Given:
[tex]M = \text{0.100 M}[/tex]
[tex]T = \text{20°C + 273 = 293 K}[/tex]
Unknown:
[tex]\pi[/tex]
Solution:
Step 1: Determine the van't Hoff factor.
Since Na₃PO₄ is a strong electrolyte, we will assume that Na₃PO₄ is dissociated completely into three sodium ions and one phosphate ion. Therefore, there are four ions in a formula unit of Na₃PO₄. This means that,
[tex]i = 4[/tex]
Step 2: Calculate the osmotic pressure of solution.
[tex]\pi = iMRT[/tex]
[tex]\pi = (4)\text{(0.100 M)[0.0821 (L • atm)/(mol • K)](293 K)}[/tex]
[tex]\boxed{\pi = \text{9.62 atm}}[/tex]
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