Molality of the solution is number of moles of the solute in ................... kg of ....................An aqueous solution of sugar boils ................. `100^@C` and freezes.......... `0^@С` .

Options

A. Solvent below, above, one
B. One, solvent, above, below
C. Above, solvent, one, below
D. One, below, above, solvent

Explanation

To solve the question, we will fill in the blanks step by step based on the definitions and properties of solutions.

### Step 1: Understanding Molality
Molality is defined as the number of moles of solute present in a specific mass of solvent. The formula for molality (m) is given by:

\[ m = \frac{\text{moles of solute}}{\text{mass of solvent in kg}} \]

### Step 2: Filling in the First Blank
From the definition of molality, we know that it is the number of moles of solute in **1 kg** of solvent. Therefore, the first blank will be filled with:

**1**

### Step 3: Filling in the Second Blank
The second blank refers to the substance in which the solute is dissolved. Since we are discussing an aqueous solution, the appropriate term to fill in the second blank is:

**solvent**

### Step 4: Understanding Boiling and Freezing Points
Next, we need to fill in the blanks regarding the boiling and freezing points of an aqueous solution of sugar. Sugar is a non-volatile solute, which means it does not contribute to the vapor pressure of the solution.

### Step 5: Filling in the Boiling Point Blank
An aqueous solution of sugar will have a boiling point that is elevated compared to pure water. Since pure water boils at **100°C**, the boiling point of the sugar solution will be:

**above 100°C**

### Step 6: Filling in the Freezing Point Blank
Similarly, the freezing point of the sugar solution will be depressed compared to pure water. Pure water freezes at **0°C**, so the freezing point of the sugar solution will be:

**below 0°C**

### Final Answer:
1. Molality of the solution is the number of moles of the solute in **1 kg of solvent**.
2. An aqueous solution of sugar boils **above 100°C** and freezes **below 0°C**.