Home
Class 11
CHEMISTRY
Calculate the pH of a 0.1 M aqueous ammo...

Calculate the `pH` of a `0.1` M aqueous ammonium cyanide solution. Given `pK_a =9.02` and `pK_b =4.76`.

Text Solution

Verified by Experts

`pH` of the solution is given as :
`pH=1/2pK_w+1/2pK_a-1/2pK_b`
`pK_w=14,pK_a=9.02 , pK_b=4.76`
`therefore pH=1/2 (14)+1/2 (9.02)-1/2 (4.76)`
`=7+4.51-2.38=9.13`
Promotional Banner

Topper's Solved these Questions

  • EQUILIBRIUM

    MODERN PUBLICATION|Exercise Practice Problems|114 Videos

  • EQUILIBRIUM

    MODERN PUBLICATION|Exercise Conceptual Question 1|24 Videos

  • ENVIRONMENTAL POLLUTION

    MODERN PUBLICATION|Exercise UNIT PRACTICE TEST|15 Videos

  • HALOALKANES AND HALOARENES

    MODERN PUBLICATION|Exercise UNIT PRACTICE TEST|12 Videos

Similar Questions

Explore conceptually related problems

What will be the pH of 0.1 M ammonium acetate solution ? pK_a=pK_b=4.74

Calculate the pH of 0.05M sodium acetate solution, if the pK_(a) of acetic acid is 4.74 .

pH of a solution of salt of weak acid and weak base is : pH=1/2pK_w+1/2pK_a-1/2pK_b and that of weak acid and strong base is pH=1/2pK_w+1/2pK_a+1/2logc pH of 0.1 M solution of ammonium cyanide ( pK_a =9.02 and pK_b =4.76 ) is

What will be the pH of an aqueous solution of 1.0 M ammonium formate? Given : pK_(a)=3.8 and pK_(b)=4.8

What is the pH of a 0.50M aqueous NaCN solution ? (pK_(b)of CN^(-)=4.70)