commercially available concentrated hydrochloric acid is an aqueous solution containing 38% HCL gas by mass if its density is 1.1 gram per centimetre cube calculate the molarity of HCL solution and also calculate molar fraction of HCL and H2O
Answers
Answer:
Explanation:
Question 1:
H
C
l
(
38
%
)
=
(
38
g
H
C
l
100
g
Soln
)
=
(
?
moles
HCl
1.0
Liter
Solution
)
=> Moles of HCl in 38 grams =
⎛
⎜
⎝
38
g
H
C
l
36
(
g
mol
)
⎞
⎟
⎠
=
1.06
mole
H
C
l
=> Volume of Solution (Liters) containing 1.06 mole of HCl
=
100
g
H
C
l
(
38
%
)
1.19
(
g
ml
)
=
84.03
m
l
H
C
l
(
38
%
)
=
0.084
L
H
C
l
(
38
%
)
=> Molarity HCl(38%) =
1.06
mole
HCl
0.084
L
HCl
Conc
=
12.62
M
o
l
a
r
H
C
l
(
a
q
)
Question 2:
Use the solution prep equation for liquid mfg stock.
Volume of Liquid Mfg Stock needed in milliliters ...
=> Vol of Mfg Stock =
(
Molarity)(
V
o
l
u
m
e
)
(
formula
Weight
)
(
P
u
r
i
t
y
)
(
Specific
G
r
a
v
i
t
y
)
=>
(
0.10
M
)
(
1.0
L
)
(
36
(
g
mole
)
)
(
0.38
)
(
1.19
(
g
ml
)
)
=
7.96
m
l
o
f
H
C
l
(
38
%
)
MIXING: Add 7.96 ml of HCL(38%) into a small quantity of water, mix to disperse; then dilute with solvent water up to but not to exceed the total needed volume of solution (in this case 1.00 Liter). => 1.0 Liter of 0.10 Molar HCl(aq) Solution. => Verify concentration with standardized NaOH(solution).
MIXING CAUTION: Always add a concentrated strong acid into a small quantity of water, mix to disperse; then dilute up to, but not to exceed needed total volume of solution.
Water onto bulk strong concentrated acid may result in uncontrolled heat generation and flash boiling due to accelerated ionization rate.
Certainly wear protective eye ware and appropriate clothing.