A compound 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?

Question

Chemistry

Jaden Rivera

28 February, 20:40

A compound 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?

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Arden · Answer 1

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