1. Determine the Molecular Weight of Aluminum Sulfate (Al₂(SO₄)₃)
* Al: 26.98 g/mol (atomic weight) x 2 = 53.96 g/mol
* S: 32.06 g/mol x 3 = 96.18 g/mol
* O: 16.00 g/mol x 12 = 192.00 g/mol
Total molecular weight = 53.96 + 96.18 + 192.00 = 342.14 g/mol
2. Calculate the Number of Moles of Aluminum Sulfate
* Moles = Mass / Molecular weight
* Moles = 10.00 g / 342.14 g/mol = 0.0292 mol
3. Determine the Number of Ions Produced per Molecule
* Aluminum sulfate dissociates into 2 aluminum ions (Al³⁺) and 3 sulfate ions (SO₄²⁻) for a total of 5 ions per molecule.
4. Calculate the Osmolarity
* Osmolarity = (Number of moles of solute x Number of ions per molecule) / Volume of solution (in liters)
* Osmolarity = (0.0292 mol x 5) / 0.200 L = 0.730 Osm
Therefore, the osmolarity of a 10.00 g aluminum sulfate solution in 200 ml of water is 0.730 Osm.
