ch 13 chem

37) A 4.55 L sample of water contains 0.115 g of sodium ions. Determine the concentration of sodium ions in ppm if the density of the solution is 1.00 g/mL. A) 52.3 ppm B) 13.2 ppm C) 12.7 ppm D) 25.3 ppm E) 36.5 ppm

D) 25.3 ppm

51) An aqueous solution has a normal boiling point of 103.0°C. What is the freezing point of this solution? For water Kb = 0.51°C/m and Kf = 1.86°C/m. A) -0.82°C B) - 3.0°C C) -3.6°C D) - 11°C

D) - 11°C

67) What is the freezing point of a solution of 7.15 g MgCl2 in 100 g of water? Kf for water is1.86°C/m. A) -0.140°C B) - 1.40°C C) - 2.80°C D) - 4.18°C

D) - 4.18°C

60) Which of the following solutions will have the lowest freezing point? A) 0.010 m K Br B) 0.010 m Na2CO3 C) 0.035 m CH3CH2OH D) 0.015 m BaCl2

D) 0.015 m BaCl2

21) Calculate the mole fraction of the total ions in an aqueous solution prepared by dissolving 0.400 moles of Ca F2 in 850.0 g of water. A) 0.00841 B) 0.0270 C) 0.00900 D) 0.0248 E) 0.0167

D) 0.0248

31) A solution is 0.0480 m LiF. What is the molarity of the solution if the density is 1.10 g/mL? A) 0.0441 M B) 0.0480 M C) 0.0436 M D) 0.0528 M E) 0.0417 M

D) 0.0528 M

14) Determine the solubility of CO2 in soda water at 25°C if the pressure of CO2 is 5.6 atm. The Henry's law constant for carbon dioxide in water at this temperature is 3.4 × 10-2 M/atm. A) 0.16 M B) 0.53 M C) 0.61 M D) 0.19 M E) 0.78 M

D) 0.19 M

28) What is the molality of a glucose solution prepared by dissolving 18.0 g of glucose, C6H12O6, in 125.9 g of water? A) 7.94 × 10-4 m B) 0.143 m C) 0.695 m D) 0.794 m

D) 0.794 m

30) A solution is prepared by dissolving 98.6 g of NaCl in enough water to form 875 mL of solution. Calculate the mass % of the solution if the density of the solution is 1.06 g/mL. A) 11.3% B) 12.7% C) 9.4% D) 10.6% E) 11.9%

D) 10.6%

55) Determine the vapor pressure of a solution at 55°C that contains 34.2 g NaCl in 375 mL of water. The vapor pressure of pure water at 55°C is 118.1 torr. The van't Hoff factor for NaCl is 1.9. A) 115 torr B) 87.1 torr C) 108 torr D) 112 torr E) 92.8 torr

D) 112 torr

52) A solution is prepared by adding 30.00 g of lactose (milk sugar) to 110.0 g of water at 55°C. The partial pressure of water above the solution is ________ torr. The vapor pressure of pure water at 55°C is 118.0 torr. The MW of lactose is 342.3 g/mol. A) 1.670 B) 94.1 C) 169.4 D) 116.3 E) 92.7

D) 116.3

27) Calculate the molality of a solution that is prepared by mixing 25.5 mL of CH3OH (d = 0.792 g/mL) and 387 mL of CH3CH2CH2OH (d = 0.811 g/mL). A) 0.630 m B) 0.812 m C) 1.57 m D) 2.01 m E) 4.98 m

D) 2.01 m

6) The Henry's law constant for helium gas in water at 30°C is 3.70 × 10-4 M/atm. When the partial pressure of helium above a sample of water is 0.650 atm, the concentration of helium in the water is ________ M. A) 5.69 × 10-4 B) 1.76 × 103 C) 1.30 -4 D) 2.41 × 10-4 E) 3.70 × 10-4

D) 2.41 × 10-4

56) The boiling point of an aqueous 1.83 m (NH4)2SO4 (molar mass = 132.15 g/mol) solution is 102.5°C. Determine the value of the van't Hoff factor for this solute if the Kb for water is 0.512°C/m. A) 3.0 B) 3.6 C) 1.8 D) 2.7 E) 2.3

D) 2.7

24) What volume of a 0.716 M KBr solution is needed to provide 30.5 g of KBr? A) 21.8 mL B) 42.7 mL C) 184 mL D) 357 mL

D) 357 mL

60) how many grams of CCl4 are needed to make a 1.20 m solution in 450g of octane? A) 127.4 g B) 184.6 g C) 221.5 g D) 83.06 g E) 62.22 g

D) 83.06 g

54) Calculate the freezing point of a solution containing 5.0 grams of KCl and 550.0 grams of water. The molal-freezing-point-depression constant (Kf) for water is 1.86°C/m. A) -0.45 oC B) +0.45 oC C) -0.23 oC D) +0.23 oC E) 1.23 oC

A) -0.45 oC

47) Determine the freezing point of a solution that contains 62.8 g of urea (CH4N2O) dissolved in 275 g of water (Kf= 1.86°C/m). A) -7.07°C B) -4.82°C C) -13.1°C D) -3.01°C E) -9.12°C

A) -7.07°C

22) Calculate the mole fraction of Ba I2 in an aqueous solution prepared by dissolving 0.400 moles of Ba I2 in 850.0 g of water. A) 0.00841 B) 0.0270 C) 0.00900 D) 0.0248 E) 0.0167

A) 0.00841

36) What is the mol fraction of ethanol, C2H5OH, in a solution of 75.3g of ethanol and 525g of water? A) 0.0531 B) 0.127 C) 0.947 D) 0.239 E) 0.0237

A) 0.0531

5) The Henry's Law constant of methyl bromide, CH3Br, is k = 0.159 mol/(L ∙ atm) at 25°C. What is the solubility of methyl bromide in water at 25°C and at a partial pressure of 270. mm Hg? A) 0.0565 mol/L B) 0.355 mol/L C) 0.448 mol/L D) 42.9 mol/L

A) 0.0565 mol/L

40) What is the mole fraction of I2 in a solution made by dissolving 55.6 g of I2 in 245 g of hexane, C6H14? A) 0.0715 B) 0.0770 C) 0.133 D) 0.154

A) 0.0715

38) A solution of LiCl in water is 20.0 wt% LiCl. What is the mole fraction of LiCl? A) 0.0960 B) 0.106 C) 0.472 D) 4.44

A) 0.0960

61) Choose the aqueous solution that has the highest boiling point. These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable. A) 0.100 m AlCl3 B) 0.100 m Li Br C) 0.100 m Ba Cl2 D) 0.100 m C6H12O6 E) They all have the same boiling point.

A) 0.100 m AlCl3

39) What is the mole fraction of ethanol in a solution made by dissolving 29.2 g of ethanol, C2H5OH, in 53.6 g of water? A) 0.176 B) 0.213 C) 0.352 D) 0.545

A) 0.176

29) Determine the molality of an aqueous solution prepared by dissolving 0.112 moles of LiCl in 13.7 moles of H2O. A) 0.454 m B) 0.220 m C) 0.818 m D) 0.122 m E) 0.153 m

A) 0.454 m

19) Calculate the molarity of a solution that contains 0.250 moles of K F in enough water to give 0.500 L of solution. A) 0.500 M B) 2.00 M C) 0.125 M D) 8.00 M E) 0.750

A) 0.500 M

73) What is the osmotic pressure of a solution containing 541 mg of aspartame (C14H18N2O5) in a total volume of 60.0 mL of water at 25°C? A) 0.749 atm B) 1.14 atm C) 2.35 atm D) 0.0624 atm

A) 0.749 atm

49) Calculate the boiling point of a solution of 500.0 g of ethylene glycol (C2H6O2) dissolved in 500.0 g of water. Kf = 1.86°C/m and Kb = 0.512°C/m. Use 100°C as the boiling point of water. A) 108°C B) 92°C C) 130°C D) 70°C E) 8.3°C

A) 108°C

62) What is the osmotic pressure of a solution of 55.8 g of sucrose (C12H22O11) in 200 mL of water at room temperature? A) 19.9 atm B) 1.67 atm C) 6.27 atm D) 11.5 atm E) 14.4 atm

A) 19.9 atm

24) What mass (in g) of NH3 must be dissolved in 475 g of methanol to make a 0.250 m solution? A) 2.02 g B) 4.94 g C) 1.19 g D) 8.42 g E) 1.90 g

A) 2.02 g

44) At 20°C, a 2.32 M aqueous solution of ammonium chloride has a density ofWhat is the molality of ammonium chloride in the solution? The formula weight of NH4Cl is 53.50 g/mol. A) 2.55 B) 0.0449 C) 2.32 D) 0.446 E) 12.00

A) 2.55

20) What mass of CuCl2 is contained in 90.85 g of a 22.4% by mass solution of CuCl2 in water? A) 20.4 g B) 4.91 g C) 24.6 g D) 40.6 g

A) 20.4 g

75) At room temperature and 1 atm, the vapor pressure of isobutyl benzoate is 237 mm Hg, and the vapor pressure of vinyl acetate is 72.5 mm Hg. What is the total vapor pressure over a solution composed of these two substances when Xisobutyl benzoate = 0.850. A) 212 mm Hg B) 118 mm Hg C) 97.2 mm Hg D) 146 mm Hg

A) 212 mm Hg

54) A 150.0 mL sample of an aqueous solution at 25°C contains 15.2 mg of an unknown nonelectrolyte compound. If the solution has an osmotic pressure of 8.44 torr, what is the molar mass of the unknown compound? A) 223 g/mol B) 294 g/mol C) 341 g/mol D) 448 g/mol E) 195 g/mol

A) 223 g/mol

34) A solution is prepared by dissolving 38.6 g sucrose (C12H22O11) in 495 g of water. Determine the mole fraction of sucrose if the final volume of the solution is 508 mL. A) 4.09 × 10-3 B) 7.80 × 10-2 C) 1.28 × 10-3 D) 7.23 × 10-2 E) 2.45 × 10-3

A) 4.09 × 10-3

20) Calculate the mass of oxygen (in mg) dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air. Assume the mole fraction of oxygen in air to be 0.21 given that kH for O2 is 1.3 × 10-3 M/ atm at this temperature. A) 49.4 mg B) 23.5 mg C) 9.87 mg D) 27.3 mg E) 13.7 mg

A) 49.4 mg

19) A sealed container contains 0.352 L of water with an atmosphere of oxygen gas. What is the concentration of O2 in the water if the external pressure is 4.24 atm given that kH for O2 is 1.66 × 10-6 M/mm Hg at this temperature? A) 5.34 × 10-3 M B) 1.53 × 10-3 M C) 9.46 × 10-2 M D) 5.34 × 10-2 M E) 3.82 × 10-4 M

A) 5.34 × 10-3 M

18) Determine the Henry's law constant for ammonia in water at 25°C if an ammonia pressure of 0.022 atm produces a solution with a concentration of 1.3 M. A) 59 M/atm B) 0.017 M/atm C) 0.029 M/atm D) 35 M/atm E) 0.038 M/atm

A) 59 M/atm

1) Choose the statement below that is TRUE. A) A solution will form between two substances if the solute-solvent interactions are of comparable strength to the solute-solute and solvent-solvent interactions. B) A solution will form between two substances if the solute-solvent interactions are small enough to be overcome by the solute-solute and solvent-solvent interactions. C) A solution will form between two substances if the solute-solute interactions are strong enough to overcome the solvent-solvent interactions. D) A solution will form between two substances only if the solvent-solvent interactions are weak enough to overcome the solute-solvent interactions. E) None of the above are true.

A) A solution will form between two substances if the solute-solvent interactions are of comparable strength to the solute-solute and solvent-solvent interactions.

56) Place the following aqueous solutions of nonvolatile, nonionic compounds in order of decreasing osmotic pressure. I. 0.011 M sucrose II. 0.00095 M galactose III. 0.0060 M glycerin A) I > III > II B) I > II > III C) II > III > I D) III > I > II E) II > I > III

A) I > III > II

10) Identify the compound whose solubility decreases with increasing temperature. A) Na2SO4 B) K2Cr2O7 C) NaNO3 D) KClO3 E) CaCl2

A) Na2SO4

52) Give the reason that antifreeze is added to a car radiator. A) The freezing point is lowered and the boiling point is elevated. B) The freezing point is elevated and the boiling point is lowered. C) The freezing point and the boiling point are elevated. D) The freezing point and the boiling point are lowered. E) None of the above.

A) The freezing point is lowered and the boiling point is elevated.

10) Choose the situation below that would result in an endothermic ΔHsolution. A) When solute > hydration B) When solute < hydration C) When solute is close to hydration D) When solvent >> solute E) There isn't enough information to determine.

A) When solute > hydration

5) Identify the polar solvent. A) acetone B) hexane C) diethyl ether D) toluene E) carbon tetrachloride

A) acetone

12) A solution containing less than the equilibrium amount is called A) an unsaturated solution. B) a dilute solution. C) a supersaturated solution. D) a concentrated solution. E) a saturated solution.

A) an unsaturated solution.

11) Identify the gas that is dissolved in carbonated sodas. A) carbon dioxide B) hydrogen C) neon D) carbon monoxide E) argon

A) carbon dioxide

47) Choose the solvent below that would show the greatest boiling point elevation when used to make a 0.10 m nonelectrolyte solution. A) carbon tetrachloride, Kb = 5.03°C/m B) benzene, Kb = 2.53°C/m C) diethyl ether, Kb = 2.02°C/m D) water, Kb = 0.512°C/m E) acetic acid, Kb = 3.07°C/m

A) carbon tetrachloride, Kb = 5.03°C/m

4) Give the major force between acetone and chloroform. A) dipole-dipole B) dispersion C) hydrogen bonding D) ion-ion E) ion-dipole

A) dipole-dipole

57) Fluids used for an intravenous transfusion must be ________ with bodily fluids. A) isosmotic B) hyperosmotic C) hyposmotic D) neosmotic E) magnosmotic

A) isosmotic

70) In an ________ solution, red blood cells ________. A) isosmotic, have a normal shape B) hyperosmotic, have a normal shape C) hyposmotic, lose water and shrivel D) isosmotic, lose water and shrivel E) isosmotic, swell and may burst

A) isosmotic, have a normal shape

22) Give the term for the amount of solute in moles per kilogram of solvent. A) molality B) molarity C) mole fraction D) mole percent E) mass percent

A) molality

59) Identify the solute with the lowest van't Hoff factor. A) nonelectrolyte B) K I C) MgSO4 D) Ca Cl2 E) AlCl3

A) nonelectrolyte

7) Dynamic equilibrium can be defined as A) rate of dissolution = rate of deposition. B) rate of dissolution < rate of deposition. C) rate of dissolution > rate of deposition. D) rate of bubbling > rate of dissolving E) rate of condensing > rate of bubbling

A) rate of dissolution = rate of deposition.

16) A solid can be purified through what technique? A) recrystallization B) dilution C) dissolution D) boiling E) melting

A) recrystallization

48) Calculate the freezing point of a solution of 500.0 g of ethylene glycol (C2H6O2) dissolved in 500.0 g of water. Kf = 1.86°C/m and Kb = 0.512°C/m. A) 30.0°C B) -30.0°C C) 8.32°C D) -8.32°C E) 70.2°C

B) -30.0°C

65) Choose the aqueous solution below with the lowest freezing point. These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable. A) 0.075 m Li Cl B) 0.075 m (NH4)3PO4 C) 0.075 m NaBrO4 D) 0.075 m KCN E) 0.075 m KNO2

B) 0.075 m (NH4)3PO4

62) Choose the aqueous solution that has the highest boiling point. These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable. A) 0.100 mKNO2 B) 0.100 m Li2SO4 C) 0.200 m C3H8O3 D) 0.060 m Li3PO4 E) They all have the same boiling point.

B) 0.100 m Li2SO4

61) A student makes a solution containing 125g of acetonitrile (CH3CN) and 300g of water. What is the mol fraction of acetonitrole? A) 0.845 B) 0.155 C) 0.294 D) 0.706 E) 0.0453

B) 0.155

41) What is the mole fraction of oxygen in a gas mixture that is 37% oxygen and 63% nitrogen by volume? A) 0.34 B) 0.37 C) 0.25 D) 0.52

B) 0.37

74) What is the mole fraction of acetone, (CH3)2CO, in a solution containing 500 g of acetone in 800 g of benzene, C6H6? A) 0.841 B) 0.457 C) 0.314 D) 0.227

B) 0.457

34) A solution is prepared by dissolving 16.2 g of benzene (C6H6) in 282 g of carbon tetrachloride (CCl4). The concentration of benzene in this solution is ________ molal. The molar masses of C6H6 and CCl4 are 78.1 g/mol and 154 g/mol, respectively. A) 7.36 × 10-4 B) 0.736 C) 0.102 D) 0.0543 E) 5.43

B) 0.736

29) To make a 2.00 m solution, one could take 2.00 moles of solute and add A) 1.00 L of solvent. B) 1.00 kg of solvent. C) enough solvent to make 1.00 L of solution. D) enough solvent to make 1.00 kg of solution.

B) 1.00 kg of solvent.

35) A solution is prepared by dissolving 76.3 g NaI in 545 g of water. Determine the mole fraction of NaI if the final volume of the solution is 576 mL. A) 6.04 × 10-3 B) 1.65 × 10-2 C) 1.40 × 10-3 D) 1.32 × 10-2 E) 8.84 × 10-2

B) 1.65 × 10-2

45) Determine the freezing point depression of a solution that contains 30.7 g glycerin (C3H8O3, molar mass = 92.09 g/mol) in 376 mL of water. Some possibly useful constants for water are Kf = 1.86°C/m and Kb = 0.512°C/m. A) 0.887°C B) 1.65°C C) 2.18°C D) 3.33°C E) 0.654°C

B) 1.65°C

39) Commercial grade HCl solutions are typically 39.0% (by mass) HCl in water. Determine the molality of the HCl, if the solution has a density of 1.20 g/mL. A) 39.0 m B) 17.5 m C) 6.39 m D) 10.7 m E) 9.44 m

B) 17.5 m

69) A KCl solution is prepared by dissolving 25.0 g KCl in 250.0 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) 21.6 mm Hg B) 22.7 mm Hg C) 23.2 mm Hg D) 24.9 mm Hg

B) 22.7 mm Hg

42) A solution is 2.25% by weight NaHCO3. How many grams of NaHCO3 are in 150.0 g of solution? A) 1.50 g B) 3.38 g C) 66.7 g D) 225 g

B) 3.38 g

26) How many moles of KF are contained in 244 mL of 0.135 m KF solution? The density of the solution is 1.22 g/mL. A) 4.31 × 10-2 mol KF B) 4.02 × 10-2 mol KF C) 3.29 × 10-2 mol KF D) 2.32 × 10-2 mol KF E) 1.67 × 10-2 mol KF

B) 4.02 × 10-2 mol KF

53) A compound is found to have a molar mass of 598 g/mol. If 35.8 mg of the compound is dissolved in enough water to make 175 mL of solution at 25°C, what is the osmotic pressure of the resulting solution? A) 3.42 torr B) 6.36 torr C) 5.01 torr D) 5.99 torr E) 8.36 torr

B) 6.36 torr

44) Determine the vapor pressure of a solution at 25°C that contains 85.3 g of naphthalene (C10H8) in 540 g of benzene (C6H6). The vapor pressure of benzene at 25°C is 74.6 torr. A) 74.6 toff. B) 68.0 torr. C) 54.9 torr. D) 7.52 torr. E) 22.4 toff.

B) 68.0 torr.

37) How much water must be added to 40.0 g of CaCl2 to produce a solution that is 35.0 wt% CaCl2? A) 54.0 g B) 74.2 g C) 87.5 g D) 114 g

B) 74.2 g

59) What is the molecular weight of a polymer if 3.50 g are dissolved in enough water to give 252 mL of the solution and give a osmotic pressure of 28.52 mm Hg at 25°C? A) 6.49 × 105 g/mol B) 9.05 × 103 g/mol C) 2.63 × 103 g/mol D) 28.5 g/mol E) 8.88 × 104 g/mol

B) 9.05 × 103 g/mol

4) Which cation in each set is expected to have the larger (more negative) hydration energy? I Be2+ or Ca2+ II Rb+ or Zn2+ A) Be2+ in set I and Rb+ in set II B) Be2+ in set I and Zn2+ in set II C) Ca2+ in set I and Rb+ in set II D) Ca2+ in set I and Zn2+ in set II

B) Be2+ in set I and Zn2+ in set II

12) Which of the following should have the largest Henry's law constant (kH) in water? A) Ne B) CO C) Br2 D) CH3CH3 E) CO2

B) CO

17) Which of the following statements is TRUE? A) In general, the solubility of a solid in water decreases with increasing temperature. B) In general, the solubility of a gas in water decreases with increasing temperature. C) The solubility of a gas in water usually increases with decreasing pressure. D) The solubility of an ionic solid in water decreases with increasing temperature. E) None of the above statements are true.

B) In general, the solubility of a gas in water decreases with increasing temperature.

1) Which of the following compounds will be most soluble in nonane (C9H20)? A) pentanol (CH3CH2CH2CH2CH2OH) B) benzene (C6H6) C) acetic acid (CH3CO2H) D) ethyl methyl ketone (CH3CH2COH3) E) None of these compounds should be soluble in pentane.

B) benzene (C6H6)

64) A fluid with as osmotic pressure greater than those of bodily fluids are referred to as A) isosmotic. B) hyperosmotic. C) hyposmotic. D) neosmotic. E) magnosmotic

B) hyperosmotic.

21) Give the term for the amount of solute in moles per liter of solution. A) molality B) molarity C) mole fraction D) mole percent E) mass percent

B) molarity

11) Determine DHsolute for KBr if the DHsolution (KBr) = +19.9 kJ/mol and the ΔHhydration(KBr) = -670. kJ/mol. A) +650 kJ/mol B) -650 kJ/mol C) +690 kJ/mol D) -710 kJ/mol E) -690 kJ/mol

C) +690 kJ/mol

68) What is the expected freezing point of a 0.50 m solution of Li2SO4 in water? Kf for water is 1.86°C/m. A) -0.93°C B) -1.9°C C) -2.8°C D) -6.5°C

C) -2.8°C

55) The osmotic pressure of a solution formed by dissolving 25.0 mg of aspirin (C9H8O4) in enough water to make 0.250 L of solution at 25°C is ________ atm. A) 13.6 B) 1.14 × 10-3 C) 0.0136 D) 2.45 E) 1.38

C) 0.0136

31) A solution is prepared by dissolving 1.928 g of KNO3 into enough water to make 651 mL. What is the molarity of the solution? A) 0.159 M B) 0.381 M C) 0.0293 M D) 2.48 M E) 0.0832 M

C) 0.0293 M

63) Choose the aqueous solution with the lowest vapor pressure. These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable. A) 0.120 m C2H6O2 B) 0.040 m (NH4)2SO4 C) 0.060 m Li2CO3 D) 0.030 m RbC2H3O2 E) They all have the same vapor pressure

C) 0.060 m Li2CO3

66) Choose the aqueous solution below with the highest freezing point. These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable. A) 0.200 m Mg(ClO4)2 B) 0.200 m Na3PO3 C) 0.200 m HOCH2CH2OH D) 0.200 m Ba(NO3)2 E) These all have the same freezing point.

C) 0.200 m HOCH2CH2OH

46) An aqueous solution is 0.467 M in HCl. What is the molality of the solution if the density is 1.23 g/mL? A) 0.115 m B) 0.268 m C) 0.380 m D) 0.574 m E) 0.318 m

C) 0.380 m

72) What is the change in boiling point of a solution of 31.1 g Na3PO4 in 750. g of water? Kb for water is 0.512 °C/m. Assume ideal behavior. A) 0.103°C B) 3.60°C C) 0.515°C D) 1.43°C

C) 0.515°C

46) Determine the freezing point of a solution that contains 78.8 g of naphthalene (C10H8, molar mass = 128.16 g/mol) dissolved in 722 mL of benzene (d = 0.877 g/mL). Pure benzene has a melting point of 5.50°C and a freezing point depression constant of 4.90°C/m. A) 4.76°C B) 4.17°C C) 0.74°C D) 1.33°C E) 1.68°C

C) 0.74°C

30) What molality of pentane is obtained by dissolving 15 g pentane, C5H12, in 245.0 g hexane, C6H14? A) 0.058 m B) 0.068 m C) 0.85 m D) 61 m

C) 0.85 m

36) What is the weight percent of a caffeine solution made by dissolving 8.35 g of caffeine, C8H10N4O2, in 75 g of benzene, C6H6? A) 0.010% B) 0.011% C) 10% D) 11%

C) 10%

35) What is the weight percent of vitamin C in a solution made by dissolving 6.50 g of vitamin C, C6H8O6, in 55.0 g of water? A) 0.547% B) 1.21% C) 10.6% D) 11.8%

C) 10.6%

49) At a given temperature the vapor pressures of benzene and toluene are 183 mm Hg and 59.2 mm Hg, respectively. Calculate the total vapor pressure over a solution of benzene and toluene with Xbenzene = 0.580. A) 106 mm Hg B) 121 mm Hg C) 131 mm Hg D) 242 mm Hg

C) 131 mm Hg

43) Determine the vapor pressure of a solution at 25°C that contains 76.6 g of glucose (C6H12O6) in 250.0 mL of water. The vapor pressure of pure water at 25°C is 23.8 torr. A) 70.8 torr B) 72.9 torr C) 23.1 torr D) 22.9 torr E) 7.29 torr

C) 23.1 torr

48) 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 Hg B) 20.5 mm Hg C) 23.6 mm Hg D) 24.0 mm Hg

C) 23.6 mm Hg

50) Calculate the freezing point of a solution of 40.0 g methyl salicylate, C7H6O2, dissolved in 800. g of benzene, C6H6. Kf for benzene is 5.10°C/m and the freezing point is 5.50°C for benzene. A) - 2.09°C B) 2.09°C C) 3.41°C D) 7.59°C

C) 3.41°C

33) What mass of NaCl is contained in 24.88 g of a 15.00% by mass solution of NaCl in water? A) 20.00 g B) 21.15 g C) 3.73 g D) 1.50 g E) 12.44 g

C) 3.73 g

43) At 20°C, an aqueous solution that is 24.0% by mass in ammonium chloride has a density of What is the molarity of ammonium chloride in the solution? The formula weight of NH4Cl is 53.50 g/mol. A) 5.90 B) 0.479 C) 4.79 D) 0.0445 E) 22.5

C) 4.79

27) How many grams of KBr are required to make 350. mL of a 0.115 M KBr solution? \A) 0.338 g B) 3.04 g C) 4.79 g D) 40.3 g

C) 4.79 g

32) A solution of LiCl in water has XLiCl = 0.0900. What is the molality? A) 4.46 m LiCl B) 5.00 m LiCl C) 5.49 m LiCl D) 9.89 m LiCl

C) 5.49 m LiCl

25) How many moles of KF are contained in 347 g of water in a 0.175 m KF solution? A) 1.65 × 10-2 mol KF B) 5.04 × 10-2 mol KF C) 6.07 × 10-2 mol KF D) 3.22 × 10-2 mol KF E) 1.98 × 10-2 mol KF

C) 6.07 × 10-2 mol KF

25) What volume of 3.00 M CH3OH solution is needed to provide 0.220 mol of CH3OH? A) 1.52 mL B) 13.6 mL C) 73.3 mL D) 660 mL

C) 73.3 mL

13) Determine the solubility of N2 in water exposed to air at 25°C if the atmospheric pressure is 2.0 atm. Assume that the mole fraction of nitrogen is 0.78 in air and the Henry's law constant for nitrogen in water at this temperature is 6.1 × 10-4 M/atm. A) 1.6 × 10-4 M B) 6.4 × 10-4 M C) 9.5 × 10-4 M D) 1.1 × 10-4 M E) 1.2 × 10-4 M

C) 9.5 × 10-4 M

41) ________ is applied to roads in wintertime so that the ice will melt at a lower temperature. A) Antifreeze B) Water C) Salt D) Sugar E) Oil

C) Salt

14) A solution is formed at room temperature by vigorously dissolving enough of the solid solute so that some solid remains at the bottom of the solution. Which statement below is TRUE? A) The solution is considered unsaturated. B) The solution is considered supersaturated. C) The solution is considered saturated. D) The solution would be considered unsaturated if it were cooled a bit to increase the solubility of the solid. E) None of the above are true.

C) The solution is considered saturated.

9) Choose the situation below that would result in an exothermic ΔHsolution. A) When solute > hydration B) When solute is close to hydration C) When solute < hydration D) When solvent >> solute E) There isn't enough information to determine.

C) When solute < hydration

13) A solution containing more than the equilibrium amount is called A) an unsaturated solution. B) a dilute solution. C) a supersaturated solution. D) a concentrated solution. E) a saturated solution.

C) a supersaturated solution.

26) To make a 0.500 M solution, one could take 0.500 moles of solute and add A) 1.00 L of solvent. B) 1.00 kg of solvent. C) enough solvent to make 1.00 L of solution. D) enough solvent to make 1.00 kg of solution.

C) enough solvent to make 1.00 L of solution

6) Which of the following compounds will be most soluble in ethanol (CH3CH2OH)? A) trimethylamine (N(CH3)3) B) acetone (CH3COCH3) C) ethylene glycol (HOCH2CH2OH) D) hexane (CH3CH2CH2CH2CH2CH3) E) None of these compounds should be soluble in ethanol.

C) ethylene glycol (HOCH2CH2OH)

2) Give the major force between ethanol and water. A) dipole-dipole B) dispersion C) hydrogen bonding D) ion-ion E) ion-dipole

C) hydrogen bonding

58) Solutions having osmotic pressures less than those of body fluids are called A) isosmotic. B) hyperosmotic. C) hyposmotic. D) neosmotic. E) magnosmotic

C) hyposmotic.

8) Dissolving can be defined as A) rate of dissolution = rate of deposition. B) rate of dissolution < rate of deposition. C) rate of dissolution > rate of deposition. D) rate of bubbling > rate of dissolving E) rate of condensing > rate of bubbling

C) rate of dissolution > rate of deposition.

exothermic ΔHhydration? A) Na+ 2 B) Ba + 3 C)Al + 2 D)Ca +

C)Al + 2

71) Under a pressure of 298 atm at 25°C, a gas was found to have a concentration of 0.182M. What is the identity of the gas? A) CO2 B) F2 C) CO D) N2 E) Ar

D) N2

15) Which of the following statements is generally TRUE? A) The solubility of a solid is not dependent on either temperature or pressure. B) The solubility of a solid is highly dependent on pressure. C) The solubility of a solid is highly dependent on both pressure and temperature. D) The solubility of a solid is highly dependent on temperature. E) None of the above.

D) The solubility of a solid is highly dependent on temperature.

8) Choose the situation below that would result in a ΔHsolution near 0. A) When solvent >>solute B) When solute > hydration C) When solute < hydration D) When solute is close to hydration E) There isn't enough information to determine.

D) When solute is close to hydration

23) Which of the following concentration units are temperature dependent? A) mole fraction B) molality C) mass percent D) molarity E) none of the above

D) molarity

53) A solution is prepared by dissolving 7.00 g of glycerin (C3H8O3) in 201 g of ethanol (C2H5OH). The freezing point of the solution is ________°C. The freezing point of pure ethanol is -114.6°C at 1 atm. The molal-freezing-point-depression constant (Kf) for ethanol is 1.99°C/m. The molar masses of glycerin and of ethanol are 92.1 g/mol and 46.1 g/mol, respectively. A) -121.3 B) 0.752 C) -107.9 D) -113.8 E) -115.4

E) -115.4

63) What mass of water is required to give an aqueous solution containing 0.265 mol of MgCl2 with a freezing point of -3.8°C? (Van't Hoff factor of MgCl2 is 2.7) A) 1.25 kg B) 0.538 kg C) 0.113 kg D) 0.882 kg E) 0.350 kg

E) 0.350 kg

15) Determine the partial pressure of oxygen necessary to form an aqueous solution that is 6.5 × 10-4 M O2 at 25°C. The Henry's law constant for oxygen in water at 25°C is 1.3 × 10-3 M/atm. A) 1.2 atm B) 0.85 atm C) 0.78 atm D) 2.0 atm E) 0.50 atm

E) 0.50 atm

18) Calculate the molality of a solution formed by dissolving 34.8 g of LiI in 500.0 mL of water. A) 0.254 m B) 0.130 m C) 0.696 m D) 0.260 m E) 0.520 m

E) 0.520 m

7) Which of the following compounds is most soluble in hexane (CH3CH2CH2CH2CH2CH2CH3)? A) methanol B) ethanol C) 1-propanol D) 1-butanol E) 1-pentanol

E) 1-pentanol

33) A solution is prepared by adding 1.43 mol of KCl to 889 g of water. The concentration of KCl is ________ molal. A) 1.61 × 10-3 B) 622 C) 0.622 D) 1.27 × 103 E) 1.61

E) 1.61

17) Parts per million requires a multiplication factor of A) 10^-9 B) 10^-3 C) 10^3 D) 10^15 E) 10^6

E) 10^6

16) Parts per billion requires a multiplication factor of A) 10-9 B) 10-3 C) 10^3 D) 10^6 E) 10^9

E) 10^9

50) The boiling point elevation of an aqueous sucrose solution is found to be 0.39°C. What mass of sucrose (molar mass= 342.30 g/mol) would be needed to dissolve in 500.0 g of water? Kb (water) = 0.512°C/m. A) 261 g sucrose B) 528 g sucrose C) 762 g sucrose D) 223 g sucrose E) 130. g sucrose

E) 130. g sucros

45) At 20°C, a 0.376 M aqueous solution of ammonium chloride has a density ofWhat is the mass % of ammonium chloride in the solution? The formula weight of NH4Cl is 53.50 g/mol. A) 0.381 B) 0.705 C) 0.374 D) 2.68 E) 2.00

E) 2.00

28) Determine the molality of a solution prepared by dissolving 0.500 moles of CaF2 in 11.5 moles H2O. A) 1.88 m B) 4.35 m C) 5.31 m D) 4.14 m E) 2.41 m

E) 2.41 m

38) What mass of ethane (CH3CH3) is contained in 50.0 mL of a 13.9% by mass solution of ethane in hexane? The density of the solution is 0.611 g/mL. A) 2.35 g B) 8.49 g C) 11.8 g D) 6.95 g E) 4.25 g

E) 4.25 g

51) Determine the boiling point of a solution that contains 78.8 g of naphthalene (C10H8, molar mass = 128.16 g/mol) dissolved in 722 mL of benzene (d = 0.877 g/mL). Pure benzene has a boiling point of 80.1°C and a boiling point elevation constant of 2.53°C/m. A) 2.2°C B) 2.5°C C) 82.3°C D) 80.4°C E) 82.6°C

E) 82.6°C

32) A solution is prepared by dissolving 49.3 g of KBr in enough water to form 473 mL of solution. Calculate the mass % of KBr in the solution if the density is 1.12 g/mL. A) 10.4% B) 8.57% C) 10.1% D) 11.7% E) 9.31%

E) 9.31%

58) Identify the solute with the highest van't Hoff factor. A) nonelectrolyte B) K I C) MgSO4 D) Ca Cl2 E) AlCl3

E) AlCl3

57) Place the following solutions in order of increasing osmotic pressure. I. 0.15 M C2H6O2 II. 0.15 M BaCl2 III. 0.15 M Na I A) III < I < II B) II < III < I C) I < II < III D) II < I < III E) I < III < II

E) I < III < II

9) Identify the compound whose solubility is least affected by temperature. A) K Cl B) K2Cr2O7 C) NaNO3 D) Pb(NO3)3 E) NaCl

E) NaCl

64) Choose the aqueous solution with the highest vapor pressure. These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable. A) 0.50 m C4H10O4 B) 0.50 m C2H6O2 C) 0.50 m C5H12O5 D) 0.50 m C11H24O11 E) They all have about the same vapor pressure.

E) They all have about the same vapor pressure.

40) Identify the colligative property. A) vapor pressure lowering B) freezing point depression C) boiling point elevation D) osmotic pressure E) all of the above

E) all of the above

2) Identify the compounds that are soluble in both water and hexane. A) methanol and 1-pentanol B) ethanol and 1-butanol C) 1-propanol and 1-butanol D) 1-butanol and 1-pentanol E) ethanol and 1-propanol

E) ethanol and 1-propanol

3) Give the major force in seawater. A) dipole-dipole B) dispersion C) hydrogen bonding D) ion-ion E) ion-dipole

E) ion-dipole

42) The vapor pressure of a solution is always that of the pure solvent A) equal to B) twice C) one half D) higher than E) lower than

E) lower than