In: Chemistry
A 0.3999g sample of reagent grade Al2(SO4)3.xH2O was dissolved and analyzed for its aluminum content gravimetrically by precipitation as the aluminum oxinate complex, AL(C9H6NO)3, the precipitate weighing 0.4185g. Calculate the number of molecules of water of crystallization.
Ans. Moles of Aluminum oxinate, Al(C9H6NO)3 produced = Mass / Molar mass
= 0.4185 g / (459.439879 g/ mol)
= 0.000910892 mol
Note that 1 mol aluminum oxinate contains 1 mol Al-atom whereas 1 mol aluminum sulfate, Al2(SO4)3.xH2O contains 2 mol Al-atom. That is, 2 mol aluminum sulfate produces 2 mol aluminum oxinate.
So,
Moles of Al2(SO4)3.xH2O in sample = (1/2) x moles of Al(C9H6NO)3 produced
= (1/2) x 0.000910892 mol
= 0.000455446 mol
1 mol Al2(SO4)3.xH2O consists of 1 mol Al2(SO4)3.
So,
Mass of Al2(SO4)3 in sample = Moles x Molar mass
= 0.000455446 mol x (342.153878 g/ mol)
= 0.155832574 g
Now,
Mass of H2O in sample = (Mass of Al2(SO4)3.xH2O – Mass of Al2(SO4)3) in sample
= 0.3999 g – 0.155832574 g
= 0.244067426 g
Moles of water in sample = Mass / Molar mass
= 0.244067426 g / (18.01528 g /mol)
= 0.013547801 mol
# Calculate stoichiometry:
Molar stoichiometry in Al2(SO4)3.xH2O = Moles of H2O / Moles of Al2(SO4)3.xH2O
= 0.013547801 mol / 0.000455446 mol
= 29.746 : 1
= 30 : 1 (nearest whole number)
That is, there are 30 moles of H2O every mol of Al2(SO4)3.xH2O
Hence,
Molecules of water of crystallization, X = 30
And, the compound is - Al2(SO4)3.30H2O