What mass of insulin must be dissolved in 36.0 ml of water to produce a solution with an osmotic pressure of 15.9 mmhg at 25 C? the molar mass of insulin is 5808 g/mol
P= 15.9 mm Hg
= (15.9/760) atm
= 0.020921 atm
T= 25.0 oC
= (25.0+273) K
= 298 K
use:
P = C*R*T
0.020921 = C*0.0821*298.0
C =0.000855 M
volume , V = 36.0 mL
= 3.6*10^-2 L
number of mol,
n = Molarity * Volume
= 0.000855*0.036
= 3.078*10^-5 mol
mass,
m = number of mol * molar mass
= 0.000031*5808
= 0.179 g
Answer: 0.179 g
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