Part B As a scuba diver descends under water, the pressure increases. At a total air pressure of 2.59 atm and a temperature of 25.0 °C, what is the solubility of N2 in a diver's blood? [Use the value of the Henry's law constant k calculated in Part A, 6.26 x 10-4 mol/(L · atm).JAssume that the composition of the air in the tank is the same as on land and that all of the dissolved nitrogen remains in the blood. Express your answer with the appropriate units. • View Available Hint(s) HẢ ? solubility = Value Units Part C The folowing solutions aro propared by dissolving the requisite amount of solute in water to obtain the desirad concentrations. Rank the solutions according to thoir rospactive osmatic pressures in deoreasing order ansuming the complete dissociation of ionic compounds. Rank from highest to lowest osmotic presaure. To rank itema as equivalent, overlap them. • View Avallable Hint(s) Reset Help 1M C, H0, 1M MgCl 2M CH,OH 1 M NACI Highest osmotic pressuro Lowest osmotic pressure

1) What is the molality of a solution prepared by dissolving 78.8  g of ethylene glycol, HOCH2CH2OH, in 1.45  L of water? Assume the density of water is 1.00 g/mL. 2)The concentrations of Al  and K  in a sample of riverwater are 0.0500 mg/kg and 1.30 mg/kg, respectively. Express the concentration in molality.   3) What molality of nonvolatile solute is needed to lower the melting point of camphor by 1.050°C? (Kf = 39.70ºC/m)   4) Determine the melting point of an aqueous solution containing 193 mg of saccharin (C7H5O3NS) added to 1.00 mL of water (density of water = 1.00 g/mL, Kf = 1.86°C/m).   5) Which one of the following aqueous solutions should have the lowest freezing point? a. 0.0150 m Na2SO4 b. 0.0300 m KBr c. 0.00500 m C6H12O6   5) From your predicted value of the van't Hoff factor, calculate the boiling point of a 1.64  m aqueous solution of barium nitrate, Ba(NO3)2. The Kb of water is 0.52°C/m.

The partial pressure of CO2, gas above the liquid in a bottle of champagne at 20 °C is 5.2 atm. What is the solubility of CO2, in champagne? Assume the Henry's law constant for CO2, is the same in champagne as it is in water: at 20 °C, kH =3.7 × 10^-2 mol Be sure to use the correct number of significant figures.

At 25.0 °C, 100.0 mL of an aqueous solution containing 45.2 mg of a molecular solute has an osmotic pressure of 18.4 Torr. The molar mass of the solute is ___ g/mol.