Home
Class 11
CHEMISTRY
The degree of dissociation of weak elect...

The degree of dissociation of weak electrolyte is inversely proportional to the same square root of concentration. What is called Ostwald's dilution law.
`alpha = sqrt((K_(a))/(c ))` As the temperature increases, degree of dissociation will increase.
`(alpha_(1))/(alpha_(2)) = sqrt((K_(a1))/(K_(a2)))` if concentration is same. `(alpha_(1))/(alpha_(2)) = sqrt((c_(2))/(c_(1)))` if acid is same.
0.01 M `CH_(3)COOH` has 4.24% degree of dissociation, the degree of dissociation of 0.1 M `CH_(3)COOH` will be

A

`1.33%`

B

`4.24%`

C

`5.24%`

D

`0.33%`

Text Solution

Verified by Experts

The correct Answer is:
A
Use : `(alpha_(1))/(alpha_(2)) = sqrt((C_(2))/(C_(1))) rArr (4.24)/(alpha_(2)) = sqrt((0.1)/(0.01)) rArr alpha_(2) = (4.24)/(sqrt(10))% = 1.33%`
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL AND IONIC EQUILIBRIUM

    BRILLIANT PUBLICATION|Exercise Level - III (Linked Comprehension Type Questions)|1 Videos

  • CHEMICAL AND IONIC EQUILIBRIUM

    BRILLIANT PUBLICATION|Exercise Level - III (Statement Type)|6 Videos

  • CHEMICAL BONDING

    BRILLIANT PUBLICATION|Exercise LEVEL-III ( Linked Comprehension Type )|12 Videos

Similar Questions

Explore conceptually related problems

The degree of dissociation (alpha) of a weak electrolyte, A_(x)B_(y), is related to van't Hoff factor (i) by the expression

Kohlrausch's law helps to determine the degree of dissociation of a weak electrolyte at a given concentration. State Kohlrausch's law.

Calculate the p^(Ka) of 0.1M solution of acetic acid if the degree of dissociation of acetic acid is 1.32xx10^(-2)

The van' Hoff factor for 0.I M Ba(NO '_3', solu- tion is 2.74 . The degree of dissociation is -