A sucrose (C12H22O11) solution that is 45.0% sucrose by mass has a density of 1.203g/mL at 25°C. Calculate its(a) molarity.(b) molality.(c) vapor pressure .(d) normal boiling point.

We have a 1.000 M aqueous solution of C3H8O(aq) (C3H8O is the only solute). Thedensity of this solution is 0.988 g/mL. Calculate the molality, the percent mass, and themole fraction of C3H8O in this aqueous solution. The molar masses of C, O, and H are12.01, 16.00, and 1.01 g/mol

(d) Determine the freezing point and boiling point of the solution. (Assume density of water = 1.00 g/mL; Kf= 1.86oC/m; Kb= 0.512oC/m; density of EG = 1.114 g/mL

Glycerin 1C3H8O32 is a nonvolatile nonelectrolyte with a density of 1.26 g>mL at 25 °C. Calculate the vapor pressure at 25 °C of a solution made by adding 50.0 mL of glycerin to 500.0 mL of water. The vapor pressure of pure water at 25 °C is 23.8 torr (Appendix B), and its density is 1.00 g>mL.

What is the molality of a solution consisting of 9.265 mass % of C2H5OH dissolved in water?

A certain liquid  X  has a normal boiling point of  105.30°C  and a boiling point elevation constant  =Kb1.13·°C·kgmol−1 . Calculate the boiling point of a solution made of  52. g  of zinc chloride ( ZnCl2 ) dissolved in  450.g  of  X .