Refer to the information below:

Solubility:

Al$($OH$)3($s$)$ Al$3+($aq$)+3$ OH$-($aq$)$

Ksp $=1\mathrm{.}30$ x $10-33$

Complex Formation:

Al$3+($aq$)+4$ OH$-($aq$)[$Al$($OH$)4]-($aq$)$

Kf $=3\mathrm{.}0$ x $1033$

Overall Reaction:

Al$($OH$)3($s$)+$ OH$-($aq$)[$Al$($OH$)4]-($aq$)$

K $=3\mathrm{.}9$

$1.$ Calculate the molar solubility of Al$($OH$)3$ at pH $=9\mathrm{.}00($Hint: What is $[$OH$-]$ at this pH$?)$

$2.$ Calculate the molar solubility in only water.

Answer the question below by comparing the two solubilities.

By what factor does the solubility increase relative to the solubility in pure water? Enter your answer to the nearest integer.