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$\ce{Al^3+}$ in water will be hydrated, formed a complex ion $\ce{[Al(H2O)6]^3+(aq)}$ that can neutralize hydroxide ion according to the following reactions:

$$ \begin{align} \ce{[Al(H2O)6]^3+ + OH^- &<=> [Al(H2O)5OH]^2+ + H2O}\tag{1}\\ \ce{[Al(H2O)5OH]^2+ + OH^- &<=> [Al(H2O)4(OH)2]^+ + H2O}\tag{2}\\ \ce{[Al(H2O)4(OH)2]^+ + OH^- &<=> [Al(H2O)3(OH)3]^+ + H2O}\tag{3}\\ \end{align} $$

Which statement is true ?

(A) $\ce{[Al(H2O)6]^3+}$ is a Lewis base
(B) in all reactions $\ce{H2O}$ works as a base
(C) $\ce{[Al(H2O)4(OH)2]^+ }$ is amphiprotic

It is sure that $\ce{Al^3+}$ ion is a Lewis acid and $\ce{H2O}$ is a Lewis base when it is first hydrolize, but I think in the three reaction, $\ce{OH^-}$ work as a Lewis base, so the $\ce{H2O}$ is a conjugate acid right? I confused what is the true answer. Please kindly help me.

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