1. Tardigrade
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  3. Chemistry
  4. 0.6 mL of acetic acid is dissolved in 1 L of water. The value of van’t Hoff factor is 1.04 . What will be the degree of dissociation of the acetic acid?

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Q. $ 0.6 \,mL $ of acetic acid is dissolved in $ 1 \,L $ of water. The value of van’t Hoff factor is $ 1.04 $ . What will be the degree of dissociation of the acetic acid?

AMUAMU 2015Solutions

Solution:

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$ i = (1 - \alpha) + \alpha + \alpha$
$ = 1 + \alpha$
Given that $ i = 1.04$
$\therefore 1.04 = 1 + \alpha$
$\alpha = 1.04 - 1$
$= 0.04$