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Chemistry
Chemistry
Problem
A half cell reaction:
Ag
2
S
(
s
)
+
2
e
⟶
2
Ag
(
s
)
+
S
2
−
\text{Ag}_2\text{S}_{(s)} + 2e \longrightarrow 2\text{Ag}_{(s)} + \text{S}^{2-}
Ag
2
S
(
s
)
+
2
e
⟶
2
Ag
(
s
)
+
S
2
−
is carried out in a half cell
Pt
∣
Ag
2
S
/
Ag
,
H
2
S
(
0.1
M
)
\text{Pt}\,|\,\text{Ag}_2\text{S}/\text{Ag},\,\text{H}_2\text{S}\,(0.1\,\text{M})
Pt
∣
Ag
2
S
/
Ag
,
H
2
S
(
0.1
M
)
, at
[
H
+
]
=
10
−
3
[\text{H}^+] = 10^{-3}
[
H
+
]
=
1
0
−
3
. The emf of a half cell is: [if
E
Ag
+
/
Ag
∘
=
0.80
V
E_{\text{Ag}^+/\text{Ag}}^\circ = 0.80\,\text{V}
E
Ag
+
/
Ag
∘
=
0.80
V
,
K
a
H
2
S
=
10
−
21
K_{a\,\text{H}_2\text{S}} = 10^{-21}
K
a
H
2
S
=
1
0
−
21
and
K
s
p
K_{sp}
K
s
p
of
Ag
2
S
=
10
−
49
\text{Ag}_2\text{S} = 10^{-49}
Ag
2
S
=
1
0
−
49
] a.
−
0.1735
V
-0.1735 \text{ V}
−
0.1735
V
b.
−
0.19
V
-0.19 \text{ V}
−
0.19
V
c.
+
0.1735
V
+0.1735 \text{ V}
+
0.1735
V
d.
+
0.19
V
+0.19 \text{ V}
+
0.19
V
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