Which of the following colligative properties can provide molar mass of Proteins, Polymers and colloids with greater precision?
Which of the following colligative properties can provide molar mass of Proteins, Polymers and colloids with greater precision?
- Depression in Freezing Point
- Relative lowering of vapour pressure
- Osmotic Pressure
- Elevation in boiling point
The Correct Option is C
Approach Solution - 1
Osmotic pressure is a colligative property that depends on the number of solute particles present in a solution, regardless of their nature. In the case of proteins, polymers, and colloids, these substances are often too large to accurately determine their molar mass using other colligative properties such as depression in freezing point or elevation in boiling point. These properties are more suitable for smaller molecules and non-volatile solutes.
However, osmotic pressure is not affected by the size or nature of the solute particles. It depends solely on the concentration of solute particles in the solution. By measuring the osmotic pressure and using the ideal gas law equation, the molar mass of proteins, polymers, and colloids can be determined with greater precision.
Therefore, the correct answer is (C) Osmotic Pressure.
Approach Solution -2
Which of the following colligative properties can provide molar mass of proteins, polymers and colloids with greater precision
- Depression in Freezing Point – ❌ Less accurate for macromolecules
- Relative lowering of vapour pressure – ❌ Not precise for large molecules
- Osmotic Pressure – ✅ Correct
- Elevation in Boiling Point – ❌ Small change, less accurate for large solutes
Explanation:
Osmotic pressure is highly sensitive to even small concentrations of solute and shows significant measurable values even for dilute solutions. This makes it the most precise method for determining the molar mass of macromolecules like proteins, polymers, and colloids.
Correct Answer: Osmotic Pressure
Top Questions on Solutions
According to the generally accepted definition of the ideal solution there are equal interaction forces acting between molecules belonging to the same or different species. (This is equivalent to the statement that the activity of the components equals the concentration.) Strictly speaking, this concept is valid in ecological systems (isotopic mixtures of an element, hydrocarbons mixtures, etc.). It is still usual to talk about ideal solutions as limiting cases in reality since very dilute solutions behave ideally with respect to the solvent. This law is further supported by the fact that Raoult’s law empirically found for describing the behaviour of the solvent in dilute solutions can be deduced thermodynamically via the assumption of ideal behaviour of the solvent.
Answer the following questions:
(a) Give one example of miscible liquid pair which shows negative deviation from Raoult’s law. What is the reason for such deviation?
(b) (i) State Raoult’s law for a solution containing volatile components.
OR
(ii) Raoult’s law is a special case of Henry’s law. Comment.
(c) Write two characteristics of an ideal solution.- A solution of glucose (molar mass = 180 g mol\(^{-1}\)) in water has a boiling point of 100.20°C. Calculate the freezing point of the same solution. Molal constants for water \(K_f\) and \(K_b\) are 1.86 K kg mol\(^{-1}\) and 0.512 K kg mol\(^{-1}\) respectively.
- Define Azeotrope. What type of Azeotrope is formed by negative deviation from Raoult's law? Give an example.
- Give reasons:
(a) Cooking is faster in a pressure cooker than in an open pan.
(b) On mixing liquid X and liquid Y, volume of the resulting solution decreases. What type of deviation from Raoult's law is shown by the resulting solution? What change in temperature would you observe after mixing liquids X and Y? - An unripe mango placed in a concentrated salt solution to prepare pickle, shrivels because __________
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Concepts Used:
Solutions
A solution is a homogeneous mixture of two or more components in which the particle size is smaller than 1 nm.
For example, salt and sugar is a good illustration of a solution. A solution can be categorized into several components.
Types of Solutions:
The solutions can be classified into three types:
- Solid Solutions - In these solutions, the solvent is in a Solid-state.
- Liquid Solutions- In these solutions, the solvent is in a Liquid state.
- Gaseous Solutions - In these solutions, the solvent is in a Gaseous state.
On the basis of the amount of solute dissolved in a solvent, solutions are divided into the following types:
- Unsaturated Solution- A solution in which more solute can be dissolved without raising the temperature of the solution is known as an unsaturated solution.
- Saturated Solution- A solution in which no solute can be dissolved after reaching a certain amount of temperature is known as an unsaturated saturated solution.
- Supersaturated Solution- A solution that contains more solute than the maximum amount at a certain temperature is known as a supersaturated solution.