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Byju's Answer
Standard XII
Chemistry
Stoichiometric Calculations
50ml solution...
Question
50
m
l
solution of
B
a
C
l
2
(20.8 % w/v) and
100
m
l
solution of
H
2
S
O
4
(9.8 %w/v) are mixed then maximum mass of
B
a
S
O
4
formed is:
[
B
a
C
l
2
+
H
2
S
O
4
→
B
a
S
O
4
+
2
H
C
l
]
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Solution
B
a
C
l
2
+
H
2
S
O
4
→
B
a
S
O
4
+
2
H
C
l
Mass of
B
a
C
l
2
=
20.8
100
×
50
g
=10.4g
moles of
B
a
C
l
2
=
10.4
208
= 0.05 moles
Mass of
H
2
S
O
4
=
9.8
100
×
100
=9.8g
Moles of
H
2
S
O
4
=
9.8
9.8
=0/.1 moles
Therefore,
B
a
C
l
2
is a limiting reagent
Therefore , maximu moles of
B
a
S
O
4
formed is 0.05 moles
Maximum mass of
B
a
S
O
4
formed=0.05 x233g
=11.65g
Therefore maximum mass of
B
a
S
O
4
formed is 11.65 g
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Similar questions
Q.
50 mL solution of
BaCl
2
(20.8% w/v) and 100 mL solution of
H
2
SO
4
(9.8% w/v) are mixed then maximum mass of
BaSO
4
formed is:
[
BaCl
2
+ H
2
SO
4
→
BaSO
4
+ 2HCl
]
Q.
100 mL of 20.8%
B
a
C
l
2
solution and 50 mL of 9.8%
H
2
S
O
4
solution will form
B
a
S
O
4
(
B
a
=
137
,
C
l
=
35.5
,
S
=
32
,
H
=
1
,
O
=
16
)
B
a
C
l
2
+
H
2
S
O
4
→
B
a
S
O
4
+
2
H
C
l
Q.
50 ml of 20.8% (w/V)
B
a
C
l
2
(aq) and 100 ml of 9.8% (w/V)
H
2
S
O
4
(aq) solutions are mixed. Molarity of
C
l
−
ions in the resulting solution is : (At mass of Ba =137)
Q.
50 mL of 20.8% (w/v)
B
a
C
l
2
(
a
q
)
and 100 mL of 9.8% (w/v)
H
2
S
O
4
solutions are mixed. Find the mass the
B
a
S
O
4
formed.
(Molar mass of Ba = 137 g/mL)
Q.
The amount of
B
a
S
O
4
formed upon mixing
100
ml of
20.8
%
B
a
C
l
2
solution with
50
ml of
9.8
%
H
2
S
O
4
solution will be:
(Given that molecular weight of
B
a
=
137
,
C
l
=
35.5
,
S
=
32
,
H
=
1
and
O
=
16
g/mol)
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