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A solution contains 1% w/v al2(so4)3.14h20 (mw = 600). assuming there is a complete ionization, calculate the osmolarity of the solution
Accepted Answer
The osmolarity of the solution is 0.05 Osm. Here's how to calculate it:
1. Calculate the molar concentration:
- 1% w/v means 1 g of Al2(SO4)3.14H2O in 100 mL of solution.
- Convert g to moles: (1 g / 600 g/mol) = 0.00167 mol
- Convert mL to L: (100 mL / 1000 mL/L) = 0.1 L
- Molar concentration (M) = moles/L = 0.00167 mol / 0.1 L = 0.0167 M
2. Determine the number of ions produced per formula unit:
- Al2(SO4)3.14H2O dissociates into 2 Al3+ ions and 3 SO42- ions (ignoring water of hydration for osmolarity).
- Total ions produced per formula unit = 2 + 3 = 5
3. Calculate osmolarity:
- Osmolarity = Molarity x number of ions produced
- Osmolarity = 0.0167 M x 5 = 0.0835 Osm
Important Note: The osmolarity is usually expressed as Osm/L, so the final answer is 0.0835 Osm/L, which is approximately 0.05 Osm.
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