Adamson UniversityCollege of Engineering

Chemical Engineering Department

Colligative PropertiesLQ3

1) Which of the following mixtures have components which can be separated by filtration?A) colloidsB) solutionsC) suspensionsD) all of the above2) In most liquid solutions, the component present in the larger amount is called theA) dispersed medium.B) emulsifying agent.C) solute.D) solvent.3) The rubbing alcohol sold in drug stores often is composed of 70% isopropyl alcohol and 30% water. In this solutionA) isopropyl alcohol is the solvent.B) water is the solvent.C) both water and isopropyl alcohol are solvents.D) neither water nor isopropyl alcohol is a solvent.

4) 10 grams of table sugar (sucrose, ) is dropped into a beaker containing 100 grams of water and stirred until a clear liquid is visible and all of the sugar has dissolved. This process may be described as A) the formation of a heterogeneous mixture.B) the formation of a homogeneous solution.C) sublimation.D) the formation of a chemical compound.5) Iodine, I2(s), is more soluble in dichloromethane, CH2Cl2(l), than in

water becauseA) both iodine and dichloromethane have strong ion-dipole interactions.B) the dipole-dipole forces in dichloromethane are much stronger than the dispersion forces in iodine.C) the intermolecular forces are similar in both iodine and dichloromethane.D) iodine is polar and dichloromethane has a large number of hydrogen bonds.6) Which of the following pairs of liquids are likely to be miscible?

A) OH and O

B) and O

C) and O

D) and O7) Molarity is defined as moles of solute perA) kilogram of solvent.B) liter of solution.C) mole of solvent.D) total moles present.8) Which concentration becomes smaller as the temperature is increased from 20°C to 80°C?A) mass %B) molalityC) molarityD) mole fraction9) A saturated solution is defined asA) a concentrated solution.B) a solution that is in equilibrium with pure solvent.C) a solution than is in equilibrium with undissolved solute.D) a solution that is in equilibrium with both pure solvent and undissolved solute.10) Which of the following does not affect the solubility of a solute in a given solvent?A) polarity of the soluteB) polarity of the solvent

C) rate of stirringD) temperature of the solvent and solute11) Which of the following statements is true for a supersaturated solution?A) The solute in the solution is at equilibrium with undissolved solute.B) The solution contains more than the equilibrium amount of solute.C) The solution is stable and the solute will not precipitate.D) A supersaturated solution is more than 50% solute by mass.12) Which of the following is not an application of colligative properties?A) adding silver to mercury to lower the vapor pressure of mercuryB) desalinating sea water by reverse osmosisC) melting snow by application of saltD) reduced boiling points of pure liquids at increased altitudes13) Two aqueous solutions, A and B, are separated by a semipermeable membrane. The osmotic pressure of solution A immediately begins to decrease. Which of the following statements is true?A) Solvent molecules are moving from solution B into solution A.B) The initial osmotic pressure of solution B is greater than that of solution A.C) The solvent molecules are moving from the solution of higher osmotic pressure to that of lower osmotic pressure.D) Both B and C are true statements.14) A solution is prepared by dissolving 40.0 g of sucrose, C12H22O11,

in 250. g of water at 25°C. What is the vapor pressure of the solution if the vapor pressure of water at 25°C is 23.76 mm Hg?A) 0.198 mm HgB) 20.5 mm HgC) 23.6 mm HgD) 24.0 mm Hg15) Naproxen is a commercially important anti-inflammatory agent that can be isolated from the thyroid gland. A solution of 1.138 g of naproxen in 25.00 g benzene has an osmotic pressure of 4.00 atm at 20°C. The density of benzene is 0.8787 g/mL at this temperature. Calculate the molar mass of naproxen, assuming it remains intact upon dissolution and the density of the solution equals the density of pure benzene.A) 176 g/molB) 230 g/molC) 307 g/mol

D) 3.80 × 105 g/molProblem Part:1. (10 points)

2. (20 points)

3. (20 points)

4. (10 points)