Question

Calculate the osmotic pressure of a solution containing 1.502 g of (Nh4)2SO4 in 1 L at 36.54 Degrees Celcius. (The gas constant is .08206 Latm/molK. The molar mass of (Nh4)2SO4 is 132.16)

Answer 1

Answer:

0.2886 atm is the osmotic pressure of a solution.

Explanation:

Osmotic pressure of solution =$\pi$

Concentration of the solution = c

Mass of the ammonium sulfate = 1.502 g

Moles of ammonium sulfate = $\frac{1.502 g}{132.16 g/mol}=0.01136 mol$

Volume of the solution = 1 L

Concentration of the solution:

$=\frac{\text{Moles of ammonium sulfate}}{\text{Volume of the solution}}$

$c=\frac{0.01136 mol}{1 L}=0.01136 mol/L$

Temperature of the solution ,T= 36.54°C = 309.69 K

R = universal gas constant = 0.08206 L atm/mol K

$\pi=cRT$

$\pi=0.01136 mol/L\times 0.08206 L atm/mol K\times 309.69 K$

$\pi=0.2886 atm$

0.2886 atm is the osmotic pressure of a solution.