Chemistry: Chapter 13 Review: Properties of Solutions

Pressure has an appreciable effect on the solubility of __________ in liquids. a. solids b. solids and liquids c. gases d. salts e. liquids

c. gases

An unsaturated solution is one that __________. a. has no double bonds b. contains no solute c. has a concentration lower than the solubility d. contains more dissolved solute than the solubility allows e. contains the maximum concentration of solute possible, and is in equilibrium with undissolved solute

c. has a concentration lower than the solubility

The magnitudes of Kf and Kb depend on the identity of the __________. a. solution b. solute and solvent c. solvent d. solute e. solvent and on temperature

c. solvent

If the partial pressure of oxygen in the air a diver breathes is too great, __________. a. respiratory tissue is damaged by oxidation b. hyperventilation results c. the urge to breathe is reduced and not enough CO2 is removed from the body d. the urge to breathe is increased and excessive CO2 is removed from the body e. No problems result from this situation.

c. the urge to breathe is reduced and not enough CO2 is removed from the body.

The most likely van't Hoff factor for an 0.01 m CaI2 solution is __________. a. 3.29 b. 1.27 c. 1.00 d. 2.69 e. 3.00

e. 3.00

The solubility of nitrogen gas at 25C and 1 atm is 6.8 x 10^-4 mol/L. If partial pressure of nitrogen gas in air is 0.76 atm, what is the concentration (molarity) of dissolved nitrogen? a. 5.2 x 10^-4 M b. 6.8 x 10^-4 M c. 3.8 x 10^-4 M d. 1.1 x 10^-5 M e. 4.9 x 10^-4 M

a. 5.2 x 10^-4 M S = Solubility P = Partial Pressure K = Constant (proportionality) S=KP s/p = K K = 6.8 x 10^-4/1 (6.8 x 10^-4)(.76) = 5.2 x 10^-4

Which one of the following substances is more likely to dissolve in benzene (C6H6)? a. CCl4 b. HBr c. CH3CH2OH d. NH3 e. NaCl

a. CCl4

Which one of the following is most soluble in water? a. CH3OH b. CH3CH2CH2OH c. CH3CH2OH d. CH3CH2CH2CH2OH e. CH3CH2CH2CH2CH2OH

a. CH3OH

The process of a substance sticking to the surface of another is called a. adsorption b. diffusion c. effusion d. absorption e. coagulation

a. adsorption

Compounds composed of a salt and water combined in definite proportions are known as __________. a. hydrates b. homogenates c. ionic solids d. clathrates e. molecular solids

a. hydrates

Of the concentration units below, only __________ uses kg of solvent in its calculation. a. molality b. mass % c. molarity d. ppb e. ppm

a. molality

Which of the following liquids will have the highest freezing point? a. pure H2O b. aqueous CoI2 (0.030 m) c. aqueous FeI3 (0.030 m) d. aqueous NaI (0.030 m) e. aqueous glucose (0.050 m)

a. pure H2O

Which of the following liquids will have the highest freezing point? a. pure H2O b. aqueous FeI3 (.24 m) c. aqueous glucose (0.60 m) d. aqueous sucrose (0.60 m) e. aqueous KF (0.50 m)

a. pure H2O

Hydration is a specific example of the phenomenon known generally as __________. a. solvation b. disordering c. dilution d. salutation e. condensation

a. solvation

In a saturated solution of a salt in water, __________. a. the rate of crystallization = the rate of dissolution b. seed crystal addition may cause massive crystallization c. addition of more water causes massive crystallization d. the rate of crystallization > the rate of dissolution e. the rate of dissolution > the rate of crystallization

a. the rate of crystallization = the rate of dissolution

A solution contains 11% by mass of sodium chloride. This means that __________. a. there are 11 g of sodium chloride in 1.0 mL of this solution b. 100 g of the solution contains 11 g of sodium chloride c. the molality of the solution is 11 d. 100 mL of the solution contains 11 g of sodium chloride e. the density of the solution is 11g/mL

b. 100 g of the solution contains 11 g of sodium chloride

Calculate the vapor pressure of a solution made by dissolving 109 grams of glucose (molar mass = 180.2 g/mol) in 920.0 mL of water at 25C. The vapor pressure of pure water at 25C is 23.76 mm Hg. Assume the density of the solution is 1.00 g/mL. a. 0.278 mm Hg b. 23.48 mm Hg c. 22.98 mm Hg d. 0.605 mm Hg e. 23.76 mm Hg

b. 23.48 mm Hg Psolution = Xsolv * Psolv Psolution = .988 * 23.76

The concentration of CO2 in a soft drink with a partial pressure of CO2 of 4.0 atm over the liquid at 25C is 1.2 x 10^-1 M. The Henry's law constant for CO2 at this temperature is _________. a. 5.6 x 10^-3 mol/L-atm b. 3.0 x 10^-2 mol/L-atm c. 4.5 x 10^-3 mol/L-atm d. 2.3 x 10^-2 mol/L-atm e. More information is needed to solve the problem.

b. 3.0 x 10^-2 mol/L-atm S = solubility p = partial pressure K = constant (proportionality S = Kp K = S/P 1.2 x 10^-1/4 = 3.0 x 10^-2 mol/L-atm

A 0.100 m solution of which one of the following solutes will have the lowest vapor pressure? a. sucrose b. Al(ClO4)3 c. NaCl d. KClO4 e. Ca(ClO4)2

b. Al(ClO4)3 more moles = less pressure

Of the following, a 0.1 M aqueous solution of __________ will have the lowest freezing point. a. NaCl b. Al(NO3)3 c. Na2SO4 d. K2CrO4 e. sucrose

b. Al(NO3)3 more moles = lower boiling point

Which one of the following vitamins is water soluble? a. A b. B c. K d. D e. E

b. B

Which of the following substances is least likely to dissolve in water? a. CHCl3 b. CCl4 c. CH3(CH2)8CH2OH d. HOCH2CH2OH e. CH3(CH2)9COH

b. CCl4

Which component of air is the primary problem in a condition known as "the bends"? a. CO2 b. N2 c. O2 d. He e. CO

b. N2

Which one of the following solutes has a limiting van't Hoff factor (i) of 3 when dissolved in water? a. CCl4 b. Na2SO4 c. KNO3 d. CH3OH e. sucrose

b. Na2SO4

Hydrophobic colloids __________. a. will separate into two phases if they are stabilized b. can be stabilized by adsorption of ions c. are those that contain water d. are those that do not contain water e. can be stabilized by coagulation

b. can be stabilized by adsorption of ions

A supersaturated solution _________. a. exists only in theory and cannot actually be prepared b. is one with a higher concentration than the solubility c. must be in contact with undissolved solid d. is one with more than one solute e. is one that has been heated

b. is one with a higher concentration than the solubility

Which one of the following concentration units varies with temperature? a. mass percent b. molarity c. molality d. mole fraction e. all of the above

b. molarity

Molality is defined as the __________. a. moles solute/moles solvent b. moles solute/kg solvent c. moles solute/kg solution d. moles solute/liters solution e. none (dimensionless

b. moles solute/kg solvent

The phrase "like dissolves like" refers to the fact that __________. a. solvents can only dissolve solutes of similar molar mass b. polar solvents dissolve polar solutes and nonpolar solvents dissolve nonpolar solutes. c. polar solvents dissolve nonpolar solutes and vice versa. d. condensed phases can only dissolve other condensed phases. e. gases can only dissolve other gases.

b. polar solvents dissolve polar solutes and nonpolar solvents dissolve nonpolar solutes.

A solution with a concentration higher than the solubility is __________. a. unsaturated b. supersaturated c. not possible d. saturated e. supercriticl

b. supersaturated

When argon is placed in a container of neon, the argon spontaneously disperses throughout the neon because __________. a. of solvent-solute interactions b. the dispersion of argon atoms produces an increase in disorder c. of the large attractive forces between argon and neon atoms. d. of hydrogen bonding e. a decrease in energy occurs when the two mix.

b. the dispersion of argon atoms produces an increase in disorder.

The principal reason for the extremely low solubility of NaCl in benzene (C6H6) is the __________. a. strong solvent-solvent interactions b. weak solvation of Na+ and Cl- by C6H6 c. hydrogen bonding in C6H6 d. increased disorder due to mixing of solute and solvent e. strength of the covalent bond in NaCl

b. weak solvation of Na+ and Cl- by C6H6

The concentration of CO2 in a soft drink bottled with a partial pressure of CO2 of 6.5 atm over the liquid at 29C is 2.2 x 10^-1 M. The Henry's law constant for CO2 at this temperature is __________. a. 5.6 x 10^-3 mol/L-atm b. 2.2 x 10^-1 mol/L-atm c. 3.4 x 10^-2 mol/L-atm d. 7.6 x 10^-3 mol/L-atm e. More information is needed to solve the problem.

c. 3.4 x 10^-2 mol/L-atm S = solubility p = partial pressure K = constant (proportionality) S = Kp K = s/p 2.2 x 10^-1/6.5 = .034 = 3.4 x 10^-2 mol/L-atm

Which one of the following substances is more likely to dissolve in CCl4? a. CH3CH2OH b. NaCl c. CBr4 d. HCl e. HBr

c. CBr4

Which of the following choices has the compounds correctly arranged in order of increasing solubility in water? (least soluble to most soluble) a. CH4 < NaNO3 < CHCl3 b. CH3OH <Cl4 < CHCl3 c. CCl4 < CHCl3 < NaNO3 d. LiF < NaNO3 < CHCl3 e. CH3OH < CH4 < LiF

c. CCl4 < CHCl3 < NaNO3

Which one of the following is least soluble in water? a. CH3OH b. CH3CH2CH2CH2OH c. CH3CH2CH2CH2CH2OH d. CH3CH2OH e. CH3CH2CH2OH

c. CH3CH2CH2CH2CH2OH

A 1.35 m aqueous solution of compound X had a boiling point of 101.4C. Which one of the following could be compound X? The boiling point elevation constant for water is .52C/m. a. CH3CH2OH b.C6H12O6 c. KCl d. CaCl2 e. Na3PO4

c. KCl 1.4 = i(.52)(1.35) i=2 KCl = 2 moles

Which of the following liquids will have the lowest freezing point? a. pure H2O b. aqueous FeI3 (0.24 m) c. aqueous KF (0.50 m) d. aqueous sucrose (0.60 m) e. aqueous glucose (0.60 m)

c. aqueous KF 0.50 m) change in Tf = -(4)(Kf)(.24) greater change in temperature Tf = -(2)(Kf)(.5) (-1)Kf(.6) (-1)KF(.6) change in Tf = -i (number of moles) Kf (constant) m

A solution contains 15 ppm of benzene. The density of the solution is 1.00 g/mL. This means that __________. a. 100 g of the solution contains 15 g of benzene b. 1.0 L of the solution contains 15 g of benzene c. there are 15 mg of benzene in 1.0 g of this solution d. 1.0 g of the solution contains 15. 10^-6 g of benzene. e. the solution is 15% by mass of benzene

d. 1.0 g of the solution contains 15 x 10^-6 g of benzene

Which of the following substances is more likely to dissolve in CH3OH? a. CCl4 b. H2 c. Kr d. CH3CH2OH e. N2

d. CH3CH2OH

Which of the following substances is more likely to dissolve in water? a. CH3(CH2)8CH2OH b. CHCl3 c. CH3(Ch2)9COH d. HOCH2CH2OH e. CCl4

d. HOCH2CH2OH

Which of the following cannot be a colloid? a. an emulsion b. an aerosol c. a foam d. a homogeneous mixture e. All of the above are colloids

d. a homogeneous mixture

Which of the following liquids will have the lowest freezing point? a. pure H2O b. aqueous NaI (0.030 m) c. aqueous glucose (0.050 m) d. aqueous FeI3 (0.030 m) e. aqueous CoI2 (0.030 m)

d. aqueous FeI3 (0.030 m)

The ratio of the actual value of a colligative property to the value calculated, assuming the substance to be a nonelectrolyte, is referred to as __________. a. vapor pressure lowering b. Henry's law c. osmotic pressure d. the van't Hoff factor e. freezing point depression

d. the van't Hoff factor

Which of the following aqueous solutions will have the highest boiling point ? a. 0.10 m NaCl b. 0.10 m SrSO4 c. 0.20 m glucose d. 0.25 m sucrose e. 0.10 m Na2SO4

e. 0.10 m Na2SO4

A solution is prepared by dissolving calcium chloride in water and diluting to 500.0 mL. If this solution contains 44 ppm chloride ions, the concentration of calcium ions is __________ ppm. a. 88 b. 44 c. 500 d. 11 e. 22

e. 22 1 ppm = 1mg solute/1L solution 44 ppm = x/.5 L solution (500 mL = .5L) X mg = 22 22/.5 = 11 11 mg/.5 = 22mg Ca+

Which one of the following is most soluble in hexane (C6H14)? a. Ch3OH b. CH3CH2CH2OH c. CH3CH2OH d. CH3CH2CH2CH2OH e. CH3CH2CH2CH2CH2OH

e. CH3CH2CH2CH2CH2OH

Calculate the molarity of 17.5% (by mass) aqueous solution of nitric acid. a. 4.33 m b. 2.74 m c. 0.274 m d. 3.04 m e. The density of the solution is needed to solve the problem.

e. The density of the solution is needed to solve the problem.

Calculate the molarity of a 10.0% (by mass) aqueous solution of hydrochloric acid. a. 4.33 m b. 0.274 m c. 3.04 m d. 2.74 m e. The density of the solution is needed to solve the problem.

e. The density of the solution is needed to solve the problem.

Which of the following statements is false? a. Substances with similar intermolecular attractive forces tend to be soluble in one another. b. The solubility of a gas increases in direct proportion to its partial pressure above the solution. c. The solubility of gases in water decreases with increasing temperature. d. Nonpolar liquids tend to be insoluble in polar liquids. e. The weaker the attraction between the solute and solvent molecules, the greater the solubility.

e. The weaker the attraction between the solute and solvent molecules, the greater the solubility.

As the concentration of a solute in a solution increases, the freezing point of the solution __________ and the vapor pressure of the solution __________. a. decreases, is unaffected b. increases, increases c. increases, decreases d. decreases, increases e. decreases, decreases

e. decreases, decreases Boiling point elevation freezing point depression

When solutions of strong electrolytes in water are formed, the ions are surrounded by water molecules. These interactions are described as a case of __________. a. dehydration b. supersaturation c. crystallization d. saturation e. hydration

e. hydration

The dissolution of water in octane (C8H18) is prevented by __________. a. London dispersion forces between octane molecules b. repulsion between like-charged water and octane molecules c. dipole-dipole attraction between octane molecules d. ion-dipole attraction between water and octane molecules e. hydrogen bonding between water molecules

e. hydrogen bonding between water molecules

Of the following, a 0.1 M aqueous solution of __________ will have the highest freezing point. a. K2CrO4 b. Al(NO3)3 c. Na2SO4 d. NaCl e. sucrose

e. sucrose

A 0.100 m solution of which one of the following solutes will have the highest vapor pressure? a. Al(ClO4)3 b. Cl(ClO4)2 c. NaCl d. KClO4 e. sucrose

e. sucrose less moles = more pressure

Colligative properties of solutions include all of the following except __________. a. elevation of the boiling point of a solution upon addition of a solute to a solvent b. depression of vapor pressure upon addition of a solute to a solvent. c. depression of the freezing point of a solution upon addition of a solute to a solvent d. an increase in the osmotic pressure of a solution upon the addition of more solute. e. the increase of reaction rates with increase in temperature

e. the increase of reaction rates with increase in temperature