What will be the osmotic pressure of a solution containing 3.42 g sugar in one litre of solution at 27 [ Mol. Wt of sugar =342 ], R= 0.082 litre-atm/mol.deg].
To calculate the osmotic pressure of a solution, you can use the formula:
Π = MRT
Where:
Π is the osmotic pressure (in atm)
M is the molarity of the solution (in mol/L)
R is the ideal gas constant (0.082 L·atm/mol·K)
T is the temperature (in Kelvin)
First, we need to determine the molarity of the solution.
Given:
Mass of sugar = 3.42 g
Molecular weight of sugar = 342 g/mol
Volume of solution = 1 L
1. Convert the mass of sugar to moles.
Moles of sugar = mass / molecular weight
Moles of sugar = 3.42 g / 342 g/mol
Moles of sugar = 0.01 mol
2. Calculate the molarity of the solution.
Molarity = moles of solute / volume of solution
Molarity = 0.01 mol / 1 L
Molarity = 0.01 M
3. Convert the temperature from degrees Celsius to Kelvin.
Kelvin = Celsius + 273.15
Kelvin = 27 + 273.15
Kelvin = 300.15 K
Now, plug the values into the osmotic pressure formula:
Π = MRT
Π = (0.01 M) * (0.082 L·atm/mol·K) * (300.15 K)
Π = 0.0244953 atm
Therefore, the osmotic pressure of the solution containing 3.42 g of sugar in 1 liter of solution at 27°C is approximately 0.0245 atm.