Home
Class 12
CHEMISTRY
The dissociation constant of a monobasic...

The dissociation constant of a monobasic acid which is `3.5%` dissociated in `(N)/(20)` solution at `20^(@)C` is

A

`3.5 xx 10^(-2)`

B

`5 xx 10^(-3)`

C

`6.125 xx 10^(-5)`

D

`6.75 xx 10^(-2)`

Text Solution

Verified by Experts

The correct Answer is:
C
Concentration of acid `=N/20` = 0.05 N
Out of 100 molecules, 3.5 molecules have been dis- sociated
`therefore` Out of 1 molecules the no. of dissociated molecules `=(35)/(100)=0.035=alpha`
`K_(a)=(Calpha^(2)0/((1-alpha))), K_(a)=alpha^(2)C`
`K_(a)=(0.035 xx 0.035 xx 1)/(20)`
`K_(a)=6.125 xx 10^(-5)`
Promotional Banner

Topper's Solved these Questions

  • IONIC EQUILIBRUIM

    MOTION|Exercise Exercise -1|58 Videos

  • IONIC EQUILIBRUIM

    MOTION|Exercise Exercise -2 (Level -1)|37 Videos

  • HYDROCARBON

    MOTION|Exercise Exercise - 4 (Level-II)|15 Videos

  • ISOMERISM

    MOTION|Exercise Exercise 4|26 Videos

Similar Questions

Explore conceptually related problems

Find the dissocation constant K_(a) of HA (weak monoabsic acid) which is 3.5% dissociated in an M//20 solution.

The dissociation constant of a weak monoprotic acid, which is 0.01 % ioniosed in 1 .00M solution , is

Dissociation Constant of water at 25^(@)C is "

The dissociation constant of a weak monobasic acid in 0.01 M solution is 10^(-8) . What is its [OH^(-)] concentration?

The dissociation constant of a weak monobasic acid K_(a) is 1xx 10^(-5) . The pH of 0.1 M of that acid would be

The dissociation constant of an acid is 1xx10^(-5) . The pH of its 0.1 M solution will be approximately

The dissociation constant for an acid HA is 1.6 xx 10^(-5) . Calculate its H_(3)O^(+) in concentration in 0.01 M solution .