Homework answers / question archive / Chapter 11: 1) Which of the following substances is a strong electrolyte?             A)  CH3OH    B)  C6H14    C)  C6H12O6    D)  LiCl    E)  SO2           2

Chapter 11: 1) Which of the following substances is a strong electrolyte?             A)  CH3OH    B)  C6H14    C)  C6H12O6    D)  LiCl    E)  SO2           2

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Chapter 11:

1) Which of the following substances is a strong electrolyte?

            A)  CH₃OH    B)  C₆H₁₄    C)  C₆H₁₂O₆    D)  LiCl    E)  SO₂

 

        2.  Which of the following substances is a strong electrolyte?

            A)  CH₃CH₂OH    B)  C₆H₆    C)  KOH    D)  SO₂    E)  PCl₃

 

        3.  Which of the following substances is a strong electrolyte?

            A)  CH₃CH₂OH    B)  C₈H₁₈    C)  LiOH    D)  CO₂    E)  PCl₅

 

        4.  Which of the following substances is a nonelectrolyte?

            A)  KMnO₄    B)  CH₃CH₂OH    C)  NaOH    D)  K₂SO₄    E)  Na₂O

 

        5.  Which of the following substances is a nonelectrolyte?

            A)  Na₂SO₄    B)  CH₃OH    C)  KOH    D)  LiNO₃    E)  RbCl

 

        6.  Which of the following substances is a nonelectrolyte?

            A)  NaNO₃    B)  LiOH    C)  C₆H₁₂O₆    D)  LiCN    E)  CsCl

 

        7.  What ions, atoms, or molecules are present after CH₃CH₂OH(l) mixes with water?

            A)      CH₃CH₂OH(aq) and H₂O(l)

            B)      CH₃CH₂O^-(aq), H⁺(aq), and H₂O(l)

            C)      CH₃CH₂O^-(aq), and H₃O⁺(aq)

            D)      2C(aq), 6H(aq), and H₂O₂(l)

            E)      CH₃⁺(aq), CH₂O^-(aq), H⁺(aq), and H₂O(l)

 

        8.  What ions, atoms, or molecules (in addition to the water molecules) are present after Na₂SO₄(s) mixes with water?

            A)      Na₂SO₄(l)                                              D)      Na₂SO₃²⁺(aq) + O^2-(aq)

            B)      Na₂SO₄ (aq)                                          E)      2Na⁺(aq) + SO₄^2-(aq)

            C)      Na⁺(aq) + NaSO₄^-(aq)                                   

 

        9.  What ions, atoms, or molecules (in addition to the water molecules) are present after HNO₃(l) mixes with water?

            A)      HNO₃(l)                                                 D)      H(aq) + NO₃(aq)

            B)      HNO₃(aq)                                              E)      H(aq) + N(aq) + 3O(aq)

            C)      H⁺(aq) + NO₃^-(aq)                                         

 

      10.  Which of the diagrams in the figure best represents an aqueous solution of MgCl₂?

           

 

            A)  I    B)  II    C)  III    D)  either I or III    E)  none of these is correct

 

      11.  Which of the diagrams in the figure best represents an aqueous solution of Na₂SO₄?

           

 

            A)  I    B)  II    C)  III    D)  either I or III    E)  none of these is correct

 

      12.  Which of the following statements regarding the rule “like dissolves like” is incorrect?

            A)      Since cooking oil is composed primarily of hydrocarbons, it is insoluble in water.

            B)      Iodine, I₂, is very soluble in water.

            C)      Ethanol, CH₃CH₂OH, is water-soluble.

            D)      Cooking oil, a nonpolar substance, is soluble in hexane, C₆H₁₄.

            E)      Potassium nitrate, KNO₃, is soluble in water.

 

      13.  Which of the following statements regarding the rule “like dissolves like” is incorrect?

            A)      Since cooking oil is composed primarily of hydrocarbons, it is soluble in water.

            B)      Oxygen, O₂, is not very soluble in water.

            C)      Methanol, CH₃OH, is water-soluble.

            D)      Cooking oil, a nonpolar substance, is soluble in heptane, C₇H₁₆.

            E)      Sodium nitrate, NaNO₃, is soluble in water.

 

      14.  Which of the following statements regarding the rule “like dissolves like” is incorrect?

            A)      Since grease is nonpolar, it is not soluble in water.

            B)      Nitrogen, N₂, is not very soluble in water.

            C)      Methanol, CH₃OH, is not very water-soluble.

            D)      Butane, C₄H₁₀, is soluble in cooking oil, a nonpolar substance.

            E)      Calcium nitrate, Ca(NO₃), is soluble in water.

 

      15.  Which of the following should be most soluble in water?

            A)      fat (a nonpolar triglyceride molecule)   D)      I₂(s)

            B)      C₆H₆(l)                                                   E)      O₂(g)

            C)      CH₃NH₂(l)                                                     

 

      16.  Which of the following should be most soluble in water?

            A)      Vitamin C (a very good hydrogen bonder)

            B)      Vitamin A (a mostly nonpolar molecule)

            C)      C₆H₆(l)

            D)      I₂(s)

            E)      O₂(g)

 

      17.  Which of the following should be most soluble in hexane, C₆H₁₄?

            A)  NaCl    B)  NaNO₃    C)  H₂O    D)  CH₃OH    E)  Br₂

 

      18.  Which of the following should be most soluble in benzene, C₆H₆?

            A)  H₂O    B)  CH₃OH    C)  I₂    D)  NaCl    E)  NaNO₃

 

      19.  Which of the following should be most soluble in ethanol, CH₃CH₂OH?

            A)  CH₃NH₂    B)  CCl₄    C)  I₂    D)  C₆H₆    E)  CO₂

 

      20.  Sodium chloride, NaCl, dissolves in water because

            A)      there are attractive forces between ions and water molecules.

            B)      there are no attractive forces between ions and water molecules.

            C)      the entropy of the solution is greater than the entropy of pure NaCl and pure H₂O.

            D)      the entropy of the solution is less than the entropy of pure NaCl and pure H₂O.

            E)      Both A and C

 

      21.  Which of the following occurs when an ionic compound dissolves in water to form a solution?

            A)      Ionic bonds break.                                 D)      Entropy increases.

            B)      Hydrogen bonds are disrupted.            E)      All of these

            C)      H₂O – Ion attractive forces form.                  

 

      22.  Many cold packs contain ammonium nitrate and water.  The dissolving of ammonium nitrate is endothermic.  Which of the following best describes the energy and entropy changes that occur for the NH₄NO₃ system when ammonium nitrate and water are mixed to make a solution?

            A)      There is a net energy increase and an entropy increase.

            B)      There is a net energy increase and an entropy decrease.

            C)      There is a net energy decrease and an entropy decrease.

            D)      There is no a net change in energy or entropy.

 

      23.  Which of the following statements regarding the solution process is incorrect?

            A)      In a sodium chloride solution, the ions interact with the water molecules through ion-dipole forces.

            B)      Hydration is the process whereby water molecules surround solute particles.

            C)      A hydrated cation is surrounded by the partially positive end of the water molecules.

            D)      When an ionic compound dissolves, the ionic bonds break.

            E)      Some of the hydrogen bonds among the water molecules must break.

 

      24.  Which of the following statements regarding the solution process is incorrect?

            A)      When a solution is formed from an ionic compound, the anions and cations are evenly distributed throughout the solution.

            B)      When a polar covalent compound dissolves in water, dipole-dipole interactions take place between the water molecules and the solute molecules.

            C)      A nonpolar compound such as hexane, C₆H₁₄, forms London dispersion forces with a nonpolar solute, such as I₂ during the solution process.

            D)      The solution process is always exothermic.

            E)      When an ionic solute dissolves, the entropy of the solution is greater than the original entropy of the crystalline form of the ionic substance.

 

      25.  When potassium nitrate is dissolved in water, the resulting solution feels cool to the touch.  This means that:

            A)      the strength of attraction between the solute particles is greater than that of the attraction between the solute and solvent.

            B)      the strength of attraction between the solute and solvent particles is greater than that of the attraction between the solute particles.

            C)      the strength of attraction between the solute particles is equal to that of the attraction between the solute and solvent.

            D)      hydrogen bonds must be broken, which is an exothermic process.

            E)      there is a decrease in entropy for the solution.

 

      26.  Which of the following statements regarding solubility is incorrect?

            A)      A polar compound will dissolve an ionic compound due to ion-dipole interactions.

            B)      A nonpolar solvent will not interact strongly enough with ions to dissolve an ionic compound.

            C)      Nonpolar liquids will dissolve in one another because the intermolecular forces in the pure liquids are weak, and there is an increase in entropy.

            D)      Most solids are more soluble at higher temperature than at a lower temperature of the solvent.

            E)      Most gases are more soluble at a higher temperature than at a lower temperature of the solvent.

 

      27.  Which of the following statements regarding the solubility of oxygen in water is incorrect?

            A)      Water in contact with air contains a small amount of dissolved oxygen.

            B)      When water is heated, the first tiny bubbles that you see escaping from the warm water contain O₂.

            C)      In warm weather, fish must come to the surface more often to get oxygen, since there is less dissolved oxygen in the water than in cooler weather.

            D)      If a sealed container has both oxygen and water, changing the pressure of the oxygen above the water will have no effect on the solubility of the oxygen in the water.

            E)      An increase in temperature causes an increase in the kinetic energy of the molecules in a solution, allowing oxygen molecules to escape more readily.

 

      28.  Which of the following increases the solubility of a gas in solution?

            A)      increasing gas pressure and increasing temperature

            B)      increasing gas pressure and decreasing temperature

            C)      decreasing gas pressure and increasing temperature

            D)      decreasing gas pressure and decreasing temperature

            E)      adding more water

 

      29.  If the solubility of a solid substance is 18.2 g/100 g water, which of the following best describes what eventually forms after 10.0 grams of the substance is mixed with 50.0 grams of water?

            A)      a saturated solution with some undissolved solid

            B)      an unsaturated solution with some undissolved solid

            C)      a saturated solution with no undissolved solid

            D)      an unsaturated solution with no undissolved solid

            E)      a supersaturated solution

 

      30.  If the solubility of sodium chloride at 25°C is 38.0 g/100 g water, which of the following best describes what eventually forms after 15.0 grams of sodium chloride is mixed with 50.0 grams of water at 25°C?

            A)      a saturated solution with some undissolved solid

            B)      an unsaturated solution with some undissolved solid

            C)      a saturated solution with no undissolved solid

            D)      an unsaturated solution with no undissolved solid

            E)      a supersaturated solution

      31.  Given that the solubility of potassium chlorate in water is 10.0 g/100 g water at 30°C, what mass of potassium chlorate is dissolved in 250 grams of a saturated solution at 30°C?

            A)      any mass greater than 25.0 g                 D)      25.0 g

            B)      any mass less than 10.0 g                      E)      10.0 g

            C)      any mass less than 25.0 g                               

 

      32.  What is the percent-by-mass concentration of KCl in a solution that is prepared by adding 13.0 g of KCl to 85.0 g of water?

            A)  15.3%    B)  17.2%    C)  13.3%    D)  72.0%    E)  65.4%

 

      33.  What is the percent-by-mass concentration of KOH in a solution that is prepared by adding 18.0 g of KOH to 95.0 g of water?

            A)  18.9%    B)  15.9%    C)  31.5%    D)  5.28%    E)  77.0%

 

      34.  What is the percent-by-mass concentration of NaCl in a solution that is prepared by adding 14.0 g of  NaCl to 75.0 g of water?

            A)  61.0%    B)  15.7%    C)  18.7%    D)  24.0%    E)  5.36%

 

      35.  What mass of sodium nitrate is dissolved in 455 g of a solution that is 15.0% by mass NaNO₃?

            A)  68.3 g    B)  30.3 g    C)  4.40 ´ 10² g    D)  3.03 ´ 10³ g    E)  15.0 g

 

      36.  What mass of sodium hydroxide is dissolved in 295 g of a solution that is 12.0% by mass NaOH?

            A)  3540 g    B)  35.4 g    C)  4.07 g    D)  40.7 g    E)  12.0 g

 

      37.  What mass of sodium chloride is dissolved in 365 g of a solution that is 14.0% by mass NaCl?

            A)  5110 g    B)  26.1 g    C)  351 g    D)  51.1 g    E)  14.0 g

 

      38.  What is the percent-by-mass concentration of antifreeze (ethylene glycol, C₂H₆O₂) in an aqueous solution that contains 420.0 g of ethylene glycol in 1.00 L of solution.  The density of the solution is 1.05 g/mL.

            A)  2.50%    B)  42.1%    C)  40.0%    D)  44.1%    E)  60.0%

 

      39.  What is the percent-by-mass concentration of hydrogen peroxide, H₂O₂, in an aqueous solution that contains 30.0 g of hydrogen peroxide in 1.00 L of solution.  The density of the solution is 1.00 g/mL.

            A)  30.0%    B)  3.00%    C)  33.3%    D)  31.0%    E)  70.0%

 

      40.  What is the percent-by-mass concentration of citric acid, C₆H₈O₇, in an aqueous solution that contains 263.2 g of citric acid in 1.00 L of solution.  The density of the solution is 1.10 g/mL.

            A)  73.7%    B)  26.3%    C)  23.9%    D)  3.80%    E)  29.0%

 

      41.  A solution of ethanol, C₂H₅OH, is prepared by dissolving 25.0 mL of ethanol in enough water to give a total volume of 250.0 mL.  What is the percent-by-volume concentration of ethanol?

            A)  10.0%    B)  9.09%    C)  90.0%    D)  1.00%    E)  225%

 

      42.  A solution of acetic acid, CH₃CO₂H, is prepared by dissolving 30.0 mL of acetic acid in enough water to give a total volume of 150.0 mL.  What is the percent-by-volume concentration of acetic acid?

            A)  16.7%    B)  15.0%    C)  30.0%    D)  20.0%    E)  25.0%

 

      43.  A solution of acetic acid, CH₃CO₂H, is prepared by dissolving 40.0 mL of acetic acid in enough water to give a total volume of 250.0 mL.  What is the percent-by-volume concentration of acetic acid?

            A)  19.0%    B)  16.0%    C)  25.0%    D)  40.0%    E)  13.8%

 

      44.  How many moles of NaOH are contained in 100.0 mL of 3.00 M NaOH?

            A)      0.300 moles                                           D)      0.00300 moles

            B)      300.0 moles                                           E)      0.333 moles

            C)      33.3 moles                                                      

 

      45.  How many moles of NaCl are contained in 50.0 mL of 2.50 M NaCl?

            A)      2.50 moles                                             D)      2.45 moles

            B)      0.050 moles                                           E)      0.125 moles

            C)      5.00 moles                                                      

 

      46.  How many moles of HCl are contained in 75.0 mL of 2.00 M HCl?

            A)      2.00 moles                                             D)      37.5 moles

            B)      1.50 ´ 10² moles                                    E)      26.7 moles

            C)      0.150 moles                                                    

          

 

      47.  What volume of 2.00 M HCl contains 0.50 mol HCl?

            A)  1.0 L    B)  0.25 L    C)  2.5 L    D)  0.50 L    E)  1.5 L

             48.       What volume of 6.00 M NaOH contains 2.50 mol NaOH?

            A)  2.50 L    B)  6.00 L    C)  2.40 L    D)  0.417 L    E)  15.0 L

          

 

      49.  What volume of 3.00 M NaOH contains 1.75 mol NaOH?

            A)  1.75 L    B)  3.00 L    C)  4.75 L    D)  0.583 L    E)  1.71 L

             50.       A solution contains 15.5 g of NaOH dissolved in sufficient water to give a total mass of 125.0 g.  What is the molality of the solution?

            A)  3.54 m    B)  0.124 m    C)  0.00310 m    D)  3.10 m    E)  124 m

          

 

      51.  A solution contains 25.5 g of NaCl dissolved in sufficient water to give a total mass of 325.0 g.  What is the molality of the solution?

            A)  0.146 m    B)  0.785 m    C)  1.34 m    D)  1.46 m    E)  134 m

 

      52.  A solution contains 22.0 g of HCl dissolved in sufficient water to give a total mass of 125.0 g.  What is the molality of the solution?

            A)  0.250 m    B)  5.86 m    C)  2.75 m    D)  4.83 m    E)  0.176 m

 

      53.  What is the molal concentration of ions in a 2.40 m solution of Al(NO₃)₃?

            A)  2.40 m    B)  7.20 m    C)  9.60 m    D)  0.800 m    E)  31.2 m

 

      54.  What is the molal concentration of ions in a 1.60 m solution of Fe(NO₃)₃?

            A)  1.60 m    B)  3.20 m    C)  4.80 m    D)  6.40 m    E)  20.8 m

 

      55.  A 150.0 g sample of ocean water contains 3.5 mg of mercury.  How many parts per million of mercury are in the sample?

            A)  15 ppm    B)  23 ppm    C)  2.4 ´ 10² ppm    D)  2.3 ´ 10⁴ ppm    E)  43 ppm

 

      56.  A 200.0 g sample of river water contains 6.5 mg of lead.  How many parts per million of lead are in the sample?

            A)  6.5 ppm    B)  21 ppm    C)  3.2 ´ 10² ppm    D)  32 ppm    E)  54 ppm

 

      57.  A 200.0 g sample of rainwater contains 4.8 mg of sulfuric acid.  How many parts per million of sulfuric acid are in the sample?

            A)  42 ppm    B)  21 ppm    C)  2.4 ´ 10² ppm    D)  4.8 ppm    E)  24 ppm

 

      58.  The EPA has determined that the maximum safe level of lead ion in drinking water is 15 ppb.  If a sample of tap water has a lead ion concentration of 0.0065 ppm, what is the concentration of the lead ion in ppb, and is the water safe to drink?  Assume the density of the solution is 1.00 g/mL.

            A)      65 ppb, not safe                                     D)      0.65 ppb, safe

            B)      6.5 ppb, safe                                          E)      6.5 ´ 10^-6 ppm, safe

            C)      650 ppb, not safe                                           

 

      59.  The EPA has determined that the maximum safe level of lead ion in drinking water is 15 ppb.  If a sample of tap water has a lead ion concentration of 0.016 ppm, what is the concentration of the lead ion in ppb, and is the water safe to drink?  Assume the density of the solution is 1.00 g/mL.

            A)      160 ppb, not safe                                   D)      0.16 ppb, safe

            B)      16 ppb,  not safe                                    E)      1.6 ´ 10^-6 ppm, safe

            C)      1600 ppb, not safe                                         

 

      60.  Silver nitrate, AgNO₃, can be used to test for the presence of chloride ions in solution, because it readily forms a precipitate of AgCl.  What volume of 2.0 M AgNO₃ will be required to react with 50.0 mL of a 0.10 M HCl solution?

            AgNO₃(aq) + HCl(aq) ® AgCl(s) + HNO₃(aq)

            A)  0.25 mL    B)  25 mL    C)  5.0 ´ 10¹ mL    D)  2.5 ´ 10² mL    E)  2.5 mL

 

      61.  Silver nitrate, AgNO₃, can be used to test for the presence of chloride ions in solution, because it readily forms a precipitate of AgCl.  What volume of 1.5 M AgNO₃ will be required to react with 30.0 mL of a 0.45 M HCl solution?

            AgNO₃(aq) + HCl(aq) ® AgCl(s) + HNO₃(aq)

            A)  45 mL    B)  9.0 mL    C)  9.0 L    D)  1.0 L    E)  1.1 ´ 10² mL

 

      62.  How many moles of  potassium iodide, KI, are required to precipitate all of the lead(II) ion from 50.0 mL of a 1.2 M  Pb(NO₃)₂ solution?  (First, write a balanced equation for the reaction.)

            A)  0.12 mole    B)  0.060 mole    C)  0.24 mole    D)  0.030 mole    E)  0.048 mole

      63.  How many moles of  potassium iodide, KI, are required to precipitate all of the lead(II) ion from 25.0 mL of a 1.6 M  Pb(NO₃)₂ solution?  (First, write a balanced equation for the reaction.)

            A)  0.040 mole    B)  0.080 mole    C)  0.020 mole    D)  64 mol    E)  0.64 mol

      64.  What volume of 0.1243 M KOH is required to neutralize 25.00 mL of 0.1540 M H₂SO₄?  (First, write a balanced equation for the reaction.)

            A)  10.09 mL    B)  30.97 mL    C)  61.95 mL    D)  20.18 mL    E)  40.36 mL

 

      65.  What volume of 0.1452 M KOH is required to neutralize 25.00 mL of 0.1020 M H₂SO₄?  (First, write a balanced equation for the reaction.)

            A)  17.79 mL    B)  17.56 mL    C)  8.781 mL    D)  35.12 mL    E)  71.18 mL

 

      66.  When a 25.00 mL sample of H₂SO₄ is titrated with 0.2453 M NaOH, 32.47 mL of NaOH solution is required to neutralize the H₂SO₄.  What is the molarity of the H₂SO₄?

            A)  0.3186 M    B)  0.1889 M    C)  0.3777 M    D)  3.309 M    E)  0.1593 M

 

      67.  When a 25.00 mL sample of H₂SO₄ is titrated with 0.3423 M NaOH, 26.67 mL of NaOH solution is required to neutralize the H₂SO₄.  What is the molarity of the H₂SO₄?

            A)  0.3652 M    B)  0.3209 M    C)  0.1604 M    D)  0.1826 M    E)  0.1988 M

 

      68.  When a 25.00 mL sample of NaOH is titrated with 0.4523 M H₂SO₄, 36.69 mL of H₂SO₄ solution is required to neutralize the NaOH.  What is the molarity of the NaOH?

            A)  0.3319 M    B)  0.6638 M    C)  1.328 M    D)  0.6164 M    E)  0.1988 M

 

      69.  When a 25.00 mL sample of NaOH is titrated with 0.2523 M H₂SO₄, 26.69 mL of H₂SO₄ solution is required to neutralize the NaOH.  What is the molarity of the NaOH?

            A)  0.1347 M    B)  0.4726 M    C)  0.5387 M    D)  0.2694 M    E)  0.2363 M

 

      70.  Consider two aqueous glucose solutions of different concentrations, separated by a semi-permeable membrane.  Which of the following best describes the process of osmosis at the molecular level?

            A)      The smaller water molecules move in a net direction from the more dilute side to the more concentrated side.

            B)      The smaller water molecules move in a net direction from the more concentrated side to the more dilute side.

            C)      The larger glucose particles move in a net direction from the more dilute side to the more concentrated side.

            D)      The larger glucose particles move in a net direction from the more concentrated side to the more dilute side.

            E)      Osmosis will not occur.

 

      71.  What will happen to a blood cell that is placed in pure water?

            A)      The cell will shrink because there will be a net flow of water to the outside of the cell.

            B)      The cell will shrink because there will be a net flow of electrolytes to the outside of the cell.

            C)      The cell will expand because there will be a net flow of water to the inside of the cell.

            D)      The cell will expand because there will be a net flow of electrolytes to the inside of the cell.

            E)      Nothing will happen because the cell is impermeable.

      72.  What will happen to a blood cell that is placed in an aqueous solution that has a high salt concentration relative to the blood cell concentration?

            A)      The cell will shrink because there will be a net flow of water to the outside of the cell.

            B)      The cell will shrink because there will be a net flow of electrolytes to the outside of the cell.

            C)      The cell will expand because there will be a net flow of water to the inside of the cell.

            D)      The cell will expand because there will be a net flow of electrolytes to the inside of the cell.

            E)      Nothing will happen because the cell is impermeable.

 

      73.  Calculate the freezing point of a 2.0 m solution of sucrose in water?  Sucrose is a nonelectrolyte. The normal freezing point of pure water is 0.00°C. 

            K_f (water) = –1.86°C/m

            A)  –1.86 °C    B)  –3.72°C    C)  –2.00°C    D)  3.72°C    E)  1.86°C

 

      74.  Calculate the boiling point of a 4.0 m solution of sucrose in water?  Sucrose is a nonelectrolyte. The normal boiling point of pure water is 100.0°C.

            K_b (water) = 0.52°C/m

            A)  2.1°C    B)  97.9°C    C)  96.0°C    D)  94.0°C    E)  102.1°C

 

      75.  Calculate the freezing point of a 2.0 m solution of NaCl in water?  Remember that NaCl is an electrolyte. The normal freezing point of pure water is 0.00°C.

            K_f (water) = –1.86°C/m

            A)  –2.08 °C    B)  –3.72°C    C)  –7.44°C    D)  7.44°C    E)  3.74°C

 

      76.  Calculate the boiling point of a 4.0 m solution of KI in water?  Remember that KI is an electrolyte. The normal boiling point of pure water is 100.0°C.

             K_b (water) = 0.52°C/m

            A)  101.0 °C    B)  104.2°C    C)  96.0°C    D)  102.1°C    E)  4.16°C

 

      77.  Calculate the freezing point of a 1.0 m solution of Ca(NO₃)₂ in water?  Remember that Mg(NO₃)₂ is an electrolyte. The normal freezing point of pure water is 0.00°C.

            K_f (water) = –1.86°C/m

            A)  1.56 °C    B)  5.58°C    C)  1.86°C    D)  –5.58°C    E)  –1.86°C

 

      78.  Which of the following aqueous solutions should have the lowest freezing point?

            A)      1.0 m C₁₂H₂₂O₁₁

            B)      1.0 m NaNO₃

            C)      1.0 m NaCl

            D)      1.0 m MgCl₂

            E)      All should have the same freezing point

      79.  Which of the following aqueous solutions should have the highest boiling point?

            A)      1.0 m MgCl₂                                          D)      1.0 m C₁₂H₂₂O₁₁

            B)      1.0 m NaNO₃                                        E)      All should have the same boiling point

            C)      1.0 m NaCl                                                     

 

      80.  Which of the following properties of water increases as the concentration of particles dissolved in the water increases?

            A)      vapor pressure                                       D)      melting point

            B)      boiling point                                          E)      none of these

            C)      freezing point                                                 

      81.  What happens to the vapor pressure, boiling point, and freezing point of a liquid when a solute is dissolved in the liquid to form a solution?

            A)      vapor pressure increases, boiling point decreases, and freezing point decreases

            B)      vapor pressure decreases, boiling point decreases, and freezing point decreases

            C)      vapor pressure decreases, boiling point increases, and freezing point decreases

            D)      vapor pressure increases, boiling point decreases, and freezing point increases

            E)      vapor pressure increases, boiling point increases, and freezing point increases

 

      82.  What happens to the osmotic pressure, boiling point, and freezing point

            of a solution when the concentration of the solute is decreased?

            A)      osmotic pressure increases, boiling point increases, and freezing point increases

            B)      osmotic pressure decreases, boiling point increases, and freezing point decreases

            C)      osmotic pressure decreases, boiling point decreases, and freezing point decreases

            D)      osmotic pressure decreases, boiling point decreases, and freezing point increases

            E)      osmotic pressure increases, boiling point decreases, and freezing point increases

 

      83.  Rank the following solutions in order of increasing boiling point:  2.5 m fructose, C₆H₁₂O₆, 2.0 m NaCl, 1.5 m methanol, CH₃OH, and 2.2 m Al(NO₃)₃

            A)      C₆H₁₂O₆  < Al(NO₃)₃ < NaCl < CH₃OH

            B)      CH₃OH < Al(NO₃)₃ < NaCl < C₆H₁₂O₆

            C)      Al(NO₃)₃ < NaCl < C₆H₁₂O₆ < CH₃OH

            D)      CH₃OH < C₆H₁₂O₆  < NaCl < Al(NO₃)₃

            E)      CH₃OH < C₆H₁₂O₆  < Al(NO₃)₃ < NaCl

 

      84.  Rank the following solutions in order of increasing boiling point:  3.5 m fructose, C₆H₁₂O₆, 3.0 m NaCl, 2.5 m methanol, CH₃OH, and 2.2 m Al(NO₃)₃

            A)      C₆H₁₂O₆  < Al(NO₃)₃ < NaCl < CH₃OH

            B)      CH₃OH < Al(NO₃)₃ < NaCl < C₆H₁₂O₆

            C)      Al(NO₃)₃ < NaCl < C₆H₁₂O₆ < CH₃OH

            D)      CH₃OH < C₆H₁₂O₆  < NaCl < Al(NO₃)₃

            E)      CH₃OH < C₆H₁₂O₆  < Al(NO₃)₃ < NaCl

 

      85.  Rank the following solutions in order of increasing boiling point:  1.5 m fructose, C₆H₁₂O₆, 1.2 m NaCl, 2.0 m methanol, CH₃OH, and 2.2 m Al(NO₃)₃

            A)      C₆H₁₂O₆  < Al(NO₃)₃ < NaCl < CH₃OH

            B)      CH₃OH < Al(NO₃)₃ < NaCl < C₆H₁₂O₆

            C)      Al(NO₃)₃ < NaCl < C₆H₁₂O₆ < CH₃OH

            D)      C₆H₁₂O₆ < CH₃OH < NaCl < Al(NO₃)₃

            E)      NaCl < C₆H₁₂O₆  < CH₃OH < Al(NO₃)₃

 

      86.  The images represent a solution of NaCl, a solution of glucose, and a more dilute solution of glucose.  Rank the aqueous solutions in order of highest to lowest freezing point.

           

 

            A)  I > II > III    B)  II > I > III    C)  II > III > I    D)  III > II > I    E)  III > I > II

 

      87.  The images represent a solution of NaNO₃, a more concentrated solution of NaNO₃, and an MgCl₂ solution.  Rank the aqueous solutions in order of highest to lowest freezing point.

           

 

            A)  I > II > III    B)  II > I > III    C)  III > II > I    D)  I > III > II    E)  III > I > II

      88.  Which of the following is not a colligative property?

            A)      osmotic pressure                                    D)      boiling point

            B)      vapor pressure                                       E)      freezing point

            C)      density                                                           

 

      89.  Determine the moles of solute particles in 1.0 kg of a 3.0 m CH₃OH solution.

            A)  6.0 moles    B)  3.0 moles    C)  18 moles    D)  12 moles    E)  1.0 mole

 

      90.  Determine the moles of solute particles in 1.0 kg of a 3.0 m Ca(NO₃)₂ solution.

            A)  6.0 moles    B)  3.0 moles    C)  18 moles    D)  9.0 moles    E)  27 mole

 

      91.  Determine the moles of solute particles in 1.0 kg of a 3.0 m C₂H₅OH solution.

            A)  6.0 moles    B)  3.0 moles    C)  18 moles    D)  9.0 moles    E)  27 moles

 

      92.  Rank the following solutions in order of increasing osmotic pressure:  1.0 m C₂H₅OH, 1.0 m Ca(NO₃)₂, 2.0 m NaCl, 3.0 m C₆H₁₂O₆

            A)      C₂H₅OH = Ca(NO₃)₂ < NaCl < C₆H₁₂O₆

            B)      C₆H₁₂O₆ < NaCl < C₂H₅OH = Ca(NO₃)₂

            C)      C₂H₅OH < Ca(NO₃)₂ < NaCl < C₆H₁₂O₆

            D)      C₂H₅OH < Ca(NO₃)₂ = NaCl < C₆H₁₂O₆

            E)      C₂H₅OH < Ca(NO₃)₂ = C₆H₁₂O₆ < NaCl

 

      93.  Rank the following solutions in order of increasing osmotic pressure:  2.0 m CH₃OH, 1.0 m Ba(NO₃)₂, 3.0 m KCl, 3.0 m C₆H₁₂O₆

            A)      Ba(NO₃)₂ < CH₃OH < KCl = C₆H₁₂O₆

            B)      C₆H₁₂O₆  = KCl < CH₃OH < Ba(NO₃)₂

            C)      CH₃OH < Ba(NO₃)₂ = C₆H₁₂O₆ < KCl

            D)      CH₃OH < Ba(NO₃)₂ < C₆H₁₂O₆ < KCl

            E)      KCl < CH₃OH < Ba(NO₃)₂ < C₆H₁₂O₆

 

      94.  Rank the following solutions in order of increasing osmotic pressure:  1.0 m CH₃OH, 1.0 m Ba(NO₃)₂, 2.0 m KCl, 3.0 m C₆H₁₂O₆

            A)      Ba(NO₃)₂ < CH₃OH < KCl = C₆H₁₂O₆

            B)      C₆H₁₂O₆  = KCl < CH₃OH < Ba(NO₃)₂

            C)      CH₃OH < Ba(NO₃)₂ = C₆H₁₂O₆ < KCl

            D)      CH₃OH < Ba(NO₃)₂ < C₆H₁₂O₆ < KCl

            E)      KCl < CH₃OH < Ba(NO₃)₂ < C₆H₁₂O₆

 

      95.  Vinegar is a mixture of about 5 g of acetic acid to every 95 g of water.  Therefore, the acetic acid is the solvent, and the water is the solute.

 

      96.  Sterling silver is an alloy consisting of silver mixed with a small amount of copper.  Therefore, the silver is the solvent and the copper is the solute.

      97.  The solute in the solution shown in the figure is a nonelectrolyte.

           

 

      98.  The solute in the solution shown in the figure is a nonelectrolyte.

           

 

 

      99.  Gases are more soluble in water at higher temperature.

 

    100.  Gases are more soluble in water at higher pressure.

 

    101.  Solids are generally more soluble in water at higher temperature.

    102.  The solubility of sodium chloride is 35 g/100 g of water at 20^oC.  The solution that would be formed when 46 g of sodium chloride is added to 100.0 g of water at this temperature would consist of 35 g of sodium chloride dissolved in the water, and 11 g of sodium chloride remaining undissolved.

    103.  Percent-by-volume concentrations are often used for solutions with a liquid dissolved in a liquid.

 

    104.  The units of molality are moles of solute per kilogram of solution.

 

    105.  Colligative properties depend on the concentration of the particles in a solution, rather than on their identity.

 

    106.  Compared to a pure solvent, a solution in the same liquid has a lower boiling point.

    107.  The molality of a solution does not change with temperature, whereas the molarity does vary with temperature.

 

    108.  Write a chemical equation that describes the dissolving of HCl(g) in water.

 

    109.  Write a chemical equation that describes the dissolving of CH₃OH(l) in water.

    110.  Explain why it is so difficult to wash grease off of your hands using only water.

 

    111.  When solid sodium hydroxide is dissolved in water, the resulting solution feels warm to the touch.  Explain what this means in regard to the attractive forces in the solution.

 

    112.  The solubility of potassium chloride is 32 g/100 g of water at 20^oC.  Describe the solution that would be formed when 46 g of potassium chloride is added to 100.0 g of water at this temperature.

 

    113.  Calculate the molality of a solution prepared by dissolving 12.5 g of KNO₃ in enough water to make 98.0 g of solution.

 

    114.  What volume of 0.2500 M NaOH is required to neutralize 25.00 mL of 0.2000 M HCl?

 

    115.  What volume of 0.2500 M NaOH is required to neutralize 10.00 mL of 0.4000 M H₂SO₄?

 

    116.  What volume of 0.2500 M NaOH is required to neutralize 50.00 mL of 0.1000 M H₃PO₄?

 

    117.  What changes in temperature and pressure will decrease the solubility of a gas in solution?

 

    118.  The solubility of NaCl at 30^oC is 36.3 g/100 g of water.  What mass of NaCl is contained in a saturated solution that contains 300.0 grams of water?

 

    119.  A solution is prepared by dissolving 100.0 g of cesium chloride (CsCl) in 100.0 g of water.  The density of the solution is 1.58 g/cm³.  Calculate the mass percent of the cesium chloride.

 

    120.  A solution is prepared by dissolving 100.0 g of cesium chloride (CsCl) in 100.0 g of water.  The density of the solution is 1.58 g/cm³.  Calculate the molarity of the cesium chloride.

 

    121.  A solution is prepared by dissolving 100.0 g of cesium chloride (CsCl) in 100.0 g of water.  The density of the solution is 1.58 g/cm³.  Calculate the molality of the cesium chloride.

 

    122.  When solutions of silver nitrate, AgNO₃, and calcium iodide, CaI₂, are mixed, a yellow precipitate of silver iodide is formed. Write the balanced equation for the reaction.

 

    123.  When solutions of silver nitrate, AgNO₃, and calcium iodide, CaI₂, are mixed, a yellow precipitate of silver iodide is formed. Calculate the mass of silver iodide that is formed if 50.00 mL of 1.00 M AgNO₃ is combined with 30.00 mL of 1.25 M CaI₂.