method used is called

a)

Iodometry

b)

Iodimetry

c)

Cerimetry

d)

Permanganometry

51.

The 0.1N Iodine solution is standardized using:

a)

Potassium permanganate

b)

Potassium hydrogen phthalate

c)

Arsenic trioxide

d)

Sodium carbonate

52.

Assay of sulfa drugs can be determined by this reaction with sodium nitrite.

a)

Neutralization

b)

Complexation

c)

Precipitation

d)

Diazotization

53.

Which of the following volumetric solutions is used in diazotization analysis of sulfa drugs?

a)

0.1 M sodium nitrite

b)

0.05 Edentate disodium

c)

0.01 M sodium nitrite

d)

0.1 N Iodine solution

54.

Phenol is assayed using this method of analysis.

a)

Residual alkalimetry

b)

Volumetric precipitation

c)

Residual iodometry using excess bromine

d)

Iodimetry

55.

Assay of sodium nitrite is an example of what method of analysis

a)

Direct titration – Redox

b)

Indirect titration – Redox

c)

Residual titration – Redox

d)

Iodimetry

56.

It is employed as an oxidizing agent in the assay of aniline, phenol and resorcinol

a)

0.1 N Iodine

b)

0.1 N Bromine

c)

0.1 N Potassium

d)

0.1 N Oxalic acid

57.

The titrant in the assay of sodium hypochlorite solution is:

a)

0.1 N Sodium thiosulfate

b)

0.1N Iodine solution

c)

0.1 N KMnO₄

d)

0.1 N Oxalic acid

58.

The solubility of iodine in water is one gram of iodine is soluble in:

a)

2920 mL

b)

2930 mL

c)

2940 mL

d)

2950 mL

59.

A 4.0570 g sample of chlorinated lime was mixed with enough water to make 1000 mL. A 100 mL of the mixture was treated with Potassium iodide and Acetic acid, then titrated with 22.4 mL of Sodium thiosulfate solution. A 20 mL sample of Sodium thiosulfate was found to be equivalent to 0.2996 g of pure iodine. Calculate the available chlorine in the sample. MW Iodine = 126.9; MW Cl = 35.45

a)

27.35%

b)

27.45%

c)

29.02

d)

23.1

60.

A 0.5110 g samples of Sulfathiazole was assayed using 18.8 mL of 0.1005 M Sodium nitrite solution in a titration. Each mL of 0.1 M Sodium nitrite is equivalent to 25.53 mg of C₉H₉N₃O₂S₂. Calculate the % C₉H₉N₃O₂S₂ in the sample.

a)

99%

b)

95%

c)

94%

d)

93%

61.

A sample of 0.1350 g of As₂O₃ was assayed iodimetrically using 23.4 mL of 0.1055 N iodine solution (Atomic Weights: As = 74.92, O = 16). The percentage purity of the sample is:

a)

90.44

b)

90.23

c)

89.0

d)

90.54

62.

Twenty tablets of Ascorbic acid weighed 4.250 g and a powdered sample of 0.3075 g used up 21.5 mL of 0.1085 N iodine solution. What was the amount of Ascorbic acid per dose of 2 tablets? Each mL of 0.1 N iodine is equivalent to 8.80 mg of C₆H₈O₆ (Ascorbic acid). The amount is:

a)

283.7 mg

b)

141.86 mg

c)

0.2837 g

d)

A and C

63.

Which of the following statement/s is are correct according to USP 27?

I. In azeotropic method of water of analysis toluene is used as solvent.

II. In azeotropic method of analysis toluene and xylene are used as solvents.

III. In azeotropic method of analysis toluene, xylene, and water are used as solvents.

a)

I only

b)

I and II only

c)

I, II, and III

d)

None of the statement is correct

64.

Which of the following statement/s is/are correct?

I. Method I of water content determination in USP 27 is the azeotropic toluene distillation method.

II. Method II of water content determination in USP 27 is the titrimetric method.

III. Method III of water content determination in USP 27 is the gravimetric method.

IV. Method IV of water content determination in USP 27 is the Karl Fischer method

a)

I only

b)

II only

c)

III only

d)

IV only

65.

Primary standard used to standardize Karl Fischer reagent is:

a)

Anhydrous sodium carbonated

b)

Sodium tartrate

c)

Potassium hydrogen phthalate

d)

Sodium oxalate

66.

Negligible is defined as a quantity not exceeding:

a)

0.3 mg

b)

0.4 mg

c)

0.5 mg

d)

0.6 mg

67.

Ways to separate constituent in gravimetric analysis is/are

a)

A.

Neutralization

b)

B.

Physical means

c)

C.

Chemical means

d)

B and C

68.

The laws and theories of chemistry involved in the chemical reaction in gravimetric analysis are:

a)

Reversible reaction

b)

Solubility product principle

c)

Common-ion effect

d)

All of the choices

69.

If a 0.47 g sample of Potassium iodide yielded 0.7564 g of Silver iodide precipitate by gravimetric assay, compute for the % purity of the Potassium iodide. MW KI = 165.90; MW AgI = 234.76.

a)

83.7%

b)

93.7%

c)

103.7%

d)

113.7%

70.

To determine the total ash, the sample is incinerated at a temperature of 675 ±25 ⁰C. This temperature is represented by:

a)

Very dull red heat

b)

Dull red heat

c)

White red heat

d)

Bright red heat

71.

Which of the following chemicals is not included in preparing the Karl Fischer reagent?

a)

Pyridine

b)

Acetone

c)

Sulfur dioxide

d)

Iodine

72.

The type of ash where sulfuric acid is used to whiten the ash is:

a)

Acid insoluble ash

b)

Sulfated ash

c)

Loss on ignition

d)

ROI

73.

Karl Fischer method of determining moisture is also called:

a)

Toluene

b)

Dew point

c)

Titrimetric

d)

Azeotropic

74.

The temperature in ⁰C of ignition described as dull red heat is:

a)

500 – 1000

b)

550 – 700

c)

500 – 750

d)

300 – 450

75.

The acid-insoluble residue derived from the soil adhering to the drug is:

a)

Crude oil

b)

Cellulose

c)

Silica

d)

Inorganic matter

76.

A place to perform test with obnoxious, suffocating fumes is

a)

Laminar flow hood

b)

HEPA filter

c)

Fume hood

d)

A and B

77.

It is use in the ignition of most drugs and precipitates:

a)

Plain crucible

b)

Evaporating dish

c)

Goch crucible

d)

Watch glass

78.

Calculate the water content of Streptomycin powder using 3.50 g sample. The water equivalent factor, F, of the KF reagent was 4.6 and the volume consumed was 9.2 mL. The % water content is:

a)

1.20

b)

1.21

c)

12.10

d)

1.10

79.

Calculate the water equivalence (F) of Karl Fischer reagent if a 250 mg sample of Sodium tartarate dehydrate required 18.5 mL of Karl Fischer reagent.

a)

1.28 mg/mL

b)

1.35 mg/mL

c)

2.12 mg/mL

d)

2.30 mg/mL

80.

Each mL of the Karl Fischer reagent is equivalent to how much mg of water?

a)

2

b)

3

c)

4

d)

5

81.

Karl Fischer electrometric titration method is specific only for the analysis of:

a)

Food

b)

Water

c)

Gas

d)

Air

82.

Hexane is the best solvent in extracting:

a)

Resins

b)

Fats

c)

Volatile oil

d)

Acid

83.

The crude fiber of a drug usually consists of:

a)

Cellulose

b)

Cholesterol

c)

Phytosterol

d)

All of the choices

84.

The unsoponifiable matter present in vegetable oils and fats is:

a)

Cholesterol

b)

Cellulose

c)

Phytosterol

d)

Lard

85.

A one percent (1%) solid in liquid solution is officially (USP) understood as:

a)

1 g in 100 mL

b)

100 mg in 1 mL

c)

10 g in 100 mL

d)

10 g in 1 L

86.

The soluble constituent of a crude drug in a certain solvent is called:

a)

Extractive

b)

Ash

c)

Crude fiber

d)

Unsaponifiable matter

87.

To separate immiscible solvent effectively, it is necessary to use:

a)

Graduated pipet

b)

Separatory funnel

c)

Filter funnel

d)

Xylene tube

88.

Which of the following statement/s is/are correct?

I. Iodine value is a quantitative measure of the amount of unsaturated fatty acid in fats.

II. Method I of determining iodine value is also known as Hanus method.

III. Wij’s method is also a method determining iodine value.

IV. Hübl’s method is official method of determining iodine value.

a)

I only

b)

I and II

c)

I, II, & III

d)

All of the statements are correct

89.

Koettsdorfer number is also known as

a)

Acid value

b)

Saponification value

c)

Ester value

d)

Iodine value

90.

Method II of determining Iodine value is also known as:

a)

Hübl method

b)

Wij’s method

c)

Hanus method

d)

All of the choices

91.

When the alcoholic KOH is used to neutralize the acid and saponify the ester of 1 gram of the oil or fat, the constant determined is:

a)

Acid value

b)

Ester value

c)

Hydroxyl value

d)

Saponification value

92.

The iodine value of an oil is a quantitative measure of:

a)

Phenol content

b)

Saturated fatty acid

c)

Unsaturated fatty acid

d)

Unsaponifiable matter

93.

The ester value determination of substances is applicable to the following, except

a)

Fats

b)

Volatile oils

c)

Alcohols

d)

Fatty oils

94.

The number of mg of KOH required to saponify the esters in fat or oil is:

a)

Saponification value

b)

Ester value

c)

Acid value

d)

Iodine value

95.

The ester value determination of substance is applicable to fats, oil and other, similar substances, whereas unsaponifiable matter is applicable fats and oil that are not saponified by:

a)

Water

b)

Alcohol

c)

Alkali hydroxide

d)

Acetone

96.

If 10 g of olive oil required 20 mL of 0.0211 N NaOH in the titration of the free fatty acids. What is the acid number of the oil?

a)

2.9

b)

2.4

c)

11.50

d)

115

97.

Determine the Iodine value of an unknown sample of oil weighing 0.21 g if 26 mL and 12 mL of 0.1100 N of Sodium thiosulfate are required for the blank and residual titration respectively.

a)

90

b)

93

c)

108

d)

200

98.

If a sample of white wax is found to have an ester value of 65.7 and a saponification value of 74.2, what is the acid value of the sample?

a)

8.5

b)

86.5

c)

186.5

d)

56.5

99.

The oil from peppermint spirit can be determined by using

a)

Cassia flask

b)

Babcock bottle

c)

Pycnometer

d)

Titration

QC (PQ) 100 - 200

Total questions: 99

Worksheet time: 50mins

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