chapter 11 review questions

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General Chemistry: Atoms First, 2e (McMurry and Fay)

Chapter 11 Solutions and Their Properties

11.1 Multiple Choice Questions

1) Which of the following mixtures have components which can be separated by filtration?) colloids

!) solutions

C) suspensions") all of the above

nswer# C

"iff# 1

$opic# %ection 11.1 %olutions

&) %tainless steel is an example of a '''''''' solution.

) gas(solid

!) liuid(liuidC) solid(liuid

") solid(solidnswer# "

"iff# 1


*) +n most liuid solutions, the component present in the larger amount is called the

) dispersed medium.

!) emulsifying agent.C) solute.

") solvent.nswer# ""iff# 1


-) $he rubbing alcohol sold in drug stores often is composed of /0 isopropyl alcohol and */0

water. +n this solution

) isopropyl alcohol is the solvent.

!) water is the solvent.C) both water and isopropyl alcohol are solvents.

") neither water nor isopropyl alcohol is a solvent.

nswer# "iff# 1


1

Copyright © 2014 Pearson Education, Inc.



) Which is not a solution?

) brass

!) fogC) hydrochloric acid

") wine

nswer# !"iff# 1


2) 1/ grams of table sugar 3sucrose, ) is dropped into a bea4er containing 1// grams

of water and stirred until a clear liuid is visible and all of the sugar has dissolved. $his process

may be described as) the formation of a heterogeneous mixture.

!) the formation of a homogeneous solution.

C) sublimation.") the formation of a chemical compound.

nswer# !"iff# 1


) 5or a liuid solution made by dissolving a solid or a gas in a liuid, the

) liuid is the solute.!) liuid is the solvent.

C) solute is the component present in the greatest amount.

") solvent is the component present in the greatest amount.nswer# !

"iff# 1


6) +odine, +&3 s), is more soluble in dichloromethane, C7&Cl&3l ), than in water because

) both iodine and dichloromethane have strong ion8dipole interactions.

!) the dipole8dipole forces in dichloromethane are much stronger than the dispersion forces in

iodine.C) the intermolecular forces are similar in both iodine and dichloromethane.

") iodine is polar and dichloromethane has a large number of hydrogen bonds.

nswer# C"iff# &

$opic# %ection 11.& 9nergy Changes and the %olution :rocess

2




;) Which of the following pairs of liuids are li4ely to be miscible?

) <7 and <

!) and <

C) and <

") and <

nswer# "iff# &


1/) Which of the following pairs of liuids are li4ely to be not miscible?

) and <

!) <7 and <

C) C and

") and

nswer#

"iff# &


11) 5or which case would = H soln be expected to be negative?

) if solute8solute interactions are much greater than solvent8solvent and solute8solvent

interactions

!) if solvent8solvent interactions are much greater than solute8solvent and solute8soluteinteractions

C) if solute8solvent interactions are much greater than solvent8solvent and solute8solute

interactions") if solute8solvent interactions are the same as solvent8solvent and solute8solute interactions

nswer# C

"iff# &$opic# %ection 11.& 9nergy Changes and the %olution :rocess

1&) >!r does not dissolve well in nonpolar solvents because

) solute8solute interactions are much larger than solvent8solvent or solute8solvent interactions.!) solvent8solvent interactions are much larger than solute8solvent or solute8solute interactions.

C) solute8solvent interactions are much larger than solvent8solvent or solute8solute interactions.

") solute8solvent interactions are similar to solvent8solvent and solute8solute interactions.nswer#

"iff# *


3




1*) Commercial cold pac4s often contain solid 7- <* and a pouch of water. $he temperature

of the pac4 drops as the 7- <* dissolves in water. $herefore, for the dissolving of 7- <*

in water,

) = H soln is negative and =S soln may be negative or positive.

!) = H soln is negative and =%soln is positive.

C) = H soln is positive and =S soln may be negative or positive.

") = H soln is positive and =S soln is positive.

nswer# "

"iff# *


1-) When a particular solid begins to dissolve in water, the temperature rises dramatically. 5or

the dissolving of this solid in pure water

) = H soln is always negative and =S soln may be negative or positive.

!) = H soln is always negative and =S soln is always positive.

C) = H soln is always positive and =S soln may be negative or positive.") = H soln is always positive and =S soln is always positive.

nswer#

"iff# *


1) +n the process of dissolving ionic compounds, the cations and anions are separated from thecrystal lattice and surrounded by an ordered shell of solvent molecules. +f the solvent is water,

the dissolved ions are said to be

) halogenated.!) homogeni@ed.

C) hybridi@ed.") hydrated.

nswer# ""iff# 1


12) <ne reason ionic compounds do not dissolve well in nonpolar solvents is that

) ion8dipole interactions are too large for effective solvation to occur.

!) ion8solvent interactions are not strong enough to solvate the ions in solution.C) not all cations and anions have the same magnitude of charge and therefore do not form

neutral ion pairs.

") there are no forces of attraction between ions and nonpolar molecules.nswer# !

"iff# *


4




1) Which cation in each set is expected to have the larger 3more negative) hydration energy?

+ Mg&A or !a&A

++ > A or l*A

) Mg&A in set + and > A in set ++

!) Mg&A in set + and l*A in set ++

C) !a&A in set + and > A in set ++

") !a&A in set + and l*A in set ++nswer# !

"iff# *

$opic# %ection 11.& 9nergy Changes and the %olution :rocesslgo. <ption# algorithmic

16) Which cation in each set would be expected to have the larger 3more negative) hydration

energy?

+ 5e&A or 5e*A

++ BiA or 7-A) 5e&A in set + and BiA in set ++

!) 5e&A in set + and 7-A in set ++

C) 5e*A in set + and BiA in set ++

") 5e*A in set + and 7-A in set ++

nswer# C

"iff# *


1;) lthough there are exceptions, which is most likely to be true for the dissolving of a solid in

a liuid?) = H soln is positive.

!) = H soln is negative.

C) =S soln is positive.

") =S soln is negative.

nswer# C


&/) When two similar liuids mix to form a solution, the entropy of solution 3=S soln) is expected

to be) negative.

!) @ero.

C) positive.") negative at low temperatures but positive at high temperatures.

nswer# C


5




&1) When an ionic solute dissolves in water to form an unsaturated solution, the free energy

change 3=Gsoln) is

) negative.!) @ero.

C) positive.

") either or C, depending on the ionic compoundnswer# "iff# &


&&) $he change in the ibbs free energy for dissolving more solute in a supersaturated solution is

) negative.

!) @ero.C) positive.

") positive at low temperatures and negative at high temperatures.

nswer# C


&*) $he change in the ibbs free energy for dissolving solute in a saturated solution is) negative.

!) @ero.

C) positive.") positive at low temperatures and negative at high temperatures.

nswer# !


&-) 5or the process of dissolving a solid in a liuid, which of the following statements is true?) = H soln is always negative and =S soln is usually positive.

!) = H soln is always positive and =S soln is usually negative.

C) = H soln is either positive or negative and =S soln is usually positive.

") = H soln is either positive or negative and =S soln is usually negative.

nswer# C


6




&) Most gases become less soluble in water as the temperature increases. What can be

concluded about the signs of and in this case?

) = H soln is negative and =S soln is negative.

!) = H soln is negative and =S soln is positive.

C) = H soln is positive and =S soln is negative.

") = H soln is positive and =S soln is positive.

nswer#

"iff# -


&2) rrange the following compounds in order of their expected increasing solubility in water#

>Cl, C7*C7&8<8C7&C7*, C7*C7&C7&C7&8<7, C7*C7&C7&C7&C7*.

) C7*C7&C7&C7&C7* D >Cl D C7*C7&8<8C7&C7* D C7*C7&C7&C7&8<7

!) >Cl D C7*C7&8<8C7&C7* D C7*C7&C7&C7&8<7 D C7*C7&C7&C7&C7*C) C7*C7&C7&C7&C7* D C7*C7&8<8C7&C7* D >Cl D C7*C7&C7&C7&8<7

") C7*C7&C7&C7&C7* D C7*C7&8<8C7&C7* D C7*C7&C7&C7&8<7 D >Clnswer# "

"iff# &


&) Which of the following should most favor the solubility of an ionic solid in water?

) a low lattice energy for the solid and a low hydration energy for its ions!) a low lattice energy for the solid and a high hydration energy for its ions

C) a high lattice energy for the solid and a low hydration energy for its ions

") a high lattice energy for the solid and a high hydration energy for its ionsnswer# !

"iff# *$opic# %ection 11.& 9nergy Changes and the %olution :rocess

7




&6) Which should be least soluble in water?

)

!)

C)

")

nswer# "iff# &


&;) What are the maEor solute8solvent interactions created when >!r dissolves in water?) dipole8dipole

!) dispersionC) hydrogen bonding") ion8dipole

nswer# "


*/) What are the maEor solute8solvent interactions created when 7<C7&C7&<7 dissolves in

water?) dipole8dipole

!) dispersion

C) hydrogen bonding") ion8dipolenswer# C

"iff# &





*1) %ubstances with high lattice energies tend to be less soluble than substances with low lattice

energies. <n that basis predict the relative aueous solubility at &/FC, from highest to lowest, of

the following ionic compounds# Ce&3%<-)*, > &%<-, >!r, aCl.

) Ce&3%<-)* G > &%<- G >!r G aCl

!) Ce&3%<-)* G > &%<- G aCl G >!r

C) >!r G aCl G > &%<- G Ce&3%<-)*") aCl G >!r G > &%<- G Ce&3%<-)*

nswer# C

"iff# &


*&) Molarity is defined as moles of solute per

) 4ilogram of solvent.!) liter of solution.

C) mole of solvent.

") total moles present.nswer# !

"iff# 1

$opic# %ection 11.* Concentration# Hnits for %olutions

**) Molality is defined as moles of solute per

) 4ilogram of solvent.

!) liter of solution.C) mole of solvent.

") total moles present.

nswer# "iff# &


*-) Which concentration becomes smaller as the temperature is increased from &/FC to 6/FC?

) mass 0

!) molality

C) molarity") mole fraction

nswer# C

"iff# &$opic# %ection 11.* Concentration# Hnits for %olutions

!




*) What is the mole fraction of ethanol in a solution made by dissolving 1-.2 g of ethanol,

C&7<7, in *.2 g of water?

) /./;2-!) /.1/2

C) /.&1-

") /.&&nswer# "iff# &


lgo. <ption# algorithmic

*2) What is the molality of ethanol in a solution made by dissolving 1-.2 g of ethanol, C&7<7,

in *.2 g of water?) /.//;1 m

!) /.&& m

C) .;1 m

") && mnswer# C

"iff# &


*) What is the mole fraction of +& in a solution made by dissolving &.6 g of +& in &- g of

hexane, C271-?

) /./*1!) /./*6

C) /./1

") /.//

nswer# "iff# &



*6) What is the mole fraction of oxygen in a gas mixture that is &&0 oxygen and 60 nitrogen

by volume?) /.&/

!) /.&&

C) /.&

") /.&6

nswer# !"iff# *

$opic# %ection 11.* Concentration# Hnits for %olutionslgo. <ption# algorithmic

10




*;) solution is prepared by dissolving 1. g sulfuric acid, 7&%<-, in enough water to ma4e

1//./ mB of solution. +f the density of the solution is 1.1/;- g(mB, what is the mole fraction

7&%<- in the solution?

) /./161!) /./**6

C) /./*/") 1;./nswer# !

"iff# -


-/) solution is prepared by dissolving 1. g sulfuric acid, 7&%<-, in enough water to ma4e

1//./ mB of solution. +f the density of the solution is 1.1/;- g(mB, what is the molarity?

) /.1 M 7&%<-

!) /.161/ M 7&%<-C) 1.61/ M 7&%<-") 1.;-/ M 7&%<-nswer# C

"iff# &


-1) solution is prepared by dissolving 1. g sulfuric acid, 7&%<-, in enough water to ma4e

1//./ mB of solution. +f the density of the solution is 1.1/;- g(mB, what is the molality?

) /.1 m 7&%<-

!) /.161/ m 7&%<-C) 1.61/ m 7&%<-

") 1.;-/ m 7&%<-nswer# "

"iff# *


-&) solution is prepared by dissolving 1. g sulfuric acid, 7&%<-, in enough water to ma4e

exactly 1//./ mB of solution. +f the density of the solution is 1.1/;- g(mB, what is the mass 0

7&%<- in the solution?

) 12.//0!) 16.//0

C) 1;.//0") 6-.//0nswer#

"iff# *


11




-*) solution is prepared by dissolving 11 g of CdCl& in enough water to ma4e &/./ mB of

solution. +f the density of the solution is 1.2 g(mB, what is the molarity of the solution?

) /.--/ M!) /.26- M

C) /.;** M

") *.* Mnswer# ""iff# &


--) solution is prepared by dissolving 11 g of CdCl& in enough water to ma4e exactly &/./

mB of solution. +f the density of the solution is 1.2 g(mB, what is the mass percent of CdCl& in

the solution?

) .10!) --./0

C) 2./0

") 26.-0nswer# !

"iff# *


-) What is the mass percent of vitamin C in a solution made by dissolving 1.*/ g of vitamin C,

C276<2, in ./ g of water?

) /.1;0!) /.&-&0

C) &.*10

") &.*20

nswer# C"iff# &



-2) What is the mass percent of a caffeine solution made by dissolving -.* g of caffeine,

C671/ -<&, in g of ben@ene, C272?

) /./0!) /./60

C) .0

") .60

nswer# C"iff# &



12




-) What volume of /.12 M >!r solution is needed to provide 1/. g of >!r?

) .& mB

!) 1-. mBC) 2*.& mB

") 1&* mB

nswer# ""iff# &



-6) What volume of *.// M C7*<7 solution is needed to provide /.&/ mol of C7*<7?

) 1.&* mB

!) 11.1 mBC) ;/./ mB

") 61/ mB

nswer# C



-;) 7ow much water must be added to -&./ g of CaCl& to produce a solution that is *./ mass 0

CaCl&?

) 2. g

!) 6./ gC) 6*.* g

") 1&/ g

nswer# !



/) $o ma4e a &./ M solution, one could ta4e &.// moles of solute and add

) 1.// B of solvent.

!) 1.// 4g of solvent.C) enough solvent to ma4e 1.// B of solution.

") enough solvent to ma4e 1.// 4g of solution.

nswer# C"iff# 1


13




1) $o ma4e a &.// m solution, one could ta4e &.// moles of solute and add




nswer# !"iff# &



&) What molality of pentane is obtained by dissolving ./ g pentane, C71&, in &-./ g hexane,

C271-?

) /./&/ m

!) /./&- mC) /.&6 m

") &/. m

nswer# C"iff# &



*) solution is &.&0 by mass a7C<*. 7ow many grams of a7C<* are in -/./ g of

solution?

) /.// g

!) 1/.1 gC) &// g

") && g

nswer# !"iff# &



-) 7ow many grams of >!r are reuired to ma4e 2/. mB of a /.11 M >!r solution?

) /.2&6 g!) .2 g

C) 6.;/ g

") -.6 gnswer# C

"iff# &$opic# %ection 11.* Concentration# Hnits for %olutionslgo. <ption# algorithmic

14




) What is the molality of a glucose solution prepared by dissolving 16./ g of glucose,

C271&<2, in 1&.; g of water?

) .;- I 1/8- m

!) /.1-* mC) /.2; m

") /.;- mnswer# ""iff# &



2) ueous solutions of */0 3by mass) hydrogen peroxide, 7&<&, are used to oxidi@e metals or

organic molecules in chemical reactions. iven that the density of the solution is 1.11 g(mB,

calculate the molarity.

) /.;- M!) 2.6 M

C) ;.; M") 1&.2 Mnswer# C

"iff# *


) ueous solutions of */./0 3by mass) hydrogen peroxide, 7&<&, are used to oxidi@e metals

or organic molecules in chemical reactions. Calculate the molality of this solution.

) /.;- m!) 2.6 m

C) ;.; m

") 1&.2 mnswer# ""iff# *


6) %odium hydroxide is available commercially as a /./0 by weight aueous solution. $he

density of the solution is 1.* g(mB. Calculate the molarity of this sodium hydroxide solution.

) /.-/ M!) 1;.1 M

C) &./ M

") 1&. M

nswer# !"iff# *


15




;) %odium hydroxide is available commercially as a /./0 by weight aueous solution.

Calculate the molality of this sodium hydroxide solution.

) /.-/ m!) 1;.1 m

C) &./ m

") 1&. mnswer# C

"iff# *


2/) 1.*/ M solution of CaCl& in water has a density of 1.11 g(mB. What is the molality?

) 1.1 m CaCl&

!) 1.& m CaCl&

C) 1.* m CaCl&

") 1.-- m CaCl&

nswer# C"iff# -


21) *.1 m solution of CaCl& in water has a density of 1.&- g(mB. What is the molarity?

) &.2 M CaCl&!) &.;1 M CaCl&

C) *./ M CaCl&

") *.;* M CaCl&

nswer# !

"iff# -


2&) &.// M solution of CaCl& in water has a density of 1.1 g(mB. What is the mole fraction of

CaCl&?

) /./*-6!) /./*2/

C) /./*22

") /./*6/nswer# C

"iff# -


16




2*) solution of BiCl in water has JBiCl K /.///. What is the molality?

) &.2/ m BiCl

!) &. m BiClC) &.;& m BiCl

") .&2 m BiCl

nswer# C"iff# -$opic# %ection 11.* Concentration# Hnits for %olutions


2-) solution of BiCl in water is 16./ mass 0 BiCl. What is the mole fraction of BiCl?

) /./6*!) /./;**

C) /.-&

") -.2

nswer#

"iff# *$opic# %ection 11.* Concentration# Hnits for %olutions


2) t &./FC, a solution has a concentration of *.1; M and a density of 1.&2/ g(mB. $he

density of the solution at /./FC is 1.&-; g(mB. What is the molarity of the solution at /./FC?) &.- M

!) *.11 M

C) *.1; M

") *.&*/ Mnswer# !


22) saturated solution is defined as

) a concentrated solution.!) a solution that is in euilibrium with pure solvent.

C) a solution than is in euilibrium with undissolved solute.

") a solution that is in euilibrium with both pure solvent and undissolved solute.nswer# C

"iff# 1

$opic# %ection 11.- %ome 5actors $hat ffect %olubility

2) Which of the following does not affect the solubility of a solute in a given solvent?

) polarity of the solute

!) polarity of the solventC) rate of stirring

") temperature of the solvent and solute

nswer# C"iff# 1


17




26) Which of the following statements is true for a supersaturated solution?

) $he solute in the solution is at euilibrium with undissolved solute.!) $he solution contains more than the euilibrium amount of solute.

C) $he solution is stable and the solute will not precipitate.

") supersaturated solution is more than /0 solute by mass.nswer# !

"iff# 1


2;) +n general, as the temperature increases, the solubility of gases in water '''''''' and the

solubility of most solids in water ''''''''.) decreases, decreases

!) decreases, increases

C) increases, decreases") increases, increases

nswer# !

"iff# 1$opic# %ection 11.- %ome 5actors $hat ffect %olubility

/) $he solubility of gaseous solutes in liuid solvents is greater when the

) external pressure over the solution is increased.!) external pressure is decreased.

C) partial pressure of the gas above the solution is increased.

") partial pressure of the solvent is increased.nswer# C

"iff# 1


1) +n which case should C<&3 g ) be more soluble in water?

) $he total pressure is atm and the partial pressure of C<& is 1 atm.

!) $he total pressure is * atm and the partial pressure of C<& is & atm.

C) $he total pressure is 1 atm and the partial pressure of C<& is /./* atm.

") $he total pressure is 1 atm and the partial pressure of C<& is /. atm.

nswer# !"iff# 1



1




&) $he 7enryLs Baw constant of methyl bromide, C7*!r, is k K /.1; mol(3B atm) at &FC.

What is the solubility of methyl bromide in water at &FC and at a partial pressure of &/. mm

7g?) /./&* mol(B

!) /.*&; mol(B

C) /.-6* mol(B") *;.6 mol(Bnswer#

"iff# &

$opic# %ection 11.- %ome 5actors $hat ffect %olubilitylgo. <ption# algorithmic

*) $he solubility of argon in water at &FC is /./1/ mol(B. What is the 7enryLs Baw constantfor argon if the partial pressure of argon in air is /.//;*- atm?

) 1.-/ I 1/8- mol(3B atm)

!) /.2&* mol(3B atm)

C) 1.21 mol(3B atm)") -.1/ mol(3B atm)

nswer# C

"iff# &


-) Which of the following is not an application of colligative properties?) adding silver to mercury to lower the vapor pressure of mercury

!) desalinating sea water by reverse osmosis

C) melting snow by application of salt") reduced boiling points of pure liuids at increased altitudes

nswer# ""iff# 1

$opic# %ection 11. :hysical !ehavior of %olutions# Colligative :roperties

) solution is prepared by dissolving -/./ g of sucrose, C1&7&&<11, in &/. g of water at

&FC. What is the vapor pressure of the solution if the vapor pressure of water at &FC is &*.2

mm 7g?) /.1;6 mm 7g

!) &/. mm 7g

C) &*.2 mm 7g") &-./ mm 7g

nswer# C"iff# *$opic# %ection 11.2 Napor8:ressure Bowering of %olutions# OaoultLs Baw


1!




2) >Cl solution is prepared by dissolving -/./ g >Cl in &/./ g of water at &FC. What is the

vapor pressure of the solution if the vapor pressure of water at &FC is &*.2 mm 7g?

) &/. mm 7g!) &&.1 mm 7g

C) &&.; mm 7g

") &. mm 7gnswer# C

"iff# *

$opic# %ection 11.2 Napor8:ressure Bowering of %olutions# OaoultLs Bawlgo. <ption# algorithmic

) t a given temperature the vapor pressures of ben@ene and toluene are 16* mm 7g and ;.&

mm 7g, respectively. Calculate the total vapor pressure over a solution of ben@ene and toluenewith J ben@ene K /.2//.

) 11/ mm 7g

!) 1&1 mm 7g

C) 1** mm 7g") &-& mm 7g

nswer# C

"iff# *$opic# %ection 11.2 Napor8:ressure Bowering of %olutions# OaoultLs Baw


6) t a given temperature the vapor pressures of ben@ene and toluene are 16* mm 7g and ;.&

mm 7g, respectively. Calculate the mole fraction of ben@ene in the vapor phase over a solution

of ben@ene and toluene with J ben@ene K /.2//.

) /.2//

!) /.26C) /.2

") /.6&*nswer# "

"iff# -

$opic# %ection 11.2 Napor8:ressure Bowering of %olutions# OaoultLs Baw

;) 7ow many grams of sucrose, C1&7&&<11, must be added to //. g of water at 1//FC to

change the vapor pressure to & mm 7g?

) /.&; g!) .*& g

C) 1/.2 g") 1/1 gnswer# "

"iff# *


20




6/) +f one mole of each is dissolved in 1.// B of water, which will lower the vapor pressure the

most?

) C1&7&&<11!) a<*C) C*7<7

") MgCl&nswer# "

"iff# &


61) When &.*2 g of a nonvolatile solute is dissolved in 1// g of solvent, the largest change in

free@ing point will be achieved when the solvent is) ben@ene, K f K ./.

!) camphor, K f K *.6.

C) chloroform, K f K -./.

") ll are expected to have the same free@ing point.nswer# !

"iff# &$opic# %ection 11. !oiling8:oint 9levation and 5ree@ing8:oint "epression of %olutions

6&) /./ m solution of which solute has the largest vanLt 7off factor?) CaCl&

!) > *:<-

C) BiC<*

") a<*

nswer# !


6*) /./&/ m aueous solution containing which solute will have the lowest free@ing point?

) BiCl

!) aCl

C) >Cl") ll will have approximately the same free@ing point.

nswer# "

"iff# 1$opic# %ection 11. !oiling8:oint 9levation and 5ree@ing8:oint "epression of %olutions

21




6-) Which of the following solutions will have the lowest free@ing point?

) /./1// m aCl

!) /./1// m Bi&%<-C) /./* m C7*C7&C7&<7

") /./1 m MgCl&

nswer# ""iff# &

$opic# %ection 11. !oiling8:oint 9levation and 5ree@ing8:oint "epression of %olutionslgo. <ption# algorithmic

6) Which of the following pairs of solutions have roughly the same boiling point elevation?) /.1// m C271&<2 and /./*** m CuCl&!) /.1// m aCl and /.1// m C271&<2C) /.&// m aCl and /.*// m a&%<-") /.1// m >Cl and /./// m Mg!r &

nswer# "iff# &

$opic# %ection 11. !oiling8:oint 9levation and 5ree@ing8:oint "epression of %olutions

62) What is the expected free@ing point of a /./ m solution of a&%<- in water? K f for water is

1.62FC(m.) 8/.;*FC

!) 81.;FC

C) 8&.6FC

") 82.FCnswer# C

"iff# &$opic# %ection 11. !oiling8:oint 9levation and 5ree@ing8:oint "epression of %olutionslgo. <ption# algorithmic

6) Calculate the free@ing point of a solution of &/./ g methyl salicylate, C72<&, dissolved in

6//. g of ben@ene, C272. K f for ben@ene is and the free@ing point is ./FC for ben@ene.

) 81./FC!) 1./FC

C) -.-FC

") 2.-FCnswer# C

"iff# *$opic# %ection 11. !oiling8:oint 9levation and 5ree@ing8:oint "epression of %olutionslgo. <ption# algorithmic

22




66) What is the free@ing point of a solution of 1.-* g MgCl& in 1// g of water? K f for water is

1.62FC(m for water.

) 8/./&;FC!) 8/.&;FC

C) 8/.;FC

") 8/.6*6FCnswer# ""iff# *



6;) $he normal boiling point of pure ben@ene is found to be 6/.1/FC. What is the approximate

molecular weight of a nonioni@ing substance if a solution of *. g of the substance dissolved in

1//. g of ben@ene has a normal boiling point of for ben@ene, C272.

) &/ amu

!) // amu

C) &/// amu") &/,/// amu

nswer# C"iff# *


;/) n aueous solution has a normal boiling point of 1/&./FC. What is the free@ing point of this

solution? 5or water K b is and

) 8/.FC

!) 8&./FCC) 8*.2FC

") 8.*FCnswer# ""iff# *



;1) solution of /.&11* g of water dissolved in &./ g of a solvent free@es at 11.FC below the

free@ing point of the solvent. What is K f for this solvent?

) /.*FC(m

!) 1.*2FC(mC) .*;FC(m

") &-.FC(mnswer# ""iff# *


23




;&) /.1 m aueous solution of an un4nown solute has a boiling point elevation of /.2&FC. $he

boiling point elevation of a /.1 m solution of a nonioni@ing molecular solute in water is /.&2FC.

7ow many moles of particles are formed per mole of solute when the un4nown solute isdissolved in water?

) 1.-

!) &./C) &.-

") *./

nswer# C"iff# *


;*) n aueous CsCl solution is 6.// mass 0 CsCl and has a density of 1./2-* g(mB at &/FC.What is the boiling point of this solution? K b K /.1FC(m for water.

) 1//.&FC

!) 1//.*FC

C) 1/*.6FC") 1/-.*FC

nswer# !

"iff# $opic# %ection 11. !oiling8:oint 9levation and 5ree@ing8:oint "epression of %olutions

;-) Chloroform has a boiling point of 21.1FC and dichloromethane has a boiling point of -/./FC.When /.1// mol of dichloromethane is added to /.;// mol of chloroform, the resulting solution

will have a boiling point

) between -/./FC and 21.1FC, but closer to 21.1FC.!) between -/./FC and 21.1FC, but closer to -/./FC.

C) greater than 21.1FC.") less than -/./FC.

nswer# "iff# *


;) $wo aueous solutions, and !, are separated by a semipermeable membrane. $he osmotic

pressure of solution immediately begins to decrease. Which of the following statements is

true?) %olvent molecules are moving from solution ! into solution .

!) $he initial osmotic pressure of solution ! is greater than that of solution .

C) $he solvent molecules are moving from the solution of higher osmotic pressure to that oflower osmotic pressure.") !oth ! and C are true statements.

nswer#

"iff# *$opic# %ection 11.6 <smosis and <smotic :ressure

24




;2) Oed blood cells are placed into pure water. Which of the following statements is true?

) Water molecules flow out of the red blood cells, causing them to collapse.

!) Water flows into the red blood cells, causing them to swell and burst.C) $he osmotic pressure of the cell contents increases, causing the cells to burst.

") $he osmotic pressure inside the cells euals the osmotic pressure outside.

nswer# !"iff# *

$opic# %ection 11.6 <smosis and <smotic :ressure

;) 7ow will the osmotic pressure of an aueous solution change as evaporation occurs?

) $he osmotic pressure will increase.

!) $he osmotic pressure will not change.

C) $he osmotic pressure will decrease.") $he osmotic pressure will increase or decrease until it euals the vapor pressure of water.

nswer#

"iff# &

$opic# %ection 11.6 <smosis and <smotic :ressure

;6) ssuming that sea water is a *. mass 0 solution of aCl in water, calculate its osmotic pressure at &/FC. $he density of a *.0 aCl solution at &/FC is 1./&* g(mB.

) 1./ atm

!) 1 atmC) &; atm

") 1// atm

nswer# C

"iff# -$opic# %ection 11.6 <smosis and <smotic :ressure

;;) solution is made by dissolving 1* g of sucrose, C1&7&&<11, in 11 g of water, producing

a solution with a volume of 1& mB at &/FC. What is the expected osmotic pressure at &/FC?) .* atm

!) 1/ atm

C) 1- atm") 6 atm

nswer#


1//) $he average osmotic pressure of blood is about atm. $herefore) the average blood pressure is about atm.!) the average pressure inside the body is about atm above the external pressure.

C) a pressure of about atm would be reuired to prevent osmosis if blood is in contact with

pure water across a semipermeable membrane.") ll of the above are true.

nswer# C


25




1/1) When /.// g of vitamin > is dissolved in 1/./ g of camphor 3> f K -/./FC(m), the free@ing

point of the solution is -.-*FC lower than that of pure camphor. ssuming vitamin > is a

nonelectrolyte in camphor, calculate its molar mass.) /.-1 g(mol

!) .- g(mol

C) -1 g(mol") *.- I 1/- g(molnswer# C

"iff# -


1/&) When ethylene glycol, 7<C7&C7&<7, is added to the water in an automobile radiator, the

effect is to

) lower the boiling point and lower the free@ing point.

!) lower the boiling point and raise the free@ing point.C) raise the boiling point and lower the free@ing point.

") raise the boiling point and raise the free@ing point.nswer# C"iff# &


1/*) $he coolant in automobiles is often a /(/ 0 by volume mixture of ethylene glycol,

7<C7&C7&<7, and water. t &/FC, the density of ethylene glycol is 1.1/66 g(mB and the

density of water is /.;;6& g(mB. ssuming that the volumes are additive, what is the expected

free@ing point of a /(/3v(v)0 ethylene glycol(water solution? K f K 1.62FC(m for water.

) 812FC!) 81FC

C) 8*/FC

") 8**FCnswer# "

"iff# -


1/-) aproxen is a commercially important anti8inflammatory agent that can be isolated from

the thyroid gland. solution of 1.1*6 g of naproxen in &.// g ben@ene has an osmotic pressure

of -.// atm at &/FC. $he density of ben@ene is /.66 g(mB at this temperature. Calculate themolar mass of naproxen, assuming it remains intact upon dissolution and the density of the

solution euals the density of pure ben@ene.

) 12 g(mol!) &*/ g(mol

C) */ g(mol

") *.6/ I 1/ g(mol

nswer# !"iff# -

$opic# %ection 11.; %ome Hses of Colligative :roperties

26




1/) solution of 2&.- g of insulin in enough water to ma4e 1./// B of solution has an osmotic

pressure of /.*/ atm at &FC. !ased on these data, what is the molar mass of insulin?

) 2&1 g(mol!) /// g(mol

C) / g(mol

") 1,;// g(molnswer# !

"iff# -

$opic# %ection 11.; %ome Hses of Colligative :roperties

1/2) Which drawing above represents the system with the highest entropy?

) drawing 3a)!) drawing 3b)

C) drawing 3c)

") drawing 3d)

nswer# C"iff# &


1/) Which drawing above represents the system with the lowest entropy?

) drawing 3a)!) drawing 3b)C) drawing 3c)

") drawing 3d)

nswer# "iff# &


1/6) Which drawing above represents the system with the second lowest entropy?) drawing 3a)

!) drawing 3b)

C) drawing 3c)") drawing 3d)

nswer# "


27




1/;) Which drawing above represents the system with the second highest entropy?

) drawing 3a)

!) drawing 3b)C) drawing 3c)

") drawing 3d)

nswer# !"iff# &


rrows in the energy diagram below represent enthalpy changes occurring in the exothermic

formation of a solution#

= H soln K enthalpy of solution

= H solute8solute K enthalpy change involving solute8solute interactions

= H solute8solvent K enthalpy change involving solute8solvent interactions

= H solvent8solvent K enthalpy change involving solvent8solvent interactions

11/) Which arrow represents = H soln?

) arrow 3a)

!) arrow 3b)C) arrow 3c)

") arrow 3d)

nswer# ""iff# &


111) Which arrow represents = H solute8solvent?

) arrow 3a)

!) arrow 3b)

C) arrow 3c)") arrow 3d)

nswer# C

"iff# &


2




11&) Which arrows represent = H solute8solute and = H solvent8solvent?

) arrow 3a) and arrow 3b)

!) arrow 3a) and arrow 3c)C) arrow 3a) and arrow 3d)

") arrow 3c) and arrow 3d)

nswer# "iff# &$opic# %ection 11.& 9nergy Changes and the %olution :rocess

rrows in the energy diagram below represent enthalpy changes occurring in the endothermicformation of a solution#

= H soln K enthalpy of solution

= H solute8solute K enthalpy change involving solute8solute interactions

= H solute8solvent K enthalpy change involving solute8solvent interactions

= H solvent8solvent K enthalpy change involving solvent8solvent interactions

11*) Which arrow represents = H soln?

) arrow 3a)

!) arrow 3b)C) arrow 3c)

") arrow 3d)

nswer# ""iff# &


11-) Which arrow represents = H solute8solvent?

) arrow 3a)

!) arrow 3b)

C) arrow 3c)") arrow 3d)

nswer# C


2!




11) Which arrows represent = H solute8solute and = H solvent8solvent?

) arrow 3a) and arrow 3b)

!) arrow 3a) and arrow 3c)C) arrow 3a) and arrow 3d)

") arrow 3c) and arrow 3d)

nswer# "iff# &$opic# %ection 11.& 9nergy Changes and the %olution :rocess

112) Which ion8dipole interaction results in the larger 3more negative) hydration energy?

) diagram 3a)!) diagram 3b)

C) diagram 3c)") diagram 3d)nswer#

"iff# *


30




11) Which ion8dipole interaction results in the larger 3more negative) hydration energy?

) diagram 3a)!) diagram 3b)

C) diagram 3c)

") diagram 3d)nswer# C

"iff# *


116) "rawing 31) shows a system in which an euilibrium exists between dissolved and

undissolved gas particles at : K 1 atm. ccording to 7enryLs law, if the pressure is increased to &

atm and euilibrium is restored, which drawing 3&)83) best represents the euilibrium at & atm?

) drawing 3&)

!) drawing 3*)C) drawing 3-)

") drawing 3)

nswer# ""iff# &

$opic# Conceptual :roblems

31




11;) "rawing 31) shows a system in which an euilibrium exists between dissolved and

undissolved gas particles at : K 1 atm. ccording to 7enryLs law, if the pressure is decreased to

/. atm and euilibrium is restored, which drawing 3&)83) best represents the euilibrium at /.atm?

) drawing 3&)!) drawing 3*)C) drawing 3-)

") drawing 3)

nswer# C"iff# &


32




1&/) "rawing 31) shows the euilibrium vapor pressure of a pure liuid. Which drawing 3&)83)

represents the euilibrium vapor pressure when a nonvolatile solute is dissolved in the liuid?

) drawing 3&)

!) drawing 3*)

C) drawing 3-)") drawing 3)

nswer# !

"iff# &$opic# Conceptual :roblems

33




1&1) "rawings 31) and 3&) show the euilibrium vapor pressures of two pure liuids. Which

drawing 3*)832) represents the euilibrium vapor pressure of a solution made by mixing eual

moles of each liuid?

) drawing 3*)

!) drawing 3-)

C) drawing 3)") drawing 32)

nswer# C

"iff# &


34




$he following diagram shows a close8up view of the vapor pressure curves for a pure solvent and

a solution containing a nonvolatile solute dissolved in this solvent.

1&&) Which curve is the solvent and what happens to the vapor pressure when the solute is

dissolved in the solvent?

) Curve 3a) is the solvent and the vapor pressure decreases.!) Curve 3a) is the solvent and the vapor pressure increases.

C) Curve 3b) is the solvent and the vapor pressure decreases.") Curve 3b) is the solvent and the vapor pressure increases.

nswer# "iff# &


1&*) Which curve is the solvent and what happens to the boiling point when the solute is

dissolved in the solvent?) Curve 3a) is the solvent and the boiling point decreases.

!) Curve 3a) is the solvent and the boiling point increases.

C) Curve 3b) is the solvent and the boiling point decreases.

") Curve 3b) is the solvent and the boiling point increases.nswer# !

"iff# &


35




1&-) $he following diagram shows a close8up view of the vapor pressure curves for two pure

liuids and two different solutions composed of these two liuids. Which curves represent pure

liuids and which curves represent the solutions?

) Curves 3a) and 3b) are the pure liuids and curves 3c) and 3d) are the solutions.!) Curves 3a) and 3c) are the pure liuids and curves 3b) and 3d) are the solutions.

C) Curves 3a) and 3d) are the pure liuids and curves 3b) and 3c) are the solutions.

") Curves 3c) and 3d) are the pure liuids and curves 3a) and 3b) are the solutions.nswer# C

"iff# &


36




1&) "rawing 31) shows a noneuilibrium system comprised of pure water separated from an

aueous solution by a semipermeable membrane. %haded spheres represent solute particles and

unshaded spheres represent water molecules. Which drawing 3&)83) represents this system aftereuilibrium is reached?

) drawing 3&)

!) drawing 3*)

C) drawing 3-)") drawing 3)

nswer#


37




1&2) $wo bea4ers, one with pure water 3light gray) and the other with an aueous solution of

>!r 3dar4 gray), are placed in a closed container represented by drawing 3a). Which of the

drawings 3a)83d) represents what the bea4ers will loo4 li4e after a substantial amount of time has passed?

) drawing 3a)!) drawing 3b)

C) drawing 3c)

") drawing 3d)nswer# !

"iff# *


3




phase diagram of temperature versus composition for a mixture of the two volatile liuids

octane 3bp K and decane 3bp K 1&2FC) is shown.

1&) ssume that you start with a mixture containing /.6/ mol of decane and /.&/ mol of octane,

what region of the diagram corresponds to liuid?) region a

!) region b

C) region c

") regions a and cnswer# C

"iff# &


1&6) ssume that you start with a mixture containing /.6/ mol of decane and /.&/ mol of octane,what region of the diagram corresponds to vapor?

) region a

!) region b

C) region c") regions a and c

nswer#


3!




phase diagram of temperature versus composition for a mixture of the two volatile liuids

octane 3bp K and decane 3bp K 1&2FC) is shown.

1&;) ssume that you start with a mixture containing /.6/ mol of decane and /.&/ mol of octane,

at what approximate temperature will the mixture begin to boil?) temperature at point a

!) temperature at point bC) temperature at point d") temperature at point f

nswer# !


1*/) ssume that you start with a mixture containing /.6/ mol of decane and /.&/ mol of octane,

what is the liuid composition at the boiling point?) 1//0 decane

!) composition at point b

C) composition at point c") composition at point e

nswer# !


1*1) ssume that you start with a mixture containing /.6/ mol of decane and /.&/ mol of octane,what is the vapor composition at the boiling point?

) 1//0 decane

!) composition at point bC) composition at point c

") composition at point enswer# C"iff# &


40




1*&) ssume that the vapor at point c is condensed and reboiled. What is the liuid composition

of the condensed vapor prior to reboiling?

) 1//0 decane!) composition at point b

C) composition at point d

") composition at point enswer# C

"iff# &


1**) ssume that the vapor at point c is condensed and reboiled. What is the vapor composition

during reboiling?

) 1//0 decane!) composition at point b

C) composition at point c

") composition at point e

nswer# ""iff# &


1*-) ssume that the vapor at point c is condensed and reboiled. What is the boiling point?

) temperature at point b!) temperature at point c

C) temperature at point d

") temperature at point f

nswer# C"iff# &


41




1*) What is the approximate boiling temperature of a mixture that is /./ J

and /.*/ J!

?

) /FC!) FC

C) ;FC

") 1//FC

nswer# !"iff# &


1*2) What is the approximate vapor composition above a boiling solution that is /./ J and

/.*/ J! ?

) /./ J, /.*/ J!!) /./ J, /./ J!

C) /.*/ J, /./ J!

") / J, 1.// J!

nswer# C"iff# &


1*) What is the approximate boiling temperature of the liuid formed from the condensation ofthe vapor above a boiling solution that is /./ J and /.*/ J!?

) /FC!) FC

C) ;/FC") 1//FC

nswer# !


42




1*6) t 6/FC, pure liuid has a vapor pressure of // mm 7g and pure liuid ! has a vapor

pressure of ;-/ mm 7g. What is J for a solution of and ! with a normal boiling point of

) /.&

!) /./

C) /.") solution of and ! cannot boil at 6/FC.nswer# C

"iff# &


11.& lgorithmic Questions

1) Which cation in each set is expected to have the larger 3more negative) hydration energy?

+ !e&A or Ca&A

++ ObA or Pn&A

) !e&A in set + and ObA in set ++

!) !e&A in set + and Pn&A in set ++

C) Ca&A in set + and ObA in set ++

") Ca&A in set + and Pn&A in set ++

nswer# !"iff# *



&) What is the mole fraction of ethanol in a solution made by dissolving &;.& g of ethanol,

C&7<7, in *.2 g of water?) /.12!) /.&1*

C) /.*&

") /.-nswer#

"iff# &



43




*) What is the mole fraction of +& in a solution made by dissolving .2 g of +& in &- g of

hexane, C271-?

) /./1

!) /.//C) /.1**

") /.1-nswer# "iff# &



-) What is the mole fraction of oxygen in a gas mixture that is *0 oxygen and 2*0 nitrogen by

volume?) /.*-

!) /.*

C) /.&

") /.&nswer# !

"iff# *


) What is the mass percent of vitamin C in a solution made by dissolving 2./ g of vitamin C,C276<2, in ./ g of water?

) /.-0

!) 1.&10

C) 1/.20

") 11.60nswer# C



2) What is the weight percent of a caffeine solution made by dissolving 6.* g of caffeine,C671/ -<&, in g of ben@ene, C272?

) /./1/0

!) /./110

C) 1/0

") 110nswer# C



44




) What volume of a /.12 M >!r solution is needed to provide */. g of >!r?

) &1.6 mB

!) -&. mBC) 16- mB

") * mB

nswer# ""iff# &



6) What volume of *.// M C7*<7 solution is needed to provide /.&&/ mol of C7*<7?

) 1.& mB

!) 1*.2 mBC) *.* mB

") 22/ mB

nswer# C



;) 7ow much water must be added to -/./ g of CaCl& to produce a solution that is *./ mass 0

CaCl&?

) -./ g

!) -.& gC) 6. g

") 11- g

nswer# !



1/) $o ma4e a /.// M solution, one could ta4e /.// moles of solute and add




nswer# C"iff# 1


45




11) $o ma4e a &.// m solution, one could ta4e &.// moles of solute and add




nswer# !"iff# &



1&) What molality of pentane is obtained by dissolving 1 g pentane, C71&, in &-./ g hexane,

C271-?

) /./6 m

!) /./26 mC) /.6 m

") 21 m

nswer# C"iff# &



1*) solution is &.&0 by mass a7C<*. 7ow many grams of a7C<* are in 1/./ g of

solution?

) 1./ g

!) *.*6 gC) 22. g

") && g

nswer# !"iff# &



1-) 7ow many grams of >!r are reuired to ma4e */. mB of a /.11 M >!r solution?

) /.**6 g!) *./- g

C) -.; g

") -/.* gnswer# C

"iff# &$opic# %ection 11.* Concentration# Hnits for %olutionslgo. <ption# algorithmic

46




1) What is the molality of a glucose solution prepared by dissolving 16./ g of glucose,

C271&<2, in 1&.; g of water?

) .;- I 1/8- m

!) /.1-* mC) /.2; m

") /.;- mnswer# ""iff# &



12) solution of BiCl in water has JBiCl K /./;//. What is the molality?

) -.-2 m BiCl

!) .// m BiCl

C) .-; m BiCl") ;.6; m BiCl

nswer# C"iff# -$opic# %ection 11.* Concentration# Hnits for %olutions


1) solution of BiCl in water is &/./ mass 0 BiCl. What is the mole fraction of BiCl?

) /./;2/

!) /.1/2

C) /.-&") -.--

nswer#



16) +n which case should C<&3 g ) be more soluble in water?

) $he total pressure is atm and the partial pressure of C<& is /. atm.

!) $he total pressure is * atm and the partial pressure of C<& is 1 atm.

C) $he total pressure is 1 atm and the partial pressure of C<& is /./* atm.

") $he total pressure is 1 atm and the partial pressure of C<& is /.- atm.

nswer# !

"iff# *$opic# %ection 11.- %ome 5actors $hat ffect %olubility


47




1;) $he 7enryLs Baw constant of methyl bromide, C7*!r, is k K /.1; mol(3B atm) at &FC.

What is the solubility of methyl bromide in water at &FC and at a partial pressure of &/. mm

7g?) /./2 mol(B

!) /.* mol(B

C) /.--6 mol(B") -&.; mol(Bnswer#

"iff# &

$opic# %ection 11.- %ome 5actors $hat ffect %olubilitylgo. <ption# algorithmic

&/) solution is prepared by dissolving -/./ g of sucrose, C1&7&&<11, in &/. g of water at

&FC. What is the vapor pressure of the solution if the vapor pressure of water at &FC is &*.2mm 7g?

) /.1;6 mm 7g

!) &/. mm 7gC) &*.2 mm 7g

") &-./ mm 7g

nswer# C



&1) >Cl solution is prepared by dissolving &./ g >Cl in &/./ g of water at &FC. What is the

vapor pressure of the solution if the vapor pressure of water at &FC is &*.2 mm 7g?

) &1.2 mm 7g

!) &&. mm 7gC) &*.& mm 7g

") &-.; mm 7gnswer# !

"iff# *



&&) t a given temperature the vapor pressures of ben@ene and toluene are 16* mm 7g and ;.&

mm 7g, respectively. Calculate the total vapor pressure over a solution of ben@ene and toluenewith J ben@ene K /.6/.

) 1/2 mm 7g!) 1&1 mm 7g

C) 1*1 mm 7g") &-& mm 7g

nswer# C



4




&*) Which of the following solutions will have the lowest free@ing point?

) /./1/ m > !r

!) /./1/ m a&C<*C) /./* m C7*C7&<7 ") /./1 m !aCl&

nswer# ""iff# *


&-) What is the expected free@ing point of a /./ m solution of Bi&%<- in water? > f for water is

1.62FC(m.) 8/.;*FC

!) 81.;FC

C) 8&.6FC") 82.FC

nswer# C"iff# *


&) Calculate the free@ing point of a solution of -/./ g methyl salicylate, C72<&, dissolved in

6//. g of ben@ene, C272. and the free@ing point is ./FC for ben@ene.

) 8&./;FC

!) &./;FC

C) *.-1FC

") .;FCnswer# C

"iff# *


&2) What is the free@ing point of a solution of .1 g MgCl& in 1// g of water? K f for water is

) 8/.1-/FC

!) 81.-/FC

C) 8&.6/FC

") 8-.16FCnswer# "

"iff# *


4!




&) n aueous solution has a normal boiling point of 1/*./FC. What is the free@ing point of this

solution? 5or water and

) 8/.6&FC!) 8*./FC

C) 8*.2FC

") 811FCnswer# "

"iff# -


&6) solution of fructose, , exerts an osmotic pressure of 6./ torr at &F C. What is the

molarity of the fructose solution?

) /.//-1; M!) *.1; M

C) -.&1 M

") /.///; Mnswer#

"iff# *

$opic# %ection 11.6 <smosis and <smotic :ressurelgo. <ption# algorithmic

&;) solution of sucrose, , exerts an osmotic pressure of *./2 atm at &F C. What is

the molality of the sucrose solution? $he density of the solution is 1./1* g(mB.) /.1&; m

!) /.1& m

C) 1.-; m

") 1. mnswer#

"iff# -$opic# %ection 11.6 <smosis and <smotic :ressure


50




11.* %hort nswer Questions

1) +n a solution that is 0 ethyl alcohol and -0 water, the solute is '''''''' and the solventis ''''''''.

nswer# water, ethyl alcohol

"iff# &$opic# %ection 11.1 %olutions

&) ccording to the rule of thumb li4e dissolves li4e. ionic solids li4e aCl or polar substancesli4e glucose are more soluble in '''''''' solvents, whereas nonpolar substances li4e + & are

more soluble in '''''''' solvents.

nswer# polar, nonpolar


*) When >+ is dissolved in water, the maEor forces overcome are '''''''' forces in the solute

and '''''''' forces in the solvent, and the maEor forces created between solute and solvent particles are '''''''' forces.

nswer# ionic bonding, hydrogen bonding, ion8dipole"iff# *


-) Molarity is defined as '''''''', whereas molality is defined as ''''''''.

nswer# moles of solute(liters of solution, moles of solute(4ilograms of solvent

"iff# &


) $he number of moles of ions in & mB of &./ M a&%<- is '''''''' moles.nswer# /.1


2) $he volume of /.&// M 7&%<- that contains .// mmol of 7A is '''''''' mB.

nswer# 1&."iff# &


) $he solubility of a gas in a liuid is greatest at '''''''' pressures and ''''''''

temperatures.nswer# high, low

"iff# &$opic# %ection 11.- %ome 5actors $hat ffect %olubility

51




6) 5ree@ing point depression, boiling point elevation, vapor pressure lowering, and osmotic

pressure are examples of '''''''' properties, which depend on the amount but not the chemical

identity of dissolved particles.nswer# colligative

"iff# 1

$opic# %ection 11. :hysical !ehavior of %olutions# Colligative :roperties

;) $he boiling point of a solution containing a nonvolatile solute will be '''''''' than the

boiling point of the pure solvent, whereas the boiling point of a solution of two volatile liuidswill be '''''''' than the boiling point of the more volatile liuid and '''''''' than the boiling

point of the less volatile liuid.

nswer# higher, higher, lower


1/) 1./ m aueous CaCl& solution will have a '''''''' vapor pressure, '''''''' free@ing

point, and '''''''' boiling point than a 1./ m aueous solution of aCl.nswer# lower, lower, higher

"iff# *


chapter 11 review questions

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