What is the pH of a solution containing 1.95 g pure H2SO4 per dm' of a solution?
Answers
Answered by
3
Answer:
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Explanation:
Explanation:
We assume complete dissociation of the sulfuric acid:
H
2
S
O
4
(
a
q
)
+
2
H
2
O
(
l
)
→
2
H
3
O
+
+
S
O
2
−
4
And so
[
H
2
S
O
4
]
≡
1.95
⋅
g
98.08
⋅
g
⋅
m
o
l
−
1
1
⋅
d
m
3
=
0.0199
⋅
m
o
l
⋅
L
−
1
. However, this is a FORMAL concentration and corresponds to
[
S
O
2
−
4
]
.
[
H
3
O
+
]
=
0.0398
⋅
m
o
l
⋅
L
−
1
, i.e. TWICE the formal concentration.
Now since,
p
H
=
−
log
10
[
H
3
O
+
]
,
p
H
=
−
log
10
(
0.0398
)
=
?
?
Answered by
3
Answer:
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Explanation:
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