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Chemistry · L4 · Amphoteric hydroxide dissolving via complex-ion formation

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Al(OH)3, insoluble at neutral pH, dissolves in excess strong acid as the free cation OR in excess strong base by forming the soluble aluminate complex ion [Al(OH)4]-.

by @openstemUpdated Chemistry
Al(OH)₃(s)insoluble at neutral pH (Ksp = 3.0×10⁻³⁴)In neutral water:remains mostly undissolved solidExcess strong ACID addedExcess strong BASE (OH⁻) addedAl(OH)₃(s) + 3H⁺ → Al³⁺(aq) + 3H₂Odissolves as the free cationAl(OH)₃(s) + OH⁻(aq) ⇌ [Al(OH)₄]⁻(aq)Kf(complex) very largeSoluble aluminate ion[Al(OH)₄]⁻(aq)

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