9. Using pure water, 1.0 M NACI, and 1.0 M CaCl,: a) List the substances in decreasing melting point b) List the substances in increasing boiling point

Select the correct statement about cryoscopic constant. O It relates molality to freezing point elevation. O It relates molarity to freezing point elevation. O It relates molarity to freezing point depression. O The other statements are false. O It relates molality to freezing point depression.

0.0821 kg of biphenyl (C12H10) is dissolve in benzene (CHo) to create a solution with a total volume of 350.0 mL. (Assume the change in volume is negligible) a) What intermolecular forces are shared between biphenyl and benzene? b) If the boiling point of pure benzene is 80.1 °C, then what would be the boiling point of this solution in °C? (Kb for benzene is 2.53 °C/m and the density of benzene is 0.877 g/mL) c) If the vapor pressure of pure benzene is 24.4 kPa at 40.0 °C, then what will the vapor pressure of the solution be in kPa? (Consider biphenyl to be nonvolatile and the density of benzene is 0.877 g/mL) d) What would be the osmotic pressure (in atm) of this solution at 40.0 °C? Assume the density of the solution is the same as benzene, 0.877 g/mL.

18. A solution of 0.640 g of an organic compound (i-1) in 100.0 g of benzene boils at 80.23oC. The boiling point of benzene is 80.10oC; the Kb is 2.53 oC/molal. What is the molar masst of the compound? Group of answer choices 135 g/mol 125 g/mol 115 g/mol 145 g/mol   19. An aqueous solution of 0.864 g of a hormone in 100.0 mL of solution has an osmotic pressure of 0.195 atm at 25oC. What is the molecular weight of the hormone? Group of answer choices  1.08 x 104  1.08 x 103 8.20 x 102 8.20 x 103 0.990 x 103   20. What volume (mL) of 1.25 M AgNO3 should be used to prepare 250.0 mL of a 0.100 M solution? Group of answer choices 30.0 15.0 10.0 20.0     21. The density of a 3.00 M solution of KI is 1.350 g/cm3. What is the molality of the solution? Group of answer choices 5.26 2.56 5.32 3.52

25. A solution is made using 28.3 percent by mass CH₂Cl₂ in CHCl₃. At 30 °C, the vapor pressure of pure CH₂Cl₂ is 490 mm Hg, and the vapor pressure of pure CHCl₃ is 260 mm Hg. The normal boiling point of CHCl₃ is 61.7 °C.   F) What is the boiling point in  °C of the solution? (Kb for CHCl₃ is 3.67 °C/m).

A solution contains 17.83 grams of magnesium chloride and 811.7 grams of water.  What is the vapor pressure (in torr) of this solution at 40.00°C?  The vapor pressure of water at this temperature is 55.30 torr.  You should use the experimental value of the van't Hoff factor for this calculation.   (4 significant figures)

97. Consider an aqueous solution that freezes at -0.229°C and is composed of 4.00% by mass maltose. a) Calculate the molar mass of maltose. b) Explain what causes a solution to have a lower freezing point than pure solvent. c) Explain why an aqueous solution actually freezes over a broader temperature range than pure water (which freezes sharply at 0.00°C).

Given the following mixture of two compounds 45.00 mL of X (MW =82.00 g/mol)(density 1.077 g/mL) and 710.00 mL of Y (91.00 g/mol))(density 0.907 g/mL). The boiling point of pure Y is -18.00 degrees C. The molal boiling constant is 2.049 degrees C/m. What is the boiling point of the solution, in degrees C?

11. Why is the boiling point of 2 M NaCl solution higher than the boiling point of 1 M of NaCl solution? The 2 M NaCl solution has a higher vapor pressure and requires more energy to reach boiling point. The 2 M NaCl solution has a lower vapor pressure and requires more energy to reach boiling point. The 2 M NaCl solution has a lower vapor pressure and requires less energy to reach boiling point. The 2 M NaCl solution has a higher vapor pressure and requires less energy to reach boiling point.

Predict