# What will be the Lewis acid and Lewis base in the reactions between aluminium(III) aqua complex and hydroxide?

$$\ce{Al^3+}$$ 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.