The osmotic pressure of blood is $8.21$ atm at $37^{o}$ C. How much glucose is used per lit for an intravenous injection that is to isotonic with blood?

180

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342

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58.06

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55.55

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Solution

The correct option is D $58.06$ gm
$π v = \frac{w_{2}}{M_{2}} R T$
Given that
$π = 8.21$
$v = 1 L$
$M_{2} = 180$ --- Molar mass of glucose
$T = 273 + 37 = 310 K$
$R = 0.0821$
$w_{2} = ?$
put the values
$w_{2} = \frac{π v M_{2}}{R T}$
$= 58.13$

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