a solution is prepared by dissolving 4.9 g of sucrose (C12H22O11) in 175 g of water. calculate the boiling point and osmotic pressure of this solution at 25°c. assume that molarity and molality of this solution are equal. E(h2O) = 0.52.

Answer 1

delta T = i*Kb*molality
i = 1 for sucrose
Kb. You need to look up that constant. For water it is approximately 0.51 C/m but don't assume I am correct. Confirm that.
molality = moles sucrose/kg solvent. mols = g/molar mass and solvent is 0.175 kg.
Substitute and solve for delta T, then add that increment to the normal boiling point of water.
For osmotic pressure use
p = MRT. The problem tells you to use as M the same you calculated for m. You know R and T. Solve for osmotic pressure in atm if you use R = 0.08205. Post your work if you get stuck.