Advertisements
Advertisements
Question
Arrange the following in increasing order of boiling points:
(CH3)3 N, C2 H5 OH, C2 H5 NH2
Advertisements
Solution
This increasing order of boiling points can be explained by intermolecular hydrogen bonding. Tertiary amines, cannot engage in hydrogen bonding because they have no hydrogen atom bonded to the nitrogen atom, while primary amine undergoes intermolecular hydrogen bonding. But in the case of alcohol, the extent of hydrogen bonding is more as compared to amines because of a more electronegative oxygen atom in alcohol.
(CH3)3N<C2H5NH2<C2H5OH
APPEARS IN
RELATED QUESTIONS
Calculate the boiling point of solution when 4g of MgSO4 (M= 120 g mol-1) was dissolved in 100g of water, assuming MgSO4 undergoes complete ionization. (Kb for water = 0.52 K kgmol-1)
Define the following term:
Molal elevation constant (Kb)
Derive the relation between the elevation of boiling point and molar mass of solute.
Account for the following :
H2S has lower boiling point than H2O.
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:
Which of the following aqueous solutions should have the highest boiling point?
Which of the following has the lowest boiling point?
AB2 is 10% dissociated in water to A2+ and B−. The boiling point of a 10.0 molal aqueous solution of AB2 is ______°C. (Round off to the Nearest Integer).
[Given: Molal elevation constant of water Kb = 0.5 K kg mol−1 boiling point of pure water = 100°C]
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 solution will have the highest boiling point?
