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

0.2886 atm is the osmotic pressure of a solution.

Step-by-step explanation:

Osmotic pressure of solution =
`\pi`

Concentration of the solution = c

Mass of the ammonium sulfate = 1.502 g

Moles of ammonium sulfate =
`(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=(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* 0.08206 L atm/mol K* 309.69 K`

`\pi=0.2886 atm`

0.2886 atm is the osmotic pressure of a solution.