A salt made of ions of Barium as well as Nitrate is known as Barium Nitrate. It exists naturally as the incredibly uncommon mineral nitrobarite. As an oxidant, barium nitrate interacts violently with common reducing compounds. 2 parts of nitrate & 1 part of barium are combined to create the chemical known as barium nitrate. Barium nitrate's molecular formula is thus represented as $\mathrm{Ba(NO_{3})_{2}}$.
An inorganic chemical called barium nitrate is sometimes referred to as barium dinitrate, Nitrobarite, or even barium salt. Barium salt is typically found as a white, crystalline substance. The substance is inherently incombustible. However, it burns with a green flame when used as an oxidizer and can explode if exposed to flame for a prolonged period.
Structure
One Barium cation $\mathrm{Ba^{2+}}$ and 2 nitrate anions $\mathrm{NO_{3}^{-}}$ to form. Moreover, the crystal structure is cubic with 1 barium cation surrounded by 4 nitrate anions.
| Properties | Barium Nitrate |
|---|---|
| Molecular Weight | 261.37 g/mol |
| Appearance | Crystalline solid |
| Colour | White |
| Combustibility | Non-combustible |
| Melting Point | 590 $\mathrm{^{\circ}C}$ |
| Odour | Odourless |
| Boiling point | 83 $\mathrm{^{\circ}C}$ |
| IUPAC Name | Barium(2+) dinitrate |
| Refractive Index | 1.5659 |
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It is a very powerful oxidising agent that reacts violently with metals. Barium nitrate is frequently used for military purposes since it contains a significant amount of nitrate. For instance, it is used to create explosives such as grenades. Despite not being combustible itself, it improves the combustibility of other compounds. Barium nitrate should not be exposed to intense heat for an extended period since it may explode or provide a fire danger. Additionally, it serves as an oxidising agent for many chemical processes; this ability has a range of uses.
It may split down or decompose at high temperatures to produce Barium Oxide and Nitrogen Dioxide.
$$\mathrm{2\:Ba(NO_{3})_{2}\to 2\:BaO\:+\:4NO_{2}\:+\:O_{2}}$$
Barium carbonate is initially dissolved in $\mathrm{HNO_{3}}$. Iron impurities precipitate to the surface as these chemicals react. You must eliminate these contaminants using the filtration procedure. The leftover mixture must then be evaporated after that. After crystallisation, we finally obtain pure $\mathrm{Ba(NO_{3})_{2}}$, which is frequently used in industry.
$$\mathrm{BaCO_{3}\:+\:2HNO_{3}\to Ba(NO_{3})_{2}\:+\:CO_{2}\:+\:H_{2}O}$$
The first step in the preparation of barium nitrate is either the reaction of $\mathrm{HNO_{3}}$ and $\mathrm{Ba}$ or $\mathrm{HNO_{3}}$ and $\mathrm{BaO}$.
$$\mathrm{2HNO_{3}\:+\: Ba\to Ba(NO_{3})_{2}\:+\:H_{2}}$$
$$\mathrm{2HNO_{3}\:+\: BaO\:\to\: Ba(NO_{3})_{2}\:+\:H_{2}O}$$
This substance can be severely harmful to humans in high doses. Be careful not to breathe in too many of its fumes. Several hazardous symptoms can also result from direct exposure to the skin & eyes. Some symptoms of barium nitrate poisoning include upper lung inflammation, skin irritation, & eye irritation. Notably, they are easily avoidable by using basic safety precautions when handling them.
Some of these major uses are discussed below in detail.
The home's wall paints are just a combination of different chemical compounds. One of these substances is barium nitrate. Notably, because it is frequently utilised as a fundamental component, the majority of paintings would not exist without this specific barium nitrate.
A primary element in the production of premium glass products is barium nitrate. The oxygen molecule that is connected to this substance can aid in preventing the discolouration of glass objects. Such glassware is also incredibly transparent. When making optical glasses, experts also employ this substance. Clearer images can be obtained by using barium nitrate in camera lenses to increase the refractive index.
Because it can aid in the creation of green flames, barium nitrate is a prized substance in the fireworks industry. One can detect the usage of this substance in a variety of pyrotechnic displays, in addition to fireworks. Similar to how barium nitrate produces green flames, sodium chloride produces yellow flames, while copper chloride burns with a blue flame. As a result, fireworks frequently combine all of these.
Making tracer bullets is aided by barium nitrate. Thanks to a $\mathrm{Ba(NO_{3})_{2}}$, charge put directly at the end of such ammunition, 1 can precisely trace the path the bullet follows when shot. When such bullets are shot from a gun, this charge ignites. This area's smoke can be seen, clearly showing the bullet's route.
Barium nitrate is also one of the main ingredients used to make flares, which are used to direct troops to a specific spot. Finally, this substance is also present in explosive detonators. Likewise, barium nitrate is a crucial component of explosives because of its oxidising nature.
Barium nitrate works well as a rodenticide as well. It will keep different rodents, such as mice & rats, from entering or remaining within the premises if you leave it outside your home.
$\mathrm{Ba(NO_{3})_{2}}$ can occasionally be used to make specific kinds of propellants. However, pyrotechnic and military applications continue to be their primary uses.
It can be concluded that barium nitrate is crystalline. It is a salt with a very slight acidic flavour. Despite being non-flammable in most situations, this chemical can explode at very high temperatures. As an oxidising agent, barium nitrate promotes the burning of other substances. There are two ways to make this chemical. This substance has a melting point of around 590 $\mathrm{^{\circ}}$ C. It simply decomposes at high temperatures. People who are exposed to this material may experience barium nitrate poisoning symptoms, such as well as skin irritation.
Q1. Is barium nitrate salt insoluble in nature?
Ans. All nitrate salts are soluble. Because it can be absorbed by the body, barium nitrate's solubility makes it very dangerous to people.
Q 2. Barium nitrate burns green and why?
Ans. When heated to a high temperature, several substances emit a distinctive colour. The metal ions are excited by the flame's heat, which makes them radiate visible light. Barium emits light at a wavelength that corresponds to the colour green, which is why it has a green hue.
Q3. What product will be formed when we burn barium nitrate?
Ans. Barium nitrate burns with a green flame. When heated, it breaks down into barium oxide, oxygen, & nitrogen dioxide. As a result, nitric dioxide is produced from barium nitrate.
$$\mathrm{2\:Ba(NO_{3})_{2}\to\:2\:BaO\:+\:4NO_{2}\:+\:O_{2}}$$
Q4. Is it possible to make Barium Sulphate soluble in water?
Ans. The chemical will be soluble in water if the hydration energy of the ions is high enough to outweigh the molecule's lattice energy. It won't dissolve in water if the hydration energy of the ions does not exceed the lattice energy of the molecule. In the case of Barium Sulphate, the size of Barium ions and sulphate ions is almost similar. Because of this, the lattice energy of the molecule will get higher and which will overcome the hydration energy. Hence, it is not possible to make Barium sulphate soluble in water.
Qns. 5. Why Barium Nitrate does not react with Sulphuric acid?
Ans. Reacting Barium Nitrate with Sulphuric acid will produce Barium Sulphate and Nitric acid. As Barium sulphate is insoluble in water it will form a white precipitate out of the solution.
$$\mathrm{Ba(NO_{3})_{2}\:+\:H_{2}SO_{4}\to\:BaSO_{4}\:+\:2\:HNO_{3}}$$
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