The hydroxide of barium, characteristics, properties and production, and chemical reactions.
Barium hydroxide is an inorganic substance and has chemical formula Ba(OH)2.
Brief description of the hydroxide of barium
Physical properties of barium hydroxide
Chemical properties of barium hydroxide
The chemical reaction of barium hydroxide
The application and use of barium hydroxide
Brief description of the hydroxide of barium:
Barium hydroxide is an inorganic substance of white color.
The chemical formula of barium hydroxide Ba(OH)2.
Has hygroscopic, but less than that of sodium hydroxide.
Highly soluble in water. It forms crystalline hydrates with one, two, seven and eight water molecules. As a result of dissolution in water forms a strongly alkaline solution. Saturated aqueous solution of hydroxide of barium called barium with water.
Soluble in ethanol. Not soluble in liquid ammonia, diethyl ether. It is soluble in acetone.
Barium hydroxide is corrosive, toxic and corrosive substance. It refers to the substances of the second class of danger. So working with them requires caution. After contact with skin, mucous membranes and eyes are serious chemical burns.
Does not burn, does not explode.
Physical properties of barium hydroxide:
| Parameter name: | Value: |
| Chemical formula | Ba(OH)2 |
| Synonyms and foreign language names | barium hydroxide (eng.)
barium hydroxide (Rus.) |
| The type of substance. | inorganic |
| Appearance | colorless monoclinic crystals |
| Color | white, colorless |
| Taste | —* |
| The smell | — |
| Aggregate state (at 20 °C and atmospheric pressure of 1 ATM.) | solid |
| Density (state of matter – solid, at 20 °C), kg/m3 | 4500 |
| Density (state of matter – solid, at 20 °C) g/cm3 | 4,5 |
| Melting point, °C | 480 |
| Boiling point, °C | 780 |
| Decomposition temperature, °C | 1000 |
| Hygroscopicity | hygroscopic |
| Molar mass, g/mol | 171,35474 |
* Note:
— no data.
Obtaining of barium hydroxide:
In the laboratory, the hydroxide of barium is obtained by the following chemical reactions:
1. the interaction of metallic barium with water:
Ba + 2H2O → Ba(OH)2 + H2.
2. the interaction of barium oxide and water:
BaO + H2O → Ba(OH)2.
3. the result of the interaction of barium sulfide with hot water:
BaS + 2H2O → Ba(OH)2+ H2S.
Chemical properties of barium hydroxide. The chemical reaction of barium hydroxide:
Hydroxide barium is a chemically active substance, the chemical basis.
Aqueous solutions of Ba(OH)2 are alkaline.
Chemical properties of barium hydroxide are similar to the properties of the hydroxides of other metals. So it is characterized by the following chemical reactions:
1. the reaction of barium hydroxide with chlorine:
6Ba(OH)2 + 6Cl2 5BaCl2 + Ba(ClO3)2 + 6H2O (to).
The reaction formed chloride of barium, chlorate of barium and water.
2. the reaction of barium hydroxide with phosphoric acid:
Ba(OH)2 + H3PO4 → BaHPO4 + 2H2O
3Ba(OH)2 + 2H3PO4 → Ba3(PO4)2 + 6H2O.
In the first case, the reaction formed gidrogenfosfat barium and water. Thus as starting materials phosphoric acid is used in concentrated solution.
In the second case, the reaction, the formed orthophosphate of barium and water. Thus as starting materials phosphoric acid is used in dilute solution.
3. the reaction of barium hydroxide with nitric acid:
Ba(OH)2 + 2HNO3 → Ba(NO3)2 + 2H2O.
The reaction produces barium nitrate and water.
Similarly, are the reaction of barium hydroxide and other acids.
4. the reaction of barium hydroxide with hydrogen sulfide:
Ba(OH)2 + H2S → BaS + 2H2O
Ba(OH)2 + 2H2S → Ba(HS)2 + 2H2O.
In the first case, the reaction, the formed barium sulfide and water. The hydrogen sulfide as a starting material is used in the form of a dilute solution.
In the second case the resulting reaction creates hydrogen sulphide of barium and water. The hydrogen sulfide as a starting material is used in the form of saturated solution.
5. the reaction of barium hydroxide with hydrogen fluoride:
Ba(OH)2 + 2HF → BaF2 + 2H2O.
In the reaction, the formed fluoride of barium and water. The hydrogen fluoride as a starting material is used in the form of saturated solution.
6. the reaction of barium hydroxide with carbon dioxide (carbon dioxide):
Ba(OH)2 + CO2 → BaCO3 + H2O
Ba(OH)2 + 2CO2 → Ba(HCO3)2.
Carbon dioxide is an acidic oxide. As a result of reaction formed in the first case, the barium carbonate and water, in the latter case, carbonate of barium and water.
7. the reaction of barium hydroxide with sulfur dioxide:
Ba(OH)2 + SO2 → BaSO3 + H2O
Ba(OH)2 + 2SO2 → Ba(HSO3)2.
Sulfur dioxide is an acidic oxide. As a result of reaction formed in the first case, the sulfite of barium and water, in the second case – the hydrogen sulphite barium.
8. the reaction of barium hydroxide with potassium chromate:
Ba(OH)2 + K2CrO4 → BaCrO4 + 2KOH.
In the reaction, the formed chromate of barium and potassium hydroxide.
9. the reaction of barium hydroxide with manganese detonator:
Ba(OH)2 + MnS2O6 → BaS2O6 + Mn(OH)2 (t = 40-70 oC).
The reaction formed ditional barium and hydroxide of manganese.
10. the reaction of barium hydroxide with ammonium chlorate:
Ba(OH)2 + 2NH4ClO3 → Ba(ClO3)2 + 2NH3 + 2H2O (to).
The reaction produces barium chlorate, ammonia and water. The barium hydroxide as a starting material is used in the form of saturated solution, and ammonium chlorate in the concentrated solution. The reaction proceeds while boiling.
11. the reaction of barium hydroxide with sodium sulfate:
Na2SO4 + Ba(OH)2 → BaSO4 + 2NaOH.
In the reaction, the formed barium sulfate and sodium hydroxide.
12. the reaction of barium hydroxide with potassium sulfate:
K2SO4 + Ba(OH)2 → BaSO4 + 2KOH.
In the reaction, the formed barium sulfate and potassium hydroxide.
13. the reaction of barium hydroxide with sodium carbonate:
Na2CO3 + Ba(OH)2 → BaCO3 + 2NaOH.
In the reaction, the formed barium carbonate and sodium hydroxide. The barium hydroxide as a starting material is used in the form of saturated solution.
Similarly, are the reaction of barium hydroxide and other salts.
14. the decomposition reaction of barium hydroxide:
Ba(OH)2 → BaO + H2O (t = 780-800 oC).
In the reaction, the formed oxide of barium and water.
The application and use of barium hydroxide:
Barium hydroxide is used:
– in the form of barium water as a reagent for SO42− and CO32− (sulfate and carbonate ions);
for purification of vegetable oils and animal fats;
– as a component of lubricants;
– to obtain barium salts and of the hydroxides of rubidium and cesium from their sulphates, and carbonates;
to remove SO42− (sulfate ions) from industrial solutions.
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