The osomotic pressure `pi` depends on the molar concentration of the solution `(pi=CRT)`. If two solutions are of equal solute concentration and, hence, have the same omotic pressure, they are said to be isotonic. If two solutions are of unequal osmotic pressures, the more concentrated solution is said to be hypertonic and the more diluted solution is described as hypotonic.
Osmosis is the major mechanism for transporting water upward in the plants. Answer the following questions:
Osmotic rise of a solution depends on

Options

A. Density
B. Temperature
C. Nature of solvent
D. All of these

Explanation

To determine how the osmotic rise of a solution depends on various factors, we can analyze the equation for osmotic pressure and the factors involved. Here's the step-by-step solution:

### Step 1: Understand the formula for osmotic pressure
The osmotic pressure (π) of a solution is given by the formula:
\[ \pi = CRT \]
Where:
- \( \pi \) = osmotic pressure
- \( C \) = molar concentration of the solute
- \( R \) = universal gas constant
- \( T \) = absolute temperature (in Kelvin)

### Step 2: Identify the factors affecting osmotic pressure
From the formula, we can see that osmotic pressure depends on:
- **Molar Concentration (C)**: The concentration of solute in the solution directly affects the osmotic pressure. Higher concentration leads to higher osmotic pressure.
- **Temperature (T)**: The absolute temperature also affects osmotic pressure. As temperature increases, the kinetic energy of the molecules increases, which can lead to an increase in osmotic pressure.
- **Nature of the Solvent**: The solvent's properties can influence how solute particles interact with the solvent and affect the overall osmotic pressure.

### Step 3: Conclusion
Thus, the osmotic rise of a solution depends on:
- The molar concentration of the solute
- The temperature of the solution
- The nature of the solvent

### Final Answer:
The osmotic rise of a solution depends on the molar concentration of the solute, the temperature, and the nature of the solvent.

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