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?

Question

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? (A)  0.01  (B)  0.02  (C)  0.03  (D)  0.04

Tardigrade Admin · Accepted Answer

<img class="img-fluid question-image" alt="image" src="https://cdn.tardigrade.in/img/question/chemistry/b7b14eb2bc093c59c8908008e9f49c1f-.png" /> i = (1 - α) + α + α = 1 + α Given that i = 1.04 ∴ 1.04 = 1 + α α = 1.04 - 1 = 0.04

Q. $0.6 m L$ 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?

$0.01$

$0.02$

$0.03$

$0.04$

$i = (1 - α) + α + α$
$= 1 + α$
Given that $i = 1.04$
$∴ 1.04 = 1 + α$
$α = 1.04 - 1$
$= 0.04$

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

0.01

0.02

0.03

0.04