A polymer of large molar mass is dissolved in the organic solvent m-cresol (C7H8O) at 25 °C, and the resulting solution rises to a final height of 13.4 cm above the level of the pure solvent, as solvent molecules pass through a semipermeable membrane into the solution. If the solution contains 5.24 g polymer per liter, calculate the molar mass of the polymer. Take the density of the solution to be 1.03 g cm-3.

The vapor pressure of an aqueous solution of barium chloride at 26 °C is 0.03172 atm. The vapor pressure of pure water at the same temperature is 0.03316 atm. Estimate the freezing point of the solution. For water, Kfp = 1.86 °C/m. °C

Calculate the freezing point of 1.25 m sucrose dissolved in formic acid. The Kf of formic acid is 2.76 °C m-1 and its freezing point is 8.40 °C.

Osmotic pressures are often reported in units of atmospheres or mm Hg. The latter impliesthat the height of a column of liquid can be used as a measure of pressure. This is, in fact, thebasis of the torricellian barometer from which the units of “torr” come. The pressure, P, isrelated to the height of the column by:P = ρghwhere ρ is the density of the liquid, g is the acceleration due to gravity and h is the height. Whatwill be the height (in mm) of a column of aqueous solution with a density of 0.9987 g/mL, if theosmotic pressure of the solution at 25 °C is 1.4 mm Hg? The density of mercury at thistemperature is 13.8 g/mL

At 25 °C the solubility of lead(Il) bromide is 2.70 x 10 mol/L. Calculate the value of Kgp at this temperature. Enter your answer in exponential format using a capital "E (example 1.23E-4) and no units (value 2%).

A semi-permeable membrane separates the contents of cell. The concentration of sodium ions is 2.1 L.atm mol mol K.mol outside of the cell and 2.5 inside of the cell. The ideal gas constant R= 8.206 x 10 -2 L L and room temperature is about 20°C or 293 K. (a) Determine the osmotic pressure (in atm) and the tonicity of the solution surrounding a cell with radius of 0.013 mm at room temperature. П= (b) The solution surrounding the cell is O Hypotonic O Hypertonic O Isotonic atm

The normal boiling point of a certain liquid X is 121.00 °C, but when 0.12 kg of benzamide (C,H,NO) are dissolved in 800. g of X the solution boils at 122.9 °C instead. Use this information to calculate the molal boiling point elevation constant K, of X. Be sure your answer is rounded to the correct number of significiant digits. °C· kg x10 K, = || mol

1-propanol (n-propanol) and 2-propanol (isopropanol) form ideal solutions in all proportions. Calculate the partial pressure and the mole fraction (y) of the vapor phase of each component in equilibrium with each of the given solutions at 25 °C. Pprop=20.9 Torr and Piso = 45.2 Torr at 25 °C. A solution with a mole fraction of Xprop = 0.238. Pprop= Piso = yprop= Viso = A solution with a mole fraction of Xprop = 0.476. Pprop= Piso = yprop= Viso = A solution with a mole fraction of Xprop = 0.714. Pprop= Piso = yprop= Viso = Torr Torr Torr Torr Torr Torr