The hydrolysis constang of `0.1M` aqueous solution of sodium acetate if `K_(a)` of `CH_(3)COOH = 1.8 xx 10^(-5)` is

The hydrolysis constant of 0.1M aqueous solution of sodium acetate if K_(a) of CH_(3)COOH = 1.8 xx 10^(-5) is

Calculate the degree of hydrolysis of 0.1 M solution of sodium acetate at 298 K : K_(a) = 1.8 xx 10^(-5) .

Calculate the degree of hydrolysis of 0.1 M solution of sodium acetate at 298 K : K_(a) = 1.8 xx 10^(-5) .

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)

Determine the hydrolysis constantand degree of hydrolysis of 0.01 M solution of ammonium acetate , given that K_(a) =1.752 xx 10^(-5) , K_(b) =1.74 xx 10^(-5)

What will be the hydrogen ion concentration of a solution obtained by mixing 500ml of 0.2 M acetic acid and 500ml of 0.4 M sodium acetate ? (K_(a)CH_(3)COOH)=1.8 xx 10^(-5))

Calculate the degree of hydrolysis of a decimolar solution of ammonium acetate at 25^@C . K_a(CH_3COOH)=1.75xx10^(-5), K_b(NH_4OH)=1.81xx10^(-5)