Ch. 14/15 Prep-Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1. The intermolecular forces between particles in a liquid can involve all of the following except a. London dispersion forces. c. dipole-dipole attractions. b. hydrogen bonding. d. gravitational forces. 2. The attractive forces in a liquid are a. strong enough to prevent the particles from changing positions. b. too weak to hold the particles in fixed positions. c. more effective than those in a solid. d. too weak to limit the movements of the particles. 3. What causes particles in a liquid to escape into a gas state? a. high kinetic energy c. surface tension b. a freezing temperature d. the combining of liquids 4. In general, most substances are a. least dense in the liquid state. c. less dense as solids than as liquids. b. more dense as gases than as solids. d. most dense in the solid state. 5. What causes the high density of solids? a. The particles are more massive than those in liquids. b. The intermolecular forces between particles are weak. c. The particles are packed closely together. d. The energy of the particles is very high. 6. A volatile liquid a. has strong attractive forces between particles. b. evaporates readily. c. has an odor. d. is ionic. 7. At pressures greater than 760 mm Hg, water will boil at a. a temperature higher than 100ºC. c. 100ºC. b. a temperature lower than 100ºC. d. 4ºC. 8. Why would a camper near the top of Mt. Everest find that water boils at less than 100ºC? a. There is greater atmospheric pressure than at sea level. b. The flames are hotter at that elevation. c. There is less atmospheric pressure than at sea level. d. The atmosphere has less moisture. 9. Carbon dioxide in water is an example of which solute-solvent combination? a. gas-liquid c. liquid-liquid b. liquid-gas d. cannot be determined 10. A metal solution is a(n) a. colloid. c. suspension. b. alloy. d. electrolyte. 1
11. Increasing the surface area between solute and solvent a. increases the rate of dissolution. b. decreases the rate of dissolution. c. has no effect on the rate of dissolution. d. can increase, decrease, or have no effect on the rate of dissolution. 12. Stirring increases the rate of dissolution because it a. raises the temperature. b. lowers the temperature. c. brings fresh solvent into contact with the solute. d. decreases surface area of the solute. 13. If the amount of solute present in a solution at a given temperature is less than the maximum amount that can dissolve at that temperature, the solution is said to be a. saturated. c. supersaturated. b. unsaturated. d. concentrated. 14. Which of the following is an example of a polar solvent? a. carbon tetrachloride c. water b. benzene d. gasoline 15. Which of the following is an example of a nonpolar solvent? a. water c. both a and b b. carbon tetrachloride d. neither a nor b 16. Which of the following is soluble in water? a. potassium nitrate c. benzene b. silver d. carbon tetrachloride 17. Sugar is soluble in water because sugar molecules are a. massive. c. nonpolar. b. large. d. polar. 18. Pressure has the greatest effect on the solubility of a. solids in liquids. c. gases in gases. b. liquids in liquids. d. gases in liquids. 19. What is the molarity of a solution that contains 1.5 mol KCl in 3.00 L solution? a. 0.5 M c. 0.4 M b. 4.5 M d. 1.5 M 20. What is the molarity of a solution that contains 20. g NaOH in 4.00 L solution? a. 0.13 M c. 8.0 M b. 0.50 M d. 20 M 21. How many moles of HCl are present in 0.50 L of a 2 M HCl solution? a. 1.0 mol c. 0.5 mol b. 2.0 mol d. 2.0 mol 22. An NaOH solution contains 2 mol of NaOH, and its concentration is 0.5 M. What is its volume? a. 0.5 L c. 1.05 L b. 0.2 L d. 4.0 L 23. What causes water's low vapor pressure? a. dispersion forces c. hydrogen bonding b. covalent bonding d. ionic attractions 2
24. Which of the following usually makes a substance dissolve faster in a solvent? a. agitating the solution b. increasing the particle size of the solute c. lowering the temperature d. decreasing the number of particles 25. What is the molarity of a solution that contains 6 moles of solute in 2 liters of solution? a. 6 M c. 7 M b. 12 M d. 3 M 26. What is the molarity of 200 ml of solution in which 2.0 moles of sodium bromide is dissolved? a. 2.0 M c. 0.40 M b. 10 M d. 4.0 M 27. The amount of heat needed to melt one mole of a solid at a constant temperature is called. a. molar heat of vaporization c. heat of reaction b. molar heat of fusion d. enthalpy 28. During a phase change, the temperature of a substance. a. increases c. remains constant b. decreases d. may increase or decrease 29. In a metallic bond, electrons are. a. held tightly. c. held loosely and flow freely. b. not shared. d. paired evenly. 30. A solution of sugar contains 35 grams of sucrose, C 12 H 22 O 11 in 100 ml of solution. What is the concentration in parts per million of the solution? a. 25 ppm c. 5,000,000 ppm b. 350,000 ppm d. 0.76 ppm 31. What is going on in the area between D and E? a. melting c. condensing b. freezing d. boiling 32. What phase(s) of matter are present between C and D? a. Solid c. liquid b. liquid and solid d. liquid and gas 33. A KCl solution contains 149.1 g of KCl (molar mass 74.55 g/mol) in 4000 ml of solution. What units do the amount of solute and the volume of solution need to be in to obtain the molarity of 0.5 M? a. mol and L c. grams and L b. grams and mol d. mol and cubic centimeters 3
34. Which of the following is true about ionic crystals? a. They consist of molecules held together by intermolecular forces. c. Their structure consists of positive and negative ions arranged in a regular pattern. b. They are polar. d. They are atomic solids. 35. Liquid in a sealed container kept at constant pressure will show no change in its vapor pressure. Why is this? a. particles stay in the liquid form and do c. gas particles above the liquid do not not vaporize into gas b. liquid and gas particles are condensing and vaporizing at the same rate producing an equilibrium condense into liquid d. none of these 36. 40 g of NaCl at 50 C in 100g of water would be considered a(n) solution. a. saturated c. supersaturated b. unsaturated d. none of these 37. 85 g of NaNO 3 at 15 C in 100 g of water would be considered a(n) solution. a. saturated c. supersaturated b. unsaturated d. none of these 4
ID: A Ch. 14/15 Prep-Test Answer Section MULTIPLE CHOICE 1. ANS: D PTS: 1 DIF: I OBJ: 12-1.1 2. ANS: B PTS: 1 DIF: I OBJ: 12-1.1 3. ANS: A PTS: 1 DIF: I OBJ: 12-1.2 4. ANS: D PTS: 1 DIF: I OBJ: 12-2.1 5. ANS: C PTS: 1 DIF: I OBJ: 12-2.1 6. ANS: B PTS: 1 DIF: I OBJ: 12-3.3 7. ANS: A PTS: 1 DIF: I OBJ: 12-3.4 8. ANS: C PTS: 1 DIF: II OBJ: 12-3.4 9. ANS: A PTS: 1 DIF: II OBJ: 13-1.2 10. ANS: B PTS: 1 DIF: I OBJ: 13-1.3 11. ANS: A PTS: 1 DIF: I OBJ: 13-2.1 12. ANS: C PTS: 1 DIF: I OBJ: 13-2.1 13. ANS: B PTS: 1 DIF: I OBJ: 13-2.2 14. ANS: C PTS: 1 DIF: II OBJ: 13-2.3 15. ANS: B PTS: 1 DIF: II OBJ: 13-2.3 16. ANS: A PTS: 1 DIF: II OBJ: 13-2.3 17. ANS: D PTS: 1 DIF: I OBJ: 13-2.3 18. ANS: D PTS: 1 DIF: I OBJ: 13-2.5 19. ANS: A PTS: 1 DIF: III OBJ: 13-3.1 20. ANS: A PTS: 1 DIF: III OBJ: 13-3.1 21. ANS: A PTS: 1 DIF: III OBJ: 13-3.2 22. ANS: D PTS: 1 DIF: III OBJ: 13-3.3 23. ANS: C PTS: 1 DIF: L1 REF: p. 447 OBJ: 15.1.1 STA: Ch.2.h 24. ANS: A PTS: 1 DIF: L2 REF: p. 471 p. 472 OBJ: 16.1.1 STA: Ch.6.b 25. ANS: D PTS: 1 DIF: L1 REF: p. 481 OBJ: 16.2.1 STA: Ch.6.d 26. ANS: B PTS: 1 DIF: L2 REF: p. 481 OBJ: 16.2.1 STA: Ch.6.d 27. ANS: B PTS: 1 DIF: L1 REF: p. 520 OBJ: 17.3.1 STA: Ch.7.d 28. ANS: C PTS: 1 DIF: L1 REF: p. 520 OBJ: 17.3.1 STA: Ch.7.d 29. ANS: C PTS: 1 30. ANS: B PTS: 1 31. ANS: D PTS: 1 32. ANS: C PTS: 1 33. ANS: A PTS: 1 34. ANS: C PTS: 1 35. ANS: B PTS: 1 1
ID: A 36. ANS: B PTS: 1 37. ANS: A PTS: 1 2