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AcidlBase Chemist Worksheet
K’ ey
Name:
(show or change arrows where appropriate.)
1.
Write the equations showing the three steps for the ionization for :
4
P
3
H
0
1.
//o
F
2.
i [
3.
I_-I cc;, —
F
/-/
P
// C
F
i-I I
Write one equation showing all three steps as a single reaction:
q
3 // 2
I] r
;
2.
Write the equation for HSO
3 acting as a Bronsted-Lowry base when added to water:
3
HSO
3.
+
‘ +
tii
-
-
0
2
H
-*
// p,
1120
—*
H
—
1—4
0
‘
0
2
H
+
2—
-*
Write the equation for the ionization of the strong base Ba(OH)
2 in 1120:
2
Ba(OH)
7.
/
Write the equation for HS0
4 ‘acting as a Bronsted-Lowry acid when added to water:
’
4
HS0
6.
)-- )
Write the equation for 4
PO acting as a Bronsted-Lowry acid when added to water:
2
H
’
4
P
2
H
0
5.
-*
Write the equation for 11P0
2 acting as a Bronsted-Lowry base when added to water:
4
2
4
HP0
4.
0
2
H
+
+
0
2
H
->
t
) 1W
Write the equation for the ionization of the weak base Mg(OH)
2 in H
0:
2
2
Mg(OH)
+
0
2
H
•
Y1
Page 2
8.
Label the conjugate acid-base pairs for the following acids in water:
a.
2
HCIO
+
b.
0
2
H
+
0
2
H
oI
-
S
2
H
/‘73
/
/1 5
1
U
—
(13
c.
3
HBrO
0
2
H
+
13 03
(/3
1
0
-)
Complete the overall (molecular) equation and also write the total ionic equation and the net ionic
equation for the following:
9.
a.
H
*
KOH
—
7
HC1-
/4
F (1
F t /-/
/LL()
—
/
1—7
b.
0
4
S
2
H
+
i—
)
k
(overall)
7<
/
/17 Q
2
Ba(OH)
plF
(net ionic)
i(,)
tH
c
2
—*
)
(total ionic)
r
(overall)
(total ionic)
(net ionic)
Complete the following equations:
7
N
HC ‘(aq)
a.
Mg(s)
+
b.
3 (aq)
HNO
+
c.
CaO(S)
+
2 HCI(aq)
d.
BaO(S)
+
SO3(g)
*
e.
HC1(g)
+
0(I)
2
H
+
Ho
7
f.
CO
2
Na
(
3
)
+
S0 (aq)
2
H
4
>
-
g.
2 (g)
CO
+
NaOH(aq)
>
iV
h.
KOH(S)
+
0(l)
2
H
*
/4 F
i.
MgO>
+
j.
Na(S)
+
H2S04(aq)
k.
3 (s)
A1(OH)
+
0(I)
2
H
1.
)
5
CaO(
+
2 (g)
CO
NaOH(aq)
7,
IO3 (aq)
*
T
_
/4 NOy
/1’ —(-e)
Cci C
t
(i
i—
—
Ci
/_/
C 03
i-f
_fD,-
(
—
).5
$
/1/
1—/I- (c)
/-
‘
3
(C
H
3
(/Vt’
)L
(t
(C
0(i)
2
F1
1
/f C
m.
S0 (aq)
2
[[
4
+
n.
ZflO(S)
+
0.
3 (s)
0
2
A1
+
3 (aq)
FO
p.
S0 (aq)
2
H
4
+
BaO()
q.
3 (g)
SO
+
KOH(aq)
r.
O()
2
Na
+
S.
HC2H302(aq)
+
NH4OH(aq)
t.
MgO(S)
+
0(I)
2
H
5
/‘A
U.
2 (g)
SO
+
0(I)
2
H
/—/
_+
HBr(aq)
L HBr(aq)
/)ç
,_
Q/
//7 U
k4
/1/c JVt2y )3
U
c
3
/
()
—>
5
((
)
(I)
K H S 0(7
)—/-
O)
2
(
/V/
)/f)
j
i
0
-)
c)
1. Name each of the following acids or bases:
P0
3
H
4
1i /1
3
I{N0
1
P0 j) h
H
3
2
O
S0
2
H
4
NaOH
S0
2
H
3
2
Mg(OH)
3
A1(OH)
€ic:c
3
HC1O
2
HC1O
HF /l/f-)
HI
e
i
C
1’
11
S
2
H
/4yh
P
3
H
i,i4
d
7
//
I
1
li
1
áe./
/\/
/---t&.
J)
/
‘
LL
?
/77 (/t/t/
/(1
2
Fe(OH)
(Ii)
3
Fe(OH)
(iii)
hy
CuOH
U)
2
Cu(OH)
C/
AgOH
ii
ii
7
.(
2. Write formulas for the following acids and bases
/
Hydrochloric acid
Perchioric acid
Chromic acid
Hypochiorous acid
Dichromic acid
)-/.
Hydrobromic acid
Acetic acid
Li
(:7
/_-/
J3
—
I-I c H
1
t/-/
)Lif.7’
Dy
L/C
Zinc hydroxide
Nickel (II) hydroxide
Calcium hydroxide
/V,
(t,) L.
“iLJL
-
Major Naming Practice Mixed bag
1-lydrophosphoric acid
-:-‘.
JJ
r’
acids, bases, salts, and covalent compounds
—
potassium chromate
/4
use strategy!
—
ammonium hydroxide
t
1
/Vi-/
/
sodium bicarbonate
aluminum periodate
chromium (III) oxide
carbonic acid
carbon disulfide
carbon tetrachioride
sulfur trioxide
silver nitrate
fr( tij
silicon tetrabromide
s( j3,
iron (Ill)sulfate
5
,/1
3
C
lead (II) oxide
/VC’
tin (II) dichromate
c
0
7
C,
iron (II) sulfate
lead (II) phosphide
tin (II) chromate
3
FeSO
PbO
7
O
2
SnCr
1
V
Co
T
) Cii)
4
Mn(HS
2
)
O
(ii)
2
so
15
/V
J
( Iz’JJ /- ‘1
j
3
H
2
Ag
PO
4
CuHCrO
4
HC1O
t(
$/7 :/1i71i
C”
(r
S
2
)
4
(NH
5
PF
3
Al(BrO)
S
2
H
3
HgI-1C0
5
4
P
3
H
0
f
i),: h q
f/(’c
t