calculate the osmotic pressure of a solution obtained by mixing 100ml of 0.25M solution of urea and 100ml of 0.1m solution of cane sugar at 293k
To calculate the osmotic pressure of a solution, you need to know the concentration of solute particles and the temperature.
In this case, we have two solutes: urea and cane sugar.
First, let's calculate the total concentration of the solute particles in the solution.
For the urea solution:
Volume (V) = 100 mL = 0.1 L
Concentration (C) = 0.25 M
The number of moles can be calculated using the formula:
Number of moles (n) = concentration (C) * volume (V)
For the urea solution:
number of moles (n1) = 0.25 mol/L * 0.1 L
Next, we calculate the number of moles for the cane sugar solution:
For the cane sugar solution:
Volume (V) = 100 mL = 0.1 L
Concentration (C) = 0.1 M
For the cane sugar solution:
number of moles (n2) = 0.1 mol/L * 0.1 L
To find the total number of moles, we add the moles from both solutions:
Total number of moles (ntotal) = n1 + n2
Now that we have the total number of moles, we can calculate the osmotic pressure (π) using the formula:
Osmotic Pressure (π) = ntotal * R * T
Where:
R = ideal gas constant (0.0821 L.atm/(mol.K))
T = temperature in Kelvin (293K)
Now, let's put the values into this formula:
Osmotic Pressure (π) = (n1 + n2) * 0.0821 L.atm/(mol.K) * 293 K
Calculate the value of (n1 + n2), then multiply it by 0.0821 L.atm/(mol.K), and multiply that by 293 K.
This will give you the osmotic pressure of the solution obtained by mixing 100 mL of 0.25 M urea and 100 mL of 0.1 M cane sugar at 293 K.
pi = MRT
I suppose you are to assume that 0.1m = 0.1M.
Then 100 mL x 0.25 = millimols urea.
100 mL x 0.1M = millimols sugar.
Total M = total millimols/total mL.
Solve for pi.