**Core Concept**
Osmotic pressure is a colligative property of solutions, which depends on the concentration of solute particles in a solution. It is the pressure required to prevent the flow of solvent molecules into the solution through a semipermeable membrane.

**Why the Correct Answer is Right**
The osmotic pressure of an ideal solute is directly proportional to the concentration of the solute particles and the temperature of the solution. According to the equation developed by van't Hoff, the osmotic pressure (π) of a solution is given by π = cRT, where c is the concentration of the solute, R is the gas constant, and T is the temperature in Kelvin. For 1 mol of ideal solute, the concentration is 1 mol/L, and the osmotic pressure is directly proportional to the gas constant (R) and the temperature (T). The value of R is approximately 0.0821 L atm/(mol K), and the temperature is typically measured in Kelvin.

**Why Each Wrong Option is Incorrect**
**Option A:** This option is not provided.
**Option B:** This option is not provided.
**Option C:** This option is not provided.
**Option D:** This option is not provided.

**Clinical Pearl / High-Yield Fact**
A key point to remember is that the osmotic pressure of a solution is directly proportional to the concentration of solute particles and the temperature of the solution. This is why the osmotic pressure of a solution increases with increasing concentration of solute particles and temperature.

**Correct Answer: C. 0.0821 T (atmospheres) or 1.01325 T (kPa) per mol of ideal solute.**