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-17%
Barium Acetate 500gm
Original price was: $2,500.00.$2,300.00Current price is: $2,300.00.
Benzoic Acid 500gm
Original price was: $2,500.00.$2,300.00Current price is: $2,300.00.
Barium Hydroxide 8 hydrate
Original price was: $1,085.00.$900.00Current price is: $900.00.
Barium hydroxide, with the chemical formula Ba(OH)2text{Ba(OH)}_2Ba(OH)2, is an inorganic compound that is used in various applications. Here’s a detailed overview:
Properties
- Appearance: White crystalline solid.
- Solubility: Moderately soluble in water, forming a strongly alkaline solution.
- Molecular Weight: 171.34 g/mol.
- Density: Approximately 2.18 g/cm³.
- Melting Point: 78 °C (anhydrous form); decomposes in water to form barium oxide and water.
Chemical Behavior
- Basicity: Barium hydroxide is a strong base and dissociates completely in water to form barium ions (Ba2+text{Ba}^{2+}Ba2+) and hydroxide ions (OH−text{OH}^-OH−).
- Reaction with Acids: Reacts with acids to form barium salts and water. For example: Ba(OH)2+2HCl→BaCl2+2H2Otext{Ba(OH)}_2 + 2text{HCl} rightarrow text{BaCl}_2 + 2text{H}_2text{O}Ba(OH)2+2HCl→BaCl2+2H2O
- Hydrate Forms: Often found as the octahydrate (Ba(OH)2⋅8H2Otext{Ba(OH)}_2 cdot 8text{H}_2text{O}Ba(OH)2⋅8H2O).
Description
Uses of Barium Hydroxide
1. Titration
- Acid-Base Titrations: Barium hydroxide is often used as a titrant in acid-base titrations. It serves as a strong base to titrate weak or strong acids. Its high solubility and complete dissociation in water make it ideal for this purpose.
2. Chemical Synthesis
- Preparation of Barium Salts: Barium hydroxide is used to synthesize various barium salts by reacting with corresponding acids. For instance, reacting barium hydroxide with sulfuric acid yields barium sulfate, a key compound in qualitative inorganic analysis: Ba(OH)2+H2SO4→BaSO4↓+2H2Otext{Ba(OH)}_2 + text{H}_2text{SO}_4 rightarrow text{BaSO}_4 downarrow + 2text{H}_2text{O}Ba(OH)2+H2SO4→BaSO4↓+2H2O
3. Qualitative Inorganic Analysis
- Testing for Sulfate Ions: In qualitative analysis, barium hydroxide is used to test for the presence of sulfate ions (SO42−text{SO}_4^{2-}SO42−) in a solution. When barium hydroxide is added to a solution containing sulfate ions, a white precipitate of barium sulfate forms: Ba2++SO42−→BaSO4↓text{Ba}^{2+} + text{SO}_4^{2-} rightarrow text{BaSO}_4 downarrowBa2++SO42−→BaSO4↓
4. Precipitation Reactions
- Removal of Sulfates and Carbonates: In analytical procedures, barium hydroxide can be used to precipitate sulfate and carbonate ions from solutions, aiding in their removal or quantitative analysis.
5. pH Adjustment
- Buffer Solutions: Barium hydroxide is used to adjust the pH of buffer solutions. Its strong basicity helps in maintaining the desired pH levels in various experimental setups.
6. Dehydrating Agent
- Removal of Moisture: In some laboratory processes, barium hydroxide is used to remove moisture from organic solvents and other materials due to its hygroscopic nature.
7. Chemical Reactions and Catalysis
- Reagent in Organic Synthesis: It can be used as a base in organic synthesis reactions, such as the formation of enolates, aldol reactions, and other base-catalyzed reactions.
- Catalyst: Barium hydroxide can act as a catalyst in certain chemical reactions, promoting faster reaction rates and better yields.
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Mutangwa –
Barium hydroxide helps remove sulfate irons from water by forming insoluble barium sulfate