Presentation on theme: "Acids - like electrolytes". Presentation on the topic: "Acids - as electrolytes" Presentation on the use of electrolytes in medicine

"History of Medicine" - Craniotomy. Methods used in studying the history of medicine. Sources of the study of medicine in primitive society. Types of traditional medicine. Reliable coverage of the history of medicine. From the collection of T. Meyer-Steineg. Features of medicine of ancient civilizations. Types of ancient medicine. The oldest written documents.

"Computers in Medicine" - Heart rate generator (driver). Poll results. Examples of computer devices and methods of treatment and diagnosis. Breathing and anesthesia devices. What and how did we learn about the use of computers in medicine? Computer technology is used to teach practical skills to health workers. Based on the symptoms generated by the computer, the trainee must determine the course of treatment.

"Electrolysis of solutions and melts" - Chemistry. Cathode. Insoluble, simple, organic substances, oxides. Electrolytes are complex substances, melts and solutions of which conduct electric current. CuSO4 + Fe \u003d Cu + FeSO4. The process of donating electrons from ions is called oxidation. Avoid splashing electrolyte. Cu2 + is an oxidizing agent. Recovery (accession e).

"Use of resources" - Psychological and pedagogical features of the formation and use of the catalog of educational resources on the Internet. Directions for improving the Catalog 1. An increase in the list of academic disciplines, further gradation into smaller subsections 2. Introduction of additional structuring criteria (for example, combining links to resources by type - simulators, games, etc.), 3. Increasing the number of links to methodological, technological and technical manuals 4. More detailed description of teaching methods using educational resources.

"Laws of electrolysis" - Derivation of the formula. © Stolbov Yu.F., physics teacher, secondary school №156 St. Petersburg 2007. The second law of electrolysis. Electrolytic dissociation - the decomposition of a substance into ions upon dissolution. Output. Electrolysis. m \u003d kq. NaOH? Na ++ OH- HCl? H ++ Cl- CuSO4? Cu2 ++ SO42-. Definitions. k \u003d (1 / F) X F \u003d 96500C / kg X \u003d M / z. M-mass of matter q-transferred charge k-electrochemical equivalent.

"Application of electrolysis" - Application of electrolysis. Conductive. Obtaining chemically pure substances. Non-conductive. A copy of the bas-relief obtained by electroforming. 2. Electroplating. The electrochemical equivalent and the Faraday number are related by the ratio. Does not contain free charged particles (non-dissociating). Electric current in liquids.

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Dissociation of ionic compounds

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Lesson topic: "Strong and weak electrolytes"

Test your knowledge 1. Write stepwise dissociation: H 2 SO 4, H 3 PO 4, Cu (OH) 2, AlCl 3 2. The two-electron outer shell has an ion: 1) S 6+ 2) S 2- 3) Br 5+ 4) Sn 4+ 3. The number of electrons in the iron ion Fe 2+ is: 1) 54 2) 28 3) 58 4) 24 4. The same electronic configuration of the external level: have Ca 2+ and 1) K + 2) Ar 3) Ba 4) F -

substances, solutions and melts of which conduct electric current Substances Electrical conductivity Electrolytes Non-electrolytes Substances, solutions and melts of which do not conduct electric current

Ionic or strongly polar covalent bond Bases Acids Salts (solutions) Covalent non-polar or low-polarity bonds Organic compounds Gases (simple substances) Non-metals Electrolytes Non-electrolytes

The theory of electrolytic dissociation S.A. Arrhenius (1859-1927) the process of dissolution of electrolytes is accompanied by the formation of charged particles capable of conducting electric current The process of dissolution or melting of electrolytes is accompanied by the formation of charged particles capable of conducting electric current

Dissociation of ionic compounds

Dissociation of compounds with a covalent polar bond

Quantitative characteristics of the dissociation process Ratio of the number of disintegrated molecules to the total number of molecules in solution Electrolyte strength

non-electrolyte strong electrolyte weak electrolyte

Fixation 1. What is the degree of dissociation of the electrolyte, if, when dissolved in water, out of every 100 molecules into ions, the following decomposed: a) 5 molecules, b) 80 molecules? 2. In the list of substances, underline weak electrolytes: H 2 SO 4; H 2 S; CaCl 2; Ca (OH) 2; Fe (OH) 2; Al 2 (SO 4) 3; Mg 3 (PO 4) 2; H 2 SO 3; KOH, KNO 3; HCl; BaSO 4; Zn (OH) 2; CuS; Na 2 CO 3.

Acids - like electrolytes

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receiving

application

properties

IN E SCHE FROM T IN ABOUT

structure

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H Cl  H + + Cl -

H NO 3  H + + NO 3 -

CH 3 COO H  CH 3 COO + H +

H 2 SO 4  2 H + + SO 4 -2

H 3 PO 4  3 H + + PO 4 -3

Acid - electrolytes, in solutions which contain hydrogen ions

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Strong and weak acids

Strong acids

Molecules completely decay into ions

HCl H 2 SO 4 HNO 3

Weak acids

Molecules partially decay into ions

H 2 S H 2 SO 3 H 2 CO 3 CH 3 COOH

( CO 2 + H 2 O )

amount H + - acid strength

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Classification of acids

Number of hydrogen atoms

Monobasic

Multi-base

HNO 3

CH 3 COOH

Number of H atoms

H 2 SO 4

H 3 PO 4

H 2 CO 3

Acid residue charge

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The presence of oxygen in the acid residue

Oxygen-free

Oxygen-containing

H 2 S

H 2 SO 3

CH 3 COOH

Mineral acids

Organic acids

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Acid formula

Name acid

Acidic residue

Name acid residue

fluoride

F (I)

hydrofluoric

H F

H Cl

hydrochloric (hydrochloric)

Cl (I)

chloride

bromide

hydrobromic

Br (I)

H Br

H I

iodine

I (I)

iodide

sulfide

H 2 S

S (Ii)

hydrogen sulfide

sulfite

sulphurous

SO 3 (Ii)

H 2 SO 3

H 2 SO 4

sulfuric

SO 4 (Ii)

sulfate

nitrate

H NO 3

NO 3 (I)

nitric

phosphate

PO 4 (III)

phosphoric

H 3 PO 4

H 2 CO 3

coal

CO 3 (Ii)

carbonate

silicate

H 2 SiO 3

SiO 3 (Ii)

silicon

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Getting acids

Anoxic acids

H 2 + S  H 2 S

H 2 + Cl 2  2 HCl

Oxygenated acids

Acidic oxide + water

SO 2 + H 2 O  H 2 SO 3

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Acidic oxide

Corresponding acid

Acid residue in salt

H 2 O

Me SO 3 (Ii) sulfite

SO 2

H 2 SO 3

Me SO 4 (Ii) sulfate

H 2 SO 4

SO 3

Me PO 4 (Iii) phosphate

H 3 PO 4

P 4 O 10

N 2 O 5

H NO 3

Me NO 3 (I) nitrate

Me CO 3 (Ii) carbonate

CO 2

H 2 CO 3

Me SiO 3 (Ii) silicate

H 2 SiO 3

SiO 2

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sand

Physical properties of acids

Sour taste

The density is greater than the density of water

Corrosive action

Water, baking soda solution

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First water, then acid -

otherwise it will happen big trouble!

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Chemical properties of acids

Acids change the color of indicators

Indicator

Methyl orange

Litmus

Red coloring

Indicator detects the presence of ions H + in acid solution

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Acids react with metals standing in the line of activity to hydrogen

Zn + 2HCl  ZnCl 2 + H 2 

Reducing agent, oxidizes

Zn 0 - 2e  Zn +2

H +1 + 1e  H 0

Oxidizing agent, recovers

The interaction of a metal with an acid is redox reaction

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Acids react with metal oxides

Mg O + H 2 SO 4  MgSO 4 + H 2 O

Acids react with grounds

Na OH + H Cl  NaCl + H 2 O

Neutralization

Salt + water

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TOPIC TESTS

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1. Gas is released during the interaction of solutions

2) hydrochloric acid and potassium hydroxide

3) sulfuric acid and potassium sulfite

4) sodium carbonate and barium hydroxide

2. Insoluble salt is formed by interaction

1) KOH (solution) and H 3 PO 4 (solution)

2) HNO 3 (solution) and CuO

3) HC1 (solution) and Mg (NO 3) 2 (solution)

4) Ca (OH) 2 (solution) and CO 2

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3. Simultaneously can not be in the solution of the group:

1) K +, H +, NO 3 -, SO 4 2-

2) Ba 2+, Ag +, OH-, F -

3) H 3 O +, Ca 2+ Cl -, NO 3 -

4) Mg 2+, H 3 O +, Br -, Cl -

4. Which molecular equation corresponds to the reduced ionic equation

H + + OH - \u003d H 2 O?

1) ZnCl 2 + 2NaOH \u003d Zn (OH) 2 + 2NaCl

2) H 2 SO 4 + Cu (OH) 2 \u003d CuSO 4 + 2H 2 O

3) NaOH + HNO 3 \u003d NaNO 3 + H 2 O

4) H 2 SO 4 + Ba (OH) 2 \u003d BaSO 4 + 2H 2 O

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5. Gas is released during the interaction of solutions

1) potassium sulfate and nitric acid

2) hydrochloric acid and barium hydroxide

3) nitric acid and sodium sulfide

4) sodium carbonate and barium hydroxide.

6. Simultaneously can not all ions of the series are in solution

1) Fe 3+, К +, Сl -, S0 4 2-

2) Fe 3+, Na +, NO 3 -, SO 4 2-

3) Ca 2+, Li +, NO 3 -, Cl -

4) Ba 2+, Cu 2+, OH -, F -

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7. Salt and alkali are formed when solutions interact

1) А1С1 3 and NaOH

2) K 2 COz and Ba (OH) 2

3) H 3 PO 4 and KOH

4) MgBr 2 and Na 3 PO 4

8. Insoluble salt is formed when draining aqueous solutions

1) potassium hydroxide and aluminum chloride

2) copper (II) sulfate and potassium sulfide

3) sulfuric acid and lithium hydroxide

4) sodium carbonate and hydrochloric acid

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9. The precipitate will fall out when the solutions interact

1) H 3 PO 4 and KOH

2) Na 2 SO 3 and H 2 SO 4

3) FeCl 3 and Ba (OH) 2

4) Cu (NO 3) 2 and MgSO 4

10. Abbreviated ionic equation Fe 2+ + 2OH - \u003d Fe (OH) 2

corresponds to the interaction of substances:

1) Fe (NO 3) 3 and KOH

2) FeSO 4 and LiOH

3) Na 2 S and Fe (NO) 3

4) Ba (OH) 2 and FeCl 3

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11. When sodium hydroxide solution was added to a solution of an unknown salt, a colorless gelatinous precipitate was formed and then disappeared. Unknown salt formula

A1C1 3
FeCl 3
CuSO 4
KNO 3

12. Brief ionic equation

Cu 2+ + S 2- \u003d CuS corresponds to the reaction between

I) Cu (OH) 2 and H 2 S

2) CuCl 2 and Na 2 S

3) Cu 3 (P0 4) 2 and Na 2 S

4) CuCl 2 and H 2 S

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13. The products of the irreversibly proceeding ion exchange reaction not may to be

1) sulfur dioxide, water and sodium sulfate

2) calcium carbonate and sodium chloride

3) water and barium nitrate

4) sodium nitrate and potassium carbonate

14. The addition of sodium hydroxide solution to the unknown salt solution resulted in a brown precipitate. Unknown salt formula

BaC1 2
FeCl 3
CuSO 4
KNO 3

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15. Brief ionic equation

H + + OH - \u003d H 2 O corresponds to the reaction between

2) H 2 S and NaOH

3) H 2 SiO 3 and KOH

4) HC1 and Cu (OH) 2

16. Sodium chloride can be obtained in the ion exchange reaction in solution between

1) sodium hydroxide and potassium chloride

2) sodium sulfate and barium chloride

3) sodium nitrate and silver chloride

4) copper (II) chloride and sodium nitrate

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17. Products of the irreversibly proceeding ion exchange reaction can not to be

1) water and sodium phosphate

2) sodium phosphate and potassium sulfate

3) hydrogen sulfide and iron (II) chloride

4) silver chloride and sodium nitrate

18. When sodium hydroxide solution was added to the unknown salt solution, a blue precipitate formed. Unknown salt formula

1) ВаСl 2 2) FeSO 4 3) CuSO 4 4) AgNO 3

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19. Brief ionic equation of the reaction between Cu (OH) 2 and hydrochloric acid

1) H + + OH - \u003d H 2 O

2) Сu (ОН) 2 + 2Сl - \u003d CuCl 2 + 2OH -

3) Cu 2+ + 2HC1 \u003d CuCl 2 + 2H +

4) Cu (OH) 2 + 2H + \u003d Cu 2+ + 2H 2 O

20. An almost irreversible reaction between

1) K 2 SO 4 and HC1

2) NaCl and CuSO 4

3) Na 2 SO 4 and KOH

4) BaCl 2 and CuSO 4

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21. Abbreviated ionic equation

2H + + CO 3 2- \u003d CO 2 + H 2 O corresponds to the interaction

1) nitric acid with calcium carbonate

2) hydrogen sulfide acid with potassium carbonate

3) hydrochloric acid with potassium carbonate

4) calcium hydroxide with carbon monoxide (IV)

22.With the precipitation of a precipitate, a reaction occurs between the sodium hydroxide solution and

1) CrCl 2 2) Zn (OH) 2 3) H 2 SO 4 4) P 2 O 5

23. With the evolution of gas, the reaction between nitric acid and

1) Ba (OH) 2 2) Na 2 SO 4 3) CaCO 3 4) MgO

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24. Abbreviated ionic equation

СО 3 2 - + 2Н + \u003d СО 2 + Н 2 О corresponds to the interaction

5. Abbreviated ionic reaction equation

NH 4 + + OH \u003d NH 3 + H 2 O

corresponds to interaction

Na 2 CO 3 and H 2 SiO 3

Na 2 CO 3 and HCl

CaCO 3 and H 2 SO 4

NH 4 Cl and Ca (OH) 2

NH 4 Cl and Fe (OH) 2

NH 4 Cl and AgNO 3

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H 2 O + CO 2 + 2Сl - 2H + + CO 3 2- - H 2 O + CO 2 2H + + K 2 CO 3 - 2K + + H 2 O + CO 2 2К + + 2Сl - --2КС1 Podlesnaya O.N. 10/22/16 "width \u003d" 640 "

30. Brief ionic equation

Zn 2+ + 2OH - \u003d Zn (OH) 2

corresponds to the interaction of substances

zinc sulfite and ammonium hydroxide

zinc nitrate and aluminum hydroxide

zinc sulfide and sodium hydroxide

zinc sulfate and potassium hydroxide

31. The short ionic equation corresponds to the interaction of hydrochloric acid and potassium carbonate

2HCl + CO 3 2- - H 2 O + CO 2 + 2Сl -

2H + + CO 3 2- - H 2 O + CO 2

2H + + K 2 CO 3 - 2K + + H 2 O + CO 2

2K + + 2Сl - --2KS1

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32. In an aqueous solution, interaction between

Na 2 CO 3 and NaOH

Na 2 CO 3 and KNO 3

Na 2 CO 3 and KCl

Na 2 CO 3 and BaCl 2

33. The precipitate is formed by the interaction of solutions of substances:

Zn (NO 3) 2 and Na 2 SO 4

Ba (OH) 2 and NaCl

MgCl 2 and K 2 SO 4

The essence of electrolysis Electrolysis is a redox
the process that occurs on the electrodes during the passage
direct electric current through the solution or
melt of electrolytes.
To carry out electrolysis to negative
pole of external DC power supply
connect the cathode, and to the positive pole -
anode, after which they are immersed in an electrolyzer with
solution or molten electrolyte.
The electrodes are usually metal, but
non-metallic are also used, for example graphite
(conductive).

As a result of electrolysis at the electrodes (cathode and
anode) corresponding products are released
reduction and oxidation, which depending
from conditions can react with
solvent, electrode material, etc., - so
called secondary processes.
Metal anodes can be: a)
insoluble or inert (Pt, Au, Ir, graphite
or coal, etc.), during electrolysis they serve only
electron transmitters; b) soluble
(active); they are oxidized during electrolysis.

In solutions and melts of various electrolytes
there are ions of opposite sign, i.e., cations and
anions that are in chaotic motion.
But if in such an electrolyte melt, for example
melt sodium chloride NaCl, lower the electrodes and
pass a constant electric current, then cations
Na + will move to the cathode, and Cl– anions - to the anode.
The process takes place at the cathode of the electrolyzer
reduction of Na + cations by electrons of the external
current source:
Na + + e– \u003d Na0

Chlorine anions are oxidized at the anode,
moreover, the detachment of excess electrons from Cl–
carried out by the energy of an external source
current:
Cl– - e– \u003d Cl0
Released electrically neutral chlorine atoms
connect to each other, forming a molecular
chlorine: Cl + Cl \u003d Cl2, which is released at the anode.
The general equation of electrolysis of chloride melt
sodium:
2NaCl -\u003e 2Na + + 2Cl– -electrolysis-\u003e 2Na0 +
Cl20

Redox action
electric current can be many times
stronger than the action of chemical oxidants and
reducing agents. Changing the voltage to
electrodes, you can create almost any strength
oxidizing and reducing agents, which
are the electrodes of the electrolytic bath
or electrolyser.

It is known that none of the strongest chemical
the oxidizing agent cannot take away from the fluoride ion F– its
electron. But this is feasible with electrolysis,
for example, molten salt NaF. In this case, at the cathode
(reducing agent) is released from the ionic state
metallic sodium or calcium:
Na + + e– \u003d Na0
fluorine ion F– is released at the anode (oxidizer),
passing from negative ion to free
state:
F– - e– \u003d F0;
F0 + F0 \u003d F2

Products emitted on the electrodes
can enter into a chemical
interaction, therefore the anodic and cathodic
the space is divided by a diaphragm.

Practical application of electrolysis

Electrochemical processes are widely used in
various fields of modern technology, in
analytical chemistry, biochemistry, etc.
chemical industry by electrolysis
get chlorine and fluorine, alkalis, chlorates and
perchlorates, persulfuric acid and persulfates,
chemically pure hydrogen and oxygen, etc.
some substances are obtained by reduction
at the cathode (aldehydes, paraaminophenol, etc.), others
electrooxidation at the anode (chlorates, perchlorates,
potassium permanganate, etc.).

Electrolysis in hydrometallurgy is one of the
stages of processing metal-containing raw materials,
providing the production of commercial metals.
Electrolysis can be carried out with soluble
anodes - the process of electrorefining or with
insoluble - the process of electro-extraction.
The main task in the electrorefining of metals
is to ensure the required purity of the cathode
metal with acceptable energy costs.

In nonferrous metallurgy, electrolysis is used for
extraction of metals from ores and their purification.
By electrolysis of molten media,
aluminum, magnesium, titanium, zirconium, uranium, beryllium and
dr.
For refining (cleaning) metal
plates are cast from it by electrolysis and placed
them as anodes in the electrolyzer. When passing
current, the metal to be cleaned is subjected to
anodic dissolution, i.e. goes into solution in the form
cations. Then these metal cations are discharged to
cathode, due to which a compact deposit is formed
already pure metal. Impurities in the anode
either remain insoluble, or pass into
electrolyte and removed.

Electroplating - a field of applied
electrochemistry dealing with processes
metal coating on
surface of both metal and
non-metallic products when passing
direct electric current through
solutions of their salts. Electroplating
divided into electroplating and
electroforming.

Electroplating (from the Greek. To cover) is an electrodeposition on
metal surface of another metal that is durable
binds (adheres) to the covered metal (object),
serving as the cathode of the electrolyzer.
Before coating the product, its surface must be
thoroughly clean (degrease and pickle), otherwise
case, the metal will be deposited unevenly, and in addition,
adhesion (bond) of the coating metal to the surface of the product
will be fragile. Electroplating can be used to coat
detail with a thin layer of gold or silver, chrome or nickel. FROM
using electrolysis, you can apply the finest
metal coatings on various metal
surfaces. With this method of coating, the part
used as a cathode placed in a salt solution
metal to be coated. As
the anode uses a plate of the same metal.

Electroplating - obtaining by electrolysis
accurate, easily detachable metal copies
relatively considerable thickness with various
non-metallic and metallic objects,
called matrices.
Busts are made using electroplating
statues, etc.
Electroforming is used to apply
relatively thick metal coatings on
other metals (for example, the formation of "overhead"
layer of nickel, silver, gold, etc.).

English physicist and chemist, one of the founders of electrochemistry At the end of the 18th century, he gained a reputation as a good chemist. In the early years of the 19th century, Davy became interested in studying the effect of electric current on various substances, including molten salts and alkalis.

To protect metals from oxidation, as well as to give products strength and a better appearance, they are covered with a thin layer of precious metals (gold, silver) or low-oxidizing metals (chromium, nickel). The object to be galvanized is thoroughly cleaned, polished and degreased, and then immersed as a cathode in an electroplating bath. The electrolyte is a solution of the metal salt used for the coating. A plate of the same metal serves as the anode. Electroplating Plating metals with a layer of another metal using electrolysis

To give the impression of electrical conductivity, it is covered with graphite dust, immersed in a bath as a cathode, and a layer of metal of the required thickness is obtained on it. Then the wax is removed by heating.To obtain copies from metal objects (coins, medals, bas-reliefs, etc.), casts are made from some plastic material (for example, wax) Obtaining copies from objects using electrolysis Electroforming

Yakobi Boris Semenovich () - Russian physicist and inventor in the field of electrical engineering, developer of the electroforming process in the 19th century

Invented the first electric motor with direct shaft rotation Created a collector for rectifying current Invented telegraph writing apparatus Moved a boat using electrical energy Created instruments for measuring electrical resistance, made a resistance standard, designed a voltmeter

Acid Batteries The active substances of a battery are concentrated in the electrolyte and positive and negative electrodes, and the combination of these substances is called the electrochemical system. In lead-acid storage batteries, the electrolyte is a solution of sulfuric acid (H 2 SO 4), the active substance of the positive plates is lead dioxide (PbO 2), the negative plates are lead (Pb)

The relevance of electrolysis is explained by the fact that many substances are obtained in this way. Obtaining inorganic substances (hydrogen, oxygen, chlorine, alkalis, etc.). Obtaining metals (lithium, sodium, potassium, beryllium, magnesium, zinc, aluminum, copper, etc.). Cleaning of metals (copper, silver, ...) Obtaining metal alloys Obtaining electroplated coatings Treatment of metal surfaces (nitriding, boriding, electropolishing, cleaning) Obtaining organic substances Electrodialysis and water demineralization Film application using electrophoresis

Links to sources of information and images: I.I. Novoshinsky, N.S. Novoshinskaya Chemistry profile level 10 grade Primenenie-elektroliza.jpg G. Ya. Myakishev, BB Bukhovtsev N.N. Sotsky Physics Grade 10

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