Do we know everything about salt? Research paper "Where does salt go when dissolved in water?" The white salt was dissolved in water.

To determine the qualitative composition of an unknown white crystalline substance, a potassium hydroxide solution was added to its solution. Wherein

a precipitate formed. Barium nitrate solution was added to the other part of the test substance solution. The formation of an acid-insoluble white precipitate was observed.
It is known that the metal cation contained in this compound is also part of chlorophyll, and the metal itself was previously used in photography to obtain flash.
Determine the composition and write down the name of the starting material. Write down two reaction equations that were carried out in the process of determining the qualitative composition of an unknown substance.

To demonstrate the genetic relationship between non-metal compounds, the teacher used a simple substance X - a red powder, without metallic

gloss and non-conductive. When burned in air, a white crystalline substance is formed, which dissolves well in water. The resulting solution was divided into two parts and indicators were added: the color of phenolphthalein did not change, and the purple litmus turned red. What substance did the teacher use for the demonstration experiment? Make the equations for the reactions described. ACCORDING TO EQUATION # 2 Calculate the mass of the product formed if 71 g of a white crystalline substance, readily soluble in water, was taken for the reaction.

ГИА-9-2011, С3 To establish the qualitative composition of the unknown substance, the schoolchildren were given a metal salt, which is part of the

meteorites and has pronounced magnetic properties. The students dissolved the brown crystals of this salt in water, then the resulting yellow-brown solution was poured into two test tubes. Potassium hydroxide solution was added to one of them, and a brown precipitate was formed. A solution of silver nitrate was poured into the other, resulting in a white "curdled" precipitate. Write down the chemical formula and name of the unknown salt. Make two molecular equations of the reactions that were carried out in the process of its recognition.

To determine the qualitative composition of an unknown colorless gas with an unpleasant odor, part of it was absorbed with a barium hydroxide solution. When pom dropped b

white precipitate, soluble in acids. The other part was heated with hydrogen sulfide. In this case, the formation of a substance with a wife of color, insoluble in water, was observed. Write down the chemical formula and name of the given substance. Make two equations of the reactions that were carried out in the process of studying its properties.

About salt mia!

We were not mistaken in mentioning the famous Italian song "My sun!": Many peoples of the world have the words "salt" and "sun" of the same root. Salt is mentioned in the Bible about 30 times, from there the expression "salt of life" came to us.
Salt symbolized wealth and power, protected from evil forces: ancient rulers often sat on a throne of salt. Many traditions have remained from those distant times. Russians greet "high" guests with bread and salt. The Sabbath Jews wash their hands, break bread and dip it in a salt shaker, distributing it to the whole family. On the tables of many peoples, out of habit to this day, there is a salt shaker, because before food was cooked without salt, but was salted on the table. And a boring, uninteresting life or a person is still called the word "insipid", the opposite in meaning "salty".

Do we know everything about salt?

Salt or sodium chloride is a naturally occurring white crystalline mineral; dissolves in water; one of the few minerals that humans eat. Salt is the oldest spice.
For centuries, salt has been a valuable commodity. Because of salt, wars were fought, states were formed and destroyed. At the end of the Roman era and throughout the Middle Ages, salt was a valuable commodity that was transported along the "Salt Roads" to the center of the Germanic tribes. The cities, states and principalities, through which the "salt road" passed, imposed huge taxes on merchants for the transport of salt through their territory. This marked the beginning of wars, and even became the reason for the founding of some cities, for example, Munich in 1158.

No one will argue that salt is a basic necessity.

Its human body contains 300 g.

This stock is consumed every day, and it must be replenished every day.

Do not assume that salt is only necessary for the taste of food. It serves as the material from which hydrochloric acid is formed in the stomach.

Thanks to this acid, food is digested and microbes die. In addition, salt saves us from dehydration by retaining moisture in the body.

Now salt is generally available and we do not appreciate it, but it was not always like this. In the old days, real wars broke out because of salt, taxes were paid with it, and peasant riots were extinguished by distributing salt.

In China, they even made money from salt. To do this, the brine was boiled until thick, until it took the form of a dough. Then they made pies from this "dough", put the emperor's stamp on them and dried them.

Salt has had a profound effect on different languages. The greatest influence occurred in the languages interacting with the Romance and Greek civilizations while salt was in value.
Roman soldiers were given permission to purchase salt (in Latin: sal), salarium argentum, from which the English word salary ( wage). The Romans also preferred to salt greens, with the result that the Latin word for salt was included in the new word salad. In barbarian Latin salata meant "salty".

In countries where there were no deposits of salt, it was mined in some intricate way. For example, Miklouho-Maclay wrote that the Papuans collected pieces of wood that had lain in sea water for a long time, burned them and ate salted ash.

Salt is obtained in two ways: by mining and by evaporation of sea water.

Chemical composition different types the salts are the same - 99% sodium chloride - but the structure of the crystals changes greatly. Ordinary table salt consists of small kranul, kosher salt is much more uneven in structure, coarser. For popcorn, salt is used, which dissolves easily. Rock salt is large chunks of the mineral, sodium chloride. The difference in shape and structure allows for different flavors and is useful for different dishes. The rate at which it dissolves is also very important, and the salting salt must be very fine to dissolve even in cold liquid.

Sea salt, which is made from sea water, also comes in different varieties. Due to the substances in the water, sea salt has a unique taste that is used in many cuisines.

ROCK SALT. This species is probably the most popular and widespread. Solid salt deposits are found in many regions of the world, where they occur at depths ranging from a few hundred to over a thousand meters. Special harvesters chop salt underground and it is transported to the surface of the earth by conveyors.

There it gets into mills and crumbles to obtain particles (crystals) of various sizes. The coarser salt is used mainly for industrial purposes, the finer salt is used for food. Rock salt is distinguished by the lowest content of impurities, low humidity and the highest sodium chloride content - up to 99%. This means that it will be more saturated than others.

GARDEN SALT is formed by natural evaporation of salt in water bodies. From the lessons of geography, everyone remembers the famous salt lakes in the Astrakhan region Elton and Baskunchak.

Special harvesters (harvesters) remove a layer of salt on dried up lakes and send it along a conveyor for crushing, washing, drying and further processing. The salt contains more impurities (clay, sand), and the mass fraction of sodium chloride can be 95-96% (because of this, it often has a grayish appearance).

VACUUM VAPORIZED SALT. Where the salt is very deep, it is extracted by the dissolution method. A pipe is placed in the salt layer and fresh water is pumped into it under high pressure, which dissolves the salt, forming cavities in the deposit. Then the concentrated brine is raised through pipes to the surface, where it is processed and evaporated under vacuum in vats to obtain a highly purified product.

Sometimes the brine raised to the surface is evaporated under the sun in open containers. Salt in deposits is often very clean and requires only minor additional treatment.

Evaporated salt is the most expensive and at the same time the most chemically pure and high quality. In our country, it is sold under the Extra brand.

Evaporator is also rich in sodium. Therefore, the hostess should pay attention to what salt she uses, and from here calculate its amount.

Since salt is a food that we eat every day in approximately the same quantities, it is increasingly used as a carrier of trace elements. Salt is enriched mainly with iodine and fluorine.

For example, 60% of the salt sold in Germany and 80% of the salt sold in Switzerland are fortified with fluorine. This salt is used for the prevention of dental diseases. Agree that the effect of the toothpaste is much less, its action is local and very short-term.

In countries where iodine deficiency is observed, iodine-fortified salt is produced. In our body, such salt quickly decomposes and releases iodine, which the thyroid gland needs to synthesize thyroid hormones. The use of such salt in an amount of 5-6 g per day fully satisfies the body's need for iodine.

Today the problem of iodine deficiency is very acute. First of all, due to the sheer number of people it affects, and possible consequences for individuals and society. In Russia, for example, 98 million people are susceptible to iodine deficiency, of which more than half are children, adolescents and pregnant women.

Lack of iodine in the diet leads to irreversible changes in the nervous system. Due to damage to the central nervous system in children in areas with low iodine intake, mental retardation develops - one of the most severe manifestations of iodine deficiency.

Salt is our main seasoning, and it is necessary for humans, since its natural amount in water and food is not enough for our body.
Do not forget that a person's needs for table salt depend on energy consumption, climatic conditions, etc. With increased physical activity, a person loses up to 20 grams of salt per day, therefore, in a temperate climate, salt consumption is 10-15 grams per day.

Please note that lack or lack of salt impairs the taste of food. If a person does not receive table salt for a long time, it can cause dizziness, fainting, weakness and other painful phenomena. Excess salt is no less harmful.

Make sure that the taste of the salt is purely salty, without any foreign aftertaste, and odorless. The color of the salt (extra) is pure white. For other varieties, shades are allowed: grayish, yellowish and pinkish. There should be no contamination visible to the eye.

Store salt in a dry place with relatively high humidity. At lower humidity, it gives off moisture to the external environment, i.e. dries up, and at a higher level it is moisturized. Salt is capable of caking, loses its flowability, and fine salt is stronger, coarse salt is weaker. Raw salt cakes more strongly than dry salt.

Iodized salt, containing potassium iodide, oxidizes in the presence of moisture, air and light, releasing iodine, which then evaporates. There is always moisture in table salt and in the air, which promotes the decomposition of potassium iodide. As iodized salt is stored, the iodine content gradually decreases. Store it in a dry place in a sealed container. After six months, it is considered normal food.

Known deposits

* Artyomovskoye field is the largest in Europe. Extraction in the mine of the Artyomsol State Production Association.
* Baskunchakskoye field, production from the lake Bassol OJSC. For the export of salt, the Baskunchak Railway
* Iletskoye deposit, production at the mine of OJSC "Iletsksol"
* Odessa estuaries (production was carried out from 1774 to 1931)
* Elton field Elton

Interesting Facts

* Ordinary table salt can be the strongest poison. On the one hand, it is impossible to live without salt, on the other hand, a dose 10 times higher than usual is lethal. The lethal dose is 3000 milligrams per kilogram of body weight. In other words, for a person weighing 80 kg, you need to use a quarter of a kilogram pack.

* In countries with a cold climate, the daily norm required by the body is much lower than in countries with a hot climate, due to different sweating. Average daily intake for an adult: 3-5 grams of salt in cold countries and up to 20 grams in hot ones.

* In stores, salt consists of up to 97% of NaCl, the rest is accounted for by various impurities. Iodates and carbonates are most often added; in recent years, fluorides have been added more and more often. For the prevention of dental diseases, use salt with fluoride. Since the 1950s, fluoride has been added to salt in Switzerland, and thanks to positive results In the 1980s, fluoride began to be added to salt in the fight against tooth decay in France and Germany. Up to 60% of the salt sold in Germany and up to 80% in Switzerland is salt with fluorides.

* The systematic intake of excess salt in comparison with the physiological norm leads to an increase in blood pressure. Excessive salt intake causes heart and kidney disease.

* In Russia in the 17th century, the Salt Riot took place, caused by the prohibitively high prices for salt.

Alkali metals react easily with non-metals:

2K + I 2 = 2KI

2Na + H 2 = 2NaH

6Li + N 2 = 2Li 3 N (the reaction proceeds already at room temperature)

2Na + S = Na 2 S

2Na + 2C = Na 2 C 2

In reactions with oxygen, each alkali metal shows its individuality: when burning in air, lithium forms an oxide, sodium - peroxide, potassium - superoxide.

4Li + O 2 = 2Li 2 O

2Na + O 2 = Na 2 O 2

K + O 2 = KO 2

Obtaining sodium oxide:

10Na + 2NaNO 3 = 6Na 2 O + N 2

2Na + Na 2 O 2 = 2Na 2 O

2Na + 2NaOH = 2Na 2 O + H 2

Interaction with water leads to the formation of alkali and hydrogen.

2Na + 2H 2 O = 2NaOH + H 2

Interaction with acids:

2Na + 2HCl = 2NaCl + H 2

8Na + 5H 2 SO 4 (conc.) = 4Na 2 SO 4 + H 2 S + 4H 2 O

2Li + 3H 2 SO 4 (conc.) = 2LiHSO 4 + SO 2 + 2H 2 O

8Na + 10HNO 3 = 8NaNO 3 + NH 4 NO 3 + 3H 2 O

When interacting with ammonia, amides and hydrogen are formed:

2Li + 2NH 3 = 2LiNH 2 + H 2

Interaction with organic compounds:

Н ─ C ≡ С ─ Н + 2Na → Na ─ C≡C ─ Na + H 2

2CH 3 Cl + 2Na → C 2 H 6 + 2NaCl

2C 6 H 5 OH + 2Na → 2C 6 H 5 ONa + H 2

2CH 3 OH + 2Na → 2 CH 3 ONa + H 2

2CH 3 COOH + 2Na → 2CH 3 COOONa + H 2

A qualitative reaction to alkali metals is the coloring of the flame with their cations. The Li + ion colors the flame in carmine red, the Na + ion - in yellow, K + - in purple

Alkali metal compounds

Oxides.

Alkali metal oxides are typical basic oxides. Reacts with acidic and amphoteric oxides, acids, water.

3Na 2 O + P 2 O 5 = 2Na 3 PO 4

Na 2 O + Al 2 O 3 = 2NaAlO 2

Na 2 O + 2HCl = 2NaCl + H 2 O

Na 2 O + 2H + = 2Na + + H 2 O

Na 2 O + H 2 O = 2NaOH

Peroxides.

2Na 2 O 2 + CO 2 = 2Na 2 CO 3 + O 2

Na 2 O 2 + CO = Na 2 CO 3

Na 2 O 2 + SO 2 = Na 2 SO 4

2Na 2 O + O 2 = 2Na 2 O 2

Na 2 O + NO + NO 2 = 2NaNO 2

2Na 2 O 2 = 2Na 2 O + O 2

Na 2 O 2 + 2H 2 O (cold) = 2NaOH + H 2 O 2

2Na 2 O 2 + 2H 2 O (hot) = 4NaOH + O 2

Na 2 O 2 + 2HCl = 2NaCl + H 2 O 2

2Na 2 O 2 + 2H 2 SO 4 (decompression) = 2Na 2 SO 4 + 2H 2 O + O 2

2Na 2 O 2 + S = Na 2 SO 3 + Na 2 O

5Na 2 O 2 + 8H 2 SO 4 + 2KMnO 4 = 5O 2 + 2MnSO 4 + 8H 2 O + 5Na 2 SO 4 + K 2 SO 4

Na 2 O 2 + 2H 2 SO 4 + 2NaI = I 2 + 2Na 2 SO 4 + 2H 2 O

Na 2 O 2 + 2H 2 SO 4 + 2FeSO 4 = Fe 2 (SO 4) 3 + Na 2 SO 4 + 2H 2 O

3Na 2 O 2 + 2Na 3 = 2Na 2 CrO 4 + 8NaOH + 2H 2 O

Bases (alkalis).

2NaOH (excess) + CO 2 = Na 2 CO 3 + H 2 O

NaOH + CO 2 (excess) = NaHCO 3

SO 2 + 2NaOH (excess) = Na 2 SO 3 + H 2 O

SiO 2 + 2NaOH Na 2 SiO 3 + H 2 O

2NaOH + Al 2 O 3 2NaAlO 2 + H 2 O

2NaOH + Al 2 O 3 + 3H 2 O = 2Na

NaOH + Al (OH) 3 = Na

2NaOH + 2Al + 6H 2 O = 2Na + 3H 2

2KOH + 2NO 2 + O 2 = 2KNO 3 + H 2 O

KOH + KHCO 3 = K 2 CO 3 + H 2 O

2NaOH + Si + H 2 O = Na 2 SiO 3 + H 2

3KOH + P 4 + 3H 2 O = 3KH 2 PO 2 + PH 3

2KOH (cold) + Cl 2 = KClO + KCl + H 2 O

6KOH (hot) + 3Cl 2 = KClO 3 + 5KCl + 3H 2 O

6NaOH + 3S = 2Na 2 S + Na 2 SO 3 + 3H 2 O

2NaNO 3 2NaNO 2 + O 2

NaHCO 3 + HNO 3 = NaNO 3 + CO 2 + H 2 O

NaI → Na + + I -

at the cathode: 2H 2 O + 2e → H 2 + 2OH - 1

at the anode: 2I - - 2e → I 2 1

2H 2 O + 2I - H 2 + 2OH - + I 2

2H 2 O + 2NaI H 2 + 2NaOH + I 2

2NaCl 2Na + Cl 2

at the cathode at the anode

KNO 3 + 4Mg + 6H 2 O = NH 3 + 4Mg (OH) 2 + KOH

4KClO 3 KCl + 3KClO 4

2KClO 3 2KCl + 3O 2

KClO 3 + 6HCl = KCl + 3Cl 2 + 3H 2 O

Na 2 SO 3 + S = Na 2 S 2 O 3

Na 2 S 2 O 3 + H 2 SO 4 = Na 2 SO 4 + S ↓ + SO 2 + H 2 O

2NaI + Br 2 = 2NaBr + I 2

2NaBr + Cl 2 = 2NaCl + Br 2

I A group.

1. Electric discharges were passed over the surface of the caustic soda solution poured into the flask, while the air in the flask turned brown, which disappears after a while. The resulting solution was carefully evaporated and the solid residue was found to be a mixture of two salts. When this mixture is heated, gas is released and only one substance remains. Write down the equations for the reactions described.

2. The substance released at the cathode during the electrolysis of the sodium chloride melt was burned in oxygen. The resulting product was placed in a gas meter filled with carbon dioxide. The resulting substance was added to the ammonium chloride solution and the solution was heated. Write down the equations for the reactions described.

3) The nitric acid was neutralized with baking soda, the neutral solution was carefully evaporated and the residue was calcined. The resulting substance was introduced into a solution of potassium permanganate acidified with sulfuric acid, and the solution became discolored. The nitrogen-containing reaction product was placed in a sodium hydroxide solution and zinc dust was added, while a gas with a pungent odor was released. Write down the equations for the reactions described.

4) The substance obtained at the anode during the electrolysis of a sodium iodide solution with inert electrodes was introduced into a reaction with potassium. The reaction product was heated with concentrated sulfuric acid, and the evolved gas was passed through a hot potassium chromate solution. Write the equations of the described reactions

5) The substance obtained at the cathode during the electrolysis of sodium chloride melt was burned in oxygen. The obtained product was sequentially treated with sulfur dioxide and barium hydroxide solution. Write the equations of the described reactions

6) White phosphorus dissolves in a solution of caustic potassium with the release of a gas with a garlic odor, which spontaneously ignites in air. The solid product of the combustion reaction reacted with sodium hydroxide in such a ratio that the resulting white substance contains one hydrogen atom; when the latter is ignited, sodium pyrophosphate is formed. Write the equations of the described reactions

7) Unknown metal burned in oxygen. The reaction product, interacts with carbon dioxide, forms two substances: a solid, which interacts with a hydrochloric acid solution with the release of carbon dioxide, and a gaseous simple substance that supports combustion. Write down the equations for the reactions described.

8) A brown gas was passed through an excess of potassium hydroxide solution in the presence of a large excess of air. Magnesium shavings were added to the resulting solution and heated, nitric acid was neutralized with the released gas. The resulting solution was carefully evaporated, and the solid product was calcined. Write down the equations for the reactions described.

9) During the thermal decomposition of salt A in the presence of manganese dioxide, a binary salt B and a gas that supports combustion and is part of the air were formed; when this salt is heated without a catalyst, salt B and a salt of a higher oxygen-containing acid are formed. When salt A interacts with hydrochloric acid, a yellow-green gas (a simple substance) is released and salt B is formed. Salt B colors the flame purple; when it interacts with a solution of silver nitrate, a white precipitate is formed. Write down the equations for the reactions described.

10) Copper shavings were added to heated concentrated sulfuric acid and the released gas was passed through a solution of sodium hydroxide (excess). The reaction product was isolated, dissolved in water and heated with sulfur, which was dissolved as a result of the reaction. Dilute sulfuric acid was added to the resulting solution. Write down the equations for the reactions described.

11) Table salt was treated with concentrated sulfuric acid. The resulting salt was treated with sodium hydroxide. The resulting product was calcined with an excess of coal. The gas released in this case reacted in the presence of a catalyst with chlorine. Write down the equations for the reactions described.

12) Sodium reacted with hydrogen. The reaction product was dissolved in water, while a gas was formed that reacted with chlorine, and the resulting solution, when heated, reacted with chlorine to form a mixture of two salts. Write down the equations for the reactions described.

13) Sodium was burned in an excess of oxygen, the resulting crystalline substance was placed in a glass tube and carbon dioxide was passed through it. The gas exiting the tube was collected and phosphorus was burned in its atmosphere. The resulting substance was neutralized with an excess of sodium hydroxide solution. Write down the equations for the reactions described.

14) To the solution obtained as a result of the interaction of sodium peroxide with water upon heating, a solution of hydrochloric acid was added until the end of the reaction. The solution of the formed salt was subjected to electrolysis with inert electrodes. The gas formed as a result of electrolysis at the anode was passed through a suspension of calcium hydroxide. Write down the equations for the reactions described.

15) Sulfur dioxide was passed through the sodium hydroxide solution until a medium salt was formed. An aqueous solution of potassium permanganate was added to the resulting solution. The formed precipitate was separated and acted on with hydrochloric acid. The evolved gas was passed through a cold potassium hydroxide solution. Write down the equations for the reactions described.

16) A mixture of silicon oxide (IV) and metallic magnesium was calcined. The simple substance obtained as a result of the reaction was treated with a concentrated solution of sodium hydroxide. The evolved gas was passed over heated sodium. The resulting substance was placed in water. Write down the equations for the reactions described.

17) The product of the interaction of lithium with nitrogen was treated with water. The resulting gas was passed through a sulfuric acid solution until the termination of chemical reactions. The resulting solution was treated with a barium chloride solution. The solution was filtered and the filtrate was mixed with sodium nitrate solution and heated. Write down the equations for the reactions described.

18) Sodium was heated in a hydrogen atmosphere. On adding water to the obtained substance, gas evolution and the formation of a clear solution were observed. A brown gas was passed through this solution, which was obtained as a result of the interaction of copper with a concentrated solution of nitric acid. Write down the equations for the reactions described.

19) Sodium hydrogen carbonate was calcined. The resulting salt was dissolved in water and mixed with an aluminum solution, as a result of which a precipitate formed and a colorless gas evolved. The precipitate was treated with an excess of nitric acid solution, and the gas was passed through a potassium silicate solution. Write down the equations for the reactions described.

20) Sodium was fused with sulfur. The resulting compound was treated with hydrochloric acid, the released gas completely reacted with sulfur oxide (IV). The resulting material was treated with concentrated nitric acid. Write down the equations for the reactions described.

21) Sodium was burned in excess of oxygen. The resulting substance was treated with water. The resulting mixture was boiled, after which chlorine was added to the hot solution. Write down the equations for the reactions described.

22) Potassium was heated under nitrogen atmosphere. The resulting substance was treated with an excess of hydrochloric acid, after which a suspension of calcium hydroxide was added to the resulting mixture of salts and heated. The resulting gas was passed radially with hot copper (II) oxide. Write down the equations of the described reactions.

23) Potassium was burned in a chlorine atmosphere, the resulting salt was treated with an excess of an aqueous solution of silver nitrate. The formed precipitate was filtered off, the filtrate was evaporated and heated carefully. The resulting salt was treated with an aqueous solution of bromine. Write down the equations for the reactions described.

24) Lithium reacted with hydrogen. The reaction product was dissolved in water, and a gas was formed that reacted with bromine, and the resulting solution, when heated, reacted with chlorine to form a mixture of two salts. Write down the equations for the reactions described.

25) Sodium was burned in air. The resulting solid absorbs carbon dioxide, releasing oxygen and salt. The latter salt was dissolved in hydrochloric acid, and a solution of silver nitrate was added to the resulting solution. This resulted in a white precipitate. Write down the equations for the reactions described.

26) Oxygen was exposed to an electric discharge in an ozonizer. The resulting gas was passed through an aqueous solution of potassium iodide, while a new colorless and odorless gas was released, supporting combustion and respiration. In an atmosphere of the latter gas, sodium was burned, and the resulting solid was reacted with carbon dioxide. Write down the equations for the reactions described.

I A group.

1.N 2 + O 2 2NO

2NO + O 2 = 2NO 2

2NO 2 + 2NaOH = NaNO 3 + NaNO 2 + H 2 O

2NaNO 3 2NaNO 2 + O 2

2.2NaCl 2Na + Cl 2

at the cathode at the anode

2Na + O 2 = Na 2 O 2

2Na 2 O 2 + 2CO 2 = 2Na 2 CO 3 + O 2

Na 2 CO 3 + 2NH 4 Cl = 2NaCl + CO 2 + 2NH 3 + H 2 O

3. NaHCO 3 + HNO 3 = NaNO 3 + CO 2 + H 2 O

2NaNO 3 2NaNO 2 + O 2

5NaNO 2 + 2KMnO 4 + 3H 2 SO 4 = 5NaNO 3 + 2MnSO 4 + K 2 SO 4 + 3H 2 O

NaNO 3 + 4Zn + 7NaOH + 6H 2 O = 4Na 2 + NH 3

4.2H 2 O + 2NaI H 2 + 2NaOH + I 2

2K + I 2 = 2KI

8KI + 5H 2 SO 4 (conc.) = 4K 2 SO 4 + H 2 S + 4I 2 + 4H 2 O

3H 2 S + 2K 2 CrO 4 + 2H 2 O = 2Cr (OH) 3 ↓ + 3S ↓ + 4KOH

5.2NaCl 2Na + Cl 2

at the cathode at the anode

2Na + O 2 = Na 2 O 2

Na 2 O 2 + SO 2 = Na 2 SO 4

Na 2 SO 4 + Ba (OH) 2 = BaSO 4 ↓ + 2NaOH

6.P 4 + 3KOH + 3H 2 O = 3KH 2 PO 2 + PH 3

2PH 3 + 4O 2 = P 2 O 5 + 3H 2 O

P 2 O 5 + 4NaOH = 2Na 2 HPO 4 + H 2 O

2Na 2 HPO 4 Na 4 P 2 O 7 + H 2 O

Job catalog.
Tasks 22. Chemical properties of simple and complex substances

Version for printing and copying in MS Word

Substances are given:,.

Using water and the necessary substances only from this list, get iron (II) hydroxide in two stages. Describe the signs of the reactions being carried out. For an ion exchange reaction, write the abbreviated ionic reaction equation.

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Substances are given:. Using water and the necessary substances only from this list, get manganese (II) hydroxide in two stages. Describe the signs of the reactions being carried out. For an ion exchange reaction, write the abbreviated ionic reaction equation.

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