Which one of the following statements is false ? (a) The...

Which one of the following statements is false ? (a) The correct order of osmotic pressure for $0.01 M$ aqueous solution of each compound is $\mathrm{BaCl}_{2}>\mathrm{KCl}>\mathrm{CH}_{3} \mathrm{COOH}>$ sucrose (b) Isotonic solutions are those solutions which have the same osmotic pressure (c) Raoult's law states that the vapour pressure of a component over a solution is proportional to its mole fraction in liquid state (d) Two sucrose solutions of same molality prepared in different solvents will have the same freezing point depression

Which one of the following statements is false ?
(a) The correct order of osmotic pressure for $0.01 M$ aqueous solution of each compound is $\mathrm{BaCl}_{2}>\mathrm{KCl}>\mathrm{CH}_{3} \mathrm{COOH}>$ sucrose
(b) Isotonic solutions are those solutions which have the same osmotic pressure
(c) Raoult's law states that the vapour pressure of a component over a solution is proportional to its mole fraction in liquid state
(d) Two sucrose solutions of same molality prepared in different solvents will have the same freezing point depression

Key Concepts

Osmotic Pressure

Osmotic pressure is a colligative property that depends on the number of solute particles in a solution rather than their identity. It is a measure of the tendency of water to move from a region of lower solute concentration to one of higher solute concentration through a semipermeable membrane. The dissociation of electrolytes into multiple ions increases the number of particles, which in turn increases the osmotic pressure.

Isotonic Solutions

Isotonic solutions are those that have the same osmotic pressure, meaning they have an equal concentration of solute particles. This equilibrium in osmotic pressure prevents the net movement of water across a semipermeable membrane, a principle that is critical in biological systems to maintain cell integrity and proper physiological function.

Raoult's Law

Raoult's Law establishes that the vapor pressure of a solvent in an ideal solution is directly proportional to its mole fraction in the solution. It explains the vapor pressure lowering phenomenon, indicating that the presence of a non-volatile solute reduces the solvent's vapor pressure relative to the pure solvent, and serves as a fundamental principle in the study of colligative properties.

Freezing Point Depression

Freezing point depression is a colligative property where the addition of a solute to a solvent lowers the freezing point of the solution compared to that of the pure solvent. The magnitude of the freezing point depression is directly related to the number of solute particles present, rather than their specific identity, making it a useful concept when comparing solutions with different solutes in terms of their effect on the solvent's freezing point.

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