How many grams of a stock solution that is 87.0 percent H2SO4 by mass would be needed to make 200 grams of a 35.5 percent by mas
1 answer:
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Answer:
0.13 m of → Highest boiling point
0.19 m of → Second Highest boiling point
0.17 m of → Third highest boiling point
0.31 m Sucrose (nonelectrolyte) → Lowest boiling point
Explanation:
Elevation in boiling is given by :
Where :
i = van't Hoff factor
= Molal Elevation constant of solvent
m = molaity of the solution
1) 0.19 m of
i = 2 (electrolyte)
Molality of the solution = 0.19
Elevation is boiling point of solution:
2) 0.17 m of
i = 2 (electrolyte)
Molality of the solution = 0.17
Elevation is boiling point solution :
3) 0.13 m of
i = 3 (electrolyte)
Molality of the solution = 0.13
Elevation is boiling point solution :
4) 0.31 m Sucrose (nonelectrolyte)
i = 1 ( non electrolyte)
Molality of the solution = 0.31 m
Elevation is boiling point solution :
Higher the value of elevation in temperature higher will be the boiling point of the solution .
The decreasing order of solution from highest boiling point to lowest boiling point is :
0.13 m of → Highest boiling point
0.19 m of → Second Highest boiling point
0.17 m of → Third highest boiling point
0.31 m Sucrose (nonelectrolyte) → Lowest boiling point