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
answer
e. hydrogen bonding between water molecules
question
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.
answer
b. the dispersion of argon atoms produces an increase in disorder.
question
Hydration is a specific example of the phenomenon known generally as __________.
a. solvation
b. disordering
c. dilution
d. salutation
e. condensation
answer
a. solvation
question
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.
answer
b. polar solvents dissolve polar solutes and nonpolar solvents dissolve nonpolar solutes.
question
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
answer
e. hydration
question
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
answer
a. the rate of crystallization = the rate of dissolution
question
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
answer
a. hydrates
question
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
answer
c. has a concentration lower than the solubility
question
A solution with a concentration higher than the solubility is __________.
a. unsaturated
b. supersaturated
c. not possible
d. saturated
e. supercriticl
answer
b. supersaturated
question
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
answer
b. is one with a higher concentration than the solubility
question
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
answer
b. weak solvation of Na+ and Cl- by C6H6
question
Which one of the following vitamins is water soluble?
a. A
b. B
c. K
d. D
e. E
answer
b. B
question
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
answer
d. HOCH2CH2OH
question
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
answer
b. CCl4
question
Which of the following substances is more likely to dissolve in CH3OH?
a. CCl4
b. H2
c. Kr
d. CH3CH2OH
e. N2
answer
d. CH3CH2OH
question
Which one of the following substances is more likely to dissolve in CCl4?
a. CH3CH2OH
b. NaCl
c. CBr4
d. HCl
e. HBr
answer
c. CBr4
question
Which one of the following substances is more likely to dissolve in benzene (C6H6)?
a. CCl4
b. HBr
c. CH3CH2OH
d. NH3
e. NaCl
answer
a. CCl4
question
Which one of the following is most soluble in water?
a. CH3OH
b. CH3CH2CH2OH
c. CH3CH2OH
d. CH3CH2CH2CH2OH
e. CH3CH2CH2CH2CH2OH
answer
a. CH3OH
question
Which one of the following is least soluble in water?
a. CH3OH
b. CH3CH2CH2CH2OH
c. CH3CH2CH2CH2CH2OH
d. CH3CH2OH
e. CH3CH2CH2OH
answer
c. CH3CH2CH2CH2CH2OH
question
Which one of the following is most soluble in hexane (C6H14)?
a. Ch3OH
b. CH3CH2CH2OH
c. CH3CH2OH
d. CH3CH2CH2CH2OH
e. CH3CH2CH2CH2CH2OH
answer
e. CH3CH2CH2CH2CH2OH
question
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
answer
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
question
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.
answer
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
question
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.
answer
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
question
Pressure has an appreciable effect on the solubility of __________ in liquids.
a. solids
b. solids and liquids
c. gases
d. salts
e. liquids
answer
c. gases
question
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.
answer
e. The weaker the attraction between the solute and solvent molecules, the greater the solubility.
question
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
answer
c. CCl4 < CHCl3 < NaNO3
question
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
answer
b. N2
question
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.
answer
c. the urge to breathe is reduced and not enough CO2 is removed from the body.
question
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.
answer
e. The density of the solution is needed to solve the problem.
question
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.
answer
e. The density of the solution is needed to solve the problem.
question
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
answer
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+
question
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
answer
b. moles solute/kg solvent
question
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
answer
b. molarity
question
Of the concentration units below, only __________ uses kg of solvent in its calculation.
a. molality
b. mass %
c. molarity
d. ppb
e. ppm
answer
a. molality
question
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
answer
b. 100 g of the solution contains 11 g of sodium chloride
question
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
answer
d. 1.0 g of the solution contains 15 x 10^-6 g of benzene
question
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
answer
b. Al(ClO4)3
more moles = less pressure
question
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
answer
e. sucrose
less moles = more pressure
question
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
answer
c. solvent
question
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
answer
e. decreases, decreases
Boiling point elevation
freezing point depression
question
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)
answer
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
question
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)
answer
a. pure H2O
question
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)
answer
d. aqueous FeI3 (0.030 m)
question
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)
answer
a. pure H2O
question
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
answer
c. KCl
1.4 = i(.52)(1.35)
i=2
KCl = 2 moles
question
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
answer
b. Al(NO3)3
more moles = lower boiling point
question
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
answer
e. sucrose
question
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
answer
e. 0.10 m Na2SO4
question
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
answer
e. 3.00
question
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
answer
b. Na2SO4
question
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
answer
d. the van't Hoff factor
question
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
answer
e. the increase of reaction rates with increase in temperature
question
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
answer
b. 23.48 mm Hg
Psolution = Xsolv * Psolv
Psolution = .988 * 23.76
question
The process of a substance sticking to the surface of another is called
a. adsorption
b. diffusion
c. effusion
d. absorption
e. coagulation
answer
a. adsorption
question
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
answer
d. a homogeneous mixture
question
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
answer
b. can be stabilized by adsorption of ions
Haven't found what you need?
Search for quizzes and test answers now
Quizzes.studymoose.com uses cookies. By continuing you agree to our cookie policy
