Barium nitrate (Ba(NO3)2) is a white solid. It dissolves in water and forms barium and nitrate ions. It can explode when heated or mixed with combustibles.
| IUPAC name | Barium dinitrate |
| Molecular formula | Ba(NO3)2 |
| CAS number | 10022-31-8 |
| Synonyms | Barium nitrate, Bariumdinitrat, Dinitrate de baryum, CQ9625000, (nitrooxy)bario nitrate |
| InChI | InChI=1S/Ba.2NO3/c;22-1(3)4/q+2;2-1 |
Barium Nitrate Properties
Barium Nitrate Formula
The molecular formula of barium nitrate is Ba(NO3)2. It shows that one molecule of barium nitrate consists of one atom of barium and two molecules of nitrate. The nitrate ion has a charge of -1 and the barium ion has a charge of +2, so they combine in a 1:2 ratio to form a neutral compound.
Barium Nitrate Molar Mass
The molar mass of Ba(NO3)2 is 261.337 g/mol. It is the mass of one mole of Ba(NO3)2 molecules. To calculate it, we need to add the atomic masses of all the atoms in the formula:
Molar mass of Ba(NO3)2 = (1 x 137.327) + (2 x 14.007) + (6 x 15.999) = 261.337 g/mol
Barium Nitrate Boiling Point
The boiling point of Ba(NO3)2 is 83°C. It is the temperature at which Ba(NO3)2 changes from liquid to gas. However, Ba(NO3)2 decomposes before reaching its boiling point, so it is not possible to boil it without breaking it down into other substances.
Barium Nitrate Melting Point
The melting point of Ba(NO3)2 is 592°C. It is the temperature at which Ba(NO3)2 changes from solid to liquid. Ba(NO3)2 is a white crystalline solid at room temperature and pressure, but it melts when heated above its melting point.
Barium Nitrate Density g/ml
The density of Ba(NO3)2 is 3.23 g/ml. It is the mass per unit volume of Ba(NO3)2. To calculate it, we need to divide the mass of a sample of Ba(NO3)2 by its volume:
Density of Ba(NO3)2 = Mass / Volume
For example, if we have a sample of 10 g of Ba(NO3)2 and its volume is 3.1 ml, then its density is:
Density of Ba(NO3)2 = 10 / 3.1 = 3.23 g/ml
Barium Nitrate Molecular Weight
The molecular weight of Ba(NO3)2 is the same as its molar mass, which is 261.337 g/mol. It is the mass of one mole of Ba(NO3)2 molecules. Sometimes, the term molecular weight is used interchangeably with molar mass, but they are not exactly the same. Molecular weight refers to the average mass of one molecule of a substance, while molar mass refers to the mass of one mole of a substance.
Barium Nitrate Structure
The structure of Ba(NO3)2 shows how the atoms and ions are arranged in space. Ba(NO3)2 is an ionic compound, which means it consists of positively charged barium ions and negatively charged nitrate ions held together by electrostatic forces. The structure of Ba(NO3)2 can be represented by a unit cell, which is the smallest repeating unit that shows the arrangement of ions in a crystal lattice.
A unit cell of Ba(NO3)2 has a cubic shape, with one barium ion at each corner and one nitrate ion at the center of each face. The coordination number of each ion is six, which means each ion is surrounded by six oppositely charged ions. The length of each edge of the unit cell is 0.65 nm.
Barium Nitrate Solubility
The solubility of Ba(NO3)2 is the amount of Ba(NO3)2 that can dissolve in a given amount of solvent, usually water. The solubility depends on several factors, such as temperature, pressure, and the presence of other substances in the solution.
At 20°C and atmospheric pressure, the solubility of Ba(NO3)2 in water is about 34 g per 100 ml. This means that 34 g of Ba(NO3)2 can dissolve in 100 ml of water at this condition. The solubility increases with increasing temperature and decreases with increasing pressure.
Ba(NO3)2 is also soluble in other solvents, such as ethanol, acetone, and methanol, but less soluble than in water.
| Appearance | White solid |
| Specific gravity | 3.23 |
| Color | Colorless, silver, or gray |
| Odor | Odorless |
| Molar mass | 261.337 g/mol |
| Density | 3.23 g/ml |
| Melting point | 592°C |
| Boiling point | 83°C |
| Flash point | Non-flammable |
| Water solubility | 34 g per 100 ml at 20°C |
| Solubility | Soluble in ethanol, acetone, and methanol; insoluble in ether and chloroform |
| Vapour pressure | Negligible |
| Vapour density | Not applicable |
| pKa | Not applicable |
| pH | Not available |
Barium Nitrate Safety and Hazards
Ba(NO3)2 is a toxic and oxidizing substance. It can harm you if you swallow it or breathe it in. It can irritate your eyes, skin, and respiratory system. Ba(NO3)2 can also cause muscle spasms, heart problems, and death. You should avoid contact with Ba(NO3)2 and wear protective equipment when handling it. You should also keep it away from heat, sparks, flames, and combustible materials. If you get exposed to Ba(NO3)2, you should rinse your eyes and skin with water and seek medical help. You can also take sulfate salts to reduce the toxicity of barium.
| Hazard symbols | O (Oxidizing), Xn (Harmful) |
| Safety description | S13: Keep away from food, drink and animal feeding stuffs. S17: Keep away from combustible material. S22: Do not breathe dust. S26: In case of contact with eyes, rinse immediately with plenty of water and seek medical advice. S36/37/39: Wear suitable protective clothing, gloves and eye/face protection. |
| UN IDs | UN1446 |
| HS code | 2834 29 10 |
| Hazard class | 5.1 (Oxidizing substances) |
| Packing group | III |
| Toxicity | LD50 (oral, rat) = 355 mg/kg; LC50 (inhalation, rat) = 0.15 mg/L/4h |
Barium Nitrate Synthesis Methods
Different methods can be used to create Ba(NO3)2, which is a white solid substance.
One method is to react barium carbonate with nitric acid. This produces Ba(NO3)2 and carbon dioxide. Filter the Ba(NO3)2 solution to remove any iron impurities, then evaporate it to obtain solid crystals.
Another method is to react barium sulfide with nitric acid. This produces Ba(NO3)2 and hydrogen sulfide. To purify and crystallize the Ba(NO3)2 solution, we follow the same process as before.
A third method is to dissolve barium metal or barium oxide in nitric acid. This produces Ba(NO3)2 and hydrogen or water. The solution containing Ba(NO3)2 is then concentrated and undergoes crystallization.
A fourth method is to use molten salt synthesis. This involves heating a mixture of Ba(NO3)2 and an inorganic vesicant, such as ammonium chloride, sodium bicarbonate, or sodium nitrite. The vesicant decomposes and creates pores in the Ba(NO3)2 crystals. This makes them more reliable as a pyrotechnic oxidizers.
These are some of the methods to synthesize Ba(NO3)2. They all use nitric acid as a common reactant and produce Ba(NO3)2 as a product.
Barium Nitrate Uses
Some of the uses of Ba(NO3)2 are:
- Barium oxide compounds – Used in the production of barium oxide-containing materials, such as ceramics, glass, and cathode ray tubes.
- Green Flame – Used in green signal lights and fireworks, as it burns with a green flame due to the emission of barium ions.
- Rodenticide – Used as a rodenticide to kill rats and mice, as it is toxic to them.
- Oxidizer – Used in detonators and explosives, it is a strong oxidizer and can enhance the combustion of other substances.
- Primer – Used in primers and tracer bullets, as it provides ignition and visibility to the ammunition.
- Pigment – Used in the making of paints and pigments, as it can impart a white or green color to them.
- Oxidizing agent – Used as an oxidizing agent in various chemical reactions, such as the synthesis of barium peroxide and barium hydroxide.
- Explosives – Used in making explosives such as Baratol, which is a mixture of Ba(NO3)2, TNT, and binder.
Questions:
Q: Is barium nitrate soluble?
A: Ba(NO3)2 is soluble in water and some other solvents, such as ethanol, acetone, and methanol.
Q: Is barium nitrate useful for concrete?
A: Ba(NO3)2 is not useful for concrete, as it can cause corrosion of steel reinforcement and cracking of concrete.
Q: Will a precipitate form if solutions of potassium sulfate and barium nitrate are combined?
A: Yes, a precipitate of barium sulfate (BaSO4) will form if solutions of potassium sulfate (K2SO4) and barium nitrate (Ba(NO3)2) are combined.
Q: Barium nitrate has the formula Ba(NO3)2. Which statement is true about barium nitrate?
A: A possible true statement is: Ba(NO3)2 is an ionic compound that consists of one barium ion and two nitrate ions.
Q: Is barium nitrate volatile?
A: No, Ba(NO3)2 is not volatile, as it has a high melting point and decomposes before boiling.
Q: Is barium nitrate neutral?
A: No, Ba(NO3)2 is not neutral, as it is an acidic salt that can lower the pH of a solution.
Q: What is produced during the replacement reaction of Ba(NO3)2 and Na2SO4?
A: NaNO3 and BaSO4 are produced during the replacement reaction of Ba(NO3)2 and Na2SO4.
Q: Is Ba(NO3)2 soluble in water?
A: Yes, Ba(NO3)2 is soluble in water, as it dissolves to form barium ions and nitrate ions.
Q: What is the net ionic equation of the reaction of MgSO4 with Ba(NO3)2?
A: The net ionic equation of the reaction of MgSO4 with Ba(NO3)2 is:
Ba2+ + SO42- → BaSO4
Q: What is the number of moles in 432 g Ba(NO3)2?
A: The number of moles in 432 g Ba(NO3)2 is:
n = m / M, n = 432 / 261.337, n = 1.653 moles
Q: Is Ba(NO3)2 soluble?
A: Yes, Ba(NO3)2 is soluble, as it dissolves to form barium ions and nitrate ions.