Home
Class 12
CHEMISTRY
Calculate the PH of 0.01 M aqueous solut...

Calculate the PH of 0.01 M aqueous solution of `NH_4CN`. Given dissociation constants Of HCN is 6.2×10 −10 and of `NH_3` is 1.6×10 −5

Promotional Banner

Topper's Solved these Questions

  • ENVIRONMENTAL CHEMISTRY

    MBD PUBLICATION|Exercise QUESTION BANK|299 Videos

  • GENERAL PRINCIPLES OF ISOLATION OF ELEMENTS

    MBD PUBLICATION|Exercise QUESTION BANK|564 Videos

Similar Questions

Explore conceptually related problems

The pH of 10 M HCl aqueous solution is:

The ph of 1 M aqueous solution of the weak acid HA is 6.0.Find its dissociation constant.

An aqueous solution of 0.1 M NH_4Cl will have a pH closer to:

Calculate the PH of KOH solution 5.6 gm of which is dissolved in 10 litre solution .

Find the pH of a 0.01 M solution of acetic acid having degree of dissociation 12.5%.

A monotropic acid in 1.00 M solution is 0.01% ionised. What is the dissociation constant of the acid ?

Calculate PH Of 0.01 M acetic acid . K_a = 1.8 xx 10^-5 at 298 K.

Formic acid is 4.6% dissociated in a 0.1 N solution at 20^@C . The ionisation constant of formic acid is :

The dissociation constant of NH_4OH is 1.8xx10^(-5) predict the hydrolysis constant of NH_4Cl

The dissociation constant of HCN is 1.3 xx 10^-9 . The value of hydrolysis constant of KCN will be: