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Hydroxides are compounds containing the hydroxide ion, OH⁻, typically bonded to a metal or cation (M–OH). They are commonly basic, and many serve as key inorganic bases and precursors to oxides.
Aluminium Hydroxide Al(OH)3 - 1000g
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Aluminium Hydroxide Al(OH)3 - 100g
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Aluminium Hydroxide Al(OH)3 - 25 000g
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Aluminium Hydroxide Al(OH)3 - 5000g
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Aluminium Hydroxide Al(OH)3 - 500g
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Barium hydroxide ( Ba(OH)2 ) - 1000g
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Barium hydroxide ( Ba(OH)2 ) - 100g
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Barium hydroxide ( Ba(OH)2 ) - 10g
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Barium hydroxide ( Ba(OH)2 ) - 500g
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Lithium hydroxide ( LiOH ) - 100g
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Lithium hydroxide ( LiOH ) - 10g
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Lithium hydroxide ( LiOH ) - 1g
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Lithium hydroxide ( LiOH ) - 50g
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Potassium Hydroxide ( KOH ) caustic potash - 1000g
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Potassium Hydroxide ( KOH ) caustic potash - 100g
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Potassium Hydroxide ( KOH ) caustic potash - 25 000g = 25kg Bag
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Potassium Hydroxide ( KOH ) caustic potash - 5000g
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Potassium Hydroxide ( KOH ) caustic potash - 500g
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Sodium Hydroxide ( Lye ) Caustic Soda - 1000g = 1kg
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Sodium Hydroxide ( Lye ) Caustic Soda - 100g
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Sodium Hydroxide ( Lye ) Caustic Soda - 25 000g = 25kg Bag
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Sodium Hydroxide ( Lye ) Caustic Soda - 500g
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Strontium hydroxide 500g
199,30 zł
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Aluminium hydroxide 47-60% Loba gel extra pure op.500 g
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Aluminium hydroxide PureLand chda Op.1000 g HDPE bottle
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Hydroxides consist of OH⁻ ions paired with cations, ranging from highly ionic alkali-metal hydroxides (e.g., NaOH, KOH) to more covalent or polymeric metal hydroxides (e.g., Al(OH)₃, Fe(OH)₃). In water, soluble hydroxides dissociate to release OH⁻, raising pH and acting as Brønsted–Lowry bases. Their basicity and solubility follow periodic trends: Group 1 hydroxides are strongly basic and highly soluble; Group 2 hydroxides are also basic but show decreasing solubility down the group (with Mg(OH)₂ sparingly soluble). Many transition-metal hydroxides are poorly soluble and often exist as hydrated, polymeric solids.
Acid–base and amphoterism.
Hydroxides can be classified as:
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Basic hydroxides, which neutralize acids to form salts and water (e.g., NaOH + HCl → NaCl + H₂O).
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Amphoteric hydroxides, which react with both acids and strong bases, reflecting borderline Lewis acidity/basicity of the metal center (e.g., Al(OH)₃ dissolves in acid to give Al³⁺ and in base to give aluminate [Al(OH)₄]⁻). Representative amphoteric hydroxides include those of Al, Zn, Sn, Pb, and Cr.
Thermal behavior and formation of oxides.
On heating, many metal hydroxides decompose to metal oxides and water:
M(OH)ₙ → MO_(n/2) + (n/2) H₂O.
This dehydration is central to materials synthesis (e.g., producing MgO, Al₂O₃) and to geochemical processes. Alkali hydroxides are comparatively thermally stable, while many transition-metal hydroxides dehydrate readily.
Structural aspects.
Solid hydroxides often form extended lattices with hydrogen bonding networks. Layered hydroxides (e.g., brucite-type Mg(OH)₂) can intercalate ions and water; related layered double hydroxides (LDHs) are important anion-exchange materials and catalysts. In coordination chemistry, terminal or bridging hydroxo ligands (–OH) are common in metal complexes, influencing reactivity via proton transfer and metal–metal bridging.
Reactivity and applications.
Strong hydroxide bases drive nucleophilic substitution and elimination in organic synthesis, promote saponification of esters, and deprotonate weak acids to form reactive anions. Industrially, hydroxides are essential in pulp and paper processing, soap manufacture, alumina extraction (Bayer process), CO₂ scrubbing (forming carbonates/bicarbonates), and water treatment via precipitation of metal hydroxides. Biologically and environmentally, hydroxide equilibria control mineral solubility and buffer natural waters.