Acompound is found to have a molar mass of 598 g/mol. if 35.8 mg of the compound is dissolved in enough water to make 175 ml of solution at 25°c, what is the osmotic pressure of the resulting solution?

The computation for molarity is: 
(x) (0.175 L) = 0.0358 g / 598 g/mol 
x = 0.000342093 M 
Whereas the osmotic pressure calculation: 
pi = iMRT 
pi = (1) (0.000342093 mol/L) (0.08206 L atm / mol K) (298 K) 
pi = 0.0083655 atm 
Converting the answer to torr, will give us:
0.0083655 atm times (760 torr/atm) = 6.35778 torr 
which rounds off to 6.36 torr

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