NAME:
I~
~
PERlOD:
CHAPTER 14 REVIEW PROBLEMS
1. Write the dissociation reaction for each of the following acids in water and identify the
conjugate acid-base pairs:
a.
Formic acid (HCOOH)
J.i
COO
I-l
(o.;?
H 1- Co.])
~>
COO 1-/
-t-
c.8
CfJ..
b.
Perchloric acid (HCl04)
I-ICeO'1 (001
I-rr
-'7
(tl~)
C.l a 4 -
+
cA
c.
co.r;)
(a.~)
c.8
The hydrated iron (III) ion [Fe(H20)63+]
.3+
[Fe (Ii.l 0 ) (" ]
({).(1J'
H- -rctp)
~
[i="~ (OH)
-+
( I-Id 0) s
J
~+
('i)
cA
2. Complete the following table:
pH
Solution a
1. I ;:)
o.qa
Solution c
It),
Solution d
~
7,00
[OH-]
_'1
6.88
Solution b
[H+]
pOH
/3. O~
9
1.3"1.101'1
-~
7. ~ XIO
f'1
I~
8.4 x 10-14
o .t d
If
1'1
3.11
-II
1.3yro
l'1 ?
- 'I
f' X 10 f'1
1.0 x 10-7
7.00
Acid, base or
neutral
-7
t3
Ai
/.0 X 10 M
- 1" I~
10
OVER
-
----
-
--
-
-- ----
-
---
---
-------
-----
--
3. The pH of gastric juice in a person's stomach is 2.1. Calculate the pOH, [H+], and [OH-] for
is sam le.
\
It_~~~.J
~. I
10
-J
[OH
! 0, 001
-~. I
[li+ ]
z:
10
z:
- II. Cj
ql{ fYl \
----~.:T~--~--!
I ------.
I
~ I J. a ~ x
IV
f1
." .~-~~~
L.
4. Calculate the concentration of an aqueous HN03 solution that has a pH
J
r
UfT
10
z:
=
5.10.
-DJ-l
r
- S./O
s:
10
7. q t.f X I 0
==
-t..
'1
5. Monochloroacetic acid, HC2H2CI02, is a skin irritant that is used in "chemical peels" intended
to remove the top layer of dead skin from the face and ultimately improve the complexion. The
value of K, for mono chi oro acetic acid is 1.35 x 10-3. Calculate the pH ofa 0.10 M solution of
monochloroacetic acid.
H C d ~:J C.Q 0 ~(~j) ~7'
H -+ (~) -+ C;;.H ~ CiO a - (~ )
o
J:
•
C
- -y.
~
, I - -y
I
+')(
_4
X
&.J.
_3
-/.3SxJO
•
_.
I.
:
J
[~C~Hi!Cl0a
00 135
1C
oO,,3S
-
~ ~
-
t
:=
0.0
Y..
'0
z
J(
000 13 S :::0
(.OO/3S)d_
~(I ')
x "[H J
ss
~
X
•
fli ~ -.ty(otl)
_3
Kl\ ;; [Hi] [C.~Hd (103- ]
1.3~X/O
0
I' 1'1
'-I
(1}(-.()OOI3~)
---
{t:Ctt:-7
6. Trichloroacetic acid, CChC02H, is a corrosive acid that is used to precipitate proteins. The
pH of a 0.050 M solution oftrichloroacetic acid is the same as the pH of a
0.040 M ~I04 solution. Calculate K, for trichloroacetic acid.
rb
fl-f
Cd
CD ~ H ("-1)
H + (~)
~
C C1.3 COf)- -
+
(()Jb)
0
.,. . 0 3'1 ~
E
;: - 10~ (.0 t() :: I. tf 0
He~O-l
0.0...,0 fV)
.0.5
I
e
3
t-I
-I-
[H-t
aq ~
• o~q~
d,
.010
• ()
J [CCi3CO J
-
he)("K )
d
-----
c. 03r.;S-) (r
.OS-)!
[ce13 CO~ H]
• 010 ~
7. Calculate the pH of a 0.20 M solution of iodic acid, HI03. K, = 0.17.
H I 0.3
("i,)
H + ((t.~)
~
I 03 -
+
0
,aO
- :X
.J--y.
+'X
x
[H -t ] [TO
[HIOs
£ •
J
~)
0
+)(
X
("'I-) ("'/.)
:;
J
0./1
::
.d.-j!
034 - • (I ~ ~ it J
x ~ + • , 1'Y- .Il
-
•
034
~~ (./l):;'
:: 0
- (4"')(I)(-.03L/)
----5(0-.~-----.--.-*.-
7::
O. 11 g
M :.
( f'"(=I---:--:q-J--j
\\.._-----.~,-~-
[l4-t
0 3qe)
.:.
J
OVER
;XfJ
-
.J-Y-
8. Write the reaction and corresponding Ks equilibrium expression for each of the following
substances acting as bases in water:
a. Hydroxylamine, HONH2
1+0 N I-b lOon'>
~ j~~ 0 (1.)
~6
:=
[\-lONH3+]
[O/-l-J
[HOAJH~J
b. Pyridine, CsHsN
CS.I-l5~
((;.1)
1<6
C s H.s N
N H +] [01-/ - J
1-1:1.0 (~)
of
[Csl-i5
z:
~
l-t (~)
0)-1 - (~)
-+
[Csl-IstJ]
9. Calculate the concentration of an aqueous solution of Al(OH)3 that has a pH = 10.50.
fOI-\
z: ILf,DO
- lb. SO
:: 3.~O
Lol-I-) ~ IO-~'sO
lA Q (01") s ]
B.'
=
=
3.110
)<.J(j'1't
v: 10- 4 f"1
It,
1O. .Calculate the [OR], [H+], and the pH of 0.20 M solutions of each of the following (the Ks
values are in Table 14.3):
a. aniline
C(; 1-1s N t-1 J (~
:r
.., 1-17.0 (1) ~
'!.., 0
-.0
C(, 1-15 '"
.dO
c.
-
[C.c.~sN"./
0
"tl!
-+?C
• a- 'Y-:
oH -
1-13 ., Co.li) *
0
-')C
t:
~b
K"b :: 3. ~
~
'X
J
(OH'J
-- J.8x/0
[e(' ~s ~U-hJ
1tJ
z
,Cl-')C
~!..S
}(2-
::
:
r--------....
I.OY/O-1"{
r,7dXIO-
("x)(1t. )
-10
XIO-~fVl"J
.J
V)
(().I
b.
o
"1
~ I. 7
Pyridine
Csl-l.s fJ ~b)
-'1
')( 10
~20 (1) ~
-t
I
• J.
o
c
- /l
+}C
E
o
• d.-)t
I. 7 X I 0
'X
z.
.5,l/ y- 10
s:
X ~
-'I
=
H-t:.
- fe
1,;;'1~~ ft--:-r;=jl
I
N Ii C'iJ) +
H2.0
(.0 ~
-
t
&\.('1.10- s
Kb = 1.3 X 10-3.
(C/··b)., tJ I-la + (Q-~I +-
.05
c
- If(
1.0 '/: 10
-s
11. Calculate me pH of a O·.O·5lrlvrs~CH3)2NH,
3) d
::
.a
I.
1
(tIt
(x)C'k)
0
H -('1)
0
0
+"f
'Y.OS--y:
ex) c,,}
,OS -
x
=-
4--J
-1
(t. '3
z.
-ao
-!»2..
- (tt)(I)(-f."SX/O
.,"2 (I)
=
f
0H
1"
0.00/4:;
z:
H~
-
r(jl~-J
Jo,j (.0014)
/4. 00 -
d,
:
I ~,
'X
d. 13
@
OVER
-5)
12. A 0.025 M solution of hydroxylamine has a pH of9.11.
Calcuate the Ki, of this weak base.
H2NOH (aq) + H20 (1) ~ H3NOH+ (aq) + OH- (aq)
r
.o~S
0
C
- -x:
+ ')(
E
,Q.;JS-)L
~b
0
t
X
= [ ~ a NO H ~ J [01-\ -
J
1C
(I.
.::
't-
;l'1 ¥ I
o -s)
_10
a
J.~~
X 10
::
, 0 ~ l(~g
[H~MOH )
= 4. gq
_os
I,
Q.tj
Y-(O
M
13. Write out the stepwise K, reactions and stepwise K, expressions for ascorbic acid
(H2C6H606), a diprotic acid.
I~~ C,.
l-t" 0 {, (~)
~ / 1-/ C~ I~(, 0" - (~)
[He" ~ ~ 0 (,-]
+
J-J
of
[H.J]
[H~ C.,l l-lt, O~)
C/; /-1 c 0(,J - +
[c<. H(.0 (,eJ-] [Ht]
(~)
<!:'
=7
[ ~C(,\-\" 0 f, -
J
1-1 -+
(ilt)
14. The sodium salt of propanoic acid, NaCH3CH2C03, is used as an antifungal agent by
veterinarians. Calculate the equilibrium concentrations of H+, OR, and the pH, for a solution of
0.10M NaCH3CH2C03.
Net
C I-) :1 ().-l,;) CO J
c'4 3 tl-l ;}CJ) 3-
+
C I-/~ CH CO3 J
I~.l0 coJ
+-
<E
C(~ 3 CJ1~(J)~~I(~)
-;;>
+
0
c..
--X-
f
.I-/C
c
(~)
l'
. I
T
~b
-'),J\.h
J
J ~ k'w- I. 0 ~ 10
co,-,J
~ :: 1.3 '" I;-~ :: 7.?
[Cl-t3Ct-·\z CO 3 \~ [011-
[t43C~L
'X .: [0 Ii -]
fOH
s:
z:
[CI4J
-10"
x:
-It{
y
10
-
•I
-t..
C.H~C04H]
Z, ~ '110- (.::
_ 10
:: 2. g"X 10
fH
S.O ~
fI\
14.00-
.=
S.o~
-
15. Calculate the pH of a 0.1 OM CoCh solution. The K, value for CO(H20)63+ is 1.0
[Co
(Q,01,..
~
[c., (OH)(
.1
I
- Y-
E
.1- Y
.2+~)
-
.:>.+J
.. --~--
LCo (1-\,,0 )1. 3+ J
'110
X=[HiJ::
+
If
10-5.
t ("7J)
0
+'X
.: ([Co(O~f)( ~~O)s ]
1,0
IM)J
0
L
k4
J 3 c;)
X
-0
=X
[\4t]
-oS
:::'.0 X 10
1-
.001
OVER
::
I
16. Identify the Lewis acid and Lewis base in each of the following reactions:
a.
HN02 (aq) + OR ~ N02" (aq) + H20 (1)
LA
b.
L6
FeBf3 (s) + Br (aq) ~ FeBr4" (aq)
L.A
Lib
c. Zn2+(aq) + 4 NH3 (aq) ~ Zn(NH3)l+ (aq)
LA
L6
d. S02 (g) + H20 (I) ~ H2S03 (aq)
LA
MULTUPLE
.e
CHOICE
17. The Ka, acid dissociation constant, for an acid is 9 x 10-4 at room temperature. At this
temperature what is the approximate percent dissociation of the acid in a 1.0 M solution?
A. 0.03%
B. 0.09%
(93%
D.5%
E. 9%
l(t,t: [I·P] [4- J
[IiA
J
-'Z.
'X.::
~ 't(0
70 ~
q '{..I 0
=
=
(1
s:
, -")(
_,
$, 't,
(
:!_l.._
_I.{
10)
'1
~
100l'Q
-
a 10
18. Phenol, C6H50H, has a K, = 1.0 X 10"10.What is the pH of a 0.010 M solution of phenol?
@ between
3 and 7
B. 10
C. 2
D. between 7 and 10
E.7
KOl .La
it.:..
~
m1.(M}
fH
(j.~~
,<)0
it
a-tl..cJ dL.:v~~
t .ht elM ~
a.
f
Cin~
.
A
AO
ruJd.
~'\4
JlA.-a
tt
J
Pht'l'lJ.k,
H 14 ~
Cl
.L4ft.J.
Mid
~.
--.-----~
19. H2P04- (aq) + H20 (1) ~ H30+ (aq) + HP042- (aq)
Which species in the above equilibrium behaves as bases?
I. HP04II. H2P04III. H20
AA) ~
r:F~;t -;tk ,ifU ) ffi
~~
~
I-li}- 0
:Ru Ii + 3:0 ~rt
~.3 0 1.. lJ~\ .::I:h ~\;
Af :it I-J Po~'"- ~
/.;+ 1-' I/., 0" ,
~
A. I only
B. I and II
C. II and III
@IandIII
E. III only
20. This is a strong electrolyte.
(A)HN03
1rHCN
C. H2C03
D. HF
E. H20
21. Which of the following salts will produce a solution with a pH of greater than 7 when
dissolved in distilled water?
@NaCN
B. KCI
C. NaN03
D. NH4N03
E. KI
J!~
JJu.
t\
.
ffi CiJ)'t~o..k 1a ~~ ~ (Ak +) ~tc(
CIDfaC~.JL 1\o. J.v-f!.J w.d (CtJ - ). 'VItia /.;Jt~
~
~
~'\;.
22. A solution of which of the following salts will have the lowest pH?
OVER