[QUALITY CONTROL] PACOP PINK

Other name of Ferric ammonium sulfate

a. Ferric alum

b. Fe NH4 (SO4)2

c. Fe (NH4)2(SO4)2

d. A and B

e. A and C

D

The following is/are example/s of metal-ion indicators.

I. Murexide

II. Calmagite

III. Pyrocathecol violet

IV. Ferric alum

a. I only

b. I and II only

c. I, II, and III

d. I, II, III and IV

C

Assay of diluted HCl is expressed in:

a. % w/w

b. % w/v

c. Both a and b

d. None of the choices

B

Standard solution in precipitation method od analysis

a. Disodium edetate

b. Silver nitrate

c. Sodium Methoxide

d. Perchloric acid

B

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

A

Argentometric titration is titration with ______ ion.

a. Magnesium

b. Sodium

c. Silver

d. Potassium

C

Fajans titration uses ____ indicator.

a. Acid-base

b. Adsorption

c. Metal-ion

d. None of the choices

B

Reasons why residual titration are performed.

a. Reaction proceeds slowly

b. Poor solubility of the sample

c. Sample does not give sharp end point

d. All of the choices

D

Solutions containing all the reagents and solvents used in the analysis, but no

deliberately added analyte.

a. Blank solution

b. Solution with sample

c. Standard solution

d. Test solution

A

Describes how close a measured value is to the true value.

a. Accuracy

b. Precision

c. Range

d. Standard deviation

A

Primary standard in the standardization of perchloric acid

a. Potassium hydrogen phthalate

b. Calcium carbonate

c. Benzoic acid

d. Sodium carbonate

A

Primary standard in the standardization of sodium methoxide.

a. Benzoic acid

b. Sodium bicarbonate

c. Sodium carbonate

d. Potassium hydrogen phthalate

A

The term dried to constant weight means that two consecutive weighing do not differ by

more than:

a. 0.0002 g

b. 0.2 mg

c. 0.5 mg/g

d. All of the choices

e. C only

D

Other name of systematic error

a. Determinate

b. Indeterminate

c. Random

d. Both b and c

A

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

a. Silver nitrate

b. Ammonium thiocyanate

c. Edetate disodium

d. All of the choices

B

The end point of using number ferric ammonium sulfate is:

a. White precipitate

b. Red-brown color

c. Pink color

d. Blue color

B

Limit moisture in nonaqueous titrimetric analysis is less than:

a. 0.5 %

b. 0.05 %

c. 0.2 %

d. 0.02 %

B

Complete reaction: H2C4H4O6 + NaOH -

a. Na2C4H4O6

b. H2O

c. Both a and c

d. None of the choices

C

A ligand that binds to a metal ion through only one atom.

a. Monodentate

b. Bidentate

c. Tridentate

d. Tetradentate

A

Which of the following is added to maintain the pH of sodium thiosulfate in optimum

range for the stability of the solution?

a. Sodium bicarbonate

b. Chloroform

c. Thymol

d. Sodium carbonate

D

Standard solution in non-aqueous titrimetric analysis-acidimetry

a. perchloric acid

b. hydrogen bromide

c. both a and b

d. none of the choices

C

Standards solutions are also known as:

a. test solutions

b. volumetric solutions

c. saturated solution

d. none of the choices

B

If starch 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

C

Types of chemical reaction used in the volumetric analysis

a. redox

b. neutralization

c. diazotization

d. all of the choices

e. a and b only

D

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

A

Other name of ferrous phenanthroline.

a. eosin Y

b. crystal violet

c. ferroin

d. ferric alum

C

Color of the complex resulting from reaction with ferrous phenanthroline:

a. blue

b. red

c. pink

d. violet

B

Primary standard in the standardization of ceric sulfate solution

a. potassium hydrogen phthalate

b. calciuim carbonate

c. sodium bicarbonate

d. arsenic trioxide

D

In the standardization of iodine solution, why is there a need to boil the solution of

arsenic trioxide?

a. it increases the solubility

b. it makes the solution stable

c. both a and c

d. none of the choices

A

Indicator in iodometric method of analysis.

a. KMnO4

b. Methyl red TS

c. Methyl orange TS

d. Starch TS

D

A molecule which provides groups of attachment to metal ions.

a. Ligand

b. Chelate

c. Both a and b

d. None of the choices

A

HCl + Calcium carbonate will react to form a primary product known as:

a. Carbonic acid

b. Calcium hydroxide

c. Both a and c

d. None of the choices

D

The reaction between HCl and calcium carbonate can be seen in the standardization of:

a. Silver nitrate

b. Ammonium thiocyanate

c. Edetate disodium

d. Sulfuric acid

C

A substance which gains electrons in a redox reaction.

a. Oxidizing agent

b. Reducing agent

c. Both a and c

d. None of the choices

A

The equilibrium constant for the reaction of the metal ion with a ligand is called _____.

a. Formation constant

b. Solubility product constant

c. Solubility constant

d. None of the choices

A

NaCl ______ the stability of EDTA complex.

a. Increases

b. Decreases

c. No effect

d. None of the choices

B

Organic solvents _______ the stability of EDTA complex.

a. Increases

b. Decreases

c. No effect

d. None of the choices

A

Indicator in Redox Titration using KMnO4

a. Starch TS

b. KMnO4

c. Methyl red TS

d. Methyl orange

B

Developed in 1883, this method of analysis remains as one of the accurate and widely

used method for determining nitrogen in substance.

a. Non-aqueous titrimetry

b. Precipitation

c. Redox itration

d. Kjeldahl method

D

Most suitable indicator to use in titration of organic acids

a. Methyl red TS

b. Methyl orange TS

c. Phenolphthalein

d. All of the choices

C

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

D

Indicator/s used in nonaqueous titrimetry

I. Nile blue

II. Crystal violet

III. Malachite green

IV. Phenolphthalein

a. I only

b. I and II only

c. I, II, and III only

d. I, II, III and IV

C

Standard solutions in nonaqueous alkalimetry.

I. Lithium methoxide

II. Perchloric acid

III. Hydrogen bromide

IV. Sodium hydroxide

a. I only

b. I and II only

c. I, II, and III only

d. I, II, III and IV

A

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 pH of the solution

C

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

I. The utility of starch as indicator is reduced in the presence of organic solvent.

II. The utility of starch as indicator is reduced in the presence of electrolytes.

III. The utility of starch as indicator is reduced at temperature above 25 °C

IV. The utility of starch as indicator is reduced at temperature of 25°C.

a. I only

b. I and II only

c. I, II, and III

d. I, II, III and IV

C

When a weak base is to be titrated with weak acid, the indicator used is:

a. Phenolphthalein

b. Methyl orange

c. Methyl red

d. No indicator is suggested

D

The formula to compute the equivalent weight of a reducing agent.

a. Molecular weight/ no. of electrons gain

b. Molecular weight/ no. of electrons loss

c. Both a and b

d. None of the choices

B

The used of sodium bicarbonate in the standardization of iodine solution ______.

a. Increase the solubility

b. as buffer

c. As preservative

d. To prevent bacterial growth

B

Method/s determining the total nitrogen in a sample

a. Macromethod

b. Semimicro method

c. Both a and c

d. None of the choices

C

To keep samples moisture free, the appropriate apparatus to use is:

a. Desiccator

b. Separatory funnel

c. Furnace

d. Incubator

A

The following is/are true about EDTA:

I. EDTA forms strong 1:1 complexes with most metal ions.

II. It prevents metal-catalyzed oxidation of food.

III. It is a pentadentate molecule

IV. It contains 3 oxygen and 2 hydrogen atoms that are capable of entering

complexation reaction with metal ion.

a. I only

b. I and II

c. II and III

d. III and IV

B

Sulfamic acid (H3NSO3) is a primary standard that can be used to standardized sodium

hydroxide. What is the molarity if 33.26 mL reacts with 0.3337 g sulfamic acid. MW=97

a. 0.304

b. 0.1004

c. 0.1005

d. 0.403

B

A 0.2185 g sample of NaCl was assayed using Volhard method using 50 mL of 0.998N

silver nitrate and 11.9 mL of 0.1350N ammonium thiocyanate. Calculate the NaCl in the

sample. MW NaCl = 58.45

a. 42.6

b. 62.4

c. 90.5

d. 6.24

A

A 4.59 mL sample of HCl, specific gravity 1.3, required 50.5 mL of 0.9544N NaOH in a

titration. Calculate the % w/w HCl.

a. 29%

b. 1%

c. 92%

d. 69%

A

What is the titer value for 0.05 M calcium chloride with 2 moles of water? MW= 142.9

a. 3.57 mg

b. 7.15 mg

c. 73.5 mg

d. 53.7 mg

B

A 10 mL sample of sulfuric acid solution required 16.85 mL of NaOH solution in a

titration. Each mL of the NaOH solution was equivalent to 0.2477 g of potassium

hydrogen phthalate. Calculate the sulfuric acid content in %w/v. MW=98

a. 10%

b. 20%

c. 30%

d. 40%

A

Limestone consists mainly of the mineral calcite, CaCO3. The carbonate content of

0.5413 g of powdered limestone was measured by suspending the powder in water,

adding 10 mL of 1.392 M HCl and heating to dissolve the solid and expel CO2. The

excess acid required 39.96 mL of 0.1004 M NaOH for complete titration to a

phenolphthalein end point. Find the weight % of the calcite in the limestone. MW=100

a. 29%

b. 39%

c. 92%

d. 96%

C

The Kjeldahl procedure was used to analyzed 256µL of a solution containing 37.9 mg

protein/mL. The liberated ammonia was collected in 5 mL of 0.0336 M HCl, and the

remaining acid required 6.34 mL of 0.010 M NaOH for complete titration. What is the

weight % of nitrogen in the protein? MW= 14

a. 3.86

b. 15.1

c. 51.5

d. 5.65

B

How many grams of Cupric (II) Sulfate pentahydrate should be dissolves in a volume of

500 ml to make 8 X 10

-3

M solution?

MW= 249.54

a. 0.998

b. 9.98

c. 99.8

d. 109.1

A

The molarity of concentrated HCl purchased in the laboratory is approximately 12.1 M.

How many mL of this reagent should be diluted to 2 L to make 0.1 M?

a. 1.65

b. 6.53

c. 16.53

d. 165.3

C

A solution with a final volume of 500 mL was prepared by dissolving 25 mL of methanol

(density= 0.7914 g/mL) in chloroform. Calculate the molarity of methanol in the solution.

MW= 32.

a. 0.12

b. 1.24

c. 12.4

d. 124

B

The above solution (question no.61) has a density of 1.454 g/mL. Find the molality of

methanol.

a. 0.87

b. 0.77

c. 8.7

d. 7.7

A

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

C

Process of measuring the actual quantity mass, volume, force, etc. that correspond to an

indicated quantity on the scale of an instrument.

a. Weighing

b. Calibration

c. Both a and c

d. None of the choices

B

Also known as Eosin Y.

a. Dichlorofluorescein

b. Tetrabromophenolpthalein

c. Tetrabromofluorescein

d. Xylenol orange

C

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

a. Amylopectin

b. Amylose

c. Glucose

d. Sucrose

B

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

a. Iodometry

b. Iodimetry

c. Cerimetry

d. Permanganometry

B

The 0.1 N iodine solution is standardized using

a. Potassium permanganate

b. Potassium hydrogen phthalate

c. Arsenic trioxide

d. Sodium carbonate

C

Iodimetry is an indirect analysis of:

a. Oxidizing agent

b. Reducing agent

c. Acid

d. Base

A

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

A

What weight of arsenic trioxide (93.73%) would be used as a sample so that 26.6 mL of

0.1120 N iodine would be needed to titrate it? MW = 197.46

a. 0.14896 g

b. 0.4896 g

c. 0.1111 g

d. 0.9145 g

A

The type of alkaliodal assay where the total alkaloid is determined.

a. Ultimate

b. Specific

c. Proximate

d. Extraction

C

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 I of water content determination in USP 27 is the Karl Fischer

method.

a. I only

b. II only

c. III only

d. IV only

C

Residue on ignition is also called:

a. Loss on ignition

b. Loss on drying

c. Acid-soluble ash

d. Sulfated ash

D

Primary standard used to standardized Karl Fischer reagent is:

a. Anhydrous sodium carbonated

b. Sodium tartrate

c. Potassium hydrogen phthalate

d. Sodium oxalate

B

Method 1 for determining alcohol-soluble extractives is also known as:

a. Hot extraction method

b. Cold extraction method

c. Hot compressed method

d. Cold compressed method

A

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 of determining iodine value.

IV. Hubl's method is official method of determining iodine value.

a. I only

b. I and II

c. I, II and III

d. All of the statements are correct

C

Koettsdorfer number is also known as:

a. Acid value

b. Saponification value

c. Ester value

d. Iodine value

B

The gram-equivalent weight of sodium oxalate (MW = 134 g/mole) is:

a. 67

b. 0.067

c. 0.114

d. 0.026

A

Orthophenanthroline TS is used as indicator in

a. Permanganometry

b. Ceric sulfate titration

c. iodometry

d. Iodimetry

B

A sample of Chlorpheniramine maleate weighing 0.502 g was assayed by nonaqueous

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

A

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

C

If 10g 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

B

Does the acid value of the above conform with the official requirement? (In 10g of olive

oil, the specification is <5mL of 0.1N NaOH.)

a. Yes

b. No

c. Uncertain

d. None of the above

A

In phenol contain determination of a volatile oil, the layer in the graduated neck of the

cassia flask read 2.3 mL obtained from a sample of 10 mL of the oil after treatment with

KOH solution. The % phenol is:

a. 73

b. 69

c. 7.3

d. 77

D

A 4.0570 g sample of chlorinated lime was mixed with enough water to make 1000mL. 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%

D

Military standard table is also known as:

a. Government sampling plan

b. MIL-STD-105D

c. ABC-STD 105D

d. All of the choices

D

The % hexane extractive obtained from 27.5820 g of crude drug yielding a residue of

0.9155g of extractive is:

a. 3.32%

b. 33.2%

c. 4.30%

d. 4.6%

A

Calculate the menthyl acetate content in % if 9.5 g sample of peppermint oil was

refluxed with 25 mL of 0.5N alcoholic KOH and required 22.5 ml of 0.4900N HCl for the

residual titration. The blank was run using the same volume of 0.5N alcoholic KOH and

required 26.0mL of 0.4900N HCl to bring about the end point. Each mL of 0.5N alcoholic

KOH consumed in the saponification is equivalent to 99.15 mg menthyl acetate.

a. 4.82%

b. 3.58%

c. 4.80%

d. 8.4%

B

Calculate the % alkaloid extracted from a bark of plant using 1.0215g of the crude drug;

the volume of 0.0245N sulfuric acid added to the extract was 25.7 mL, the excess was

back titrated by 21.75 mL of 0.0225N sodium hydroxide solution. Each ml of 0.02N

sulfuric acid is equivalent to 3.8858 mg of the alkaloid.

a. 2.67%

b. 6.72%

c. 7.62%

d. 6.5%

A

Determine the iodine value of an unknown sample of oil weighing 0.21g if 26mL 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

A

Identify the sample of the above question with USP requirement of:

a. Persic oil 90-108

b. Corn oil 102-128

c. Olive oil 79-88

d. None of the choices

A

Find the acid value of oleic acid sample weighing 2g which require 45mL 0f 0.1102

NaOH to bring about the end point.

a. 196

b. 200

c. 345

d. 139

D

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

A

A 50 mL aliquot of solution containing .450g of magnesium sulfate in 0.5L 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. 9943 mg

A

The following is/are true about auxillary complexing agent.

I. Eriochrome black is an example of an auxillary complexing agent

II. Auxillary complexing agents are also ligands

III. Auxillary complexIng agents binds the metal strong enough to prevent the

hydroxide from precipitating, but weakly enough to give up the metal ion when

EDTA is added.

IV. It is used to permit many metals to be titrated in alkaline solution with EDTA.

a. I only

b. II and III

c. II, III, and IV

d. III, and IV

e. I, II, III and IV

C

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 EDTA indicator.

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

e. I, II, III and IV

D

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

I. A redox indicator is a compound that changes color when it goes from oxidized to

reduced state

II. Starch is a redox indicator

III. Ferroin is a redox indicator

IV. The hydrolysis is product of starch is glucose which is a reducing agent

a. I only

b. I and II

c. III, I, II, and III

d. I, III, and IV

e. I, II, III, and IV

D

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

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. II and IV

e. I, II, III and IV

C

Which of the following statements is/are correct?

I. Potassium dichromate is an oxidizing agent

II. Potassium dichromate is used chiefly for the determination Fe+2

and indirectlysample that will oxidized Fe+2

to Fe+3

III. Potassium dichromate to chronous ion, gains 6 electrons

a. I only

b. II only

c. III only

d. I, II, and III

D