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Calculate osmotic pressure for 0.100 M Na3PO4  aqueous solution at 20°C.​

Sagot :

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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