Why does Al(OH3) not dissociate when more base is added? Al(OH)_3 is only slight

Question

Why does Al(OH3) not dissociate when more base is added?

Al(OH)_3 is only slightly soluble in water but dissolves readily in either acidic or basic solutions. Write balanced reaction equations that explain this behavior. Addition of H^+: Al(OH)_3 + 3H^+ rightarrow Al^3+ + 3H_2 O or [Al(OH)_6]^3- OR Al(OH)_3 rightarrow Al^3+ + 3OH^- and OH^- + H^+ rightarrow H_2 O Addition of OH^-: Al(OH)_3 + OH6- rightarrow [Al(OH)_4]^- or [Al(OH)6]^- or Al(OH)_3 rightarrow + Al^3+ + 3OH^- and Al^3 + 4OH^- rightarrow [Al(OH)_4]^- or [Al(OH)_6]^3-

Explanation / Answer

for addition of H+:

Al(OH)3 + 3H3O+(aq) ---> 3H2O(l) + Al+3(aq)

when adding OH-.

Al(OH)3 + OH-(aq) ---> Al(OH)4-(aq)

note that both cases, the aluminium is always in aquous (ionic) that is, soluble

they won't reamain as OH- ions since they will form a complex... this is veyr known complex when there is excess OH- ions

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