Home
Class 11
CHEMISTRY
pKb of CN^(-) is 4.7 Calculate (a) h...

`pK_b `of ` CN^(-)` is 4.7 Calculate (a) hydrolysis constant and (b) degree of hydrolysis of 0.5M aqueous NaCN solution.

Text Solution

Verified by Experts

`pk_b `of ` CN^(-) = 4.7 `
therefore `k_b `of ` CN^(-) = 10^(-4.7) = 2 xx 10^(-5)`
Hydrolysis constant (K) is given in terms of ionic product of water (`K_w`) as
`k_h = (k_w)/(k_a) =k_w xx (k_b)/(k_w) =k_b = 2 xx 10^(-5)`
Degree of hydrolysis (h ) is given as , h`= sqrt( k_h //c) = sqrt(2 xx 10^(-5) //0.5 ) = 6.3 xx 10^(-3)`
Promotional Banner

Similar Questions

Explore conceptually related problems

pK_a of acetic acid is 4.76 and pk_b is NH_4 OH is 4.75. Calculate the hydrolysis constant and degree of hydrolysis of ammonium acetate.

Calculate (a) hydrolysis constant, (b) degree of hydrolysis and (c) pH of 0.01 M sodium acetate, if K_a of CH_3 COOH is 1.9 xx 10^(-5)

K_a for a weak monobasic acid HA is 1 xx 10^(-4) . Calculate (a) hydrolysis constant of KA and (b) neutralisation constant for the reaction of HA with KOH.

The pH of 0.1M solution of cyantic acid (HCNO) is 2.34 .Calulate the ionization constant of the acid and its degree of ionization in the solution.

A weak acid HX has the dissociation constant 1xx 10 ^(-5) M.It forms a salt NaX on reactions with alkali. The percentage hydrolysis of 0.1 M solution of NaX is :

The ionization constant of nitrous acid is 4.5xx10^(-4) . Calculate the pH of 0.04M sodium nitrite solution and also its degree of hydrolysis.

pK_(b) of aq. NH_(3) is 4.74 hence pH of 0.01 M NH_(3) solution is

E_("cell") for the reaction Pt , H_2 (1atm)//H^(+) (1M)"//" C_6H)5NH_3Cl (1//32 M)//H_2(1 atm) , Pt at 300K is -0.188 V. Calculate the proton concentration and hydrolysis constant of aniline hydrochloride.

The pH of 0.004M hydrazine solution is 9.7 . Calculate its ionization constant K_(b) and pK_(b) .