Home
Class 12
CHEMISTRY
At 25^(@)C, the dissociation constant of...

At `25^(@)C`, the dissociation constant of a base, BOH id `1.0xx10^(-12)`. The concentration of hydroxyl ions in 0.01 M aqueous solution of the base would be

A

`2.0 xx 10^(-6) mol L^(-1)`

B

`1.0 xx 10^(-5) mol L^(-1)`

C

`1.0 xx 10^(-6) mol L^(-1)`

D

`1.0 xx 10^(-7) mol L^(-1)`

Text Solution

Verified by Experts

The correct Answer is:
2

`{:(,BOH,hArr,B^(+),+,OH^(-)),("initial",C,,0,,0),("At.eq.",C-Calpha,,Calpha,,Calpha):}`
`K_(b) = (C^(2)alpha^(2))/(C(1-alpha)) = Calpha^(2) " assuming a " lt lt 1, 1 - a gt gt 1`
` 10^(-12) = 10^(-2) xx a^(2) , a^(2) = 10^(-10) , a = 10^(-5)`
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • IONIC EQUILIBRIUM

    VMC MODULES ENGLISH|Exercise PRACTICE EXERCISE - 1|4 Videos
  • IONIC EQUILIBRIUM

    VMC MODULES ENGLISH|Exercise PRACTICE EXERCISE - 2|8 Videos
  • IONIC EQUILIBRIUM

    VMC MODULES ENGLISH|Exercise Illustration - 29|1 Videos
  • INTRODUCTION TO ORGANIC CHEMISTRY

    VMC MODULES ENGLISH|Exercise JEE ADVANCED ARCHIVE|81 Videos
  • JEE MAIN - 5

    VMC MODULES ENGLISH|Exercise PART II : CHEMISTRY (SECTION - 2)|5 Videos

Similar Questions

Explore conceptually related problems

At 25^(@)C , the dissociation constant of a base. BOH is 1.0xx10^(-12) . The concentration of hydroxyl ions in 0.01 M aqueous solution of the base would be

Calculate the concentration of hydroxyl ions in a 0.1 M solution of ammonia if the value of K_b is 1.76 xx 10^(-5)

The ionization constant of phenol is 1.0xx10^(-10) . What is the concentration of phenolate ion in 0.05 M solution of phenol? What will be its degree of ionization if the solution is also 0.01 M in sodium phenolate?

The dissociation constant of an acid, HA is 1 x 10^-5 The pH of 0.1 M solution of the acid will be

The dissociation constant of a base MOH is 4xx10^(-6) then calculate the dissociation constant of its conjugate acid

The dissociation constant of a base MOH is 4xx10^(-6) then calculate the dissociation constant of its conjugate acid

The dissociation constatn of 0.01 M CH_(3)COOH is 1.8xx10^(-5) then calculate CH_(3)COO^(-) concentration of 0.1 M HCl solution.

The dissociation constatn of 0.01 M CH_(3)COOH is 1.8xx10^(-5) then calculate CH_(3)COO^(-) concentration of 0.1 M HCl solution.

The dissociation constant of a weak acid HA is 1.2 xx 10 ^(-10) Calculate its pH in a 0.1 M solutions

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