Solutions

A dilute aqueous solution of sodium chloride shows a greater elevation in boiling point than an equimolal solution of glucose because:

1. Sodium chloride has a higher molar mass.
2. Glucose is more soluble in water.
3. Sodium chloride dissociates into ions, increasing the number of solute particles.
4. Sodium chloride lowers the vapour pressure less than glucose.

A solution contains a non-volatile solute. Which one of the following properties of the solvent decreases?

1. Boiling point
2. Freezing point
3. Vapour pressure
4. Osmotic pressure

Which of the following substances will have the highest Van't Hoff factor in dilute aqueous solution?

1. Glucose
2. Urea
3. NaCl
4. AlCl3

The Van't Hoff factor (i) is defined as:

1. Observed colligative property / Calculated colligative property
2. Calculated colligative property / Observed colligative property
3. Molarity / Molality
4. Mole fraction / Molarity

An ideal solution is one that:

1. Shows positive deviation from Raoult's law.
2. Shows negative deviation from Raoult's law.
3. Obeys Raoult's law over the entire range of concentration.
4. Has zero vapour pressure.

A solution is prepared by dissolving 2 moles of urea in 4 kg of water. The molality of the solution is:

1. 0.25 m
2. 0.50 m
3. 1.00 m
4. 2.00 m

The osmotic pressure of a dilute solution is given by:

1. Pi = Kb x m
2. Pi = CRT
3. Delta Tf = Kf x m
4. P = XP0

Which of the following solutions shows a positive deviation from Raoult's law?

1. Acetone + Chloroform
2. Water + Nitric acid
3. Ethanol + Water
4. Ethanol + Acetone

The depression in freezing point of a solution is given by:

1. Delta Tf = Kf x m
2. Delta Tf = Kb x m
3. Delta Tb = Kf x m
4. Pi = CRT

The boiling point of a solution is higher than that of the pure solvent because:

1. The vapour pressure of the solution is higher than that of the pure solvent.
2. The vapour pressure of the solution is lower than that of the pure solvent.
3. The solvent molecules become heavier.
4. The density of the solution decreases.

Henry's law states that at constant temperature, the solubility of a gas in a liquid is directly proportional to:

1. Vapour pressure of the solvent
2. Total pressure of the atmosphere
3. Partial pressure of the gas above the solution
4. Density of the liquid

The relative lowering of vapour pressure of a dilute solution is equal to:

1. Mole fraction of the solvent
2. Mole fraction of the solute
3. Molarity of the solution
4. Molality of the solution

According to Raoult's law, the vapour pressure of an ideal solution containing a non-volatile solute is:

1. Equal to the vapour pressure of the pure solvent.
2. Greater than the vapour pressure of the pure solvent.
3. Less than the vapour pressure of the pure solvent.
4. Independent of the amount of solute.

Which concentration term is independent of temperature?

1. Molarity
2. Normality
3. Molality
4. Strength

A solution is prepared by dissolving 0.5 mole of glucose in enough water to make 2 L of solution. The molarity of the solution is:

1. 0.10 M
2. 0.25 M
3. 0.50 M
4. 1.00 M