Advertisements
Advertisements
Question
Which of the following aqueous solution will have the highest boiling point?
Options
1.0 M KCl
1.0 M K2SO4
2.0 M KCl
2.0 M K2SO4
Advertisements
Solution
2.0 M K2SO4
Explanation:
The higher the van't Hoff factor (i) and molarity, the higher the boiling point.
APPEARS IN
RELATED QUESTIONS
Out of 1 M glucose and 2 M glucose, which one has a higher boiling point and why?
Define the following term:
Colligative properties
Account for the following :
H2S has lower boiling point than H2O.
Arrange the following increasing order of their boiling point:
CH3CH2OH, CH3CHO, CH3–O–CH3
0.450 g of urea (mol. wt. 60) in 22.5 g of water show 0.170°C of elevation in boiling point. The molal elevation constant of water is:
Exactly 1 g of urea dissolved in 75 g of water gives a solution that boils at 100.114°C at 760 torrs. The molecular weight of urea is 60.1. The boiling point elevation constant for water is:
Molal elevation of boiling point constant is the elevation of boiling point produced by ______
Assertion (A): Elevation in boiling point is a colligative property.
Reason (R): The lowering of vapour pressure of solution causes elevation in boiling point.
Calculate the boiling point elevation for a solution prepared by adding 10 g of MgCl2 to 200 g of water, assuming MgCl2 is completely dissociated.
(Kb for Water = 0.512 K kg mol−1, Molar mass MgCl2 = 95 g mol−1)
Which of the following aqueous solutions will exhibit the highest boiling point?
