Relative molecular masses in solution questions | form five Chemistry

1. Boiling point of a solvent is elevated by addition of a non-volatile solute. Briefly explain.
2. Arrange the following aqueous solutions in order of increasing freezing point: 0.01 M ; 0.01 M ; 0.01 M ; 0.01 M KCl ; 0.01 M . Provide clear reason(s) for the arrangement.

You are provided with the following information.

Calculate the boling point and freezing point of a solution made by dissolving 2.40g of biphenyl, in 75.0 g of benzene, . Show your work clearly including manipulationsof units.

An aqueous solution of urea, at a concentration of 1.754 g dm^-3 is isotonic at the same temperature with an aqueous solution of sugar at a concentration of 10.00 g dm^-3 . Calculate the relative molecular mass of sugar.

Differentiate between cryoscopic constant and ebullioscopic constant.

Derive an expression relating the van`t Hoff factor (​i) and the degree of dissociation (α).

Briefly, explain the effect of degree of dissociation of a solute on the boiling point of a
solution.

What mass of ethylene glycol, C​_2​H​_6​O₂​ , the main component of antifreezing agent which must be added to a 10.0L of water to produce a solution for use in a car radiator, that freezes at -23.3^oC? Assume that the density of water is exactly 1g/mL and cryoscopic constant is 1.86^oC kg/mol.

A 0.120g of haemoglobin, the protein which carries oxygen in the blood was dissolved in 200cm​³ of benzene at 20^oC. The solution exerted an osmotic pressure of 25.6Pa. Find the relative molecular mass of haemoglobin.

A 1% solution of sodium chloride freezes at -0.604^oC. Calculate the degree of dissociation of the sodium chloride if the molal freezing point depression constant for water is 1.86^oC kg/mol.

State four colligative properties useful for determination of molecular masses.