. Assume ideal solutions at the same temperature.a) Which solution has the higher osmotic pressure? urea Na2SO4they are equal(Circle one):b) In order to stop water from flowing, pressure must be applied to which side of the tube? urea Na2SO4neither(Circle one):c) If water is allowed to flow through the semipermeable membrane at a constant temperature, what will the concentration of Na2SO4(aq)be when equilibrium is reached? (It might be helpful to break down concentration into moles solute per L solution and to consider that there is a total of 2 L of solution in the tube.)[Na2SO4] = M339
CHEM230 _W16 _PREP 3 _blankp 14191) The standardboiling point of ethanol (C2H6O) is 78.4oC. 9.15 g of a molecular solute dissolves in 100 g of ethanol. The vapor pressure of the resulting solution is 730.6 torr at 78.4oC.a) What is the mole fraction of ethanol in the solution? (1 bar = 750.06 torr)Xethanol=b) What is the molar mass of the solute?MWsolute= g/molc) What is the boiling point of the solution? (kb(ethanol) = 1.07 (oC kg)/mol)Tboiling= oC686
CHEM230 _W16 _PREP 3 _blankp 15b) Rank the following saturated aqueous solutions (all at the same temperature) in order of increasing osmotic pressure: Ag(IO3) (Ksp= 3.17x10-8), Ba(IO3)2(Ksp= 4.01x10-4), and Cr(IO3)3(Ksp= 5x10-6). Write the name of one salt in each box.lowest osmotic pressure<<highestosmotic pressure198) Find the osmotic pressure of a saturated solution of Cr(IO3)3(Ksp= 5x10-6) at 298K.Π= atmc) What is the ΔHhydof IO3-given the follwing data: ΔHhyd(Na+) = -406 kJ/mol; ΔHlat(NaIO3) = 766 kJ/mol; ΔHsol(NaIO3)= 20.3 kJ/mold) What mass of NaIO3(s)(MW =197.89) must be added to 250 mL of a 0.086 M solution of Cr+3(aq)in order for start precipitate formation. (You may need data provided earlier in the problem.)mass NaIO3g128ΔHhyd(IO3-) = kJ/mol48
CHEM230 _W16 _PREP 3 _blankp 16199) a) Data shows that carbon dioxide (CO2) has a solubility of 0.3346 g CO2per 100 mL of water at 273K when the partial pressure of CO2is 1 atm. a) Find the Henry's law (kH) constant for CO2in water at 273K in molality units: mol/(kg bar). Use units of bar for pressure. Assume the density of water is 1.0 g/mL.molkgbarkH=b) In J. Chem. Educ. (87,2010,993) it is reported that the freezing point for an unopened can of LaCroix brand sparkling water is -0.49oC. Given the kffor water is 1.86 (oC kg)/mol, what is the partial pressure of CO2in the can?PCO2= bar68200) Two beakers, one containing 0.01 m NaNO3(aq)and the other containing 0.01 m Fe(NO3)3(aq)are placed inside a bell jar and sealed. The beakers are left until the water vapor has come to equilibrium with any liquid in the container. The levels of the liquid in each beaker at the beginning of the experiment are both at the 1L mark as pictured. Draw the relative levels of the liquid at equilibrium. If there is no change in the liquid level, write no change.1LNaNO3(aq)1LFe(NO3)3(aq)4
CHEM230 _W16 _PREP 3 _blankp 17Inspite of the fact that silver nitrate (AgNO3MW = 169.87) is considered a soluble salt, it does have a limited solubility in water. The maximum solubility of AgNO3is 206g in 100 mL of water at 25oC.