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Chemistry
Chemistry
Problem
For the reaction,
2
F
e
3
+
(
a
q
.
)
+
(
H
g
2
)
2
+
(
a
q
.
)
⇌
2
F
e
2
+
(
a
q
.
)
+
2
H
g
2
+
(
a
q
.
)
2Fe^{3+}(aq.) + (Hg_2)^{2+}(aq.) \rightleftharpoons 2Fe^{2+}(aq.) + 2Hg^{2+}(aq.)
2
F
e
3
+
(
a
q
.
)
+
(
H
g
2
)
2
+
(
a
q
.
)
⇌
2
F
e
2
+
(
a
q
.
)
+
2
H
g
2
+
(
a
q
.
)
K
C
=
9.14
×
10
−
6
K_C = 9.14 \times 10^{-6}
K
C
=
9.14
×
1
0
−
6
at 25°C. If the initial concentration of the ions are
F
e
3
+
=
0.5
M
Fe^{3+} = 0.5 M
F
e
3
+
=
0.5
M
,
(
H
g
2
)
2
+
=
0.5
M
(Hg_2)^{2+} = 0.5 M
(
H
g
2
)
2
+
=
0.5
M
,
F
e
2
+
=
0.03
M
Fe^{2+} = 0.03 M
F
e
2
+
=
0.03
M
and
H
g
2
+
=
0.03
M
Hg^{2+} = 0.03 M
H
g
2
+
=
0.03
M
. What will be the concentrations of ions at equilibrium?
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