A
4
5
A
3.
y,
"•
•4 --
PIT
ir
Ijl
1st , f i 1
sK
Multiple Choice Questions . ;'
' • • ' ' • • - . ..-:.,;fti:;^||fc
;*:'::*,,.
• - -• • .:•• - - . : . ? - . - ' • . • •
"V '- ' -.;'r'^.?-.:ijfe", -^v^'^*.' -'j:ij " •& •''
1. According
to the Lewis defimtion^^aMSa^ubltance
that
"
' . - ' : • . .-IS,.YTi-'.y^H2K!i*-.-:'Ss«i-*J«r-'*l...'
; lj
i
7
m
t
m
m
J
,,
..
,,
,
?
*.'••.-.
,. •
.,r:vfe^afif^2K|fe;|ft.
/f increases the hydrogen ion
concentrMioWwf&erhi'
' , - • ' • • 'i **i'i-.jl3'i*?js*"-ps'7*^i • j"."i' •v*yj r :
B) can react with water to'form
'
'
v
" • ':- .'• :- /-iii^^ri^^M^v^^
ffi-m^j^jff^^jj^
:.
•
•
' •
- -i . - -=y-ii%^v*fa^w:^:
: .::,;ri*fjS^:::S::;?||-;:, '
liiliBiaBailtfaMtaaaiiHaaBAtt^
V..^;v<£iwV :''" ' -^^'-V;=-- •"
.•. •.-.;-^«r.^>--y,'S..Si^arir.i.v:. .
' -- ' : r*^&;%v ^'^ Jv-fe ' ;' "-; • :
;
•^'f^Mm^&iSM^ms^,
S§p
.•1!
'«:*t|r' i|
•• ':iW£*^K,$%&.
. ••• • .-r^-«w-a'' ,•: y>x::>: •
•:-:^^£|i^^SMi,. . !,-•,
. • ivvfe-je'1. Vw. ••-; •t:--:.-.-.'1".. •
. :• '-•>•' .-.V^H;,..,..: ^..v^' •;
' .-"-'-•
-•••-"^:-.,^^ViH'--'^-V^W--"• ' • V;var"'^Vi:'N ' '"v:X^:5iM->'' - 1' •*
i
ii
ll
feif
I
iWi'!
'W
' " . . ' • "./••"" ^^^•^.^••^'^^'^^r-»'^'^1' "•- ;
^tincan accept an electron pair to JbrmWc^inff^^
A
y
L^
pp
£jp
*
* •
»
,
i[
•Hi ft
1( if
I
1
!
|
iU'r-'i
;-Vifni
i$i
^
;S| ?S
304
TOPIC
16
D) can donate a proton to a base.
E) can react with water toform hydronium ions.
2.
Which pair of chemical species is not a conjugate acid-base pair?'.
B) OH and HtO
C) HPO*-andPC
D) NH3andNH;
E)
3. Which oxide when mixed in equal molar amounts with water forms
solution with the lowest pH?
5; 03,
O 50,
4. When 0.2 moles of each of these salts are dissolved in one liter of
water, what is the order of increasing pH (lowest pH first) of the
resulting soultions?
A) NaCO3 < NaCfIp2
< NaCl < NHfl
B) NaCl < Na2CO3 < NaCfIp2
< NHfl
C) NHCl < NaCftp2 < NaCl < NafO3
NHfl <NaCl <
< Na2CO3
E) Na2CO3 < NaCl < NaCfl3O2 < NHfl
5. Aqueous solutions of equal molar concentrations of these salts are
listed in order of increasing pH. NaBr < NaIO3 < NaF <
NaCfip2<Na,S03
WJtich acid is the weakest?
A) HBr
B) HIO,
ACID-BASE EQUILIBRIA
C) HF
D) CH3COOH
NaHSO,
6. The net-ionic equationfor rthe addition of 10.0 mL of 0.10 M sulfurous acid to 10.0 ml of Q.10M aqueous sodium hydroxide is
A) H2SO3 + 2OH-* 2H2O +SO*
B) H2SO4 + OH-^ Hp
+ HSO+HSO;
'D) H+ + OH-* H20
E) HSO; + NaOH-^ NaSO; + H2O
7. Which is the acid anhydride of chlorous acid, HCIO2?
A) Clp
C\ Clp
5
8. Equal molar aqueous solutions of the chloride salts of the following
metals in their highest oxidation states were prepared and their respective pH's measured. Which is the correct order ofpH?
<Al<Cu<Ca<K
B) K<Ca<Cu<Al<Sn
^
' < * < * . {^^J^^>
C) Al<Cu<Ca Sn <K
D) Sn <Al<Ca<Cu<K
E) K<Cu<Ca<Al<Sn
9. The acid dissociation constants for the diprotic acid, malonic acid,
are Ka = 1.5 X 103 and Ka = 2.0X 10s.
What is Kb for
A)
305
306
TOPIC
16
B) KwxKa,
D) Kw/Ka,
E)
10. What is the percent ionization of a 0.10 M solution ofhydroazoic acid,
HN3? Ka = 1.9Xias.
A) 1.9X10*
B) 1.9.
C) 0.19
ib
1.4
E) 0.14
'
V- / • i
Free Response Questions
1. Sulfurous acid, H2SO3 is a diprotic acid.
X103.
= 1.7 X1O2. Ka=6.4
a. Write an ionic equation for the aqueous ionization that corresponds
to Kaf
Write an ionic equation for the aqueous ionization that corresponds
Identify the conjugate acid-base pairs in each of your two equations.
b. Identify any amphoteric species, other than water, in your equations.
c. Assume the amphoteric species you identified in Part bis a base.
Write an ionic equation for its aqueous ionization and calculate the
corresponding Kb.
d. Is an aqueous solution ofNaHSO3 acidic or basic? Explain your reasoning.
&
e. Calculate the pH of a 0.50 M solution ofNa2SOf
2. It isfound that 0.30 M solutions of the three salts XCly YC12 and
ZClhavepH's of 5.5, 7.0and3.7, not necessarily in order. (X, Yand
Z are metal ions. Cl is chloride ion)
a. i. Explain how metal ions can act as acids in aqueous solution,
ii. Which pH goes with which salt? Explain.