Calculate the pH of 0.025 molar barium hydroxide solution
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58
Answer:
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Answered by
2
Answer:
Barium hydroxide is a strong base for both stages of dissociation:
Ba
(
OH
)
2
(
s
)
→
Ba
2
+
+
2
OH
−
So the solution will have 0.20 M hydroxide ions. Now use the autodissociation product for water:
[
H
+
]
[
OH
−
]
=
1.0
×
10
−
14
M
[
OH
−
]
=
2.0
×
10
−
1
M
[
H
+
]
=
5.0
×
10
−
14
M
And then
pH
=
−
log
10
(
[
H
+
]
=
5.0
×
10
−
14
)
=
13.30
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