General, organic biological chemistry, 5e chapter 9

Which of the following correctly describes the solubility of the solute?A mineral oil, soluble in water B CaCl2, soluble in hexane C NaHCO3, soluble in water D CCl4, soluble in water E o

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General, Organic & Biological Chemistry, 5e (Timberlake)

Chapter 9 Solutions

9.1 Multiple-Choice Questions

1) The O-H bond in water is polar because

A) it is an ionic bond

B) oxygen is much more electronegative than hydrogen

C) oxygen occupies more space than hydrogen

D) hydrogen is much more electronegative than oxygen

B) a covalent bond between H and O

C) an ionic bond between H and another atom

D) a bond that is stronger than a covalent bond

E) the polar O-H bond in water

Answer: A

Objective: 9.1

Global Outcomes: GO2

3) Hydrogen bonds are a major factor in the structure of

4) In a solution, the solvent

A) is a liquid

B) can be a liquid or gas

C) can be a solid, liquid, or gas

D) is never a solid

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5) Which of the following molecules can form hydrogen bonds?

6) A solution is prepared by dissolving 2 g of KCl in 100 g of H2O In this solution, H2O is theA) solute

7) Oil does not dissolve in water because

8) When KCl dissolves in water

A) the Cl- ions are attracted to dissolved K+ ions

B) the Cl- ions are attracted to the partially negative oxygen atoms of the water molecule.C) the K+ ions are attracted to Cl- ions on the KCl crystal

D) the K+ ions are attracted to the partially negative oxygen atoms of the water molecule.E) the K+ ions are attracted to the partially positive hydrogen atoms of the water molecule.Answer: D

Objective: 9.1

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9) Water is a polar solvent and hexane (C6H14) is a nonpolar solvent Which of the following correctly describes the solubility of the solute?

A) mineral oil, soluble in water

B) CaCl2, soluble in hexane

C) NaHCO3, soluble in water

D) CCl4, soluble in water

E) octane, soluble in water

Answer: C

Objective: 9.1

10) In water, a substance that ionizes completely in solution is called a

11) In water, a substance that partially ionizes in solution is called a

A) the amount of ion that has a 1+ charge

B) the amount of ion that has a 1- charge

C) the amount of ion that carries 1 mole of electrical charge

D) 1 mole of any ion

E) 1 mole of an ionic compound

Answer: C

Objective: 9.2

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13) How many equivalents are present in 5.0 g of Al3+?

14) How many equivalents are present in 5.0 moles of Al3+?

15) An intravenous replacement solution contains 4.0 mEq/L of Ca2+ ions How many grams

of Ca2+ are in 3.0 L of the solution?

16) How many equivalents are present in 0.40 moles of SO42-?

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17) When some of the sugar added to iced tea remains undissolved at the bottom of the glass, the solution is

18) The solubility of KI is 50 g in 100 g of H2O at 20 °C If 110 grams of KI are added to 200 grams of H2O

A) all of the KI will dissolve

B) the solution will freeze

C) the solution will start boiling

D) a saturated solution will form

E) the solution will be unsaturated

Answer: D

Objective: 9.3

19) An increase in the temperature of a solution usually

A) increases the boiling point

B) increases the solubility of a gas in the solution

C) increases the solubility of a solid solute in the solution

D) decreases the solubility of a solid solute in the solution

E) decreases the solubility of a liquid solute in the solution

Answer: C

Objective: 9.3

20) Which one of the following compounds will NOT be soluble in water?

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21) Which one of the following compounds will NOT be soluble in water?A) LiOH

22) Which one of the following compounds will be soluble in water?A) AgCl

23) Which one of the following compounds will be soluble in water?A) AgBr

24) Which one of the following compounds will be insoluble in water?A) AgNO3

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25) When solutions of KCl and Pb(NO3)2 are mixed, a precipitate forms Which of the following is the balanced equation for the double replacement reaction that occurs?

A) KCl(aq) + Pb(NO3) 2(aq) → KNO3(aq) + PbCl2(s)

B) KNO3(aq) + PbCl2(s) → KCl(aq) + Pb(NO3) 2(aq)

C) K+(aq) + NO3-(aq) → KNO3(aq)

D) 2KCl (aq) + Pb(NO3)2(aq) → 2KNO3(aq) + PbCl2 (s)

E) KCl(aq) + Pb(NO3)2(aq) → KNO3(aq) + PbCl(s)

Answer: D

Objective: 9.3

26) When solutions of NaCl and AgNO3 are mixed,

A) a precipitate of AgCl forms

B) a precipitate of NaNO3 forms

C) no precipitate forms

D) precipitate of NaNO3 and AgCl form

E) a precipitate of AgCl2 forms

Answer: A

Objective: 9.3

27) According to Henry's law, the solubility of a gas in a liquid

A) decreases as the gas pressure above the liquid increases

B) increases as the gas pressure above the liquid increases

C) remains the same as the temperature increases

D) depends on the liquid polarity

E) depends on the liquid density

Answer: B

Objective: 9.3

28) The mass percent concentration refers to

A) grams of solute in 1 kg of solvent

B) grams of solute in 1 kg of solution

C) grams of solute in 100 g of solvent

D) grams of solute in 100 g of solution

E) grams of solvent in 100 g of solution

Answer: D

Objective: 9.4

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29) The mass/volume percent concentration refers to

A) grams of solute in 1 L of solvent

B) grams of solute in 1 L of solution

C) grams of solute in 100 mL of solvent

D) grams of solute in 100 mL of solution

E) grams of solvent in 100 mL of solution

Answer: D

Objective: 9.4

30) What is the concentration, in mass percent, of a solution prepared from 50.0 g NaCl and 150.0 g of water?

31) Rubbing alcohol is 70.% isopropyl alcohol by volume How many mL of isopropyl alcohol are in a 1 pint (473 mL) container?

32) What is the concentration, in m/v percent, of a solution prepared from 50 g NaCl and 2.5

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33) How many grams of glucose are needed to prepare 400 mL of a 2.0%(m/v) glucose solution?

34) A patient needs to receive 85 grams of glucose every 12 hours What volume of a 5.0%(m/v) glucose solution needs to be administered to the patient each 12 hours?

35) What volume (mL) of a 15% (m/v) NaOH solution contains 120 g NaOH?

36) How many milliliters of a 25% (m/v) NaOH solution would contain 75 g of NaOH?

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37) What is the molarity of a solution that contains 17 g of NH3 in 0.50 L of solution?

38) What is the molarity of a solution that contains 3.25 moles of NaNO3 in 250 mL of solution?

39) When 200 mL of water are added to 100 mL of 12% KCl solution the final concentration

of KCl is (Assume the volumes add.)

40) The molarity (M) of a solution refers to

A) moles of solute/L of solution

B) moles of solute/L of solvent

C) moles of solute/100 mL of solution

D) grams of solute/100 mL of solution

E) grams of solute/L of solution

Answer: A

Objective: 9.4

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41) What is the molarity of a solution containing 5.0 moles of KCl in 2.0 L of solution?A) 2.5 M

42) What is the molarity of a solution which contains 58.5 g of sodium chloride dissolved in 0.500 L of solution?

43) How many moles of CaCl2 are in 250 mL of a 3.0 M of CaCl2 solution?

44) What volume of a 1.5 M KOH solution is needed to provide 3.0 moles of KOH?

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45) How many grams of PbCl2 are formed when 25.0 mL of 0.654 M KCl react with

46) How many mL of 0.246 M Pb(NO3)2 are needed to react with 36.0 mL of 0.322 M KCl ?

2KCl(aq) + Pb(NO3) 2(aq) → 2KNO3(aq) + PbCl2(s)

47) Use the reaction: 2AgNO3(aq) + H2SO4(aq) → Ag2SO4(s) + 2H2O(l)

What volume of 0.123 M AgNO3(aq) is needed to form 0.657 g of Ag2SO4(s)?

48) During the process of diluting a solution to a lower concentration,

A) the amount of solute does not change

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Answer: B

Objective: 9.5

50) What volume of 2.5% (m/v) KOH can be prepared from 125 mL of a 5.0% KOH solution?A) 0.0040 mL

51) What volume of 0.10 M NaOH can be prepared from 250 mL of 0.30 M NaOH?

52) What volume of a 2.00 M KCl solution is required to prepare 500 mL of a 0.100 M KCl solution?

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53) What is the new mass/volume (m/v)% of a KOH solution that is prepared by diluting 110

54) A homogeneous mixture that does not settle out upon standing is

55) In the process known as osmosis, moves through a semipermeable membrane into an area of concentration

A) solute; lower solute

B) solute; higher solute

C) solvent; lower solute

D) solvent; lower solvent

E) solvent; higher solvent

Answer: D

Objective: 9.6

For the question(s) that follow, consider a 4% starch solution and a 10% starch solution separated by a semipermeable membrane.

56) Which starch solution will decrease in volume as osmosis occurs?

A) 4%

B) 10%

C) Neither exerts osmotic pressure

D) They exert equal osmotic pressures

E) They exert opposite osmotic pressures

Answer: A

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57) The process that occurs in this system is

58) Which of the following occurs in this system?

A) Water flows equally in both directions

B) There is a net flow of water from the 4% starch solution into the 10% starch solution.C) There is a net flow of water from the 10% starch solution into the 4% starch solution.D) Water does not cross the membrane at all

E) Starch moves out of the 10% starch solution into the 4% starch solution

Answer: B

Objective: 9.6

59) A solution with the same osmotic pressure as the blood is

A) isotonic to the blood

B) hypotonic to the blood

C) hypertonic to the blood

D) nontonic to the blood

E) molar to the blood

Answer: A

Objective: 9.6

60) A solution that has an osmotic pressure less than that of red blood cells is calledA) saturated

61) A red blood cell will undergo crenation in

A) water

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Objective: 9.6

63) A red blood cell will undergo hemolysis in

64) The process by which a semipermeable membrane allows water molecules, small molecules, and ions to pass through while retaining large particles is called

65) An aqueous mixture containing starch (a colloid), NaCl, glucose, and albumin (a colloid)

is placed in a dialyzing bag and immersed in distilled water Which of the following correctly describes the location of the indicated substance after dialysis?

A) albumin, inside

B) starch outside

C) albumin inside and outside

D) water inside only

E) starch inside and outside

Answer: A

Objective: 9.6

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66) 1.0 mole of NaCl is added to 1.0 kg of water The freezing point of the solution will be the freezing point of pure water.

67) 0.50 mole of KCl is added to 2.0 kg of water The boiling point of the solution will be the boiling point of pure water

68) 0.50 mole of NaCl is added to 1.0 kg of water The freezing point of the solution will be

69) What is the osmolarity of a solution made by dissolving 0.50 mole of the strong

electrolyte CaCl2 in 1.0 L of solution?

70) What is the osmolarity of a solution made by dissolving 25.0 g of the strong electrolyte KCl in 1.0 L of solution?

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D) strong electrolyte

E) ionic compound

Answer: C

Objective: 9.2

2) NaCl can be classified as a

3) Methanol, CH3OH, can be classified as a

4) The molarity of a solution of 5.0 g of KCl in 100 mL of solution is A) 0.038 M

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5) If 100 mL of water is added to 25 mL of 5.0 M NaCl, the final concentration is A) 25 M

6) Using a kidney machine to remove waste products from the blood is known as .A) osmosis

7) A mixture in which one component settles is called a(n)

9.3 Short Answer Questions

1) A substance that carries an electric current when dissolved in water is called a(n)

Answer: electrolyte

Objective: 9.2

2) A substance that produces only a small number of ions in solution is known as a electrolyte

Answer: weak

Objective: 9.2

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4) A solution of sodium carbonate, Na2CO3, that has a molarity of 0.0100 M contains equivalents of sodium ions per liter of the solution.

Answer: 0.0200

Objective: 9.2

5) Is barium sulfate, BaSO4, soluble or insoluble in water?

Answer: insoluble

Objective: 9.3

6) In the following equation, will form a precipitate

NaCl + AgNO3 → AgCl + NaNO3

Answer: AgCl

Objective: 9.3

7) In the following equation, will form a precipitate

BaCl2 + H2SO4 → BaSO4 + 2HCl

Answer: BaSO4

Objective: 9.3

8) The number of moles of a compound dissolved in one liter of a solution is called the

Answer: molarity

Objective: 9.4

9) If 25.0 mL of a 0.800 M KCl solution is diluted to a final volume of 100 mL, the new concentration is

Answer: 0.200 M

Objective: 9.4

10) Substances whose particles in solution scatter light and pass through filters but cannot pass through semipermeable membranes are called

Answer: colloids

Objective: 9.6

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2) the major attraction between water molecules

Objective: 9.1

3) the association of several water molecules with ions produced in a solutionObjective: 9.1

4) a solution in which more solute can be dissolved

Objective: 9.3

5) a solution that has a higher osmotic pressure than the red blood cells of the bodyObjective: 9.6

Answers: 1) E 2) B 3) F 4) C 5) D

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Match the type of mixture with the appropriate characteristics.

7) a mixture whose particles settle on standing

Objective: 9.6

8) a homogeneous mixture in which suspended particles cannot pass through a

semipermeable membrane

Objective: 9.6

9) a mixture whose particles cannot be separated by filters or semipermeable membranesObjective: 9.6

10) a mixture whose particles can be separated by filters

Objective: 9.6

Answers: 6) C 7) A 8) B 9) C 10) A

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Compare the osmotic pressure of these solutions to the osmotic pressure of red blood cells.

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Indicate whether each of the following compounds dissolves in water to give ions, molecules, or both.

17) HI, a strong electrolyte

Objective: 9.2

18) CH3CH2OH, a nonelectrolyte

Objective: 9.2

19) KNO3, a strong electrolyte

Objective: 9.2

20) glucose, a nonelectrolyte

Objective: 9.2

21) H2CO3, a weak electrolyte

Objective: 9.2

Answers: 16) B 17) A 18) C 19) B 20) C 21) A

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