Home
Class 12
CHEMISTRY
The ionization constant of chloroacetic ...

The ionization constant of chloroacetic acid is `1.35xx10^(-3)`. What will be the `pH` of `0.1 M` acid and its `0.1M` sodium salt solution?

Text Solution

Verified by Experts

`CH_(2)ClCOOH + H_(2)O to CH_(2)ClCOO^(-) + H_(3)O^(+), K_(a)=1.35 O^(-3)`
(a) `pK_(a)=-logK_(a)=-log[1.35xx10^(-3)]=2.87`
By Oswald’s dilution law :`[H_(3)O^(+)]=sqrt(K_(a).C) = sqrt(1.35xx10^(-3)xx0.1)=1.16xx10^(-2)M`
pH acid = `– log[H_(3)O^(+)] = – log (1.6xx10^(-2))M=1.94`
(b) A `0.1M CH_(2)ClCOONa)` aqueous solution (sodium chloro-acetate) is basic due to hydrolysis.
`CH_(2)ClCOO^(-) + H_(2)O to CH_(2)ClCOOH + OH^(-)`
Using standard result for pH of a salt of strong base and weak acid:`pH=7 + (pK_(a) + logC)/2= (2.87+log0.1)/2= 7.94`
Promotional Banner

Similar Questions

Explore conceptually related problems

The ionisatioln constant of a mono basic acid is 5 xx 10^(-2) . The pH of 0.01 M acid solution is

The ionization constant of propanoic acid is 1.32xx10^(-5) . Calculate the degree of ionization of the acid in its 0.05 M solution and also its pH . What will be its degree of ionization if the solution is 0.01 M on HCl also?

The ionization constant of propionic acid is 1.32xx10^(-5) . Calculate the degree of ionization of the acid in its 0.05 M solution and also its pH. What will be its degree of ionization in the solution of 0.01N HCI ?

The dissociation constant of a weak monobasic acid K_(a) is 1xx 10^(-5) . The pH of 0.1 M of that acid would be

The dissociation constant of a substitude benzoic acid at 25^(@)C is 1.0xx10^(-4) . The pH of a 0.01M solution of its sodium salt is

The dissociation constant of a substituted benzoic acid at 25^(@)C is 1.0xx10^(-4) . The pH of 0.01M solution of its sodium salt is

The acid dissociation constant K_(a) of acetic acid is 1.74 xx 10^(-5) at 298 K. The pH of a solution of 0.1 M acetic acid is