BARIUM NITRATE – OVERVIEW
Chemical Formula: Ba(NO₃)₂
Molecular Weight: 261.34 g/mol
Appearance: White crystalline salt, soluble in water
Nature: Strong oxidizer and toxic (handled with care)
⚗️ RAW MATERIALS REQUIRED
Raw Material Formula Purpose
Barium Carbonate BaCO₃ Primary source of barium
Nitric Acid HNO₃ Provides nitrate ion and enables neutralization
Water H₂O Solvent for reaction and recrystallization
🔬 CHEMICAL REACTION
📌 Primary Reaction (Neutralization):
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BaCO₃ + 2 HNO₃ → Ba(NO₃)₂ + CO₂↑ + H₂O
Byproduct: CO₂ gas (bubbled out)
The resulting solution contains Barium Nitrate, which is then crystallized.
🏭 MANUFACTURING PROCESS
✅ Step 1: Acid Neutralization
In a glass-lined or acid-resistant steel reactor, slowly add nitric acid to barium carbonate under stirring.
Maintain temperature at 50–70°C to aid reaction and gas release (CO₂).
Ensure complete neutralization by pH monitoring (~pH 5–6 at end point).
✅ Step 2: Filtration
Filter the resulting solution to remove unreacted BaCO₃ or impurities.
✅ Step 3: Crystallization
Concentrate the filtrate by evaporation until saturation.
Cool the solution to room temperature or lower (~20°C) to form Ba(NO₃)₂ crystals.
✅ Step 4: Separation & Washing
Filter out crystals, wash with cold distilled water to remove acidic residues.
✅ Step 5: Drying
Dry in a tray dryer at 50–60°C.
Avoid overheating, as decomposition may occur.
📦 TYPICAL YIELD (Per 100 kg batch)
Material Quantity
Barium Carbonate ~74 kg
Nitric Acid (60%) ~70–75 kg
Water ~100–120 L
Barium Nitrate Output ~110–120 kg (depending on purity and process control)
🧯 SAFETY & HANDLING
Toxic: Barium salts are poisonous — avoid ingestion and inhalation.
Oxidizer: Keep away from flammable materials and reducing agents.
Use PPE, fume hoods, and store in dry, sealed containers.
🏭 USES OF BARIUM NITRATE IN VARIOUS INDUSTRIES
Industry Application
Fireworks & Pyrotechnics Produces bright green color flames, acts as oxidizer
Explosives Used in military-grade detonators, flash powders
Glass & Ceramics Improves gloss and thermal properties of special glasses
Vacuum Tubes & Electronics Used in getter materials to remove gases
Metal Surface Treatment Part of nitrating salt baths for heat treating steels
Chemical Reactions Intermediate in barium compound synthesis (e.g., BaTiO₃)
🔁 Alternative Production Method (Less Common):
Reacting Barium Chloride (BaCl₂) with Sodium Nitrate (NaNO₃) in solution:
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BaCl₂ + 2 NaNO₃ → Ba(NO₃)₂↓ + 2 NaCl
This method is less economical due to the use of pure barium salts.
Chemical Formula: Ba(NO₃)₂
Molecular Weight: 261.34 g/mol
Appearance: White crystalline salt, soluble in water
Nature: Strong oxidizer and toxic (handled with care)
⚗️ RAW MATERIALS REQUIRED
Raw Material Formula Purpose
Barium Carbonate BaCO₃ Primary source of barium
Nitric Acid HNO₃ Provides nitrate ion and enables neutralization
Water H₂O Solvent for reaction and recrystallization
🔬 CHEMICAL REACTION
📌 Primary Reaction (Neutralization):
scss
Copy
Edit
BaCO₃ + 2 HNO₃ → Ba(NO₃)₂ + CO₂↑ + H₂O
Byproduct: CO₂ gas (bubbled out)
The resulting solution contains Barium Nitrate, which is then crystallized.
🏭 MANUFACTURING PROCESS
✅ Step 1: Acid Neutralization
In a glass-lined or acid-resistant steel reactor, slowly add nitric acid to barium carbonate under stirring.
Maintain temperature at 50–70°C to aid reaction and gas release (CO₂).
Ensure complete neutralization by pH monitoring (~pH 5–6 at end point).
✅ Step 2: Filtration
Filter the resulting solution to remove unreacted BaCO₃ or impurities.
✅ Step 3: Crystallization
Concentrate the filtrate by evaporation until saturation.
Cool the solution to room temperature or lower (~20°C) to form Ba(NO₃)₂ crystals.
✅ Step 4: Separation & Washing
Filter out crystals, wash with cold distilled water to remove acidic residues.
✅ Step 5: Drying
Dry in a tray dryer at 50–60°C.
Avoid overheating, as decomposition may occur.
📦 TYPICAL YIELD (Per 100 kg batch)
Material Quantity
Barium Carbonate ~74 kg
Nitric Acid (60%) ~70–75 kg
Water ~100–120 L
Barium Nitrate Output ~110–120 kg (depending on purity and process control)
🧯 SAFETY & HANDLING
Toxic: Barium salts are poisonous — avoid ingestion and inhalation.
Oxidizer: Keep away from flammable materials and reducing agents.
Use PPE, fume hoods, and store in dry, sealed containers.
🏭 USES OF BARIUM NITRATE IN VARIOUS INDUSTRIES
Industry Application
Fireworks & Pyrotechnics Produces bright green color flames, acts as oxidizer
Explosives Used in military-grade detonators, flash powders
Glass & Ceramics Improves gloss and thermal properties of special glasses
Vacuum Tubes & Electronics Used in getter materials to remove gases
Metal Surface Treatment Part of nitrating salt baths for heat treating steels
Chemical Reactions Intermediate in barium compound synthesis (e.g., BaTiO₃)
🔁 Alternative Production Method (Less Common):
Reacting Barium Chloride (BaCl₂) with Sodium Nitrate (NaNO₃) in solution:
scss
Copy
Edit
BaCl₂ + 2 NaNO₃ → Ba(NO₃)₂↓ + 2 NaCl
This method is less economical due to the use of pure barium salts.
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