94.
SrX
2
(aq)
+
H
2
SO
4
(aq)
→
SrSO
4
(s)
+
2 HX(aq)
Calculation of the molar mass of X gives 35.5 g/mol; therefore, the original halide
formula is SrCl
2
.
H1CH3
:
x = (0.013668 mol H
2
O) / (0.00113895 mol KAl(SO
4
)
2
) = 12.00
complete formula = KAl(SO
4
)
2
•
12 H
2
O
66.
(a) 0.0664 L
(b) 7.2 x 10
25
Cu
2+
ions
(c) 0.491 M glucose
68.
(a) 312.5 mL
(b) 4.52 mL
(c) 39.9 mL
74.
0.0245 moles H
2
SO
4
are in excess
H2CH3
:
57.5% Mg
Chapter 4
11.
(a) Yes.
KOH is a strong base.
(b) No.
Glucose is not an acid, a base, or a salt, so
it is a nonelectrolyte, even though it is soluble in water.
25.
(a) balanced molecular equation:
3 CaCl
2
+
2 Cs
3
PO
4
→
6 CsCl
+
Ca
3
(PO
4
)
2
(s)
total ionic equation:
3 Ca
2+
+
6 Cl
–
+
6 Cs
3+
+
2 PO
4
3–
→
6 Cs
+
+
6 Cl
–
+
Ca
3
(PO
4
)
2
(s)
net ionic equation:
3 Ca
2+
+
2 PO
4
3–
→
Ca
3
(PO
4
)
2
(s)
spectator ions:
Cl
–
and
Cs
3+
Note:
In the equations above and below, one should write the state symbol (aq) on all
species for which the state symbol has been omitted.
(b) balanced molecular equation:
Na
2
S + ZnSO
4
→
Na
2
SO
4
+ ZnS(s)
total ionic equation:
2 Na
+
+
S
2–
+
Zn
2+
+
SO
4
2–
→
2 Na
+
+
SO
4
2–
+
ZnS(s)
net ionic equation:
S
2–
+
Zn
2+
→
ZnS(s)
spectator ions:
Na
+
and SO
4
2–
27.
(a) barium carbonate, BaCO
3
, is the precipitate.
(b) aluminum phosphate, AlPO
4
, is the precipitate.
37.
(a)
CsOH + HNO
3
→
CsNO
3
+ H
2
O(
ℓ
)
Cs
+
+ OH
–
+ H
+
+ NO
3
–
→
Cs
+
+ NO
3
–
+ H
2
O(
ℓ
)
OH
–
+ H
+
→
H
2
O(
ℓ
)
or
OH
–
+ H
3
O
+
→
2 H
2
O(
ℓ
)
spectator ions:
Cs
+
and NO
3
–
(b)
Ca(OH)
2
+
2 CH
3
COOH
→
(CH
3
COO)
2
Ca
+
2 H
2
O(
ℓ
)
Ca
2+
+
2 OH
–
+
2 CH
3
COOH
→
2 CH
3
COO
–
+
Ca
2+
+
2 H
2
O(
ℓ
)
OH
–
+
CH
3
COOH
→
CH
3
COO
–
+
H
2
O(
ℓ
)
spectator ions:
Ca
2+
39.
The nitric acid reacts with the bound OH
–
.
Balanced molecular equation:
Zn(OH)
2
(s)
+
2 HNO
3
(aq)
→
Zn(NO
3
)
2
(aq)
+
2 H
2
O(
ℓ
)
total ionic equation:
Zn(OH)
2
(s) + 2 H
+
+
2 NO
3
–
→
Zn
2+
+
2 NO
3
–
+
2 H
2
O(
ℓ
)
net ionic equation:
Zn(OH)
2
(s) + 2 H
+
→
Zn
2+
+
2 H
2
O(
ℓ
)
or
Zn(OH)
2
(s) + 2 H
3
O
+
→
Zn
2+
+
4 H
2
O(
ℓ
)
41.
0.06211 M H
2
SO
4
(aq)
76.
31.61% Fe

Chapter 5
12.
The statement is incomplete with respect to temperature and mass of sample.
At
constant temperature and moles of gas, the volume of the gas is inversely proportional to
the pressure.
13.
(a) variables: V and T;
fixed: P and n
(b) variables: n and V;
fixed: T and P
(c) variables: P and T;
fixed: V and n
34.
Molar mass = 20.2 g/mol.
The gas is neon.
38.
0.0044 mol Ar
87.
Molar mass = 171 g/mol; molecular formula is Si
2
F
6
.
106.
9.69 x 10
22
molecules CH
4
45.
1.57 g KClO
3
85.
(a) partial pressure of N
2
= 188.5 mmHg
(b) partial pressure of Cl
2
= 566 mmHg
(b) 4.94 g NCl
3
61.
(a) curve 1
(b) curve 2
(c) curve 2
65.
(a) 1.30 x 10
3
m/sec at 0
o
C
and
1.37 x 10
3
m/sec at 30
o
C
(b) rate
helium
/ rate
xenon
= 5.72
(c) E
k
= ½ m
2
u
= (3/2)(R / N
A
)T , where m is the mass of an
atom or molecule.
For helium and xenon at 30
o
C, E
k
= 3.78 kJ/mol.
(d) 6.27 x 10
–21
J
Chapter 6
23.
initial temperature = 42.8
o
C
27.
53 mL of water
H1CH6
:
q
V
=
–25.7 kJ/g
30.
The reaction is 2 KOH(aq) + H
2
SO
4
(aq)
→
K
2
SO
4
(aq)
+
2 H
2
O(
ℓ
).

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- Spring '08
- smith
- Atom, coo, Chemical bond, net ionic equation, total ionic equation