0 - 2 ) BaCl, + H.SO 4 (aq.) (aq.) solution
Answers
Answer:
An aqueous solution of 2% non-volatile solute exerts a pressure of 1.004 bar at the normal boiling point of the solvent. What is the molar mass of the solute?
Hard
Solution
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Vapour pressure of pure water at boiling point (P
∘
) =1 atm=1.013 bar
Vapour pressure of solution (P
s
) =1.004 bar
Mass of solute =(w)=2g
Mass of solution =100g
Mass of solvent =98g
Applying Roault’s law for dilute solution (being 2%)
p
0
p
0
−p
s
=
n
1
+n
2
n
2
≈
n
1
n
2
=
w
1
M
1
w
2
/M
2
=
M
2
w
2
×
w
1
M
1
∴
1.013 bar
(1.013−1.004)
=
M
2
2g
×
98g
18g mol
−1
M
2
=
98
2×18
×
0.009
1.013
g mol
−1
M
2
=41.35 mol
−1
Explanation:
Answer:
Ba(pericipitate)+ClSO4(liquid) +H(gas)