Olimpíada Internacional de Química

1. The atom

1.1.

Introduction

1.1.1.

Counting of nucleons

1

1.1.2.

Isotopes

1

1.2.

The hydrogen atom

1.2.1.

Concept of energy levels

1

1.2.2.

Shape of s-orbitals

1

1.2.3.

Shape and orientation of p-orbitals

1

1.2.4.

Shape and orientation of d-orbitals

3

1.2.5.

Understanding the simplest Schrodinger equation

3

1.2.6.

Square of the wave function and probability

3

1.2.7.

Quantum numbers (n, l, m_l)

3

1.3.

Radioactivity

1.3.1.

Types of radioactivity

1

1.3.2.

Radioactive decay

1

1.3.3.

Nuclear reactions

2

2. Chemical bonding

2.1.

VSEPR – Simple molecular structures with

2.1.1.

no more than four electron pairs about central atom

1

2.1.2.

with central atom exceeding the “octet rule”

3

2.2.

Delocalization and resonance

3

2.3.

Hybrid orbital theory

3

2.4.

Molecular orbital theory

2.4.1.

molecular orbital diagram (H₂ molecule)

3

2.4.2.

molecular orbital diagram (N₂ and O₂ molecules)

3

2.4.3.

bond orders in O₂, O₂^–, O₂⁺

3

2.4.4.

unpaired electrons and paramagnetism

3

3. Chemical calculations

3.1.1.

Balancing equations

1

3.1.2.

Stoichiometric calculations

1

3.1.3.

Mass and volume relations (including density)

1

3.1.4.

Empirical formula

1

3.1.5.

Avogadro’s number

1

3.1.6.

Concentration calculations

1

4. Periodic trends

4.1.

Electron configuration

4.1.1.

Pauli exclusion principle

1

4.1.2.

Hund’s Rule

1

4.1.3.

Main group elements

1

4.1.4.

Transition metal elements

1

4.1.5.

Lanthanide and actinide metals

3

4.2.

Electronegativity

1

4.3.

Electron affinity

2

4.4.

First ionization energy

1

4.5.

Atomic size

1

4.6.

Ion size

1

4.7.

Highest oxidation number

1

5. Inorganic Chemistry

5.1.

Introduction

5.1.1.

Trends in physical properties of elements (Main groups)

5.1.1.1.

melting point

1

5.1.1.2.

boiling point

1

5.1.1.3.

metal character

1

5.1.1.4.

magnetic properties

3

5.1.1.5.

electrical conductivity

2

5.1.2.

Oxidation number

1

5.1.3.

Nomenclature

5.1.3.1.

main group compounds

1

5.1.3.2.

transition metal compounds

1

5.1.3.3.

simple metal complexes

3

5.2.

Groups 1 and 2

5.2.1.

Trend in reactivity of (heavy elements more reactive)

1

5.2.2.

Products of reaction with

5.2.2.1.

water

1

5.2.2.2.

halogens

1

5.2.2.3.

oxygen

2

5.2.3.

Basicity of oxides

1

5.2.4.

Properties of hydrides

3

5.2.5.

Other compounds, properties and oxidation states

3

5.3.

Groups 13 – 18 and Hydrogen

5.3.1.

Binary molecular compounds of hydrogen

5.3.1.1.

Formulae

1

5.3.1.2.

Acid-base properties of CH₄, NH₃, H₂O, H₂S

1

5.3.1.3.

Other properties

3

5.3.2.

Group 13

5.3.2.1

The oxidation state of boron and aluminium in their oxides and chlorides is +3

1

5.3.2.2.

The acid-base properties of aluminium oxide/hydroxide

2

5.3.2.3.

Reaction of boron(III) oxide with water

3

5.3.2.4.

Reaction of boron(III) chloride with water

3

5.3.2.5.

Other compounds, properties and oxidation states

3

5.3.3.

Group 14

5.3.3.1.

The oxidation state of Si in its chloride and oxide is +4

1

5.3.3.2.

The +2 and +4 oxidation states of carbon, tin and lead, the acid-base and redox properties of the oxides and chlorides

2

5.3.3.3.

Other compounds, properties and oxidation states

3

5.3.4.

Group 15

5.3.4.1.

Phosphorus(+5) oxide and chloride, and their reaction with water

2

5.3.4.2.

Phosphorus(+3) oxide and chloride, and their reaction with water

2

5.3.4.3.

Oxides of nitrogen

a. Reaction of NO to form NO₂

1

b. Dimerization of NO₂

1

c. Reaction of NO₂ with water

1

5.3.4.4.

Redox properties of

a. HNO₃ and nitrates

1

b. HNO₂ and NH₂NH₂

3

5.3.4.5.

Bi(+5) and Bi(+3)

3

5.3.4.6.

Other compounds, properties and oxidation states

3

5.3.5.

Group 16

5.3.5.1.

The +4 and +6 oxidation states of sulfur, reaction of their oxides with water, properties of their acids

1

5.3.5.2.

Reaction of thiosulfate anion with I₂

3

5.3.5.3.

Other compounds, properties and oxidation states

3

5.3.6.

Group 17 (Halogens)

5.3.6.1.

Reactivity and oxidant strength decreases from F₂ to I₂

1

5.3.6.2.

Acid-base properties of the hydrogen halides

1

5.3.6.3.

The oxidation state of fluorine in its compounds is –1

1

5.3.6.4.

The –1, +1, +3, +5, +7 oxidation states of chlorine

1

5.3.6.5.

Mononuclear oxoanions of chlorine

2

5.3.6.6.

Reactions of halogens with water

3

5.3.6.7.

Reaction of Cl₂O and Cl₂O₇ with water

3

5.3.6.8.

Other compounds, properties and oxidation states

3

5.3.7.

Group 18

3

5.4.

Transition elements

5.4.1.

Common oxidation states of common transition metals:
Cr(+2), Cr(+3) Mn(+2), Mn(+4), Mn(+7) Ag(+1)
Fe(+2), Fe(+3) Co(+2) Zn(+2)
Hg(+1), Hg(+2) Cu(+1), Cu(+2) Ni(+2)

1

5.4.2.

Colours of ions listed above in aqueous solution

2

5.4.3.

Insolubility of Ag, Hg and Cu in HCl

2

5.4.4.

M²⁺ arising by dissolution of the other metals in HCl

2

5.4.5.

Cr(OH)₃ and Zn(OH)₂ are amphoteric and the other +2
oxides/hydroxides of the metals listed above are basic

2

5.4.6.

MnO₄^– and Cr₂O₇^2– are strong oxidants in acid solution

1

5.4.7.

pH dependence of products of MnO₄^– acting as oxidant

2

5.4.8.

Interconversion between CrO₄^2– and Cr₂O₇^2–

3

5.4.9.

Other compounds, properties and oxidation states

3

5.5.

Lanthanides and actinides

3

5.6.

Coordination chemistry including stereochemistry

5.6.1.

Definition of coordination number

1

5.6.2.

Writing equations for complexation reactions given all formulae

1

5.6.3.

Formulae of common complex ions

5.6.3.1.

Ag(NH₃)₂⁺

1

5.6.3.2.

Ag(S₂O₃)₂^3–

3

5.6.3.3.

FeSCN²⁺

3

5.6.3.4.

Cu(NH₃)₄²⁺

1

5.6.3.5.

Other complex ions

3

5.6.4.

(6.5) Ligand field theory (eg and t2g terms, high and low spin)

3

5.6.5.

Stereochemistry

5.6.5.1.

(6.7) cis and trans

3

5.6.5.2.

enantiomers

3

5.7.

Selected industrial processes

5.7.1.

Preparation of H₂SO₄

1

5.7.2.

Preparation of NH₃

1

5.7.3.

Preparation of Na₂CO₃

2

5.7.4.

Preparation of Cl₂ and NaOH

2

5.7.5.

Preparation of HNO₃

2

6. Physical chemistry

6.1.

Gases

6.1.1.

Ideal gas law

1

6.1.2.

van der Waal’s gas law

3

6.1.3.

definition of partial pressure

2

6.1.4.

Dalton’s Law

3

6.2.

Thermodynamics

6.2.1.

First Law

6.2.1.1.

Concept of system and surroundings

2

6.2.1.2.

Energy, heat and work

2

6.2.2.

Enthalpy

6.2.2.1.

Relationship between internal energy and enthalpy

3

6.2.2.2.

Definition of heat capacity

2

6.2.2.3.

Difference between C_p and C_v (ideal gas only)

3

6.2.2.4.

Enthalpy is a state property (Hess’s Law)

2

6.2.2.5.

Born-Haber cycle for ionic compounds

3

6.2.2.6.

Use of standard formation enthalpies

2

6.2.2.7.

Enthalpies of solution and solvation

3

6.2.2.8.

Bond enthalpies (definition and use)

2

6.2.3.

Second Law (Entropy and Free Energy)

6.2.3.1.

Entropy definition (dq / T)

3

6.2.3.2.

Entropy and disorder

3

6.2.3.3.

Entropy definition (S = k ln W)

3

6.2.3.4.

Gibbs energy definition (DG = DH – TDS)

3

6.2.3.5.

Using DG to predict direction of natural change

3

6.2.3.6.

Relationship between DG° and equilibrium constant K

3

6.3.

Equilibrium

6.3.1.

Acid-base

6.3.1.1.

Arrhenius definitions of acids and bases

1

6.3.1.2.

Bronsted-Lowry definitions

1

6.3.1.3.

Conjugate acids and bases

1

6.3.1.4.

pH definition

1

6.3.1.5.

K_w definition

1

6.3.1.6.

K_a and K_b as a measure of acid and base strength

1

6.3.1.7.

Acidity or basicity of ions

1

6.3.1.8.

Calculation of pH from pK_a(weak acid)

1

6.3.1.9.

Calculation of pH of a simple buffer solution

2

6.3.2.

Gas phase

6.3.2.1.

Equilibrium constant in partial pressures

3

6.3.2.2.

Relating K_p and K_c

3

6.3.3.

Solubility

6.3.3.1.

Solubility constant (product) definition (K_sp)

2

6.3.3.2.

Calculation of solubility in water from K_sp

2

6.3.4.

Compleximetric

6.3.4.1.

Complex formation constant (definition)

3

6.3.4.2.

Problems involving compleximetric equilibria

3

6.3.4.3.

Lewis acids and bases

3

6.3.4.4.

Hard and soft Lewis acids and bases

3

6.3.5.

Phase

6.3.5.1.

Temperature dependence of vapour pressure

3

6.3.5.2.

Clausius-Clapeyron equation

3

6.3.5.3.

Single component phase diagrams

a. triple point

3

b. critical point

3

6.3.5.4.

liquid-vapour system

a. ideal and nonideal systems

3

b. diagram

3

c. use in fractional distillation

3

6.3.5.5.

Henry’s Law

3

6.3.5.6.

Raoult’s Law

3

6.3.5.7.

Deviation from Raoult’s Law

3

6.3.5.8.

Boiling point elevation

3

6.3.5.9.

Freezing point depression

3

6.3.5.10.

Osmotic pressure

3

6.3.5.11.

Partition coefficient

3

6.3.5.12.

Solvent extraction

3

6.3.6.

Multiple

6.3.6.1.

Calculation of pH for multiprotic acids

3

6.3.6.2.

Calculation of pH for weak acid mixtures

3

6.4.

Electrochemistry

6.4.1.

Electromotive force (definition)

1

6.4.2.

First kind electrodes

1

6.4.3.

Standard electrode potential

1

6.4.4.

Nernst equation

3

6.4.5.

Second kind electrodes

3

6.4.6.

Relationship between DG and electromotive force

3

7. Chemical kinetics (Homogeneous reactions)

7.1.

Introduction

7.1.1.

Factors affecting reaction rate

1

7.1.2.

Reaction coordinates and the basic idea of a transition state

1

7.2.

Rate law

7.2.1.

Differential rate law

2

7.2.2.

Concept of reaction order

2

7.2.3.

Rate constant definition

2

7.2.4.

First order reactions

7.2.4.1.

Dependence of concentration on time

3

7.2.4.2.

Concept of half life

3

7.2.4.3.

Relationship between half life and rate constant

3

7.2.4.4.

Calculation of first order rate constant from

a. differential rate law

3

b. integrated rate law

3

7.2.4.5.

Rate constant for second and third order reactions

3

7.3.

Reaction mechanisms

7.3.1.

Concept of molecularity

3

7.3.2.

Rate-determining step

3

7.3.3.

Basic concepts of collision theory

3

7.3.4.

Opposing parallel and consecutive reactions

3

7.3.5.

Arrhenius’s law

3

7.3.5.1.

Definition of activation energy

3

7.3.5.2.

Calculation of activation energy

3

8. Spectroscopy

8.1.

UV/visible

8.1.1.

Identification of aromatic compound

3

8.1.2.

Identification of chromophore

3

8.1.3.

Dyes: colour vs structure

3

8.1.4.

Beer’s Law

3

8.2.

Infrared

8.2.1.

Interpretation using a table of frequencies

3

8.2.2.

Recognition of hydrogen bonds

3

8.3.

x-Ray

8.3.1.

Bragg’s Law

3

8.3.2.

Concept of

8.3.2.1.

coordination number

3

8.3.2.2.

unit cell

3

8.3.3.

Solid structures

8.3.3.1.

NaCl

3

8.3.3.2.

CsCl

3

8.3.3.3.

metals

3

8.4.

NMR

8.4.1.

General Concepts

8.4.1.1.

chemical shift

3

8.4.1.2.

spin-spin coupling and coupling constants

3

8.4.1.3.

integration

3

8.4.2.

Interpretation of a simple 1H spectrum (like ethanol)

3

8.4.3.

Identification of o- and p-disubstituted benzene

3

8.4.4.

Interpretation of simple spectra of 13C (proton decoupled) and other 1/2 spin nuclei

3

8.5.

Mass spectrometry

8.5.1.1.

Recognition of molecular ion

3

8.5.1.2.

Recognition of fragments with the help of a table

3

8.5.1.3.

Recognition of typical isotope distribution

3

9. Organic Chemistry

9.1.

Introduction

9.1.1.

(3.1.1) Alkane naming (IUPAC)

1

9.1.2.

Trends in boiling points of

9.1.2.1.

(3.1.3) alkanes with structure

1

9.1.2.2.

(3.7.1) alcohols vs ethers due to hydrogen-bonding

1

9.1.3.

(3.3.1, 3.4.1) Geometry at singly, doubly, and triply bonded carbon

1

9.1.4.

Identification of common functional groups

1

9.1.5.

Isomerism of alkenes

9.1.5.1.

cis-trans

1

9.1.5.2.

E/Z

3

9.1.6.

Enantiomers

9.1.6.1.

Optical activity

2

9.1.6.2.

R/S nomenclature

3

9.2.

Reactivity

9.2.1.

Alkanes

9.2.1.1.

reaction with halogens

a. products

1

b. free radical mechanism (initiation, termination)

2

9.2.1.2.

Cycloalkanes

a. names

2

b. Strain in small rings

3

c. chair/boat conformations of cyclohexane

3

9.2.2.

Alkenes

9.2.2.1.

Products from Br₂, HBr and H₂O/H⁺

1

9.2.2.2.

Markownikoff’s rule

2

9.2.2.3.

Mechanism involving carbocation intermediates

3

9.2.2.4.

Relative stability of carbocations

3

9.2.2.5.

1,4 addition to dienes

3

9.2.3.

Alkynes

9.2.3.1.

Acidity relative to alkenes

3

9.2.3.2.

Differences in chemical properties from alkenes

2

9.2.4.

Benzene

9.2.4.1.

formula

1

9.2.4.2.

stabilization by resonance

1

9.2.4.3.

electrophilic substitution (nitration, halogenation)

a. directing effect of first substituent

3

b. effect of first substituent on reactivity

3

c. explanation of substituent effects

3

9.2.5.

Halogen compounds

9.2.5.1.

Nomenclature of monofunctional

1

9.2.5.2.

Substitution reactions

a. giving alcohols

3

b. in which halogen is exchanged

3

c. reactivity

i. primary vs secondary vs tertiary

3

ii. aliphatic vs aromatic

3

d. S_N1 and S_N2 mechanisms

3

9.2.5.3.

Elimination reactions

2

9.2.5.4.

Competition of elimination and substitution

2

9.2.6.

Alcohols

9.2.6.1.

Nomenclature of monofunctional

1

9.2.6.2.

Comparison of acidity of alcohols and phenols

2

9.2.6.3.

Dehydration to alkenes

1

9.2.6.4.

Esters with inorganic acid

2

9.2.6.5.

Oxidation reactions

1

9.2.7.

Aldehydes and ketones

9.2.7.1.

Nomenclature of monofunctional

1

9.2.7.2.

Oxidation of aldehydes

1

9.2.7.3.

Reduction to alcohols (LiAlH₄, NaBH₄)

3

9.2.7.4.

Keto/enol tautomerism

3

9.2.7.5.

Nucleophilic addition reactions with

a. HCN

3

b. RNH₂ (R = alkyl, HO, NH₂)

3

c. enolate anions (aldol condensation)

3

d. alcohols to form acetals/ketals

3

e. Grignard reagents

3

9.2.8.

Carboxylic acids and their derivatives

9.2.8.1.

Nomenclature of carboxylic acids and their derivatives (esters, acid halides, amides)

2

9.2.8.2.

Acidity strength related to inductive effects

3

9.2.8.3.

Preparation of carboxylic acids by hydrolysis of

a. esters (including soaps)

1

b. amides

2

c. nitriles

3

9.2.8.4.

Reaction of carboxylic acids

a. with alcohols to form esters

1

b. to form acid chlorides

3

c. to form anhydrides

3

9.2.8.5.

Reaction of acid chlorides to form amides

3

9.2.8.6.

Mechanism of esterification

3

9.2.8.7.

Multifunctional acids (hydroxyacids, ketoacids)

3

9.2.8.8.

Polycarboxylic acids

3

9.2.9.

Amines

9.2.9.1.

Nomenclature

a. simple amines

1

b. recognition of primary, secondary, tertiary

1

9.2.9.2.

Basicity

a. As a property of an amine

1

b. Comparison of basicity of aliphatic and aromatic

3

c. Comparison of basicity of amines and amides

3

d. Preparation of amines

i. from halides

3

ii. from aromatic nitro compounds

3

iii. from amides (by hydrolysis)

3

9.2.9.3.

Diazotization

a. of aliphatic amines

3

b. of aromatic amines

3

10. Polymers

10.1.

Synthetic

10.1.1.

Addition polymers

10.1.1.1.

polystyrene

2

10.1.1.2.

polyethene

1

10.1.1.3.

chain mechanism of formation

2

10.1.2.

Condensation polymers

10.1.2.1.

polyesters

2

10.1.2.2.

polyamides

2

10.1.3.

Silicones

3

10.1.4.

Concept of cross-linking and its affect on properties

3

10.2.

Natural

10.2.1.

Silicates

3

10.2.2.

Rubber

3

11. Biochemistry

11.1.

Carbohydrates

11.1.1.

Glucose and fructose

11.1.1.1.

chain formulae

1

11.1.1.2.

Fischer projections

2

11.1.1.3.

Haworth formulae

3

11.1.2.

Difference between starch and cellulose

2

11.1.3.

Difference between a- and b- D glucose

2

11.2.

Fats

11.2.1.

Structure of fats in relationship to properties

2

11.2.2.

Formula of glycerol

1

11.3.

Nitrogen-containing Compounds of Biological Importance

11.3.1.

Amino acids

11.3.1.1.

Ionic structure

1

11.3.1.2.

Isoelectric point

3

11.3.1.3.

20 amino acids (classification with structures provided)

2

11.3.1.4.

Separation by electrophoresis

3

11.3.1.5.

The peptide linkage

1

11.3.2.

Proteins

11.3.2.1.

Primary structure

1

11.3.2.2.

–S-S- bridges

3

11.3.2.3.

Sequence analysis

3

11.3.2.4.

Secondary structure

3

11.3.2.5.

Details of a-helix structure

3

11.3.2.6.

Tertiary structure

3

11.3.2.7.

Denaturation (change in pH, temperature, metals, ethanol)

2

11.3.3.

Nuclei Acids and Protein Synthesis

11.3.3.1.

Pyrimidine and purine

3

11.3.3.2.

Nucleosides and nucleotides

3

11.3.3.3.

Formulae of pyrimidine and purine bases

3

11.3.3.4.

Difference between ribose and 2-deoxyribose

3

11.3.3.5.

Base combination CG and AT (hydrogen-bonding)

3

11.3.3.6.

Difference between DNA and RNA

3

11.3.3.7.

Difference between mRNA and tRNA

3

11.4.

Enzymes

11.4.1.1.

General properties, active centers

3

11.4.1.2.

Nomenclature, kinetics, coenzymes, function of ATP

3

12. Analytical chemistry

12.1.

Titrations

12.1.1.

acid-base

12.1.1.1.

Titration curve; pH (strong and weak acid)

2

12.1.1.2.

Choice of indicators for acidimetry

2

12.1.2.

Redox titration

3

12.2.

Qualitative analysis

12.2.1.

Ions (Inorganic)

12.2.1.1.

Identification of Ag⁺, Ba²⁺, Cl^–, SO₄^2–

2

12.2.1.2.

Identification of other anions and cations

3

12.2.2.

Organic functional groups

12.2.2.1.

Lucas reagent (1-, 2-, 3-alcohols)

3

12.2.2.2.

Iodoform reaction

3

12.2.2.3.

Identification of primary, secondary, tertiary,

quarternary amines in the laboratory

3

12.3.

Chromatographic methods of separation

3

Experimental part

Level 1:

is assigned to the basic experimental activities which are supposed to be mastered by competitors very well

Level 2:

is assigned to the activities which are parts of school experimental exercises in developed countries and the authors of IChO tasks may incorporate them into the tasks without being bounded to mention it in advance

Level 3:

is assigned to such activities which are not in the chemistry syllabus in the majority of participating countries and the authors are obliged to mention them in the set of preparatory tasks

If the organizer wants to apply a technique which is not mentioned in the above syllabus, this technique is set to level 3 automatically.

1. Synthesis of inorganic and organic compounds

1.1.

Heating with burners and hotplates

1

1.2.

Heating of liquids

1

1.3.

Handling the work with inflammable substances and materials

1

1.4.

Measuring of masses (analytical balance)

1

1.5.

Measuring of volumes of liquids (measuring cylinder, pipette, burette)

1

1.6.

Preparation of solutions from a solid compound and solvent

1

1.7.

Mixing and dilution of solutions

1

1.8.

Mixing and stirring of liquids

1

1.9.

Using mixer and magnetic stirrer

2

1.10.

Using a dropping funnel

1

1.11.

Syntheses in flat bottom vessels – general principles

1

1.12.

Syntheses in round bottom vessels – general principles

1

1.13

Syntheses in a closed apparatus – general principles

1

1.14.

Using microscale equipment for synthesis

3

1.15.

Apparatus for heating of reaction mixture under reflux

2

1.16.

Apparatus for distillation of liquids at normal pressure

2

1.17.

Apparatus for distillation of liquids at reduced pressure

2

1.18.

Apparatus for steam distillation

3

1.19.

Filtration through flat paper filter

1

1.20.

Filtration through a folded paper filter

1

1.21.

Handling a water vacuum pump

1

1.22.

Filtration through a Büchner funnel

1

1.23.

Suction through a glass filter

1

1.24.

Washing of precipitates by decantation

1

1.25.

Washing of precipitates on a filter

2

1.26.

Drying of precipitates on a filter with appropriate solvents

2

1.27.

Recrystallization of substances from aqueous solution

1

1.28.

Recrystallization of substances from a known organic solvent

2

1.29.

Practical choice of an appropriate solvent for recrystallization of a substance

3

1.30.

Drying of substances in a drying box

2

1.31.

Drying of substances in a desiccator

2

1.32.

Connecting and using of a gas washing bottle

2

1.33.

Extraction with an inmiscible solvent

1

2. Identification of inorganic and organic compounds:
general principles

2.1.

Test-tube reactions

1

2.2.

Technique of reactions performed in a dot dish and on a filter paper

1

2.3.

Group reactions of some cations and anions specified by the organizer

2

2.4.

Selective reactions of some cations and anions specified by the organizer

2

2.5.

Specific reactions of some cations and anions specified by the organizer

3

2.6.

Identification of elements by flame coloration (using a platinum wire/MgO rod, Co-glass)

2

2.7.

Using a hand spectroscope/Bunsen spectroscope

3

2.8.

Melting point determination with Kofler or similar type of apparatus

3

2.9.

Qualitative evidence of basic functional groups of organic substances specified by the organizer

2

2.10.

Exploitation of some specific reactions for identification of organic compounds (specified by the organizer)

3

3. Determination of some inorganic and organic compounds:
general principles

3.1.

Quantitative determinations using precipitation reactions

2

3.2.

Igniting of a precipitate in a crucible

1

3.3.

Quantitative volumetric determinations

1

3.4.

Rules at titrating

1

3.5.

Use of a pipetting ball

1

3.6.

Preparation of a standard solution

2

3.7.

Alkalimetric and acidimetric determinations

2

3.8.

Color transitions of indicators at alkalimetric and acidimetric determinations

2

3.9.

Direct and indirect determinations (back titration)

3

3.10.

Manganometric determinations

3

3.11.

Iodometric determinations

3

3.12.

Other types of determinations on basis of redox reactions

3

3.13.

Complexometric determinations

3

3.14.

Color transitions of solutions at complexometric determinations

3

3.15.

Volumetric determinations on basis of precipitation reactions

3

3.16.

Thermometric titration

3

4. Special measurements and procedures

4.1.

Measuring with a pH-meter

2

4.2.

Chromatography on thin layers

3

4.3.

Column chromatography

3

4.4.

Separation on ion exchanger

3

4.5.

Measuring of UV-VIS absorbances with a spectral photometer

3

4.6.

Performing of conductivity measurements

3

5. Evaluation of results