Question

What would be the osmotic pressure of a 0.02molar aqueous solution of urea at 27degree C?

Answer 1

Answer:

Explanation:

Apply the formula p= m× R× t

P= 0.02×0 .082×300

0.492

Answer 2

Answer:

The osmotic pressure of a 0.02M aqueous solution of urea at 27°C is equal to 0.4926atm.

Explanation:

According to the Boyle Van't Hoff law that the temperature remaining constant, the osmotic pressure of a dilute solution is directly proportional to the molar concentration of the solution.

$\pi =CRT$                                                                             ....................(1)

where π is the osmotic pressure of the solution,

C is the concentration of the solution,

R is the gas constant and R = 0.0821 Lmol⁻¹atmK⁻¹

T is the temperature (in K),

We have given the concentration of the urea solution C 0.02molL⁻¹

T = 27°C =273+27=300K , put the value of C, R and T in equation (1):

$\pi = (0.02molL^{-1})(0.0821Latm^{}K^{-1}mol^{-1})(300K)$

$\pi =0.4926atm$

Therefore, the osmotic pressure of urea solution is equal to 0.4926atm.