MINISTRY OF HEALTHCARE OF UKRAINE
PIROGOV VINNYTSYA NATIONAL MEDICAL UNIVERSITY
The Pharmaceutical Chemistry Department
Analytical chemistry
MODULE 2
Methodical guidelines
for self-preparatory work
of second-year students
Vinnytsya 2013
«Approved» by
Methodical council of
Pirogov National Medical University of Vtinnytsya
Minutes №2 from 20.11.2013 year
Approved
at the meeting of the
Pharmaceutical Chemistry
Department
Re- Approved
Minutes № 4 from 01.11.2013 year
Head of the Pharmaceutical
Chemistry Department
_______________________
PhD Assistant Professor Yuschenko T.I.
Minutes № 1 from 28.08.2014 year
Head of the Pharmaceutical
Chemistry Department
Re- Approved
________________________
Minutes № ___ from 20____ year
Head of the Pharmaceutical
Chemistry Department
_______________________
Authors
Teachers of Pirogov Vinnytsya National Medical University (the pharmaceutical chemistry
department): T.I. Yuschenko, A.E. Kosareva, L.V. Slobodyanyuk
Рецензенти:
- доцент кафедри хімії та хімічної технології Вінницького національного
технічного університету, к.х.н., М.В.Євсєєва
- доцент кафедри біологічної та загальної хімії Вінницького національного
медичного університету імені М.І. Пирогова, к.х.н. О.В.Смірнова
The Methodical guidelines created at the Pharmaceutical Chemistry Department of the
Pirogov Vinnytsya National Medical University.
The Methodical guidelines is made according to the requirements of the typical curriculum
in analytical chemistry for the students of pharmaceutical higher schools and pharmaceutical
departments of medical higher schools of the IIId – IVth accreditation levels (Specialization
"Pharmacy ", "Clinical Pharmacy"). The given guidelines are intended for self-preparation and
control of the mastering the level of knowledge of second-year students from module 2.
Introduction
The program of analytical chemistry is structured into 3 modules. It is consistent with the
teaching standarts, the principles of Bologna process and improves students performance.
Module 2 includes the study of theoretical foundations and mastering practical skills of chemical
methods of quantitative analysis. Control mastering of knowledge of the modules is carried out
after its the completion on the final lessons. These guidelines are intended for self-preparation of
students to the practical lessons and final control of knowledge from module 2 "Quantitative
Analysis". Test questions for the studens in – class and out – of class training are presented in the
guidelines, which help to check the degree of learning of the theoretical material. At the end of
the guidelines there is a list of recommended literature.
The Methodical guidelines is made according to the requirements of the typical curriculum
in analytical chemistry for the students of pharmaceutical higher schools and pharmaceutical
departments of medical higher schools of the IIId – IVth accreditation levels (Specialization
"Pharmacy ", "Clinical Pharmacy"). The given guidelines are intended for self-preparation and
control of the mastering the level of knowledge of second-year students from module 2.
The content of the test task
The answer and substantiation
1. Gravimetric analysis
1.1. To determine calcium mass concentration
in a medical preparation the gravimetric
precipitation method was applied. Ammonium
oxalate solution was used as a precipitator. The
gravimetric form in this case is:
A. Monohydrous calcium oxalate
B. Anhydrous calcium oxalate
C. Calcium carbonate
D. Calcium oxide
E. Calcium hydroxide
1.2. To determine Cu2+ mass concentration in a
medical
preparation
the
gravimetric
precipitation method was applied. What matter
can be used as a precipitator for this
determination:
A. NH4OH
B. NaOH
C. HCl
D. H2SO4
E. HNO3
1.3. Choose the precipitation form which will
coincide after a chemical formula with a
gravimetrical form:
A. BaSO4
B. CaC2O4
C. Fe(OH)3
D. Al(OH)3
E. Cr(OH)3
1.4. In In determining the moisture content of
pharmaceuticals, the drug was heated to convert
water into gas state. What method of analysis
has been applied?
A. Electrogravimetry
B. Indirect Volatilization gravimetry
C. Precipitation gravimetry
D. Particulate gravimetry
E. Precipitation titrimetry
1.5.
To
determine
aluminum
mass
concentration in a medical preparation the
gravimetric
precipitation method was applied. Ammonium
solution was used as a precipitator. The
gravimetric form in this case is:
A. Aluminum carbonate
B. Ammonium carbonate
C. Aluminum oxide
D. Ammonium hydroxide
E. Aluminum hydroxide
1.6. Which material should be selected as the
precipitable form by gravimetric determination
of sulphate ions:
А. PbSO4, KSP = 1,6∙10 -8
B. CaSO4 , KSP = 2,5∙10-7
C. BaSO4, KSP = 1,1∙10-10
D. SrSO4, KSP = 3,2∙10-7
E. AgSO4, KSP = 1,6∙10-5
1.7. To determine sulfate ions mass
concentration in a medical preparation the
gravimetric precipitation method was applied.
Barium chloride solution was used as a
precipitator. Choose a solution for washing the
precipitate of barium sulfate:
A. Distilled water
B. Diluted sulfuric acid solution
C. Sodium sulfate solution
D. Barium chloride
E. Diluted nitric acid solution
1.8. To determine Cr3+ mass concentration in a
medical
preparation
the
gravimetric
precipitation method was applied. What matter
can be used as a precipitator for this
determination:
A. NaOH
B. H2O2
C. NH4OH
D. H2SO4
E. HCl
1.9. During gravimetric determination of mass
fraction of sulfate ions in the magnesium
sulphate preparation precipitation is performed
by means of barium chloride solution.
Precipitated barium sulfate should be rinsed
with:
A. Diluted solution of sulfate acid
B. Distilled water
C. Solution of barium chloride
D. Solution of sodium sulfate
E. Solution of hydrochloride acid
1.10. Gravimetric determination of carbonate
ions in the contaminated sample CaCO3
conducted by:
A. Electrogravimetry
B. Direct volatilization gravimetry
C. Precipitation gravimetry
D. Particulate gravimetry
E. Precipitation titrimetry
1.11. Specify the balance for the mass exact
measuring:
A. Hand balance
B. Technochemical balance
C. Technical balance
D. Analytical balance
E. Torsion balance
2. Titrimetric analysis
2.1. Select chemical vessels to measure the
exact amount of titrant in titrimetric methods of
analysis:
A. Measuring cylinder
B. Volumetric flask
C. Burette
D. Conical flask
E. Pipette
2.2. Select the substance from which you can
prepare a primary standard solution:
A. NaOH
B. K2Cr2O7
C. HCl
D. KMnO4
E. CH3COOH
2.3. Specify the titration method, in which a
standardized titrant solution is gradually added
to the solution under study until a titration
endpoint is reached:
A. Direct titration
B. Back titration
C. Indirect titration
D. Substitution titration
E. Residue titration
3. Acid-base titration
3.1. What methods of acid-base titration can be
used to determine the amount of acetic acid in
the solution:
A. Argentometry
B. Acidimetry
C. Alkalimetry
D. Mercurometry
E. Mercurimetry
3.2. A chemist in analytical laboratory needs to
standardize solution of sodium hydroxide. What
primary standard solution can be applied for
this purpose?
A. Chloride acid
B. Nitric acid
C. Oxalic acid
D. Acetic acid
E. Sodium tetraborate
3.3. Ammonia concentration in solution was
determined by acid-base titration. Solution of
sodium hydroxide was used as titrant. What
standard solution can be used to standardize a
solution of sodium hydroxide:
A. Sodium tetraborate
B. Acetic acid
C. Silver nitrate
D. Chloride acid
E. Potassium carbonate
3.4. What pH indicator is used to determine the
endpoint for the titration of acetic acid solution
by NaOH solution:
A. Titrated without indicator
B. Phenolphthalein
C. Methyl orange
D. Both indicators
E. Eosin
3.5. pH indicator is used to determine the
endpoint in the acid-base titration. One of the
methods for selecting the indicator - on the
titration curve. Titration curve of the acid-base
titration - a graphical dependence of:
A. pH on the volume of analyzed solution
B. Concentration of analyzed solution on the
volume of added titrant
C. pH on the volume of added titrant
D. Concentration of analyzed solution on the
concentration of titrant
E. Concentration of titrant on the volume of
analyzed solution
3.6. Which of the laws is the theoretical basis of
titrimetric methods of analysis:
A. Law of equivalent proportions
B. Law of definite composition
C. Law of conservation of mass
D. Law of multiple proportions
E. Nernst law
3.7. Select the secondary standard for
standardization 0.1M potassium hydroxide
solution:
A. Chloride acid
B. Sodium chloride
C. Oxalic acid
D. Sodium hydroxide
E. Sodium tetraborate
3.8. What is the result of the titration is
necessary to calculate the concentration of the
analyzed solution in titrimetric methods of
analysis:
A. Concentration of the titrant, which reacted
with analyzed substance
B. The volume of titrant, which is expended for
the reaction with the analyzed substance
C. The mass of the reagent, which reacted with
the analyzed substance
D. The volume of analyzed solution, which
reacted with titrant
E. The mass of analyzed solution
3.9. Choose a couple of standard materials
which can be used for standardization acid
solutions:
A. CaCO3, Na2B4O7 .10 H2O
B. Na2CO3, NaCl
C. H2C2O4 .2 H2O, Na2B4O7 .10 H2O
D. Na2CO3, Na2B4O7 .10 H2O
E. CaCO3, Na2CO3
3.10. Select the definition for the equivalence
point in acid-base titration: Equivalence point is
the point at which:
A. You observe change of solution color
B. Volume of the added titrant is equal to the
volume of analyzed solution
C. Number of titrant is strictly equivalent to the
amount of titrated substance
D. The time of the titration when the pH = 7
E. Occurrence of sediment
3.11. A chemist in an analytical laboratory
needs to standardize a hydrochloric acid
solution. What primary standard solution can be
used for this purpose?
A. Sodium hydroxide
B. Oxalic acid
C. Sodium tetraborate
D. Acetic acid
E. Sodium chloride
3.12. The drug contains sodium bicarbonate and
sodium chloride. Suggest a method for
quantitative
determination
of
sodium
bicarbonate:
A. Argentometry
B. Acid-base titration
C. Complexometric titration
D. Oxidation-Reduction titration
E. Mercurimetry
3.13. Specify standard substances used for
standardization of titrant solutions (NaOH,
KOH) in the alkalimetric method:
A. Oxalic and succinic acids
B. Acetic and succinic acids
C. Formic and acetic acids
D. Sulphanilic and oxalic acids
E. Sulphanilic and salicylic acids
3.14. What method of titrimetric analysis can be
applied for the quantitative determination of
sulphuric acid by means of the potassium
hydroxide solution?
A. Alkalimetry
B. Acidimetry
C. Oxidation-reduction
D. Precipitation
E. Complexation
3.15. Choose a pair of titrants for the qualitative
determination of ammonia in a solution by the
method of back titration:
A. HCl, NaOH
B. HCl, H2SO4
C. KOH, NaOH
D. NaOH, KCl
E. H2SO4, K2SO4
3.16. Specify the equivalence factor of Na2СО3
in quantitative determination according to the
reaction Na2СО3 + HCl = NaCl+NaHCO 3:
А. f=2
B. f=1/2
C. f=1/4
D. f=1
E. f=1/3
3.17. Specify the equivalence factor of H2SО4
in quantitative determination according to the
reaction H2SО4 + 2NaOH = Na2SО4+2H2O:
А. f=2
B. f=1/2
C. f=1/4
D. f=1
E. f=1/3
3.18. Choose a pair of titrants for the qualitative
determination of ammonia in a solution by the
method of back titration:
A. HCl, NaOH
B. HCl, H2SO4
C. KOH, NaOH
D. NaOH, KCl
E.H2SO4, K2SO4
4. Redox titration
4.1. The endpoint in the analysis of oxidizing
and reducing agents by methods of the redox
titration is determined:
A.Without indicator
B. Using redox indicators
C. With specific indicator
D. By instrumental methods
E. By all these methods
4.2. Redox indicators are used to determine the
endpoint in redox titration methods. The color
of the redox indicator depends on:
A. The degree of ionization of the substance
B. Concentration of hydrogen ions
C. Ionic strength of solution
D. Redox potential of the system
E. Concentration of hydroxide ions
4.3. Titration curve of the redox titration - a
graphical dependence of:
A. pH on the volume of analyzed solution
B. Concentration of analyzed solution on the
volume of added titrant
C. pH on the volume of added titrant
D. Concentration of analyzed solution on the
concentration of titrant
E. Redox potential of the system on the volume
of added titrant
4.4. 0,1M solution of potassium permanganate
is used as a titrant in permanganatometry. The
solution is prepared like the secondary standard
solution and standardized according to:
A. Sodium chloride
B. Potassium dichromate
C. Sodium oxalate
D. Sodium carbonate
E. Calcium oxide
4.5. Which indicatorless method enables
quantitative determination of iron (II) content?
A. Permanganatometry
B. Chelatometry
C. Argentometry
D. Iodometry
E. Nitritometry
4.6. Choose a pair of substances that can be
used for standardization of 0,1 M solution of
KMnO4:
A. Na2C2O4, CH3COOH
B. K2CO3, CH3COOH
C. CH3COOK, H2C2O4
D. KHC2O4, HCOOH
E. Na2C2O4, H2C2O4
4.7. Permanganatometry can be can be used for
determination of H2O2 in high-acidity medium.
What acid can be used for production of such
medium?
A. HCl
B. H2SO4
C. HNO3
D. CH3COOH
E. H3PO4
4.8. What substance can be quantitatively
determined by method of acid-base titration and
oxidation-reduction titration?
A. Sodium hydroxide
B. Acetic acid
C. Sodium sulphate
D. Oxalate acid
E. Ammonium chloride
4.9. In permanganatometric titration, a solution
containing iron (II) ion is titrated with a
solution
of
potassium
permanganate.
Equivalence factor
of the potassium
permanganate in the reaction equal to:
A. 1/3
B. 1
C. 1/2
D. 1/5
E. 1/4
4.10. 0,1M solution of potassium permanganate
is used as a titrant in permanganatometry for
determination of reducing agents. The endpoint
of permanganatometric titration is determined:
A. Without indicator
B. Using redox indicators
C. With specific indicator
D. By instrumental methods
E. With external indicator
4.11. Select indicatorless method for
quantitative determination of reducing agents
(for example, sodium nitrite) content?
A. Cerimetry
B. Dichromatometry
C. Permanganatometry
D. Iodometry
E. Nitritometry
4.12. In permanganatometric titration, a
solution containing iron (II) ion is titrated with
a solution of potassium permanganate.
Equivalence factor of the iron (II) in the
reaction equal to:
A. 1/3
B. 1
C. 1/2
D. 1/5
E. 1/6
4.13. Reinhardt-Zimmerman solution (H2SO4
con. + H3PO4 + MnSO4) is used for iron in
permanganatometry for iron (II) determination
phosphoric acid should be added to:
A. Create a highly acidic environment
B. As an indicator
C. For the masking of Fe(III) ions
D. Create an alkaline environment
E. As a catalyst
4.14. Reinhardt-Zimmerman solution (H2SO4
con. + H3PO4 + MnSO4) is used for iron in
permanganatometry for iron (II) determination
manganese sulfate is added to:
A. Create a highly acidic environment
B. As an indicator
C. For the masking of Fe(III) ions
D. Create an alkaline environment
E. As a catalyst
Iodometry
4.15. Concentration of potassium dichromate in
a solution was determined by means of
iodometry. Name a titrant of iodometric method
for determination of strong oxidizer:
A. Potassium iodide
B. Sodium hydroxide
C. Sodium thiosulfate
D. Potassium permanganate
E. Potassium bromate
4.16. Concentration of potassium dichromate in
a solution was determined by means of
iodometry. Name a titrant of iodometric method
for determination of strong oxidizer:
A. Potassium iodide
B. Sodium hydroxide
C. Sodium thiosulfate
D. Potassium permanganate
E. Potassium bromate
4.17. Iodometric determination of formaldehyde
in formaline can be done by the back titration.
Iodine surplus is titrated with the standard
solution of:
A. Sodium thiosulphate
B. Sodium nitrate
C. Sodium sulphate
D. Sodium carbonate
E. Sodium phosphate
4.18. Name the type of reaction that takes place
during detection of ascorbic acid in a
preparation by iodometric method:
A. Neutralization
B. Acylation
C. Oxidation-reduction
D. Precipitation
E. Complexing
4.19. Specify the standardized solutions that can
be used for direct and back titration of reducing
agents in the iodimetric method:
A. K2Cr2O7, I2
B. K2Cr2O7, Na2S2O3
C. I2, KI
D. KMnO4, KI
E. I2, Na2S2O3
4.20. Name a standard solution of iodimetric
determination of reducing agents (direct
titration)?
A. Solution of KI
B. Solution of KMnO4
C. Solution of Na2S2O3
D. Solution of K2Cr2O7
E. Solution of I2
4.21. Quantitative determination of iodide can
be done by method of:
A. Chelatometry
B. Acid-base titration
C. Oxidation-reduction titration
D. Spectrophotometry
E. Precipitating titration
4.22. Iodometric determination of formaldehyde
in formaline can be done by the back titration.
Iodine surplus is titrated with the standard
solution of:
A. Sodium thiosulphate
B. Sodium nitrate
C. Sodium sulphate
D. Sodium carbonate
E. Sodium phosphate
4.23. Standardized sodium thiosulfate solutions
are used as titrant in iodometric titration.
Equivalence factor of the sodium thiosulfate
(Na2S2O3) equal to:
A. 1/3
B. 1
C. 1/2
D. 1/5
E. 1/4
4.24. Choose a pair: standardized solution and
additional reagent, that can be used for indirect
titration of oxidizing agents in the iodometric
method:
A. K2Cr2O7, I2
B. Na2S2O3, KI
C. I2, KI
D. KMnO4, KI
E. I2, Na2S2O3
4.25. In which method of redox titration starch
(specific indicator) is used to detect the end
point:
А. Cerimetry
B. Bromatometry
C. Iodometry
D. Nitritometry
E. Permanganatometry
4.26. Potassium dichromate can be used for
standardization of sodium thiosulfate solution.
What titration method is used in this case:
A.Back titration in an alkaline environment
B.Direct titration in strongly acidic medium
C.Back
titration
in
acidic
medium
D.Indirect titration in acidic medium
E. Direct titration in an alkaline environment
Nitritometry
4.27. Specify the relevant indicators for fixation
of the titration endpoint when using
nitritometric method:
A. Methylene orange
B. Methylene blue
C. Tropeolin 00 + methylene blue
D. Starch solution
E. Diphenylamine
4.28. Nitritometric determination of compounds
containing primary aromatic amino group can
be carried out under the following conditions:
A. With observation of all the mentioned
conditions
B. At a temperature up to 10oC
C. With adding of the crystalline KBr (catalyst)
D. Chloric acid excess
E. Slow titration
4.29. Nitritometric determination of primary
aromatic amines in acidic medium results in
generation of the following reaction product:
A. Azide
B. Nitrosoamine
C. Nitrose arylenamine
D. Nitrose antipyrine
E. Diazonium salt
4.30. Name the method of redox titration in
which both external and internal indicators are
used to determine the end point:
А. Cerimetry
B. Bromometry
C. Chelatometry
D. Nitritometry
E. Permanganatometry
4.31. Streptocide can be quantitatively
determined
by
nitritometric
titration.
Equivalence factor of the streptocide equal to:
A. 1/3
B. 1
C. 1/2
D. 1/5
E. 1/4
Bromatometry
4.32. It is required to determine the amount of
sodium salicylate in a solution. What titrimetric
method can be applied for the quantitative
determination of aromatic compounds?
A. Bromometry
B. Mercurimetry
C. Cerimetry
D. Argentometry
E. Chelatometry
4.33. Choose an appropriate indicator for
fixation of titration end point in method of
bromatometry:
A. Tropeolin 00
B. Phenolphthalein
C. Starch
D. Methyl blue
E. Methyl red
4.34. Select the method in which pH indicators
are used to determine the end point:
А. Cerimetry
B. Bromatometry
C. Iodometry
D. Nitritometry
E. Permanganatometry
4.35. What titrimetric method can be applied
for the quantitative determination of phenol
(carbolic acid)?
A. Nitritometry
B. Bromometry
C. Chelatometry
D. Argentometry
E. Cerimetry
4.36. Streptocide can be quantitatively
determined by bromatometric titration. What
standard solution is used as titrant?
A. Potassium permanganate solution
B. Potassium iodide solution
C. Potassium bromate solution
D. Sodium nitrite solution
E. Cerium (IV) sulphate solution
4.37. Streptocide can be quantitatively
determined
by bromatometric
titration.
Equivalence factor of the streptocide equal to:
A. 1/6
B. 1
C. 1/2
D. 1/5
E. 1/4
Dichromatometry
4.38. Choose a reduction-oxidation method for
the quantitative determination of iron (II) salts
in a solution that contains hydrochloric acid:
A. Dichromatometry
B. Iodometry
C. Permanganatometry
D. Nitritometry
E. Ascorbinometry
4.39. Content of potassium dichromate in a
solution was determined by iodometric method.
Name the titrant of iodometric method for
oxidant determination:
A. Potassium permanganate
B. Sodium hydroxide
C. Potassium iodide
D. Sodium thiosulfate
E Potassium bromate
4.40. Iron (II) ion was determined by
dichromatometric titration. Equivalence factor
of the potassium dichromate in the reaction
equal to:
A. 1/3
B. 1
C. 1/2
D. 1/6
E. 1/4
4.41
0,1M
solution
of
potassium
dichromatomate is used as a titrant in
dichromatometry for determination of reducing
agents. The endpoint of dichromatometric
titration is determined:
A. Without indicator
B. Using redox indicators
C. With specific indicator
D. By instrumental methods
E. With external indicator
Cerimetry
4.42. A chemist in an analytical laboratory
needs to standardize a cerium(IV) sulphate
solution by iodometric titration. What primary
standard solution can be used for this purpose?
A. Potassium permanganate
B. Sodium hydroxide
C. Potassium iodide
D. Sodium thiosulphate
E. Potassium bromate
4.43. Ascorbic acid was determined by
cerimetric titration. The endpoint was
determined by a color change of the solution
from red to blue. What indicator was used to
determine the endpoint?
A. Tropeolin 00
B. Phenolphthalein
C. Ferroin
D. Methyl red
E. Starch
4.44. 0,1 M solution of cerium(IV) sulphate is
used as a titrant in cerimetry for determination
of reducing agents, for example iron (II)
sulphate in drug. Equivalence factor of the
cerium(IV) sulphate in the reaction equal to:
A. 1/3
B. 1
C. 1/2
D. 1/6
E. 1/4
5. Precipitation titration
5.1. Thiocyanatometry is based upon using of
secondary standard solution of potassium
thiocyanate that should be standardized
according to the following standard solution of:
A. Silver nitrate
B. Hydrochloric acid
C. Sulfuric acid
D. Iron (II) sulfate
E. Copper (II) nitrate
5.2. Determination of sodium and potassium
chlorides in pharmaceuticals can be done by
means of:
A. Argentometry, Mohr method
B. Reduction-oxidation titration
C. Alkalimetry
D. Acidimetry
E. Chelatometry
5.3. What standard solution (titrant) is used in
Folgard's method of direct titration?
A. Ammonium thiocyanate
B.Sodium chloride
C. Silver nitrate
D. Potassium chromate
E. Potassium dichromate
5.4. A composition under examination contains
ions of Cl–, Br– and I– in equimolar quantities.
The sequence of precipitate formation in course
of argentometric titration will be determined by:
A. Solubility product of the corresponding
silver halogenides
B. Value of oxidation-reduction potentials
C. Way of titration - either back or direct
D. Value of corresponding ion mobility
E. Ionic strength of solution
5.5. What is the primary standard for
standardization of Hg2(NO3)2 solution?
A. Sodium chloride
B. Sodium bromide
C. Sosium sulphate
D. Sodium hydroxide
E. Sodium dichromate
5.6. Determination of sodium chloride by
Folgard's method involves the following
techniques:
A. Back titration, argentometry
B. Direct titration, argentometry
C. Substitute titration
D. Back titration, mercurimetry
E. Direct titration, mercurimetry
6. Complexometric titration
6.1. Calcium chloride quantitative content can
by measured by direct chelatometric titration
method. Choose an indicator for the titration
end point registering:
A. Methyl red
B. Starch
C. Eosin
D. Phenolphthalein
E. Eriochrome black T
6.2. Chlorides presence in drinking water can be
detected by mercurimetry method. One of the
following solutions is used as titrant:
A. Hg2(NO3)2
B. Hg(NO3)2
C. HgSO4
D. HgCl2
E. Hg2Cl2
6.3. Titrant of chelatometry method is trilon B
solution that forms complex compounds with
metal cations irrespective of their valence at a
ratio of:
A. 1  3
B. 1  2
C. 1  1
D. 2  1
E. 3  1
6.4. The drug contains calcium chloride.
Suggest a method for quantitative determination
of calcium:
A. Precipitation titration
B. Acid-base titration
C. Chelatometry titration
D. Oxidation-Reduction titration
E. Mercurimetry titration
6.5. A chemist in an analytical laboratory
needs to standardize an EDTA solution. What
primary standard solution can be used for this
purpose?
A. Sodium chloride
B. Zinc sulfate
C. Chlorohydrogen acid
D. Potassium sulfate
E. Mercury (II) nitrate
6.6. Mercurometry method is used to determine
the amount of halides in the solution. Select
indicator to determine the endpoint for the
mercurometric titration:
A. Eriochrome black T
B. Diphenylcarbazone
C. Methyl orange
D. Titrated without indicator
E. Phenolphthalein
6.7. Chelatometry method is used for
quantitative determination of:
A. Halides
B. Alkaline metals
C. Alkaline heavy metals
D. Alkaline earth and heavy metals
E. Acids and bases
6.8. Mercury (II) nitrate solution is used as
titrant to determine the amount of halides in the
solution. What the primary standard substance
can be used to standardize the mercury (II)
nitrate solution:
A. Chloride acid
B. Sodium sulfate
C. Sodium chloride
D. Zinc sulfate
E. Zinc chloride
6.9. Water Hardness can be determined by
complexometric titration. Select conditions of
determination:
A. Ammonium buffer solution, eriochrome
black T
B. Ammonium buffer solution,
diphenylcarbazone
C. Acetic buffer solution, eriochrome black T
D. Ammonium buffer solution, titrated without
indicator
E. Acetic buffer solution, diphenylcarbazone
6.10. In a complexometric titration, a solution
containing the free metal ion is titrated with a
solution of chelating agent until all of the metal
ions are completely complexed. Equivalence
factor of the metal in the complexometric
titration method always equal to:
A. 1/3
B. 1
C. 1/2
D. 2
E. 1/4
6.11. Mercurometry method is used to
determine the amount of halides in the solution.
What solution is used as titrant:
A. Mercury (II) nitrate
B. Mercury (I) nitrate
C. Mercury (II) chloride
D. Mercury (I) chloride
E. Mercury (II) sulfate
6.12. Magnesium sulfate solution titrated using
Eriochrome Black T to the end point. What
analytical effect is observed at the point?
A. Occurrence of sediment
B. Restores proper color of indicator
C. Colored solution becomes colorless
D. Dissolution of sediment
E. Colorless solution becomes colored
6.13. Mercurometry method is used for
quantitative determination of:
A. Heavy metals
B. Alkaline metals
C. Alkaline earth and heavy metals
D. Halides
E. Acids and bases
6.14. The drug contains aluminum nitrate.
Suggest a method for quantitative determination
of aluminum in the solution of the drug sample:
A. Precipitation titration
B. Acid-base titration
C. Chelatometry titration
D. Oxidation-Reduction titration
E. Mercurimetry titration
6.15. Quantitative determination of calcium
chloride is carried out by method of direct
chelatometric titration. Choose an indicator for
fixation of the titration endpoint:
A. Eriochrome black T
B. Phenolphthalein
C. Methyl red
D. Eosin
E. Starch
6.16. Determination of medications containing
cations of magnesium and calcium is done by
trilonometric titration. What type of chemical
reaction takes place in this case?
A. Complexation
B. Oxidation-reduction
C. Electrophylic substitution
D. Alkylation
E. Precipitation
6.17. You are given 0,05 M solution of versene
(chelating agent). What is standard substance
for standardization of this solution?
A. Metallic zinc
B. Sodium tetraborate
C. Sodium hydroxide
D. Oxalic acid
E. Potassium dichromate
THE KEYS TO THE TESTS
1. Gravimetric analysis
№ of the test
task
1.1
1.2
1.3
1.4
1.5
1.6
The correct
answer
D.
B.
A.
B.
C.
C.
№ of the test
task
1.7
1.8
1.9
1.10
1.11
The correct
answer
D.
C.
C.
B.
D.
2. Titrimetric analysis
№ of the test
task
2.1
2.2
2.3
The correct
answer
C.
B.
A.
The correct
answer
C.
C.
D.
D.
C.
A.
A.
B.
D.
№ of the test
task
3.10
3.11
3.12
3.13
3.14
3.15
3.16
3.17
3.18
3. Acid-base titration
№ of the test
task
3.1
3.2
3.3
3.4
3.5
3.6
3.7
3.8
3.9
The correct
answer
C.
C.
B.
A.
A.
A.
D.
B.
A.
4. Redox titration
№ of the test
task
4.1
4.2
4.3
4.4
4.5
4.6
4.7
4.8
4.9
4.10
4.11
4.12
4.13
4.14
4.15
4.16
4.17
4.18
4.19
The correct
answer
E.
D
E
C.
A.
E.
B.
D.
D.
A.
C.
B.
A.
E.
C.
C.
A.
C.
E.
№ of the test
task
4.20
4.21
4.22
4.23
4.24
4.25
4.26
4.27
4.28
4.29
4.30
4.31
4.32
4.33
4.34
4.35
4.36
4.37
4.38
The correct
answer
E.
C.
A.
B.
B.
C.
D.
C.
A.
E.
D.
B.
A.
E.
B.
B.
C.
E.
A.
№ of the test
task
4.39
4.40
4.41
4.42
4.43
4.44
5. Precipitation titration
№ of the test
task
5.1
5.2
5.3
5.4
5.5
5.6
The correct
answer
A.
A.
A.
A.
A.
A.
6. Complexometric titration
№ of the test
task
6.1
6.2
6.3
6.4
6.5
6.6
6.7
6.8
6.9
The correct
answer
E.
B.
C.
C.
B.
B
D
C.
A.
№ of the test
task
6.10
6.11
6.12
6.13
6.14
6.15
6.16
6.17
The correct
answer
C.
A.
B.
D.
C.
A.
A.
A.
The correct
answer
D.
D.
B.
D.
C.
B.
The list of the recommended literature
1. V.V. Bolotov, L.Yu. Klimenko, T.A. Kostina, S.V. Kolisnyk, K.V. Dynnik, T.V.
Zhukova. ANALYTICAL CHEMISTRY
COLLECTION OF LECTURES ON
QUANTITATIVE ANALYSIS. The manual for students of higher schools. Edited by professor
V.V.Bolotov . Kharkiv NUPh "Original" 2011
2. Harvey, David, 1956 – Modern analytical chemistry / David Harvey. — 1st ed.p. cm. 1.
Chemistry, Analytic. I. Title.QD75.2.H374 2000, 543— dc21