Question

A) A solution is prepared by dissolving 50.7 g sucrose (C12H22O11) in 0.423 kg of water. The final volume of the solution is 355 mL. 1) For this solution, calculate molarity. 2) For this solution, calculate molality. 3) For this solution, calculate percent by mass. 4) For this solution, calculate mole fraction. B) Calculate the vapor pressure at 25 ∘C of a solution containing 55.2 g ethylene glycol (HOCH2CH2OH) and 286.6 g water. The vapor pressure of pure water at 25 ∘C is 23.8 torr. C) A solution containing ethylene glycol and water has a vapor pressure of 7.95 torr at 10 ∘C. Pure water has a vapor pressure of 9.21 torr at 10 ∘C. What is the mole fraction of ethylene glycol in the solution? D) Calculate the osmotic pressure (in atmospheres) of a solution containing 1.90 g ethylene glycol (C2H6O2) in 53.0 mL of solution at 25∘C. E) Calculate the osmotic pressure of a solution containing 17.05 mg of hemoglobin in 14.2 mL of solution at 35 ∘C . The molar mass of hemoglobin is 6.5×104 g/mol.

If anybody can answer any of these question parts it would be greatly appreciated! Thank you so much in advance!

Answer 1

2) as P⁰-P_s/ P_s = n₂/n₁ no of moles = given mass / molar mass

P^{0 -} 7.95 /7.95 = (55.2/62.07)/  286.6 /18

P^{0 -} 7.95 = 7.07 / 15.92

P⁰= 8.39 torr

3) V =n R T

=1.90/62.07 * 0.0821 * 298 / 53 * 10 ^-3

= 0.01413 *10³ atm

4)   V =n R T

=  (17.05  * 10 ^-3 /6.5×10⁴) * 0.0821* 308 / 14.2 * 10 ^-3

= 66.32 * ×10^-4 atm