Expand ▼

The directory contains the main tables used to calculate the results of various chemical analyzes, as well as almost all the information necessary for the work of analytical chemists.
In the sixth edition (the fifth was published in 1979), the values ​​of the constants of the products of solubility, ionization of acids and bases, stability complex compounds, standard oxidation potentials, etc.
New data have been introduced on the masking of interfering ions and on atomic-adsorption methods for the determination of various metals. Obsolete material has been eliminated, necessary additions and clarifications have been made.
The guide is intended a wide range employees of chemical analytical laboratories and will be a necessary tool for students of higher and secondary specialized educational institutions.
CONTENT
Preface to the sixth edition
Preliminary remarks
Table 1. Relative atomic masses
Table 2. radioactive elements
Table 3 Ionic radii
Table 4 Relative masses atoms molecules and atomic groups
Table 5. Analytical and stoichiometric factors (factors)
Table 6. Solubility of inorganic and some organic compounds in water
Table 6a. Solubility of some other compounds
Table 7. Solubility of some inorganic compounds in organic solvents at 18-25°C.
Table 8. Solubility products of the most important poorly soluble substances
Table 9. Activity coefficients of various ions
Table 10. Activity coefficients of various ions at high values ​​of the ionic strength of the solution
Table 11. The most important organic reagents for the determination of organic matter
A. B alphabetical order reagents
B. In alphabetical order of defined elements
Table 12. The most important organic reagents for the determination of organic substances
Table 13. Some inorganic reagents used to determine organic substances
Table 14. Glassware Calibration
Table 15. Calculation of results of titrimetric determinations
A. Acid-base titrations
B. Methods of oxidation - recovery
B. Precipitation and complexation methods
D. EDTA Titration Methods
Table 16. Formulas for the transition from some expressions of solution concentrations to others
Table 17. Densities and concentrations of solutions
A. Densities and concentrations of solutions nitric acid s
B. Densities and concentrations of sulfuric acid solutions
B. Densities and concentrations of hydrochloric acid solutions
D. Densities and concentrations of solutions phosphoric acid
E. Densities and concentrations of perchloric acid solutions
E. Densities and concentrations of solutions acetic acid
G- Densities and concentrations of potassium hydroxide solutions
3. Densities and concentrations of sodium hydroxide solutions
I. Densities and concentrations of ammonia solutions
J. Densities and concentrations of sodium carbonate solutions
K. Densities and concentrations of solutions of some commercial reagents
Table 18. Ionic product of water at temperatures from 0 to 100°C
Table 19. The most important acid-base indicators
Table 20. Salt corrections for the most important indicators at different ionic strengths of solutions
Table 21. Some mixed indicators
Table 22. Universal indicators
Table 23. Important fluorescent indicators
Table 24. Some Chemiluminescent Indicators
Table 25. The most important adsorption indicators
Table 26. The most common indicators in complexometry (metal indicators)
Table 27. Masking reagents
Table 28
Table 29 buffer solutions
A. Buffer solutions pH = 1.10-3.50
B. Buffer solutions with pH = 1.10-4.96
B. Buffer solutions pH = 2.20-3.80
D. Buffer solutions with pH = 4.00-6.20
E. Buffer solutions with pH = 4.96-6.69
E. Buffer solutions with pH == 4.80-8.00
G. Buffer solutions with pH = 7.71-9.23
3. Buffer solutions with pH = 9.23-11.02
I. Buffer solutions with pH == 8.53-12.90
Table 30. Acetate buffer solutions
Table 31. Universal buffer mix
Table 32. Buffer solutions of individual substances
Table 33. Standard oxidation potentials(E°) with respect to the potential of a standard hydrogen electrode at 25°C
Table 34. pH of precipitation of metal hydroxides
Table 35. Ionization constants essential acids and grounds
Table 35. Stability constants of complex ions
A. Complexes with inorganic ligands
B. Complexes with organic ligands
Table 37. Mobility of some ions at 25 °C and infinite dilution
Table 38. The most important redox indicators
A. Indicators that are little dependent on pH and ionic strength of the solution
B. Indicators sensitive to changes in pH and ionic strength of the solution
Table 39
Table 40. Conditions for amperometric titration of certain substances
Table 41. Overvoltage of hydrogen and oxygen on various electrodes
Table 42 solutions of some compounds
Table 43. Wavelengths of the spectrum and their corresponding colors
Table 44. Determination of metals by atomic absorption spectrometry
Table 45. Photometric methods, definitions of some elements
Table 46. Flame photometric method for the determination of elements
Table 47. Properties of some solvents
Table 48. Extraction with organic solvents
A. Extraction various elements in the form of dithizonates
B, Extraction of various elements as diethyldithiocarbamates
B. Extraction of various elements as cupferronates
D. Extraction of various elements as oxyquinolates
E. Extraction of various elements of hydrochloric, hydrobromic, hydroiodic and nitric acids
equal volume of diethyl ether
Table 49. Distribution constants of some organic substances between organic solvents and water
Table 50. Separation of organic compounds
A. Classification of individual compounds according to their relation to the action of certain reagents
B. Composition of groups
B. Membership in major groups of various organic compounds
D. Common compounds whose position in groups is difficult to predict
E. Separation of mixtures
Table 51
A. Drying gases
B. Drying liquids
Table 52
Table 53. Sieve Scale
Table 54 Mathematical processing analysis results
A. Q-test values ​​depending on total number performed definitions (n) and from the accepted confidence level(a)
B. Values ​​of Studentent coefficients for calculating confidence limits
Applications. Examples of using some tables
Table 5
Table 15
Table 17
Table 19
Subject index

UDC 545 (083)

The directory contains the main tables used to calculate the results of various chemical analyzes.

The book is intended for employees of chemical analytical laboratories and can serve as a guide for students of higher and secondary specialized educational institutions when studying the course analytical chemistry.

Preface to fourth edition	7
From the preface to the first edition	7
Preliminary remarks	9
Table 1. Atomic weights elements	14
Table 2. Radioactive elements	18
Table 3. Ionic radii	19
Table 4. Ionization potentials of atoms and ions	23
Table 5. Structures of outer electron layers, ionic potentials and analytical groups cations	25
Table 6. Atomic weights, molecular weights, atomic group weights and their logarithms	26
Table 7. Analytical and stoichiometric factors (factors)	64
Table 8 Solubility of inorganic and some organic compounds in water	70
Table 9. Solubility of some inorganic compounds in organic solvents at 18-25°C	90
Table 10. Solubility products of the most important poorly soluble substances	94
Table 11. Activity coefficients of various ions	105
Table 12. Activity coefficients of various ions at high values ​​of the ionic strength of the solution	107
Table 13. Glassware Calibration	108
Table 14. Calculations of the results of volumetric analytical determinations	109
A. Acid-base titrations	109
B. Methods of oxidation - reduction	111
B. Precipitation and complexation methods	115
D. Methods of titration with complexone III	116
Table 15. Masking reagents for titration with complexone III	118
Table 16. Calculation of results of gas and gasometric analyzes	122
A. Bringing the volume of gas to normal conditions	124
B. Water vapor pressure over water and over absorption solutions	141
B. Densities of gases and vapors (ρ)	142
D. Gasometric (volumetric) determination of substances that form gases	144
Table 17. Formulas for the transition from some expressions of the concentration of solutions to others	145
Table 18. Density and concentration of solutions	146
A. Density and concentration of nitric acid solutions	146
B. Densities and concentrations of sulfuric acid solutions	147
B. Densities and concentrations of solutions of hydrochloric acid	149
D. Densities and concentrations of phosphoric acid solutions	150
E. Densities and concentrations of perchloric acid solutions	152
E. Density and concentration of acetic acid solutions	154
G. Densities and concentrations of caustic potash solutions	154
I. Densities and concentrations of solutions caustic soda	156
K. Densities and concentrations of ammonia solutions	157
L. Densities and concentrations of sodium carbonate solutions	158
M. Densities and concentrations of some commercial reagents	159
Table 19. The most important acid-base indicators	160
Table 20. Ionic product of water at temperatures from 0 to 100 ° C	181
Table 21. Colorimetric determination of pH solutions	182
Table 22. Indicator ionization constants	183
A. Single color indicators	183
B. Two-color indicators	183
Table 23. Some mixed indicators	184
Table 24. Universal indicators	187
Table 25. Important fluorescent indicators	188
Table 26. Some Chemiluminescent Indicators	197
Table 27. The most important adsorption indicators	198
Table 28. The most common indicators in complexometry	202
Table 29	230
Table 30. Preparation of buffer solutions	231
A. Buffer solutions pH 1.10-3.50	231
B. Buffer solutions with pH 1.10-4.96	232
B. Buffer solutions with a pH of 2.20-3.80	233
D. Buffer solutions pH 4.00-6.20	233
E. Buffer solutions pH 4.96-6.69	234
E. Buffer solutions pH 4.80-8.00	235
G. Buffer solutions pH 7.71-9.23	235
I. Buffer solutions with pH 9.23-11.02	236
J. Buffer solutions pH 8.53-12.90	237
Table 31 Acetic Acetate Buffer Solutions	238
Table 32. Universal buffer mix	238
Table 33. Buffer solutions from individual substances	239
Table 34. Definition electrode potentials	239
A. Values ​​of υ at n = 1 and temperatures from 0 to 50° C	242
B. Composition and potential of some electrodes compared with a normal hydrogen electrode	243
Table 35 Electrometric determination of pH	244
A. Normal potential of the quinhydron electrode E° chin./hydg. at temperatures from 0 to 50° C	245
B. Potentials of calomel electrodes at temperatures from 0 to 50 ° C	246
C. The difference between the normal potential of the hydron electrode ( E° quin./hydg.) and potentials of calomel reference electrodes ( E EC) at temperatures from 0 to 50° C	247
Table 36. pH precipitation of metal hydroxides	248
Table 37. Ionization constants of the most important acids and bases	247
Table 38. Instability constants of complex ions	255
A. Complexes with inorganic ligands	255
B. Complexes with organic ligands	266
Table 39. Mobility of some ions at 25°C and infinite dilution	270
Table 40. Normal oxidation potentials ( E°) in relation to the potential of a normal hydrogen electrode at 25° C	271
Table 41. The most important redox indicators	288
A. Indicators that are little dependent on pH and ionic strength of the solution	288
B. Indicators sensitive to changes in pH and ionic strength of the solution	290
Table 42. Wavelengths of the spectrum and their corresponding colors	294
Table 43. Photometric methods for the determination of various ions	295
Table 44. Properties of some solvents	306
Table 45. Extraction with organic solvents	310
A. Extraction of various elements in the form of dithizonates	310
B. Extraction of various elements in the form of diethyldithiocarbamates	314
B. Extraction of various elements as cupferronates	316
D. Extraction of various elements as oxyquinolates	317
E. Extraction of various elements from hydrochloric, hydrobromic, hydroiodic and nitric acids with an equal volume of diethyl ether	319
Table 46. Separation of organic compounds	320
A. Classification of individual compounds according to their relation to the action of certain reagents	320
B. Composition of groups	321
B. Belonging to the main groups of various organic compounds	324
D. Common compounds whose position in groups is difficult to predict	325
E. Separation of mixtures	328
Table 47	330
A. Drying gases	330
B. Drying liquids	330
Table 48. Preparation of hygrostats	331
Table 49	332
A. In alphabetical order of reagents	332
B. In alphabetical order of defined elements	374
Table 50. Sieve Scale	377
Table 51. Potential values ​​of polarographic half-waves on a mercury drop electrode	378
Table 52. Conditions for amperometric titration of certain substances	383
Table 53	399
Table 54. Overvoltage of hydrogen and oxygen on various electrodes	412
Table 55 solutions of some compounds	414
Table 56. Flame photometry	414
Table 57 English measures and US measures versus metric	415
Table 58	416
A. Logarithms	416
B. Antilogarithms	420
Applications. Examples of using some tables	424
Table 7	424
Table 14	426
Table 16	431
Table 18	434
Table 20	435
Table 21	437
Table 40	439
Subject index	443

4th ed., revised. and additional - M.: Chemistry, 1971. - 456 p. The reference book contains the main tables used to calculate the results of various chemical analyzes, as well as almost all the information necessary for the work of analytical chemists. Tables: Atomic weights of elements.
radioactive elements.
Ionic radii.
Ionization potentials of atoms and ions.
Structures of outer electron layers, ionic potentials and analytical groups of cations.
Atomic weights, molecular weights, atomic group weights and their logarithms.
Analytical and stoichiometric factors (factors).
Solubility of inorganic and some organic compounds in water.
Solubility of some inorganic compounds in organic solvents at 18-25C.
Solubility products of the most important poorly soluble substances.
Activity coefficients of various ions.
Activity coefficients of various ions at high values ​​of the ionic strength of the solution.
Calibration of glassware.
Calculations of the results of volume-analytical determinations.
Masking reagents during titration with complexone III.
Calculation of results of gas and gasometric analyses.
Formulas for the transition of some expressions of concentrations of solutions to others.
Density and concentration of solutions.
The most important acid-base indicators.
Ionic product of water at temperatures from 0 to 100C.
Colorimetric determination of the pH of solutions.
Indicator ionization constants.
Some mixed indicators.
Universal indicators.
The most important fluorescent indicators.
Some chemiluminescent indicators.
The most important adsorption indicators.
The most common indicators in complexometry.
Recalculation of the hydrogen index (pH) to the activity of hydrogen ions and vice versa.
Preparation of buffer solutions.
Acetic-acetate buffer solutions.
Universal buffer mix.
Buffer solutions from individual substances.
Determination of electrode potentials.
Electrometric determination of pH.
pH precipitation of metal hydroxides.
Ionization constants of the most important acids and bases.
Instability constants of complex ions.
Mobility of some ions at 25°C and infinite dilution.
Normal oxidation potentials in relation to the potential of a normal hydrogen electrode at 25C.
The most important redox indicators.
The wavelengths of the spectrum and their corresponding colors.
Photometric methods for the determination of various ions.
properties of some solvents.
Extractions with organic solvents.
Separation of organic compounds.
Drying agents.
Preparation of hygrostats.
The most important organic reagents.
Sieve scale.
The value of the potentials of polarographic half-waves on a mercury drop electrode.
Conditions for amperometric titration of certain substances.
Conditions for amperometric titration with two polarized indicator electrodes.
Overvoltage of hydrogen and oxygen on various electrodes.
Decomposition potentials 1 n. solutions of some compounds.
Flame photometry.
English measures and US measures compared to metric.
Simplified table of five-digit logarithm mantissas.

2Вr - -2ē →Br 2, E 0 1 \u003d -1.065V;

PbO 2 + 4H + +2ē → Pb 2+ + 2H 2 O, E 0 2 = 1.449V.

EMF \u003d E 0 ok - E 0 restore \u003d 1.449 - (−1.065) \u003d 2.514V.

The oxidizing agent is always the system with the higher electrode potential. Since here E 0 2 is much greater than E 0 1, then at almost any concentration of interacting substances, the bromide ion will serve as a reducing agent, and lead (IV) oxide as an oxidizing agent. The reaction will proceed from left to right, because The EMF of the reaction is greater than zero.

Laboratory work No. 7 Redox reactions

Experience 1. The influence of the medium on the nature of the reduction of potassium permanganate.

Completing of the work. Add 4 drops of potassium permanganate solution (KMnO 4) to three test tubes. Add 2 drops of 2 N sulfuric acid solution (H 2 SO 4) to the 1st tube, 2 drops of distilled water to the 2nd test tube, 2 drops of 2 N alkali solution (NaOH) to the 3rd tube. Add a few crystals of sodium sulfite (Na 2 SO 3) to each test tube at the tip of a microspatula and mix the solutions thoroughly until the salt is completely dissolved. Note the change in color of the solutions in all test tubes. The following reactions take place in test tubes:

1. KMnO 4 + Na 2 SO 3 + H 2 SO 4 → MnSO 4 + Na 2 SO 4 + K 2 SO 4 + H 2 O;

2. KMnO 4 + Na 2 SO 3 + H 2 O → MnO 2 + Na 2 SO 4 +KOH;

3. KMnO 4 + Na 2 SO 3 + NaOH → K 2 MnO 4 + Na 2 MnO 4 + Na 2 SO 4 + H 2 O.

Recording experience data. Write the reaction equations for the reduction of potassium permanganate with sodium sulfite in acidic, neutral and alkaline media. Select the coefficients by the method of electron-ion balance. At the same time, take into account that manganese compounds in various degrees of its oxidation have characteristic colors: Mn 2+ is a slightly pink color, and at a low concentration it is practically colorless, MnO 2 (manganese dioxide) and manganese hydroxide are hardly soluble brown substances, MnO 4 2− (manganate ion) - green color.

To what degree of oxidation is potassium permanganate reduced in solutions having pH< 7, рН = 7, рН >7? Calculate the molar mass equivalent of KMnO 4 in each of these cases, knowing that M E = M (KMnO 4) / nē (the number of electrons accepted by 1 mol of oxidizing agent).

Experiment 2. Oxidative and reducing properties of p-element atoms in intermediate oxidation states.

a) Sulfur compounds (+ IV) in redox reactions.

Completing of the work. In the 1st test tube with a solution of potassium dichromate (K 2 Cr 2 O 7), in the 2nd with a solution of sodium sulfide (Na 2 S), add 1 drop of a 2 n solution of sulfuric acid and at the tip of the spatula a few crystals of sodium sulfite (Na 2 SO 3). How did the color of the solution change in the 1st test tube? Why did the solution become cloudy in the 2nd test tube? An oxidizing agent or a reducing agent can be in chemical reactions K 2 Cr 2 O 7? Na2S? Does Na 2 SO 3 exhibit oxidizing or reducing properties?

Write the equations of the reactions carried out. Select the coefficients by the half-reaction method.

Experience 3. Intramolecular redox reactions.

a) Decomposition of ammonium dichromate.

Completing of the work. Place several microspatulas of crystalline ammonium dichromate ((NH 4) 2 Cr 2 O 7) in a pile in a porcelain cup. Insert a piece of magnesium tape into the top of the slide and light it. After a few seconds, observe the rapid decomposition of the salt: (NH 4) 2 Cr 2 O 7 → Cr 2 O 3 + N 2 + 4H 2 O.

Green pellets are Cr 2 O 3 - chromium (III) oxide. Atoms of which element are oxidizing agents? Restorers? How has their oxidation state changed?

Experience 4. Oxidizing and reducing properties of tin compounds (II) Performance of work. Add 3 drops of a solution (FeCl 3) of iron (III) chloride and 3 drops of a solution (K 3) of potassium hexacyanoferrate (III) into a test tube. Mark the color of the solution and add a solution of (SnCl 2) tin (II) chloride to it drop by drop until a precipitate forms. The intense blue coloring of the solution is due to the appearance of Fe 2+ ions, which form a blue precipitate with K 3 . Tin (II) chloride in this case passes into tin (IV) chloride.

FeCl 3 + SnCl 2 → FeCl 2 + SnCl 4 (equate using the electron balance method); 3FeCl 2 + 2K 3 → Fe 3 2 + 6KCl.

Is the Sn 2+ ion an oxidizing or reducing agent in this reaction?

Add a piece of zinc and 5 drops of tin (II) chloride solution to another test tube, observe the formation of shiny tin crystals on the zinc surface. Write the reaction equation for the interaction of tin (II) chloride with zinc, select the coefficients using the electronic balance method. Is the Sn 2+ ion an oxidizing or reducing agent in this reaction?

Lurie Yu.Yu.
Name: Handbook of Analytical Chemistry
Publisher: Moscow: "Chemistry"
Number of pages: 448 (1989)
ISBN: 5-7245-0000-0
The year of publishing: 1971 (4th edition) and 1989 (6th edition)

Page examples

Review in Russian:1971 (4th edition)
The directory contains the main tables used to calculate the results of various chemical analyzes.
The book is intended for employees of chemical-analytical laboratories and can serve as a guide for students of higher and secondary specialized educational institutions in the study of the course of analytical chemistry.
1989 (6th edition)
The reference book contains the main tables used to calculate the results of various chemical analyzes, as well as almost all the information necessary for the work of analytical chemists.
The sixth edition (the fifth edition appeared in 1979) revised and in some cases corrected the constants of the products of solubility, ionization of acids and bases, stability of complex compounds, standard oxidation potentials, etc. New data on the masking of interfering ions and on the atomic adsorption methods for the determination of various metals. Obsolete material has been eliminated, necessary additions and clarifications have been made.
The handbook is intended for a wide range of employees of chemical analytical laboratories and will be an indispensable guide for students of higher and secondary specialized educational institutions.
Download from the site 6th edition 1989:Download from the site 4th edition 1971:Content:

Preface to the Sixth Edition Preliminary Remarks
Table 1. Relative atomic masses
Table 2. Radioactive elements
Table 5. Ionic radii
Table 4. Relative masses of atoms of molecules and atomic groups
Table 5. Analytical and stoichiometric factors (factors)
Table 6. Solubility of inorganic and some organic compounds in water
Table 6a. Solubility of some other compounds
Table 7. Solubility of some inorganic compounds in organic solvents at 18-25 °C
Table 8. Solubility products of the most important poorly soluble substances.
Table 9. Activity coefficients of various ions
Table 10. Activity coefficients of various ions at high values ​​of the ionic strength of the solution
Table 11. The most important organic reagents for the determination of inorganic substances
A. In alphabetical order of reagents
B. In alphabetical order of defined elements
Table 12. The most important organic reagents for the determination of organic substances
Table 13. Some inorganic reagents used for the determination of organic substances
Table 14. Glassware Calibration
Table 15. Calculation of results of titrimetric determinations
A. Acid-base titrations
B. Methods of oxidation - recovery
B. Precipitation and complexation methods
D. EDTA Titration Methods
Table 16. Formulas for the transition from some expressions of solution concentrations to others
Table. 17. Density and concentration of solutions
A. Densities and concentrations of nitric acid solutions
B. Densities and concentrations of sulfuric acid solutions
C. Densities and concentrations of hydrochloric acid solutions
D. Density and concentration of phosphoric acid solutions
E. Densities and concentrations of perchloric acid solutions
E. Densities and concentrations of acetic acid solutions
G. Densities and concentrations of potassium hydroxide solutions
3. Densities and concentrations of sodium hydroxide solutions
I, Densities and concentrations of ammonia solutions
J. Densities and concentrations of sodium carbonate solutions
K. Densities and concentrations of solutions of some commercial reagents
Table 18. Ionic product of water at temperatures from 0 to 100 C
Table 19. The most important acid-base indicators
Table 20. Salt corrections for the most important indicators at different ionic strengths of solutions
Table 21. Some mixed indicators
Table 22. Universal indicators
Table 23. Important fluorescent indicators
Table 24. Some Chemiluminescent Indicators
Table 25. The most important adsorption indicators
Table 26. The most common indicators in complexometry (metal indicators)
Table 27. Masking reagents
Table 28
Table 29. Buffer solutions
A. Buffer solutions pH = 1.10-3.50
B. Buffer solutions with pH = 1.10-4.96
B. Buffer solutions pH = 2.20-3.80
D. Buffer solutions with pH = 4.00-6.20
E. Buffer solutions with pH = 4.95-6.69
E. Buffer solutions with pH = 4.80-8.00
G. Buffer solutions with pH = 7.71-9.23
3. Buffer solutions with pH = 9.23-11.02
I. Buffer solutions with pH = 8.53-12.90
Table 30. Acetate buffer solutions
Table 31. Universal buffer mix
Table 32. Buffer solutions of individual substances
Table 33 Standard oxidation potentials (E0) vs. standard hydrogen electrode potential at 25°C
Table 34. pH of precipitation of metal hydroxides
Table 35. Ionization constants of the most important acids and bases
Table 36. Stability constants of complex ions
A. Complexes with inorganic ligands
B. Complexes with organic ligands
Table 37. Mobility of some ions at 25°C and infinite dilution
Table 38. The most important redox indicators
A. Indicators that are little dependent on pH and ionic strength of the solution
B. Indicators sensitive to changes in pH and ionic strength of the solution
Table 39
Table 40. Conditions for amperometric titration of certain substances
Table 41. Overvoltage of hydrogen and oxygen on various electrodes
Table 42 solutions of some compounds
Table 43. Wavelengths of the spectrum and their corresponding colors
Table 44. Determination of metals by atomic absorption spectrometry
Table 45. Photometric methods for the determination of some elements
Table 46. Flame photometric method for the determination of elements
Table 47. Properties of some solvents
Table 48. Extraction with organic solvents
A. Extraction of various elements as dithizonates
B. Extraction of various elements in the form of diethyldithiocarbamates
B. Extraction of various elements as cupferronates
D. Extraction of various elements as oxyquinolates
E. Extraction of various elements of hydrochloric, hydrobromic, hydroiodic and nitric acids with an equal volume of diethyl ether
Table 49. Distribution constants of some organic substances between organic solvents and water
Table 50. Separation of organic compounds
A. Classification of individual compounds according to their relation to the action of certain reagents
B. Composition of groups
B. Membership in major groups of various organic compounds
D. Common compounds whose position in groups is difficult to predict
E. Separation of mixtures
Table 51
A. Drying gases
B. Drying liquids
Table 52
Table 53. Sieve Scale
Table 54. Mathematical processing of analysis results
A. Q-test values ​​depending on the total number of determinations performed (n) and on the accepted confidence level (alpha)
B. Values ​​of Student coefficients for calculating confidence limits
Applications. Examples of using some tables
Table 5
Table 15
Table 17
Table 19
Subject index