Preparation of Solution from Solid: Practical General Chemistry Techniques
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A
solution
is a homogeneous mixture created by dissolving
one
or
more
solutes in a solvent. The chemical present in a smaller amount, the solute, is
soluble in the solvent (the chemical
present
in a larger amount).
Solutions
with
accurately known concentrations can be referred to as
standard (stock)
solutions
. These
solutions
are bought directly
from
the manufacturer or
formed by dissolving the desired amount of solute into a volumetric
flask
of a
specific
volume.
Stock solutions are frequently diluted to solutions of lesser concentration
for
experimental
use
in the
laboratory.
A
solution of known concentration can be prepared
from
solids
by
two similar methods. Although inherent
errors exist with each of the methods, with careful
technique either will suffice
for
making solutions in
General Chemistry
Laboratory.
Watch glass –Stirrer –Beaker –Spatula
–
funnel – volumetric Flask – Washing bottle –
Balance.
Sodium
carbonate
Na
2
CO
3
to
prepare
0.1 M
in
100
ml
of D.W.
Procedure:
1.
Weight the solid substance in a watch
glass.
2.
Transfer to a
beaker
and add a
small
amount of
solvent to the beaker and stirred the solution until the
solid substance is
dissolved.
3.
Transfer the solution to the
volumetric
flask.
4.
Put a
funnel
into the slim
neck
of the volumetric
flask
.
5.
Complete the
additional
of solvent to required volume
(add
solvent
until the liquid level reaches the calibration
mark).
6.
Capped the volumetric flask and inverted until
the
contents are thoroughly
mixed
and completely
dissolved.
M
o
l
a
r
i
t
y
(
M
)
=
m
a
s
s
(
g
)
*
1
0
0
0
/
M
.
w
t
*
V
(
m
l
)
M
o
l
a
r
m
a
s
s
f
o
r
N
a
=
2
3
,
C
=
1
2
,
O
=
1
6
M
.
w
t
o
f
(
N
a
2
C
O
3
)
=
(
2
*
2
3
)
+
1
2
+
(
3
*
1
6
)
=
1
0
6
M
o
l
a
r
i
t
y
(
M
)
*
M
.
w
t
*
V
(
m
l
)
/
1
0
0
0
M
a
s
s
(
g
)
=
1
0
0
0
/
0
.
1
*
1
0
6
*
1
0
0
=
1.06 g of Na
2
CO
3
dissolve in 100
ml
D.W.
Solutions are homogeneous mixtures where a solute is dissolved in a solvent. Known concentration solutions can be prepared using solid substances through careful techniques. This process involves weighing the solid, dissolving it in a beaker, transferring to a volumetric flask, and finalizing the solution volume. The concentration of the solution can be calculated based on the mass, molar weight, and desired molarity of the solute. Key equipment includes a watch glass, stirrer, beaker, spatula, funnel, volumetric flask, washing bottle, and balance.
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Presentation Transcript
AL-Mustaqbal University College Medical laboratory Techniques Department Practical General Chemistry Lecture four (Preparation Solution from Solid)
A solution is a homogeneous mixture created by dissolving one or more solutes in a solvent. The chemical present in a smaller amount, the solute, is soluble in the solvent (the chemical present in a larger amount). Solutions with referred to as standard (stock) accurately known concentrations can be solutions. These solutions are bought directly from the manufacturer or formed by dissolving the desired amount of solute into a volumetric flask of a specific volume. Stock solutions are frequently diluted to solutions of lesser concentration for experimental use in the laboratory.
A solution of known concentration can be prepared from solids by two similar methods. Although inherent errors exist with each of the methods, with careful technique either will suffice for making solutions in General Chemistry Laboratory.
Watch glass Stirrer Beaker Spatula funnel volumetric Flask Washing bottle Balance.
Procedure: 1.Weight the solid substance in a watch glass. 2.Transfer to a beaker and add a small amount of solvent to the beaker and stirred the solution until the solid substance is dissolved. 3.Transfer the solution to the volumetric flask. 4.Put a funnel into the slim neck of the volumetric flask.
5.Complete the additional of solvent to required volume (add solvent until the liquid level reaches the calibration mark). 6.Capped the volumetric flask and inverted until the contents are thoroughly mixed and completely dissolved.
Molarity(M) = mass(g) *1000/ M.wt * V(ml) Molar mass for Na=23 , C=12 , O=16 M.wt of (Na2CO3) =(2*23)+12+(3*16) =106 Mass(g)= Molarity(M) *M.wt*V(ml) /1000 1000 / 0.1 *106 *100 =
