Chemistry Reference
In-Depth Information
9.9
Write a net ionic equation for the reaction of (a) Zn with
HCl, (b) Zn with any strong acid, and (c) Zn with a
strong acid.
9.10 Assuming that each of the following compounds is in
aqueous solution, write its formula to best represent it:
(a)
9.12 Write a net ionic equation for each of the following
reactions:
(a)
Ba(OH)
2
(aq)
2 HCl(aq) £
BaCl
2
(aq)
2 H
2
O(
/
)
(b)
Ba(OH)
2
(s)
2 HCl(aq) £
BaCl
2
(aq)
2 H
2
O(
/
)
NH
4
ClO
3
(b)
HC
2
H
3
O
2
(c)
CO
2
(c) Is the same quantity of heat expected in each
reaction?
9.13
A bottle labeled “ Test Reagent” in a chemistry lab
is used to test for the presence of silver ion. What does
the bottle contain?
(d) (e) (formaldehyde)
9.11
Which ones of the following are strong electrolytes?
Which conduct electricity?
(a) HCl(g)
AlCl
3
CH
2
O
Ag
(b) KCl(s)
(c) H
2
SO
3
(
/
)
Problems
9.1 Properties of Ionic Compounds in Aqueous
Solution
9.21 Balance each of the following net ionic equations:
(a)
(b)
(c)
(d)
Co
3
(aq) £ Co
2
(aq)
Mn
2
(aq)
Mn(s)
NH
3
(aq)
Cu
2
(aq) £ Cu(NH
3
)
2
9.14
Assuming that each of the following compounds is in
aqueous solution, write its formula to best represent it:
(a)
(aq)
4
Ce
4
(aq)
Pd
2
(aq) £ Pd
4
(aq)
Ce
3
(aq)
CuSO
4
(b)
H
2
S
(c)
HNO
2
PbSO
4
(s)
H
2
O(
/
) £
2
(aq)
H
(aq)
Pb(s)
(d) (e)
9.15
Write the formula for each of the following compounds
to best represent it in the presence of water:
(a) (b) (c)
(d) (e) AgCl (f )
9.16 Write the formula for each of the following compounds
to best represent it in the presence of water:
(a) (b) (c)
(d) (e) (f )
9.17
(a) Would HF or NaF be better for making a solution con-
taining fluoride ion, or doesn't it make any difference?
(b) Would HCl or NaCl be better for making a solution
containing chloride ion, or doesn't it make any dif-
ference?
9.18 Would an alkali metal phosphate or a transition metal
phosphate be better for making a solution containing
phosphate ion?
UO
2
(NO
3
)
2
(NH
4
)
2
Cr
2
O
7
PbO
2
(s)
SO
4
9.22
Write a net ionic equation for each of the following
reactions:
(a)
(b)
HClO
4
CuCl
2
HClO
2
BaI
2
(aq)
K
2
CO
3
(aq) £ 2 KI(aq)
BaCO
3
(s)
Cu
2
S
(NH
4
)
2
SO
3
2 HNO
3
(aq)
Ba(OH
2
)(s) £
Ba(NO
3
)
2
(aq)
2 H
2
O(
/
)
(c)
NaHCO
3
(aq)
NaOH(aq) £
Na
2
CO
3
(aq)
H
2
O(
/
)
ZnCl
2
(NH
4
)
2
S
2
O
3
Hg
2
O
(d)
NaHCO
3
(aq)
HCl(aq) £
BaCO
3
(s)
Li
2
SO
4
H
3
PO
4
NaCl(aq)
H
2
O(
/
)
CO
2
(g)
(e)
(f )
NaBr(aq)
AgNO
3
(aq)£NaNO
3
(aq)
AgBr(s)
Pb(C
2
H
3
O
2
)
2
(aq)
2 KI(aq) £
PbI
2
(s)
2 KC
2
H
3
O
2
(aq)
9.23
Do either part (a) or part (b).
(a) Write a total equation for the reaction of 15 different
soluble metal chlorides with each of the following:
lead(II) nitrate, lead(II) acetate, and lead(II) chlorate.
(b) Write one net ionic equation representing all 45
equations of part (a).
9.24 Write six total equations that correspond to the following
net ionic equation and have an alkali metal ion and ni-
trate ion as spectator ions:
9.2 Writing Net Ionic Equations
9.19
Balance each of the following net ionic equations:
(a)
(b)
(c)
(d)
(e)
9.20
Write a net ionic equation for the reaction of an insoluble
metal oxide, represented as
Cr
3
(aq) £ Cr
2
(aq)
Pb
2
(aq)
Pb(s)
Br
(aq)
Ce
4
(aq) £ Ce
3
(aq)
Br
2
(aq)
Pb
2
(aq)
S
2
(aq) £ PbS(s)
Ag
(aq)
Cu(s) £ Cu
2
(aq)
Ag(s)
9.25 Write a net ionic equation for the reaction of silver acetate
with each of the following in aqueous solution:
(a) Aluminum chloride
(b) Vanadium(II) chloride
(c) Cadmium chloride
Cu
2
O(s)
H
(aq)£Cu(s)
Cu
2
(aq)
H
2
O(
/
)
Co
3
(aq)
Co(s) £ Co
2
(aq)
M
2
O
3
,
with a strong acid, H
2
X.
