Barium Hydroxide: Properties, Uses, and Safety Information
Barium hydroxide is a strong inorganic base with the chemical formula Ba(OH)₂. It plays a critical role in chemical synthesis, analytical chemistry, and several industrial processes. Known for its strong alkalinity and ability to absorb carbon dioxide, barium hydroxide is typically encountered as a white powder or in its more stable hydrated form, barium hydroxide octahydrate (Ba(OH)₂·8H₂O).
Chemical Identity
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Chemical Name: Barium Hydroxide
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Chemical Formula: Ba(OH)₂
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Molar Mass: 171.34 g/mol (anhydrous)
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Appearance: White crystalline solid or powder
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Solubility: Soluble in water; insoluble in alcohol
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pH: Strongly basic in aqueous solution
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Melting Point: 407 °C (anhydrous)
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Boiling Point: Decomposes before boiling
Physical and Chemical Properties
Barium hydroxide dissolves in water to form a highly alkaline solution. In water, it dissociates completely into Ba²⁺ and OH⁻ ions, making it a strong base comparable to sodium and potassium hydroxides. It is capable of absorbing carbon dioxide from the air, forming barium carbonate:
Ba(OH)₂ + CO₂ → BaCO₃ + H₂O
This property makes it useful in gas purification and analytical procedures.
Common Hydrated Form: Barium Hydroxide Octahydrate
In most applications, barium hydroxide is handled as Ba(OH)₂·8H₂O, a more stable form that appears as colorless crystals and retains strong basic properties. It is used interchangeably with the anhydrous form in many cases, especially in aqueous reactions.
Applications
1. Analytical Chemistry
Barium hydroxide is used in titrations involving weak acids and in gravimetric analysis. Its ability to form insoluble barium salts (like BaSO₄) makes it valuable in sulfate determination and other ionic precipitation reactions.
2. Chemical Manufacturing
It serves as a precursor to other barium compounds, including barium salts like barium nitrate, chloride, or carbonate. It is also used as a catalyst or base in various organic synthesis reactions.
3. Water Treatment
Due to its alkalinity and ability to neutralize acids, barium hydroxide is employed in pH adjustment of industrial wastewater and in removing sulfate ions from solution.
4. Lubricants and Grease
In some specialized lubricants, barium hydroxide is used to improve water resistance and thermal stability.
5. Plastics and Resins
It is involved in the manufacture of thermosetting resins, particularly phenolic resins, where it acts as a curing catalyst.
Handling and Storage
Storage Guidelines:
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Store in a cool, dry place
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Use airtight containers to avoid moisture absorption and carbonation
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Keep away from acids and incompatible materials
Handling Precautions:
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Always use gloves, eye protection, and protective clothing
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Avoid inhalation of dust or contact with skin and eyes
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Use in a well-ventilated area or fume hood
Safety and Toxicity
Barium hydroxide is highly corrosive and toxic. Barium ions can disrupt biological potassium channels and are harmful if ingested, inhaled, or absorbed through the skin.
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Health Hazards:
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Causes severe skin and eye irritation or burns
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Inhalation may result in respiratory tract damage
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Ingestion can lead to muscle weakness, irregular heartbeat, and even death
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Environmental Hazards:
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Harmful to aquatic life
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Should not be released into waterways or soil
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First Aid Measures:
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Skin/Eye Contact: Rinse immediately with water for at least 15 minutes; seek medical attention
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Inhalation: Move to fresh air; administer oxygen if needed
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Ingestion: Seek medical help immediately; do not induce vomiting
Conclusion
Barium hydroxide is a strong and versatile base used in a wide array of chemical, analytical, and industrial applications. While its reactivity and solubility make it a useful reagent and precursor, it must be handled with great care due to its corrosive and toxic nature. With proper safety protocols and responsible handling, barium hydroxide remains a valuable chemical across many scientific and industrial disciplines.
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