Home
Class 12
CHEMISTRY
What will be the degree of dissociation ...

What will be the degree of dissociation of 0.005M `NH_(4)OH`solution. If `pK_(b)` for `NH_(4)OH` is 4.7

A

`2%`

B

`0.03%`

C

`1.4%`

D

`6. 32%`

Text Solution

Verified by Experts

The correct Answer is:
D
`pK_(b)=4.2`
`K_(b)=10^(-5)xx10^(0.3)`
`K_(b)=2xx10^(-5)=Calpha^(2)`
`2xx10^(-5)=5xx10^(-3) a^(2)`
`alpha^(2)=(2xx10^(-5))/(5xx10^(-3))=0.4xx10^(-2)`
`alpha^(2)=6.32xx10^(-2)xx100=6.32%`
Promotional Banner

Topper's Solved these Questions

  • CHEMISTRY AT A GLANCE

    ALLEN|Exercise INORGANIC CHEMISTRY|300 Videos

  • CHEMISTRY AT A GLANCE

    ALLEN|Exercise ORGANIC CHEMISTRY|483 Videos

  • Chemical Equilibrium

    ALLEN|Exercise All Questions|24 Videos

  • ELECTROCHEMISTRY

    ALLEN|Exercise EXERCISE -05 [B]|38 Videos

Similar Questions

Explore conceptually related problems

Calculate the degree of hydrolysis and pH of 0.2M solution of NH_(4)C1 Given K_(b) for NH_(4)OH is 1.8 xx 10^(-5) .

Determine the dergee of dissociation of 0.05 M NH_(3) at 25^(@)C in a solution of pH = 11 . K_(b) = 1.77 xx 10^(-5) (pK_(b) = 4.75)

At pH lt3.1 , the indicator methyl red is coloured red ,at pH gt 6.3 , it is yellow and at the intermediate values of the pH ,it is orange .What will the colour of indicator be in a 0.1 M solution of NH_(4)Br ? Take pK_(b)(NH_(4)OH)=4.74 .

0.05 M ammonium hydroxide solution is dissolved in 0.001 M ammonium chloride solution. What will be the OH^(-) ion concentration of this solution ? (K_(b) (NH_(4) OH) = 1.8 xx 10^(-5)

The pH of a buffer solution of 0.1 M NH_(4)OH [ pK_(a)=4.0] and 0.1 M NH_(4)Cl is

In which of the following, dissociation of NH_(4)OH will be minimum?