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Determine the osmotic pressure of a solution prepared by dissolving 25 mg of K2SO4 in 2 litre of water at 25° C, assuming that it is completely dissociated.

Jayant Kumar , 10 Years ago

Grade 11

2 Answers

Pankaj

Last Activity: 9 Years ago

Mass of K₂SO₄, w = 25 mg = 0.025g (use 1 g = 1000 mg )
Volume V = 2 liter
T = 25 + 273 = 298 K
The reaction of dissociation of K2SO4
K₂SO₄ → 2K+ + SO₄^2-
Number if ions produced = 2+ 1 = 3
So van’t Hoff factor i = 3
Now
$\pi = i\frac{w}{M}\frac{1}{v}RT$
Substituting the values and calculationg we get,
π= 5.27 × 10^-3 atm

ankit singh

Last Activity: 4 Years ago

Given, that mass of K2SO4, w=25 mg=0.025 g

Volume V=2 L

T=25+273 =298 K

The reaction of dissociation of K2SO4 is,

K2SO4→2K++SO42−

Number of ions produced=3=van't Hoff factor

Hence, π=iCRT

⟹π=3×1740.025×0.5×0.0821×298=5.27×10−3 atm

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