Advanced Chemistry: What is Barium Nitrate?
Barium nitrate is an inorganic compound that is officially known by many other names as well. Some prefer to call it barium dinitrate, while others may know the compound as Nitrobarite. However, unofficially, people may refer to this particular compound as barium salt.
Barium nitrate formula is Ba(NO3)2. If you are appearing for your final year examinations soon, you need to have distinct knowledge about this particular chemical, along with all of its properties. By the end of this chapter, you will also learn about this salt’s various applications. Furthermore, major preparation processes are also discussed in detail.
The key to understanding how any compound functions is to learn about its various properties. Refer to the table below to gain insight into its various basic features and natural properties.
Properties of Barium Nitrate
Additionally, another interesting property of barium nitrate is that it enhances the combustibility of other compounds, even though it is not itself combustible. However, one must be wary of exposing barium nitrate to high heat for prolonged periods, as the compound can explode or act as a fire hazard. Moreover, it acts as an oxidising agent for separate chemical reactions; a property which also finds uses in various applications.
How to Produce Barium Nitrate
The formula of barium nitrate indicates its composition. However, when it comes to mass-producing this product, one of two standard procedures are generally followed. Let us learn about these processes in detail.
First Method
The first process begins with dissolving barium carbonate or BaCO3 with nitric acid (HNO3). As the two compounds react, iron impurities precipitate to the surface. With the help of filtration technique, you must remove these impurities. Next, the remaining mixture must undergo evaporation. Finally, after crystallisation, we receive pure barium nitrate which is often used industrially.
Second Method
Some manufacturers also use a secondary method for the creation of barium nitrate. This alternative method involves a chemical reaction between barium sulphide and nitric acid. Still, one must maintain a close watch on temperature during this production method, as intense temperatures can lead to the decomposition of Ba(NO3)2 into barium oxide, nitrogen dioxide and oxygen.
2Ba(NO3)2 → 2BaO + 4NO2 + O2
Precautionary Measures to Follow While Handling Barium Nitrate
High concentrations of this compound can be extensively poisonous to humans. One must take care not to inhale too much of its fumes. Similarly, direct exposure to the eyes and skin can also lead to several harmful symptoms. Upper lung irritation, skin irritation and eye irritation are some of the signs of barium nitrate poisoning. Notably these can be easily avoided by taking simple precautionary measures while handling it.
Applications of Barium Nitrate
Simply learning about the solubility of barium nitrate is not enough. You should also study about the various cases where this compound proves immensely useful. Some of these major uses are discussed below in detail.
1. In the Fireworks Industry
Barium nitrate is a prised compound when it comes to the fireworks industry because it can help in the production of green flames. Apart from just fireworks, one can also perceive this compound’s use in several pyrotechnic displays as well. Just as barium nitrate produce green flames; sodium chloride leads to yellow flame formation, while copper chloride turns blue during combustion. Therefore, often all of these are used together in fireworks.
2. In Glasswork Factories
Barium nitrate is a crucial product in the creation of high quality glass items. The oxygen molecule attached to this compound can help keep the glass items free from discolouration. Additionally, such glassware is exceptionally clear. Experts also use this compound when producing optical glasses.
Barium nitrate in camera lenses can improve refractive index, leading to clearer pictures.
3. Military Usage
Barium nitrate helps in the production of tracer bullets. When fired, one can follow the exact route that the bullet takes, thanks to a Ba(NO3)2 charge placed right at the end of such ammunition. This charge lights when such bullets are fired from a gun. The smoke from this portion is visible, precisely indicating the bullet’s path.
Additionally, barium nitrate is one of the primary compounds in the creation of flares, used to signal troops to a certain location. Lastly, explosive detonators contain this compound as well. Similarly, due to its oxidising nature, barium nitrate is an integral component for explosives.
4. Rodenticide
Simply knowing the colour of barium nitrate is not sufficient. One must also understand its other types of applications. For instance, apart from its military and fireworks usage, this compound is also a reliable rodenticide. Leaving it out in the open at your home will prevent various rodents, such as mice and rats from entering or staying inside the premises.
5. Paints
The paints on your home walls are simply a mixture of various chemical compounds. Barium nitrate is just one of these compounds. Notably, most paints would not exist without this specific nitrate of barium since it is often used as a primary constituent.
In some cases, this compound can also be used to produce propellants of some types. Nevertheless, its primary usage remains restricted to the military and pyrotechnic works.
Key Takeaways
Students need to remember a few crucial aspects about this salt compound when learning about it. Here is a brief summarisation of the important points that you must remember.
Barium nitrate is a crystalline substance that is generally white in colour.
It is a salt with subtle acidic properties.
Although non-combustible under normal circumstances, this substance can cause explosions under extremely high temperatures.
Barium nitrate is an oxidising agent, helping other compounds to burn
You can produce this compound in two methods, both of which involve nitric acid.
The melting point of this compound is around 592 degree Celsius.
Barium nitrate cannot be boiled. Under high temperatures, it simply decomposes.
Individuals exposed to this substance may undergo symptoms of barium nitrate poisoning, which includes irritation of skin, eyes and lungs.
Simply learning about barium nitrate from your textbooks is not enough. You need to look for an edge that propels you ahead of the competition in the upcoming examinations. At Vedantu, we provide a substantial amount of study materials and other assistance to students regarding each topic.
Our expert teachers can provide you with in-depth knowledge regarding the various barium nitrate uses, along with everything else that you should know about class 11 and class 12 chemistry. Now you can even download our Vedantu app for enhanced accessibility.
FAQs on Barium Nitrate
1. What is Barium Nitrate, and what is its chemical formula?
Barium Nitrate is an inorganic chemical compound with the formula Ba(NO₃)₂. It is the salt formed from the reaction of barium and nitric acid. Under standard conditions, it exists as a white, crystalline solid that is soluble in water. It is non-combustible on its own but acts as a strong oxidiser, enhancing the combustion of other materials.
2. What are the primary industrial applications or uses of Barium Nitrate?
Barium Nitrate has several important applications across different industries. The most notable uses include:
- Pyrotechnics: It is a key ingredient in fireworks and signal flares, where it acts as an oxidiser and produces a distinct bright green flame.
- Glass and Ceramics: It is used in the manufacturing of high-quality optical glass and ceramic glazes. It helps prevent discolouration and increases the refractive index of the glass.
- Military: It is used in the production of tracer ammunition, where a charge at the back of the bullet ignites to create a visible trail. It is also a component in some explosives and detonators.
- Chemical Manufacturing: It serves as a raw material for producing other barium compounds, such as barium oxide and barium peroxide.
3. Why does Barium Nitrate produce a green flame when used in fireworks?
The green flame is a result of a process called atomic emission. When Barium Nitrate is subjected to the high heat of a firework explosion, the barium ions (Ba²⁺) absorb energy, causing their electrons to jump to higher, unstable energy levels. As these electrons fall back to their original, stable state, they release the excess energy in the form of light. For barium, the specific wavelength of this emitted light falls within the green part of the visible spectrum, creating the characteristic colour.
4. What safety precautions are necessary when handling Barium Nitrate?
Barium Nitrate is toxic to humans and requires careful handling. Key safety measures include:
- Avoiding inhalation of its dust or fumes, as it can irritate the respiratory system.
- Preventing direct contact with skin and eyes by using protective gear like gloves and safety goggles.
- Never ingesting the compound, as it can lead to severe poisoning with symptoms like muscle spasms, gastroenteritis, and cardiac issues.
- Storing it away from combustible materials due to its strong oxidising properties, which can create a fire hazard.
5. How is Barium Nitrate prepared on an industrial scale?
There are two primary methods for the industrial production of Barium Nitrate:
- Method 1: This involves reacting nitric acid (HNO₃) with solid barium carbonate (BaCO₃). The reaction produces barium nitrate, water, and carbon dioxide. The resulting solution is then filtered to remove impurities, evaporated, and crystallised.
- Method 2: An alternative method involves combining barium sulphide (BaS) with nitric acid. This process requires careful temperature control to prevent the decomposition of the newly formed Barium Nitrate.
6. Is an aqueous solution of Barium Nitrate acidic, basic, or neutral?
In theory, an aqueous solution of Barium Nitrate is neutral. This is because it is a salt formed from a strong acid (Nitric Acid, HNO₃) and a strong base (Barium Hydroxide, Ba(OH)₂). In such cases, the constituent ions do not undergo significant hydrolysis, resulting in a solution with a pH of approximately 7. Any slight acidity observed in a real-world sample is often due to dissolved atmospheric carbon dioxide.
7. What happens when Barium Nitrate is heated strongly, and why can't it be boiled?
Barium Nitrate does not have a boiling point because it undergoes thermal decomposition before it can turn into a gas. When heated to its melting point and beyond (around 592°C), it breaks down into Barium Oxide (BaO), Nitrogen Dioxide (NO₂), and Oxygen (O₂). The chemical equation for this reaction is: 2Ba(NO₃)₂ → 2BaO + 4NO₂ + O₂. This release of oxygen is what makes it a powerful oxidising agent in applications like explosives and fireworks.
8. As per the CBSE/NCERT curriculum, how is the presence of Barium Nitrate confirmed in a salt analysis experiment?
To confirm Barium Nitrate in a qualitative salt analysis, you must test for both the cation (Ba²⁺) and the anion (NO₃⁻):
- Test for Barium ion (Ba²⁺): To the aqueous salt solution, add a few drops of potassium chromate (K₂CrO₄) solution. The formation of a distinct yellow precipitate of barium chromate (BaCrO₄) confirms the presence of the Ba²⁺ ion.
- Test for Nitrate ion (NO₃⁻): The classic confirmation is the brown ring test. To the salt solution, add freshly prepared ferrous sulphate (FeSO₄) solution. Then, carefully pour concentrated sulphuric acid (H₂SO₄) down the side of the test tube. The formation of a brown ring at the junction of the two liquid layers confirms the presence of the NO₃⁻ ion.
