Aluminum metal dissolves in dilute mineral acids to form the al3+ ion. hot alkali
solutions also react with aluminum metal to produce solutions containing aluminate
ions, al(oh)4– with the evolution of hydrogen gas.
2al(s) + 2koh(aq) + 6h2o(l) → 2kal(oh)4(aq) + 3h2(g)
when sulfuric acid is added to the alkaline aluminate solution, a series of reactions
take place. excess potassium hydroxide is neutralized,
2koh(aq) + h2so4 (aq) → k2so4 (aq) + 2h2o(l)
with the liberation of heat. the aluminate ions first react with sulfuric acid to produce
insoluble aluminum hydroxide,
2k+(aq) + 2al(oh)-

4 (aq) + h2so4 (aq) → 2k+(aq) + 2al(oh)3 (s) + 2h2o(l) + so4 2-
(aq)

then further addition of sulfuric acid dissolves the aluminum hydroxide.
2al(oh)3 (s) + 3h2so4 (aq) → 2al3+(aq) + 3so4 2-

(aq) + 6h2o(l)

the aluminum, potassium, and sulfate ions crystallize in the form of a double salt or
“alum” according to the following equation,
k+(aq) + al3+(aq) + 2so4
2-
(aq) + 12h2o(l) → kal(so4)2·12h2o(s)

potassium aluminum sulfate dodecahydrate

calculations:
1. calculate the theoretical mass of potassium aluminum sulfate dodecahydrate
that could have been produced. (hint: remember to include the mass of the 12
waters of hydration when you are calculating the molar mass of your product).
2. calculate the percent yield of the potassium aluminum sulfate dodecahydrate.

considering i used 0,51 grams of pure aluminium scrap, what would be the theoretical mass of the precipitate, alum? ?

and also, what would be the net ionic equation for the formation of the product from al3+? ?
you