what is the osmotic pressure produced by a 1.20M glucose (C6H12O6) solution at 25 degree celsuis?
To calculate the osmotic pressure produced by a solution, you can use the formula:
π = iMRT
Where:
- π is the osmotic pressure
- i is the van't Hoff factor, which represents the number of particles into which the solute dissociates in solution.
- M is the molar concentration of the solute (in mol/L)
- R is the gas constant (0.0821 L·atm/(mol·K))
- T is the absolute temperature (in Kelvin)
First, let's consider the van't Hoff factor for glucose. Glucose does not dissociate in water; it remains as a single undissociated molecule. Therefore, the van't Hoff factor (i) for glucose is equal to 1.
Given:
Molar concentration (M) = 1.20 mol/L
Temperature (T) = 25 degrees Celsius = 25 + 273.15 = 298.15 K
Now, we can substitute the values into the formula:
π = (1)(1.20 mol/L)(0.0821 L·atm/(mol·K))(298.15 K)
Simplifying:
π = 0.0979 atm
Therefore, the osmotic pressure produced by a 1.20M glucose solution at 25 degrees Celsius is approximately 0.0979 atm.