Question

What is osmotic pressure of a solution that contains 13.7 g of propyl alcohol (C3H7OH) dissolved in enough water to make 500 mL of solution at 27C ?

Answer 1

11.23 atm

Step-by-step explanation:

Given

Mass = 13.7 g

Volume = 500mL = 0.5 L

Molar concentration =
`\frac{\text{Moles}}{\text{Volume}}\\`

Moles =
`\frac{\text{MassC3H7OH }}{\text{Molar mass C3H7OH }}` =
`(13.7)/(0.5)`= 0.2279534 moles

Molar concentration =
`(0.2279534)/(0.5)` = 0.4559 M

π = icRT

where

Osmotic pressure = π

Van't Hoff factor (i) = 1

Molar concentration of solute (c) = 0.4559 M

Ideal gas constant (R) = 0.0821 L.atm/K.mol

Kelvin Temperature (T) = 273 + 27 = 300 K

`\pi` = 1 * 0.4559 * 0.0821 * 300

= 11.23 atm