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Class 11 NEET Chemistry Some Basic Concepts Of Chemistry
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© examsnet.com
Question : 18
Total: 60
What is the mass of the precipitate formed when
50
mL
of
16.9
%
solution of
AgNO
3
is mixed with
50
mL
of
5.8
%
NaCl
solution ?
(
Ag
=
107.8
,
N
=
14
,
O
=
16
,
Na
=
23
,
Cl
=
35.5
[NEET 2015]
3.5
g
7
g
14
g
28
g
Validate
Solution:
👈: Video Solution
50
ml
of
16.9
%
solution of
AgNO
3
(
16.9
100
×
50
)
=
8.45
g
of
AgNO
3
n
mole
=
8.45
g
(
107.8
+
14
+
16
×
3
)
g
∕
mol
=
(
8.45
g
169.8
g
∕
mol
)
=
0.0497
moles
50
ml
of
5.8
%
solution of
NaCl
contain
NaCl
=
(
5.8
100
×
50
)
=
2.9
g
n
NaCl
=
2.9
g
(
23
+
35.5
)
g
∕
m
o
l
=
0.0495
moles
AgNO
3
1
mole
0.048
mole
+
NaCl
1
mole
0
.049
mole
⇒
AgCl
1
mole
0
.049
mole
of
AgCl
+
Na
⊕
+
Cl
⊖
n
=
w
M
⇒
w
=
(
n
AgCl
)
×
Molecular mass
=
(
0.049
)
×
(
107.8
+
35.5
)
=
7.02
g
© examsnet.com
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