Addition of non-volatile solute always increases the boiling point of the solution. Why?

Addition of non-volatile solute to a solvent always increases the colligative properties such as osmotic pressure. Delta P . Delta T_b and Delta T_f . All these colligative properties are directly proportional to molality if solutions are dilute. The increases in colligative properties on addition of non-volatile solute is due to increases in number of solute particles. For different aqueous solutions of 0.1 N NaCI, 0.1 N urea, 0.1 N Na_2SO_4 and 0.1 N Na_3PO_4 solution at 27^@C , the correct statements are : 1. The order of osmotic pressure is NaCI = Na_2SO_4 = Na_3PO_4 = urea 2. pi = (Delta T_b)/k_b xx RT for urea solution 3. Addition of salt on ice increases its melting point 4. Addition of salt on ice bring in melting of ice earlier

Noble gases have very low boiling points. Why?

The relative lowering of vapour pressure of an aqueous solution containing a non-volatile solute is 0.0125. The molality of the solution is

This question has statement I and II. Of the four choices given after the statements, choose the one that best describes the two statements. Statement - I : The boiling point of 0.1 M urea solution is less than that of 0.1 M KCI solution. Statement -II : Elevation of boiling point is directly proportional to the number of moles of non-volatile solute particles present in the solution.

The vapour pressure of a solvent decreases by 10 mm of Hg when a non-volatile solute is added to it. The mole fraction of the solute in solution is equal to 0.2. What should be the mole fraction of solvent if the decrease in vapour pressure is to be 20 mm Hg?

This question has statement I and II. Of the four choices given after the statements, choose the one that best describes the two statements. Statement - I : When 'a' mL of a 0.1 molal urea solution is mixed with another 'b' mL of 0.1 molal glucose solution, the boiling point of the solution is no different from the boiling points of the samples prior to mixing but if a mL of molal urea is mixed with 'b' mL of 0.1 molal HF the boiling point is different from the separate samples Statement -II : HF is an electrolyte (weak) whereas glucose is a non electrolyte.

A solution contains 5.6 gm of glucose in 1000 gm of water. Calculate the boiling point of the solution. ( k_b for water = 0.52 K kg mol^-1 )

Addition of a solute to pure water causes

A solution containing 6 gm of a solute dissolved in 250 ml of water gave an osmotic pressure of 4.5 atmosphere at 27^(@)C . Calculate the boiling point of the solution. The molal elevation constant for water is 0.52