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1-propanol (P1 degree = 20.9 Torr at 25 degree C) and 2-propanol (P2 degree = 45.2 Torr at 25 degree C) form ideal solutions in all proportions. Let x1 and X2 represent the mole fractions of 1-propanol and 2-propanol in a liquid mixture, respectively, and y1 and y2 represent the mole fractions of each in the vapor phase. For a solution of these liquids with X1 = 0.340, calculate the composition of the vapor phase at 25 degree C. In reverse osmosis, water flows out of a salt solution until the osmotic pressure of the solution equals the applied pressure. If a pressure of 78.0 bar is applied to seawater, what will be the final concentration of the seawater at 20 degree C when reverse osmosis stops? Assuming that seawater has a total ion concentration (a.k.a colligative molarity) of 1.10 Mc, calculate how many liters of seawater are needed to produce 38.4 L of fresh water at 20 degree C with an applied pressure of 78.0 bar. Intravenous, or IV solutions used in medicine must exert the same osmotic pressure as blood to prevent a net flow of water into or out of the blood cells. The proper concentration for an intravenous NaCl solution is 0.90 g NaCI per 100. mL of water (sometimes refered to as 0.90% m/v). If the van't Hoff factor of NaCI is i = 1.8, what is the osmotic pressure of blood at body temperature, 37 degree C? When 4.36 g of a nonelectrolyte solute is dissolved in 585 mL of water at 24 degree C, the resulting solution exerts an osmotic pressure of 963 torr. What is the molar concentration of the solution? How many moles of solute are in the solution? What is the molar mass of the solute? Assuming 100% dissociation, calculate the freezing point and boiling point of 1.88 m K3PO4(aq). Constants may be found here. The boiling point of an aqueous solution is 101.08 degree C. What is the freezing point? Constants can be found here. Quinine is a natural product extracted from the bark of the cinchona tree, which is native to South America. Quinine is used as an antimalarial agent. When 2.55 g of quinine is dissolved in 25.0 g of cyclohexane, the freezing point of the solution is lowered by 6.55 degree C. The freezing point and Kf constant for cyclohexane can be found here. Calculate the molar mass of quinine. A solution is made by dissolving 0.740 mol of nonelectrolyte solute in 767 g of benzene. Calculate the freezing point and boiling point of the solution. Constants may be found here. A solution is made by mixing 33.0 mL of ethanol, C2H6O, and 67.0 mL of water. Assuming ideal behavior, what is the vapor pressure of the solution at 20 degree C? Given that the vapor pressure of water is 17.54 Torr at 20 degree C, calculate the vapor-pressure lowering of aqueous solutions that are 2.50 m in (a) sucrose, C12H22O11, and (b) calcium chloride. Assume 100% dissociation for electrolytes. sucrose, C12H22O11 calcium chloride Biphenyl, C12H10, is a nonvolatile, nonionizing solute that is soluble in benzene, CeH6. At 25 degree C, the vapor pressure of pure benzene is 100.84 torr. What is the vapor pressure of a solution made from dissolving 14.1 g of biphenyl in 34.0 g of benzene? At 298 K, the Henry's law constant for oxygen is 0.00130 M/atm. Air is 21.0% oxygen. At 298 K, what is the solubility of oxygen in water exposed to air at 1.00 atm? At 298 K, what is the solubility of oxygen in water exposed to air at 0.891 atm? If atmospheric pressure suddenly changes from 1.00 atm to 0.891 atm at 298 K, how much oxygen will be released from 4.70 L of water in an unsealed container? At 25 degree C and 775 Torr, carbon dioxide has a solubility of 0.0347 M in water. What is its solubility at 25 degree C and 1750 Torr? Express the concentration of a 0.0780 M aqueous solution of fluoride, F-, in mass percentage and in parts per million. Assume the density of the solution is 1.00 g/mL. You need to dissolve CaCl2 in water to make a mixture that is 30.5% calcium chloride by mass. If the total mass of the mixture is 345.4 g, what masses of CaCl2 and water should be used? 8.60 g of NH4Cl is added to 10.6 g of water. Calculate the molality of the solution. When a 6.00-g sample of KBr is dissolved in water in a calorimeter that has a total heat capacity of 4.181 kJ middot K-1, the temperature decreases by 0.240 K. Calculate the molar heat of solution of KBr. In an ionic compound, the size of the ions affects the internuclear distance (the distance between the centers of adjacent ions), which affects lattice energy (a measure of the force need to pull ions apart), which affects the enthalpy of solution. Based on ion sizes, rank these compounds by their expected heats of solution.

Explanation / Answer

1) P = x1P1 + x2P2

P= 0.34 x 20.1 + 0.66 x 45.2

P= 36.666

y1 = x1p1/P

y1 = 0.34 x 20.1 / 36.66

y1 = 0.186

y2 = 0.813

2) P =MRT

conc M = 78 / 760 x 0.0821 x 293

M = 4.266 x 10-3

38.4 L = 38.4 kg

moalrity = moles /volume

volume = 38.4 x 1000/ 18 x 1.10

volume =1939.39 L

So 1939.39 L of sea water is required .

3) p = i MRT

p= 1.8 x 0.90 x 1000 x 0.0821 x 310 / 100 x 58.5

P = 7.047 atm

4) 963 /760 = M x 0.0821 x 297

M = 0.0519

molar conc is 0.0519 M

moles = 0.0519 x 585 /1000 = 0.0304

moles is 0.0304

6) 1.08 /dTb = 0.512 / -1.86

Tb=3.923

freezing point is -3.923 C

7) 6.55 = m x 20.2

m = 0.32425

2.55 x 1000 / M x 25 =0.32425

M = 314.56

molar mass is 314.56 grams

8) molality = 0.740 x 1000/ 767 = 0.96479

dTb = 0.96479 x 2.65

Tb = 82.656 C

Tf = 0.56 C

9) mass of ethanol = 33 x 0.789 = 26.037

moles of ethanol = 26.037 / 46 = 0.566

mass of water = 67 x 0.998 = 66.866

moles of water = 66.866 / 18 = 3.714

Total pressure = 5.805 + 15.185 = 20.99

vapour pressure is 20.99

11) moles of bi phenyl = 14.1 / 154 = 0.091558

moles of benzene = 0.4359

vapour pressure = 83.336 torr

12) solubilty = 0.0013

solubility = 0.001158

moles = 0.0209

13)

S1/S2 = P1/P2

S2 = 1750 x 0.0347 / 775 = 0.07835

the solubility is 0.07835

14) mass % = molairty x M.w / density

mass % = 0.1482

ppm = 1482

15) mass of calc2 = 345.4 x 30.5 /100 = 105.347

mass of CaCl2 = 105.347 grams

mass of H20= 240.053 grams

16) molality = ( moles of solute / mass of solvnet )

molality = 8.60 x 1000 / 53.5 x 10.6

molality = 15.16

17) heat = 19.90 kJ /mol

18) most exothermic KF , Kcl ,Kbr ,Ki most endothermic

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