Question

In an experiment, osmotic
pressure of 0.1 M aq CH3COOH
solution at 300 K is found to be
2.706 atm and osmotic pressure
of 0.2 M aq CH3COOH solution at
300 K is found to be 5.166 atm.
Select the correct statement(s) on
the basis of this experimental
observation.​

Answer 1

Explanation:

= iCRT 4.92 = i × 0.1 × 0.0821 × 300 i = 1.99 α = i - 1n - 1 α = 1.99 - 13 - 1 = 0.992 = 0.49 Percentage ionization = 49%

Top answer

Answer 2

We can conclude that the association in case 1 is slightly higher than in case 2.

Explanation:

The question is incomplete.

But, the following can be deduced from the given information.

Case 1:

Osmotic pressure $\pi = 2.706$ atm

Concentration $C = 0.1 M$

Temperature $T = 300 K$

Thus, using the formula for osmotic pressure, we can write, $\pi = iCRT$, where 'i' is the Van't Hoff factor.

$i_1 = \frac{\pi }{CRT} = \frac{2.706}{0.1 R T}$

Case 2:

Osmotic pressure$\pi = 5.166$ atm

Concentration $C = 0.2 M$

Temperature $T = 300 K$

Hence, $i_2 = \frac{\pi }{CRT} = \frac{5.166}{0.2 R T}$

Taking the ratio of both, we obtain

$\frac{i_1}{i_2} = \frac{(2.706/0.1RT)}{(5.166/0.2RT)} = \frac{27.06}{25.83} = 1.047$

$i_1 = 1.047\times i_2$

Thus, we can conclude that the association in case 1 is slightly higher than in case 2.