To determine the identity of an electrolyte in a solution, the solution's osmotic pressure may be measured. A solution containing 0.250 mol L1 of an unknown electrolyte was prepared and the osmotic pressure of the solution at 298 K was determined to be 1053 KPa. Use the reference table below in helping you to suggest the possible identity of the unknown electrolyte Electrolytic substance Van't Hoff factor (i) at 0.25 mol L1 NacI 1.70 NaBr 1.76 NaNO3 NH,CI 1.83 1.88 NH,Br 1.91 NH,NO3 1.96 ONACI ONaBr ONH4Br ONH4CI ONANO3 ONH4NO3

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You have a sucrose solution of 28°Brix or 28 grams of sugar per 100 grams solution in a ripe grape ready to be made into wine. What is the molality of the solution? Look up the freezing point depression constant KF and figure out what the new freezing temperature would be for that solution.

. The vapor pressure of benzene is 10 kPa while methylbenzene is 2.8 kPa. Determine the total pressure of an equimolar solution.

A certain dilute solution has an osmotic pressure of 11.1 atm at 25°C. Calculate the difference between the chemical potential of the solvent in the solution and that of pure water. Assume that the density is the same as that of water at 25°C, 0.99705 g-cm-3. (Hint: Express the chemical potential in terms of mole fraction, x1, and rewrite the osmotic pressure equation as OV = n2RT, where n2 is the number of moles of the solute and V = 1.00 L.)

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

In addition to filling in the blanks below, show all of your work for this problem on paper for later upload. Calculate the molality of a 25.0% by mass aqueous solution of Ca(NO3)2. Enter your value in the first box and an appropriate unit of measure in the second box.

The osmotic pressure of an unknown substance is measured at 298 K. Determine the molar mass if the concentration of this substance is 28.5 kg m^-3 and the osmotic pressure is 4.00×10^4 Pa.

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

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