At what minimum pH will `10^(-3)` mol of `Al(OH)_(3)` go into solution (V = 1L) as `Al(OH)_(4)` and at what maximum pH it will dissolve as `Al^(3+)` ? Given
`Al (OH)_(4)^(-) hArr Al^(3+) +4OH^(-) , K_(eq) = 1.3 xx10^(-34)`
` Al(OH)_(3)hArr Al^(3+) +3OH^(-) , K_(sp) = 5.0 xx10^(-33)`

Explanation

To solve the problem, we need to determine two pH values: the minimum pH at which \( Al(OH)_3 \) will dissolve as \( Al(OH)_4^- \) and the maximum pH at which it will dissolve as \( Al^{3+} \). We will use the given equilibrium constants \( K_{eq} \) and \( K_{sp} \) for our calculations.

### Step 1: Determine the minimum pH for \( Al(OH)_4^- \)

1. **Write the relevant equilibrium reactions:**
- For \( Al(OH)_4^- \):
\[
Al(OH)_4^- \rightleftharpoons Al^{3+} + 4OH^-
...