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Osmotic Pressure

The osmotic p...

Question

The osmotic pressure of a solution in atm obtained on mixing each $50$ mL of $1.2$ % mass/volume urea solution and $2.4$ % mass/volume glucose solution at $300$ K is: $(R = 0.08$ litre atm $K^{- 1} m o l^{- 1})$

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Solution

The molar masses of glucose and urea are 60 g/mol and 180 g/mol respectively.
The number of moles of urea $= \frac{50 m L \times 1.2 g}{100 m L \times 60 g / m o l}$
$= 0.01 m o l$
The number of moles of glucose $= \frac{50 m L \times 2.4 g}{100 m L \times 180 g / m o l}$
$= 0.0067 m o l$
Total molar concentration $= \frac{0.01 m o l + 0.0067 m o l}{50 m L + 50 m L} \times \frac{1000 m L}{1 L}$
$= 0.167 M$
The osmotic pressure is $Π = C R T$
$= 0.167 M \times 0.08 L . a t m / m o l / K \times 300 K$
$= 4 a t m$

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