Advertisements
Advertisements
Question
The observed depression in the freezing point of water for a particular solution is 0.093°C calculate the concentration of the solution in molality. Given that molal depression constant for water is 1.86 K Kg mol-1.
Advertisements
Solution
∆Tf = 0.093°C = 0.093 K, m = ?
Kf = 1.86 K Kg mol-1
∆Tf = Kf.m
∴ m = `(Delta "T"_"f")/"K"_"f" = (0.093 "K")/(1.86 "K K g mol"^-1)`
= 0.05 mol Kg-1 = 0.05 m
APPEARS IN
RELATED QUESTIONS
Suggest the most important type of intermolecular attractive interaction in the following pair.
acetonitrile (CH3CN) and acetone (C3H6O)
The molality of a solution containing 1.8 g of glucose dissolved in 250 g of water is
The partial pressure of nitrogen in air is 0.76 atm and its Henry’s law constant is 7.6 × 104 atm at 300 K. What is the mole fraction of nitrogen gas in the solution obtained when air is bubbled through water at 300 K?
Which one of the following is incorrect for an ideal solution?
For ideal solution the volume of mixing of the pure components to form the solution is ____________.
Which relationship is not correct?
Explain the terms ideal and non-ideal solutions in the light of forces of interactions operating between molecules in liquid solutions.
Lowering of vapour pressure of an aqueous solution of a non-volatile, non-electrolyte 1 molal aqueous solution at 100°C is ______.
If liquids A and B form an ideal solution, the ______.
Assertion (A): The enthalpy of mixing Δmix H is equal to zero for an ideal solution.
Reason (R): For an ideal solution the interaction between solute and solvent molecules is stronger than the interactions between solute-solute or solvent-solvent molecules.
