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Questions
Determine the osmotic pressure of a solution prepared by dissolving 25 mg of K2SO4 in 2 liter of water at 25°C, assuming that it is completely dissociated.
Determine the osmotic pressure of a solution prepared by dissolving 25 mg of K2SO4 in 2 liter of water at 25°C, assuming that it is completely dissociated. (mol. wt. of K2SO4 = 174 g mol−1)
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Solution
Given: K2SO4 dissolved (w) = 25 mg = 0.025 g
Volume of solution (V) = 2 L
Temperature (T) = 25°C = (25 + 273) K = 298 K
R = 0.0821 L atm K−1 mol−1
When K2SO4 is dissolved in water, K+ and \[\ce{SO^{2-}4}\] ions are produced.
\[\ce{K2SO4 -> 2K+ + SO^{2-}4}\]
Total number of ions produced = 3
∴ i = 3
Molar mass of K2SO4 (M) = (2 × 39) + (1 × 32) + (4 × 16)
= 174 g mol−1
Applying the following relation,
π = `i n/V RT`
= `i xx w/M xx 1/V RT`
= `3 xx 0.025/174 xx 1/2 xx 0.0821 xx 298`
= 5.27 × 10−3 atm
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