Question

The nonvolatile, nonelectrolyte sucrose, C12H22O11 (342.3 g/mol), is soluble in water H2O.

Calculate the osmotic pressure (in atm) generated when 12.8 grams of sucrose are dissolved in 278 mL of a water solution at 298 K.

Answer 1

Answer: The osmotic pressure of the solution is 3.29 atm

Step-by-step explanation:

To calculate the concentration of solute, we use the equation for osmotic pressure, which is:

`\pi=iMRT`

or,

`\pi=i* \frac{\text{Mass of solute}* 1000}{\text{Molar mass of solute}* \text{Volume of solution (in mL)}}* RT`

where,

`\pi` = osmotic pressure of the solution = ?

i = Van't hoff factor = 1 (for non-electrolytes)

Mass of sucrose = 12.8 grams

Molar mass of sucrose = 342.3 g/mol

Volume of solution = 278 mL

R = Gas constant =
`0.082\text{ L atm }mol^(-1)K^(-1)`

T = temperature of the solution = 298 K

Putting values in above equation, we get:

`\pi=1* (12.8* 1000)/(342.3* 278)* 0.0821\text{ L. atm }mol^(-1)K^(-1)* 298K\\\\\pi=3.29atm`

Hence, the osmotic pressure of the solution is 3.29 atm