Deck 8: Solutions

Question 1

The attraction of an ion with a dipole in a molecule is called

A)a dipole-dipole interaction.
B)an ion-dipole interaction.
C)hydrogen bonding.
D)London dispersion forces.
E)van der Waals forces.

Answer 1

B

Question 2

A particular wine contains 11.2% (v/v)ethanol. What volume of ethanol is in a 750.-mL bottle of this wine?

A)84.0 mL ethanol
B)0.840 mL ethanol
C)6.70 mL ethanol
D)14.9 mL ethanol

Answer 2

A

Question 3

Which pair of compounds will form a solution?

A)Benzene (C₆H₆)and hexane (C₆H₁₄)
B)Na₂SO₄ and benzene (C₆H₆)
C)NaCl and hexane (C₆H₁₄)
D)H₂O and CCl₄
E)More than one of the combinations above will form solutions.

Answer 3

A

Question 4

Henry's law states that the solubility of a gas in a liquid is proportional to the

A)partial pressure of the gas above the liquid.
B)temperature of the liquid.
C)temperature of the gas above the liquid.
D)molecular weight of the gas above the liquid.

Question 5

A saline solution used in intravenous drips for patients who cannot take oral fluids contains 0.92% (w/v)NaCl in water. How many grams of NaCl are contained in 575 mL of this solution?

A)53 g NaCl
B)529 g NaCl
C)5.3 g NaCl
D)0.016 g NaCl
E)1.6 g NaCl

Question 6

Which ionic compound is soluble in water?

A)PbBr₂
B)Fe(OH)₃
C)BaSO₄
D)Ca(NO₃)₂
E)More than one of the ionic compounds above is soluble in water.

Question 7

A sample of seawater contains 1.3 g of calcium ions in 3, 100 kg of solution. What is the calcium ion concentration of this solution in units of ppm?

A)4.2 × 10^-4 ppm Ca²⁺ ions
B)0.42 ppm Ca²⁺ ions
C)420 ppm Ca²⁺ ions
D)4.0 ppm Ca²⁺ ions
E)4.0 × 10³ ppm Ca²⁺ ions

Question 8

Nonpolar compounds are soluble in

A)ionic compounds.
B)electrolytes.
C)polar solvents.
D)nonpolar solvents.

Question 9

What is the molarity of a solution made by dissolving 36.29 g of NaCl in 2.30 L of solution?

A)15.78 M NaCl
B)0.0634 M NaCl
C)0.270 M NaCl
D)2.70 M NaCl

Question 10

What is the molarity of a solution made by dissolving 3.09 moles of NaCl in 1.50 L of solution?

A)4.64 M NaCl
B)4.85 M NaCl
C)2.06 M NaCl
D)0.673 M NaCl

Question 11

A saline solution used in intravenous drips for patients who cannot take oral fluids contains 0.92% (w/v)NaCl in water. What volume of the saline solution must be administered to the patient in order to deliver 7.7 g of NaCl?

A)8.4 mL of saline solution
B)840 mL of saline solution
C)7.1 mL of saline solution
D)140 mL of saline solution

Question 12

A solution is made by mixing 569 mL of water and 238 mL ethanol. What is the concentration of ethanol in units of volume/volume percent?

A)41.8% (v/v)ethanol
B)0.418% (v/v)ethanol
C)29.5% (v/v)ethanol
D)0.295% (v/v)ethanol
E)70.5% (v/v)ethanol

Question 13

Which substance is a nonelectrolyte?

A)NaCl
B)(NH₄)₂SO₄
C)H₂O₂
D)KOH

Question 14

A solution is made by dissolving 3.88 g of NaCl in enough water to make 67.8 mL of solution. What is the concentration of sodium chloride in units of weight/volume percent?

A)5.41% (w/v)NaCl
B)94.3% (w/v)NaCl
C)5.72% (w/v)NaCl
D)0.0572% (w/v)NaCl

Question 15

Which ionic compound is not soluble in water?

A)NaCl
B)AgCl
C)(NH₄)₂SO₄
D)Ca(CH₃CO₂)₂

Question 16

How many grams of glucose (C₆H₁₂O₆)are contained in 555 mL of a 1.77 M glucose solution?

A)0.982 g C₆H₁₂O₆
B)177 g C₆H₁₂O₆
C)0.555 g C₆H₁₂O₆
D)0.177 g C₆H₁₂O₆

Question 17

What is the molarity of a solution made by dissolving 4.88 g of KCl in 423 mL of solution?

A)0.0115 M KCl
B)11.5 M KCl
C)1.55 × 10^-4 M KCl
D)0.155 M KCl

Question 18

Which solution contains the smallest number of moles of sucrose (C₁₂H₂₂O₁₁, molar mass = 342.30 g/mol)?

A)2, 000 mL of a 5.0 × 10^-5% (w/v)sucrose solution
B)2, 000 mL of a 5.0 ppm sucrose solution
C)20 mL of a 5.0 M sucrose solution
D)All of the solutions above contain the same number of moles of sucrose.

Question 19

Which is not an example of a solution?

A)a dental filling
B)chicken noodle soup
C)gasoline
D)tap water

Question 20

Which substance is a colloid?

A)mayonnaise
B)a dental filling
C)mint chocolate chip ice cream
D)gasoline

Question 21

Which compound will be the most soluble in water?

A)
B)
C)
D)

Question 22

What is the concentration of a solution formed by adding 65.0 mL of water to 25.0 mL of a 3.2 M NaCl solution?

A)0.89 M NaCl
B)1.2 M NaCl
C)2.3 M NaCl
D)12 M NaCl

Question 23

A flask contains two compartments (A and

A)
B)
B)with equal volumes of solution separated by a semipermeable membrane. Which diagram represents the final level of the liquids if A is initially a 10% (w/v)glucose solution and B is initially a 20% (w/v)glucose solution?
C)

Question 24

An unknown amount of water is added to 75 mL of a 3.5 M aqueous glucose solution. What can be said about the concentration of the resulting solution?

A)The concentration of the resultant glucose solution will be less than 3.5 M.
B)The concentration of the resultant glucose solution will be greater than 3.5 M.
C)The concentration of the resultant glucose solution will remain the same because the amount of glucose has not changed.
D)It is impossible to say anything about the concentration of the resultant glucose solution because the amount of added water has not been provided.

Question 25

A hypotonic solution has _____ osmotic pressure than/as body fluids.

A)a higher
B)a lower
C)the same

Question 26

If cells are placed in a hypertonic solution,

A)water diffuses out of the cells and the cells shrink in a process called hemolysis.
B)water diffuses out of the cells and the cells shrink in a process called crenation.
C)water diffuses into the cells and the cells swell and eventually burst in a process called hemolysis.
D)water diffuses into the cells and the cells swell and eventually burst in a process called crenation.

Question 27

Which compound will be the least soluble in water?

A)
B)
C)
D)

Question 28

Which solution has the greatest mass of solute?

A)2.00 L of a 0.75 M NaCl solution
B)2.00 L of a 0.75 M CaCl₂ solution
C)2.00 L of a 0.75 M Ca(NO₃)₂ solution
D)2.00 L of a 0.75 M Na₂CO₃ solution
E)All of the solutions above have the same mass of solute.

Question 29

Which solution has the highest freezing point?

A)A solution formed by dissolving 0.75 mol of KCl in 1.00 kg of water.
B)A solution formed by dissolving 0.25 mol of KCl in 1.00 kg of water.
C)A solution formed by dissolving 0.75 mol of KCl in 4.00 kg of water.
D)A solution formed by dissolving 0.25 mol of KCl in 0.50 kg of water.
E)All of the solutions described above have the same freezing point.

Question 30

What is the molarity of a 11.5% (w/v)glucose (C₆H₁₂O₆, molar mass 180.16 g/mol)solution?

A)0.0638 M
B)0.638 M
C)1.15 M
D)1.76 M

Question 31

Which solution has the lowest boiling point?

A)A solution formed by dissolving 0.75 mol of KCl in 1.00 kg of water.
B)A solution formed by dissolving 0.75 mol of glucose (C₆H₁₂O₆)in 1.00 kg of water.
C)A solution formed by dissolving 0.75 mol of Ca(NO₃)₂ in 1.00 kg of water.
D)A solution formed by dissolving 0.75 mol of Na₃PO₄ in 1.00 kg of water.
E)All of the solutions described above have the same boiling point.

Question 32

What is the concentration of a solution formed by diluting 25.0 mL of a 3.2 M NaCl solution to 135.0 mL?

A)17 M NaCl
B)0.59 M NaCl
C)0.50 M NaCl
D)2.7 M NaCl

Question 33

What is the molarity of a 25.0% (v/v)aqueous isopropyl alcohol solution? The density of isopropyl alcohol (C₃H₈O, molar mass 60.09 g/mol)is 0.786 g/mL.

A)0.529 M
B)1.18 M
C)0.327 M
D)3.27 M

Question 34

The solubility of a substance is best described by which of the following?

A)the ability of the substance to dissolve in water
B)the ability of the substance to dissociate into ions when dissolved in water
C)the maximum amount of a substance that can dissolve in a specific amount of solvent
D)the mass of solvent necessary to completely dissolve 100 g of the substance

Question 35

Which solution has the highest boiling point?

A)A solution formed by dissolving 0.75 mol of KCl in 1.00 kg of water.
B)A solution formed by dissolving 0.75 mol of glucose (C₆H₁₂O₆)in 1.00 kg of water.
C)A solution formed by dissolving 0.75 mol of Ca(NO₃)₂ in 1.00 kg of water.
D)A solution formed by dissolving 0.75 mol of Na₃PO₄ in 1.00 kg of water.
E)All of the solutions described above have the same boiling point.

Question 36

Which of the following statements concerning a solution is NOT true?

A)A solution is a heterogeneous mixture of two or more pure substances.
B)A solution is composed of a solvent and one or more solutes; the solute(s)dissolve in the solvent.
C)A solution has its components uniformly distributed.
D)A solution is likely to form when the solute(s)and the solvent have similar polarities.

Question 37

What is the maximum volume of a 0.788 M CaCl₂ solution that can be prepared using 85.3 g CaCl₂?

A)1.00 L
B)0.769 L
C)0.975 L
D)67.2 L

Question 38

How many milliliters of a 5.25% (w/v)HCl solution must be used to prepare 250 mL of a 0.175% (w/v)HCl solution?

A)8.3 mL HCl solution
B)7, 500 mL HCl solution
C)230 mL HCl solution
D)240 mL HCl solution
E)8.6 mL HCl solution

Question 39

Which of the following statements concerning solution concentration is NOT true?

A)An unsaturated solution contains less than the maximum amount of solute that can be dissolved in the solvent.
B)A saturated solution contains more than 100 g of dissolved solute.
C)A solution can be made less concentrated by adding additional solvent.
D)The number of moles of solute present in exactly one liter of solution is referred to as the solution's molarity.

Question 40

The maximum level of lead allowed in drinking water is 15 $\mu$ g/kg. What is this concentration in units of parts per million?

A)15 ppm
B)1.5 × 10^-2 ppm
C)1.5 × 10⁴ ppm
D)3.1 ppm

Question 41

A nonvolatile solute makes it harder for solvent molecules to form a crystalline solid, thus decreasing its melting point.

Question 42

For most ionic and molecular solids, solubility generally increases as temperature increases.

Question 43

The greater the number of dissolved particles in a solution, the lower the solution's osmotic pressure.

Question 44

Ethylene glycol is more soluble in water than propane.

Question 45

Only solids dissolve in water to form solutions.

Question 46

The solubility of gases increases with increasing temperature.

Question 47

Dialysis is a process that involves the selective passage of water, protein molecules, and ions across a semipermeable membrane.

Question 48

What interactions are responsible for holding dissolved Cl^- ions in an aqueous solution?

A)ion-ion attractions between K⁺ and Cl^- ions
B)ion-dipole attractions between Cl^- ions and the hydrogen atoms of water
C)ion-dipole attractions between Cl^- ions and the oxygen atom of water
D)hydrogen bonding between the Cl^- ions and water

Question 49

Since living cells are surrounded by biological solutions separated by a semipermeable membrane, the osmotic pressure must be higher in the cell than outside the cell membrane.

Question 50

Magnesium hydroxide can be made by the reaction shown below. If a chemist requires 0.725 moles of NaOH for this reaction, what volume of a 1.50 M NaOH solution is needed to provide this amount? MgCl₂(aq)+ 2 NaOH(aq) $\rightarrow$ Mg(OH)₂(s)+ 2 NaCl(aq)

A)0.483 L of a 1.50 M NaOH solution
B)0.967 L of a 1.50 M NaOH solution
C)1.09 L of a 1.50 M NaOH solution
D)967 mL of a 1.50 M NaOH solution

Question 51

Heptane (C₇H₁₆)is soluble in water.

Question 52

In solution formation, solvation always releases more energy than that required to separate particles, so the overall process is always exothermic.

Question 53

The ionic compound (NH₄)₂SO₄ is soluble in water.

Question 54

Pure water has an osmotic pressure of 1 atm.

Question 55

Any mixture of two or more components is a solution.

Question 56

Methanol (CH₃OH)is soluble in water.

Question 57

Water solubility for neutral molecules occurs only for small polar molecules or those with many O or N atoms that can hydrogen bond to water.

Question 58

The ionic compound CaCO₃ is soluble in water.

Question 59

If the attractive forces between the ions and water are stronger than the attraction between the ions in the crystal, an ionic compound dissolves in water.

Question 60

The solubility of helium gas in water is greater at 25 °C than at 50 °C.

Question 61

The presence of a solute reduces the vapor pressure of the solvent above the solution, raising its boiling point.

Question 62

Liquid solutions are always transparent and colorless.

Question 63

Vitamin D is tested for its solubility in water and benzene (C₆H₆), and is found to be insoluble in water and soluble in benzene. These solubility results indicate that Vitamin D is most likely a nonpolar compound.

Question 64

An aqueous solution with the label 0.25 M sucrose contains 0.25 grams of sucrose in every 1 L of solution.

Question 65

The boiling point of a solution that contains 0.64 mol of Mg(NO₃)₂ in 1.00 kg of water is 100.98 °C.

Question 66

The solubility of Ba(NO₃)₂ in water is lower at 25 °C than at 50 °C.

Question 67

When calculating the concentration of a solution in units of parts per million, the "parts" must be expressed in units of grams.

Question 68

All nonvolatile solutes are ionic compounds that do not readily escape into the vapor phase, and thus they have a negligible vapor pressure at a given temperature.

Question 69

A liquid solution that contains a nonvolatile solute has a higher boiling point than the solvent alone.

Question 70

A solution containing the maximum number of grams of solute that can dissolve in the solvent is said to be supersaturated.

Question 71

Osmosis is the passage of water and small molecules across a semipermeable membrane from a solution of high solute concentration to a solution of lower solute concentration.

Question 72

A 6.10 M NaCl solution is made by adding 356 g of NaCl to a flask that contains 1.00 L of water.

Question 73

Compared to the pure solvent, the freezing point depression caused by adding 0.05 mol of sucrose to 1.0 L of water is greater than the boiling point elevation of the same solution.

Question 74

The solubility of KI in water at 20 °C is 140 g KI/100 g H₂O. If 160 g of KI is mixed with 150 g of water, all of the KI will dissolve and the solution that results will be unsaturated.

Question 75

The concentration unit of weight/volume percent concentration, (w/v)%, is the number of grams of solute dissolved in 100 mL of solution.

Question 76

Dilution is the addition of solute to decrease the concentration of solvent.

Question 77

A solution can be made less concentrated by adding additional solvent.

Question 78

Nonpolar compounds are soluble in nonpolar solvents and insoluble in polar solvents.

Question 79

Colligative properties are properties of a solution that depend on the concentration of the solute particles but not their identity.

Question 80

Sodium chloride is soluble in nonpolar solvents such as octane (C₈H₁₈).