Answer:
The problem with this question is that you can't really have an aqueous solution of calcium oxide,
CaO
, because this compound will react with water to form calcium hydroxide,
Ca
(
OH
)
2
.
CaO
(
s
)
+
H
2
O
(
l
)
→
Ca
(
OH
)
2
(
a
q
)
+
energy
Keep in mind that this reaction is highly exothermic!
So, you can't talk about a solution that contains calcium oxide, which you'll maybe recognize as quicklime, because calcium oxide does not exist as such in aqueous solution, it exists as calcium hydroxide, or slacked lime.
Moreover, you should also keep in mind that calcium hydroxide is not that soluble in water to begin with, so chances are that some calcium hydroxide will precipitate out of the solution.
In your case, you're mixing
32.5
g
⋅
1 mole CaO
56.0774
g
=
0.5796 moles CaO
and
212
g
⋅
1 mole H
2
O
18.015
g
=
11.768 moles H
2
O
so the reaction will produce
0.5796
moles of calcium hydroxide--keep in mind that calcium oxide acts as a limiting reagent because of the
1
:
1
mole ratio that exists between the two reactants.
This is equivalent to
0.5796
moles Ca
(
OH
)
2
⋅
74.093 g
1
mole Ca
(
OH
)
2
=
42.9 g
of calcium hydroxide. So your resulting solution will contain
11.768 moles
−
0.5796 moles
=
11.188 moles H
2
O
Step-by-step explanation: